Methanol Steam Reforming Promoted by Molten Salt-Modified Platinum on Alumina Catalysts

Article abstract of DOI:10.1002/cssc.201402357

We herein describe a straight forward procedure to increase the performance of platinum-on-alumina catalysts in methanol steam reforming by applying an alkali hydroxide coating according to the “solid catalyst with ionic liquid layer” (SCILL) approach. We demonstrate by diffuse reflectance infrared Fourier transform spectroscopy (DRIFTS) and temperature-programmed desorption (TPD) studies that potassium doping plays an important role in the catalyst activation. Moreover, the hygroscopic nature and the basicity of the salt modification contribute to the considerable enhancement in catalytic performance. During reaction, a partly liquid film of alkali hydroxides/carbonates forms on the catalyst/alumina surface, thus significantly enhancing the availability of water at the catalytically active sites. Too high catalyst pore fillings with salt introduce a considerable mass transfer barrier into the system as indicated by kinetic studies. Thus, the optimum interplay between beneficial catalyst modification and detrimental mass transfer effects had to be identified and was found on the applied platinum-on-alumina catalyst at KOH loadings around 7.5 mass %.

Full text of DOI:10.1002/cssc.201402357

CHEMSUSCHEM
FULL PAPERS
DOI: 10.1002/cssc.201402357
Methanol Steam Reforming Promoted by Molten Salt-
Modified Platinum on Alumina Catalysts
Matthias Kusche,[a] Friederike Agel,[a] Nollaig Nꢀ Bhriain,[a] Andre Kaftan,[b] Mathias Laurin,[b]
Jçrg Libuda,[b] and Peter Wasserscheid*[a]
We herein describe a straight forward procedure to increase
the performance of platinum-on-alumina catalysts in methanol
steam reforming by applying an alkali hydroxide coating ac-
cording to the “solid catalyst with ionic liquid layer” (SCILL) ap-
proach. We demonstrate by diffuse reflectance infrared Fourier
transform spectroscopy (DRIFTS) and temperature-pro-
grammed desorption (TPD) studies that potassium doping
plays an important role in the catalyst activation. Moreover,
the hygroscopic nature and the basicity of the salt modifica-
tion contribute to the considerable enhancement in catalytic
performance. During reaction, a partly liquid film of alkali hy-
droxides/carbonates forms on the catalyst/alumina surface,
thus significantly enhancing the availability of water at the cat-
alytically active sites. Too high catalyst pore fillings with salt in-
troduce a considerable mass transfer barrier into the system as
indicated by kinetic studies. Thus, the optimum interplay be-
tween beneficial catalyst modification and detrimental mass
transfer effects had to be identified and was found on the ap-
plied platinum-on-alumina catalyst at KOH loadings around
7.5 mass%.
Introduction
Methanol steam reforming is the method of choice to produce
hydrogen from methanol in high yields.[1] Under optimal pro-
cess conditions, the reaction converts one mol of methanol
and water into carbon dioxide and three mol of hydrogen, as
shown in Equation (1).
To complete the storage cycle, hydrogen release from meth-
anol requires attention. For decentralized hydrogen produc-
tion, highly efficient hydrogen release under mild conditions is
desired, for example, to allow heat integration of the endo-
thermic steam reforming step with available low caloric heat
streams. Currently, the upper limit for high-temperature proton
exchange membrane (PEM) fuel cells is 1808C.[3] It would be
highly desirable to efficiently operate methanol steam reform-
ing at this temperature level to provide the necessary heat for
the endothermic methanol reforming step from the exother-
mic operation of the fuel cell. Moreover, the product gas
should be virtually free of CO to allow its use in a PEM fuel
cell. As CO is a known poison to fuel cell catalysts,[4] high con-
centrations of CO in the product gas would require costly addi-
tional gas processing steps, such as CO adsorption, preferential
oxidation (PROX), or methanation. To fulfil these requirements,
the development of more effective catalyst systems for metha-
nol steam reforming is of great technical interest.
CH3OH þ H2O ! CO2 þ 3 H2 DH0298 ¼ 49:4 kJ molꢀ1
ð1Þ
Nowadays, methanol steam reforming is receiving considera-
ble attention in the context of a methanol-based energy stor-
age and release cycle.[2] Methanol is considered as a promising
candidate to store hydrogen produced by electrolysis with
electricity from regenerative excess energies (e.g., from wind
and solar). In this context, methanol should not be produced
via synthesis gas from fossil energy reserves but by hydrogena-
tion of CO2. The latter may be recovered from the flue gas of
power plants or from the exhaust gas of the cement industry.
For MeOH steam reforming two different classes of hetero-
geneous catalysts dominate research and industrial practice.
The commercial Cu/ZnO systems are indeed very active and
selective, but they require lengthy activation procedures. For
this purpose, the catalyst is typically brought in contact with
a diluted stream of hydrogen for several hours. However, such
catalyst preformation is inappropriate for most fluctuating, on-
demand hydrogen production scenarios. In addition, copper-
based catalysts are highly pyrophoric materials in their activat-
ed state and require reasonable treatment to avoid deactiva-
tion during standby. These facts complicate the practical han-
dling of copper-based catalysts in dynamic on–off cycles. Cata-
lyst formulations based on noble metals are easier to handle
[a] M. Kusche, Dr. F. Agel, Dr. N. Nꢀ Bhriain, Prof. Dr. P. Wasserscheid
Lehrstuhl fꢁr Chemische Reaktionstechnik
Friedrich-Alexander-Universitꢂt Erlangen-Nꢁrnberg
Egerlandstrasse 3, 91058 Erlangen (Germany)
Fax: (+49)9131-8527421
E-mail: wasserscheid@crt.cbi.uni-erlangen.de
Homepage: www.crt.cbi.uni-erlangen.de
[b] A. Kaftan, Dr. M. Laurin, Prof. Dr. J. Libuda
Lehrstuhl fꢁr Physikalische Chemie II
Friedrich-Alexander-Universitꢂt Erlangen-Nꢁrnberg
Egerlandstrasse 3, 91058 Erlangen (Germany)
Fax: (+49)9131-8528867
Supporting Information for this article is available on the WWW under
http://dx.doi.org/10.1002/cssc.201402357.
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2516

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
and often show immediate start up. Here, especially the use of
palladium or platinum on different types of support materials
has been reported for the methanol steam reforming reac-
tion.[5]
setup (see the Supporting Information for details) by bringing
the catalyst in contact with a diluted gas stream of methanol
and water (in equimolar ratio).
As dynamic hydrogen production scenarios are the focus of
our research, we investigated in this study the optimization of
supported platinum catalysts for methanol steam reforming.
We expand here on an earlier communication of our group,[6]
which demonstrated that platinum-on-alumina (Pt/Al2O3) cata-
lysts exhibit an exceedingly enhanced activity and selectivity
after surface modification with basic and strongly hygroscopic
inorganic salts.
