organoamines-grafted on nano-sized silica for carbon dioxide capture
TRANSCRIPT
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Organoamines-grafted on nano-sized silica for carbon dioxide capture
Miklos Czaun, Alain Goeppert, Robert B. May, Drew Peltier, Hang Zhang, G.K. Surya Prakash *,George A. Olah *
Loker Hydrocarbon Research Institute and Department of Chemistry, University of Southern California, University Park Campus, Los Angeles, CA 90089-1661, USA
1. Introduction
The ever increasing consumption of fossil fuels by humankind
has resulted in a rapid increase of carbon dioxide concentration in
the atmosphere from 270 ppm at the dawn of the industrial
revolution to the present 395 ppm. It is generally accepted that this
higher atmospheric carbon dioxide concentration is one of the
major contributors to global warming. However, global warming is
not the only effect of the increasing anthropogenic emission of CO2.
The oceans of our planet are net sinks of CO2 but their absorption
capacity is also finite. Furthermore, the dissolution of CO2 in the
oceans lowers the pH of seawater resulting in a reduction in the
abundance and/or size of shellfish, corals and crustaceans [1]. In
order to avoid further increase in CO2 concentration, the
management of this greenhouse gas has to gain more attention
and we believe that the reduction of anthropogenic CO2 emission
should be among the highest priorities of this century. Various
sequestration techniques that have been suggested may provideonly a temporary answer to our CO2 management problem. For
example pumping CO2 to deep aquifers, coal bed, depleted oil or
natural gas fields are promising solutions [2,3] but these methods
need to be validated on a large scale to ensure the long term safe
storage of CO2. As an alternative to sequestration, the capture,
recycling and utilization of CO2 promises an ultimate solution. An
elegant way to recycle CO2, for example, is to use it in reforming
reactions such as dry reforming or bi-reforming to produce syngas,
a mixture of carbon monoxide and hydrogen [4]. Presently,
approximately 130 million tonnes per year [5] of CO2 are used in
the energy and chemical industries and the majority is converted
to urea. This is still a drop in the bucket considering that humanity
now emits more than 30 billion tonnes of CO2 per year.
Fortunately, there are an increasing number of scientific projects
[5–7] that consider CO2 as a valuable industrial feedstock rather
than just a greenhouse gas harmful for the Planet’s ecosystem. As a
result of the predicted improvements, the amount of CO2 utilized
in the industry may grow to 300 million tonnes per year [8] in the
short term and higher in the following decades.
The most widely used post-combustion capture technologies
are based on the chemisorption of CO2 (Scheme 1) in aqueous
alkanolamine solutions such as monoethanolamine (MEA) [9],
diethanolamine (DEA) and methyldiethanolamine (MDEA).
The continuous regeneration of alkanolamine solutions (recov-ery of CO2) is a very energy intensive process due to high heating
and pumping costs. While for example an aqueous solution of DEA/
MDEA has a heat capacity of approximately 4.50 J gÀ1 8CÀ1
( xH2O ¼ 0:6, xDEA / xMDEA = 0.24/0.16, t = 50 8C) [10], silica based
adsorbents show significantly lower heat capacities
(0.73 J gÀ1 8CÀ1)1 making this kind of adsorbents more energeti-
cally efficient candidates for large scale CO2 capture and recycling.
Journal of CO2 Utilization 1 (2013) 1–7
A R T I C L E I N F O
Article history:
Received 2 February 2013
Received in revised form 26 March 2013Accepted 26 March 2013
Available online 24 April 2013
Keywords:
Nanosilica
Chemically grafted organoamines
Carbon dioxide capture
A B S T R A C T
Organoamine–inorganic hybrid adsorbent materials were synthesized by covalent immobilization of
alkylaminotrimethoxysilanes and polyethyleneiminetrimethoxysilane onto fumed silica (nanosilica).
