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NANOSCALE SURFACE ENGINEERING FOR CERAMIC FUEL CELLS
A DISSERTATION
SUBMITTED TO THE DEPARTMENT OF MECHANICAL ENGINEERING
AND THE COMMITTEE ON GRADUATE STUDIES
OF STANFORD UNIVERSITY
IN PARTIAL FULFILLMENT OF THE REQUIREMENTS FOR THE DEGREE OF
DOCTOR OF PHILOSOPHY
Young Beom Kim
August 2011
http://creativecommons.org/licenses/by-nc/3.0/us/
This dissertation is online at: http://purl.stanford.edu/sy490sp5158
© 2011 by Young Beom Kim. All Rights Reserved.
Re-distributed by Stanford University under license with the author.
This work is licensed under a Creative Commons Attribution-Noncommercial 3.0 United States License.
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I certify that I have read this dissertation and that, in my opinion, it is fully adequatein scope and quality as a dissertation for the degree of Doctor of Philosophy.
Friedrich Prinz, Primary Adviser
I certify that I have read this dissertation and that, in my opinion, it is fully adequatein scope and quality as a dissertation for the degree of Doctor of Philosophy.
Thomas Kenny
I certify that I have read this dissertation and that, in my opinion, it is fully adequatein scope and quality as a dissertation for the degree of Doctor of Philosophy.
Xiaolin Zheng
Approved for the Stanford University Committee on Graduate Studies.
Patricia J. Gumport, Vice Provost Graduate Education
This signature page was generated electronically upon submission of this dissertation in electronic format. An original signed hard copy of the signature page is on file inUniversity Archives.
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ABSTRACT
Ceramic fuel cell (CFC) is an all-solid-state energy conversion device and usually refers
to fuel cells employing solid ceramic electrolytes. The present generation of ceramic fuel
cells can be classified into two types according to the electrolytes they use: oxygen ion
conducting fuel cells, or solid oxide fuel cells (SOFCs) and proton conducting fuel cells
(PCFC or PCOFC). CFCs usually have the highest operating temperature of all fuel cells
at about 600~1000oC for reasonably active charge transfer reactions at the electrode-
electrolyte interface and ion transport through the electrolyte. This high CFC’s operating
temperature has limited practical applications. The goal of my Ph.D. research is to
minimize the activation losses at the electrode/electrolyte interface by nanoscale
engineering to achieve decent performance of ceramic fuel cells at lower operating
temperatures (300~500oC). This dissertation has three main nanoscale surface
engineering approaches according to the fuel cell components: electrode structure,
composite electrolyte structures with thin interlayers, and the fabrication of three-
dimensional fuel cell membrane-electrode assemblies (MEAs).
We would call the first part of the dissertation as nanoscale electrode structure
engineering for ceramic fuel cells. It describes the fabrication and investigation of
morphologically stable model electrode structures with well-defined and sharp
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platinum/yttria stabilized zirconia (YSZ) interfaces to study geometric effects at triple
phase boundaries (TPB), which is known as the actual electrochemical reaction site. A
nanosphere lithography (NSL) technique using monodispersed silica nanoparticles is
employed to deposit nonporous platinum electrodes containing close-packed arrays of
circular openings through the underlying YSZ surface. These nano-structured dense Pt
array cathodes exhibited better structural integrity and thermal stability at the fuel cell
operating temperature of 450~500oC when compared to porous sputtered Pt electrodes.
More importantly, electrochemical studies on geometrically well-defined Pt/YSZ sharp
interfaces demonstrated that the cathode impedance and cell performance both scale
almost linearly with aerial density of TPB length. These controlled experiments also
allowed for the estimation of the area of the electrochemical reaction zone. This
information can be used as a platform for designing the electrode structure to maximize
the performance of ceramic fuel cells.
The second part of the experiment is about electrolyte surface structure engineering by
fabricating composite electrolyte structures. This study describes, both theoretically and
experimentally, the role of doped ceria cathodic interlayers and their surface grain
boundaries in enhancing oxygen incorporation kinetics. Quantum mechanical simulations
of oxygen incorporation energetics support the experimental results and indicate a low
activation energy of only 0.07eV for yttria-doped ceria (YDC), while the incorporation
reaction on YSZ is activated by a significantly higher energy barrier of 0.38eV. For
experiments, epitaxial and polycrystalline YDC, gadolinia-doped ceria (GDC) thin films
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were grown by pulsed laser deposition (PLD) on the cathode side of 300µm-thick single
crystalline (100) and 100µm-thick polycrystalline YSZ substrates, respectively. For the
composite electrolyte sample with YDC interlayer, the Oxygen isotope exchange
experiment was conducted employing secondary ion mass spectrometry (SIMS) with
high spatial resolution (50nm). The surface mapping result of 18
O/16
O shows high activity
at surface grain boundary regions indicating that the grain boundary regions are
electrochemically active for oxygen incorporation reaction. Fuel cell current-voltage
behavior and electrochemical impedance spectroscopy measurements were carried out in
the temperature range of 350oC-450
oC on both single crystalline and polycrystalline
interlayered cells. Results of dc and ac measurements confirm that cathodic resistances of
cells with epitaxial doped-cerium oxides (GDC, YDC) layers are lower than that for the
YSZ-only control cell. This is attributed to the higher surface exchange coefficient for
doped-cerium oxides than for YSZ. Moreover, the role of grain boundary density at the
cathode side external surface was investigated on surface-engineered electrode-
membrane assemblies (MEA) having different doped-ceria surface grain sizes. MEAs
having smaller surface grain size show better cell performance and correspondingly
lower electrode interfacial resistance. Electrochemical measurements suggest that doped-
ceria grain boundaries at the cathode side contribute to the enhancement of oxygen
surface kinetics. These results provide an opportunity and a microstructure design
pathway to improve performance of LT-SOFCs by surface engineering with nano-
granular, catalytically superior thin doped-ceria cathodic interlayers.
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Thirdly, as a reaction surface engineering for SOFC, we investigated a novel method for
creating a three-dimensional (3-D) fuel cell architecture to enhance fuel cell performance
by increasing the area of the electrolyte membrane. The research describes the fabrication
and operation of a low temperature 3-D protonically conducting ceramic fuel cell
featuring a close packed and free standing crater patterned architecture achieved by
nanospherical patterning (NSP) and dry etching techniques. The cell employed conformal
layers of yttria-doped barium zirconate (BYZ) anhydrous electrolyte membrane
(~120nm) sandwiched between thin (~70nm) sputtered porous Pt electrode layers. The
fuel cell structure achieved the highest reported peak power densities up to 186 mW/cm2
at 450oC using hydrogen as fuel. To further investigate the proton conductivity of the
electrolyte, which is BYZ, we studied the effect of crystalline structures on proton
conductivity of BYZ thin films. The results showed that the grain boundaries impede the
proton transport through the grain boundary and cause extremely high resistance for ionic
transport in the film. This experimental result also can provide significant implications in
designing proton conducting ceramic fuel cells.
All these efforts and investigations were intended to enhance the ceramic fuel cell
performance at low operating temperatures (300–500oC) by improving
electrode/electrolyte interface electrochemical reactions. We expect to achieve further
enhancement when we combine the approaches each other. For example, fabrication of
three-dimensional fuel cells with doped-ceria interlayers and composite electrolyte
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structures with optimized electrode nano-structures. Investigations are on-going in our
laboratory as a future work.
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ACKNOWLEDGMENTS
First of all, I would like to thank all the members in Nanoscale Prototyping Laboratory at
Stanford. This work would have not been possible without their support throughout my
graduate career. Especially, I would like to express my great depth of gratitude to my
principal advisor, Prof. Fritz Prinz. There is a saying that “Water changes its shape
depending on the containers. Similarly, people vary depending on whom he/she with”
and I personally believe that. After joining Prof. Prinz’s research group, I can say that my
attitude toward my life and scientific research has been changed. He is a great leader and
motivator. His remarkable guidance, encouragement, and enthusiasm for scientific
research have truly helped me to make it this far. Also, I am truly grateful to Prof. Turgut
Gür for his thoughtful guidance and intellectual contributions throughout my research. I
would also like to thank my dissertation committee members for their insightful reviews,
valuable comments and time: Prof. Thomas Kenny, Prof. Xiaolin Zheng, and Prof. Sally
Benson.
I would like to thank especially to my close colleagues, Dr. Joon Hyung Shim, Dr.
Wonyoung Lee, Joong Sun Park, Jihwan An, Dr. Pei-Chen Su, Dr. Cheng-Chieh Chao,
Dr. Jason Komadina for their valuable discussions, advice, and dedicated collaborations.
I would also like to thank former NPL members who inspired me, Dr. Suk Won Cha, Dr.
Sangkyun Kang, Dr. Rainer Fasching, Dr. Won Hyung Ryu, Dr. Minhwan Lee, Dr. Tim
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Holme, Dr. Rojana Pornpransertsuk, Dr. Seoung-jai Bai, Masayuki Sugawara, Dr. Kyle
Hammerick, Dr. Yu-Chi Chang, and Dr. Jeremy Cheng.
Also, I am grateful to all NPL members, Dr. Neil Dasgupta, Dr. Munekazu Motoyama,
Hee-Joon Jung, Hark Lee, Xu Tian, Orlando Trejo, Mike Langston, James Mack, Phil
Van Stockum, Andrei Iancu, John Xu, Zubin Huang, Zeng Fan, Takane Usui, Ushio
Harada, and Hitoshi Iwadate for their support and collaboration.
I must recognize all my friends in Korea for being always supportive and cheerful. They
have really helped me not to lose my focus. I thank all my KME and KCF friends for
their support and prayer.
In addition, I would like to thank my family members. I am deeply thankful to In-Soo
Kim, Heung-Soo Kim, and Sung-Duk Lee for their support throughout my life and also
thank to all my cousins. I would like to thank my in-laws, Sung-Min Choi, Young-Ja
Song, Bryan Cho, Woo-Ri Choi (Yuna and Yennie), and Dan-Bi Choi for their prayers.
Last but not least, I must thank my dad, Sung-Soo Kim, mom, Shin-Ae Moon, brother,
Young-Jun Kim (and Se-Hee Kim), my lovely wife, Ji-Soo Choi for their endless love,
support, and prayers.
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DEDICATION
The author wishes to dedicate this dissertation to his grandfathers, grandmothers, father,
mother, brother, wife, and everyone in his family.
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TABLE OF CONTENTS
List of tables .......................................................................................................................xv
List of figures ................................................................................................................... xvi
Chapter 1: Intdroduction ..................................................................................................1
1.1 Dissertation Overview .............................................................................................1
1.2 Outline......................................................................................................................3
1.3 Individual/Group Research Statement .....................................................................5
1.4 References ................................................................................................................6
Chapter 2: Fuel Cell Overview .........................................................................................8
2.1 Fuel Cell Basics .......................................................................................................8
2.2 Types of Fuel Cells ...............................................................................................11
2.3 Fuel Cell Performance and Loss Mechanisms .......................................................13
2.3.1 Thermodynamic Reversible Voltage ............................................................15
2.3.2 Activation Losses ..........................................................................................18
2.3.3 Ohmic Losses ................................................................................................21
2.3.4 Mass Transport Losses ..................................................................................23
2.4 Ceramic Fuel Cells .................................................................................................24
2.5 References ..............................................................................................................27
Chapter 3: Materials for Ceramic Electrolytes and A Fabrication Technique .........28
3.1 Ceramic Electrolyte Materials ...............................................................................28
3.1.1 Oxygen Ion Conducting Ceramics ................................................................28
3.1.2 Proton Conducting Ceramics ........................................................................32
3.2 Pulsed Laser Deposition ........................................................................................34
3.2.1 Background ...................................................................................................34
3.2.1 Example Materials of Pulsed Laser Deposition ............................................38
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3.3 References ..............................................................................................................41
Chapter 4: Nano-pore Structured Platinum Electrode Arrays for LT-SOFCs .........43
4.1 Introduction ............................................................................................................43
4.2 Experimental ..........................................................................................................48
4.2.1 Spherical Silica Particle Fabrication .............................................................48
4.2.2 Nanosphere lothography (NSL) for Nano-Structured Electrodes .................49
4.3 Results and Discussion ..........................................................................................53
4.3.1 Thermal Stability of the Nano-pore Structured Electrode ............................53
4.3.2 Investigation of TPB Scaling Behavior ........................................................59
4.3.3 TPB Width Estimation for Pt/YSZ Interface ................................................65
4.4 Conclusion .............................................................................................................70
4.5 References ..............................................................................................................72
Chapter 5: Cathodic Surface Engineered LT-SOFCs ..................................................75
5.1 Introduction ............................................................................................................75
5.2 Experimental ..........................................................................................................80
5.2.1 Quantum Simulation of Oxygen Incorporation Energies .............................80
5.2.2 Oxygen Isotope Exchange and NanoSIMS...................................................81
5.2.3 Composite Electrolyte Fuel Cell Fabrication and Characterization .............83
5.3 Results and Discussion ..........................................................................................85
5.3.1 Surface Engineered SOFC with YDC Cathodic Interlayer...........................85
5.3.2 Surface Engineered SOFC with GDC Cathodic Interlayer.........................109
5.4 Conclusion ...........................................................................................................116
5.5 References ............................................................................................................117
Chapter 6: Three-dimensional Proton Conducting Fuel Cell Architecture with
Ultra Thin Ceramic Electrolyte ....................................................................................121
6.1 Introduction ..........................................................................................................121
6.2 Experimental ........................................................................................................124
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6.3 Results and Discussion ........................................................................................127
6.4 Conclusion ...........................................................................................................139
6.5 References ............................................................................................................139
Chapter 7: Effect of Crystallinity on Proton Conductivity in Yttrium-doped
Barium Zirconate Thin Films .......................................................................................142
7.1 Introduction ..........................................................................................................143
7.2 Experimental ........................................................................................................145
7.3 Results and Discussion ........................................................................................148
7.4 Conclusion ...........................................................................................................165
7.5 References ............................................................................................................166
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LIST OF TABLES
Number Page
Table 2-1: Characteristics of five major fuel cell types ....................................................11
Table 3-1: Wavelength of excimer lasers .........................................................................36
Table 3-2: Example materials deposited by pulsed laser deposition and applications
of those materials .............................................................................................40
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LIST OF FIGURES
Number Page
Figure 2-1: Schematic of a typical hydrogen-oxygen fuel cell ...........................................9
Figure 2-2: Schematic of a typical fuel cell current-voltage (I-V) curve .........................15
Figure 3-1: Schematic of PLD mechanism (Top) and a sample picture of PLD process:
deposition of BYZ on MgO (100) substrate ....................................................35
Figure 4-1: Synthesized spherical silica particles with different diameters: (a) 130nm,
(b) 300nm, (c) 650nm ......................................................................................49
Figure 4-2: Schematic of the Langmuir –Blodgett trough .................................................50
Figure 4-3: Fabrication process schematic of nano-pore structured electrode by using
nanosphere lithography (NSL) technique ........................................................51
Figure 4-4: SEM images of nano-pore structured dense Pt electrodes ..............................52
Figure 4-5: Schematic illustration of the probing station for electrochemical
characterization of fuel cell MEAs ..................................................................53
Figure 4-6: SEM images of (a) as sputtered porous Pt layer, (b) after short time (~
30mins) operation of fuel cell at elevated temperature (450oC), clearly
indicate a dramatic change in Pt morphology and a proportionate reduction
in the TPB density ............................................................................................54
Figure 4-7: Potentioamperometry data at 0.6V, comparing the behavior of SOFC MEA
with porous Pt electrode and SOFC with nano-pore structured Pt electrode.
Measurement was conducted for 12 hours continuously at 500oC. (a)
Absolute output current densities indicating severe degradation in
performance of porous Pt within a short time as opposed to stable behavior
of patterned dense Pt. (b) Normalized current densities plot showing
relative amounts of degradation from the initial performance .........................55
Figure 4-8: High resolution SEM images of nano-structured fresh Pt electrode before
running (top (a) and tilted (c) views), and after running
chronoamperometrically for 12 hours at 500oC (top (b) and tilted (d)
xvii
views). Clearly, nano-structured Pt does not show any major morphological
change and the TPBs are well conserved after long operation ........................57
Figure 4-9: V-I-P comparison of SOFC at 450oC employing DC sputtered porous Pt
electrode versus nano-pore structured Pt electrode at the cathode ..................58
Figure 4-10: Nano-pore structured dense Pt electrode with different final pore sizes
and TPB density, (a) 300nm, (b) 400nm. SEM images were taken with the
same magnification and the image with smaller initial particle size shows
denser pores, which relates to increased TPB density .....................................61
Figure 4-11: (a) Fuel cell I-V measurement of SOFC samples at 450oC with structured
electrode with different pore diameters. (b) V-I-P plot where current is
normalized by TPB density. The plots overlay in good registry especially in
the activation regime as expected, and indicates that fuel cell performance
scales with TPB density ...................................................................................62
Figure 4-12: EIS Nyquist spectra of SOFC samples featuring nano-pore structured
dense Pt cathodes with different TPB densities ..............................................64
Figure 4-13: (a) Schematic of the TPB. (b) Cross-section image showing TPB width .....65
Figure 4-14: Graphical estimation of electrode/electrolyte interface resistance as the
TPB density increases. Interface resistance will be decrease as we increase
the TPB density by decreasing the pore size since we are introducing more
electrochemical reaction site. If the TPB width overlap starts, the resistance
will not decrease anymore and will show saturation behavior ........................68
Figure 4-15: SEM images of nano-pore structured Pt electrodes on single crystalline
YSZ substrates. TPB linear density was estimated by measuring the pore
size and spacing between the pores. As we have smaller pore size, we have
larger TPB density. The electrode pore sizes are (a) 240nm, (b) 350nm, (c)
430nm, and (d) 570nm .....................................................................................69
Figure 5-1: (a) Change in energy as a function of height for atomic oxygen diffusing
into a vacancy in the first layer of YSZ. Height and energy is referenced to
the stable adsorbed state. Charge, plotted on the right axis, is the electron
density integrated within a Wigner Seitz sphere of radius 0.82Å around the
xviii
radius (a more positive value corresponds to higher electron density). (b)
Snapshots of atom structure as oxygen is incorporated. Oxygen atoms are
shown in red, Y in yellow, Zr in purple, and Pt in silver .................................86
Figure 5-2: (a) Change in energy as a function of height for atomic oxygen diffusing
into a vacancy in the first layer of YDC. Height and energy is referenced to
the stable adsorbed state. Charge, plotted on the right axis, is the electron
density integrated within a Wigner Seitz sphere of radius 0.82Å around the
radius. (b) Snapshots of atom structure as oxygen is incorporated. Oxygen
atoms are shown in red, Y in yellow, Ce in blue, and Pt in silver ...................87
Figure 5-3: XRD patterns of PLD YDC films deposited on single crystalline YSZ
(100) substrate. Spectra show only (100) peak up to the film thickness of
130nm, which indicates perfect epitaxial growth of YDC films .....................89
Figure 5-4: I-V performance of YDC interlayered SOFC and YSZ-only control sample
measured at 450oC. The plot shows gradual performance enhancement up
to about 50nm of YDC interlayer thickness, beyond which the fuel cell
performance remains unchanged with increasing YDC thickness ..................90
Figure 5-5: EIS data of YDC interlayered fuel cell measured at different cell voltage
conditions at 400oC. Two loops are observed. The high frequency loop
seems to be independent of cell voltage, indicating that this arc corresponds
to ionic transport through the electrolyte (Rohmic). In contrast, the low
frequency loop is dependent on cell voltage indicating that this arc
corresponds to the electrode interface resistance (Relectrode) .............................91
Figure 5-6: Extracted ohmic resistances of YDC interlayered SOFCs for different
YDC thicknesses at temperatures of 350oC~450
oC. Zero in the x-axis
indicates the bare YSZ sample with no interlayer. The plot shows no
discernable change in cell ohmic resistance with increasing interlayer
thickness up to 130nm .....................................................................................94
Figure 5-7: Electrode interface resistance values for the YDC interlayered SOFCs with
different thicknesses extracted from impedance measurements. The
resistance starts to drop immediately after the introduction of a thin layer
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YDC (<10nm). After forming a full covered YDC layer, the electrode
resistance reaches a plateau, and does not change with further increase in
YDC thickness .................................................................................................94
Figure 5-8: AFM scanned surface topography images of YDC interlayers with
different thicknesses. (Left) Bare single crystalline YSZ, (Center) ~14nm
YDC, (Right) ~80nm YDC on top of YSZ. It shows grain formation as the
YDC thickness increases..................................................................................96
Figure 5-9: Surface sensitive XPS analysis of surface modified samples with three
different YDC thickness within the binding energy regime of one of the
main Zr peaks. As the YDC interlayer thickness increases Zr peak
decreases and at the thickness about 26nm, almost no Zr peak is observed ....97
Figure 5-10: (a) Surface SEM image of YDC sintered pellet, where dashed line shows
clear grain boundaries. (b) 18
O/16
O concentration map of corresponding
YDC surface obtained from NanoSIMS. 18
O/16
O count ratio was observed
higher at grain boundary regions (dashed) than bulk regions indicating
oxygen isotopes were more populated in grain boundary regions .................100
Figure 5-11: AFM images of YDC surface additionally deposited on polycrystalline
YSZ substrate and post-annealed at different temperatures. (a) 750oC, (b)
1100oC, (c) 1300
oC, and (d) 1500
oC ..............................................................101
Figure 5-12: Average grain size of YDC interlayer as a function of post-annealing
temperature ....................................................................................................102
Figure 5-13: Current-Voltage (I-V) behavior of fuel cell MEAs measured at 400oC.
Fuel cells with smaller surface grain size show higher performance in terms
of peak power densities ..................................................................................104
Figure 5-14: Electrochemical impedance spectroscopy (EIS) data of 1500oC annealed
YDC/YSZ composite fuel cell sample measured at 350oC indicating three
loops. The two high frequency loops seem to be independent of cell voltage
conditions, indicating that these arcs correspond to ionic transport through
electrolyte and representing bulk (arc I) and grain boundary (arc II)..