Results and Discussion
Figure 1 shows a comparison of the methanol steam reforming
performance of the neat Pt/Al2O3 catalyst and the same cata-
lyst coated with a loading of w=30 wt% potassium acetate at
T=2308C under otherwise identical reaction conditions.[6]
Initially, our idea was to modify a commercial Pt/Al2O3 cata-
lyst (Alfa Aesar, platinum content 4.86 wt%) with a molten salt
coating to benefit from the known low hydrogen solubility of
these liquids. In other words, our initial goal was to alter the
sorption behavior of substrates and products in methanol
steam reforming by the salt coating.[7]
Chemical modification of heterogeneous catalysts with
a thin film of a liquid salt is not new. In literature, this ap-
proach has been extensively studied for low melting salts, so-
called ionic liquids (ILs), and the term “solid catalyst with ionic
liquid layer” (SCILL) has been coined for this approach.[8] SCILL
systems take advantage of specific physicochemical properties
of the IL coating (e.g., differential solubility effects),[7] but also
benefit from distinct chemical interactions between the liquid
salt and the active surface sites (e.g., alteration of adsorption/
desorption processes). The IL film resides on the catalyst sur-
face at conditions of continuous gas phase processes due to
its exceedingly low vapor pressure. Remarkable enhancement
of selectivity has been observed in a number of hydrogenation
reactions after SCILL-type surface modifications (typically at
the expense of some activity loss).[9] Moreover, extensive sur-
face science studies have elucidated the microscopic origin of
the observed selectivity effects for SCILL systems.[10]
Figure 1. Continuous steam reforming of methanol using the uncoated Pt/
Al2O3 catalyst (left side) and the Pt/Al2O3 catalyst coated with K[OAc]
w=30 wt% (right side). TOF (coarse diagonal filling), SCO (crossed filling),
2
and EA (fine diagonal filling); experimental conditions: T=2308C; ptot =5 bar;
p
MeOH =pH O =0.5 bar; mcat. =401.4 mg; t=10 s.
2
Remarkably, by coating the Pt/Al2O3 contact with potassium
acetate an increase in activity by a factor of 1.5 and an increase
in CO2 selectivity (SCO ) from 62% to 99% could be realized. To
2
From our previous work it was known, that ILs carrying or-
ganic heterocyclic cations would not withstand the reaction
conditions required for methanol steam reforming.[11] For the
imidazolium cation, it has been found that temperatures
above 1808C in combination with water vapor lead to ring hy-
drolysis liberating coordinating amines. Therefore, we initially
selected the inorganic molten salt mixture Li/K/Cs acetate
(molar ratio=0.2:0.275:0.525)[12] as coating for the Pt/Al2O3 cat-
alyst. Following these first investigations,[6] the salt selection
for catalyst modification has been expanded to alkali hydrox-
ides and carbonates. Note that all successfully applied salts
leading to catalyst activation were highly hygroscopic. It was
assumed that under reaction conditions a highly concentrated
salt solution forms in the catalyst pores regardless of the melt-
ing point of the water-free salt. In general, all salt-modified Pt/
Al2O3 catalysts were obtained by adding a defined amount of
salt to the heterogeneous catalyst in form of an aqueous solu-
tion, followed by solvent removal and drying under vacuum.
The amount of applied salt(s) resulted in a certain mass load-
ing, with w being the mass of salt divided by the mass of the
uncoated Pt/Al2O3 catalyst. All methanol steam reforming ex-
periments were carried out in a continuous fixed bed reactor
explain this strong positive effect of the salt coating, a variation
in salt loading was carried out. Moreover, coatings with several
individual alkali acetates were tested, with the result that po-
tassium acetate shows the strongest enhancement in per-
formance. Anion variation of the salt coating included acetate,
hydroxide, hydrogen carbonate and [NTf2]ꢀ salts and revealed
that catalyst modification by KOH was the most effective.[6] We
identified three different reasons for the observed enhanced
catalytic performance after salt coating: a) alkali doping has
been demonstrated to be relevant for the increased CO2 selec-
tivity; b) the hygroscopic nature of the applied salt was as-
sumed to be relevant for increasing water availability at the
catalytic site; and c) the basicity of the salt was regarded to be
important for the promotion of the water–gas-shift reaction
step, that is, the conversion of CO and water into CO2 and hy-
drogen.[13] The latter reaction forms an important part of the
methanol steam reforming reaction sequence.
Based on the particularly promising results for the KOH-
coated system, a variation in loading of KOH (3.75, 7.5, 17.15,
and 30 wt%) on the Pt/Al2O3 contact was performed at a reac-
tion temperature of 2308C (Figure 2). Although the uncoated
reference catalyst showed only a CO2 selectivity of 62%, the
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2517

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
Figure 3. Comparison of catalytic performance of different salt coated Pt/
Al2O3 catalysts in MeOH steam reforming at T=2308C variation in salt load-
*
*
Figure 2. Comparison of TOF ( ) and selectivity ( ) for a Pt/Al2O3 contact
coated with four different loadings of KOH (3.75 wt%, 7.5 wt%, 17.15 wt%,
30 wt%) at T=2308C, otherwise equal reaction conditions: pabs =5 bar,
ing w; TOF (coarse diagonal filling), SCO (crossed filling) and EA (fine diagonal
2
filling); otherwise identical reaction conditions: pabs =5 bar,
p
MeOH =pH O =0.5 bar, mcat. =401.4 mg, nPt =0.10 mmol, t=10 s.
2
p
MeOH =pH O =0.5 bar, mcat. =401.4 mg, nPt =0.10 mmol, t=10 s; pore filling
degree adry calculated with 1KOH =2.04 cm3 gꢀ1
2
.
LiOH and CsOH coatings led to excellent selectivities but at
somewhat lower activity. Considering the activation energies
(variation of T=200–2308C in steps of 108C), a difference be-
tween the uncoated (EA =63 kJmolꢀ1) and the hydroxide-
coated catalysts (e.g., KOH: EA =50 kJmolꢀ1) was observed.
This could be attributed to a change in reaction mechanism
(e.g., different rate-determining step) or an altered adsorption/
desorption behavior of reactants (note that changing concen-
trations/activities of reactants and products with temperature
are included in this formal EA figure).
same contact coated with KOH resulted in selectivities above
99% regardless of the KOH loading. In contrast to this loading-
independent step change in selectivity, the observed catalytic
activity was quite sensitive to the amount of salt used. The
highest activity was obtained for a KOH loading of 7.5 wt%
(turnover frequency TOF=67 hꢀ1), whereas higher salt loadings
led to a steep decline in activity. We assume that this is an
effect of an increasing share of aqueous salt solution in the
pores of the catalyst causing mass transport limitation effects,
as will be discussed in detail later. Note that the applied salt
loadings caused only low pore filling degrees based on the dry
mass of KOH (adry), but a significant expansion in volume can
be expected during water saturation of this salt under reaction
conditions.
Diffuse reflectance infrared Fourier transform spectroscopy
investigations
It is known that the presence of alkali species in catalyst coat-
ings can result in enhancement of activity and selectivity.[6]
This type of modification, typically referred to as alkali doping,
is highly relevant for many industrial catalysts, such as for ex-
ample, catalysts for ammonia, methanol, and sulfuric acid syn-
thesis, as well as hydrogenation reactions.[14] For hydrogen pro-
duction through decomposition of formic acid it has been
stated that the reaction rate of a Pd/C catalytic system was en-
hanced by one to two orders of magnitude through a modifica-
tion with potassium.[15] For a ruthenium-based water–gas-shift
catalyst it could be shown, that the activity and selectivity was
enhanced through an impregnation of the catalytic surface
with K2CO3.[16]
In a next set of experiments we were interested whether
these effects can also be achieved by modification of the cata-
lyst with other alkali hydroxides. LiOH, NaOH, and CsOH were
tested; for better comparison the molar amount of salt was
kept constant with respect to the sample with 7.5 wt% KOH.