The obtained silica–organic hybrid materials were characterized by thermogravimetry and diffusereflectance infrared Fourier transform spectroscopy (DRIFT) confirming the successful grafting of the
amine derivatives to silica and their surface area measured using Brunauer–Emmett–Teller method
(BET). The influenceof reaction conditions on the graft density of organoamineswas investigatedand it
was found that the saturation of the silane coupling agents with carbon dioxide prior to surface
modification resulted in higher graft densities. Carbon dioxide uptake of the obtained hybridmaterials
were determined by thermogravimetric analysis at room temperature as well as higher temperatures
resulting in CO2 adsorption capacities from 32.4 to 69.7mggÀ1 adsorbent.
ß 2013 Elsevier Ltd. All rights reserved.
* Corresponding authors. Tel.: +1 213 740 5984; fax: +1 213 740 6679.
E-mail addresses: [email protected] (G.K. Surya Prakash), [email protected]
(G.A. Olah).
1 Average heat capacity of Sil-N2 determined by DSC in the temperature range
from 50 to 110 8C.
Contents lists available at SciVerse ScienceDirect
Journal of CO2 Utilization
jo urn al hom ep ag e: www.elsev ier .com/locat e/ jco u
2212-9820/$ – see front matter ß 2013 Elsevier Ltd. All rights reserved.
http://dx.doi.org/10.1016/j.jcou.2013.03.007
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Substituting aqueous adsorbents by solid analogues offers
therefore a potentially lower cost solution. Developing more
economical alternatives for CO2 adsorption is part of our ongoing
efforts (Methanol Economy1) [11] on CO2 capture and its
conversion to value added products such as methanol [11–13],
dimethyl ether, [12] formic acid [14,15], methyl formate and
eventually to most of the important petrochemical intermediates
such as ethylene and propylene, which are presently produced
from natural gas or petroleum oil.
Various approaches have been utilized to prepare inorganic–
organoamine hybrid materials. Based on the interactions that occurbetween the organic compounds and the inorganic supports, the
synthetic techniques can be divided into two main groups. Materials
in which there is physical interaction between the amines and the
supports fall into the first group (a),e.g. amine impregnated supports
[16,17]. In order to increase the stability of the adsorbents, amines
can be chemically attached to the support giving grafted organic–
inorganic hybrids constituting the second group (b). Functionaliza-
tion of surface accessible OH groups of inorganic materials using
silane coupling agents is a widely used technique to fabricate hybrid
materials for a variety of applications [18]. Chemically attached thin
films can be prepared via ‘‘grafting from’’ techniques (b1) where the
organic coating is prepared by surface-initiated oligomerization/
polymerization [19]. They can also be prepared by immobilization of
an organic compound (e.g. polymeric) bearing anchoring groupsreacting with the OH groups of the support. This latter technique is
often referred to as the ‘‘grafting to approach’’ (b2) [20–23]. While
inorganic–organoamine adsorbents in which the organic compound
is physically adsorbed often suffer from leaching of the amine
component [16,17], chemically grafted amines usually show a better
stability, that helps to maintain the adsorption capacity over many
adsorption/desorption cycles.
The application of silica–amine hybrid materials for CO2
capture has been reviewed [23–25] and it can be observed that
a majority of the reported adsorbent materials are based on porous
(high surface area) supports. Although, the high porosity and high
surface area are advantageous for gas adsorption, very often
impregnation or grafting of organic compounds to porous supports
results
in
a
significant
drop
in
the
surface
area
indicating
thenecessity to develop new adsorbent materials using more cost
effective non-porous supports such as fumed silica. It should be
added here that we use the term ‘‘adsorption’’ in this manuscript to
indicate the reversible capture of CO2 molecules as a surface
phenomenon rather than a bulk one. Since a chemical reaction
takes place between CO2 and organoamines, in fact here we deal
with the phenomenon of chemisorption.
2. Experimental
2.1. Materials
Fumed silica Aerosil1 380 (average primary particle size 7 nm)
was
obtained
from
Evonik
(formerly
Degussa).
Toluene
(Mallinckrodt, 99.5%), methanol (Mallinckrodt, 99.8%),
3-aminopropyl-trimethoxysilane (N1, Acros, 95%), 3-(2-aminoethy-
lamino)propyltrimethoxy-silane (N2, Acros, 97%), 3-[2-(2-ami-
noethylamino)ethylamino]-propyl-trimethoxysilane (N3, Acros,
technical grade), trimethoxysilylpropyl-polyethyleneimine (PEI,
Gelest, 50% in iPrOH) were used without further purification.
