Hydrogen production from decalin dehydrogenation over Pt-Ni/C bimetallic catalysts

Article abstract of DOI:10.1016/S1872-2067(14)60178-9

Pt-Ni bimetallic catalysts and the corresponding monometallic Pt catalysts supported on active carbon were prepared by incipient wetness impregnation and characterized by X-ray diffraction, N₂ adsorption, and NH₃-temperature programmed desorption. Their activities for decalin dehydrogenation were investigated at a superheated liquid film state in a batch reactor. The effects of temperature, impregnation sequence, and Pt/Ni molar ratio on the dehydrogenation activity and the naphthalene yield were investigated. The results show that the Pt-Ni bimetallic catalyst significantly enhanced hydrogen evolution compared with either Ni or Pt monometallic catalyst. The highest dehydrogenation conversion and naphthalene yield were obtained when the Pt/Ni molar ratio was 1:1 and Pt was impregnated first. The experimental results were correlated with density functional theory calculations of hydrogen binding energy (HBE) on different catalytic surfaces. The correlation confirmed that bimetallic surfaces with stronger HBEs had higher dehydrogenation activities.

Full text of DOI:10.1016/S1872-2067(14)60178-9

Chinese Journal of Catalysis 35 (2014) 1833–1839
ava i l a b l e a t w w w. s c i e n c ed i r e c t . c o m
j o u r n a l h o m e p a g e : w w w. e l s e v i e r. c o m / l o c a t e /c h n j c
Article
Hydrogen production from decalin dehydrogenation over Pt‐Ni/C
bimetallic catalysts
Suitao Qi*, Yingying Li, Jiaqi Yue, Hao Chen, Chunhai Yi, Bolun Yang
School of Chemical Engineering and Technology, Xi’an Jiaotong University, Xi’an 710049, Shaanxi, China
A R T I C L E I N F O
A B S T R A C T
Article history:
Pt‐Ni bimetallic catalysts and the corresponding monometallic Pt catalysts supported on active
carbon were prepared by incipient wetness impregnation and characterized by X‐ray diffraction, N2
adsorption, and NH3‐temperature programmed desorption. Their activities for decalin dehydro‐
genation were investigated at a superheated liquid film state in a batch reactor. The effects of tem‐
perature, impregnation sequence, and Pt/Ni molar ratio on the dehydrogenation activity and the
naphthalene yield were investigated. The results show that the Pt‐Ni bimetallic catalyst significantly
enhanced hydrogen evolution compared with either Ni or Pt monometallic catalyst. The highest
dehydrogenation conversion and naphthalene yield were obtained when the Pt/Ni molar ratio was
1:1 and Pt was impregnated first. The experimental results were correlated with density functional
theory calculations of hydrogen binding energy (HBE) on different catalytic surfaces. The correla‐
tion confirmed that bimetallic surfaces with stronger HBEs had higher dehydrogenation activities.
© 2014, Dalian Institute of Chemical Physics, Chinese Academy of Sciences.
Received 6 April 2014
Accepted 23 May 2014
Published 20 November 2014
Keywords:
Platinum
Nickel
Bimetallic
Decalin
Dehydrogenation
Density functional theory
Published by Elsevier B.V. All rights reserved.
1. Introduction
drogenation process [14–21]. It is well known that the decalin
dehydrogenation reaction is an endothermic reaction. Higher
Hydrogen as a clean energy carrier has good prospects in
hydrogen fuel cells and alternative energy sources. However,
the key to using hydrogen on a large scale lies in its storage,
transportation, and distribution [1,2]. Some cyclic hydrocar‐
bons such as decalin, tetralin, and cyclohexane are receiving an
increasing amount of attention as organic liquid hydrogen
storage materials [3–13]. Their hydrogenation and dehydro‐
genation cycles offer the possibility of using these molecules as
hydrogen storage media because of their high hydrogen stor‐
age density and convenient transportation.
temperatures would be favorable for dehydrogenation, but the
selectivity toward naphthalene would decrease because of side
effects such as hydrogenolysis or coking at high temperatures.