This led to applied mass loadings of 3.2 wt% LiOH, 5.35 wt%
NaOH, and 20 wt% CsOH. In addition, loadings of 20 wt%
LiOH and 20 wt% NaOH as well as 7.5 wt% CsOH were used
to test also for potential mass transport limitation effects of
these salts. All experiments were carried out at T=2308C and
the results (TOF, SCO , activation energy EA) are presented in
2
Figure 3.
Clearly, all catalysts impregnated with alkali hydroxide salts
show better catalytic results than the uncoated reference cata-
lyst. Samples impregnated with KOH or NaOH revealed the
highest gain in activity and selectivity. For our reference load-
ing (NaOH: 5.35 wt%; KOH: 7.5 wt%) both, NaOH- and KOH-
modified systems result in very similar catalytic activities
(TOFNaOH =68 hꢀ1; TOFKOH =67 hꢀ1) and a CO2 selectivity above
99%. Both systems show declining activity with salt amounts
above this reference loading. Also the 20 wt% loadings of
To further elucidate the molecular effects of a salt modifica-
tion on the Pt/Al2O3 catalyst in methanol steam reforming we
performed diffuse reflectance infrared Fourier transform spec-
troscopy (DRIFTS). After catalyst preparation (see the Experi-
mental Section) we performed DRIFT spectroscopy to screen
the change in CO adsorption at the Pt/Al2O3 surface induced
by coatings with LiOH, KOH, and CsOH. Again, the molar
amount of hydroxide on the catalyst samples was kept equal
by applying LiOH, KOH, and CsOH loadings of 3.2 wt%,
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2518

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
a bridged state on the terraces. Additional effects proposed
are short-range interactions between CO and the dopant and
an electron transfer from the alkali species to the antibonding
2p orbitals of CO by means of the platinum d bands.[20] These
effects account for increased CO2 selectivities during methanol
steam reforming. Because of the surface modification with
alkali species, adsorbed CO is more tightly bound to the plati-
num surface and thus the possibility for a consecutive reaction
towards CO2 is enhanced. To further confirm this correlation,
we performed CO chemisorption and temperature-pro-
grammed desorption (TPD) to analyze the strength of the CO
bonding in more detail.
Figure 4. CO region of the DRIFTS spectra for Pt/Al2O3 catalysts coated with
different alkali hydroxides: LiOH, KOH, and CsOH, compared to the CO ad-
sorption at the uncoated Pt/Al2O3 surface.
CO Chemisorption–Desorption
All CO chemisorption experiments were carried out by per-
forming CO pulse chemisorption at 408C. The catalyst disper-
sions resulting from surface coating with K[OAc], KOH, and
K2CO3 were investigated (Figure 5).
7.5 wt%, and 20 wt%, respectively. In all cases the molar ratio
of alkali metal to platinum (nAM/nPt) was 5.5. A further experi-
ment with a higher KOH loading (w=17.15 wt%, nK/nPt =12.3)
was performed to show the influence of higher salt loading.
Figure 4 presents the CO region of the corresponding DRIFT
spectra for these samples and compares these to the uncoated
Pt/Al2O3 surface.
In the spectrum for the clean Pt/Al2O3 surface, the largest
absorption is visible at 2084 cmꢀ1 with
a shoulder at
2030 cmꢀ1 and a less intense feature at 1840 cmꢀ1. The catalyst
coated with LiOH shows nearly no difference compared to the
uncoated sample. Apparently, the amount of LiOH is too low
to induce a detectable change in CO adsorption. The spectra
for the Pt/Al2O3 surface modified with KOH are quite different
compared to the unmodified one. The position of the peak at
2084 cmꢀ1 is almost unchanged, but the intensity is nearly
halved with the higher loading of KOH (w=17.15 wt%). The
shoulder previously located at 2030 cmꢀ1 gains intensity and
shifts to lower wavenumbers (2010–2020 cmꢀ1). The peak origi-
nally located at 1840 cmꢀ1 also shifts to lower wavenumbers
Figure 5. Dispersions measured by CO chemisorption for Pt/Al2O3 catalysts
~
&
^
coated with different loadings of K[OAc] ( ), KOH [ratio 0.8 ( ) and 1 ( )],
*
and becomes more intense. For the sample with wKOH
=
and K2CO3 ( ).
17.15 wt% a new feature appears at 1751 cmꢀ1, which can be
attributed to [CO3]2ꢀ.[17] Thus, the band at 1751 cmꢀ1 indicates
carbonate formation at least during catalyst preparation.[17] In
the spectrum for 20 wt% CsOH on Pt/Al2O3 the decline in in-
tensity at 2084 cmꢀ1 is clearly visible, but the formation of
a new band in the range of 1830 cmꢀ1 is only vaguely detecta-
ble. We can interpret these spectra based on literature data.
The band at 2084 cmꢀ1 is known to correlate with on-top CO
adsorbed at terraces, the feature at 2030 cmꢀ1 can be attribut-
ed to on-top CO at particle edges, and the initially less intense
band at 1840 cmꢀ1 to CO in bridged conformation on terra-
ces.[18] It is important to note that the measured intensities do
not reflect the abundances of adsorbed CO at the different
sites because of dipole coupling and intensity transfer arising
on metallic surfaces.[19] Surface science studies for alkali doping
provide an interpretation of the observed spectral changes.[20]
The intensity loss of the band at 2084 cmꢀ1 and the shift of
the two other bands suggest that the alkali cation displaces
CO from the on-top position at terraces and particle edges to
The dispersion D is determined by the number of platinum
adsorption sites measured through CO uptake divided by the
total amount of platinum on the catalyst (D=nads/nPt). Con-
cerning the stoichiometry of CO adsorption at platinum cata-
lysts, stoichiometric factors from 0.7[21] to 1.0[22] can be found
in the literature. According to the DRIFTs measurements, even
for the neat Pt/Al2O3 catalyst a small amount of CO is coordi-
nated in bridge-bonded conformation. For the calculation we
initially assumed a stoichiometry of 1:1. But for the KOH-
coated catalysts, the dispersion was additionally calculated for
a stoichiometry of 0.8:1. The mean platinum cluster size can
be calculated through the dispersion D. For the uncoated cata-
lyst, the dispersion was estimated to be 37% (1:1 stoichiome-
try), which implies that 37% of the platinum atoms are located
at the cluster surface. From this, a mean platinum cluster diam-
eter of 3 nm can be calculated. Assuming a stoichiometry of
0.8, the dispersion was estimated to be 29.8% resulting in
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2519

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
a mean particle diameter of 3.8 nm (see also TEM image in the
Supporting Information, Figure S2). If the catalyst samples
were coated with a potassium-containing molten salt, the dis-
persion values were enhanced for low salt loadings (up to w=
10 wt%). Through the modification of the platinum adsorption
sites with potassium (alkali doping), the binding sites of CO,
the binding energy, and the stoichiometry of CO adsorption
are altered.[17–23] For low salt loadings, potassium-coated Pt/
Al2O3 catalysts bind more CO than in the unmodified state.