2.2. Preparation of adsorbents
Aerosil-380 (7.0 g) was mixed in 280 mL toluene and N2 wasbubbled through the vigorously stirred suspension for 30 min.
19.95 mmol of silane coupling agent was added dropwise and the
reaction mixture was stirred at room temperature for 10 min before
heating to 110 8C. The suspension was stirred at this temperature
under a nitrogen atmosphere for 12 h. The cold reaction mixture was
separated by centrifugation and the obtained solid was re-
suspended in cold toluene. This suspension was again separated
by centrifugation. The above described purification steps were
repeated three times using cold methanol as a solvent. Finally, the
solid was transferred to a round bottom flask and the solvent was
removed by heating at 50 8C under vacuum on a rotovapor followed
by vacuum treatment overnight (65 mTorr). A small sample of the
obtained white solid material was placed in a sealable glass tube and
kept under vacuum at 85 8C for 3 h and then used either forcharacterization or for measuring the adsorption capacity.
2.3. Thermogravimetric analysis to determine the organic content of
the prepared adsorbent
Thermogravimetric measurements were carried out on a
Shimadzu TGA-50 thermogravimetric analyzer under an air flow
of 30 mL minÀ1 in a temperature range from 25 to 800 8C with a
heating rate of 10 8C minÀ1.
2.4. FTIR
Diffuse reflectance infrared Fourier transform spectroscopic
measurements
were conducted under vacuum
on a
Bruker
Vertex80v FTIRspectrometer using KBr as a reference. Samples were diluted
with KBr, placed into a PrayingMantisTM DRP-SAP diffuse reflection
accessory and scanned from 4000 to 500 cmÀ1 (number of
scans = 32).
2.5. Surface area and pore volume analysis
The supports were characterized by N2 adsorption/desorption
isotherm measurements on a Quantachrome NOVA 2200e instru-
ment. The surface area was determined by the multipoint BET
method. The total pore volume was evaluated at a P/P0 close to 0.995.
2.6. Heat capacity
Heat capacity of the solid adsorbent was measured on a PerkinElmer DSC 7 differential scanning calorimeter. In a typical
experiment, about 5 mg of the adsorbent (measured precisely
with a microbalance) was placed in an aluminium pan and inside
the sample cell of the DSC under a flow of nitrogen (20 mL minÀ1).
Temperature programme: heating from 0 to 120 8C with a heating
rate of 5 8C minÀ1; cooling from 120 to 0 8C with a rate of
20 8C minÀ1. This temperature programme was repeated two
times. The heat flow measured in the second cycle was considered
to determine the heat capacity.
2.7. Measurement of CO 2 adsorption capacity
6–13 mg of solid adsorbent was loaded in a platinum crucible
and placed into a Shimadzu TGA-50 thermogravimetric analyzer.
Scheme 1. Chemisorption of CO2 with amines.
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The sample was first heated to 110 8C under N2 atmosphere
(flow = 60 mL/min) and this temperature was maintained for
30 min for desorbing water and CO2 from the surface. The
adsorbent was exposed to pure CO2 (flow = 60 mL minÀ1) at
25 8C for 3 h, and then the sweeping gas was replaced with N2 at
85 8C for 90 min for desorption. The second adsorption cycle was
carried out under CO2 at 55 8C for 3 h followed by desorption under
N2 for 90 min at 85 8C.The third adsorption cycle was carried out at
85 8C for 3 h. Finally 10 adsorption/desorption cycles were carried
out isothermally at 85 8C. 15 min adsorption under pure CO2 wasfollowed by 25 min desorption under N2. For the 100 cycle
experiment, adsorption (10 min, 85 8C) was followed by desorp-
tion (15 min, 85 8C). Otherwise the experimental conditions were
similar to those described earlier.
