c consult author(s) regarding copyright matters notice please ... of...some tes systems employ...
TRANSCRIPT
-
This may be the author’s version of a work that was submitted/acceptedfor publication in the following source:
Sarvghad Moghaddam, M. Sarvghad, Steinberg, Ted, & Will, Geoffrey(2018)Corrosion of stainless steel 316 in eutectic molten salts for thermal energystorage.Solar Energy, 172, pp. 198-203.
This file was downloaded from: https://eprints.qut.edu.au/119350/
c© Consult author(s) regarding copyright matters
This work is covered by copyright. Unless the document is being made available under aCreative Commons Licence, you must assume that re-use is limited to personal use andthat permission from the copyright owner must be obtained for all other uses. If the docu-ment is available under a Creative Commons License (or other specified license) then referto the Licence for details of permitted re-use. It is a condition of access that users recog-nise and abide by the legal requirements associated with these rights. If you believe thatthis work infringes copyright please provide details by email to [email protected]
Notice: Please note that this document may not be the Version of Record(i.e. published version) of the work. Author manuscript versions (as Sub-mitted for peer review or as Accepted for publication after peer review) canbe identified by an absence of publisher branding and/or typeset appear-ance. If there is any doubt, please refer to the published source.
https://doi.org/10.1016/j.solener.2018.03.053
https://eprints.qut.edu.au/view/person/Sarvghad,_Madjid.htmlhttps://eprints.qut.edu.au/view/person/Steinberg,_Ted.htmlhttps://eprints.qut.edu.au/view/person/Will,_Geoffrey.htmlhttps://eprints.qut.edu.au/119350/https://doi.org/10.1016/j.solener.2018.03.053
-
1
Corrosion of stainless steel 316 in eutectic molten salts for thermal energy storage
Madjid Sarvghad*, Theodore A. Steinberg, Geoffrey Will
Science and Engineering Faculty, Queensland University of Technology (QUT), Queensland
4001, Australia
Cite this article as:
Madjid Sarvghad, Theodore A. Steinberg and Geoffrey Will, Corrosion of stainless steel 316 in
eutectic molten salts for thermal energy storage, Solar Energy, 2018
https://doi.org/10.1016/j.solener.2018.03.053
Abstract
Stainless steel 316 was examined for compatibility with the eutectic mixtures of NaCl + Na2CO3 and
NaCl + Na2SO4 at 700 °C and Li2CO3 + K2CO3 + Na2CO3 at 450 °C in air for thermal energy storage.
Electrochemical measurements combined with advanced microscopy and microanalysis techniques
were employed. NaCl + Na2CO3 was found as the most aggressive salt at 700 °C. The attack
morphology on the surface was uniform corrosion with no localized degradation at 450 ºC. Microscopy
observations showed grain boundary oxidative attack as the primary corrosion mechanism at 700 °C
with depletion of alloying elements from grain boundaries.
Keywords
Steel alloy; Molten Salt; Corrosion; Microscopy
* Corresponding author; Email: [email protected]; [email protected]
https://doi.org/10.1016/j.solener.2018.03.053mailto:[email protected]:[email protected]
-
2
1. Introduction
Thermal Energy Storage (TES) is a critical component in Concentrated Solar thermal Power (CSP)
plants through providing dispatchability and increasing the capacity factor of the plant [1-4]. To fulfil
the recent interests in raising the working temperature of these plants, considerable improvement in
material compatibility between the containment material (tank) and storage medium is a prerequisite
[5-8]. Some TES systems employ eutectic mixtures of molten salts with high thermal capacity as Phase
Change Materials (PCM) to store the thermal energy [9-11].
Steel alloys, as economic candidates for containment materials, are subject to hot corrosion and
oxidation from the molten media in TES systems [3-7, 9-22]. Molten eutectic mixtures of carbonate,
chloride-carbonate, and chloride-sulfate salts are also considered as PCM candidates that provide high
heat capacity and energy density [3, 23]. The solubility of corrosion products and oxidation potential
of the alloy are key factors that affect compatibility between the containment material and molten
medium [24]. In steel alloys, the development of protective oxides on the material surface promotes
resistance against corrosion where the material chemistry, temperature and atmosphere determine the
scaling rate [25, 26]. However, in molten salts, protective layers consisting of components like
chromium oxide are often dissolved into the salt mixture by fluxing. Once the oxide film is removed,
the least noble constituent of the exposed metal will be attacked [24, 27, 28]. For example, the corrosion
of Fe-based alloys at 450 °C in ZnCl2–KCl was shown to be due to the separation and spallation of the
oxide films [29].