This seems to be in conflict with the DRIFTS results on the first
view. The shift of CO coordination from the terminal to the
bridge-bonded configuration observed in the DRIFTS measure-
ments should result in a lower number of active platinum
sites; consequently, the dispersion should be reduced. One
possible explanation is the formation of platinum aluminate on
the nanoparticle surface resulting in a higher CO accessibility
of the remaining Pt0 adsorption sites and thus an enhanced
platinum dispersion at low salt loadings. However, a strong de-
cline in dispersion was observed for the KOH- and the K[OAc]-
coated samples with higher salt loadings. This can be con-
firmed by the DRIFT spectra. The higher the potassium loading,
the more CO is bound in bridge-bonded conformation. A load-
ing of w=30 wt% resulted in a dispersion below 17 wt%. Con-
sequently, less than half of the originally available platinum ad-
sorption sites take part in CO adsorption processes at these
high loadings. Additionally, at higher salt loadings (w=15–
75 wt%) occupation of CO adsorption sites by the solid salt
takes place under the water-free conditions of this experiment
(in contrast to methanol steam reforming). For a loading of
w=75 wt% the dispersion was nearly zero (D=2%), which
suggests that the platinum clusters are almost completely cov-
ered by the solid and nonporous salt. With a density of KOH in
the dry state of 2.04 gcmꢀ3 and a catalysts’ Brunauer–Emmett–
Teller (BET) surface area of 120 m2 gꢀ1, the thickness of the salt
film (given for KOH in Figure 6) can be calculated for a certain
salt loading w. Accordingly, with salt loadings higher than
75 wt% the film becomes thicker than 3 nm and a full cover-
age of the platinum clusters (mean diameter 3–4 nm) can be
expected. Apparently, for catalyst samples coated with K2CO3
a different mechanism applies. Here, with low salt loadings,
the dispersion was also enhanced compared to the uncoated
reference catalyst. But for higher loadings, the drop in disper-
sion was by far not as pronounced as that of the KOH- and
K[OAc]-modified catalysts. With a loading of 75 wt% K2CO3 on
the catalyst, a dispersion of nearly 30% was retained. Clearly,
the K2CO3 coating behaves differently in the pores, leaving
platinum adsorption sites uncovered and reachable for CO
probably due to the porous nature of the solid salt.
In a next set of experiments, we studied CO desorption from
the catalyst surface by TPD (Figure 6). For a better comparison,
catalysts impregnated with the same molar amount of potassi-
um salt are shown. The neat Pt/Al2O3 catalyst shows a first CO
desorption maximum at T=1208C, whereas for the catalysts
coated with potassium salts this desorption maximum is shift-
ed towards higher temperatures. The highest shift is found for
the KOH-coated catalysts. Note that for the K2CO3-impregnated
catalyst the CO signal might be overlaid by CO2 liberated from
the carbonate salt [analysis by means of a thermal conductivity
detector (TCD)]. The shift in CO desorption temperature is in
line with an alkali doping effect caused by all potassium salts.
The alkali ion causes a transfer of electron density from the
platinum adsorption site to the CO molecule. Consequently,
the CO gas is adsorbed more strongly and the desorption tem-
perature, representing bond strength, increases. In other
words, the TPD measurements confirm the data from IR spec-
troscopy, namely that the mode of CO binding is shifted from
a terminal/linear to a mainly bridged state (compare section
on DRIFTS investigations).[17–20] The effects of this modified
binding mode can be seen in the catalytic results in the meth-
anol reforming reaction. For nearly all alkali-containing Pt/Al2O3
catalysts the CO2 selectivity is significantly increased compared
to the unmodified catalyst at a given temperature (compare
Figures 3, 7, and 8). This effect is most pronounced for potassi-
um and sodium salt coatings. Despite the shift in desorption
temperature, CO desorption is observed above T=2008C for
the KOH-impregnated sample. Thus, it is reasonable that CO2
selectivity is lower than 100% above 2008C under conditions
of methanol steam reforming. Another interesting question
Figure 7. Continuous steam reforming of methanol using the KOH-coated
&
*
Figure 6. CO-TPD measurements of different catalysts: neat Pt/Al2O3, and Pt/
Al2O3 coated with 30 wt% K[OAc], 21.14 wt% K2CO3 and 17.15 wt% KOH (all
potassium salts applied in the same molar amount).
Pt/Al2O3 catalyst, w=7.5 wt% ( : TOF; : selectivity). Experimental condi-
tions: T=230–2008C (see vertical lines); ptot =5 bar; pMeOH =pH O =0.5 bar;
2
m
cat. =401.4 mg; t=10 s.
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2520

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
both the KOH- and the K2CO3-coated catalysts show stable and
remarkably similar performance (TOF is in a range of ꢁ2 hꢀ1).
Phase behavior of KOH–H2O saturated with K2CO3
As all reaction processes in methanol steam reforming occur
necessarily in the presence of water vapor, we considered in
our following experiments the phase behavior of the system
KOH–H2O–K2CO3 to gain more insight into the processes at the
catalysts’ surfaces. Figure 9 shows the literature-known phase
diagram of the system KOH–H2O under the assumption of sat-
uration with K2CO3.[24,25]
Figure 8. Continuous steam reforming of methanol using the K2CO3-coated
&
*
Pt/Al2O3 catalyst, w=9.2 wt% ( : TOF; : selectivity). Experimental condi-
tions: T=230–2008C (see vertical lines); ptot =5 bar; pMeOH =pH O =0.5 bar;
2
m
cat. =401.4 mg; t=10 s.
pertains to the interaction of the salt coating with the reaction
product CO2. This influence was probed by comparing metha-
nol steam reforming for Pt/Al2O3 catalysts impregnated with
KOH and K2CO3, respectively.
Comparison of KOH- and K2CO3-impregnated catalysts
Clearly, KOH coatings on the Pt/Al2O3 catalyst convert to the
corresponding carbonate in the presence of the reaction prod-
uct CO2. Therefore, we were interested in studying a catalyst
sample coated directly with K2CO3. The loading was chosen to
provide an identical potassium-to-platinum ratio. Thus, the
amount of impregnated carbonate salts corresponds to the ex-
pected loading after full transformation of a 7.5 wt% KOH
loading with CO2. Figures 7 and 8 compare these two KOH-
and K2CO3-coated catalysts in methanol steam reforming
under otherwise identical reaction conditions.
Figure 9. Phase behavior of the system KOH–H2O saturated with K2CO3
(K2CO3/KOH weight ratio=0.032) adapted after Refs. [24,25].
Indeed, the KOH and the K2CO3 coating of Pt/Al2O3 catalysts
results in nearly identical performance in methanol steam re-
forming. At T=2308C, the KOH-coated sample reaches a TOF
of 70 hꢀ1 in the beginning and deactivates to 63 hꢀ1 after 80 h
reaction time, whereas the K2CO3-impregnated catalyst shows
an activity of 63 hꢀ1. Both catalysts possess a CO2 selectivity
larger than 98% at T=2308C. Initially, the K2CO3 sample re-
veals a much higher apparent activity. This value must be cor-
rected, however, by the fact that additional CO2 is liberated
from the K2CO3 coating at the beginning of the catalytic test in
the process of establishing an equilibrium between carbonate,
water, hydroxide, and CO2 under reaction conditions. Extra CO2
formed by carbonate decomposition exits the reactor during
the first 2 h time on stream (TOS) and is quantified together
with the CO2 from methanol steam reforming (measured by
gas chromatography), thus influencing the measured activity.