3. Results
3.1. Preparation and characterization of adsorbent materials
Herein, we report on the facile synthesis of alkylamine-fumed
silica hybridmaterialsfromcommercially available and relatively
inexpensive starting materials. We have selected Aerosil-380
(fumedsilica, averageprimary particlesize7 nm [26], surfacearea
329 m2
gÀ1
) as a support forthe amine containing adsorbents. It isgenerally acceptedand widelypracticed that surface hydroxyls of
inorganic substrates can be functionalized with reactive groups
such as chlorosilanes [18,27], alkoxysilanes [18], and phosphonic
acid derivatives [28], establishing chemically attached organic
layers on the inorganic materials. Primary and secondary
trialkoxysilylalkylamines such as 3-aminopropyl-trimethoxysi-
lane (N1), 3-(2-aminoethylamino)propyltrimethoxysilane (N2),
3-[2-(2-aminoethylamino)ethylamino]propyl-trimethoxysilane
(N3), and trimethoxysilylpropyl-polyethyleneimine (PEI) were
immobilized onto Aerosil-380 by the reaction of alkoxysilyl
anchoring groups andsurface silanol groups of the supportgiving
siloxane linkages (Scheme 2).
The obtained suspension was separated by centrifugation
and the
adsorbent particles
were
washed
repeatedly withtoluene and methanol and dried under reduced pressure
(65 mTorr) at 85 8C. Hybrid materials were characterized by
thermogravimetric analysis (TGA) and diffuse reflectance
infrared Fourier transform spectroscopy (DRIFT). The surface
area was determined by the Brunauer–Emmett–Teller method
(BET).
Graft density and nitrogen content of adsorbent-grafted silica
particles were calculated on the basis of weight losses indicated by
the thermograms. Representative thermograms of bare
Aerosil-380 (a), Sil-N3 (b), Sil-N3-CO2 (c), Sil-PEI (d) (heating
rate 10 8C minÀ1, 30 mL minÀ1 air) are shown in Fig. 1.
Weight losses (WL) were recorded in the temperature range from
25 to 800 8C and nitrogen contents (NC) are summarized in
Table
1.
Grafting of N1 onto Aerosil-380 resulted in Sil-N1 adsorbent,
which contained 1.89 mmol N atom gÀ1 silica while immobiliza-
tion of N2 containing two nitrogen atom per molecule resulted in
an almost double amine loading (3.42 mmol N atom gÀ1 silica).
Immobilization of N3 did not follow the same trend and resulted
only in slightly higher amine content (3.56 mmol N a-
tom gÀ1 silica) compared with Sil-N2.
Not surprisingly, covalent immobilization of alkylaminotri-
methoxysilanes onto Aerosil-380 resulted in significant decrease
in surface area compared to the bare support. While Aerosil-380had a surface area of 329 m2 gÀ1, Sil-N1, Sil-N2 and Sil-N3 were
found to have 159, 148 and 157 m2 gÀ1, respectively, indicating a
54–57% drop in surface area. It can also be observed that the
surface area of the grafted silica particles are very similar
regardless of the silane coupling agent applied. Diffuse reflectance
infrared Fourier transform spectroscopy is a very powerful method
to gain structural information about the molecules immobilized on
the surface of inorganic materials. Successful grafting of the silane
coupling agents N1–3 is indicated by the antisymmetric ( yasNH2)
and symmetric stretching vibrations ( ysNH2) of hydrogen bonded
NH2 groups (3366 and 3302 cmÀ1) [29,30], respectively, and the
corresponding vibrations of CH2 groups ( yasCH2 at 2928 and ysCH2
at 2856 cmÀ1) [31].
Deformation vibration of amino groups (dNH2) could also bedetected at 1595 cmÀ1 in Sil-N1–3 while CH2 deformations were
observed at 1475 and 1449 cmÀ1 [31] in Sil-N1. These peaks are
overlapped in Sil-N2–3 giving a relatively broad band at
1458 cmÀ1. The disappearance of the signal in the DRIFT spectrum
of Aerosil-380 at 3745 cmÀ1 attributed to surface OH groups [32]
Scheme 2. Immobilization of N1, N2, N3 and PEI onto Aerosil-380.