whereas the low frequency loop shows dependence on cell voltage
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conditions indicating that this arc corresponds to the electrode interface
resistance ........................................................................................................105
Figure 5-15: A plot showing extracted electrode interface resistances (at 450oC, 0.6V)
as a function of estimated surface grain boundary densities. As expected,
the electrode resistance decreases as the surface grain boundary density
increases (lower grain sizes) ..........................................................................106
Figure 5-16: Exchange current densities for all measured samples with different grain
sizes were calculated at temperatures 350oC-450
oC. As the surface grain
size decreases (i.e., higher grain boundary density), the electrode interface
resistance decreases. This indicates that the surface grain boundaries
enhance oxygen surface kinetics at the cathode side .....................................108
Figure 5-17: X-ray diffraction patterns of (a) epitaxial and (b) fully developed
polycrystalline GDC films on single (100) and polycrystalline YSZ
substrates, respectively ..................................................................................110
Figure 5-18: Current-voltage (I-V) behavior of epitaxial GDC interlayered MEA,
measured at 450oC. The SOFC MEA with GDC interlayer shows about 2-
fold higher peak power density ......................................................................111
Figure 5-19: Atomic force microscopy (AFM) topography images of GDC surfaces,
annealed at (a) 750oC, (b) 1200
oC, and (c) 1450
oC. As the post-annealing
temperature increases, the grain size also increases ......................................112
Figure 5-20: I-V performance at 450oC of GDC/YSZ composite electrolyte MEAs
with different GDC surface grain sizes,. The smaller surface grain size
sample (lower annealing temperature), which corresponds to the higher
surface grain boundary density, shows higher peak power density ...............114
Figure 5-21: Arrhenius plot of cathodic interfacial resistances of MEAs with different
GDC surface grain sizes. As the post-annealing temperature increases (i.e.,
as the surface grain boundary density decreases), the electrode interfacial
resistance increases. MEAs with nano-granular GDC surface grains show
lower electrode interfacial resistances than those with larger surface grain
size .................................................................................................................115
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Figure 6-1: Schematic illustration of the NSP processing sequence for the fabrication
of 3-D crater patterned freestanding fuel cell MEAs. (a) Si substrate. (b)
Silica particles with Al layer on Si wafer. (c) Al mask after removing the
particles. (d) Formation of trenches by RIE etching. (e) Silicon nitride
deposition. (f) Removal of Si template by KOH etching. (g) Depositing
BYZ and removal of the nitride layer by dry etching. (g) Sputtering of
porous Pt catalyst/electrode (dots) deposited on both sides (h) .....................125
Figure 6-2: SEM images of, (a) silicon nano-trenches after removal of spherical
particles, (b) silicon nano-trench structure created after gas phase etching,
(c) free-standing 3-D nitride template after removing the backside silicon
by KOH etching .............................................................................................128
Figure 6-3: SEM images of the crater patterned BYZ fuel cell MEA, (a) after BYZ
deposition on the 3-D nitride template, (b,c) after porous Pt electrodes are
coated on both sides of the membrane, and (d) finished 3-D BYZ MEA
taken from an angle of 52o from the top (d) ..................................................129
Figure 6-4: Cross sectional HRTEM images ((a) and (c)) showing the dense columnar
grain structure, and, (b) the SAD pattern indicating the fully developed
polycrystalline nature of the BYZ film .........................................................131
Figure 6-5: (a) Electrochemical impedance spectra at 400oC at cell voltages of 0.9V
and 0.7V, with inset showing the details of the high frequency region, and
(b) voltage-current-power density (V-I-P) behavior of 3-D crater patterned
BYZ fuel cells measured at 350-450oC using hydrogen fuel .......................133
Figure 6-6: Compositional depth profiles of the PLD BYZ film ....................................136
Figure 6-7: The high resolution C1s
spectra show two peaks at ~285.0eV and ~289.9eV
assigned to surface contamination and to CO32-
(possibly in the form of
BaCO3) environment, respectively ...............................................................136
Figure 7-1: Conductivity measurement setup with microcontacting probes connected
to the EIS software ........................................................................................147
Figure 7-2: XRD patterns of BYZ thin films grown on quartz substrates (Q) with
different deposition temperatures (a) 900oC, (b) 700
oC, and (c) 400
oC .......148
xxii
Figure 7-3: XRD patterns of BYZ thin films grown on MgO(100) substrates with
different deposition temperatures (a) 900oC, (b) 800
oC, (c) 700
oC, and (d)
600oC .............................................................................................................149
Figure 7-4: High resolution TEM image: {001} planes of BYZ (perovskite structure)
grows epitaxially on {001} type planes of MgO (rocksalt structure). A
yellow-dotted rectangle shows dimensional matching of each MgO and
BYZ unit cell .................................................................................................151
Figure 7-5: Selected area diffraction (SAD) patterns of BYZ films deposited by PLD
at 900 °C (a series at top) and at 600 °C (b series at bottom): Both a-1 and
b-1 SAD patterns were taken only from MgO for setting orientation
standard. Both a-2 and b-2 SAD patterns were taken from MgO and BYZ
to check orientation relationship of BYZ films to MgO substrate. BYZ film
deposited by PLD at 900 °C (a-2) shows epitaxial growth, unlike BYZ film
deposited by PLD at 600 °C, which illustrates slight disorientation. A
digitally 4X magnified SAD of 200 type spots (b-3) confirms orientation
mismatch of each film ...................................................................................152
Figure 7-6: Bright Field (BF), Dark Field (DF), High Resolution (HR) TEM images
and SAD pattern of BYZ films deposited by PLD at 600 °C on Quartz:
Both BF (a) and DF (b) images show visual orientation difference of each
BYZ grain. HRTEM (c) shows polycrystallinity of BYZ films with grains
and grain boundaries. And SAD pattern only taken from BYZ indicates
randomly-oriented of polycrystalline BYZ grains ........................................154
Figure 7-7: Measured Nyquist impedance plots and fitting curves to the parallel R//C
circuit model. (a) BYZ-MgO(100) sample deposited at 900oC and
measured at 200oC. Bias independence of the spectra indicates that the
semicircle is associated with electrolyte impedance. (b) BYZ film
deposited on quartz at 400oC and measured at 700
oC ..................................157
Figure 7-8: EIS data measured at different temperatures for BYZ-MgO(100) film
deposited at 900oC ........................................................................................158
xxiii
Figure 7-9: Arrhenius plot showing the conductivity values of BYZ thin films
deposited on MgO(100) and amorphous quartz substrates at different
deposition temperatures. In addition, both sets of data are compared with
the reference conductivity values from the literature, including bulk and
experimentally obtained non-epi references .................................................159
Figure 7-10: Variations in the SAD patterns obtained from a cross-section sample of
MgO (100)/BYZ film (deposited by PLD at 700°C) as the SAD aperture
position is moved from MgO into the BYZ film: SAD aperture positioned
on MgO only (a), 20nm into BYZ from MgO interface (b), 40nm into BYZ
from MgO interface (c), and 100nm across the entire BYZ (d). Digitally 4X
magnified SAD patterns of 101 spots from Figure 7-10-b, c & d are shown
in Figure 7-10-e, and indicate how the epitaxy in the BYZ film near the
MgO substrate gradually changes to increasing polycrystallinity with wider
divergence in orientation as the aperture moves towards upper regions of
the BYZ film. The ranges selected for SAD patterns are indicated on the
cross-sectional bright field TEM image of Figure 7-10-f using a color
scheme (white for a, blue for b, green for c, and orange for d) ....................162
Figure 7-11: Plot showing the conductivity versus degree of crystallinity of BYZ-
quartz samples with three different deposition temperatures. Error bars are
included for one measured temperature data since all three samples have
the same error bars. The plot indicates that as the deposition temperature
increases the degree of crystallinity and the conductivity increases .............165
1
CHAPTER 1. Introduction
1.1 Dissertation Overview
Due to the scarcity of fossil fuels and their environmental pollution from carbon dioxide
(CO2) emission, interest in renewable and clean energy resources of all forms is very
high. Renewable energy resources such as solar and wind energy have been considered
as strong candidates, but both sources have the inherent problem of irregularity. Using
hydrogen as an energy carrier, fuel cells can be considered as a renewable energy and a
good sustainable energy resource.
Fuel cells are environmentally friendly energy conversion and power generation devices,
and some of the most promising candidates as a zero-emission power sources. Among the
fuel cells, ceramic fuel cells such as solid oxide fuel cells (SOFCs) and proton conducting
oxide fuel cells (PCOFCs) have attracted recent attention due to their high energy
conversion efficiency. However, the ceramic fuel cells especially SOFCs usually have
high operating temperatures (800~1000oC) due to the nature of the high activation energy
(~1eV) of ionic transport in such solid ceramic electrolytes [1-2]. This high operating
temperature limits a wide range of practical applications. It is therefore desirable to
reduce the operating temperature of SOFCs to lower than 500oC. Unfortunately, in this
2
low temperature regime, two critical factors become much more pronounced and
adversely affect the performance of low-temperature SOFCs (LT-SOFC). One is
increased ohmic resistance due to slower ionic transport through the YSZ electrolyte at
these temperatures. The other is similarly increased activation losses mostly due to the
slower kinetics of the oxygen reduction reaction at the cathode interface, and it is known
that this increase in activation energy is more severe than the increased ohmic resistance
[1-2].
To compensate for the increased ohmic resistance, many studies have sought to develop
materials having high conductivity and to reduce the electrolyte thickness [3-8]. Although
the use of thin film electrolytes mitigated ohmic losses, the electrode polarization
process, which is highly related to the electrochemical surface reactions, still remains a
key challenge at these low operating temperatures (300~500oC) due to the high activation
energy (>1.5eV) of oxygen reduction reaction. Recently, nanoscale engineering has been
intensively investigated in such energy conversion devices, and it became available from
the development of technologies for fabrication and characterization of materials in
nanometer, or even smaller, scale. In nanoscale, the increase of surface-to-volume ratio is
dramatic, and the material properties can also be changed from the macro-scale.
Therefore, by nanoscale engineering superior and/or unique material properties, which
can enhance the surface reaction kinetics, we can significantly improve the performance
of energy conversion devices.
3
This dissertation discusses nanoscale surface engineering approaches to reduce the
remaining activation loss issue for improving the performance of low temperature
ceramic fuel cells. First, a novel fabrication method for nano-structured electrodes was
developed to understand the geometry of the electrochemically active zone for solid
oxide fuel cells and to maximize the reaction sites. Second, a composite electrolyte was
fabricated using cathodic interlayers, which have higher ionic conductivity and superior
surface activity to increase electrochemical surface reaction rate. The third approach is
the fabrication of a three-dimensional ceramic fuel cell structure to improve the
performance by increasing the effective surface reaction sites in a given area.
1.2 Outline
The main body of this thesis contains 6 chapters. The first two chapters provide
fundamental backgrounds for the works in the dissertation. The following 4 chapters
present the research focused on improving the performance of ceramic fuel cells by the
nanoscale engineering of electrochemical reaction surfaces.
Chapter 2 describes the scientific and theoretical overview of fuel cell operation,
fuel cell types, fuel cell performance characteristics, and ceramic fuel cell basics.
4
Chapter 3 describes basic materials science of ceramic electrolytes including the
fundamental ion transport mechanism and exemplary materials for each type of
ionic conductors. It also provides the basics of pulsed laser deposition as a
technique for depositing those materials.
Chapter 4 introduces a novel fabrication method for nano-pore structured metal
electrodes and the investigation of the electrochemically active zone for fuel cell
operation.
Chapter 5 describes the fabrication of YSZ-based composite electrolytes using
YDC and GDC cathodic thin interlayers to enhance surface oxygen kinetics for
low temperature SOFCs.
Chapter 6 introduces a method for fabricating three-dimensional proton
conducting ceramic fuel cell electrolyte structures to increase effective reaction
sites at a given area.
Chapter 7 describes the effect of crystallinity on proton conductivity in BYZ thin
films as proton conducting ceramic electrolytes.
5
1.3 Individual/Group Research Statement
Much of the work presented here was accomplished in collaboration with outstanding
group members in the Nanoscale Prototyping Laboratory (NPL). Professor Fritz B. Prinz,
who is the principal investigator (PI) of the research group, highly encourages a
cooperative research environment and teamwork-based scientific research to expedite the
progress. The group members, having their own specialties, are highly involved in one
research project. Therefore, the lively discussions and cooperation for experiments with
all NPL members have been priceless throughout the research in this dissertation.
The initial fabrication works for the nano-pore structured layer were performed in
collaboration with Dr. Steve Connor and Ching-Mei Hsu. Dr. Pei-Chen Su and I came up
with the idea of using that structure as fuel cell electrodes. I designed and performed the
series of experiments to study structural stability of the nano structured metal electrodes
and to investigate the electrochemical reaction sites for solid oxide fuel cells.
The PLD of BYZ thin film work was initiated by Prof. Joon Hyung Shim. For further
development of PLD BYZ and other materials used for the experiments in this thesis such
as YDC and GDC, I explored the deposition conditions and characterization of the thin
films. Based on the deposition conditions, I designed and performed the doped ceria
cathodic interlayered SOFC experiments (Chapter 5).
6
The DFT simulations for calculating the oxygen incorporation energy of Pt/YSZ, Pt/YDC
systems were designed and performed by Dr. Tim Holme. The oxygen isotope exchange
experiment YDC bulk substrate was performed by Joong Sun Park (Chapter 5).
Microscale three-dimensional (3-D) SOFC fabrication by the MEMS process was
initiated by Dr. Pei-Chen Su. On this 3-D fabrication concept, I designed a nanoscale 3-D
proton conducting ceramic fuel cell by developing a novel fabrication process using
nanosphere lithography (NSL). All the TEM works (Chapter 6 and 7) were performed by
Hee-Joon Jung.
In all ceramic fuel cell experiments, I fabricated the fuel cell samples and characterized
their electrochemical performances. Much of this work has been previously presented at
conferences and/or published in scientific journals. References to the work stemming
from this thesis are provided in context throughout the dissertation. Any inaccuracies or
errors in this dissertation are wholly my responsibility.
1.4 References
[1] B. C. H. Steel, A. Heinzel, Nature, 414, 345–352 (2001)
[2] N. P. Brandon, S. Skinner, B. C. H. Steele, Annu. Rev. Mater. Res., 33, 183–213
(2003)
7
[3] U. P. Muecke, D. Beckel, A. Bernard, A. Bieberle-Hutter, S. Graf, A. Infortuna, P.
Muller, J. L. M. Rupp, J. Schneider, L. J. Gauckler , Adv. Funct. Mater., 18, 3158–
3168 (2008)
[4] P.-C. Su, C.-C. Chao, J. H. Shim, R. Fasching, and F. B. Prinz, Nano Lett., 8, 2289
(2008)
[5] J. H. Shim, C.-C. Chao, H. Huang, and F. B. Prinz, Chem. Mater., 19, 3850 (2007)
[6] H. Huang, M. Nakamura, P. Su, R. Fasching, Y. Saito, and F. B. Prinz, J.
Electrochem.Soc., 154, B20 (2007)
[7] H. Huang, T. M. Gür, Y. Saito, and F. Prinz, Appl. Phys. Lett., 89, 143107 (2006)
[8] A. Evans, A. Bieberle-Hutter, J. L.M. Rupp, L. J. Gauckler, Journal of Power
Sources, 194, 119–129 (2009)
8
CHAPTER 2. Fuel Cell Overview
This chapter describes fundamental backgrounds and technological progresses of fuel
cells based on literatures [1, 2].
2.1 Fuel Cell Basics
A fuel cell is an electrochemical device that directly converts the chemical energy of
reactants into electrical energy. Electricity is generated from the electrochemical
reactions between reactants (fuels) and oxidants. Fuel cells are often compared with other
energy conversion devices such as batteries and combustion engines. Batteries store
electric energy chemically and generate electricity by similar electrochemical reactions to
fuel cells. One of the key differences between fuel cells and batteries is the source of
reactants. Batteries produce a certain amount of electricity based on the maximum
capacity of the battery materials and the designed systems. In contrast, fuel cells consume
a reactant from an external source and generate electricity as long as fuel (reactant) is
supplied. Also, heat engines inevitably suffer from heat losses through multiple
conversions during combusting fuels for electricity generation. However, fuel cells
extract electricity from fuels in the shortest and most efficient way.
9
Figure 2-1. Schematic of a typical hydrogen-oxygen fuel cell
Typically, a fuel cell is composed of three active components which are an electrolyte, an
anode (a fuel electrode), and a cathode (an oxidant electrode). Figure 2-1 shows a
schematic of fuel cell membrane electrode assembly (MEA) and illustrates the basic
operational principle of fuel cells for both proton and oxide ion conducting electrolytes.
To generate electricity for fuel cells, electrons can be extracted directly from fuels
through electrochemical reactions and flow through the external circuit load while ions,
either protons (H+) or negative oxide ions (O
2-), internally transport across the electrolyte.
Assuming that fuel cells run on hydrogen fuel using a proton conducting electrolyte
membrane, the following reactions take place during the operation. Hydrogen (H2) is
10
delivered to the anode and at the anode/electrolyte interface the hydrogen oxidation
reaction (HOR) happens as follows:
eHH 222 (2.1)
The generated protons are transported through the proton conducting electrolyte. At the
cathode side, transported protons and electrons react with the supplied oxygen forming
water:
OHeHO 22 222
1
(2.2)
This is a basic mechanism of electricity generation in proton conducting H2-O2 fuel cells.
11
2.2 Types of Fuel Cells
Table 2-1. Characteristics of five major fuel cell types [1].
PEMFC PAFC AFC MCFC CFC
Electrolyte Polymer
membrane
Liquid
H3PO4 Liquid KOH
Molten
Carbonate Ceramic
Charge
carrier H
+, H3O
+ H
+ OH
- CO3
2- H
+, O
2-
Operating
temperature 80
oC 200
oC 60-200
oC 650
oC 600-1000
oC
Fuel
compatibility H2, methanol H2 H2 H2, CH4 H2, CH4, CO
Fuel cells may be categorized or classified in a variety of different ways depending upon
the criteria used. Those are typically the parameters related to fuel cell design and
operation such as the type of electrolyte, the type of ion transferred thorough the
electrolyte, the type of reactants, and so on. Generally, fuel cells are categorized by the
type of electrolyte used since the material properties of the electrolyte usually determine
the properties of fuel cells, including the species of ionized charge carriers, the operation
principle and the design. There are five major types of fuel cells, differentiated from one
another by the electrolytes: the phosphoric acid fuel cell (PAFC), the polymer electrolyte
membrane fuel cell (PEMFC, this often refers to the proton exchange membrane fuel
cell), the Alkaline fuel cell (AFC), the molten carbonate fuel cell (MCFC), and the
ceramic fuel cell (CFC).
12
Fuel cells’ target operating conditions and their applications are critical factors for
determining the type of fuel cells to use. PAFC is a type of the acid-electrolyte fuel cells,
and, as the name implies, it uses phosphoric acid (H3PO4) as its electrolyte. A PAFC
normally operates at temperatures of around 170oC~210
oC. PEMFC employs the proton-
conducting polymer electrolyte membrane, usually the sulfonic acid polymer, or
NafionTM
. It has a fairly low operating temperature range, and thus it is suitable for
portable applications. However, there is a water management issue. The operating
temperature of the PEMFC is limited to 90oC or lower because the polymer membrane
must be hydrated with liquid water to maintain decent proton conductivity. The AFC
employs an aqueous potassium hydroxide (KOH) electrolyte. Depending upon the
concentration of KOH in the electrolyte, the AFC can operate at temperatures between
60oC and 220
oC. The MCFC operates at higher temperatures (~650
oC) than the fuel cells
described above. The MCFC uses a molten mixture of alkali carbonates as an electrolyte
material, and the carbonate ion (CO32-
) acts as the mobile charge carrier. The CFC
employs solid ceramic electrolytes, which can conduct an oxide ion (O2-
) or a proton (H+)
as a mobile charge carrier. The operating temperature of the SOFC is typically between
600oC and 1000
oC. As the CFCs are the subject of this dissertation, they will be
discussed in more detail below.
13
2.3 Fuel Cell Performance and Loss Mechanisms
The performance of a fuel cell device is usually evaluated with a graph of its current-
voltage characteristics. This graph is a fuel cell polarization behavior curve, or current-
voltage (I-V) curve, showing the voltage output of the fuel cell for a given current output.
The maximum voltage is determined by the difference between intrinsic chemical
potentials of the reactant and the oxidant. It is achieved when the fuel cell is operated
under the thermodynamically reversible condition. This maximum possible cell potential
is called reversible cell voltage or thermodynamic fuel cell voltage. As the current is
drawn from the fuel cell, the output voltage starts to decrease from the reversible cell
voltage. This voltage drop characterizes the irreversible losses in a fuel cell operation.
The more current is drawn, the greater these losses. There are three major types of fuel
cell losses, which give a fuel cell I-V curve its characteristic shape:
1) Activation loss (ηact) from the electrochemical reaction kinetics at the
electrode/electrolyte interface
2) Ohmic loss (ηohmic) from ionic transport thorough the electrolyte
3) Concentration loss (ηconc) due to the mass transport of fuels and oxidants to the
reaction sites
Therefore, the real voltage output for a fuel cell is the reversible cell voltage minus the
voltage drops due to these losses:
14
concohmicactthermoEV (2.3)
where V is the actual fuel cell voltage, Ethermo is the thermodynamic reversible voltage,
ηact is the activation overpotential, ηohmic is the ohmic overpotential, and ηconc is the
concentration overpotential.
Figure 2-2 shows a typical fuel cell I-V curve indicating each type of loss described
above. As shown in the figure, the activation losses mostly affect the low current region
of the curve. The ohmic losses are most apparent in the middle region of the curve and
the concentration losses are significant when a fuel cell draws a large amount of current.
The power density values can be calculated by simply multiplying the voltage and the
current density values.
15
Figure 2-2. Schematic of a typical fuel cell current-voltage (I-V) curve.
2.3.1 Thermodynamic Reversible Voltage
As previously mentioned, the maximum voltage which can be obtained for a given fuel
cell can be determined by the chemical potential difference of the species. Chemical
potential measures how the Gibbs free energy of a system changes as the chemistry of the
system changes. Chemical potential of a chemical species is expressed as follows:
iii aRT ln0 (2.4)
16
where 0
i is the reference chemical potential of species i at standard-state conditions, R
is the ideal gas constant, T is absolute temperature, and ia is the activity of species i. ia
characterizes relative concentration of species involved in a reaction of interest. The
chemical potential energy is interchangeable with a voltage as in (2.5), and changes in
Gibbs free energy for a system of i chemical species is expressed as in (2.6):
nFE (2.5)
i i
iiiii dnaRTdndG )ln( 0 (2.6)
Assume that we have a hydrogen-oxygen fuel cell system. Then, the fuel cell reaction of
the system is expressed as follows:
)()(2
1)( 222 lOHgOgH (2.7)
Using the relationship in (2.6), we can calculate the Gibbs free energy change by
inserting the chemical potentials of species involved in the reaction above and subtracting
the reactant terms from the product terms. Combining the result with equation (2.5)
allows us to estimate the thermodynamic reversible cell voltage as a function of the
chemical activity of the species:
17
2/1
0
22
2lnOH
OH
thermoaa
a
nF
RTEE (2.8)
where n is the number of charges transferred in a given reaction (n=2 in this case) and F
is Faraday constant. The term 0E contains standard state chemical potentials and refers
to the standard state reversible voltage, which is not affected by temperature.
This result is known as the Nernst equation. The Nernst equation outlines how reversible
electrochemical cell voltages vary as a function of species concentration, gas pressures,
and so on. For a general case, the Nernst equation is written as:
i
i
tsreac
products
a
a
nF
RTEE
tan
0 ln (2.9)
where i represents the stoichiometric coefficient of the activity of each species.
Therefore, if we know the operating temperature and partial pressure of the reactant
species we can calculate the thermodynamic reversible voltage. For instance, if we
operate a H2-O2 fuel cell at standard conditions (298K, using 1atm air at the cathode
side), the reversible voltage is 1.219V where 0E is 1.229V for the hydrogen-oxygen fuel
cell under standard state conditions. Hence, the theoretical maximum reversible voltage
that we can achieve from the H2-O2 fuel cell, running at 298K and ambient air condition,
is 1.219V.
18
2.3.2 Activation Losses
The activation losses associated with a fuel cell are mainly due to the overpotential
necessary to drive the electrochemical reactions occurring at the electrodes. These
activation losses usually come from the electrochemical reactions at the
electrode/electrolyte interface. These losses are referred to as ‘activation’ losses because
they are the losses (overpotentials) required to ‘activate’ or drive the chemical reactions
from their equilibrium state to the forward direction. The electrochemical reaction rate
depends on the probability of the surface reaction, and the probability ( RTGeP / ) is
exponentially dependent on the size of the activation barrier or the Gibbs energy barrier
( G ) and the temperature. The reaction rate can be expressed as follows:
RTG
R efcJ/
1
*
11
(2.10)
where J1 is the reaction rate (mol/s) in the forward direction (reactants → products), *
Rc is
the reaction surface concentration, and 1f is the decay rate to the products. The decay rate
characterizes the lifetime of the activated species and the possibility that it will convert to
a product instead of back to a reactant. The exchange current density (j) can be obtained
from the reaction rate J from the relationship of nFJj . Therefore, the forward current
19
density and the reverse current density (j2, products → reactants) can be expressed as the
following equations:
RTG
R efnFcj/
1
*
11
(2.11)
RTG
P efnFcj/
2
*
22
(2.12)
At thermodynamic equilibrium, the forward and reverse current densities must be in
balance ( 21 jj ), and there is no net current density. In other words, at equilibrium, we
have:
021 jjj (2.13)
This equilibrated current is called the exchange current density ( 0j ) for the reaction.
When a net current is produced from the electrode reaction, the electrode reaction
becomes irreversible and an imbalance of electron transfer exists. The net amount of
current flow to the electrode depends on the extent to which the potential at the electrode
differs from its equilibrium value. This electrode potential difference is defined as the
overpotential of the electrode reaction ( act ). This activation overpotential changes the
dependency of the current density on Gibbs free energy barrier:
20
)exp( 11
*
1RT
nFGfnFcj act
R
(2.14)
))1(
exp( 22
*
2RT
nFGfnFcj act
P
(2.15)
where the parameter α is called the transfer coefficient (or symmetry factor); theoretically
the value lies between 0 and 1. Using the exchange current density shown above, the
equations (2.14) and (2.15) can be expressed as:
)exp(01RT
nFjj act
(2.16)
))1(
exp(02RT
nFjj act
(2.17)
Therefore, the net current is:
)])1(
exp()[exp(021RT
nF
RT
nFjjjj actact
(2.18)
This is the Butler-Volmer equation, representing the general relation between the net
current density produced and the activation overpotential act . When the electrode
overpotential is large, the backward reaction is negligible compared with the forward
21
reaction because the second term in equation (2.18) becomes much smaller than the first
term. Hence, the Butler-Volmer equation can be reduced to
)exp(0RT
nFjj act
(2.19)
or
)ln(0j
j
nF
RTact
(2.20)
which is the well-known Tafel equation, one of the fundamental relations in
electrochemistry, representing the activation overpotential as a function of the current
density. Reducing the activation loss is one of the main objectives in this dissertation. As
shown in the equation (2.20), we can reduce the activation loss by increasing the
exchange current density ( 0j ), which is highly related to the electrochemical surface
reaction rate. Various approach and study results to enhance the surface reactions will be
introduced in later chapters (Chapter 4–6).
2.3.3 Ohmic Losses
22
The ohmic losses associated with the fuel cell operation are mainly due to the resistance
of ionic transport through the electrolyte component. They are simply governed by
Ohm’s law:
A
LiiRV (2.21)
where A is fuel cell reaction area, L is the length of the ionic transport path (normally,
thickness of the electrolyte), and σ is the ionic conductivity of the electrolyte material. In
this equation, the voltage V represents the voltage, which must be applied in order to
transport charge at a rate given by i. Thus, this voltage represents a loss. Generally,
current density value is used to compare fuel cell performance instead of current.
Therefore, it is reasonable to use area-normalized fuel cell resistance, which is known as
area-specific resistance (ASR). The equation (2.21) can be re-written using the ASR and
current density, Aij / :
L
jASRjohmic (2.22)
As shown in the equation above, we can decrease the ohmic loss either by reducing the
electrolyte thickness or by using an electrolyte material with high ionic conductivity.
23
2.3.4 Mass Transport Losses
Another source of loss in some fuel cells is known as the mass transport loss, or
concentration loss ( conc ). The concentration loss is caused by a number of processes that
hinder the transport of mass. Generally, the low solubility of reactants in the electrolyte
and the slow diffusion of reactants through the electrolyte constitute the major
contribution to the concentration loss. This can be characterized as a function of the
limiting current density ( Lj ) that represents the maximum current density drawn in the
case of consuming the full amount of supplied reactants at equilibrium:
jj
j
nF
RT
L
Lconc
ln (2.23)
And this limiting current density, Lj , can be expressed as follows:
0
Reff
L
cnFDj (2.24)
where effD is the effective diffusivity of the reactants at the electrode/electrolyte
boundaries, 0
Rc is the bulk reactant concentration, δ is the diffusion length through the
electrode. In designing a fuel cell, a large Lj helps save energy due to the mass transport.
24
To maximize the limiting current density, it is necessary to optimize electrode structure to
minimize the gas depletion effect so that the reactant is consistently high across an entire
fuel cell device as well as having an effective fuel delivery scheme (low δ).