An opposite situation is found in the case of the KOH coating.
Here, CO2 from the steam reforming reaction is taken up by
the KOH coating to form carbonate species on the catalyst sur-
face. This CO2 uptake by the catalyst results in an apparently
lower catalytic activity as it leads to a reduced amount of de-
tectable CO2 at the reactor outlet. Apart from these well-under-
standable differences in the first couple of hours on stream,
Apparently, under reaction conditions of methanol steam re-
forming (T=2008C; pH O =0.5 bar), a liquid film composed of
2
73.5 wt% KOH (saturated with K2CO3) and 26.5 wt% H2O is
formed on the catalysts surface. To obtain the phase diagram
shown in Figure 9, the original diagram[25] was modified using
the freezing temperatures measured by Vogel et al. for
a K2CO3-saturated KOH–H2O mixture in the range of 70–
85 wt% KOH (K2CO3/KOH weight ratio=0.032).[24] The composi-
tion was determined from the vapor pressure curves over
molten KOH–H2O–K2CO3 at T=2008C and pH O =0.5 bar. With
2
this composition one can estimate the melting point of the re-
spective KOH–H2O mixture to 143.58C. Consequently, under re-
action conditions, a highly concentrated, aqueous salt solution
is present on the active sites of the catalyst surface. Additional-
ly, the pore-filling degree a, as given for dry KOH in Figure 2,
has to be corrected under the real conditions of catalysis (T=
2008C, pH O =0.5 bar, 73.5 wt% KOH, 26.5 wt% H2O). Under
2
these conditions, the density of the salt solution is 1=
1.68 gcmꢀ3 in comparison to 1=2.04 gcmꢀ3 for KOH in the
dry state.[24] Thus, the pore-filling degrees under real catalytic
conditions have to be corrected by a factor of roughly 1.2. This
has been realized in Figure 10, which displays TOF/selectivity
vs. real loading of the salt solution.
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2521

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
*
*
*
Figure 11. Dynamic vapor sorption for the Pt/Al2O3 catalysts ( ) and the cat-
Figure 10. Comparison of TOF ( ) and selectivity ( ) for catalysts loaded
with four different amounts of KOH (3.75 wt%, 7.5 wt%, 17.15 wt%,
30 wt%) at T=2008C, the data on the x-axis represents the resulting loading
with aqueous salt solution under the applied reaction conditions:
~
&
alysts coated with w=7.5 wt% KOH ( ) or w=17.15 wt% KOH ( ) at
T=408C, relative humidity f was varied from 0 to 80%.
p
abs =5 bar, pMeOH =pH O =0.5 bar, mcat. =401.4 mg, nPt =0.10 mmol, t=10 s;
2
pore filling degree awet calculated with 1KOH =1.68 cm3 gꢀ1
.
The general trends in Figure 10 are similar to those in
Figure 2 with the best system still remaining the one with
a dry loading of 7.5 wt% KOH. Again, a clear reduction in cata-
lyst activity is observed for the higher pore-filling degrees. This
raises the question whether at high pore-filling degrees the
overall reaction rate may be influenced by fluid–fluid mass
transport effects.
Dynamic vapor sorption experiments with alkali hydroxide-
coated catalysts
As a first step towards addressing this question we probed the
adsorption equilibrium of water with the KOH-coated Pt/Al2O3
catalysts by dynamic vapor sorption (DVS) experiments. For
this purpose, the catalyst samples were dried prior to testing
(T=3008C, t=240 min). Then, the samples were contacted
with gas streams of different humidity at T=408C and the re-
sulting mass changes were recorded. All values in Figure 11
were recorded after the samples reached equilibrium at each
humidity step, that is, until their change in mass was less than
0.001%minꢀ1.
&
Figure 12. Dynamic vapor sorption for the Pt/Al2O3 catalysts ( ) and the cat-
~
*
alysts coated with w=3.2 wt% LiOH ( ), w=7.5 wt% KOH ( ) and
!
w=20 wt% CsOH ( ) at T=408C, relative humidity f varied from 0 to 80%.
In the next set of experiments we compared the water sorp-
tion behavior of several alkali hydroxides coated onto the Pt/
Al2O3 catalyst. All catalysts were prepared with the same molar
amount of hydroxide, resulting in mass loadings of w=
3.2 wt% LiOH, 7.5 wt% KOH, and 20 wt% CsOH, respectively
(see Figure 12). The adsorption isotherm for the LiOH-coated
catalyst sample results in a straight line with a maximum water
uptake of 15 wt% at f=80%. Keeping in mind that the water
solubility for LiOH is relatively low (127.4 gLꢀ1 LiOH; 1278 gLꢀ1
KOH; 3000 gLꢀ1 CsOH at T=308C)[26] and that the correspond-
ing lithium aluminate is not soluble in water, one can assume
that for the LiOH-coated catalysts predominantly surface ad-
sorption is taking place. The trend of the adsorption isotherms
for the KOH- and CsOH-coated samples is nearly identical. Both
samples take up water up to roughly 15% at a humidity of
60% and roughly 28 wt% at a humidity of 80% and show the
same nonlinear behavior of their isotherms. Our previous as-
sumption that the nonlinear behavior of the isotherms at high
The DVS experiments reveal that the uncoated Pt/Al2O3 cata-
lyst shows an almost linear water uptake up to a 12 wt%
water content at a relative humidity f=80%. After coating the
Pt/Al2O3 with KOH water adsorption significantly increases. Cat-
alyst coating with w=7.5 wt% KOH results in a water uptake
of nearly 30 wt% at 80% humidity. With 17.15 wt% salt coat-
ing the water uptake is as high as 50 wt% at 80% humidity.
From the shape of the adsorption isotherms for the KOH-
coated samples one can conclude that linear surface adsorp-
tion of water takes place at low humidity f<40%. We inter-
pret the increasing relative water uptake at a humidity f>
40% as an additional absorption of water in the formed hy-
droxide/water layer on the catalyst surface.
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2522

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
humidity is due to water absorption into a salt/water liquid
film is further confirmed by the fact that cesium aluminate
shows deliquescence in the presence of moisture (see also the
27Al magic-angle spinning (MAS) NMR measurements probing
aluminate formation).[27] In conclusion from our DVS experi-
ments it is highly likely that water condensation within the cat-
alyst pores takes place to a significant extent and is further
promoted by the type and amount of salt coating. This results
in a relatively high degree of liquid filling in the pore system
and increases the probability of mass transfer limitations at the
fluid–fluid transition.
17.15 wt% KOH mass transfer effects influence the observed
overall reaction rate.
27Al solid state NMR measurements
To shed more light on the role of salt coating on the nature of
the alumina support, 27Al solid-state MAS NMR measurements
have been carried out, both before the reaction (hydroxide-
coated Pt/Al2O3 catalysts heated to 1508C for 4 h without con-
tact with reactants) and after the reaction (T=200–2308C,
p
H O =pMeOH =0.5 bar, t=80 h on stream). Figure 14 shows the
2
Probing the influence of mass transfer on the overall ob-
served reaction rate
For these investigations we focused on the Pt/Al2O3 catalyst
loaded with w=17.15 wt% KOH. This loading shows already
a decline in activity compared to lower salt loadings (compare
Figure 2 and Figure 10). Moreover, this sample shows the high-
est water uptake in the DVS experiments, producing a high
degree of pore filling with a liquid in the catalyst during reac-
tion. Note that the KOH–H2O system should be liquid under re-
action conditions of methanol steam reforming (as shown in
Figure 9).