Fig. 1. TGA curves of bare Aerosil-380 (a), Sil-N3 (b), Sil-N3-CO2 (c), and Sil-PEI (d).
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further confirmed the surface modification of surface OH groups
using methoxysilanes (Fig. 2).
3.2. Measurement of adsorption capacities
Adsorption capacities of the silica–alkylamine hybrids were
measured with a Shimadzu TGA-50 thermogravimetric analyzer at
room temperature, 55 8C and 85 8C using instrument grade CO2
under flow conditions. Adsorbents were heated at 110 8C for
30 min under N2 atmosphere prior to the measurements. The
weight increases were determined after an exposure to CO2 (3 h) at
each temperature. The adsorption and desorption cycles were
repeated ten times at 85 8C showing insignificant changes in the
adsorption capacities (Figs. 3 and 4).
For two selected adsorbents (Sil-N1 and Sil-PEI) the adsorp-
tion/desorption cycles were repeated 100 times at the same
temperature confirming the good stability of the hybrid adsorbents
(Fig. 5). It should be noted here that slightly lower adsorption
capacities were measured in the course of 100 cycles due to shorter
adsorption (10 min) and desorption (15 min) times.
The monoamino derivative (Sil-N1) showed moderate CO2
uptake at room temperature (32.4 mg CO2 gÀ1
adsorbent), but asexpected the adsorbents with higher nitrogen content (3.42 for Sil-
N2 and 3.56 mmol N gÀ1 for Sil-N3) exhibited a higher CO2
Table 1
Weight loss (WL), nitrogen content (NC), surface area ( ABET) and pure CO2 adsorption capacity of silica–organic hybrids.
Hybrid WL (%) NCa (mmolN gÀ1) Adsorption capacityb (mg gÀ1) Ads. CO2 per N at 25 8C ABET (m2gÀ1) Total pore
volume (mL gÀ1)
25 8C 55 8C 85 8C
Sil-N1 9.9 1.89 32.4 26.2 19.7 0.43 159 1.66
Sil-N2 14.7 3.42 35.6 27.2 18.3 0.28 148 1.61
Sil-N3 14.6 3.56 41.3 33.2 24.6 0.31 157 1.63
Sil-N1-CO2 11.8 2.29 37.4 31.5 24.5 0.42 149 1.75
Sil-N2-CO2 18.6
4.51
47.3
39.3
30.1
0.29
132
1.47Sil-N3-CO2 21.0 5.52 49.8 42.9 33.7 0.26 127 1.26
Sil-PEI 47.0 20.6 24.0 50.2 68.0 0.05 43.0 0.76
Sil-PEI-CO2 46.3 20.0 30.1 58.8 69.7 0.06 19.6 0.31
a Millimoles of NH2 and NH groups per gram silica support.b Milligrams of adsorbed CO2 per gram adsorbent.
Fig. 2. DRIFT spectra of bare Aerosil-380 (a), Sil-N1 (b), Sil-N2 (c), Sil-N3 (d), and Sil-
PEI (e).
Fig. 3. A typical thermogram of adsorption/desorption measurements for Sil-N1.
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adsorption capacities at 35.6 and 41.3 mg CO2 gÀ1 adsorbent,
respectively. CO2 adsorption was also measured at 55 and 85 8C
showing decreasing adsorption capacity, 26.2 and 19.7 mg gÀ1 for
Sil-N1, respectively, as the temperature increased. A trend could beobserved for the diamine and triamine functionalized silica giving
lower adsorption capacities, 27.2/18.3 mg gÀ1and 33.2/
24.6 mg gÀ1at 55 and 85 8C respectively.
In order to further increase the adsorption capacities of the
hybrid materials, we attempted to achieve higher graft densities byfollowing a different grafting procedure. It was shown that H-
Fig. 4. Adsorption capacities of functionalized silica particles at 25/55/85 8C followed by 10 cycles of adsorption/desorption at 85 8C.
Fig. 5. Adsorption capacity of Sil-N1 and Sil-PEI in repeated adsorption and desorption cycles at 85 8C. Inset: Adsorbent weight versus time diagram for Sil-PEI.