These side reactions would hinder the reversible cycle of hy‐
drogen storage and release.
Bimetallic catalysts [22–24], which often show distinctly
different electronic and chemical properties from those of the
parent metals, offer the opportunity to design new catalytic
materials with enhanced activity, selectivity, and stability. Ka‐
riya et al. [7] reported that Pt‐Re, Pt‐Pd, and Pt‐Rh catalyzed
cycloalkane dehydrogenation better than Pt monometallic cat‐
alysts. However, high cost prohibits widespread use of noble
metal catalysts, so some metal oxide catalysts have been inves‐
tigated in the dehydrogenation reaction [25].
Among all the liquid organic hydrides, decalin is one of the
best candidates because of its excellent hydrogen storage den‐
sity of 7.2 wt%. Moreover, decalin is an environmentally
friendly hydrogen carrier with zero CO2 emission in the dehy‐
*Corresponding author. Tel: +86‐29‐82663189; E‐mail: suitaoqi@mail.xjtu.edu.cn
This work was supported by the National Natural Science Foundation of China (21006076), the Specialized Research Fund for the Doctoral Program
of Higher Education, China (20110201130002), and the Fundamental Research Funds for the Central Universities, China (xjj2011062).
DOI: 10.1016/S1872‐2067(14)60178‐9 | http://www.sciencedirect.com/science/journal/18722067 | Chin. J. Catal., Vol. 35, No. 11, November 2014

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Suitao Qi et al. / Chinese Journal of Catalysis 35 (2014) 1833–1839
In our previous work, the Pt‐Ni bimetallic catalyst was iden‐
the different catalysts were measured by N2 adsorption‐de‐
sorption at liquid nitrogen temperature using a Beckman Coul‐
ter Sorption Analysis 3100 Plus instrument. Powder X‐ray dif‐
fraction (XRD) patterns of various catalysts were recorded with
a Rigaku D/Max‐2400 X‐ray diffractometer using Cu Kα radia‐
tion with a scanning angle (2θ) range of 5°–80°, operated at 36
kV and 80 mA. NH3‐temperature programmed desorption
(NH3‐TPD) tests were performed to determine the catalyst
surface acidity. In a U‐shaped tubular quartz reactor heated by
an electric furnace, 0.1 g sample was pretreated in flowing He
(99.99%, 30 mL/min) at 400 °C for 0.5 h, followed by NH3 sat‐
urated adsorption at 30 °C, and then flushed with flowing He at
the same temperature for 1 h. NH3‐TPD experiments were per‐
formed using a temperature ramp from 30 to 600 °C at 10
°C/min using a thermal conductivity detector.
tified as an active catalyst toward low‐temperature hydrogena‐
tion and dehydrogenation of cycloalkenes including cyclohex‐
ene, 1,3‐cyclohexadiene, and 1,4‐cyclohexadiene [26–28]. Both
experimental and theoretical investigations have revealed that
for the Pt‐Ni bimetallic catalyst, the formation of a subsurface
Pt‐Ni‐Pt structure with an atomic layer of Ni underneath the
surface Pt atoms is responsible for the higher hydrogenation
activity than the corresponding monometallic surfaces. In con‐
trast, a surface bimetallic structure, Ni‐Pt‐Pt, with a layer of Ni
residing on top of the Pt substrate, binds adsorbates more
strongly than either the Pt or Ni surfaces alone [29,30]. The
strong binding on the Ni‐Pt‐Pt surface structure leads to facile
production of hydrogen from the dehydrogenation of cycloal‐
kenes, oxygenates [31], and ammonia [32].