To test for diffusion influences, two experimental runs with
different catalyst masses were performed under otherwise
equal reaction conditions. The methanol inlet stream was
varied and the methanol conversion X was plotted against the
ꢀ1
Figure 14. 27Al solid-state MAS NMR measurements of Pt/Al2O3 coated with
alkali hydroxides before methanol steam reforming reaction (samples
heated to 1508C, t=4 h).
modified residence time mcat. nMeOH,0 (Figure 13). In such an
27Al MAS NMR spectra for the alkali hydroxide-coated Pt/g-
Al2O3 catalyst. For the uncoated reference Pt/g-Al2O3 catalyst
two broad resonances are identified. One with a maximum at
7 ppm assigned to octahedrally coordinated aluminum atom
in the alumina, whereas the other peak maximum at 65 ppm
can be assigned to tetrahedrally coordinated aluminum atoms.
Although the spectra acquired are not quantitative, they were
used for comparison purposes within this study, keeping in
mind that the aluminum site ratios may not represent all alu-
minum sites present. The ratio of tetrahedral to octahedral alu-
minum is 30:70 as known from the literature.[29] For the Pt/
Al2O3 catalysts impregnated with LiOH and heated to 1508C
(before reaction, without contact to the reactants water and
methanol), the tetrahedral resonance splits into two, with
a new narrow peak maximum appearing at 80 ppm, which can
be attributed to a lithium aluminate species.[30] Additionally,
the ratio of tetrahedrally to octahedrally coordinated alumi-
num atoms is shifted to 35:65. This shift is reasonable due to
the tetrahedral nature of the aluminum in the alkali aluminate.
For the other alkali hydroxide coatings, similar effects are ob-
served. For the NaOH-coated Pt/Al2O3, the new peak maximum
occurs at 72 ppm (tetr./oct.=50:50), for the KOH-modified Pt/
Al2O3, a new peak arises at 76 ppm (tetr./oct.=50:50), and for
the CsOH-impregnated sample, a new peak (tetr./oct.=32:68)
can be identified at 78 ppm. We interpret these findings in the
Figure 13. Test for film diffusion influence in methanol steam reforming at
T=2308C: catalyst loaded with w=17.15 wt% KOH, mcat,uncoated =200.7 mg
*
*
(
), mcat,uncoated =401.4 mg ( ); otherwise the same reaction conditions:
p
abs =5 bar, pMeOH =pH O =0.5 bar, t=10–40 s.
2
experiment the reaction would be identified as being kinetical-
ly controlled if the two graphs for the two catalyst loadings
are identical.[28] However, Figure 13 shows that the two conver-
sion vs. modified residence time graphs do not concur for the
two different amounts of catalyst. Therefore, we can conclude
that for the case of a Pt/Al2O3 catalyst loaded with w=
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2523

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
following way: By modifying the Pt/Al2O3 catalysts with alkali
hydroxides the alumina surface reacts to form surface alumi-
nate, that is, a more basic surface layer on the alumina sup-
port. Under the applied conditions support transformation to
the aluminate is far from complete as indicated by the 27Al
MAS NMR spectra. Note that in the case of LiOH coating a load-
ing of w=100 wt% would be necessary for a complete trans-
formation to the lithium aluminate. Unfortunately, it is not pos-
sible to judge from these experiments whether the formed alu-
minate exists in a partially hydrated form, as hydrated alumi-
nates exhibit nearly identical chemical shifts compared to the
non-hydrated ones.[27]
to earlier literature on the hydrolysis of aluminates[31]). In the
presence of methanol, the solubility of alumina should be fur-
ther reduced[32] so that partial alumina precipitation can be ex-
pected when methanol is present during the steam reforming
reaction. We conclude from these findings that during metha-
nol steam reforming the salt coating acts not only in the form
of a chemical support modification but also as a fluid-side in-
duced modification of the catalytic platinum sites.
To verify our hypothesis of in situ aluminate formation in the
preparation of alkali hydroxide-coated catalysts, we prepared
mixtures of alumina and the corresponding alkali hydroxides in
stoichiometric ratios to induce complete aluminate formation.
These samples were heated to 4008C for 12 h and immediately
analyzed using MAS NMR spectroscopy to avoid contact with
moisture. The resulting data are shown in the Supporting In-
formation. Except for LiOH/alumina full conversion towards the
alkali aluminate species is reached under these conditions. In
the case of the LiOH-containing sample, full conversion to the
aluminate is most likely prevented by the relatively low solubil-
ity of LiOH in water (preparation as dispersion: alumina
powder in LiOH/water). All peak maximum positions of the
thus prepared aluminates are nearly equal to the ones found
for the alkali hydroxide-coated Pt/Al2O3 catalyst prior to steam
reforming reaction (see Figure 14).
During methanol steam reforming, the as-prepared hydrox-
ide-coated catalysts are in contact with water and methanol.
After the reaction, the catalyst samples were analyzed using
27Al MAS NMR. The results are summarized in Figure 15. These
NMR spectra indicate that except for the LiOH-coated catalyst
Conclusions
We have demonstrated a synthetically straightforward proce-
dure to drastically enhance the performance of heterogeneous
Pt/Al2O3 catalysts in methanol steam reforming. The procedure
is simple, robust, and economically attractive and thus of po-
tential technical relevance. Our spectroscopic findings indicate
that alkali doping, especially with potassium, plays an impor-
tant role in activation of platinum. In addition, hygroscopicity
and basicity of the applied molten salt contribute to the signif-
icant increase in catalytic activity and selectivity. We found evi-
dence that under reaction conditions an (at least partly) liquid
film of alkali hydroxide/alkali carbonate is formed on the cata-
lyst/alumina surface. This hydroxide/water film increases the
availability of water at the active catalyst sites. However, with
too much salt present, the resulting high liquid pore filling in-
troduces mass transfer impediments as evidenced by our ki-
netic studies. Thus, the best compromise between beneficial
catalyst modification and introduction of additional mass trans-
fer barriers is obtained at relatively low amounts of salt coat-
ings, typically at 5–10 wt% salt loading. Although in the dry
preparation of alkali hydroxide salts on Pt/Al2O3 evidence for
surface aluminate formation is found, this support modification
is not expected to play a major role during catalysis as in the
presence of water and methanol the aluminate hydrolyses and
no indication for surface aluminate is found after the reaction,
at least with the most active KOH coating.
Figure 15. 27Al solid-state MAS NMR measurements of Pt/Al2O3 coated with
alkali hydroxides after continuous methanol steam reforming reaction
(varied T=200–2308C, pH O =0.5 bar, tmean,reaction =80 h).