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bonded aminopropylsilanes are less reactive and only a small
portion of alkoxysilane groups participates in Si–O–Si bond
formation [29].
It was also suggested that the saturation of alkylaminotri-
methoxysilane solutions with CO2 prior to introducing the solid
support facilitates covalent immobilization preventing the inter-
action of amine nitrogens of silane coupling agents with surface
silanols through hydrogen bonding [33]. Following these leads,
toluene solutions of N1–3were evacuated and then exposed to CO2
for 15 min before silica particles were added. The suspension was
then slowly heated to 60 8C and the temperature was maintained
for 30 min. After that, the reaction mixture was heated and kept at
110 8C for 12 h. In accordance with the results of Knowles et al.
[33], we obtained alkylamino-grafted silica with higher graft
densities (Sil-N1-CO2: 2.29; Sil-N2-CO2: 4.51; Sil-N3-CO2:
5.52 mmol N atom gÀ1 silica) which corresponds to a 21, 32 and
55% increase compared to the adsorbents prepared in the absence
of CO2. Interestingly the increase in graft density is higher when
the silane coupling agent contains more nitrogen which seems to
confirm that the reaction of amino groups with CO2 makes the
formation of hydrogen bond with surface silanol groups less
favourable. The higher graft densities resulted in higher CO2
adsorption capacities of 37.4, 47.3 and 49.8 mg CO2 gÀ1 adsorbent
at 25 8C, respectively, and similar trend could be observed at 55and 85 8C as well (Table 1).
Similarly to the adsorbents prepared from practically CO2 free
silane coupling agents and silica suspension these hybrid materials
also showed lower adsorption capacity at higher temperature
(Table 1). Immobilization of N1, N2 and N3 using solutions
saturated with CO2 resulted in slightly lower surface areas (149,
132 and 127 m2 gÀ1) than those we obtained for Sil-N1, Sil-N2 and
Sil-N3 but significantly lower than that of bare Aerosil-380.
As the increasing number of secondary amino groups in the
grafted layer resulted in better CO2 adsorption capacity per g
adsorbent, we attempted to immobilize polyethyleneimine
bearing trimethoxysilyl (PEI) anchoring groups. (The average
number of ethyleneimine groups in the PEI chain was 18 based on1
H NMR measurements).2
The high organic content of the hybridmaterials was reflected by the significant weight losses in TGA
experiments. Sil-PEI showed a weight loss of 47.0%
(20.6 mmolN gÀ1) between 200 and 800 8C.
DRIFT study of PEI-grafted silica revealed stretching vibration of
NH groups at 3255 cmÀ1 and a group of signals from 2947 to
2825 cmÀ1 due to antisymmetric and symmetric CH2 stretching
vibrations. Moreover the CH2 deformation bands overlapped
showing an intense and broad peak at 1450 cmÀ1.
Impregnation or covalent grafting of polymers onto supports
usually causes dramatic decrease of the surface area as it was
observed in the case of Sil-PEI. Surface area of Sil-PEI (43 m2 gÀ1)
showed a 87% decrease compared to that of Aerosil-380.
Regardless, the low surface area PEI-grafted silica exhibited
remarkable
adsorption
capacities
of
68.0
mg
CO2 gÀ1
at
85 8C
compared with mono-, di- and triamine functionalized silica.
We also attempted to obtain a higher graft density of amine
adsorbents on silica by saturating the toluene solution of silane
coupling agents with CO2 prior to the addition of Aerosil-380 using
PEI. Although the saturation of the silane coupling agent with CO2
resulted in higher graft density for the mono-, di- and triamine
derivatives it did not increase the graft density for PEI. (N content
of 20.0 mmolN gÀ1) compared to what we obtained under a
nitrogen atmosphere (20.6 mmolN gÀ1). Furthermore, while all the
mono-, di- and triamine-functionalized silica showed lower
adsorption capacity at higher temperature a reverse trend could
be observed in the adsorption capacity in the case of Sil-PEI and
Sil-PEI-CO2. Although the graft density of Sil-PEI-CO2 was
somewhat lower than for Sil-PEI, its CO2 adsorption was however
slightly higher. This hybrid material exhibited an adsorption
capacity of 24.0/50.2/68.0 mg gÀ1 and 30.1/58.8/69.7 mg gÀ1 at 25,
55 and 85 8C, respectively.