2.4 Ceramic Fuel Cells
A ceramic fuel cell (CFC) is an all-solid-state energy conversion device and usually
refers to fuel cells employing solid ceramic electrolytes [3]. The present generation of
ceramic fuel cells can be classified into two types. One is based on oxygen ion
conducting electrolytes (SOFC), and the other one is based on proton conducting
electrolytes (PCFC or PCOFC). The main difference between the two CFC types is the
side in the fuel cell in which water is produced (the fuel side in SOFC and the oxidant
side in PCFC). Also, certain gases, such as CO, can be used as fuel in SOFCs but not in
PCFCs. CFCs usually have the highest operating temperature of all fuel cells at about
600~1000oC. It is mainly due to the significantly lower ionic conductivity of solid state
electrolytes (ceramic electrolytes) as compared to polymer membranes. Thus, the most
practical application of CFCs so far is stationary devices such as on-site electricity
generators. However, there have been many recent efforts to reduce this high operating
temperature by using new electrolyte materials or by having smartly engineered fuel cell
structures for a wider range of practical applications for CFCs. Since the CFCs usually
operate at high temperatures, liquid production is not a problem, unlike with other types
25
of fuel cells using polymer-based or liquid-based electrolytes. For this reason, CFC is
free of the severe chemical degradation of cells, which comes from corrosive liquid. This
eliminates the intermediate step of producing hydrogen through the costly reforming
process when using other types of fuels such as hydrocarbons. Also, the rigidity of the
ceramic components enables flexible design of three-dimensional fuel cell structures such
as tubular and corrugated SOFCs while other types of fuel cells are made mostly in the
two-dimensional planar format.
As previously mentioned, solid oxide fuel cells use oxygen ions as charge carriers and
therefore use an oxygen ion conducting ceramic as an electrolyte. The most popular
electrolyte material is Yttria-stabliized zirconia (YSZ), which is a doped cubic fluorite
type oxide. The dopant has different charges to its host cation, and for the charge
neutrality, it produces oxygen vacancies. Through these oxygen vacancies, oxygen ions
transport in the electrolyte. The oxide ion conducting electrolytes will be discussed in
detail in the next chapter (Chapter 3). At the cathode, the oxygen dissociates into oxygen
ions when combined with electrons from a connected external circuit. The ionized
oxygen ions transport through the electrolyte and form water by combining with
hydrogen at the anode side. The half reactions at the anode and cathode sides are:
2
2 22
1OeO (cathode) (2.25)
eOHOH 22
2
2 (anode) (2.26)
26
The cathode reaction is known as the oxygen reduction reaction (ORR) since the
electrodes are consumed by the reaction. The anode reaction is known as the hydrogen
oxidation reaction (HOR) since the electrons are released as a product. Generally, it is
agreed that the activation loss for SOFC mainly comes from the ORR due to its sluggish
process.
As previously mentioned, the high operating temperature of SOFC (600~1000oC) hinders
a wide range of practical applications, and there have been efforts to reduce the SOFC’s
operating temperature (400~600oC). In this respect, proton conducting oxide fuel cells
have attracted attentions due to higher ionic conductivity at a similar temperature regime
to oxygen ion conducting ceramics. This means that we can reduce the operating
temperature and expect similar ionic conductivity when using proton conducting oxides.
Several acceptor-doped perovskite oxides have shown proton conductivity in hydrogen-
containing environments [4]. Unlike the SOFCs, product water is generated at the
cathode side in PCOFCs. The half reactions of PCOFCs are expressed as:
eHH 222 (anode) (2.27)
)(22
12 22 gOHeOH
(cathode) (2.28)
27
Even though the half reactions are same as the polymer based fuel cells, the generated
water is gas phase due to high operating temperature, and it is free from the water
management at the cathode side. Another difference from the PEMFC is the proton
conducting mechanism. For polymer-type electrolyte membranes, the hydration of the
membrane is an important factor since protons can transport as a form of H3O+, combined
with water molecules. In the case of PCOFC, protons transport through the crystal lattice
without water. Thus, once the electrolyte membrane is sufficiently protonated, a PCOFC
can operate in dry environments [4]. The proton conduction through ceramic electrolytes
will be discussed further in Chapter 3.
2.5 References
[1] R. O’Hayre, S. Cha, W. Colella, F. B. Prinz, Fuel Cell Fundamentals, John Wiley and
Sons, New York (2006)
[2] X. Li, Principles of Fuel Cells, Taylor & Francis (2005)
[3] N. Q. Minh, T. Takahashi, J. Am. Ceram. Soc., 76, 563 (1993)
[4] K. D. Kreuer, Annu. Rev. Mater. Res., 33, 333 (2003)
28
CHAPTER 3. Materials for Ceramic Electrolytes and A
Fabrication Technique
In the previous chapter, we discussed the basic fuel cell fundamentals and fuel cell types,
especially ceramic fuel cells. This chapter describes ceramic electrolyte materials for both
oxygen ion and proton conducting electrolytes. The pulsed laser deposition (PLD)
technique will be presented as a deposition method of the ceramic electrolytes.
3.1 Ceramic Electrolyte Materials
3.1.1 Oxygen Ion Conducting Ceramics
There are numerous candidate materials for SOFC electrolytes. One of the major
requirements for the electrolyte is having conductivity for oxygen ions over a wide range
of O2 partial pressures without having electronic conductivity. Another requirement is
chemical stability since the electrolytes are exposed to strongly oxidizing and reducing
environments. Also, it requires mechanical stability of the membrane over high operating
temperatures.
29
Perhaps the most conventional fast oxygen ion conducting materials have crystal
structures of fluorite type AO2, where A is a tetravalent cation [1-3]. And the best known
fluorite type oxygen ion conductor is acceptor-doped ZrO2. Pure zirconia is not a good
ion conductor. However, once acceptor dopants are introduced onto the cation sublattice,
oxygen vacancies are generated for the charge neutrality. Through these oxygen
vacancies, oxygen ions can diffuse in the crystal structure. This can be expressed using
Krӧger-Vink notation:
2
'' ZrOVMOZrMO OZr
x
O
x
Zr (3.1)
2
'
32 222 ZrOVROZrOR OZr
x
O
x
Zr (3.2)
where M is a divalent cation (i.e. Ca), R is a trivalent cation (i.e. Sc, Y, Ln), and
OV is a
compensating oxygen vacancy [3-4]. The oxygen vacancy concentration is a critical
factor which affects the ionic conductivity of the oxygen ion conducting electrolyte:
RT
RTGDzFc act )/exp()( 0
2 (3.3)
in which c is the vacancy concentration, z is the charge of the carrier (-2 for the oxygen
ions), F is the Faraday constant, D0 is the oxygen self-diffusion coefficient of the
30
material, actG is the activation energy barrier for diffusion, R is the gas constant, and T
is the absolute temperature [1].
From the equation above, the ionic conductivity increases as the vacancy concentration
increases. However, there is an upper limit to the amount of doping and beyond this limit
the conductivity starts to decrease. As we have more and more vacancies, the electrostatic
interaction between dopants and vacancies also increases. This ultimately impedes
oxygen ion and oxygen vacancy mobility. Thus, there is an optimal dopant concentration
value which yields the maximum ionic conductivity. For yttria-stabilized zirconia (YSZ),
which is the most commonly used electrolyte for SOFC, the optimum dopant
concentration is around 8 mol% [1-2].
As stated above, YSZ is arguably the most commonly used electrolyte material for SOFC
due to its superior chemical stability in both oxidizing and reducing environments.
Despite the chemical stability, YSZ has low ionic conductivity, about 0.02 S/cm at 800oC
and 0.1 S/cm at 1000oC and has high activation energy [2]. This is the main reason that
SOFCs have such high operating temperatures. To make the use of YSZ suitable for
intermediate (500~700oC) and low (300~500
oC) operating temperature regimes, there
have been efforts to decrease the electrolyte thickness [5-7] because the ionic
conductivity is a function of membrane thickness (Chapter 2).
31
Another popular oxygen ion conducting electrolyte material is doped ceria (CeO2).
Typical dopants include gadolinia (Gd2O3) and yttria (Y2O3), producing GDC and YDC,
respectively. These doped ceria have much higher ionic conductivities than YSZ,
especially at lower temperature regimes (500~700oC) and lower activation energies. For
example, 10 mol% doped GDC (Ce0.9Gd0.1O1.95) has an ionic conductivity of 0.01 S/cm
at 500oC [8]. This is why the doped ceria materials are attractive for the use of lower
operating temperature SOFC electrolytes. In addition to the higher ionic conductivity, the
oxygen surface exchange coefficient is much higher than that of YSZ [9-10]. In overall
electrode kinetics, the rate of exchange of oxygen between gas phase and the oxide
electrolyte is considered as the rate limiting step. Thus, this rate of surface exchange can
determine the performance of oxide electrolyte and electro-catalytic materials [11].
However, doped ceria materials do have a significant disadvantage in SOFC electrolyte
applications. At high temperature (above 600oC) and low oxygen partial pressure
environment, the conductivity is not purely ionic. Under reducing conditions, Ce4+
partially reduces to Ce3+
and this induces n-type electronic conductivity, which may lead
to internal electronic short circuits. As we increase the operating temperature, this
problem increases. In response to this stability issue of doped ceria materials in a
reducing environment, composite electrolytes (YDC/YSZ, GDC/YSZ) have been
investigated. By utilizing doped ceria at the cathode side and YSZ at the anode side, we
can enhance the oxygen exchange kinetics and achieve chemical stability. Investigation
32
details of these YDC and GDC cathodic interlayered SOFCs will be further discussed in
chapter 5.
3.1.2 Proton Conducting Ceramics
Proton transport in several members of acceptor-doped perovskites of the general formula
ABO3 is reported to be fast, with activation energies of about 0.45eV [12], which makes
them of interest as potential solid electrolytes for next generation protonic devices such
as fuel cells, electrolyzers, hydrogen sensors, and gas reformers [13-17]. Proton transport
in these anhydrous oxides occurs via the Grotthuss mechanism through hydroxide defects
that are produced by water incorporation into oxide ion vacancies generated in the crystal
lattice upon extrinsic doping of the tetravalent site by the trivalent ion. In Krӧger-Vink
notation, this process can be written as:
O
x
OO OHOVOH 22 (3.4)
The detailed mechanism of charge transport in proton conducting oxides was reviewed in
recent publications [ref. Kreue rev, 17-19]. The proton in a hydroxide defect,
OOH ,
resides asymmetrically in an interstitial position near the oxide ion. Because of the
softness of this dynamic hydrogen bonding between the proton and its eight nearest
oxygen neighbors, the protons are highly mobile in these cubic oxide structures, giving
33
rise to high ionic conductivities with relatively low activation energies [18-19]. Charge
transport involves protons jumping from one oxide ion to an adjacent one in the oxide
sublattice along the edges of the BO6 octahedra. Each jump is followed by a rotation of
the proton around the oxide ion to reorient itself for the subsequent jump.
Initially, the proton conductivity in doped perovskites was investigated with alkaline-
earth cerates and zirconates where the trivalent Ce4+ sites were partially substituted by
trivalent dopant cations such as Y3+
, Gd3+
, or Nb3+
. Despite the high ionic conductivity of
doped cerate perovskites, they suffer from significant chemical instability in CO2
environments. Several studies reported that SrCeO3 and BaCeO3 easily turn into SrCO3
and BaCO3 through reaction, even with a small amount of CO2 [12]. Also, it is reported
that BaCeO3 easily decomposed into Ba(OH)2 in the presence of water. In contrast,
alkaline-earth zirconates, especially Y-doped BaZrO3 (BYZ) has been considered one of
the most promising electrolyte materials for proton conducting fuel cells for their high
proton conductivity and excellent chemical stability [20]. In a later chapter (Chapter 6),
we will present the results of the fuel cell performance test with three-dimensional fuel
cell architecture design using a BYZ electrolyte. Moreover, detailed investigations of
BYZ thin film properties will be discussed later in Chapter 7.
34
3.3 Pulsed Laser Deposition
3.3.1 Background
Pulsed laser deposition (PLD) is a unique physical vapor deposition (PVD) technique
which has gained considerable attention for its good reproducibility of target material
properties such as chemical compositions. The technique uses high power laser pulses to
melt, evaporate and ionize material from the surface of a target. The vaporized or ablated
material from the target travels through a generated plasma plume and is deposited on a
substrate. Figure 3-1 shows a simple schematic of PLD system.
35
Figure 3-1. Schematic of PLD mechanism (Top) and a sample picture of PLD process:
deposition of BYZ on MgO (100) substrate.
Most of the PLD systems use gas excimer and Nd3+
: YAG lasers. Generally, the useful
wavelength spectra for PLD thin film deposition are between 200nm and 400nm since
most materials for PLD show strong absorption in this spectral region. Therefore, Nd3+
:
36
YAG laser, which has an operating wavelength of 1064nm, uses a beam attenuator to
adjust frequency down to 266~355nm. Unlike Nd3+
: YAG lasers, gas excimer lasers emit
their radiation directly in the ultra violet region. Table 2-1 shows the gas excimer
wavelengths for commercial laser systems [21].
Table 3-1. Wavelength of excimer lasers
Excimer Wavelength (nm)
F2 157
ArF 193
KrCl 222
KrF 248
XeCl 308
XeF 351
For effective melting of targets and evaporation of particles, laser light should be strongly
absorbed on the target with minimum optical absorption. The thermal diffusion length
(Lt) is given by
2
1
2
mol
tcn
tL
(3.5)
where δt is the pulse duration of the laser, κ is the thermal conductivity of the target, c is
the molar heat capacity of the target, and nmol is the molar density of the target. The
37
values of Lt for oxides and metals are typically in micrometers. Considering the optical
absorption length of those targets is less than 10nm, the laser in PLD is effectively used
for evaporation with strong thermal absorption on the surface of the target [21-23].
There are several factors that influence PLD process: target-sample distance, laser
energy, background gas (pressure), and substrate temperature. Among them, the laser
energy density is considered the most critical factor. Since the laser beam focuses on a
small area (2-3mm2) with high energy (60-80mJ), the energy density is quite high (3-
4J/cm2). Therefore, temperature at the local target surface is very high (about 10000K)
which allows thermal evaporation and deposition of basically all kinds of materials. The
plume also interacts with the laser, and evaporated particles acquire high kinetic energy
up to 10eV for neutral species and 1000eV for ionized species. Due to their large kinetic
energy and mobility, those particles can form dense and highly organized films on the
substrate. If we use a single crystalline substrate, the particles tend to from a film in a
highly organized fashion, and we can achieve an epitaxial PLD layer. However, kinetic
energy acquired by laser is not preserved when the chamber is filled with process gases,
usually inert gas or oxygen for oxide film deposition. Bombardments between the
evaporated particles and ambient gas molecules decrease their kinetic energy and, as a
consequence, their mean free path is reduced from kilometers to microns. The
background gas and its pressure also affect the area and the characteristics of PLD films.
Therefore, the background gas is another critical factor for PLD [21, 23].
38
The PLD technique has significant benefits over other thin film deposition methods: 1)
The capability of exact stoichiometry transfer of material from target to substrate, i.e. it
can reproduce the chemical composition of the target even though it is a complex
material. 2) Since it has the exact stoichiometry transfer capability, PLD has a wide,
almost unlimited, range of materials selection. 3) PLD has relatively high deposition
rates, typically ~100Å /min, with precise deposited film thickness by turning on and off
the laser power. 4) The use of a carousel, which holds multiple targets, enables in-situ
deposition of multilayer films without breaking the vacuum when changing between
materials. Despite these significant advantages, the area of material deposition (about
1~2cm2) is quite small in comparison to that required for industrial applications (required
area coverage of 7.5 x 7.5cm2). There have been efforts to solve this problem and it has
been solved to a large extent by using line-focus laser spots.
3.3.1 Example Materials of Pulsed Laser Deposition
As previously mentioned, the strongest benefit of PLD is exact stoichiometry transfer of
materials. In other words, the stoichiometry of the target material is preserved in the films
since the intensive laser effectively evaporates all the components or ions on the surface
at almost the same rate. For this reason, target materials are required to possess
homogeneity in composition. This characteristic is beneficial especially for deposition of
complex compounds including defect-contained oxide materials such as
39
(Y2O3)0.08(ZrO2)0.92 or superconducting materials like YBa2Cu3O7 (YBCO). Generally,
the PLD process is known as a technique producing the best quality YBCO. Table 3-2
shows the example materials deposition using PLD as summarized by Chrisey et al. [21].
40
Table 3-2. Example materials deposited by pulsed laser deposition and applications of
those materials [21].
41
3.3 References
[1] R. O’Hayre, S. Cha, W. Colella, F. B. Prinz, Fuel Cell Fundamentals, John Wiley and
Sons, New York (2006)
[2] X. Li, Principles of Fuel Cells, Taylor & Francis (2005)
[3] L. Malavasi, C. A. J. Fisher, S. Islam, Chem. Soc. Rev., 39 4370 (2010)
[4] H. Tuller, A. S. Nowick, J. Electrochem. Soc., 122, 255 (1975)
[5] H. Huang, M. Nakamura, P. Su, R. Fasching, Y. Saito, and F. B. Prinz, J.
Electrochem.Soc., 154, B20 (2007)
[6] H. Huang, T. M. Gür, Y. Saito, and F. Prinz, Appl. Phys. Lett., 89, 143107 (2006)
[7] J. H. Shim, C.-C. Chao, H. Huang, and F. B. Prinz, Chem. Mater.,19, 3850 (2007)
[8] V. V. Kharton, F. M. B. Marques, A. Atkinson, Solid State Ionics, 174, 135 (2004)
[9] B. C. H. Steele, Solid State Ionics, 75, 175 (1995)
[10] B. C. H. Steele, K. M. Hori, S. Uchino, Solid State Ionics, 135, 445 (2000)
[11] B. C. H. Steele, J. A. Kilner, P. F. Dennis, A. E. McHale, Solid State Ionics, 18-19,
1038 (1986)
[12] K. D. Kreuer, Ann. Rev. Mat. Res., 33, 333 (2003)
[13] W. Münch, G. Seifert, K. D. Kreuer, J. Maier, Solid State Ionics, 97, 39-44 (1997)
[14] N. Bonanos, B. Ellis, M. N. Mahmood, Solid State Ionics, 44, 305-11 (1991)
[15] N. Kuwata, N. Sata, T. Tsurui, H. Yugami, Jpn. J. App. Phys., 44, 8613-8618
(2005)
42
[16] T. Hibino, A. Hashimoto, M. Suzuki, M. Sano, J. Electrochem. Soc., 149, A1503-8
(2002)
[17] H. Iwahara, H. Uchida, K. Morimoto, J. Electrochem. Soc., 137, 462-465 (1990)
[18] K. D. Kreuer, S. J. Paddison, E. Spohr, M. Schuster, Chem. Rev., 104, 4637 (2004)
[19] K. D. Kreuer, E. Schonherr, J. Maier, Solid State Ionics, 1, 70-71 (1994)
[20] H. Iwahara, T. Yajima, T. Hibino, K. Ozaki, H. Suzuki, Solid State Ionics, 61, 1-3
(1993)
[21] D. B. Chrisey, G. K. Hubler, Pulsed Laser Deposition of Thin Films, John Wiley &
Sons (1994)
[22] M. Ohring, The Materials Science of Thin Films, Academic Press (2001)
[23] D. B. Chrisey, J. S. Horwitz, P. C. Dorsey, J. M. Pond, Laser Focus World, p.155,
May (1995).
43
CHAPTER 4. Nano-pore Structured Platinum Electrode
Arrays for Low Temperature SOFCs
This study presents the fabrication and investigation of morphologically stable model
electrode structures with well-defined and sharp platinum/yttria stabilized zirconia (YSZ)
interfaces to study geometric effects at triple phase boundaries (TPB), which is the actual
electrochemical reaction site for fuel cells. These nano-structured dense Pt array cathodes
exhibited better structural integrity and thermal stability at the fuel cell operating
temperature of 450~500oC when compared to porous sputtered Pt electrodes. More
importantly, electrochemical studies on geometrically well-defined Pt/YSZ sharp
interfaces demonstrated that the cathode impedance and cell performance both scale with
aerial density of TPB length. By controlling the density of TPB we could optimize and
maximize the fuel cell performance.
4.1 Introduction
Solid oxide fuel cells (SOFC) are efficient energy conversion devices that are being
developed for practical applications. Due to large activation energies (~1eV) for oxide
ion transport in solid oxide electrolytes and relatively sluggish oxygen reduction reaction
44
at the cathode, SOFCs are usually operated at elevated temperatures (800~1000oC) to
obtain practically meaningful fluxes and fuel cell performance. Typically, an SOFC
element is made of a yttria-stabilized zirconia electrolyte layer, a mixed conducting
ceramic cathode such as La1-xSrxCo1-yFeyO3 (LSCF) and La1-xSrxMnO3-δ (LSM), and a
cermet anode such as Ni/YSZ.
Operation of SOFCs at elevated temperatures may be desirable for enhanced kinetics and
transport purposes, but pose serious challenges in microstructural and thermal stability,
seal integrity, aging and degradation, thermal cycling, and cost of materials and
fabrication. To mitigate some of these problems, recent efforts have been aimed towards
lowering the operating temperature of SOFCs to intermediate temperature regime of 600-
800oC, i.e., IT-SOFCs [1-4]. Although oxygen chemical diffusion in mixed conducting
electrodes such as LSCF and LSM is relatively fast at elevated temperatures [5-9], their
catalytic activities and transport rates decrease precipitously with temperature that leads
to increased activation losses at intermediate temperatures [1, 10-13].
In recent years, the thrust of our research effort has been aimed to further lower the
operating temperature of SOFCs to a regime between 300 and 500oC by employing thin
film structures of the YSZ electrolyte and electrodes [14-17]. Expectedly, use of mixed
conducting ceramic cathodes for such low temperature (300~500oC) SOFCs (LT-SOFCs)
would not be meaningful due to severe losses expected from large overpotentials at the
electrodes. Hence, platinum is selected as a model electrode material in this study not
45
only to enhance the fuel cell performance but also to provide a stable and geometrically
well-defined platform to examine the triple phase boundary effects in SOFCs. In this
relatively low temperature regime, Pt remains to be the best catalyst to enhance the rate
for the oxygen reduction reaction at the cathode that is critically important to minimize
the activation loss, and to improve the fuel cell performance of LT-SOFCs.
The primary purpose of this study is to control the geometry of the Pt/YSZ interface that
makes it possible to investigate TPB effects in a quantifiable manner. Although similar
patterning efforts have been reported in the literature, only a handful has considered the
Pt/YSZ system [18, 19], while most were intended for mixed oxide cathodes such as La-
Sr-Mn-O [20, 21].
The methodology developed in this study allowed fabrication of morphologically stable
Pt array electrodes that exhibit sharp and well-defined triple phase boundaries (TPB).
The strategy was to define the geometry of the three phase contact interfaces while
providing a dense and nonporous Pt layer that constrains the charge transfer reaction to
TPB only as well as eliminating porosity effects at the Pt/YSZ interface under the Pt
layer. This patterning approach opens up the opportunity for other researchers to
systematically study TPB effects in SOFCs. The results presented here successfully
demonstrate that controlled TPB density correlates well with cell performance.
46
The charge transfer reaction at the cathode involves reduction of oxygen at the TPB,
where the gas, catalytic cathode, and the electrolyte are all in physical contact. Due to
relatively high activation energy of >1.5eV for the oxygen reduction reaction [22-27], it
is generally agreed that the processes at the cathode govern the overall behavior of
SOFCs even at elevated temperatures [1]. Naturally, cathodic overvoltage becomes even
more pronounced at the low operating temperatures employed in this study. To mitigate
this effect and to enhance fuel cell performance, it is not only desirable to maximize the
TPB density but also to employ Pt catalyst at the cathode to improve the reaction kinetics
for oxygen reduction in LT-SOFCs. However, performance maximization is not the focal
point of this study at this point.
Typically, DC sputtering is employed to deposit randomly structured porous Pt electrodes
that increase TPB density for improved fuel cell performance. However, this technique
poses challenges to quantify the TPB geometry and to carry out systematic studies of
TPB effects in SOFCs because control, quantification, and stability of the Pt/YSZ
interface morphology are not trivial issues. It is difficult to characterize the
morphological details of the Pt/YSZ interface with sufficient precision [28-31]. Also,
time-dependent changes [32], such as Ostwald ripening of the sputtered porous Pt
electrodes that can lead to microstructural coarsening and degradation complicate the
problem further more. Indeed, recent work in our laboratory has shown that sputtered
porous pure Pt electrodes are not thermally stable even at the low operating temperatures
of LT-SOFCs [33]. Most importantly, however, it is difficult to quantify and define the
47
exact geometry, scale and nanostructure of the TPB. This makes quantitative
investigation of the rate processes at the TPB challenging.
It is for these reasons that the present study reports on a new non-lithographic patterning
technique for fabrication of dense Pt electrodes with easily tunable and well-defined TPB
geometry. The intent is not to achieve improved cell performance but rather, to establish
a methodology that allows systematic investigation of TPB characteristic and scaling
behavior.
This study reports a dense patterned Pt architecture that forms sharp, stable Pt/YSZ
interfaces with well-defined geometries, and hence, allows determination of TPB linear
density with good accuracy. Since the Pt electrode layer is nonporous, this architecture
also restricts the charge transfer reaction to this geometrically defined interface.
Furthermore, the present study demonstrates superior microstructural and thermal
stability of such patterned electrodes for improved and consistent SOFC performance.
The nanosphere patterning (NSP) method provides the ability to vary the TPB geometry,
which makes it possible to investigate TPB characteristics in a controlled manner and it
gives implications optimizing the LT-SOFC’s electrode/electrolyte interface structures.