Intergranular corrosion of steel alloys in contact with molten chloride and chloride-carbonate salts has
been reported previously [28, 30]. Other studies confirm that intergranular attack in Fe-Ni-Cr alloys is
more severe than metal loss in molten chlorides [23]. Depletion of Cr from grain boundaries in molten
salts has been commonly identified as a key corrosion mechanism in various molten salts for high Cr
alloys [11, 28, 31, 32]. However, recent research showed acceptable resistance of stainless steel 310 to
molten carbonate salts at 750 °C [3]. Generally, steel alloys with around 20 wt% Cr and/or high nickel
content show a greater resistance to high-temperature corrosion [25, 33].
This study will examine the compatibility of stainless steel 316, as TES vessel, with some eutectic
mixtures of molten salts, as PCM, for the purpose of developing economic and functionally efficient
CSP systems.
2. Experimental procedure
Austenitic stainless steel 316 (SS316), supplied by M D Lewis & Company Pty. Ltd, with the nominal
chemical composition of (in wt%) 67.45% Fe, 12% Ni, 17.5% Cr, 3% Mo and 0.05% C was examined
for compatibility in three eutectic mixtures of molten salts.
Powders of sodium chloride (CAS No.7647-14-5), sodium sulfate (CAS No. 7757-82-6), sodium
carbonate (CAS No.497-19-8), potassium carbonate (CAS No.584-08-7) and lithium carbonate (CAS
No.554-13-2) were placed for 24 h in a 180 °C furnace to dry and then were measured and mixed
according to Table 1. The eutectic mixtures melting points and test temperatures have been also
provided in the table. Test temperature for each salt was selected close to its melting point assuming
the salt will be used as a PCM.
Table 1 Chemical composition, melting point and test temperature of the salt mixtures.
Eutectic salt mixture Composition
(wt%)
Melting point
(°c) [34, 35]
Test temperature
(°c)
Chloride sulfate 26.5 NaCl + 73.5 Na2SO4 626 700
Chloride carbonate 40 NaCl + 60 Na2CO3 632 700
Ternary carbonate 33.4 Na2CO3 + 32.1 Li2CO3 + 34.5 K2CO3 397 450
-
3
2.1. Electrochemical corrosion investigation
Electrochemical experiments were conducted using a three-electrode cell containing the molten salts in
alumina crucibles open to air at 700 °C and 450 °C in a preheated cylindrical furnace. Test coupons of
25 mm long, 5 mm wide and 1.4 mm thick were mechanically wet ground and polished down to 0.04
m by colloidal silica, washed with ethanol and dried in air. Measurements were implemented by means
of a VMP3-based BioLogic instrument controlled by EC-Lab® software. The three-electrode cell was
implemented with the polished sample as the working electrode and two same sized platinum sheets
(25×5×1 mm) as pseudo reference and counter electrodes [36-39]. Samples were subjected to open
circuit potential (OCP), electrochemical impedance spectroscopy (EIS) and potentiodynamic
polarization (PDP) measurements in this order to avoid sample deterioration. Equilibrations of
potentials (OCP) were carried out for 1 h immediately after immersion. EIS measurements were then
obtained using a frequency range of 100 kHz- 100 mHz with the amplitude of ± 10 mV. Finally, PDP
was conducted at the potential scan rate of 10 mV/min and potential range of -400 to +500 mV with
respect to the open circuit potential. Tafel fit tool of EC-Lab software was used to fit PDP curves and
calculate Tafel slopes, corrosion current density and corrosion potential.
2.2. Static corrosion
Fresh metal coupons were cut to around 25×7×1.4 mm for static corrosion tests while the front sides
were mechanically wet polished down to 1 µm in colloidal silica using standard grinding and polishing
procedures. Cylindrical alumina crucibles were used as salt vessels and the furnace temperature was set
to 700 ± 10 °C for chloride carbonate and chloride sulfate salts and 450 ± 10 °C for the ternary
carbonate.