2
all indications for alkali aluminate peaks have disappeared. For
the uncoated Pt/Al2O3 reference catalyst no obvious change is
detectable between the catalyst before reaction and after op-
eration. Again, two peak maxima are visible at 7 and 64 ppm,
reflecting tetrahedrally and octahedrally coordinated aluminum
atoms with a ratio of 30 to 70. Interestingly and in contrast to
the situation before methanol steam reforming, the NaOH-,
KOH-, and CsOH-coated catalysts show no aluminate peak in
the MAS NMR spectra after methanol steam reforming. In addi-
tion, the ratio of tetrahedrally to octahedrally coordinated alu-
minum atoms has returned for all three catalysts to a 30:70
ratio. Only the NMR data for the LiOH-modified catalyst still
show a small aluminate signal maximum at 80 ppm with the
ratio tetrahedral to octahedral being 33:67. We take these re-
sults as strong indication that the sodium, potassium, or
cesium aluminate formed at the alumina surface during cata-
lyst preparation is hydrolyzed during methanol reforming. re-
sulting in alumina coated with the corresponding hydroxide,
hydrates thereof, or alkaline aqueous solution (in accordance
We anticipate that the modification of heterogeneous cata-
lysts by molten salts can be transferred to other industrially rel-
evant reactions in the future. Moreover, this SCILL approach
using molten salts opens a new way to a rational and cost-effi-
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2524

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
40 kHz. The reference spectrum was pristine alumina exposed to
the same treatment.
cient approach to optimize heterogeneous catalysts through
surface modification or co-adsorption effects.
CO chemisorption experiments
Experimental Section
CO chemisorption experiments were carried out under dynamic
conditions in a Micromeritics Autochem 2920. The catalyst samples
were heated to 3008C (10 Kminꢀ1, 30 min isothermal, helium at-
mosphere) prior to CO adsorption. CO was dosed to the sample
(T=408C) through a loop (V=500 mL), and the sagged CO was de-
tected by means of a TCD. For the calculation of dispersion D a ad-
sorption stoichiometry of 1:1 was supposed for all catalyst samples
(if not otherwise indicated). CO desorption was performed by heat-
ing the sample to 5008C (10 Kminꢀ1, 60 min isothermal, helium at-
mosphere), detection by means of a TCD.
Materials
Platinum on aluminum oxide was purchased from Alfa Aesar (LOT:
F02R004, precise platinum content=4.86 wt%). Lithium acetate,
potassium acetate, cesium acetate, potassium hydrogen carbonate,
and potassium carbonate were obtained from Sigma Aldrich with
a purity of 99.99% and dried prior to use/weighing (1208C,
vacuum, at least 2 h). Lithium hydroxide (Merck, >98%), sodium
hydroxide (Merck, >99%), potassium hydroxide (Merck, >85%,
rest H2O, K2CO3 <1%), and cesium hydroxide (Fluka, 95%, rest
H2O) were used as stock solution, the amount of hydroxide was
determined by titration with 1m HCl (Merck).
Diffusion limitation testing
The applied testing method for film diffusional influences is based
on literature methods.[28] Two methanol reforming experiments
were performed using two different masses of catalyst (1st run:
mcat., uncoated =200.7 mg; 2nd run: mcat., uncoated =401.4 mg). The meth-
anol inlet stream was adapted to the catalysts masses to realize
comparable modified residence times mcat./nMeOH, in. All other exper-
imental conditions were kept identical: T=2308C; catalyst loaded
Synthesis of salt-modified catalysts
The calculated amount of platinum on support was immersed into
a solution of the salt or salt mixture in high-purity water (typically
20 mL). After mixing for 30 min at 258C the solvent was removed
by means of a vacuum (558C, 80 mbar). The alkali hydroxide-
coated catalysts/samples were heated to 1508C under vacuum
(<0.1 mbar) for at least 4 h prior to the methanol steam reforming
experiments. The same procedure was applied prior to the CO
chemisorption and MAS NMR experiments.
with 17.15 wt% KOH; pabs =5 bar; pMeOH =pH O =0.5 bar; t=10–
2
40 s. The evaluation was based on methanol conversion.
Dynamic vapor sorption experiments
Catalytic experiments
The water adsorption isotherms of the alkali hydroxide-coated cat-
alysts were recorded by performing dynamic vapor sorption in
a DVS elevated temperature system (DVS-ET) from Surface Mea-
surement Systems. All measurements were performed in nitrogen
(V=200 mLminꢀ1). The adsorption isotherms were recorded at T=
408C with ultrapure water. Prior to adsorption the samples were
heated to T=3008C (25 to 1008C, 32.5 min; 1008C isothermal for
60 min; 100 to 3008C, 100 min; 3008C isothermal for 240 min; 300
to 258C, 90 min). Typically, a mass of 8–10 mg of catalyst was used.
The catalyst performance in methanol steam reforming was evalu-
ated in a continuously operated gas-phase fixed-bed reactor similar
to the one described elsewhere[33] (details are found in the Sup-
porting Information). An equimolar mixture of methanol and water
was evaporated and fed to the reactor. At the reactor outlet, un-
converted methanol and water were condensed and the product
gas was analyzed by GC (Varian CP 4900). Catalyst activities are
provided as TOF, which is the total molar flow of carbon monoxide,
carbon dioxide, and methane divided by the total molar amount
of platinum in the reactor (typically 0.1 mmol). SCO is given as the
2
Solid-state 27Al MAS NMR experiments
CO2 mol fraction in the outlet gas stream divided by the sum of
CO2, CO, and CH4. The mass balance was closed by the quantifica-
tion of the inert gas nitrogen.
All 1D single-pulse 27Al solid-state MAS NMR spectra were recorded
at room temperature on an Agilent DD2 500WB spectrometer at
a resonance frequency of 130.24 MHz, using a sample spinning
rate of 15 kHz. The powder samples were packed into 3.2 mm zir-
conia rotors equipped with a Torlon spacer and caps. 2000 scans
were accumulated for qualitative spectra using a 2 ms 908 pulse
and a 1 s recycle delay. The chemical shifts were referenced accord-
ing to IUPAC guidelines.
DRIFTS experiments
The catalyst characterization was performed in a Bruker Vertex 80v
infrared spectrometer equipped with a Praying Mantis and a High
Temperature Reaction Chamber (HVC-DRP-4) from Harrick. An ex-
tension with all necessary feedthroughs was adjoined to the
sample chamber of the spectrometer to allow the evacuation of
the optical path. Mass flows and pressures were adjusted using
Bronkhorst mass flow and pressure controllers. Prior to CO adsorp-
tion, the catalyst powder was heated under argon flow (Linde,
>99.9999%, 10 mLN minꢀ1, 1 bar) at 3008C for 30 min to desorb
water and other contaminations. After exposure to CO (Linde,
>99.997%, 10 mLN minꢀ1) at 358C for 10 min, the reactor was
purged thoroughly with Ar for 60 min until no CO gas phase signal
could be detected anymore. The IR spectra were recorded with
a spectral resolution of 2 cmꢀ1, 1024 scans, and a scan speed of
Acknowledgements
The authors acknowledge financial support by the Deutsche For-
schungsgemeinschaft (DFG) within the Excellence Cluster “Engi-
neering of Advanced Materials” in the framework of the excel-
lence initiative. M.K., F.A., N.N.B., and P.W. would like to thank
the EU for support through its ERC Advanced Investigator Grant
No. 267376. Furthermore, A.K., M.L., and J.L. acknowledge addi-
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2525

CHEMSUSCHEM
FULL PAPERS
www.chemsuschem.org
[16] B. Liu, T. Huang, Z. Zhang, Z. Wang, Y. Zhang, J. Li, Catal. Sci. Technol.