48
4.2 Experimental
4.2.1 Spherical Silica Particle Fabrication
For the use of masking solution, monosize spherical silica particles were created by a
modified Stöber synthesis technique using tetraethyl orthosilicate (TEOS) [34-36]. The
TEOS molecules are easily converted to silicon dioxide via a series of condensation
reactions. The TEOS molecules are easily converted to silicon dioxide via a series of
condensation reactions.
(4.1)
The reaction rate is very sensitive to the presence of catalytic solutions. In this
experiment, a pH value of about 12 was employed in a mixture of 38% ammonium
hydroxide and ethanol as a basic catalyst for the reaction. Size of the spherical silica
particles can be controlled by varying the concentration of TEOS and the catalyst. Thus,
different sizes of silica nanopsphere particles were prepared and were used as mask for
subsequent patterning of the Pt cathode layers (Figure 4-1). After synthesis of the SiO2
particles, the surface of the particles was functionalized with aminopropyl
methyldiethoxysilane (APDES) to terminate them with positively charged amine group
and this step prevents aggregation of the particles.
49
Figure 4-1. Synthesized spherical silica particles with different diameters: (a) 130nm, (b)
300nm, (c) 650nm.
4.2.2 Nanosphere lithography (NSL) for nano-structured electrodes
Monosize spherical silica particles were transferred onto a surface of the YSZ substrate
using a Langmuir-Blodgett (LB) trough technique demonstrated by Cui and co-workers
[37]. This technique allows transferring the silica particles from the surface of water by
dipping a desired substrate (Figure 4-2). Initially, the LB trough was filled with DI water.
Then the prepared silica particles were introduced on to the surface of the water by slow
injection. Using the compression bars in the trough, a monolayer of nanospherical
particles was produced at the surface. The substrate was then dipped into the trough and
pulled out at a constant rate. In this experiment, the substrate is a 1cm by 1cm, 8 mol%
yttria-stabilized zirconia (YSZ) single and polycrystalline wafer obtained from
Marketech Inc. The transfer process involved slow insertion of the YSZ substrate
50
vertically into the LB trough and removing the adhered spherical particles as a film from
the liquid surface by steadily withdrawing the YSZ substrate from the liquid at a finite
rate. This method creates a close-packed monolayer of silica particles on the YSZ
substrate.
Figure 4-2. Schematic of the Langmuir –Blodgett trough
After forming a close-packed monolayer of spherical particles on the substrate,
anisotropic plasma etching with a gas mixture of O2 and CHF3 was used to uniformly
reduce the size of the silica particles in order to open up space between them for
depositing Pt through the interspacing between the particles. A dense Pt layer is then
deposited on the cathode side by DC sputtering under 100W plasma power and 1Pa of Ar
pressure for about 60 seconds at room temperature. This yielded a nonporous Pt film of
about 60nm in thickness [16]. Then the silica particles were removed mechanically from
51
the YSZ substrate using ultra sonication. On the anode side of the substrate, 80nm thick
porous Pt layer was deposited by DC sputtering under 50W power, 10Pa of Ar pressure
for 150 seconds at room temperature. With that, the fabrication of the SOFC membrane
electrode assembly (MEA) was complete. This novel process yields a patterned Pt
cathode layer with well-defined geometry that enables the study of TPB geometric effects
in a systematic and controlled manner (Figure 4-3 and 4-4). In addition, by appropriately
varying the silica particle size and the spacing between particles, it is possible to vary and
optimize the TPB density on the YSZ surface in a controlled manner.
Figure 4-3. Fabrication process schematic of nano-pore structured electrode by using
nanosphere lithography (NSL) technique.
52
Figure 4-4. SEM images of nano-pore structured dense Pt electrodes.
For the fuel cell performance characterization, we used a homemade experimental
chamber with a micro-manipulating probe station (Figure 4-5). During the measurements,
pure dry hydrogen is provided at the anode side as a fuel and air is used as the oxygen
source at the cathode side. Constant temperature is maintained by a temperature
controlling unit. For electrochemical characterization, a Gamry Potentiostats (Gamry
Instruments) unit is used for collecting both I-V characteristic data and Electrochemical
Impedance Spectra (EIS) in the frequency range of 300 kHz to 0.1 Hz with an AC
amplitude of 50mV.
53
Figure 4-5. Schematic illustration of the probing station for electrochemical
characterization of fuel cell MEAs.
4.3 Results and Discussion
4.3.1 Thermal stability of the nano-pore structured electrode
SOFCs that operate at elevated temperatures typically do not employ Pt electrodes for
obvious reasons. However, for LT-SOFCs the use of Pt electrodes is a near-necessity due
to sluggish reaction kinetics at these low temperatures. Micro-SOFCs utilizing 50 to 750
nm thick YSZ membranes and porous Pt electrodes have been studied and power
densities in the range 0.02 to 152mW/cm2 have been reported [38]. Comparatively,
similar work in our laboratory has demonstrated record power densities up to
861mW/cm2 at 450
oC [14-16]. Long-term stability of the sputtered Pt electrodes reported
in these studies, however, has not been fully documented or investigated. Similarly, there
is not a coherent understanding or establish process for consistent fabrication of stable Pt
54
electrode morphologies that also display optimum performance. Previously, evidence
from our laboratory has indicated that porous Pt electrodes fabricated by DC sputtering
undergo morphological changes during cell operation even at these low temperatures,
while stable morphology and performance was demonstrated with Pt-Ni alloy electrodes
[33]. Based on these observations, dense Pt electrodes with geometric openings to create
well-defined and stable TPB was pursued in the present study.
Figure 4-6. SEM images of (a) as sputtered porous Pt layer, (b) after short time (~
30mins) operation of fuel cell at elevated temperature (450oC), clearly indicate a dramatic
change in Pt morphology and a proportionate reduction in the TPB density.
55
Figure 4-7. Potentioamperometry data at 0.6V, comparing the behavior of SOFC MEA
with porous Pt electrode and SOFC with nano-pore structured Pt electrode. Measurement
was conducted for 12 hours continuously at 500oC. (a) Absolute output current densities
indicating severe degradation in performance of porous Pt within a short time as opposed
to stable behavior of patterned dense Pt. (b) Normalized current densities plot showing
relative amounts of degradation from the initial performance.
Initial performance of fuel cell sample using randomly porous Pt electrode is higher than
the sample using nano-pore (e.g. patterned with 400nm pores) structured electrode.
Although the fuel cell MEA with porous Pt electrodes outperformed that with patterned
Pt cathode in the beginning of cell testing, its performance dramatically decreased within
a short time due to electrode degradation. The change in the morphology of the DC
sputtered porous Pt electrodes before and after fuel cell testing at elevated temperature is
shown in Figures 4-6(a) and 4-6(b). It is clear that even at the moderately low
(400~450oC) operating temperature of LT-SOFC, significant changes take place in the
microstructure of the porous Pt electrode driven likely by its high surface energy.
However, due to the visibly evident changes in the Pt morphology and equally so at the
Pt/YSZ interface, reduction in the TPB density leads to a rapid degradation in the fuel
56
cell performance until it seems to stabilize at a significantly lower value. This is shown in
Figure 4-7, which compares the fuel cell performance of sputtered porous Pt electrodes
with patterned Pt electrodes under potentiostatic conditions. After completion of the I-V
experiments for both samples, the output currents of the two cells were monitored for 12
hours at 500oC at a constant voltage that corresponds to the peak power density value.
Despite the noise in the data that came from the measurement setup, particularly from the
on/off type temperature controller and the fume hood fan, Figure 4-7 clearly indicates a
stable performance by the nano-structured Pt electrode, while the current output from the
porous Pt cell clearly shows a rapid decay over time. In addition, a morphological
comparison provided in Figure 4-8 demonstrates the stability of the nano-structured Pt
electrode after running under potentiostatic conditions for 12 hours at 500oC. This
morphological degradation in porous Pt electrodes occurs even at temperature lower than
500oC and becomes observable within a short period of time. Unlike the porous Pt
cathodes, the patterned Pt morphology indicated no discernable change in the
microstructure at the test temperatures and under load in a SOFC configuration. Clearly,
the sharp interfacial edges of the Pt layer, representing the location of TPB, are uniformly
well preserved even after prolonged use. The results demonstrate that the nano-patterning
method employed in this study helped stabilize the morphology and provide thermal and
microstructural stability at fuel cell operating temperatures.
57
Figure 4-8. High resolution SEM images of nano-structured fresh Pt electrode before
running (top (a) and tilted (c) views), and after running chronoamperometrically for 12
hours at 500oC (top (b) and tilted (d) views). Clearly, nano-structured Pt does not show
any major morphological change and the TPBs are well conserved after long operation.
58
Figure 4-9. V-I-P comparison of SOFC at 450oC employing DC sputtered porous Pt
electrode versus nano-pore structured Pt electrode at the cathode.
Furthermore, nano-patterned Pt electrodes, when optimized, have the potential to provide
better cell performance due to controlled and stable TPB geometries that also offer ready
access to the gas phase. Indeed this is demonstrated in Figure 4-9, which compares the
performance of a SOFC MEA at 450oC featuring a nano-patterned Pt electrode of
approximately 400 nm diameter pore size with that of a MEA with DC sputtered porous
Pt electrodes measured after the cell performance is stabilized at the operating
temperature. It is clear that the cell featuring nano-patterned Pt performs better than the
one having porous sputtered Pt electrode. This result suggests either a higher density of
TPB for the nano-patterned Pt electrode, or possibly a significant amount closed porosity
in the case of the sputtered Pt electrode likely due to structural coarsening and
degradation, which hinders direct access from the gas phase, even though it might have
initially possessed a larger Pt/YSZ interfacial contact length. The maximum power
59
density values obtained with fuel cell MEAs with nano-patterned cathodes are still orders
of magnitude lower than previous reports from our laboratory on record performance of
LT-SOCFs using ultra-thin film YSZ electrolyte and porous Pt electrode [14-16]. This is
primarily due to two reasons, namely, that the TPB density of nano-patterned cathodes is
naturally and significantly lower than porous Pt cathodes, and also, polycrystalline
100µm thick bulk YSZ wafers were used as the electrolyte in the present study.
Therefore, it may not be meaningful to directly compare these performance values due to
the combined effect of the electrolyte thickness and deposition methods, which generate
different microstructures. Again, this study presents a fabrication methodology for nano-
pore structured electrodes not for the purpose of achieving the highest performance but
for investigation of electrochemical behavior of TPB geometry and possibly its
optimization.
4.3.2 Investigation of TPB scaling behavior
The sharp interfacial geometry of the open pores in a close-packed fashion makes it
possible to approximate the TPB density (cm/cm2) for a given patterned area. With the
help of SEM images, the TPB densities for the two patterned Pt cathodes were
approximated to be 8.93 x 104
cm/cm2 for cathodes with 300 nm opening and 5.07 x 10
4
cm/cm2 for cathodes with 400 nm opening (Figure 4-10). The SOFC MEA with the
smaller initial diameter of the silica particle showed about a factor of 1.8 higher TPB
60
density than the SOFC MEA with the larger size of the starting silica particles. Naturally,
the size of the pore opening as well as the interspacing between openings for a given
geometric area determines the TPB density. The results presented below correlate the
TPB scaling factor with cell performance and behavior.
The performance of fuel cells featuring two different nanopore sizes, or respective TPB
densities, is presented in Figure 4-11(a). As previously mentioned above, the SOFC
MEA with higher density TPB of about 8.93 x 104 cm/cm
2 of projected area (pore
diameter ~300nm) at the cathode shows better performance than the SOFC with coarser
(~400 nm) cathode openings with TPB density of about 5.07 x 104 cm/cm
2. These values
are larger than 15-150 cm/cm2 TPB densities reported for patterned Pt electrodes on YSZ
[19]. Peak power densities and open circuit voltages (OCV) of the patterned Pt cathodes
with pore openings of 300 nm and 400 nm pore size are 2.2mW/cm2
and 1.04 V, and
1.4mW/cm2 and 1.01 V, at 450
oC, respectively at about a cell operating voltage of
0.45V. Also the coarser TPB sample shows a larger exponential drop at low current
region, indicative of a larger activation loss than the denser TPB sample. However, the
differences in their relative performances vanish when these plots are normalized with
respect to the areal TPB densities of the two MEAs. This is expected since the charge
transfer reaction is restricted to TPB whose linear length per unit area is determined by
the masking process during patterning. The results are shown in Figure 4-11(b) where the
I-V-P plots of the 300 nm and 400 nm patterned MEAS overlay on top of each other in
61
almost perfect registry and agreement on the low current regime, where activation losses
and hence, the charge transfer along TPB dominates behavior.
Figure 4-10. Nano-pore structured dense Pt electrode with different final pore sizes and
TPB density, (a) 300nm, (b) 400nm. SEM images were taken with the same
magnification and the image with smaller initial particle size shows denser pores, which
relates to increased TPB density.
62
Figure 4-11. (a) Fuel cell I-V measurement of SOFC samples at 450oC with structured
electrode with different pore diameters. (b) V-I-P plot where current is normalized by
TPB density. The plots overlay in good registry especially in the activation regime as
expected, and indicates that fuel cell performance scales with TPB density.
Further characterization of the MEAs was carried out by electrochemical impedance
spectroscopy (EIS). Figure 4-12 compares the EIS spectra at 450oC of SOFC samples
with nano-patterned Pt cathodes of different pore opening sizes under 0.6 V DC biased
63
condition. From the EIS Nyquist plot of SOFC with YSZ electrolyte, it is well known
that the high frequency arc corresponds to the ohmic resistance of the electrolyte and the
low frequency arc corresponds to the electrochemical reaction at the electrolyte/electrode
interface [34]. For SOFCs, there is general agreement that cathode reaction kinetics is
much slower than that for the anode reaction, and hence, the cathode reaction dominates
the activation loss [3]. Assigning the low-frequency arc in EIS spectra to the ORR
(oxygen reduction reaction) process as suggested by others [39, 40], one can conclude
that the cathode impedance is reduced for the 300 nm pore size Pt electrode due to
increased TPB density as compared to the 400 nm pore size Pt having a lower TPB
density, and hence, a larger cathode impedance. Clearly, EIS impedance data provides
further support for faster or improved oxygen reduction kinetics at the cathode by
increasing the TPB density and the charge transfer reaction sites [41].
From the EIS spectra in Figure 4-12, it is possible to determine the corresponding
cathode resistance for the two samples. The electrode resistance of the coarser TPB MEA
(~2600 ohms) is a factor of 2.06 higher than the MEA with denser TPB (~1260 ohms),
corresponding to smaller pore openings. Although the scaling factor does not perfectly
match the ratio of 1.8 between the TPB densities of the two samples, it does suggest
within experimental error that the electrode resistance scales almost linearly with the TPB
density.
64
Figure 4-12. EIS Nyquist spectra of SOFC samples featuring nano-pore structured dense
Pt cathodes with different TPB densities.
Furthermore, a similar scaling behavior is observed between the TPB density and the
peak power densities of the two samples shown in the I-V curves of Figure 4-11. Indeed,
the ratio of 1.6 between the peak power densities of the two samples agrees within
experimental error with the TPB ratio of 1.8 between the two patterned cathode samples,
suggesting again the possibility of a linear scaling law.
Considering the fact that the linear length of the Pt/YSZ interface per circular opening in
these patterned cathodes is about 1260nm for the 400nm diameter opening, and
correspondingly 940nm for the 300nm diameter opening, the results above further
suggest that the TPB width under the test conditions is significantly smaller than its
65
length, possibly in the several nanometers to tens of nanometers range in general
agreement with estimated literature values of the same order of magnitude for this
operating condition [18]. This yields a near-linear scaling relationship and confirms the
argument that the TPB is actual electrochemical reaction site for SOFC.
4.3.3 TPB width estimation for Pt/YSZ interface
Figure 4-13. (a) Schematic of the TPB. (b) Cross-section image showing TPB width.
As previously mentioned, the actual electrochemical reaction site for charge transfer is
called TPB. This TPB is where electrolyte, reacting gas, and catalytic electrode are in
physical contact. The red lines in Figure 4-13(a) show schematic of TPB. Though the
TPB is shown as a line, it actually has its own width (Figure 4-13(b)). If the TPB width
overlaps each other, we are not fully utilizing the electrochemically active sites.
Therefore, it is very important to know the geometry of the TPB width. With the
66
information we can design the electrode structure to achieve high and optimized fuel cell
performance at a certain operating condition.
The width is determined by the electrolyte’s material properties and fuel cell operating
conditions such as operating temperature. TPB width can be expressed by following
equations [42]:
k
DwTPB (4.2)
where D is a diffusion coefficient of electrolyte material and k is the reaction rate at the
electrode/electrolyte interface. For electrochemical systems, the reaction rate constant (k)
may be expressed in terms of the current density of the electrochemical reaction, jrxn
(A/cm2):
o
rxn
c
jk (4.3)
And the reaction current density (jrxn) can be estimated from the Tafel approximation for
a given overpotential, η [42-43]:
b
rxn jj /
010 (4.4)
67
where j0 is the exchange current density (A/cm2), η is overpotential (mV), and the b is the
Tafel slope (mV). By combining the equations above, we could get an expression of TPB
width as following:
bTPBj
Dcw
/
0
0
10 (4.5)
As previously mentioned and can be seen from the equation above, the TPB width is
dependent on the material properties and the operating conditions.
For the nano-pore structured Pt electrode case, the periphery of the pore is where TPB is
located. Therefore, increasing the density of pores by decreasing the pore size in a given
reaction area, we can increase the fuel cell performance. However, since the TPB has a
certain width we will have TPB overlaps if the pore radius is smaller than TPB width. In
other words, we can estimate the TPB width by observing the saturation regime of
performance enhancement while we keep decreasing the electrode pore size. So, if we
consider the electrode interface resistance, first it will decrease as we increase the TPB
density since we have more reaction site. But when the TPB overlap happens the
electrode resistance will not decrease anymore and show a saturation behavior (Figure 4-
14). By measuring the radius of pores at this saturation regime, we can estimate the TPB
width at a certain operating condition of SOFC.
68
Figure 4-14. Graphical estimation of electrode/electrolyte interface resistance as the TPB
density increases. Interface resistance will be decrease as we increase the TPB density by
decreasing the pore size since we are introducing more electrochemical reaction site. If
the TPB width overlap starts, the resistance will not decrease anymore and will show
saturation behavior.
For the experiments, four different sizes of silica particles (about 300nm ~ 600nm) were
prepared. Using those particles, SOFC samples were fabricated having nano-pore
structured Pt electrodes with different pore sizes. During the fabrication process, the
spacing between the pores was consistent for all the electrodes in order to be able to
compare the TPB density by the pore sizes. Figure 4-15 shows the SEM images of the
structured electrodes. To estimate the TPB width during the fuel cell operation, other than
the material properties we can change the operating conditions such as temperature and
the overpotential. From the equation (4.5), since the operating temperature both affects
69
diffusion coefficient, D, and the exchange current density, j0, we chose the overpotential
value as a variable at a fixed operating temperature condition for easier approach.
Figure 4-15. SEM images of nano-pore structured Pt electrodes on single crystalline YSZ
substrates. TPB linear density was estimated by measuring the pore size and spacing
between the pores. As we have smaller pore size, we have larger TPB density. The
electrode pore sizes are (a) 240nm, (b) 350nm, (c) 430nm, and (d) 570nm.
YSZ grain boundary is known to have higher surface oxygen exchange rate and bulk
grain. This will be discussed more in the next chapter. To exclude the contribution on
electrode interface resistance which comes from randomly distributed grain boundaries,
70
we used single crystalline YSZ which has no surface grain boundary as an electrolyte
material. From the relationship shown in equation (4.5), higher overpotential (η = OCV –
cell voltage) yields smaller TPB width. Therefore, higher cell voltage yields lower
overpotential and it has larger TPB width than smaller cell voltage condition. The EIS
spectra were measured at 400oC with different cell operating voltage conditions. From
the data, the electrode interface resistances of the four samples were extracted. Figure 4-
16 shows extracted electrode interface resistances at 400mV and 800mV cell voltage
conditions as a function of the electrode pore sizes. As can be observed, 800mV case,
which has larger TPB width than 400mV, shows saturation behavior in electrode
resistance values as the pore size gets smaller while the 400mV case shows continuous
decrease in electrode resistance. This indicates that the TPB width is about 200nm when
we run the Pt/YSZ system SOFC at the operating conditions of 400oC and 800mV cell
voltage. This is the first demonstration of the TPB width estimation during the actual fuel
cell operation. And this will provide a significant implication in electrode structure
designing for maximizing LT-SOFC performance by fully utilizing the electrochemical
reaction sites.
4.4 Conclusion
In summary, the present study offers a process methodology for controlling the geometry
of the Pt/YSZ interface for the systematic study of TPB characteristics. The results
71
presented here point to several important and useful consequences. First is the near-linear
scaling law of cell impedance and, correspondingly, cell performance on the linear
density of TPB. The EIS spectra showed significant improvement in the oxygen
reduction kinetics with increased TPB density. The linear scaling behavior infers that the
charge-transfer reaction is constrained to TPB as expected. It also implies that the width
of TPB in our MEAs is negligibly small with respect to its length, which agrees with
literature. Second is the precision and versatility of the patterning method presented here
to fabricate dense electrodes with sharp interfaces and well-defined geometries. These
electrodes also exhibit superior stability compared to sputtered Pt electrodes and maintain
their morphology and microstructure intact after prolonged fuel cell operation. Third is
the opportunity of stable operation of IT to LT SOFCs that employ these dense and
patterned electrodes. Fourth is the ability to study TPB geometric effects in a controllable
and reproducible manner over a wide range of circular pore diameters using this powerful
patterning technique that does not require lithography and micromachining. The pore size
and TPB density are easily tunable by changing the initial size of the masking silica
particles and the spacing between them. By doing this, we could effectively estimate the
TPB width at desired fuel cell operating conditions. This provides significant implication
in designing the nano-electrode structure to optimize and maximize LT-SOFC
performance.
72
4.5 References
[1] J. Fleig, Annu. Rev. Mater. Res., 33, 361 (2003)
[2] Y. Jiang and A. V. Virkar, J. Electrochem. Soc., 150(7), A942 (2003)
[3] S. DeSouza, S. J. Visco, and L. C. DeJonghe, Solid State Ionics, 98, 57 (1997)
[4] E. D. Wacshman, ECS Trans., 25(2), 783 (2009)
[5] A. Belzner, T. M. Gür, and R. A. Huggins, Solid State Ionics, 57, 327 (1992)
[6] K. Nisancioglu and T. M. Gür, Solid State Ionics, 72, 199 (1994)
[7] S. Sunde, K. Nisancioglu, and T. M. Gür, J. Electrochem. Soc., 143, 3497 (1996)
[8] S. Diethelm, A. Closset, K. Nisancioglu, J. Van Herle, A. J. McEvoy, and T. M. Gür,
J. Electrochem. Soc., 146, 2606 (1999)
[9] R. Doshi, J. L. Routbort, and C. B. Alcock, Defect and Diffusion Forum, vol.127-128,
Scitec Publications, p.39 (1995)
[10] S. B. Adler, Chem. Rev., 104, 4791 (2004)
[11] S. Wang, T. Kato, S. Nagata, T. Kaneko, N. Iwashita, T. Honda, and M. Dokiya,
Solid State Ionics, 152-153, 477 (2002)
[12] B. C. H. Steele, Solid State Ionics, 134, 3 (2000)
[13] R. Doshi, V. L. Richards, J. D. Carter, X. Wang, and M. Krumpelt, J. Electrochem.
Soc., 146, 1273 (1999)
[14] P-C. Su, C-C. Chao, J. H. Shim, R. Fasching, and F. B. Prinz, Nano Lett., 8(8), 2289
(2008)
[15] J. H. Shim, C.-C. Chao, H. Huang, and F. B. Prinz, Chem. Mater., 19, 3850 (2007)
73
[16] H. Huang, M. Nakamura, P.-C. Su, R.Fasching, Y. Saito, F. Prinz, J. Electrochem.
Soc., 154(1), B20 (2007)
[17] H. Huang, T. M. Gür, Y. Saito, and F. Prinz, Appl. Phys. Lett., 89(14), 143107-1-3
(2006)
[18] J. L. Hertz, H. L. Tuller, Solid State Ionics, 178, 915-923 (2007)
[19] A. Mitterdorfer and L. J. Gauckler, Solid State Ionics 117, 203 (1999)
[20] R. Radhakrishnan, A. V. Virkar, and S. C. Singhal, J. Electrochem. Soc. 152(1),
A210 (2005)
[21] V. Brichzin, J. Fleig, H.-U. Habermeier, and J. Maier, Electrochem. Solid State Lett.
3(9), 403 (2000)
[22] E. Siebert, A. Hammouche, M. Kleitz, Electrochim. Acta 40, 1741 (1995)
[23] B.C.H. Steele., Solid State Ionics, 86-88, 1223 (1996)
[24] J. van Herle , A.J. McEvoy, K.R. Thampi, Electrochim Acta, 41, 1447 (1996)
[25] A. Mitterdorfer, L.K. Gauckler, Solid State Ionics, 111, 185 (1998)
[26] Y. Matsuzaki, I. Yasuda, Solid State Ionics, 126, 307 (1999)
[27] M. Juhl, S. Primdahl, C. Manon, M. Mogensen, J. Power Sources, 61, 173 (1996)
[28] J. Fleig, Annu. Rev. Mater. Res. 33, 361-82 (2003)
[29] E. Mutoro, S Günther, B. Luerssen, I. Valov, J. Janek, Solid State Ionics, 179 , 1835-
1848 (2008)
[30] E. Mutoro, B. Luerssen, S. Günther, J. Janek, Solid State Ionics, 179, 1214 (2008)
[31] F.S. Baumann, J. Fleig, H-U. Habermeier, J. Maier, Solid State Ionics, 177, 1071-
1081 (2006)
74
[32] T. M. Gür and R. A. Huggins, J. Appl. Electrochem. 17, 800 (1987)
[33] X. Wang, H. Huang, T. Holme, X. Tian, F. B. Prinz, J. Power Sources, vol. 175, pp.