The salt containing vessels were placed into the furnace at room temperature and then gradually heated
up to the test temperature. Once the salt melted and the chamber conditions stabilized, the metal coupons
were immersed and then removed after 120 h of exposure. All coupons were then mounted exposing
the right (or left) side into a conductive resin, ground and polished down to 0.04 µm from the side of
the sample in colloidal silica using standard procedures, washed with ethanol and finally dried in air. It
is worthy to note that although 120 h does not seem long enough to study the corrosion rate and related
phenomena, the aggressive nature of molten salts makes studying short-term impacts like attack
morphology and corrosion mechanisms possible.
2.3. Microstructural investigations
Optic microscope model Leica DMi8A (magnification 1.25 x-50 x) equipped with Leica Application
Suite software was used to take macro and micro-images for microstructural and corrosion observations.
Scanning electron microscopy (SEM) and energy-dispersive X-ray spectroscopy (EDS) were also
employed for further microstructural investigations using a field emission SEM; model: JEOL 7001F,
with automated feature detection equipped with secondary electron and EDS analysis system.
3. Results and discussion
3.1. Electrochemistry
OCP graphs of the alloy specimens in the studied molten salts are represented in Fig. 1a. In chloride
sulfate, SS316 shows an initial rapid drop followed by more noble OCP values after 1000 s and ending
to stable values over the 1 h of exposure. In chloride carbonate at 700 °C and ternary carbonate at 450
°C it shows more noble potential values over time. This could be attributed to the gradual development
of films on the surface.
-
4
Fig. 1 (a) Open circuit potential, and (b) potentiodynamic polarization curves of SS316 samples in chloride
sulfate and chloride carbonate at 700 °C and ternary carbonate at 450 °C.
Ecorr values in PDP plots in Fig. 1b reflect OCP values in Fig. 1a. Data extracted from PDP curves are
summarized in Table 2 depicting the corrosion current density values in Fig. 2b.
SS316 represents the least Icorr value in ternary carbonate at 450 °C. Between the two high temperature
salt mixtures at 700 °C, chloride carbonate seems the most aggressive one with a corrosion current
density value of around 3.3 times higher that of chloride sulfate. This could be attributed to the high
solubility of Cr and other alloying elements in chloride carbonate and the subsequent dissolution of
oxide films into the molten salt as reported previously [35]. The significant changes in Icorr and Ecorr
values could also indicate changes in mechanism between the molten salts because of dissimilar
compositions and test temperatures.
Table 2 Extracted data from polarization plots in Fig. 1b and EIS plots in Fig. 3b.
Salt mixture Ecorr
(mV)
Icorr
(µA.cm-²)
Βa
(mV/decade)
|Βc|
(mV/decade)
Rp
(Ω.cm2)
Chloride sulfate -466 74 288 262 113
Chloride carbonate -24 247 221 313 20
Ternary carbonate -539 6 56 143 225
Fig. 2 Column chart of corrosion current density values of SS316 in chloride carbonate and chloride sulfate
at 700 °C and ternary carbonate at 450 °C.
-
5
The corrosion mechanisms of steel alloys in the studied molten salts have been previously discussed in
detail [28, 40]. It has been shown that the corrosion mechanism in molten carbonate salts varies widely
with temperature and the salt composition while the salt becomes less corrosive at lower temperatures
[23]. Because of their ionic nature, molten salts interact electrochemically with metals leading to Redox
reactions [41-44] with corrosion highly dependent on the solubility of metal oxides in the liquid salt
[45]. Solubility of oxygen and the subsequent oxidation of metals (and alloying elements) has been
previously shown in molten carbonates [28, 32, 35, 46]. Formation of a variety of iron oxides, such as
FeO, Fe2O3 and Fe3O4, is a consequence of the interaction between molten carbonates and steel alloys
[45, 46]. However, molten chlorides have been reported to destabilize the oxide film due to the
formation of HCl and Cl2 gas that penetrate the film on the material surface and react with the substrate
metal [17, 43, 44, 47-49].
Analyses of Nyquist and Bode-Phase plots (Fig. 3) resulted from EIS measurements in the molten salts
provide more information. In agreement with Zeng et al. [50] and as confirmed in our previous research
[28, 40], the Nyquist plots confirm the formation of semi-protective films on the metal surface where
the transfer of ions in the scale is rate limiting [50, 51]. This is also in agreement with OCP plots in Fig.