As reflected by a large number of publications, a variety of
supports such as mesoporous [34] or delaminated [35] materials,
and metal organic frameworks (MOFs) [36] were functionalized
with organoamine derivatives in order to develop high perfor-
mance CO2 adsorbent materials. If one intends to make a detailed
comparison of present results with those reported in the literature,
one should refer to a comprehensive review by Jones et al. [23]
Furthermore, the comparison of the adsorption capacity and
surface area of some hybrid materials with present aminopropyl-
functionalized fumed silica is also given in the supplementary
information (Table S1).
Supplementary material related to this article found, in the
online version, at doi:10.1016/j.jhazmat.2012.10.056.
4. Conclusions
Silica–organoamine
hybrid
materials
were
prepared
by
cova-lent grafting of alkylamines (with one, two or three amino groups)
and polyethyleneimine bearing reactive methoxysilane groups.
The characterization of the grafted silica particles was carried out
by thermogravimetry, DRIFT and BET methods. Both the nitrogen
contents and the adsorption capacities of hybrid materials
increased (although not linearly) as the molecular weight of the
organic component increased. However the CO2/N ratio decreased,
indicating that less amino functional groups were accessible or/
and active for adsorption. Higher graft densities and higher CO2
adsorption capacities could be obtained when silane coupling
agents containing one, two or three amino groups were saturated
with CO2 prior to the reaction with surface silanol groups. Mono-,
di- and triamine-functionalized silica sorbents showed decreasing
adsorption
capacities
as
a
function
of
temperature
while
thepolyamine-functionalized ones exhibited increasing adsorption
capacity at higher temperatures. Organoamine functionalized
fumed silica adsorbents are easy to prepare, high performance
adsorbents and more cost effective alternatives to other amine-
grafted porous adsorbents based on supports for carbon dioxide
capture. To the best of our knowledge it is also the first time that
trimethoxysilylpropyl-polyethyleneimine has been used to pre-
pare materials for CO2 adsorption.
Acknowledgement
Support of our work by the Loker Hydrocarbon Research
Institute and the United States Department of Energy is gratefully
acknowledged.
References
[1] N.M. Whiteley, Mar. Ecol. Prog. Ser. 430 (2011) 257–271.[2] D.P. Schrag, Science 325 (2009) 1658–1659.[3] F.M. Orr Jr., Science 325 (2009) 1656–1658.[4] G.A. Olah, A. Goeppert, M. Czaun, G.K.S. Prakash, J. Am. Chem. Soc. 135 (2012)
648–650.[5] M. Aresta, Carbon, Dioxide as Chemical Feedstock, Wiley-VCH, Weinheim,
Germany, 2010.[6] A. Goeppert, M. Czaun, R.B. May, G.K.S. Prakash, G.A. Olah, S.R. Narayanan, J. Am.
Chem. Soc. 133 (2011) 20164–20167.[7] A.Goeppert, M.Czaun,G.K. SuryaPrakash,G.A.Olah, EnergyEnviron.Sci. 5 (2012)
7833–7853.[8] M. Aresta, A. Dibenedetto, Catal. Today 98 (2004) 455–462.[9] G.T. Rochelle, Science 325 (2009) 1652–1654.
[10]
T.-W. Shih, A.N. Soriano, M.-H. Li, J. Chem. Thermodyn. 41 (2009) 1259–1263.
2 Number of ethyleneimine groups were determined based on the integrals of
methoxide-
and
ethylene
protons
in
the
1
H
NMR
spectrum.
M. Czaun et al. / Journal of CO 2 Utilization 1 (2013) 1–7 6
7/27/2019 Organoamines-Grafted on Nano-sized Silica for Carbon Dioxide Capture
http://slidepdf.com/reader/full/organoamines-grafted-on-nano-sized-silica-for-carbon-dioxide-capture 7/7
[11] G.A. Olah, A. Goeppert, G.K.S. Prakash, Beyond Oil and Gas The MethanolEconomy, 2nd ed., Wiley VCH, Weinheim, Germany, 2009.