75-81, (2008)
[34] G. H. Bogush, M. A. Tracy and C. F. Zukoski IV, J. Non-Crystalline Solids, 104,
95-106 (1988)
[35] W. Stöber, A. Fink and E. Bohn, J. Colloid and Interface Science, 26, 62-69 (1968)
[36] G.H. Bogush and C.F. Zukoski IV, J. Colloid and Interface Science, Vol. 142, No.1
(1991)
[37] C.-M. Hsu, S. T. Connor, M. Tang,
Y. Cui, Appl. Phy. Lett., 93, 133109 (2008)
[38] A. Evans, A. Bieberle-Hütter, J. Rupp, L.J. Gauckler, J. Power Sources, 194, 119-
129 (2009)
[39] E. Barsoukov and J. R. Macdonald, Impedance Spectroscopy: Theory, Experiment,
and Applications, 2nd Ed., John Wiley and Sons (2005)
[40] H. Huang, T. Holme, and F. B. Prinz, ECS Trans., 3(32), 31 (2007)
[41] A. Optiz, A. Schintlmeister, H. Hutter, J, Fleig, ECS Trans., 25(2) 2783-2792 (2009)
[42] R. O'Hayre, D. M. Barnett, F. B. Prinz, J. Electrochem. Soc., 152(2), A439 (2005)
[43] A. J. Bard and L. R. Faulkner, Electrochemical Methods, 2nd ed., John Wiley &
Sons, New York (2001)
75
CHAPTER 5. Cathodic Surface Engineered Low Temperature
Solid Oxide Fuel Cells
In the previous chapter, we investigated the actual electrochemical reaction site for SOFC
which is the interface of the electrode/electrolyte by developing well-defined and
controllable nano-pore structured electrodes.
In this chapter, we report both experimental and theoretical results of the role of doped-
cerium oxides surface modification layer on the oxygen reduction reaction and its grain
boundaries in enhancing the oxygen incorporation kinetics of low temperature solid oxide
fuel cells (LT-SOFCs).
5. 1 Introduction
Fuel cells offer opportunities to achieve efficient energy conversion, and solid oxide fuel
cells (SOFCs) are distinguished by fuel flexibility, high quality waste heat, and simpler
water management systems. Among the range of oxide ion conducting ceramic
electrolyte materials, yttria stabilized zirconia (YSZ) has been the most commonly
utilized for its high chemical stability over a wide regime of oxygen activities ranging
76
from severely reducing to highly oxidizing conditions. However, due to the highly
activated (~1eV) nature of ionic transport in such solid oxide electrolytes and the
sluggish rate for the oxygen reduction reaction at the cathode side, SOFCs are usually
operated at relatively high temperatures (800oC~1000
oC). Such high operating
temperatures pose serious challenges for practical applications in seal integrity, structural
and thermal stability, high fabrication and materials costs, and compatibility of fuel cell
components. [1, 2] Typically, a SOFC membrane electrode assembly (MEA) is made of a
YSZ electrolyte membrane, a mixed conducting ceramic cathode such as
La1−xSrxCo1−yFeyO3 (LSCF) and La1−xSrxMnO3-δ (LSM), and a cermet anode such as
Ni/YSZ.
In recent years, there have been efforts to reduce the SOFC operating temperature to
intermediate temperatures of 500-700oC [3-5]. Most of these studies employed thin film
techniques to reduce the YSZ membrane thickness down to 10-100µm, thereby
minimizing the ohmic loss and lowering the fuel cell operating temperature. Some work,
including that done in our laboratory, has focused on depositing YSZ films as thin as 0.1-
1µm to reduce the SOFC operating regime to even lower temperatures (LT) between
300oC and 500
oC [6-10]. A recent report provides a good review of various ultra thin film
micro-SOFC efforts [11].
A key obstacle to reducing the temperature regime for SOFC operation is the poor
catalytic activity and transport properties of mixed conducting oxide based cathode
77
materials for the electrochemical reduction of oxygen at these low temperatures [2]. For
this reason, platinum (Pt) is still considered as the best catalytic cathode material at these
temperatures to enhance the oxygen reduction reaction rate or reduce the activation loss,
which is crucial for improving the performance of LT-SOFCs.
Acceptor doped cerium oxides such as gadolinia doped ceria (GDC) and yttria doped
ceria (YDC) are known to have higher ionic conductivity than YSZ below 700oC, but
exhibit mixed ionic electronic conduction at higher temperatures and under reducing
conditions. Because of this, ceria-based electrolytes are considered primarily for
intermediate temperature solid oxide fuel cell applications [12-14], but they have been
investigated at high temperatures as composite electrolytes in combination with stable
electrolytes such as YSZ [15-17]. In addition to their high ionic conductivity, doped
cerium oxides are good catalysts and exhibit fast cathodic kinetics for oxygen reduction
at the triple phase boundary (TPB) [18, 19]. The surface exchange coefficient is a good
measure to assess oxygen ion incorporation. Indeed, Steele and co-workers reported that
the surface exchange coefficient has a positive relationship with the oxygen diffusivity of
a given material [20]. It is reported that surface exchange on doped ceria at 700oC is
several times faster than that for YSZ at this temperature [21, 22]. Accordingly, the
rationale for choosing doped ceria interlayer in the present study to modify the cathode
interface and reduce the associated activation loss is based on its superior catalytic
activity and high surface exchange and oxide ion transport rates.
78
In this study, we performed quantum simulations to calculate and compare the activation
energies for oxygen incorporation into the Pt/YSZ and Pt/YDC systems. To the best of
our knowledge, this constitutes the first attempt reported in the literature to estimate the
energetics of oxygen incorporation in YDC. In addition, we experimentally investigated
the catalytic effect of surface modification on YSZ that involved deposition of ultra thin
YDC and GDC films as an interlayer between YSZ electrolyte and the Pt cathode to
promote the oxygen reduction reaction. Previous work in our laboratory had indicated
that inserting nanoscale thin GDC interlayer at the cathode side of the YSZ substrate
significantly enhanced fuel cell performance by reducing the activation loss associated
with oxygen reduction reaction (ORR) at the cathode [9, 23]. Similarly, others
theoretically observed low activation overpotentials with thin cathodes and ionic
conducting YSZ electrolyte with small grain sizes [17, 24-25]. Accordingly, we
hypothesized that surface grain structure of the YDC and GDC cathodic interlayers
contributes or enhances fuel cell performance.
In order to circumvent complications from grain boundaries, we designed the
experiments with two different approaches for each cathodic interlayer material. First, it
was decided to employ single crystalline YDC and GDC interlayer to investigate material
effect itself on oxygen kinetics at the cathode side without any contributions from the
grain boundaries. For this approach, we successfully fabricated epitaxial YDC, GDC
cathodic interlayers on single crystalline YSZ substrate and achieved composite
electrolytes by using PLD. Second, we investigated the contribution of grain size and
79
hence, the surface grain boundaries of doped cerium oxides in improving the cathode
kinetics of ORR by providing both spectrometric and spectroscopic evidences. For this
grain boundary contribution study, we investigated spectrometric and spectroscopic
evidence indicating enhanced activity at surface grain boundaries. We demonstrated
successful fabrication of polycrystalline composite electrolytes also by PLD technique.
By controlling post-annealing temperatures, we have systematically varied the size of
surface grains of doped ceria interlayers deposited on the cathode side. Then, we studied
how the performances are affected by the size of surface grains, i.e., the grain boundary
density on the doped ceria external surface at the cathode side. For both bulk grain and
grain boundary experiment cases, the fuel cell performance was characterized by current-
voltage measurements in the temperature range of 350oC~450
oC while cathode interfacial
resistances were extracted from electrochemical impedance data. Experimental results
indicate that the fuel cell performance enhances by having doped ceria interlayer by
increasing the surface reaction rate at the cathode side. Moreover, the samples with nano
size surface grains further improve the fuel cell performance by enhancing the oxygen
kinetics. The findings of this study provide important implications for engineering the
cathode as well as the surface grain structure of YSZ composite electrolytes with doped
ceria interlayer in order to enhance SOFC performance.
80
5. 2 Experimental
5.2.1 Quantum simulation of oxygen incorporation energies
Quantum mechanical simulations of oxygen incorporation in YSZ and YDC were
performed using a periodic boundary condition method as implemented in VASP [26-29].
Electron wave functions were expanded in a plane wave basis set using projector
augmented waves up to a maximum energy cutoff of 400eV with an exchange-correlation
functional as parameterized by Perdew et al. [30, 31] Gaussian smearing was used with a
width of 0.2eV to determine partial occupancies. Energy was sampled on a 2x2x1
Monkhorst Pack grid [32]. Calculations were performed assuming non-spin polarized
systems.
The supercell consists of a Pt38 cluster placed on top of a 3x3x3 YSZ slab of
stoichiometry (Y2O3)2(ZrO2)23, giving two vacancies in the anion sublattice. One
vacancy was chosen to reside on the top surface of the slab to study incorporation in the
vacancy, the other vacancy position, and the positions of the four yttrium atoms, were
chosen randomly (see Figure 5-1(b)). Before a slab relaxation in vacuum, the bulk was
constructed and relaxed to find a lattice constant of 5.12Å . This structure was then
relaxed in 20Å of vacuum in the z-direction. The Pt38 QD was separately relaxed, then
placed on top of the slab and relaxed again. To mimic the equilibrium coverage of Pt of
¼ ML in atmosphere, eight oxygen atoms were adsorbed on the surface of Pt, one near
81
the surface vacancy site. To simulate YDC, bulk CeO2 was constructed and relaxed, then
four Ce atoms were replaced by Y atoms in the same position that they were chosen in
YSZ, and the slab was relaxed in vacuum (see the final geometry in Figure 5-2(b)). The
electrochemical reaction was simulated by adding two electrons to the supercell.
The electronic self-consistent charge density was computed to a tolerance of 10-4
eV for
geometry relaxations, and all atoms are allowed to relax (i.e. no atoms are fixed) to find
adsorbed and incorporated states (i.e. initial and final positions). To calculate reaction
pathways, a single oxygen atom located above a surface vacancy was moved down into
the vacancy by constraining the z-coordinate of that atom in successive steps, while
allowing all other coordinates of all other atoms to relax. Charge densities were
calculated by integration inside a Wigner Seitz sphere of radius 0.82Å for oxygen.
5.2.2 Oxygen isotope exchange and NanoSIMS
For spectrometric observation we performed surface microstructure and oxygen exchange
measurements on commercial (Japan Fine Ceramics) sintered YDC pellets 1cmx1cm in
size and 500µm in thickness. The second category of experiments involved fuel cell and
electrode impedance studies as a function of YDC surface grain size (i.e., grain boundary
density) on composite electrolyte samples having a thin YDC layer deposited on the
cathode sides of YSZ substrates.
82
The surface microstructure of commercially available YDC pellets was analyzed by FEI
XL30 Sirion scanning electron microscopy (SEM). These pellets were also employed for
oxygen isotope exchange experiments, where incorporation was carried under DC biased
conditions applied across porous platinum cathode and anode layers sputtered on both
faces of the 500μm-thick polycrystalline YDC pellets. Isotope exchange experiments
involved evacuation of the vessel to at least 10-6
Torr followed by the introduction of
research grade (>99%) 18
O2 gas at 150±1Torr, which is equivalent to the ambient oxygen
partial pressure. The YDC samples were annealed at 400°C for 3 hours in 18
O2 under 1V
of externally applied cathodic (negative) bias. Prior to 18
O2 exchange, the samples were
annealed in 150Torr of 16
O2 environment for at least three times the isotope exchange
time.18
O and 16
O ion counts were measured simultaneously by using high spatial
resolution SIMS (NanoSIMS-50L, Cameca, France). A primary Cs+ ion beam (16keV)
was applied to analyze the secondary ions emitted from the samples. As the primary ion
beam sputters the surface (1010m2 of rastered area and 256×256 pixel with dwell time
of 1ms/pixel), the concentration of ions was measured layer by layer as a function of
depth.
83
5.2.3 Composite electrolyte fuel cell fabrication and characterization
For the fabrication of YDC, GDC interlayers on YSZ substrates, we employed pulsed
laser deposition (PLD) technique. A sintered 1-inch diameter and 0.125-inch thick YDC,
GDC disk pellets (10 mol%, Kurt J. Lesker) were used as target materials to deposit thin
films on two different types of YSZ substrates. A single crystalline YSZ substrate (1cm x
1cm x 300µm, Marketech Inc.) was used to fabricate epitaxial thin interlayers having no
grain boundaries, and polycrystalline YSZ substrates (1cm x 1cm x100µm, BEANS
International Corp.) were used to fabricate polycrystalline thin films with different grain
sizes. A Lambda Physik 248nm KrF excimer laser with energy density of 1.5J/cm2 per
pulse was used for ablating the target in a 100mTorr background oxygen gas environment
in the deposition chamber. During deposition, the sample stage was maintained at 750oC
and the sample-to-target distance was 50mm. The growth rates for YDC and GDC were
~0.22Å /pulse and ~0.23Å /pulse, respectively. For the polycrystalline interlayer samples,
the films were post-annealed at 750-1450oC for 10 hours in ambient air to achieve
different grain sizes. Membrane-electrode assembly (MEA) fabrication was completed by
dc sputtering of porous catalytic platinum (Pt) electrode on both sides for 150secs under
10Pa Ar background pressure and 50W plasma power.
For characterization of the deposited films, X-ray diffraction (XRD) was conducted for
structure and crystallinity characterization of the YDC and GDC interlayer films using a
PANalytical X’Pert PRO XRD system (Cu Kα X-ray with λ=1.54Å ) utilizing the
84
symmetrical θ/2θ scan method for phase analysis. The surface grain size of the post-
annealed films was measured by atomic force microscopy (AFM) (XE-70, Park Systems
Inc.) operated in non-contact surface scanning mode.
For fuel cell performance measurement and characterization, we employed a custom
made fuel feeding chamber sitting on a temperature-controlled heating stage with micro-
manipulating probe stations as shown in previous chapter. During fuel cell measurement,
pure dry hydrogen was supplied at the anode side as fuel while the cathode side was
exposed to ambient air as the oxygen source. For fuel cell performance evaluation, A
Gamry Potentionstat (FAS2, Gamry Instruments, Inc.) was used to obtain current-voltage
(I-V) behavior as well as the electrochemical impedance spectroscopy (EIS) data. Fuel
cell performance was measured from 350-450oC and EIS was measured under various
fuel cell voltage conditions in the frequency range of 300 kHz~0.1Hz. ZView software
(Scribner Associate, Inc) was used to analyze the EIS spectra based on complex nonlinear
least-squares fitting [33].
85
5. 3 Results and Discussion
5.3.1 Surface engineered SOFC with thin YDC cathodic interlayer
Quantum simulations for Pt/YSZ and Pt/YDC systems
Using density functional theory (DFT) simulations, oxygen adsorption on Pt38 clusters on
YDC, YSZ, and YDC|YSZ surfaces as well as oxygen incorporation into vacancies in the
surface layer of the oxide from the Pt38 cluster were investigated. Oxygen incorporation
in YSZ was found to be slightly energetically favorable by 0.09eV as compared to the
state of atomic oxygen adsorbed on Pt (Figure 5-1(a)). The incorporation reaction is
activated by an energy barrier of 0.38eV. As the oxygen atom moves away from Pt,
energy goes uphill while the O-Pt bonds are broken, and the electron charge on the
oxygen atom initially decreases. Past the activated state, the oxygen atom begins to form
bonds with surface Zr atoms, the energy goes down, and the charge on the oxygen
increases. As the oxygen atom begins to move past the stable surface site down into a
subsurface layer, the charge increases further as well as the energy since there is no
vacancy below the diffusing oxygen in this geometry.
86
Figure 5-1. (a) Change in energy as a function of height for atomic oxygen diffusing into
a vacancy in the first layer of YSZ. Height and energy is referenced to the stable
adsorbed state. Charge, plotted on the right axis, is the electron density integrated within
a Wigner Seitz sphere of radius 0.82Å around the radius (a more positive value
corresponds to higher electron density). (b) Snapshots of atom structure as oxygen is
incorporated. Oxygen atoms are shown in red, Y in yellow, Zr in purple, and Pt in silver.
87
Figure 5-2. (a) Change in energy as a function of height for atomic oxygen diffusing into
a vacancy in the first layer of YDC. Height and energy is referenced to the stable
adsorbed state. Charge, plotted on the right axis, is the electron density integrated within
a Wigner Seitz sphere of radius 0.82Å around the radius. (b) Snapshots of atom structure
as oxygen is incorporated. Oxygen atoms are shown in red, Y in yellow, Ce in blue, and
Pt in silver.
88
Compared to YSZ, oxygen incorporation in YDC shows significantly lower activation
energy, 0.07eV, and the incorporated state is of even lower energy, 0.49eV below the
adsorbed state (see Figure 5-2(a)). The difference in oxygen reaction energetics between
YSZ and YDC suggests that the nature of subsurface layers may affect reaction
energetics, demonstrating that interactions beyond the first nearest neighbor may play an
important role in fluorite ceramics. For example, it is known that oxygen and yttrium in
YSZ tend to occupy second nearest neighbor positions [34, 35] whereas they prefer first
nearest neighbors in doped ceria [36]. Further research is required to better understand
the role of different oxidation states and to clarify the behavior of YSZ and YDC
regarding oxide ion incorporation.
Grain boundary free YDC cathodic interlayer
By utilizing PLD, epitaxial films of single crystalline YDC layers of various thicknesses
were deposited on single crystalline YSZ substrates (8-mol%, 1cm x 1cm x 300µm-
thick). The main objective of employing epitaxial YDC layers was to eliminate
contributions from grain boundary effects. Figure 5-3 shows XRD spectra taken on
epitaxial YDC thin films of different thicknesses grown on single crystalline YSZ (100)
substrates. Intensity axis (y-axis) is plotted in a log scale to make the lower intensity
peaks more clearly visible. Only a strong YDC (100) peak is visible throughout the
spectra, which indicates perfect epitaxy of YDC observed for thicknesses up to 130nm.
89
Also, we observed that the peak intensity ratio of YDC to YSZ increased (roughly about
1.9-4.3) as the YDC thickness was increased.
Figure 5-3. XRD patterns of PLD YDC films deposited on single crystalline YSZ (100)
substrate. Spectra show only (100) peak up to the film thickness of 130nm, which
indicates perfect epitaxial growth of YDC films.
90
Figure 5-4. I-V performance of YDC interlayered SOFC and YSZ-only control sample
measured at 450oC. The plot shows gradual performance enhancement up to about 50nm
of YDC interlayer thickness, beyond which the fuel cell performance remains unchanged
with increasing YDC thickness.
SOFC MEAs employing epitaxial YDC interlayers grown at the cathode side on single
crystalline YSZ substrates were fabricated with different YDC film thicknesses of ~8nm,
17nm, 50nm, and 130nm. After deposition of porous Pt electrodes on both sides, fuel cell
performance was measured at temperatures from 350oC to 450
oC. Cell performance
measured at 450oC is shown in Figure 5-4, which compares the polarization behavior for
the YSZ-only control MEA with those of the YDC/YSZ MEAs having different
thicknesses of the YDC interlayer. Open circuit voltage (OCV) values of the samples
were in the range of 1.02~1.10V for all measurement temperatures. As seen in Figure 5-
4, fuel cell performance improved with YDC interlayer thickness and the peak power
91
density increased more than 2-fold. It shows enhancement after introducing even ~8nm
thin YDC layer and the performance continually improved up to a certain interlayer
thickness. Considering the deposition mechanism, the observed behavior suggests that
PLD may not form a fully and uniformly covering YDC layer below 10nm range, but
possibly does so above 20nm. Interestingly, after about 50nm the cell performance does
not enhance any further and shows the same behavior with the thicker (130nm) interlayer
MEA. We speculate that the overall ohmic loss of the cell is dominated primarily by the
ionic resistance of the 300µm-thick YSZ bottom substrate, which is about three orders of
magnitude thicker than the YDC interlayer. This and the higher ionic conductivity of
YDC compared to YSZ at this measurement temperature result in a negligibly small
contribution by the YDC layer to the overall resistive loss in the cell.
Figure 5-5. EIS data of YDC interlayered fuel cell measured at different cell voltage
conditions at 400oC. Two loops are observed. The high frequency loop seems to be
independent of cell voltage, indicating that this arc corresponds to ionic transport through
the electrolyte (Rohmic). In contrast, the low frequency loop is dependent on cell voltage
indicating that this arc corresponds to the electrode interface resistance (Relectrode).
92
For further analysis of this surface engineering effect, EIS measurements were performed
for each sample at different measurement temperatures. Figure 5-5 shows a sample EIS
data for a 50nm thick YDC interlayer sample measured at 400oC. Two loops were
observed and a commonly used equivalent circuit model shown in the figure was adopted
to fit the spectra [14]. As shown in Figure 5-5, EIS measurements were made at several
DC bias voltages. While the electrode processes are highly affected by the magnitude of
cell voltage, the ionic transport resistance in the electrolyte is generally independent of
the cell voltage conditions. The high frequency loop shows no discernable changes for
three different cell voltage conditions, namely, OCV, 600mV, and 200mV, suggesting
that this arc corresponds to ionic transport through the electrolyte. However, voltage
dependence of the low frequency semi-circle suggests that this arc is associated with
electrode processes at the electrolyte/electrode interface [28-30]. Also, the capacitance
estimated for the low frequency arc is about 10-6
F/cm2, which is a typical value for
electrode processes, while the magnitude of the capacitance value for the high frequency
arc is in the order of 10-9
/cm2 [34].
For SOFCs, there is a general agreement that cathode reaction kinetics is considerably
more sluggish than the anode reaction such that the cathode reaction dominates overall
activation losses for the cell [4, 37]. Moreover, for our MEA fabrication, the reaction area
of anode side is about 5-fold larger than the active area of the cathode. Due to reasons
above, it is likely that the smaller anode loop is merged into the much larger cathode loop
93
resulting in only one semi-circle for the electrode process rather than two. By fitting the
obtained EIS data for all samples, individual contributions of electrolyte and electrode
interface impedances were determined.
As described above, we speculate that the incremental increase in electrolyte resistance
due to the additional YDC interlayer would be small and would not have an adverse
effect on fuel cell performance. Figure 5-6 shows the ohmic resistances of the pure YSZ
SOFC control sample and different thicknesses of YDC interlayered SOFCs measured at
temperatures from 350oC to 450
oC. As expected, there is no change in the ohmic
resistance due to the electrolyte and practically no dependence on the interlayer thickness
in this experimental regime. Clearly, the ohmic resistance for the surface modified SOFC
is primarily dominated by the thick YSZ substrate and the contribution from the YDC
interlayer thickness is negligible for all practical purposes.
94
Figure 5-6. Extracted ohmic resistances of YDC interlayered SOFCs for different YDC
thicknesses at temperatures of 350oC~450
oC. Zero in the x-axis indicates the bare YSZ
sample with no interlayer. The plot shows no discernable change in cell ohmic resistance
with increasing interlayer thickness up to 130nm.
Figure 5-7. Electrode interface resistance values for the YDC interlayered SOFCs with
different thicknesses extracted from impedance measurements. The resistance starts to
drop immediately after the introduction of a thin layer YDC (<10nm). After forming a
full covered YDC layer, the electrode resistance reaches a plateau, and does not change
with further increase in YDC thickness.
95
Figure 5-7 compares the measured electrode interface resistance for the YSZ-only control
MEA with YDC/YSZ MEAs for different interlayer thicknesses in the temperature
regime of 350oC~450
oC. During PLD, deposition is initiated with surface nucleation
followed by island formation on the substrate [38]. Hence, it is likely that full and
uniform surface coverage in films less than 10~20nm thick is difficult to achieve. To
examine the microstructure and verify the uniformity of surface coverage by the
interlayer, AFM topography scanning and surface sensitive XPS were conducted on YDC
interlayered samples. For AFM topography scanning, we picked two thickness points
from the data in Figure 5-7, one from the sloped region (~14nm) and one from the
saturated region (~80nm). Figure 5-8 shows the topography image of the three samples,
bare YSZ, ~14nm YDC, and ~80nm YDC, respectively. The images show clear
differences in topography and grain formation. However, due to the limitation of the
AFM tip aspect ratio in relation to the small grain sizes, it was difficult to confirm full
coverage of YDC interlayers on the YSZ substrate by AFM. For that reason, we also
employed angle resolved XPS measurements to determine the extent of surface coverage
of YDC interlayers. By tilting the sample stage of our XPS setup (15~30o) we were able
to limit the beam penetration depth to around 3nm or less. That arrangement excluded
signal detection from the underlying YSZ substrate and allowed signals only from the top
surface. Figure 5-9 shows the measured XPS data of interlayer samples with three
different thicknesses. The XPS spectra clearly show one of the main Zr peaks at ~186eV
96
for the sample containing ~8nm thin YDC layer indicating incomplete coverage. For the
17nm thick sample, the Zr peak intensity decreased as the YDC interlayer thickness
increases suggesting increasing coverage. Full surface coverage of YSZ by the YDC
interlayer is achieved possibly in the 30-50nm thickness range under the experimental
conditions employed in our study.
Figure 5-8. AFM scanned surface topography images of YDC interlayers with different
thicknesses. (Left) Bare single crystalline YSZ, (Center) ~14nm YDC, (Right) ~80nm
YDC on top of YSZ. It shows grain formation as the YDC thickness increases.