1a. Bode plots in Fig. 3b show the highest impedance values (polarization resistance, Rp, in Table 2) at
low frequencies for the alloy in ternary carbonate at 450 °C versus chloride carbonate with the least
impedance and moderate values for chloride sulfate (at 700 °C); corresponding to corrosion current
density values reported in Table 2. Considering the results in Table 2, Fig. 1b and Fig. 2b, although the
deposit does not seem to be totally protective, it could have led to a slow corrosion rate for the alloy in
ternary carbonate at 450 °C compared to the other two salts at 700 °C. However, this does not disaffirm
the impact of temperature which is quite lower for the ternary carbonate than the two high temperature
salt mixtures.
Fig. 3 (a) Nyquist, and (b) Bode-Phase plots resulted from impedance measurements of SS316 samples in chloride
sulfate and chloride carbonate at 700 °C and ternary carbonate at 450 °C. Larger Nyquist plot in chloride carbonate
is also included in (a).
3.2. Static corrosion, microscopy and microanalysis
3.2.1. SS316 vs. chloride sulfate at 700 °C
SEM-EDS images of SS316 submerged for 120 h in the molten chloride sulfate at 700 ºC is presented
in Fig. 4. Grain boundary (GB) de-alloying of Cr, Fe and Mn followed by the formation of a Mo-Ni-S
oxide along GBs seems to be the corrosion mechanism. In agreement with EIS results, a very thin oxide
film is also detectable on the alloy surface. However, sulfur attack and the subsequent formation of
molybdenum sulfides have been previously reported to destabilize the oxide layer [40-42].
-
6
Consequently, dissolution of the surface film allows direct access of the molten salt to the underlying
metal leading to further oxidation and corrosion.
Fig. 4 SEM and the corresponding EDS map analysis of SS316 after 120 h exposure to chloride sulfate salt at 700
°C.
3.2.2. SS316 vs. chloride carbonate at 700 °C
A SEM image and its corresponding EDS map analysis of a coupon of SS316 subjected to chloride
carbonate at 700 °C for 120 h is shown in Fig. 5. Again, depletion of Fe and Cr from GBs seems to have
led to the formation of a semi-protective GB oxide as previously predicted by electrochemistry.
However, the high diffusivity of ions through the surface layer reduce the film adherence in the molten
salt [28].
Fig. 5 SEM and its corresponding EDS map analysis of SS316 after 120 h exposure to chloride carbonate salt
at 700 °C [28].
3.2.3. SS316 vs. ternary carbonate at 450 °C
Fig. 6 shows the formation of a continuous and adherent Fe-Ni-Cr-K oxide on the material surface in
ternary carbonate at 450 °C. No localized de-alloying and oxidation/corrosion attack is detectable on
the sample. Thus, it could be concluded that the oxide layer formed on the material surface acts as a
solid barrier against further corrosion in contact with the molten salt at 450 °C.
-
7
Fig. 6 SEM and the corresponding EDS map analysis of SS316 after 120 h exposure to ternary carbonate salt at 450 °C
[28].
Conclusion
Corrosion behavior of stainless steel 316 in the eutectic mixtures of NaCl + Na2CO3 and NaCl + Na2SO4
at 700 °C and Li2CO3 + K2CO3 + Na2CO3 at 450 °C in air was studied for compatibility in thermal
energy storage. A combination of optical microscopy, electrochemical measurements, SEM and EDS
techniques were employed to characterize the degradation mechanisms. Results are summarized as
below.
Electrochemical measurements showed the most cathodic potential value for the alloy in NaCl +
Na2CO3 at 700 °C which was found as the most aggressive salt through providing the highest corrosion
current density value. Impedance spectroscopy suggested the formation of films on the surface of the
alloy in all molten salts, which were shown not to be fully protective. Consequently, oxidation was
found as the attack mechanism to the alloy in all molten salt environments.
The corroded metal morphology was grain boundary oxidation because of de-alloying and subsequent
intergranular attack at 700 °C. However, uniform oxidative attack was observed for the alloy in contact
with Li2CO3 + K2CO3 + Na2CO3 at 450 °C with no localized de-alloying.
Acknowledgement
This work was funded by the Australian Solar Thermal Research Initiative (ASTRI), which is supported
by the Australian Government via the Australian Renewable Energy Agency (ARENA). The authors
would also like to thank AINSE Ltd for providing financial assistance (Award-PGRA-2016) to enable
work on the reported topic. The data reported in the paper were obtained at the Central Analytical
Research Facility (CARF) operated by the Institute for Future Environments at Queensland University
of Technology (QUT). Access to CARF was supported by generous funding from the Science and
Engineering Faculty, QUT.