2014, 4, 1286–1292.
[17] B. W. Krupay, Y. Amenomiya, J. Catal. 1981, 67, 362–370.
[18] a) N. R. Avery, Appl. Surf. Sci. 1982, 13, 171–179; b) B. E. Heyden, A. M.
Bradshaw, Surf. Sci. 1983, 125, 787–802; c) C. W. Olsen, R. I. Masel, Surf.
Sci. 1988, 201, 444–460.
[19] a) P. Hollins, Surf. Sci. Rep. 1992, 16, 51–94; b) F. M. Hoffmann, Surf. Sci.
Rep. 1983, 3, 107–192.
[20] H. P. Bonzel, Surf. Sci. Rep. 1988, 8, 43–125.
[21] R. K. Herz, D. F. McCready, J. Catal. 1983, 81, 358–368.
[22] a) V. Perrichon, L. Retailleau, P. Bazin, M. Daturi, J. C. Lavaelly, Appl. Catal.
A 2004, 260, 1–8; b) A. Renouprez, C. Hoang-Van, P. A. Compagnon, J.
Catal. 1974, 34, 411–422; c) H. Matsuhashi, S. Nishiyama, H. Miura, K.
Eguchi, K. Hasegawa, Y. Iizuka, A. Igarashi, N. Katada, J. Kobayashi, T.
Kubota, T. Mori, K. Nakai, N. Okazaki, M. Sugioka, T. Umeki, Y. Yazawa, D.
Lu, Appl. Catal. A 2004, 272, 329–338.
[23] K. Foger, J. R. Anderson, Appl. Surf. Sci. 1979, 2, 335–351.
[24] W. M. Vogel, K. J. Routsis, V. J. Kehrer, D. A. Landsman, J. G. Tschinkel, J.
Chem. Eng. Data 1967, 12, 465–471.
tional support by the Fonds der Chemischen Industrie, DAAD,
and the COST Action CM1104.
Keywords: catalyst characterization · heterogeneous catalysis ·
methanol reforming · molten salts · platinum
[1] J. Agrell, B. Lindstrçm, L. J. Pettersson, S. G. Jꢂras, Catalysis 2002, 16,
67–132.
[2] G. A. Olah, A. Goeppert, G. K. S. Prakash, Beyond Oil and Gas. The Metha-
nol Economy, Wiley-VCH, Weinheim, 2009.
[3] C. Wannek in Hydrogen Energy (Ed.: D. Stolten), Wiley-VCH, Weinheim,
2010, pp. 17–40.
[4] D. R. Palo, R. A. Dagle, J. D. Holladay, Chem. Rev. 2007, 107, 3992–4021.
[5] S. Sꢃ, H. Silva, L. Brand¼o, J. M. Sousa, A. Mendes, Appl. Catal. B 2010,
99, 43–47.
[6] M. Kusche, F. Enzenberger, S. Bajus, H. Niedermeyer, A. Bçsmann, A.
Kaftan, M. Laurin, J. Libuda, P. Wasserscheid, Angew. Chem. Int. Ed. 2013,
52, 5028–5032; Angew. Chem. 2013, 125, 5132–5136.
[25] E. Lang, Hooker Chemical Co., 1949.
[7] V. A. Cocalia, A. E. Visser, R. D. Rogers, J. D. Holbrey in Ionic Liquids in
Synthesis (Eds.: P. Wasserscheid, T. Welton), Wiley-VCH, Weinheim, 2008,
pp. 89–102.
[8] U. Kernchen, B. Etzold, W. Korth, A. Jess, Chem. Eng. Technol. 2007, 30,
985–994.
[26] D. R. Lide in Handbook of Chemistry and Physics, Internet Version 2005,
CRC Press, Boca Raton, FL, 2005, 1351–1359.
[27] R. Hoppe, H.-P. Mꢄller, Solid State Ionics 1990, 43, 23–30.
[28] J. Hagen in Chemische Reaktionstechnik (Ed.: V. Hopp), Wiley-VCH, Wein-
heim, 1992, pp. 83–89.
[9] a) J. Arras, M. Steffan, Y. Shayeghi, D. Ruppert, P. Claus, Green Chem.
2009, 11, 716–723; b) J. Arras, E. Paki, C. Roth, J. Radnik, M. Lucas, P.
Claus, J. Phys. Chem. C 2010, 114, 10520–10526.
[10] a) M. Sobota, M. Happel, M. Amende, N. Paape, P. Wasserscheid, M.
Laurin, J. Libuda, Adv. Mater. 2011, 23, 2617–2621; b) H.-P. Steinrꢄck, J.
Libuda, P. Wasserscheid, T. Cremer, C. Kolbeck, M. Laurin, F. Maier, M.
Sobota, P. S. Schulz, M. Stark, Adv. Mater. 2011, 23, 2571–2587.
[11] N. Taccardi, D. Assenbaum, M. E. M. Berger, A. Bçsmann, F. Enzenberger,
R. Wçlfel, S. Neuendorf, V. Gçke, N. Schrçdel, H.-J. Maass, H. Kistenmach-
er, P. Wasserscheid, Green Chem. 2010, 12, 1150–1156.
[12] G. G. Diogenov, G. S. Sergeeva, Zh. Neorg. Khim. 1965, 10, 292–294.
[13] a) M. Haukka, T. Venꢂlꢂinen, M. Kallinen, T. A. Pakkanen, J. Mol. Catal. A
1998, 136, 127–134; b) Y. Zhai, D. Pierre, R. Si, W. Deng, P. Ferrin, A. U.
Nnilekar, G. Peng, J. A. Herron, D. C. Bell, H. Saltsburg, M. Mavrikakis, M.
Flytzani-Stephanopoulos, Science 2010, 329, 1633–1636.
[14] W. D. Mross, Catal. Rev. Sci. Eng. 1983, 25, 591–637.
[15] D. A. Bulushev, L. Jia, S. Beloshapkin, J. R. H. Ross, Chem. Commun. 2012,
48, 4184–4186.
[29] M.-H. Lee, C.-F. Cheng, V. Heine, J. Klinowski, Chem. Phys. Lett. 1997,
265, 673–676.
[30] a) D. Mꢄller, W. Gessner, A. Samoson, E. Lippma, G. Scheler, J. Chem. Soc.
Dalton Trans. 1986, 6, 1277–1281; b) D. Mꢄller, W. Gessner, H-J. Behrens,
G. Scheler, Chem. Phys. Lett. 1981, 79, 59–62.
[31] a) Y. Zhang, Y. Li, Y. Zhang, J. Chem. Eng. Data 2003, 48, 617–620; b) S.
Ma, S. Zheng, Y. Zhang, J. Chem. Eng. Data 2007, 52, 77–79.
[32] Y. Zhang, S. Zheng, H. Du, S. Wang, Y. Zhang, J. Chem. Eng. Data 2010,
55, 1237–1240.
[33] S. Werner, N. Szesni, A. Bittermann, M. J. Schneider, P. Hꢂrter, M. Hau-
mann, P. Wasserscheid, Appl. Catal. A 2010, 377, 70–75.
Received: April 28, 2014
Revised: June 12, 2014
Published online on August 14, 2014
ꢁ 2014 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
ChemSusChem 2014, 7, 2516 – 2526 2526