97
Figure 5-9. Surface sensitive XPS analysis of surface modified samples with three
different YDC thickness within the binding energy regime of one of the main Zr peaks.
As the YDC interlayer thickness increases Zr peak decreases and at the thickness about
26nm, almost no Zr peak is observed.
These results verify that for very thin YDC films possibly less than 30nm, the YSZ
substrate surface is not fully covered with the YDC interlayer but instead has patchy
coverage with open spaces between, where YSZ is exposed to the gas phase. With the
~26nm thick sample the Zr peak was practically indistinguishable from the background
suggesting that at this thickness the YDC film forms near full coverage. This helps
explain the reason why the cathode impedance initially displays a monotonic decrease
with increasing YDC thickness up to ~26nm. If on the other hand, the coverage at the
thinnest YDC layer were to result in full and uniform instead, then one would expect to
98
observe an abrupt drop in the electrode impedance in Figure 5-7 from the case featuring
bare YSZ cell to the case where the first YDC interlayer was introduced.
To observe the full effect of YDC interlayer on oxygen incorporation, therefore, complete
surface coverage of the YDC film on YSZ substrate is required. In Figure 5-7, a
noticeable drop in the interface resistance is clearly evident right after the introduction of
the first YDC interlayer. This trend continues as the YDC thickness is further increased
until it reaches a plateau value after about 50nm. This implies that initially the coverage
of the YDC layer is far from being complete, where the Pt electrode contacts directly the
YSZ surface in some regions. The cathode interfacial resistance decreases as the surface
coverage of the YDC film on YSZ increases until the entire active Pt cathode interface is
in full and direct contact with the YDC interlayer. As the XPS data shows, we expect to
have fully covering YDC layer after about 30nm and it would show same performance
behavior as the 50nm interlayer sample.
After forming a complete YDC layer, the interface resistance saturates for each
measurement temperature. Compared to the YSZ-only control sample, about a 2-fold
decrease in electrode interface resistance was achieved by employing single crystalline
YDC surface modified cathode interlayer. The results shown above clearly confirm that
the YDC interlayer itself enhances LT-SOFC performance by improving surface oxygen
kinetics.
99
Grain boundary and grain size contribution of YDC cathodic interlayer
To investigate YDC surface grain boundary activity, we first performed spectrometric
direct observation using isotope exchange method and secondary ion mass spectrometry
(SIMS) as a characterization tool. Figure 5-10(a) shows the SEM of the microstructure
and topography of the polycrystalline YDC pellet surface, indicating an average grain
size of 6+1µm. Sintered polycrystalline YDC pellets were also employed in oxygen
exchange experiments conducted under a cathodic DC bias of 1V while annealing in 18
O2
environment at 400°C. Surface activity for ORR was determined by the use of a high
spatial resolution SIMS (NanoSIMS) with a beam size less than 100nm. The NanoSIMS
image presented in Figure 5-10(b) as the 18
O/16
O ratio clearly indicates enhanced activity
along the grain boundary regions on the YDC surface. The 18
O/16
O count ratio in grain
boundary regions are about two times higher than that in bulk regions at this operation
condition. This result agrees well with previous work and observations in our laboratory
on YSZ surfaces, and confirming that this phenomenon is not unique to YSZ [39]. It also
provides spectrometric evidence that grain boundaries on the external surfaces of ionic
conducting oxides provide preferential sites for oxygen incorporation, possibly due to
higher concentration of vacancies in the grain boundary region [40].
100
Figure 5-10. (a) Surface SEM image of YDC sintered pellet, where dashed line shows
clear grain boundaries. (b) 18
O/16
O concentration map of corresponding YDC surface
obtained from NanoSIMS. 18
O/16
O count ratio was observed higher at grain boundary
regions (dashed) than bulk regions indicating oxygen isotopes were more populated in
grain boundary regions.
To study how grain size affects electrochemical behavior, YDC films were fabricated
with size-engineered surface grains at the cathode sides of the fuel cell elements. Size
engineering of grains was achieved by controlling the post annealing temperature for
these films. YDC surface microstructure of YDC/YSZ samples was determined by AFM.
Figure 5-11 shows the AFM topography images of YDC surfaces after post-annealing at
temperatures from 750oC to 1500
oC. As expected, lower annealing temperatures yield
smaller grain size in the sub-micrometer regime, namely, 55±15nm for 750oC (Figure 5-
11(a)) and 120±30nm for the 1100oC (Figure 5-11(b)) samples. Higher annealing
temperatures result in grain sizes 2.02±1.04µm for the 1300oC sample (Figure 5-11(c))
and 6.50±1.72µm for the 1500oC sample (Figure 5-11(d)) respectively. Figure 5-12
101
shows the resulting average grain sizes as a function of annealing temperature. This post
annealing process affects grain growth only in the thin YDC interlayer, but has no
significant effect on the grain size and microstructure of the underlying YSZ substrate. In
other words, the grain size of only the cathode interface has been varied in these
experiments while the grain size at bulk and the anode interface remained practically
unchanged. This was confirmed by our previous experiments using PLD YSZ thin
interlayers in our laboratory [39]. Therefore any significant variations in the
electrochemical behavior of these samples can be associated with the role of grain size at
the cathode interface.
Figure 5-11. AFM images of YDC surface additionally deposited on polycrystalline YSZ
substrate and post-annealed at different temperatures. (a) 750oC, (b) 1100
oC, (c) 1300
oC,
and (d) 1500oC.
102
Figure 5-12. Average grain size of YDC interlayer as a function of post-annealing
temperature.
The first set of experimental evidence supporting the role of grain size comes from fuel
cell measurements. After deposition of porous Pt electrodes on both sides of these
samples under identical sputtering conditions, their fuel cell performances were measured
at temperatures from 350oC to 450
oC using hydrogen as the fuel and air as the oxidant.
Open circuit voltage (OCV) values were in the range of 1.03V - 1.06V vs air for all
measured samples. Figure 5-13 shows the current-voltage (I-V) behavior of YDC/YSZ
composite SOFC samples measured at 400oC with varied grain sizes (or, grain boundary
densities) at the cathode side. The data show consistent improvement in the fuel cell
performance with decreasing grain size at the YDC surface. Indeed, the composite
sample having the smallest grain size at the YDC surface which corresponds to the
highest grain boundary density shows the highest peak power density and the lowest
103
activation loss. In other words, having more grain boundaries at the cathode interface
significantly enhanced the fuel cell performance in terms of peak power density by up to
4-fold and this enhancement is primarily due to improved cathode activation for the
oxygen reduction reaction.
In order to exclude the possibility of surface roughness effects contributing to increased
fuel cell performance, the average roughness of YDC surface was measured by AFM for
all samples. We measured multiple spots for each sample and found the root mean square
(RMS) roughness value was about 4-20nm. Based on our previous experimental results,
the contribution from such roughness values to the effective surface area is rather
marginal, with an estimated enhancement of only 1-3%. Therefore, one can exclude
surface area effects and conclude that the improvement in fuel cell performance with
decreasing grain size is primarily due to enhanced oxygen reduction kinetics, which is
consistent with SIMS results of Figure 5-10, and not from an increase in the effective
reaction site density due to surface roughness.
104
Figure 5-13. Current-Voltage (I-V) behavior of fuel cell MEAs measured at 400oC. Fuel
cells with smaller surface grain size show higher performance in terms of peak power
densities.
The second set of experimental evidence supporting the role of grain size (i.e., surface
grain boundary density) comes from electrochemical impedance spectroscopy (EIS)
measurements. Accordingly, the effect of the YDC grain boundary density at the cathode
side was studied by EIS for each sample at different temperatures. Figure 5-14 shows a
representative Nyquist plot for the 1500oC post-annealed composite sample measured at
350oC under various cell voltage conditions. The spectra indicates three arcs, where the
two high frequency arcs (arc I and arc II) showed no discernible change under three
different cell voltage conditions indicating that these two arcs are most likely associated
with ionic transport across bulk grains and grain boundaries, respectively [14]. The total
electrolyte resistance value, which is the sum of the two high frequency arcs, matches
well with the reference conductivity value for YSZ at the measured temperature [41-42].
105
Possible increase in electrolyte resistance due to the additional thin YDC layer can be
neglected since its contribution is merely 0.1% of the ohmic resistance of YSZ under this
experimental condition. The ionic conductivity of YDC is more than an order of
magnitude higher than that of YSZ at this temperature, and the thickness of added YDC
interlayer is almost three orders of magnitude smaller than the thickness of the YSZ
substrate. Thus, it can be assumed that ohmic resistance is primarily due to the YSZ bulk
substrate. This is also confirmed by recent experiments in our laboratory [43]. In contrast,
the low frequency arc is highly affected by the cell voltage conditions suggesting that this
arc corresponds to electrode processes, most likely associated with the cathode reaction
as discussed previously.
Figure 5-14. Electrochemical impedance spectroscopy (EIS) data of 1500oC annealed
YDC/YSZ composite fuel cell sample measured at 350oC indicating three loops. The two
high frequency loops seem to be independent of cell voltage conditions, indicating that
these arcs correspond to ionic transport through electrolyte and representing bulk (arc I)
and grain boundary (arc II).. whereas the low frequency loop shows dependence on cell
voltage conditions indicating that this arc corresponds to the electrode interface
resistance.
106
Figure 5-15. A plot showing extracted electrode interface resistances (at 450oC, 0.6V) as
a function of estimated surface grain boundary densities. As expected, the electrode
resistance decreases as the surface grain boundary density increases (lower grain sizes).
By using a representative equivalent circuit model, the values for electrolyte and
electrode (cathode) resistances are extracted for all measured samples. The representative
electrode interface resistance values (450oC at 0.6V cell voltage condition) were plotted
in Figure 5-15 as a function of surface grain boundary density estimated from values in
Figure 5-12. As expected, the electrode resistance decreases with increasing surface grain
boundary density. This clearly indicates that the YDC surface grain boundary enhances
the oxygen exchange rate at the cathode surface. In addition, exchange current densities,
which are highly related to the charge transfer reaction rate at the cathode, were
calculated from the measured EIS and I-V data. From the measured I-V fuel cell
107
performances, the exchange current density (j0) was extrapolated by fitting the activation
or polarization loss (ηact) and current density (j) values with the Tafel approximation [43]:
0
lnj
j
nF
RTact
(6.1)
where R is the ideal gas constant, α is the charge transfer coefficient, n is the number of
electrons involved in the electrode interface reaction, and F is the Faradic constant.
Figure 5-16 shows the results for all the YDC/YSZ composite samples measured in the
temperature regime of 350oC-450
oC and indicates activation energies of 0.62-0.66eV.
The composite 1500oC annealed sample having the largest grain size (5~7µm), i.e., the
lowest density of surface grain boundaries, has shown the lowest exchange current
density values. It is consistently observed that cathodic interface resistances of the
samples decrease as the grain size of the YDC interlayer decreases by lowering the post-
annealing temperature. The resistance values for the nano-grain size sample (40~70nm)
which was annealed at the deposition temperature of 750oC showed the lowest resistance
values, about 6~7-fold less compared to that of the largest grain sample, at each
measurement temperature. Results in Figure 5-16 and the EIS analysis indicate that the
exchange current density as well as the cathodic interface resistance scales with grain
size, more precisely, the grain boundary density on the YDC surface. Smaller surface
grains naturally generate higher grain boundary density at the cathode interface. The fuel
cell MEA with higher YDC surface grain boundary density (i.e. smaller grain size) shows
108
higher exchange current densities. This study clearly demonstrates that such nano-
granular surface microstructure gives rise to higher charge transfer rate at the cathode
side. Based collectively on the results presented in this study, we postulate that YDC
surface grain boundaries serve as active sites for enhanced oxygen exchange kinetics.
Figure 5-16. Exchange current densities for all measured samples with different grain
sizes were calculated at temperatures 350oC-450
oC. As the surface grain size decreases
(i.e., higher grain boundary density), the electrode interface resistance decreases. This
indicates that the surface grain boundaries enhance oxygen surface kinetics at the cathode
side.
109
5.3.2 Surface engineered SOFC with thin GDC cathodic interlayer
Upon the YDC cathodic interlayer experimental results shown above, we investigated
another dope ceria, which is gadolinia doped ceria, as a cathodic interlayer for LT-SOFC.
We adopted similar experimental scheme to study the role of GDC on oxygen kinetics.
As shown in previous section, we first studied the effect of GDC material itself as an
interlayer using grain boundary free GDC thin film. Then, we investigated the
contribution of GDC grain boundaries on oxygen kinetics.
110
Grain boundary free GDC cathodic interlayer
Figure 5-17. X-ray diffraction patterns of (a) epitaxial and (b) fully developed
polycrystalline GDC films on single (100) and polycrystalline YSZ substrates,
respectively.
Figure 5-17(a) shows the x-ray diffraction pattern of the first experimental set using a
single crystalline YSZ (100) substrate. About 60nm of a GDC layer is deposited on the
cathode side. In the spectra in Figure 5-17(a), only the strong (100) peaks of GDC and
YSZ are visible, indicating the epitaxially grown GDC layer on the YSZ (100) substrate.
The main objective of this first experimental set was to exclude grain boundary
contributions and to observe only the cathodic interlayer effect on surface oxygen
kinetics.
111
Figure 5-18. Current-voltage (I-V) behavior of epitaxial GDC interlayered MEA,
measured at 450oC. The SOFC MEA with GDC interlayer shows about 2-fold higher
peak power density.
After depositing porous Pt catalytic electrodes on both sides, SOFC MEA fabrication
employing epitaxial GDC cathodic interlayer was completed and the fuel cell
performance was measured at temperatures from 350oC to 450
oC. Figure 5-18 shows
representative current-voltage behavior data measured at 450oC, comparing an MEA
made of pure YSZ electrolyte with that employing epitaxial GDC interlayer electrolyte.
Open circuit voltages (OCVs) were 1.04V for the YSZ-only control cell and 1.05V for
the interlayered cell, respectively. The measured peak power density of the interlayered
cell is about 1.9 times higher than that of the control YSZ sample. From previous
experiments conducted in our laboratory we know that the increase in ohmic resistance
due to the thickness of the additional layer on the cathode side is almost negligible [44],
112
since the ionic conductivity of GDC is more than an order of magnitude higher in that
measurement temperature regime. Also, the interlayer thickness is more than three orders
of magnitude higher than the bottom substrate thickness (300µm). Therefore, the ohmic
resistance primarily due to the ionic resistance of the thick YSZ bottom substrate. Figure
5-18 suggests that losses for the YSZ control cell are larger than that of the GDC
interlayered cell. To find out why this is the case and to further investigate the effect of
the GDC interlayer on cathodic interface resistance, EIS measurements were performed
at same temperature range under different cell voltage conditions. Similar to the
experiment using single crystalline YDC interlayer in previous section, electrode
interface resistances were extracted by using an equivalent circuit model. It showed about
1.75times lower interface resistances for the epitaxial GDC layer cell than for the YSZ
control cell. This result suggests that GDC exhibits faster surface oxygen kinetics than
YSZ and it is consistent with YDC.
Figure 5-19. Atomic force microscopy (AFM) topography images of GDC surfaces,
annealed at (a) 750oC, (b) 1200
oC, and (c) 1450
oC. As the post-annealing temperature
increases, the grain size also increases.
113
To investigate the role of GDC surface grain boundaries on oxygen kinetics, interlayered
SOFC MEAs were fabricated with different grain sizes (i.e., grain boundary densities) at
the cathode side by a post-annealing process. Fully developed polycrystalline GDC thin
layers were observed on polycrystalline YSZ (Figure 5-17(b)). The microstructure of
cathodic GDC grains was determined by AFM. Figure 5-19 shows the AFM topography
images of the GDC interlayer surfaces annealed at temperatures from 750oC to 1450
oC.
The grain size increases as the post-annealing temperature increases. Estimated grain
sizes are about 61±11nm, 198 ± 22nm, and 5.74±1.56um for 750oC, 1200
oC, and 1450
oC
annealed samples, respectively (Figure 5-19(a), (b), and (c)). In previous section of this
chapter, we confirmed with YDC/YSZ composite electrolyte that this post-annealing
process changes only the grain sizes of the YDC cathodic interlayer with no significant
effect on the grain structure of the underlying thick YSZ substrate, including its bulk and
its anode side surface. Therefore, also in this case, the difference in the electrochemical
behavior of samples can be attributed to the effect of grain microstructure of the cathode
interface.
114
Figure 5-20. I-V performance at 450oC of GDC/YSZ composite electrolyte MEAs with
different GDC surface grain sizes,. The smaller surface grain size sample (lower
annealing temperature), which corresponds to the higher surface grain boundary density,
shows higher peak power density.
Figure 5-20 shows a representative I-V performance of GDC/YSZ composite electrolyte
fuel cells with different cathodic grain sizes operated at 450oC. The measured OCVs were
1.01V-1.06V for all fuel cell samples. As expected, the MEA with smaller GDC grain
size shows higher performance in terms of peak power density and reduced activation
loss. This supports previous experiment and simulation results conducted in our
laboratory that point to higher concentration of oxygen vacancies at grain boundary
regions, which provide more reaction sites for ORR [9, 36]. Hence, we postulate that
nano-granular GDC with increased grain boundary density improves cell performance by
enhanced surface oxygen exchange at the cathodic surface. This is experimentally
verified by systematic variation of grain structure of GDC/YSZ composite electrolyte.
115
Figure 5-21. Arrhenius plot of cathodic interfacial resistances of MEAs with different
GDC surface grain sizes. As the post-annealing temperature increases (i.e., as the surface
grain boundary density decreases), the electrode interfacial resistance increases. MEAs
with nano-granular GDC surface grains show lower electrode interfacial resistances than
those with larger surface grain size.
Similarly, EIS measurements at temperatures of 350oC-450
oC were conducted on MEAs
featuring different GDC surface grain sizes. Using an equivalent circuit model which was
mentioned for YDC case in previous section, the electrode and GDC interface resistances
were extracted. Figure 5-21 presents the Arrhenius behavior of electrode interfacial
resistance for cells with different GDC grain boundary densities. The GDC/YSZ
composite MEA annealed at 1450oC, which has the largest grain size (~6µm), in other
words, the lowest grain boundary density on the surface shows the largest cathodic
interface resistance. As the post-annealing temperature decreases, interfacial resistances
consistently decrease due to increased grain boundary density. The composite MEA
116
annealed at 750oC with the GDC surface grain size of about 65nm (i.e., large grain
boundary density) shows the lowest cathodic interfacial resistance, about 5-6 times lower
than the MEA with the largest grain size sample that was annealed at 1450oC. Moreover,
EIS analysis clearly indicates that cathodic interface resistance scales well with the size
of surface grains, i.e., the surface grain boundary density on the GDC surface. These
results also support both simulation and experimental studies previously conducted in our
laboratory that were also based on the hypothesis that surface grain boundaries enhance
oxygen reduction kinetics.
5.4 Conclusion
In this chapter, we investigated engineering effect of doped ceria (YDC and GDC)
interlayers at the cathode side of YSZ electrolyte and the role of doped ceria surface grain
boundaries on LT-SOFC performance. Quantum mechanical simulations demonstrated
reduced activation energy and a larger energetic driving force for oxygen incorporation in
YDC as compared to YSZ. Surface mapping of 18
O and 16
O ions by a high spatial
resolution NanoSIMS indicated preferential enrichment of 18
O along grain boundaries on
the YDC external surface. For fuel cell performance characterization, epitaxial doped
ceria thin interlayers (both YDC and GDC) on single crystalline YSZ (100) substrate
helped decrease cathodic interfacial resistance due to their faster surface exchange rate
than that of YSZ. Composite electrolyte fuel cell MEAs with different doped ceria’s grain
117
sizes (from about 40nm to 6µm) indicated that MEAs with smaller surface grain size (i.e.,
higher surface grain boundary density) showed superior fuel cell performance in terms of
higher peak power density and lower cathodic interface resistance. Moreover, the
exchange current densities were calculated and showed similar trend that higher surface
grain boundary density results the higher charge transfer rate. These results suggest that
grain boundary regions are electrochemically more active and nano-granular surface
grains enhance surface oxygen exchange rate.
This study successfully demonstrates the substantial effect of thin YDC, GDC cathode
interlayer and size of surface grains on cell behavior. Results of this study provide
significant implications in designing nano-granular YDC surfaces to achieve enhanced
LT-SOFC performance by improving oxygen surface kinetics.
5.5 References
[1] B. C. H. Steel, A. Heinzel, Nature, 414, 345–352 (2001)
[2] N. P. Brandon, S. Skinner, B. C. H. Steele, Annu. Rev. Mater. Res., 33, 183–213
(2003)
[3] X. Chen, N. J. Wu, L. Smith, A. Ignatiev, Appl. Phys. Lett., 84, 2700–2 (2004)
[4] S. de Souza, S. J. Visco, L. C.De Jonghe, Solid State Ionics, 98, 57–61 (1997)
118
[5] A.V. Virkar, Low-temperature Anode-supported High Power Density Solid Oxide
Fuel Cells with Nanostructured Electrodes, University of Utah (2003)
[6] U. P. Muecke, D. Beckel, A. Bernard, A. Bieberle-Hu tter, S. Graf, A. Infortuna, P.
Muller, J. L. M. Rupp, J. Schneider, L. J. Gauckler , Adv. Funct. Mater., 18, 3158–
3168 (2008)
[7] P.-C. Su, C.-C. Chao, J. H. Shim, R. Fasching, and F. B. Prinz, Nano Lett., 8, 2289
(2008)
[8] J. H. Shim, C.-C. Chao, H. Huang, and F. B. Prinz, Chem. Mater.,19, 3850 (2007)
[9] H. Huang, M. Nakamura, P. Su, R. Fasching, Y. Saito, and F. B. Prinz, J.
Electrochem.Soc., 154, B20 (2007)
[10] H. Huang, T. M. Gür, Y. Saito, and F. Prinz, Appl. Phys. Lett., 89, 143107 (2006)
[11] A. Evans, A. Bieberle-Hutter, J. L.M. Rupp, L. J. Gauckler, Journal of Power
Sources, 194, 119–129 (2009)
[12] B.C.H. Steele, Solid State Ionics, 129, 95 (2000)
[13] J. A. Kilner, Solid State Ionics, 129, 13-23 (2000)
[14] H.L. Tuller, Solid State Ionics, 131, 143-157 (2000)
[15] A.V. Virkar, J. Electrochem. Soc., 138, 1481–1487 (1991)
[16] K. Eguchi, T. Setoguchi, T. Inoue, H. Arai, Solid State Ionics, 52, 165–172 (1992)
[17] T. Tsai, S. A. Barnett, Solid State Ionics, 98, 191-196 (1997)
[18] T. Hibino, A. Hashimoto, T. Inoue, J. Tokuno, S. Yoshina, M. Sano, Science, 288,
2031 (2000)
[19] H. Uchida, M. Yoshida, and M. Watanabe, J. Phys. Chem., 99, 3282 (1995)
119
[20] B. C. H. Steele, Solid State Ionics, 75, 175 (1995)
[21] B. C. H. Steele, K. M. Hori, S. Uchino, Solid State Ionics, 135, 445 (2000)
[22] J. A. Lane, J. A Kilner, Solid State Ionics, 136-137, 927 (2000)
[23] H. Huang, T. Holme, F. B. Prinz, J. Fuel Cell Sci. Tech., 7, 1-5 (2010)
[24] C. W. Tanner, K. Z. Fung, A. V. Virkar, J. Electrochem. Soc., 144, 21–30 (1997)
[25] S. H. Chan, X. J. Chen, K. A. Khor, J. Electrochem. Soc., 151, A164–A172 (2004)
[26] G. Kresse and J. Hafner, Phys. Rev. B, 47, 558 (1993)
[27] G. Kresse and J. Hafner, Phys. Rev. B, 49, 14251 (1994)
[28] G. Kresse and J. Furthmüller, Comput. Mat. Sci., 6, 15 (1996)
[29] G. Kresse and J. Furthmüller, Phys. Rev. B, 54, 11169 (1996)
[30] G. Kresse, J. Joubert, Phys. Rev. B, 59, 1758 (1999)
[31] J.P. Perdew, J. A. Chevary, S. H. Vosko, K. A. Jackson, M. R. Pederson, D. J.
Singh, C. Fiolhais, Phys. Rev. B, 46, 6671 (1992)
[32] H. J. Monkhorst, J. Pack, Phys. Rev. B, 13, 5188 (1976)
[33] E. Barsoukov, J. R. Macdonald, Impedance Spectroscopy: Theory, Experiment, and
Applications, 2nd ed., Wiley, New York (2005)
[34] P. Li, I.W. Chen, J.E. Penner-Hahn, Phys. Rev. B, 48, 10074 (1993)
[35] G. Stapper, M. Bernasconi, N. Nicoloso, M. Parrinello, Phys. Rev. B, 59, 797 (1999)
[36] H. B. Lee, F. B. Prinz, W. Cai, Acta Materialia, 58, 2197–2206 (2010)
[37] T. Holme, R. Pornprasertsuk, F. Prinz, J. Electrochem. Soc., 157, B64-70 (2009)
[38] J. D. Ferguson, G. Arikan, D. S. Dale, A. R. Woll, J. D. Brock, Physical Review
Letters, 103(25): 256103 (2009)
120
[39] J. Shim, J. Park, T. Holme, K. Crabb, W. Lee, Y. B. Kim, X. Tian, T. M. Gür, F. B.
Prinz, Acta Materialia (2011) submitted.