References
[1] M. Liu, N.H. Steven Tay, S. Bell, M. Belusko, R. Jacob, G. Will, W. Saman, F. Bruno, Review on concentrating solar power plants and new developments in high temperature thermal energy storage technologies, Renewable and Sustainable Energy Reviews, 53 (2016) 1411-1432. [2] M. Liu, W. Saman, F. Bruno, Review on storage materials and thermal performance enhancement techniques for high temperature phase change thermal storage systems, Renewable and Sustainable Energy Reviews, 16 (2012) 2118-2132. [3] J.C. Gomez-Vidal, J. Noel, J. Weber, Corrosion evaluation of alloys and MCrAlX coatings in molten carbonates for thermal solar applications, Solar Energy Materials and Solar Cells, 157 (2016) 517-525.
-
8
[4] J.C. Gomez-Vidal, E. Morton, Castable cements to prevent corrosion of metals in molten salts, Solar Energy Materials and Solar Cells, 153 (2016) 44-51. [5] S. Kuravi, J. Trahan, D.Y. Goswami, M.M. Rahman, E.K. Stefanakos, Thermal energy storage technologies and systems for concentrating solar power plants, Progress in Energy and Combustion Science, 39 (2013) 285-319. [6] L.F. Cabeza, A. Gutierrez, C. Barreneche, S. Ushak, Á.G. Fernández, A. Inés Fernádez, M. Grágeda, Lithium in thermal energy storage: A state-of-the-art review, Renewable and Sustainable Energy Reviews, 42 (2015) 1106-1112. [7] M.M. Kenisarin, High-temperature phase change materials for thermal energy storage, Renewable and Sustainable Energy Reviews, 14 (2010) 955-970. [8] M. Sarvghad, S. Delkasar Maher, D. Collard, M. Tassan, G. Will, T.A. Steinberg, Materials compatibility for the next generation of Concentrated Solar Power plants, Energy Storage Materials, 14 (2018) 179-198. [9] J. Gomez, High-Temperature Phase Change Materials (PCM) Candidates for Thermal Energy Storage (TES) Applications, in, National Renewable Energy Laboratory (NREL), Golden, CO., 2011. [10] T. Bauer, N. Pfleger, D. Laing, W.-D. Steinmann, M. Eck, S. Kaesche, 20 - High-Temperature Molten Salts for Solar Power Application, in: F.L. Groult (Ed.) Molten Salts Chemistry, Elsevier, Oxford, 2013, pp. 415-438. [11] M. Sarvghad, S. Bell, R. Raud, T.A. Steinberg, G. Will, Stress assisted oxidative failure of Inconel 601 for thermal energy storage, Solar Energy Materials and Solar Cells, 159 (2017) 510-517. [12] W. Guo, Y. Wu, J. Zhang, S. Hong, L. Chen, Y. Qin, A Comparative Study of Cyclic Oxidation and Sulfates-Induced Hot Corrosion Behavior of Arc-Sprayed Ni-Cr-Ti Coatings at Moderate Temperatures, Journal of Thermal Spray Technology, 24 (2015) 789-797. [13] K. Lovegrove, W.S. Csiro, Introduction to concentrating solar power (CSP) technology, in: K. Lovegrove, W. Stein (Eds.) Concentrating Solar Power Technology, Woodhead Publishing, 2012, pp. 3-15. [14] K. Lovegrove, J. Pye, Fundamental principles of concentrating solar power (CSP) systems, in: K. Lovegrove, W. Stein (Eds.) Concentrating Solar Power Technology, Woodhead Publishing, 2012, pp. 16-67. [15] K. Federsel, J. Wortmann, M. Ladenberger, High-temperature and corrosion behavior of nitrate nitrite molten salt mixtures regarding their application in concentrating solar power plants, Enrgy Proced, 69 (2015) 618-625. [16] B.A.T. Mehrabadi, J.W. Weidner, B. Garcia-Diaz, M. Martinez-Rodriguez, L. Olson, S. Shimpalee, Multidimensional Modeling of Nickel Alloy Corrosion inside High Temperature Molten Salt Systems, Journal of The Electrochemical Society, 163 (2016) C830-C838. [17] K. Sridharan, T.R. Allen, 12 - Corrosion in Molten