[12] G.A. Olah, A. Goeppert, G.K.S. Prakash, J. Org. Chem. 74 (2009) 487–498.[13] G.A.Olah,G.K.S. Prakash,A. Goeppert,J. Am.Chem. Soc.133 (2011)12881–12898.[14] M.Czaun, A. Goeppert,R. May,R. Haiges, G.K.S. Prakash,G.A.Olah, ChemSusChem
4 (2011) 1241–1248.[15] A. Boddien, B. Loges, H. Junge, F. Gartner, J.R. Noyes, M. Beller, Adv. Synth. Catal.
351 (2009) 2517–2520.[16] A. Goeppert, S. Meth, G.K.S. Prakash, G.A. Olah, Energy Environ. Sci. 3 (2010)
1949–1960.[17] S.Meth,A. Goeppert,G.K.S.Prakash,G.A.Olah, Energy Fuels 26(2012)3082–3090.
[18]
M. Czaun, A.K. Mallik, M. Takafuji, H. Ihara, in: W.J. Ackrine (Ed.), PolymerInitiators, Nova Science Publishers, Hauppauge, NY, USA, 2010.[19] Z. Liang, B. Fadhel, C.J. Schneider, A.L. Chaffee, Micropor. Mesopor. Mater. 111
(2008) 536–543.[20] V. Zelenak, D. Halamova, L. Gaberova, E. Bloch, P. Llewellyn, Micropor.Mesopor.
Mater. 116 (2008) 358–364.[21] G.P . Knowles, S.W. Delaney, A.L. Chaffee, Ind. Eng. Chem. Res. 45 (2006)
2626–2633.
[22] C. Knofel, J. Descarpentries, A. Benzaouia, V. Zelenak, S. Mornet, P.L. Llewellyn, V.Hornebecq, Micropor. Mesopor. Mater. 99 (2007) 79–85.
[23] S. Choi, J.H. Drese, C.W. Jones, ChemSusChem 2 (2009) 796–854.[24] Q. Wang, J. Luo, Z. Zhong, A. Borgna, Energy Environ. Sci. 4 (2011) 42–55.[25] D.M.D’Alessandro,B. Smit, J.R.Long, Angew. Chem.Int. Ed. 49 (2010) 6058–6082.[26] Product Data Sheet, Evonik Industries (Former Degussa).[27] M. Czaun, M.M. Rahman, M. Takafuji, H. Ihara, Polymer 49 (2008) 5410–5416.[28] I. Minet, J. Delhalle, L.Hevesi, Z.Mekhalif,J. ColloidInterfaceSci. 332(2009)317–326.[29] L.D. White, C.P. Tripp, J. Colloid Interface Sci. 232 (2000) 400–407.[30] K.C. Vrancken, P. Vandervoort, I. Gillisdhamers, E.F. Vansant, P. Grobet, J. Chem.
Soc., Faraday Trans. 88 (1992) 3197–3200.
[31]
N. Hiyoshi, K. Yogo, T. Yashima, Micropor. Mesopor. Mater. 84 (2005) 357–365.[32] T. Takei, K. Kato, A. Meguro, M. Chikazawa, Colloids Surf. A 150 (1999) 77–84.[33] G.P.Knowles, V. Beyton, A.L.Chaffee,Prepr. Symp.-Am.Chem Soc.Div. FuelChem.
51 (2006) 102–103.[34] V. Zelenak, M. Badanicova, D. Halamova, J. Cejka, A. Zukal, N. Murafa, G. Goerigk,
Chem. Eng. J. 144 (2008) 336–342.[35] A. Zukal, I. Dominguez, J. Mayerova, J. Cejka, Langmuir 25 (2009) 10314–10321.[36] S.N. Kim, S.T. Yang, J. Kim, J.E. Park, W.S. Ahn, CrystEngComm 14 (2012)
4142–4147.
M. Czaun et al. / Journal of CO 2 Utilization 1 (2013) 1–7 7