[40] W. Lee, M. Lee, H.-J. Jung, F. B. Prinz, Meet. Abstr. Electrochemical Society, 1001,
724 (2010)
[41] S. M. Haile, Acta Materialia, 51, 5981-6000 (2003)
[42] B. C. H. Steele, Mat. Sci. and Eng., 79, B13 (2002)
[43] R. O’Hayre, S. W. Cha, W. Colella, F. B. Prinz, Fuel Cell Fundamentals, Wiley,
New York (2005)
[44] Y. B. Kim, T. Holme, T. M. Gür, F. B. Prinz, Adv. Func. Mater.,
10.1002/adfm.201101058 (2011)
121
CHAPTER 6. Three-Dimensional Proton Conducting Fuel Cell
Architecture with Ultra Thin Ceramic Electrolyte
As a reaction surface engineering for SOFC, we investigated a novel method for creating
three-dimensional (3-D) fuel cell architecture to enhance fuel cell performance by
increasing the area of electrolyte membrane. This chapter presents the fabrication and
operation of a low temperature 3-D protonically conducting ceramic fuel cell featuring a
close packed and free standing crater patterned architecture achieved by nanospherical
patterning (NSP). The cell employed conformal layers of yttrium-doped barium zirconate
(BYZ) anhydrous electrolyte membrane (~120nm) sandwiched between thin (~70nm)
sputtered porous Pt electrode layers. The fuel cell structure achieved the highest reported
peak power densities up to 186 mW/cm2 at 450
oC using hydrogen as fuel.
6.1 Introduction
Lowering the operating temperature of ceramic fuel cells is desirable to circumvent issues
related to stability of cell materials and performance. In this regard, there have been
studies in our laboratory [1, 2] and by others [3-6] that aim at achieving lower operating
122
temperatures primarily by employing thin film solid oxide fuel cell (SOFC) structures
with yttria stabilized zirconia (YSZ) electrolyte membranes that exhibit transport of oxide
ions in the oxygen sublattice with activation energies of ~1eV.
Alternatively, proton conducting anhydrous ceramic electrolytes offer opportunities to
lower the operating temperature of oxide-based fuel cells due to high ionic conductivity.
Proton transport in several members of acceptor-doped perovskites of the general formula
ABO3 is reported to be fast, with activation energies of about 0.45eV [7], which makes
them of interest as potential solid electrolytes for next generation protonic devices such
as fuel cells, electrolyzers, hydrogen sensors, and gas reformers [7-18]. Proton transport
in these anhydrous oxides occurs via the Grotthuss mechanism through hydroxide defects
that are produced by water incorporation into oxide ion vacancies generated in the crystal
lattice upon extrinsic doping of the tetravalent Zr+4
site by the trivalent Y+3
ion. Among
the anhydrous oxides, yttrium-doped BaZrO3 (BYZ) shows better chemical stability in
acidic gas environments, as well as higher proton conductivity than doped BaCeO3 in the
intermediate temperature regime [7, 16].
We have previously reported on the fabrication, properties, and performance of thin film
planar (2D) fuel cells employing both oxide ion conducting yttria-stabilized zirconia
(YSZ) [1] and proton conducting BYZ membrane electrode assemblies (MEAs) made by
MEMS processing [19]. A recent report provides an extensive review of previous studies
and cell performance results for micro-fuel cells with planar geometries [6].
123
This study reports on the first fabrication and operation of a three-dimensional (3-D)
close packed crater shaped thin film proton conducting ceramic fuel cell MEA using
nano-sphere patterning (NSP) towards achieving enhancement in the effective reaction
surface area. Equally important, such a 3-D architecture is expected to be mechanically
more compliant than planar thin films, although no mechanical testing to verify this
hypothesis was undertaken as part of this research. This paper also reports the fuel cell
performance of this 3-D BYZ MEA structure in the temperature range of 350~450oC.
Similar work in our laboratory aimed at enhancing mechanical stability as well as
increasing the electrochemical reaction area was recently reported for a 3-D solid oxide
fuel cell (SOFC) that featured cylindrical cup architecture with vertical walls [2]. In
comparison, the NSP method described in the present study offers simplicity in
fabrication and also yields slanted walls, which facilitate effective and conformal coating
of the side walls with porous electrode layers even using an inherently directional
physical vapor deposition (PVD) method such as sputtering. This opens up wide range of
material selection for electrolytes and electrodes.
124
6.2 Experimental
The sequence of NSP and MEMS processing depicted in Figure 6-1 produces a silicon
nano-trench structure upon which the BYZ fuel cell MEA is fabricated. First, spherical
silica particles with 700nm diameter were created by a modified Stöber synthesis
technique. Using a Langmuir-Blodgett (L-B) trough, the silica particles were transferred
onto a silicon (100) substrate to form a close-packed monolayer. Then, plasma etching is
used to uniformly reduce the size of the particles to open up sufficient spacing among the
particles for the deposition of the metal mask. A dense aluminum (Al) layer (~100nm) is
deposited by DC magnetron sputtering at a partial pressure of 1Pa argon (Ar) and 100W
power at room temperature (Figure 6-1(b)). The silica particles were mechanically
removed from the substrate by ultra sonication leaving behind a nano-pore structured Al
layer on the silicon substrate (Figure 6-1(c)). Using this metal layer as a mask and
reactive ion etching (RIE) in a gaseous environment of sulfur hexafluoride (SF6) and
chlorodifluoromethane (CHClF2), combined processes of isotropic and anisotropic
etching is carried out to form the silicon nano-trench structure (Figure 6-1(d)). 100nm
thick conformal low stress nitride layers are deposited on both sides of the wafer by low
pressure chemical vapor deposition (LPCVD) (Figure 6-1(e)). A square opening is
created on the backside of the Si wafer using a simple photolithography process for
solution etching. The backside of the silicon template is then etched in 30% potassium
hydroxide (KOH) solution at 85~90oC for 5 hours utilizing the top silicon nitride as an
125
etch stop layer (Figure 6-1(f)). A free-standing crater shaped silicon nitride layer is thus
created in the square opening with a projected dimension of 100µm x 100µm.
Figure 6-1. Schematic illustration of the NSP processing sequence for the fabrication of
3-D crater patterned freestanding fuel cell MEAs. (a) Si substrate. (b) Silica particles with
Al layer on Si wafer. (c) Al mask after removing the particles. (d) Formation of trenches
by RIE etching. (e) Silicon nitride deposition. (f) Removal of Si template by KOH
etching. (g) Depositing BYZ and removal of the nitride layer by dry etching. (g)
Sputtering of porous Pt catalyst/electrode (dots) deposited on both sides (h).
126
120nm thick BYZ electrolyte layer is grown on this 3-D nitride template at 400oC at a
rate of 0.28Å /pulse by pulsed laser deposition (PLD) (Figure 6-1(g)) using a sintered
BaZr0.8Y0.2O3-δ target (Praxair Inc.) separated by 65mm from substrate. A Lambda Physik
248nm KrF excimer laser with energy density of 1.8J/cm2 per pulse was used for ablating
the target in 100mTorr oxygen environment. Samples cooled down naturally in 300Torr
oxygen pressure. After removing the nitride layer by plasma etching, 70nm thick porous
platinum electrodes were deposited at room temperature by DC sputtering at 50kW and
10Pa Ar pressure on both sides of the BYZ membrane to complete fabrication of the 3-D
crater patterned BYZ fuel cell MEA (Figure 6-1(h)).
Fuel cell performance was measured inside a test chamber using a micro-manipulating
probe station developed earlier [1]. Pure dry H2 was supplied to the anode side while the
cathode was exposed to ambient air. Gamry Potentiostats and Echem Analyst software
(Gamry Instruments) were used for fuel cell testing. Electrochemical impedance
spectroscopy (EIS) measurements were performed at various cell voltages in the
frequency range of 300 kHz - 1Hz.
127
6.3 Results and Discussion
The SEM images along the fabrication sequence of the silicon nano-trench structure and
the crater shaped BYZ electrolyte fuel cell MEA are shown in Figures 6-2 and 6-3,
respectively. The resulting silicon nano-trenches have depths of about 550-600nm. The
shape of the trenches is 3-D trapezoidal rather than semispherical or conical, due to the
isotropic/anisotropic etching recipe employed in the fabrication process. Due to the
beveled (or slanted, as opposed to vertical) walls of the trenches, a conformal BYZ
coating about 120nm thick was possible to achieve with PLD (Figure 6-3). The cross-
sectional SEM image (Figure 6-3(d)) of the finished crater patterned MEA shows the Pt
electrode layers (~70nm) whose porosity was estimated to be around 30-40%. Naturally,
the purpose of having porous electrodes is to increase the electrochemically active region,
i.e., the triple phase boundary (TPB). As expected, the upper side of the BYZ layer is
slightly thicker than inside the trenches due to the directional deposition mechanism of
PVD. Nevertheless, conformality of both the BYZ and Pt layers were satisfactory. The
inside surfaces of the crater structure adopt a quadrangular pyramid shape that resemble a
crater. Using high resolution SEM images, the geometric enhancement achieved in the
surface area by this 3-D structure is estimated to be about a factor of 1.7-1.8 per projected
planar area.
128
Figure 6-2. SEM images of, (a) silicon nano-trenches after removal of spherical particles,
(b) silicon nano-trench structure created after gas phase etching, (c) free-standing 3-D
nitride template after removing the backside silicon by KOH etching.
129
Figure 6-3. SEM images of the crater patterned BYZ fuel cell MEA, (a) after BYZ
deposition on the 3-D nitride template, (b,c) after porous Pt electrodes are coated on both
sides of the membrane, and (d) finished 3-D BYZ MEA taken from an angle of 52o from
the top (d).
130
Further microstructural analysis of the BYZ grain structure was carried out using a
transmission electron microscopy (TEM). BYZ specimens were made using a focused ion
beam (FIB, FEI Strata 235DB dual-beam FIB/SEM) lift-out Omniprobe technique
employing a Ga ion beam at 30 keV. Due to difficulties in preparing TEM specimens
directly from the 3-D MEAs, a planar 120nm thin BYZ film was deposited under
identical PLD conditions on a silicon wafer with silicon nitride overcoat. Cross-sectional
high-resolution (HRTEM) images and selected area diffraction (SAD) patterns were
taken by an FEI Tecnai G2 F20 X-TWIN microscope operated at 200 kV. The HRTEM
images and SAD patterns of this surrogate sample shown in Figure 6-4 clearly indicate a
dense columnar BYZ film with clean grain boundaries extending vertically through the
film thickness, making a well-defined interface with silicon nitride. Although the HR-
TEM images in Figure 6-4 were not produced from the 3-D MEAs, the microstructure of
the surrogate sample is nevertheless expected to represent the BYZ film in the actual
MEAs.
Results of electrochemical impedance spectroscopy (EIS) and cell performance of the 3-
D MEA are presented in Figure 6-5(a) and 6-5(b) respectively, for the fuel cell,
Air, Pt/BYZ/Pt, pure H2 (6.1)
131
In this fuel cell the transporting specie is protons, and consequently, the oxidation
product H2O forms at the air electrode (i.e., cathode) by the net reaction
eOHOH 22
12 22 . This is in contrast to SOFC based on oxide ion conducting
YSZ electrolyte, where the net cathode reaction is the reduction of molecular oxygen to
oxide ions ( 2
2 22
1 OeO ) while the oxidation reaction to form H2O occurs at the
H2 electrode (i.e., anode).
Figure 6-4. Cross sectional HRTEM images ((a) and (c)) showing the dense columnar
grain structure, and, (b) the SAD pattern indicating the fully developed polycrystalline
nature of the BYZ film.
132
The EIS spectra taken at cell voltages of 0.7 and 0.9V indicate two semi-circles. The high
frequency semi-circle in Figure 6-5(a) shows no discernable changes with varying
voltage while the second semi-circle at lower frequencies is significantly affected. This
suggests that the first semicircle is due to the BYZ electrolyte, and indeed, the impedance
of the high frequency loop matches the expected ohmic resistance. The second semicircle
at the lower frequency regime is due to electrode processes, and to a large extent due to
the cathode because of significantly higher polarization at the cathode than at the anode
reported for similar ceramic-based protonic fuel cells [20-22].
133
Figure 6-5. (a) Electrochemical impedance spectra at 400oC at cell voltages of 0.9V and
0.7V, with inset showing the details of the high frequency region, and (b) voltage-
current-power density (V-I-P) behavior of 3-D crater patterned BYZ fuel cells measured
at 350-450oC using hydrogen fuel.
134
Cell polarization curves in Figure 6-5(b) indicate significant activation loss. Open circuit
voltages (OCV) and peak power densities, respectively, were 1.01V and 30mW/cm2
at
350oC, 0.87V and 69mW/cm
2 at 400
oC, and 0.85V and 186mW/cm
2 at 450
oC. The
performance of the 3-D MEAs demonstrated at 350-450oC in this study is superior to
other studies reported in the literature, even after accounting for the enhancement in the
surface area. For example, Peng et al. recently reported 25mW/cm2 at 800
oC with a
protonic fuel cell employing pure hydrogen as fuel and featuring a 10µm thick ZnO-
doped BYZ membrane with porous Pt electrodes, while the performance of a similar cell
with 1mm thick BYZ at the same temperature was less than 4mW/cm2 [23]. Similarly,
Traversa and coworkers have reported power densities of 7mW/cm2 at 700
oC for protonic
cell with 0.6mm thick BYZ [24] and more recently, 110mW/cm2 at 600
oC from a cell
employing pulsed laser deposited BYZ membrane [25]. More recently, Sun et al
employed 20µm thick BYZ membrane on NiO/BaZr0.1Ce0.7Y0.2O3 cermet anode support
with a Sm0.5Sr0.5CoO3–Ce0.8Sm0.2O2 composite cathode and achieved 170mW/cm2 at
700oC [26].
Although the performance values achieved in this study are arguably the highest reported
in the literature for BYZ based protonic fuel cells in this intermediate temperature
regime, they are nevertheless several fold inferior to other reports especially those from
our own laboratory that employed hydrogen fuel in thin film oxide ion conducting
SOFCs in the same temperature regime [1, 2]. This is intuitively puzzling, since proton
diffusion in BYZ is inherently orders of magnitude faster than oxide ion transport in YSZ
135
in the same temperature regime. We have several speculations for this lower performance
than expected. First, we suspected that the reason for inferior performance may be due to
the formation of a carbonate layer (i.e., BaCO3) at the air side on the BYZ surface, which
would then severely block both electron and proton transport. In this temperature regime,
Kreuer’s data suggest that BYZ would be susceptible to form a carbonate layer with CO2
in the ambient air that has nominally a CO2 concentration of about 380ppmv [7]. Indeed
XPS analysis of the BYZ films kept in a covered sample box in ambient air for a week
indicated clear presence of a carbonate formation.
To determine BYZ’s propensity for carbonate formation due to susceptibility to CO2 in
the ambient air, we deposited a BYZ thin film by PLD on a 100 nm low stress silicon
nitride film grown by LPCVD on a silicon wafer. The PLD process conditions and
thickness of this 2-D sample were maintained the same as that for the 3-D BYZ MEA.
The BYZ film sample was stored inside a sample box with the lid closed (but not air-tight
sealed). After one week of minimal exposure to ambient air in the laboratory at room
temperature, the surface composition of the BYZ film was characterized in x-ray
photoelectron spectroscopy (XPS) using Physical Electronics (PHI) Quantum 2000
scanning ESCA microprobe with monochromatic Al Kα X-ray source (h = 1486.6 eV).
The depth profile of the BYZ sample was obtained with 1 keV Ar+ ion sputtering. The
carbon content was 37% at the surface but decreased monotonically with the sputtering
depth.
136
0 10 20 30 400
10
20
30
40
50
60
70
Ato
mic
concentr
ation (
%)
Depth (nm)
C
O
Y
Zr
Ba
Figure 6-6. Compositional depth profiles of the PLD BYZ film.
Figure 6-7: The high resolution C1s
spectra show two peaks at ~285.0eV and ~289.9eV
assigned to surface contamination and to CO32-
(possibly in the form of BaCO3)
environment, respectively.
137
To analyze the bonding state of the carbon, high resolution XPS scans for C1s
peak were
performed at each depth (Figure 6-7). At the surface, two C1s
peaks were observed. The
one near 285.0eV is the signature for surface contamination commonly observed due to
species in the ambient, but the other C1s
peak at 280.9eV represents carbon in CO32-
state.
The C1s
peak around 280.9eV was strongest at the surface and decreased with depth. This
matches well with the diminishing carbon content below about 20nm as shown in Figure
6-6. Thus, the carbon in the BYZ film is identified as carbonate, providing strong
evidence to suggest carbonation of the BYZ sample, most likely into BaCO3.
Also, observed OCV values were somewhat lower than theoretically expected. We
suspect that this is most likely due to gas leakage through the Au-ring seals in the cell
holder, or chemical shorting across broken MEA windows on the chip. The latter is a
frequent problem with free-standing MEA windows due to the uncontrolled mechanical
force exerted by the microcontacting probe during electrochemical testing. Existence of
pinholes in the BYZ layer, not uncommon in thin PLD films, may also be responsible.
The possibility of electronic conductivity in BYZ is less likely at these temperatures.
Indeed, oxide ion transference number in (Ba,Ca)(Zr,Y)O3 is measured to be 0.97-0.99 in
dry atmosphere at high temperatures between 600 and 1000oC [20]. The balance is most
likely due to protonic conduction. A similar finding was reported by Bonanos [27] at
138
elevated temperatures. So electronic conduction in BYZ at 350-450oC may be negligibly
small, and most likely, would not account for low OCVs.
In addition, it is known that the proton conductivity of BYZ through the grain boundary
is very low due to extremely high resistance. PLD BYZ film on the silicon nitride formed
polycrystalline with nano size grains. This high grain boundary density might lower the
proton conductivity of the BYZ electrolyte. Details regarding the relationship between
crystal structure of BYZ and proton conductivity will be discussed in the next chapter.
Although quantitative comparison of 3-D BYZ cell performance reported in this study
with 2-D BYZ cells reported earlier [19] is not meaningful due to poor control of
reproducibility of the Pt/BYZ interfacial microstructure, 120mW/cm2 reported earlier for
the 2-D PLD BYZ cell at 450oC [19] scales with 186mW/cm
2 for the 3-D cell at this
temperature by a factor of ~1.5. Since the cathode largely dominates overall cell behavior
[20-22] this scaling factor is also representative of the relative cathodic losses observed
for the 3-D (this study) and planar BYZ geometries [19]. This is in general agreement
with 1.7-1.8 enhancement in the geometric area achieved by the 3-D architecture.
139
6.4 Conclusion
This study constitutes the first reporting of three-dimensional crater patterned proton
conducting MEAs that were successfully fabricated and operated in fuel cell mode. The
3-D fuel cell architecture, which consisted of conformal layers of 120 nm thick BYZ
electrolyte with 70nm porous Pt electrodes, was accomplished by employing a Langmuir-
Blodgett based nanospherical patterning technique combined with MEMS processing
methods. A factor of 1.7-1.8 enhancement in the surface area was obtained. The 3-D
MEAs were tested with the H2/air couple in the temperature range of 350-450oC, and
achieved a power density of 186mW/cm2 at 450
oC. This constitutes the best performance
reported in the literatures for BYZ-based protonic fuel cells in this intermediate
temperature regime. Though this thin film fuel cells show outstanding fuel cell
performance, the mechanical stability of such a thin film structure could be a challenge.
To resolve the issue, on-chip fabrication method is under development in our laboratory.
6.5 References
[1] H. Huang, M. Nakamura, P. Su, R. Fasching, Y. Saito, F. B. Prinz, J. Electrochem.
Soc., 154, B20 (2007)
[2] P. C. Su, C. C. Chao, J. H. Shim, R. Fasching, F. B. Prinz, Nano Lett., 8, 2289-2292
(2008)
140
[3] Y. Jiang, A. V. Virkar, J. Electrochem. Soc., 150(7), A942 (2003)
[4] S. DeSouza, S. J. Visco, L. C. DeJonghe, Solid State Ionics, 98, 57 (1997)
[5] E. D. Wachsman, ECS Trans., 25(2), 783 (2009)
[6] A. Evans, A. Bieberle-Hütter, J. Rupp, L. J. Gauckler, J. Power Sources, 194, 119-
129 (2009)
[7] K. D. Kreuer, Ann. Rev. Mat. Res., 33, 333 (2003)
[8] W. Münch, G. Seifert, K. D. Kreuer, J. Maier, Solid State Ionics, 97, 39-44 (1997)
[9] W. Münch, K. D. Kreuer, S. Adams, G. Seifert, J. Maier, Phase Transitions, 68, 567-
586 (1999)
[10] R. C. T. Slade, N. Singh, Solid State Ionics, Diffusion & Reactions, 46, 111-15
(1991)
[11] N. Bonanos, B. Ellis, M. N. Mahmood, Solid State Ionics, 44, 305-11 (1991)
[12] N. Kuwata, N. Sata, T. Tsurui, H. Yugami, Jpn. J. App. Phys., 44, 8613-8618
(2005)
[13] T. Hibino, A. Hashimoto, M. Suzuki, M. Sano, J. Electrochem. Soc., 149, A1503-8
(2002)
[14] H. Iwahara, H. Uchida, K. Morimoto, J. Electrochem. Soc., 137, 462-465 (1990)
[15] H. Iwahara, H. Uchida, K. Ono, K. Ogaki, J. Electrochem. Soc., 135, 529-533
(1988)
[16] H. Iwahara, T. Yajima, T. Hibino, K. Ozaki, H. Suzuki, Solid State Ionics, 61, 1-3
(1993)
[17] N. Ito, M. Iijima, M. Kimura, S. Iguchi, J. Power Source, 152, 200 (2005)
141
[18] U. Balachandran, T. H. Lee, B. Ma, S. E. Dorris, Mater. Res. Soc. Symp. Proc., 972,
AA01-09 (2007)
[19] J. H. Shim, J. S. Park, J. An, T. M. Gür, S. Kang, F. B. Prinz, Chem. Mater., 21,
3290-3296 (2009)
[20] H. Uchida, S. Tanaka, H. Iwahara, J. Appl. Electrochem., 15, 93 (1985)
[21] H. Yamaura, T. Ikuta, H. Yahiro, G. Okada, Solid State Ionics, 176, 269 (2005)
[22] H. Yahiro, H. Yamaura, M. Asamoto, Mater. Res. Soc. Symp. Proc., 972, AA01-06
(2007)
[23] C. Peng, J. Melnik, J. Li, J. Luo, A. R. Sanger, K. T. Chuang, J. Power Sources, 190,
447 (2009)
[24] A. D’Epifanio, E. Fabbri, E. Di Bartolomeo, S. Licoccia, E. Traversa, Fuel Cells,
08(1), 69 (2008)
[25] D. Pergolesi, E. Fabbri, E. Traversa, abstract submitted to the 218th
Meeting of The
Electrochemical Society, Las Vegas, October 10-15 (2010)
[26] W. Sun, L. Yan, Z. Shi, Z. Zhu, W. Liu, J. Power Sources, 195, 4727 (2010)
[27] N. Bonanos, Solid State Ionics, 53-56, 967 (1992)
142
CHAPTER 7. Effect of Crystallinity on Proton Conductivity in
Yttrium-doped Barium Zirconate Thin Films
In previous chapter, we demonstrated a novel fabrication process to create 3-D proton
conducting ceramic fuel cell architecture by employing nanosphere lithography technique
(NSL). Despite BYZ’s higher proton conductivity than the oxide ion conducting
electrolytes at LT-SOFC regime, the fuel cell performance was lower compared to the
fuel cell performance conducted previously in our laboratory using YSZ electrolyte. Even
though the bulk ionic conductivity of BYZ is very high, it is known that the total
conductivity is quite low due to the extremely high grain boundary resistance. In this
chapter, we investigated the effect of crystallinity on proton conductivity in BYZ thin
films grown 120nm in thickness on amorphous (quartz) and single crystal MgO(100)
substrates has been studied. The conductivity was measured in the temperature range of
150~350oC. By altering the film deposition temperature, varying degrees of
crystallization and microstructure were observed by x-ray diffraction and transmission
electron microscopy. The epitaxial BYZ film grown on MgO(100) substrate at 900oC
showed the highest proton conductivity among other samples with an activation energy of
0.45eV, whereas polycrystalline and amorphous BYZ films showed lower conductivities
due to grain boundaries in their granular microstructure.
143
7.1 Introduction
Due to their high proton conductivity [1-12], doped perovskite oxides have been widely
studied in recent years as proton conducting solid electrolytes for a variety of
electrochemical devices such as fuel cells, hydrogen sensors, electrolyzer, and hydrogen
pumps. Best known and intensively investigated examples of such anhydrous perovskites
are alkaline-earth cerates and zirconates. Despite high proton conductivity of barium
cerate based materials [13-15], their chemical susceptibility to reactions with acid gases
(e.g., CO2, SO2) and moisture makes them unsuitable electrolytes for most fuel cell
applications [16-18]. However, Y-doped BaZrO3 (BYZ) has been considered one of the
most promising electrolyte materials for protonic fuel cells for its significant proton
conductivity as well as excellent chemical stability [10].