This work extends the previous surface science results to
supported Pt‐Ni bimetallic catalysts prepared by the incipient
wetness impregnation method. Decalin dehydrogenation was
selected as a probe reaction to demonstrate the enhanced de‐
hydrogenation activity on the bimetallic catalysts. The dehy‐
drogenation activity of the Pt‐Ni/C bimetallic catalyst was
compared with those of the corresponding monometallic Pt
and Ni catalysts. It was found that supported Pt‐Ni bimetallic
catalysts exhibited much better performance than either of the
monometallic catalysts. On the other hand, for the Pt‐Ni bime‐
tallic catalyst, an effect of the impregnation sequence was ob‐
served and discussed. In addition, the catalytic activity and
hydrogen binding energy (HBE) on different Pt‐Ni surfaces
from density functional theory (DFT) calculations were shown
to be correlated [33,34].
2.3. Catalyst evaluation
The catalytic activities of different catalysts for decalin de‐
hydrogenation were evaluated using a batch reactor. The batch
reactor consisted of a three‐necked flat‐bottomed flask of 100
mL capacity, fitted with a condenser in the central opening. A
sampling device and a thermocouple were fitted in the other
two openings. The reaction temperature was maintained by an
electric furnace equipped with a temperature controller.
In a typical run, 0.3 g catalyst was added into the bottom of
the flask and reduced with H2 for 1 h at the reaction tempera‐
ture, and then the reactor was flushed with flowing N2 for 0.5 h
to remove residual H2. Thereafter, 1 mL decalin (6.48 mmol)
was added to the reactor, and the reaction started and was
allowed to proceed for 0.5 h. During the reaction, the continu‐
ous vaporization‐condensation reflux of decalin ensured the
formation of a decalin liquid film on the catalyst surface, which
remained covered by the decalin liquid film. The temperature
of the catalyst surface was higher than the boiling point of de‐
calin, which was in an overheated state. The evolving H2 was
collected and measured by the water drainage method. After
the reaction, the contents remaining in the flask were dissolved
with n‐hexane. The dissolved mixture was collected and sepa‐
rated by centrifugation to remove the catalyst particles com‐
pletely, and then analyzed by a HP‐4890D gas chromatograph
equipped with a flame ionization detector. The yield of naph‐
thalene was calculated by dividing the moles of naphthalene
actually obtained by the moles of naphthalene theoretically
obtained.
2. Experimental
2.1. Catalyst preparation
A series of Ni or Pt catalysts were prepared by the incipient
wetness impregnation method. Ni(NO3)2·6H2O (AR, Tianjin
Chemical Reagent Research Institute, China) or chloroplatinic
acid (AR) was selected as the source of active metal and im‐
pregnated into active carbon (C). The Pt‐Ni bimetallic catalysts
were prepared by sequential impregnation and co‐impregna‐
tion. After impregnation, the different precursors were dried at
110 °C for 2 h and then calcined in N2 atmosphere at 400 °C for
1
h. The different bimetallic catalysts are denoted
1Pt‐1Ni/C(CI), 1Pt‐1Ni/C, and 1Ni‐1Pt/C. Pt‐Ni/C(CI) means
that the catalyst was prepared by Pt and Ni co‐impregnation.
Pt‐Ni/C means that Ni was impregnated first, while Ni‐Pt/C
means that Pt was impregnated first. 1Pt‐1Ni indicates that the
atomic ratio of Pt to Ni was 1:1. Other Pt‐Ni bimetallic catalysts
with different Pt/Ni ratios were also prepared for comparisons
to the 1Pt‐1Ni catalysts. They are denoted 0.5Ni‐1Pt/C,
2Ni‐1Pt/C, 4Ni‐1Pt/C, and 8Ni‐1Pt/C. Pt loadings of all catalysts
were 3 wt%.