Salts, in: F.L. Groult (Ed.) Molten Salts Chemistry, Elsevier, Oxford, 2013, pp. 241-267. [18] L.C. Olson, Materials corrosion in molten LiF-NaF-KF eutectic salt, in, University of Wisconsin--Madison, 2009. [19] L.C. Olson, J.W. Ambrosek, K. Sridharan, M.H. Anderson, T.R. Allen, Materials corrosion in molten LiF-NaF-KF salt, Journal of Fluorine Chemistry, 130 (2009) 67-73. [20] R.B. Rebak, 7 - Stress corrosion cracking (SCC) of nickel-based alloys, in: V.S. Raja, T. Shoji (Eds.) Stress Corrosion Cracking, Woodhead Publishing, 2011, pp. 273-306. [21] R.B. Rebak, Environmentally assisted cracking of nickel alloys —a review, in: S.A.S.H.J.M.O.B. Rebak (Ed.) Environment-Induced Cracking of Materials, Elsevier, Amsterdam, 2008, pp. 435-446. [22] F.J. Ruiz-Cabañas, C. Prieto, R. Osuna, V. Madina, A.I. Fernández, L.F. Cabeza, Corrosion testing device for in-situ corrosion characterization in operational molten salts storage tanks: A516 Gr70 carbon steel performance under molten salts exposure, Solar Energy Materials and Solar Cells, 157 (2016) 383-392. [23] Molten Salt Corrosion, in: G.Y. Lai (Ed.) High-temperature corrosion and materials applications, ASM International, 2007, pp. 409–421.
-
9
[24] M.S. Sohal, M.A. Ebner, P. Sabharwall, P. Sharpe, Engineering database of liquid salt thermophysical and thermochemical properties, in, Idaho National Laboratory, Idaho Falls, 2010. [25] J. Young, Chapter 1 The Nature of High Temperature Oxidation, in: Y. David John (Ed.) Corrosion Series, Elsevier Science, 2008, pp. 1-27. [26] A.S. Khanna, Introduction to high temperature oxidation and corrosion, ASM international, 2002. [27] F. Lantelme, H. Groult, Molten salts chemistry: from lab to applications, Newnes, 2013. [28] M. Sarvghad, T.A. Steinberg, G. Will, Corrosion of steel alloys in eutectic NaCl+Na 2 CO 3 at 700 °C and Li 2 CO 3 + K 2 CO 3 + Na 2 CO 3 at 450 °C for thermal energy storage, Solar Energy Materials and Solar Cells, 170 (2017) 48-59. [29] Y.S. Li, Y. Niu, W.T. Wu, Accelerated corrosion of pure Fe, Ni, Cr and several Fe-based alloys induced by ZnCl2–KCl at 450°C in oxidizing environment, Materials Science and Engineering: A, 345 (2003) 64-71. [30] M. Groll, O. Brost, D. Heine, Corrosion of steels in contact with salt eutectics as latent heat storage materials: Influence of water and other impurities, Heat Recovery Systems and CHP, 10 (1990) 567-572. [31] J.C. Gomez-Vidal, R. Tirawat, Corrosion of alloys in a chloride molten salt (NaCl-LiCl) for solar thermal technologies, Solar Energy Materials and Solar Cells, 157 (2016) 234-244. [32] M. Sarvghad, T. Chenu, G. Will, Comparative interaction of cold-worked versus annealed inconel 601 with molten carbonate salt at 450°C, Corrosion Science, 116 (2017) 88-97. [33] A. Schütz, M. Günthner, G. Motz, O. Greißl, U. Glatzel, High temperature (salt melt) corrosion tests with ceramic-coated steel, Materials Chemistry and Physics, 159 (2015) 10-18. [34] Collection of Phase Diagrams, in, FTsalt - FACT Salt Phase Diagrams, http://www.crct.polymtl.ca/fact/documentation/FTsalt/FTsalt_Figs.htm, 2016. [35] M. Sarvghad, G. Will, T.A. Steinberg, Corrosion of Inconel 601 in molten salts for thermal energy storage, Solar Energy Materials and Solar Cells, 172 (2017) 220-229. [36] A.I. Bhatt, G.A. Snook, Reference Electrodes for Ionic Liquids and Molten Salts, in: G. Inzelt, A. Lewenstam, F. Scholz (Eds.) Handbook of Reference Electrodes, Springer Berlin Heidelberg, 2013, pp. 189-227. [37] G. Inzelt, Pseudo-reference