In general, doped perovskites have oxygen vacancies that can absorb water molecules
which give rise to protonic defects via the reaction,
H2OVO OO
X 2(OH)O (7.1)
where,
VO denotes an oxygen vacancy in the oxygen sublattice in BYZ,
OOX represents
neutral oxygen in its normal lattice site in BYZ, and
(OH )O is the protonic defect
associated with a lattice oxygen in BYZ. Principal proton transport mechanism in doped
144
perovskites is generally described as a two-step Grotthuss-type diffusion mechanism
[19], which consists of fast rotational diffusion of the protonic defect followed by proton
transfer to the neighboring oxide ions, the latter most likely being the rate-limiting step
[1, 2, 20-21]. At the low-to-intermediate temperature regime, bulk ionic conductivity in
BYZ is higher than that of oxide ion conducting ceramics. However, most fuel cell
performance values reported for proton conducting fuel cells with BYZ is much lower
than the performance with oxide ion conducting ceramics such as YSZ. We speculate that
this can be due not only to the presence of high density of grain boundaries but also to the
degree of crystallinity and evolution of the crystal structure in BYZ. In this regard,
deviations from the cubic perovskite structure may impact the formation and mobility of
protonic charge carriers. The mobility of protonic defects in perovskites with structures
deviating from its parent cubic is significantly lower [22] and this effect has been
investigated by researchers in detail comparing structural and dynamical features of
protonic defects in Y:BaCeO3 and Y:SrCeO3 [3]. Also for doped BaZrO3, it is generally
agreed that structural distortions and grain separation lead to decreased proton mobility
and result in a large grain boundary resistance [2, 23-24]. Kreuer [2] describes grain
separation as highly distorted BYZ grains making reduced number of point contacts and
separated by a grain boundary region that exhibit high impedance. Particularly, the highly
refractory nature of barium zirconate compounds usually results in small grains and
consequently a high grain boundary density with considerable impedance for proton
transport [25]. As a result, the overall conductivity is significantly reduced [2, 13, 26-27].
Therefore, it is important to optimize the fabrication process and the resulting properties
145
in terms of structure, microstructure and density of grain boundaries in order to achieve
high performance in fuel cell and other protonic device applications.
In this work, we studied the effect of crystallinity on proton conductivity in BYZ using a
two-prong strategy. For one, the degree of crystallinity was varied between amorphous to
a fully crystalline structure. The second strategy involved the comparison between single
crystalline (epitaxial) BYZ and polycrystalline BYZ structures. To serve these purposes,
we have systematically fabricated BYZ films with varying degrees of structure and
microstructure formation and investigated proton conductivity in relation to structural
features. For these experiments, we chose two different substrates, namely, MgO(100)
and quartz. MgO is ideally suited for epitaxial growth of thin BYZ films, because it has a
cubic rock-salt structure with the lattice constant of 4.21Å that matches BYZ (4.19Å )
perfectly well. Amorphous quartz substrate is used for fabricating amorphous nano-
granular BYZ films to study evolution and formation of the crystalline films deposited at
different temperatures.
7.2 Experimental
BYZ deposition is carried out by utilizing the pulsed laser deposition (PLD) technique. A
sintered BaZr0.8Y0.2O3-δ pellet (Praxair Inc.) was used as a target material to deposit the
ultra thin BYZ films. A Lambda Physik 248nm KrF excimer laser with the energy
146
density of 1.8J/cm2 per pulse was used to ablate the target in 100mTorr background
oxygen gas environment in the deposition chamber and the sample-to-target distance was
maintained at 65mm during depositions. The deposition temperature, measured by a
thermocouple placed in the center of the substrate heater, was varied from 400oC to
900oC for quartz substrates and 600
oC to 900
oC for MgO(100) substrates. After
deposition, samples were naturally cooled down in the oxygen environment with the
camber pressure of 300Torr. The thickness of the BYZ films grown on quartz and
MgO(100) substrates were 130nm with a growth rate of ~0.3Å /pulse with a pulse
repetition rate of 8Hz.
Crystallinity and structural phase of the deposited films were analyzed by X-ray
diffraction (XRD) method for both quartz and MgO(100) samples using a PANalytical
X’Pert PRO XRD system (Cu Kα X-ray with λ=1.54Å ) utilizing the symmetrical θ/2θ
scan method for phase analysis. X’Pert HighScore Plus software (PANalytical) was used
to estimate the degree of crystallization. To confirm epitaxial growth and poly
crystallinity, cross-section image and electron diffraction patterns of the BYZ-MgO
specimens were obtained using transmission electron microscopy (TEM). Specimens
with a thickness of ~80 nm were made for TEM analysis using a focused ion beam (FIB,
FEI Strata 235DB dual-beam FIB/SEM) lift-out Omniprobe technique with a Ga ion
beam at 30keV. Cross-sectional high resolution transmission electron microscopy
(HRTEM) images and selected area diffraction (SAD) patterns were taken by an FEI
Tecnai G2 F20 X-TWIN operated at an accelerating voltage of 200 kV.
147
Figure 7-1. Conductivity measurement setup with microcontacting probes connected to
the EIS software.
For conductivity measurements, a planar cell geometry shown in Figure 7-1 was
employed. Platinum pads (600µm x 600µm) with a thickness of about 100nm were
deposited on the BYZ films in a planar fashion utilizing DC sputtering technique. The
cells are mounted on a temperature controlled heating station. AC impedance
spectroscopy data were obtained in ambient air (RH=30%) by using a home-made
mircomanipulating probe set-up. AC impedance measurements were made over a
frequency range from 100 kHz to 1Hz with signal amplitude of 100mV at temperatures
from 150 to 350oC for BYZ/MgO(100) samples. Impedance measurements were done in
at open circuit condition (0mV bias) or under 500mV dc bias. It is known that in this
temperature regime proton conduction in BYZ is dominant [25]. A Gamry Potentionstat
148
(Gamry Instruments, Inc) unit and ZView software (Scribner Associate, Inc) were used
for collecting and analyzing electrochemical impedance spectroscopy (EIS) data.
7.3 Results and Discussion
Figure 7-2. XRD patterns of BYZ thin films grown on quartz substrates (Q) with
different deposition temperatures (a) 900oC, (b) 700
oC, and (c) 400
oC.
XRD analysis indicated increase in the extent of crystallization of the BYZ film as the
deposition temperature is increased, irrespective of the substrate. Figure 7-2 shows the
XRD patterns of BYZ thin films deposited on amorphous quartz substrates with different
149
deposition temperatures. The BYZ film deposited at 400oC (Figure 7-2(c)) shows no
discernable peaks which indicates that the film has amorphous or nano-granular structure.
As the deposition temperature is increased, it shows crystallization and the formation of a
polycrystalline film (Figure 7-2(b) and 7-2(a)).
Figure 7-3. XRD patterns of BYZ thin films grown on MgO(100) substrates with
different deposition temperatures (a) 900oC, (b) 800
oC, (c) 700
oC, and (d) 600
oC.
Diffraction patterns of BYZ films grown on MgO(100) are shown in Figure 7-3. As
previously mentioned, the deposition temperature was varied from 600oC to 900
oC. At
the low temperature regime (600oC), the XRD pattern shows the evolution of a
polycrystalline structure rather than epitaxial. As the temperature is increased from 600oC
to 700oC, it shows the formation of a polycrystalline film (Figure 7-3(d) and 7-3(c)). We
150
speculate that initially it follows the guiding structure, which is (100), but as the film gets
thicker it relaxes and starts to form grains with different orientations. At 800oC the BYZ
film seems to have less crystalline peaks and at 900oC, only a strong BYZ(100) peak,
which indicates perfect epitaxy of BYZ, was observed (Figure 7-3(b) and 7-3(a),
respectively). Previously, epitaxial growth of BYZ film on MgO(100) was demonstrated
at around 800oC by Shim et al. [28]. The polycrystallinity as well as epitaxial growth of
BYZ thin films on MgO(100) substrates observed by XRD were further corroborated
with TEM cross-sectional images and diffraction patterns (Figure 7-4, 7-5, and 7-6).
151
Figure 7-4. High resolution TEM image: {001} planes of BYZ (perovskite structure)
grows epitaxially on {001} type planes of MgO (rocksalt structure). A yellow-dotted
rectangle shows dimensional matching of each MgO and BYZ unit cell.
152
Figure 7-5. Selected area diffraction (SAD) patterns of BYZ films deposited by PLD at
900 °C (a series at top) and at 600 °C (b series at bottom): Both a-1 and b-1 SAD patterns
were taken only from MgO for setting orientation standard. Both a-2 and b-2 SAD
patterns were taken from MgO and BYZ to check orientation relationship of BYZ films
to MgO substrate. BYZ film deposited by PLD at 900 °C (a-2) shows epitaxial growth,
unlike BYZ film deposited by PLD at 600 °C, which illustrates slight disorientation. A
digitally 4X magnified SAD of 200 type spots (b-3) confirms orientation mismatch of
each film.
153
Epitaxial growth of BYZ film deposited at 900 °C on MgO (100) substrate is clearly
visible in the high resolution TEM cross sectional image in Figure 7-4. The yellow-dotted
region in Figure 7-4 indicates a unit cell matching that of perovskite (BYZ) and rocksalt
(MgO) structures and clearly shows the lattice match between the BYZ film and the MgO
substrate. Figure 7-5 shows the SAD patterns of epitaxial and polycrystalline BYZ films
on MgO(100) using a 150 nm diameter aperture. The SAD patterns in Figure 7-5a-2
again corroborate the epitaxial growth based on that perovskite (001) type spots of BYZ
and they are completely matched to rocksalt (001) spots.
Unlike the epitaxial BYZ film deposited at 900°C on MgO(100) substrate, the BYZ film
deposited at 600°C on MgO(100) shows misorientation. As seen in Figure 7-5b-2, (110)-
related diffraction spots that can only be generated from the BYZ film shows an angle
divergence, which indicates lattice misorientation and polycrystallinity. Digitally 4X
magnified SAD pattern for (200) spots in the blue box region in Figure 7-5b-2, which
includes both MgO and BYZ diffraction spots, points out polycrystallinity of the BYZ
film with the BYZ {200} planes slightly misoriented from {200} planes of the MgO
substrate. However, because diffraction spots of same type planes of BYZ and MgO still
show very similar position (distance from center beam to diffraction spots), similarity of
lattice parameter of BYZ film and MgO substrate can be inferred.
154
20 nm20 nm 20 nm20 nm
BYZBYZ
a) Bright Field TEMa) Bright Field TEM b) Dark Field TEMb) Dark Field TEM
BYZBYZ
Grain boundaries
c) High Resolution TEMc) High Resolution TEM d) SAD (from BYZ)d) SAD (from BYZ)
Random orientation of grainsRandom orientation of grains2 nm2 nm
Figure 7-6. Bright Field (BF), Dark Field (DF), High Resolution (HR) TEM images and
SAD pattern of BYZ films deposited by PLD at 600 °C on Quartz: Both BF (a) and DF
(b) images show visual orientation difference of each BYZ grain. HRTEM (c) shows
polycrystallinity of BYZ films with grains and grain boundaries. And SAD pattern only
taken from BYZ indicates randomly-oriented of polycrystalline BYZ grains.
155
Figure 7-6 shows TEM cross-section images and SAD of BYZ thin film deposited on
amorphous quartz substrate at 600oC. Bright Field TEM (imaged only from centered
diffraction beam) and Dark Field TEM (imaged only from specific outer diffraction
beam) in Figure 7-6-a and b are showing direct visual of polycrystallinity of BYZ film.
The contrast difference in BFTEM and DFTEM stems from orientation difference of each
grain if other conditions like materials composition or thickness are reasonably same over
the imaging area. HRTEM image directly shows grain boundaries and orientation
difference of each columnar grain with lattice fringe. SAD pattern analysis also verifies
random orientation of those grains.
For most samples, the impedance spectra showed a single semicircle where the real-axis
intercept corresponds to the total ionic resistance of the electrolyte (Figure 7-7). The
spectrum was fitted to a parallel R//C circuit, where R denotes the ohmic resistance
obtained from the EIS spectra, and C is capacitance. In addition, we varied the dc bias
applied to the samples during ac impedance spectroscopy measurements. While the
electrode processes are highly affected by the magnitude of dc bias, the ionic transport
process across the grain boundary and within the bulk grain (or, intra-grain) is generally
independent of dc bias conditions. Previously, using applied dc biases up to 14V Guo et
al [29] reported voltage dependence of grain boundary impedance in oxide ion
conducting yttria-stabilized ceria (YDC) solid electrolyte. Unfortunately, they did not
156
provide independent evidence or experimental verification (e.g., using YDC samples with
different grain sizes leading to different grain boundary densities and impedances) that
their assignment of the grain boundary impedance to the second semicircle in their
impedance spectra (of Figure 2 of Guo et al [ref. 29]) was indeed correct and justified.
Assuming their analysis is correct nevertheless, their results indicate that bias dependence
of grain boundary impedance becomes discernable only at high bias values greater than
2-3V, whereas at 0V and 0.3V biases, their impedance spectra (in Figure 2 of ref. 29) did
not show evidence of bias dependence. This is also indicated in Figure 3 of ref. 29, where
at low biases over single boundaries dependence on voltage is quite weak, and perhaps
difficult to discern experimentally.
157
Figure 7-7. Measured Nyquist impedance plots and fitting curves to the parallel R//C
circuit model. (a) BYZ-MgO(100) sample deposited at 900oC and measured at 200
oC.
Bias independence of the spectra indicates that the semicircle is associated with
electrolyte impedance. (b) BYZ film deposited on quartz at 400oC and measured at
700oC.
158
This was indeed the case in the present study where no discernable changes are observed
in Figure 7-7(a) between 0mV and 500mV bias conditions and the equivalent fitting
curves are well matched. This was observed for both samples at all measured temperature
ranges (see Figure 7-8). This confirmed and verified that the measured EIS semicircle is
not from electrode but from electrolyte processes.
Figure 7-8. EIS data measured at different temperatures for BYZ-MgO(100) film
deposited at 900oC.
The total conductivity values were extracted from the measured electrolyte impedances at
different temperatures. However, this total conductivity value includes two contributions,
namely, intra-grain and grain boundary resistances. The latter contribution in
polycrystalline BYZ is known to be high [2, 23-24]. Indeed, the impedance values for the
epitaxially grown BYZ films are significantly smaller than those for polycrystalline
159
samples, as expected. Furthermore, the capacitance values estimated from the peak
frequency and the width of the real axis intercept is of the order of 10pF (~ 4–5pF in
Figure 7-8), a typical value for geometric capacitance.
Figure 7-9. Arrhenius plot showing the conductivity values of BYZ thin films deposited
on MgO(100) and amorphous quartz substrates at different deposition temperatures. In
addition, both sets of data are compared with the reference conductivity values from the
literature, including bulk and experimentally obtained non-epi references.
By using total conductivity values and the general Arrhenius relation, we obtained
activation energies for ionic conduction in each BYZ sample:
160
kT
ET aexp0 (7.2)
where Ea is the activation energy, k is the Boltzmann constant, T is the absolute
temperature, and σ0 is a pre-exponential constant. The Arrhenius plot of Figure 7-9 shows
the total conductivity data of thin BYZ films deposited on two types of substrates at
different temperatures. From the plot, the activation energies for the BYZ films deposited
on MgO(100) sample were calculated as 0.45eV for 800oC and 900
oC deposited films, in
good agreement with the reference value of 0.44eV [2, 28, 30] for bulk proton transport,
but showed slightly higher values (0.51-0.53eV) for films deposited at lower
temperatures of 600oC and 700
oC. In a similar study, Traversa and coworkers recently
reported an activation energy of 0.63eV for proton transport in 1m thick BYZ epitaxial
films also grown by PLD at 600oC on MgO(100) substrate [31]. The authors explained
this relatively high activation energy by sample-to-sample differences both in the
structure and protonation of the films.
Interestingly, there is significant enhancement in conductivity with the evolution and
formation of the crystalline structure. As illustrated in Figure 7-3, increasing the PLD
deposition temperature made it possible to move from a polycrystalline microstructure at
lower temperatures to a single crystalline epitaxial BYZ layer at 900oC. This implies
decreasing grain boundary density due to growing grain size as the deposition
temperature is increased, where finally the epitaxial film forms the single crystalline
161
structure. Therefore, the measured conductivity values at 900oC are indeed the same as
intra-grain reference values. This again verifies the hypothesis that grain separation and
grain boundaries in doped BaZrO3 films significantly impede ionic transport resulting in
high ionic resistance.
Hindrance to proton transport across BYZ grain boundaries is expected to result in a
higher activation energy than intra-grain transport. Indeed, the activation energy for the
grain boundary transport in BYZ is reported to be 0.71eV [25]. To explain the
significantly lower activation energies ranging from 0.45eV to 0.53eV depending the on
film deposition temperature, we speculate that even the polycrystalline films may possess
an epitaxial BYZ interlayer at the BYZ/MgO interface driven by the guiding MgO
structure. Given the cell geometry employed for conductivity measurements (see Figure
7-1), we hypothesize that this epitaxial interlayer may provide an alternative transport
pathway connected in parallel arrangement with the highly resistive pathway through
grain boundaries of the polycrystalline microstructure at the external surface region of the
BYZ film.
162
Fig 7-10. Variations in the SAD patterns obtained from a cross-section sample of MgO
(100)/BYZ film (deposited by PLD at 700°C) as the SAD aperture position is moved
from MgO into the BYZ film: SAD aperture positioned on MgO only (a), 20nm into
BYZ from MgO interface (b), 40nm into BYZ from MgO interface (c), and 100nm across
the entire BYZ (d). Digitally 4X magnified SAD patterns of 101 spots from Figure 7-10-
b, c & d are shown in Figure 7-10-e, and indicate how the epitaxy in the BYZ film near
the MgO substrate gradually changes to increasing polycrystallinity with wider
divergence in orientation as the aperture moves towards upper regions of the BYZ film.
The ranges selected for SAD patterns are indicated on the cross-sectional bright field
TEM image of Figure 7-10-f using a color scheme (white for a, blue for b, green for c,
and orange for d).
163
In order to test and verify this hypothesis, we have employed SAD analysis using TEM.
Figure 7-10 shows the cross-sectional image and corresponding SAD patterns of the BYZ
film deposited at 700oC on MgO(100). When the SAD aperture, which defines the
specific area for diffraction, is gradually moved from the MgO substrate through the
thickness of the BYZ film, the diffraction spots in Figure 7-10-b, 7-10-c & 7-10-d clearly
show increasing misalignment in the BYZ film deviating from the perfectly aligned
epitaxial diffraction array. As the figure shows, under the deposition condition BYZ
grows epitaxially up to ~20nm. Beyond that thickness, it seems like second nucleation
due to misorientation starts and forms hetero epitaxial BYZ layer. Especially the SAD
pattern of Figure 7-10-d, which was taken from the upper region of BYZ indicated in
Figure 7-10-f, clearly shows more randomly oriented diffraction spots. This trend is
confirmed in Figure 7-10-e, which shows a monotonic increase in the divergence angle in
digitally magnified 101 spots as larger fractions of the BYZ film microstructure are
utilized for SAD analysis.
Clearly, SAD analysis confirms that the epitaxial nature of the BYZ film immediately
next to the MgO surface changes gradually to a polycrystalline microstructure away from
this interface, as evidenced by increasingly misaligned orientation as the BYZ thickness
is traversed. These results verify the validity of our initial hypothesis that the epitaxial
BYZ interlayer shown in Figure 7-10-f most likely provides an alternative and parallel
transport pathway for proton transport that results in an activation energy of 0.51-0.53eV,
164
which is similar to that of epitaxial BYZ film, but slightly higher possibly due to
polycrystalline nature of the upper region of the BYZ film. However, it was not possible
to discern and estimate the individual or relative contributions to proton transport from
these two structurally different BYZ regions. The polycrystalline outlaying region of the
BYZ films that were deposited at lower temperatures naturally presents cross grain
boundaries to proton transport, thus significantly lowering the conductivity values while
only slightly increasing the activation energy. We believe the proposed parallel pathway
for proton transport in these thin BYZ films helps explain the low proton conductivity
values concurrent with activation energy comparable to that for single crystal BYZ.
In case of BYZ films grown on quartz substrates, a similar but a more gradual trend was
observed as shown in Figure 7-11. Although there is some inherent error in extracting
accurate values for degree of crystallinity from the XRD data, the figure nevertheless
indicates semi quantitatively that proton conductivity increases monotonically as the
BYZ film forms an increasingly more crystalline structure (see Figure 7-2 also). As
expected, the conductivity values for the amorphous and polycrystalline BYZ films
grown on amorphous quartz substrates are about four orders of magnitude lower than the
bulk values. Also, the activation energy is about 1.12eV, which is close to the reference
value of non-epitaxially grown BYZ [2]. We speculate that this high ionic resistance is
due to the formation of nano size grains and significant grain separation in films grown
on amorphous structures, which fail to provide a guiding structure for crystal habit
formation of the deposited film [2]. Nevertheless, both Figures 7-9 and 7-11 clearly
165
indicate an enhancement in conductivity with the formation of the BYZ crystalline
structure.
Figure 7-11. Plot showing the conductivity versus degree of crystallinity of BYZ-quartz
samples with three different deposition temperatures. Error bars are included for one
measured temperature data since all three samples have the same error bars. The plot
indicates that as the deposition temperature increases the degree of crystallinity and the
conductivity increases.
7.4 Conclusion
In summary, the relation between the evolution and formation of crystalline structure and
the resulting ionic conductivity in ultra thin epitaxial and polycrystalline BYZ films was
investigated. BYZ films were grown by PLD on MgO(100) and quartz substrates at
166
different deposition temperatures. XRD patterns showed that different deposition
temperatures lead to structures ranging from amorphous to polycrystalline to epitaxial
single crystal PLD BYZ films. TEM cross-section images and SAD patterns confirmed
epitaxial BYZ films deposited on MgO(100) substrate at 900oC. At lower deposition
temperatures, SAD analysis confirmed the formation of a BYZ epitaxial interlayer at the
interface due to the guiding structure of the MgO substrate, which gradually changes into
a polycrystalline microstructure towards the top surface. Experimentally obtained
conductivity values and the extracted activation energies were in good agreement with
reference values from the literature for both bulk and non-epitaxial BYZ films. The
results showed a clear trend of higher conductivity with increased crystallinity and less
grain boundary and grain separation. Therefore, the obtained results provide design
implications when using BYZ as an electrolyte material for ceramic fuel cell. It would be
beneficial to fabricate larger grain size or less grain boundary density electrolyte to
enhance the proton conductivity thorough the membrane.
7.5 References
[1] W. Münch, G. Seifert, K. D. Kreuer, J. Maier, Solid State Ionics, 97, 39-44 (1997)
[2] K. D. Kreuer, Ann. Rev. Mat. Res., 33, 333-359 (2003)
[3] W. Münch, K. D. Kreuer, S. Adams, G. Seifert, J. Maier, Phase Transitions, 68,
567-586 (1998)
167
[4] R. C. T. Slade, N. Singh, Solid State Ionics, Diffusion & Reactions, 46, 111-15 (1991)
[5] N. Bonanos, B. Ellis, M. N. Mahmood, Solid State Ionics, 44, 305-11 (1991)
[6] N. Kuwata, N. Sata, T. Tsurui, H. Yugami, Jpn. J. Appl. Phys., 44, 8613-8618 (2005)
[7] T. Hibino, A. Hashimoto, M. Suzuki, M. Sano, J. Electrochem. Soc., 149, A1503-8
(2002)
[8] H. Iwahara, H. Uchida, K. Morimoto, J. Electrochem. Soc., 137, 462-465 (1990)
[9] H. Iwahara, H. Uchida, K. Ono, K. Ogaki, J. Electrochem. Soc., 135, 529-533 (1988)
[10] H. Iwahara, T. Yajima, T. Hibino, K. Ozaki, H. Suzuki, Solid State Ionics, 61, 1-3
(1993)
[11] N. Ito, M. Iijima, K. Kimura, S. Iguchi, J. Power Sources, 152, 200 (2005)
[12] U. Balachandran, T. H. Lee, B. Ma, S. E. Dorris, Mater. Res. Soc. Symp. Proc., 972,
AA01-09 (2007)
[13] K. Katahira, Y. Kohchi, T. Chimura, H. Iwahara, Solid State Ionics, 138, 91-98
(2000)
[14] G. Ma, T. Chimura, H. Iwahara, Solid State Ionics, 110, 103-110 (1998)
[15] D. Shima, S. M. Haile, Solid State Ionics, 97, 443-455 (1997)
[16] N. Zakowsky, S Williamson, S. T. S. Irvine, Solid State Ionics, 176, 3019-3026
(2005)
[17] S. V. Bhide, A. V. Virkar, J. Electrochem. Soc., 146, 2038-2044 (1999)
[18] F. Chen, O. T. Sørensen, G. Meng, D. Peng, J. Mater. Chem., 7, 481-485 (1997)
[19] B. Merinov, W. J. Goddard III, Chem. Phys., 130, 194707 (2009)
168
[20] W. Münch, G. Seifert, K. D. Kreuer, J. Maier, Solid State Ionics, 86-88, 647-652
(1996)
[21] M. Pioinke, T. Mono, W. Schweika, T. Springer, T. Schober, Solid State Ionics, 97,
497-504 (1997)
[22] K. D. Kreuer, Solid State Ionics, 125, 285-302 (1999)
[23] S. M. Haile, G. Staneff, K. H. Ryu, J. Mater. Sci., 36, 5 (2001)
[24] P. Babilo, S. M. Haile, J. Am. Ceram. Soc., 88, 9 (2005)
[25] P. Babilo, T. Uda, S. M. Haile, J. Mater. Res., 22, 5 (2007)
[26] E. Fabbri, A. D’Epifanio, E. Di Bartolomeo, S. Licoccia, E. Traversa, Solid State
Ionics, 179, 558-564 (2008)
[27] A. D’Epifanio, E. Fabbri, E. Di Bartolomeo, S. Licoccia, E. Traversa, Fuel Cells, 8,
69-76 (2008)
[28] J. H. Shim, T. M. Gür, F. B. Prinz, Appl. Phys. Lett., 92, 253115 (2008)
[29] X. Guo, S. Mi, R. Waser, Electrochem Solid State Lett., 8, J1 (2005)
[30] H. G. Bohn, T. Schober, J. Am. Ceram. Soc., 83, 4 (2000)
[31] D. Pergolesi, E. Fabbri, A. D’Epifanio, E. Di Bartolomeo, A. Tebano, S. Sanna, S.
Licoccia, G. Balestrino, and E. Traversa, Nature Mater., 9, 846 (2010)