3. Results and discussion
Table 1 lists the surface area and average pore diameter of
the different catalysts. The addition of metal leads to a small
decrease in the catalyst surface area, which indicates that metal
species on the support might migrate into internal channels
after calcination. The surface area of the Pt‐Ni bimetallic cata‐
lysts decreases with increasing Ni content, following the order
1Ni‐1Pt/C > 1Pt‐1Ni/C(CI) > 1Pt‐1Ni/C. For the decalin dehy‐
drogenation reaction, smaller pore sizes can prevent diffusion
of the intermediate product tetralin and help tetralin further
2.2. Catalyst characterization
The specific surface area and pore volume measurements of

Suitao Qi et al. / Chinese Journal of Catalysis 35 (2014) 1833–1839
1835
80
Table 1
Surface area and average pore diameter of different catalyst samples.
70
60
50
40
30
20
Surface area
(m2/g)
407
Average pore diameter
Catalyst
(nm)
8.6
9.7
10.3
11.0
9.2
(2)
C
Pt/C
360
340
318
379
373
366
1Pt‐1Ni/C(CI)
1Pt‐1Ni/C
0.5Ni‐1Pt/C
1Ni‐1Pt/C
2Ni‐1Pt/C
(1)
9.4
9.5
100
200
300
400
500
600
T/oC
convert to naphthalene, which is favorable for dehydrogenation
selectivity.
Fig. 2. NH3‐TPD profiles of Pt/C (1) and 1Ni‐1Pt/C (2) catalysts.
The Pt diffraction peaks are clearly seen in Fig. 1, indicating
that the Pt species were in a good crystaline form and well dis‐
persed on the support surface. The impregnation sequence has
a slight impact on the particle dispersion of the bimetallic cata‐
lysts. The Pt diffraction peaks of the 1Ni‐1Pt/C catalyst are
slightly broader than those of the other two catalysts, especially
at 2θ = 40°. With increases in the Ni/Pt ratio, the Pt diffraction
peaks decrease in size, while the Ni diffraction peaks can be
seen to become sharper (Fig. 1(b)). The metal particle size of
the supported metal catalyst is correlated with the width of the
corresponding diffraction peak. The Pt particle size decreases
as the diffraction peak broadens. This implies that the addition
of Ni promotes dispersion of Pt. However, too high Ni loading
leads to aggregation of Ni particles.
quantify the acidity of the sample. Comparing the Pt/C catalyst
with the 1Ni‐1Pt/C catalyst, the amounts of desorbed NH3 are
similar. However, the peak position of the 1Ni‐1Pt/C catalyst
shifts to higher temperatures than that of the Pt/C catalyst. This
implies an increase in the strength of acid sites, which is sug‐
gested to be associated with the interaction of Ni and Pt. The
1Ni‐1Pt/C catalyst shows better dehydrogenation activity, in‐
dicating that the slight increase of the number of acid centers
has a positive effect on the catalytic dehydrogenation activity.
Figure 3 is the product distribution of decalin dehydrogena‐
tion over the Pt/C catalyst at different temperatures when the
decalin feedstock was 1 mL. At this point the catalyst surface
was at an overheated liquid film state, having a higher temper‐
ature and larger contact area. The results show that the yield
for naphthalene keeps increasing from 230 to 290 °C, while the
amount of the intermediate product tetralin remains at nearly
the same level over this range. This indicates that high temper‐
atures favor the further dehydrogenation of tetralin.