Electrodes, in: G. Inzelt, A. Lewenstam, F. Scholz (Eds.) Handbook of Reference Electrodes, Springer Berlin Heidelberg, 2013, pp. 331-332. [38] G.Z. Chen, D.J. Fray, T.W. Farthing, Direct electrochemical reduction of titanium dioxide to titanium in molten calcium chloride, Nature, 407 (2000) 361-364. [39] T. Nohira, K. Yasuda, Y. Ito, Pinpoint and bulk electrochemical reduction of insulating silicon dioxide to silicon, Nature Materials, 2 (2003) 397-401. [40] M. Sarvghad, G. Will, T.A. Steinberg, Corrosion of steel alloys in molten NaCl + Na 2 SO 4 at 700 °C for thermal energy storage, Solar Energy Materials and Solar Cells, 179 (2018) 207-216. [41] R.V. Carter, D.L. Douglass, F. Gesmundo, Kinetics and mechanism of the sulfidation of Fe-Mo alloys, Oxidation of Metals, 31 (1989) 341-367. [42] J. Young, Chapter 8 Corrosion by Sulfur, in: Y. David John (Ed.) Corrosion Series, Elsevier Science, 2008, pp. 361-396. [43] S.N. Liu, Z.D. Liu, Y.T. Wang, J. Tang, A comparative study on the high temperature corrosion of TP347H stainless steel, C22 alloy and laser-cladding C22 coating in molten chloride salts, Corrosion Science, 83 (2014) 396-408. [44] A. Nishikata, H. Numata, T. Tsuru, Electrochemistry of Molten-Salt Corrosion, Mat Sci Eng a-Struct, 146 (1991) 15-31. [45] T. Tzvetkoff, A. Girginov, M. Bojinov, Corrosion of nickel, iron, cobalt and their alloys in molten salt electrolytes, Journal of Materials Science, 30 (1995) 5561-5575. [46] M. Azzi, J.J. Rameau, Corrosion in molten Na2CO3-K2CO3 at 800° C—I. Effect of oxygen partial pressure on iron corrosion, Corrosion Science, 24 (1984) 935-944. [47] A.M. Kruizenga, Corrosion mechanisms in chloride and carbonate salts, in: Sandia National Laboratories, Livermore, CA Report No. SAND2012-7594, 2012.
http://www.crct.polymtl.ca/fact/documentation/FTsalt/FTsalt_Figs.htm
-
10
[48] H.J. Grabke, E. Reese, M. Spiegel, The effects of chlorides, hydrogen chloride, and sulfur dioxide in the oxidation of steels below deposits, Corrosion Science, 37 (1995) 1023-1043. [49] J.M. Abels, H.H. Strehblow, A surface analytical approach to the high temperature chlorination behaviour of Inconel 600 at 700 °C, Corrosion Science, 39 (1997) 115-132. [50] C.L. Zeng, W. Wang, W.T. Wu, Electrochemical impedance models for molten salt corrosion, Corrosion Science, 43 (2001) 787-801. [51] X.X. Sheng, Y.P. Ting, S.A. Pehkonen, The influence of sulphate-reducing bacteria biofilm on the corrosion of stainless steel AISI 316, Corrosion Science, 49 (2007) 2159-2176.
Table of figures
Fig. 1 (a) Open circuit potential, and (b) potentiodynamic polarization curves of SS316 samples in
chloride sulfate and chloride carbonate at 700 °C and ternary carbonate at 450 °C. Fig. 2 Column chart of corrosion current density values of SS316 in chloride carbonate and chloride
sulfate at 700 °C and ternary carbonate at 450 °C. Fig. 3 (a) Nyquist, and (b) Bode-Phase plots resulted from impedance measurements of SS316
samples in chloride sulfate and chloride carbonate at 700 °C and ternary carbonate at 450 °C. Larger
Nyquist plot in chloride carbonate is also included in (a). Fig. 4 SEM and the corresponding EDS map analysis of SS316 after 120 h exposure to chloride
sulfate salt at 700 °C. Fig. 5 SEM and its corresponding EDS map analysis of SS316 after 120 h exposure to chloride
carbonate salt at 700 °C [28]. Fig. 6 SEM and the corresponding EDS map analysis of SS316 after 120 h exposure to ternary
carbonate salt at 450 °C [28].