Figure 2 shows the NH3‐TPD profiles of Pt and Pt‐Ni cata‐
lysts. Both spectra exhibit a single characteristic peak. Normal‐
ly, the area of a specific peak corresponds to the amount of NH3
desorbed from the sample, and it can be taken as a standard to
Figure 4 shows the dehydrogenation behavior of decalin
over Pt‐based catalysts at 290 °C in a batch reactor. The dehy‐
drogenation of decalin over the 1 wt% Ni/C catalyst was also
examined, and the catalytic activity for this sample was nearly
zero. The naphthalene yields over Pt‐Ni/C bimetallic catalysts
were much higher than that obtained over Ni/C or Pt/C mon‐
ometallic catalysts. On the other hand, both catalytic activity
and naphthalene yield over the Pt‐Ni catalysts were influenced
Pt
Ni
(a)
1Pt-1Ni/C
1Pt-1Ni/C(CI)
1Ni-1Pt/C
6
Residual decalin
Naphthalene
Tetralin
(b)
5
4
3
2
1
0
8Ni-1Pt/C
4Ni-1Pt/C
2Ni-1Pt/C
0.5Ni-1Pt/C
10
20
30
40
50
60
70
80
2/(o )
220 230 240 250 260 270 280 290 300
T/oC
Fig. 1. XRD patterns of carbon supported Pt‐Ni bimetallic catalysts
prepared by various impregnation sequences (a) and various Pt/Ni
molar ratios (b).
Fig. 3. Effect of temperature on decalin dehydrogenation over the Pt/C
catalyst.

1836
Suitao Qi et al. / Chinese Journal of Catalysis 35 (2014) 1833–1839
100
80
60
40
20
0
Table 2
Tetralin yield
Naphthalene yield
Decalin conversion
Hydrogen binding energies (HBE) on Pt(111), Ni(111), and Ni/Pt(111)
surface as predicted by DFT.
Surface
Pt(111)
Ni‐Pt‐Pt(111)
Pt‐Ni‐Pt(111)
HBE (kJ/mol)
–267.3
–285.6
–238.3
drogenation. Table 2 shows the DFT results of HBE on the
closed‐packed Pt(111) surface, the Ni‐Pt‐Pt(111) surface with a
monolayer of Ni residing on top of Pt(111), and the subsurface
Pt‐Ni‐Pt(111) configuration with one monolayer of Ni between
the first and second layers of Pt. The DFT calculations were
performed using the Vienna ab‐initio simulations package
(VASP) with spin polarization. The Generalized Gradient Ap‐
proximation with Perdew Burke Ernzerhof (GGA‐PBE) ex‐
change‐correlation functional was used. A 3×3 slab with four
metal layers was used to model the adsorption of atomic hy‐
drogen (one adsorbate per unit cell). The top two layers were
allowed to relax to the lowest energy configuration while the
bottom two layers were fixed at a bulk Pt–Pt bond length as
previously described in detail [28,29]. A 3×3×1 Monk‐
horst‐Pack K‐point grid mesh was used to determine the elec‐
tronic energies.
That the HBE is higher on the Ni‐Pt‐Pt(111) surface than on
either the Pt(111) or Pt‐Ni‐Pt(111) surfaces suggests that the
Ni‐Pt‐Pt surface structure should be more thermodynamically
favored than the other two surfaces for the dehydrogenation
reaction. Although more detailed experimental studies are
needed in regards to controllable syntheses of bimetallic cata‐
lysts, it is clear that the presence of the Ni‐Pt‐Pt structure is
responsible for the higher dehydrogenation activity on the
1Ni‐1Pt/C bimetallic catalyst when compared with the mono‐
metallic catalysts and the other two bimetallic catalysts.
1Ni-1Pt/C 1Pt-1Ni/C(CI) 1Pt-1Ni/C
Catalyst
1Pt/C
Fig. 4. Decalin dehydrogenation over different Pt‐based catalysts in a
batch reactor. Reaction conditions: 290 °C, decalin 1 mL, catalyst 0.3 g,
0.5 h.
by the impregnation sequence; they followed the order of
1Ni‐1Pt/C > 1Pt‐1Ni/C(CI) > 1Pt‐1Ni/C. The 1Ni‐1Pt/C catalyst,
which has Ni residing on top of the Pt substrate, has the best
catalytic activity, which is consistent with the DFT results (dis‐
cussed below). It is most likely that Pt deposited first would
remain outside the support and further prevent subsequently
deposited Ni from entering the inter cavities of the support,
facilitating the formation of the Pt–Ni bond [30,33].
The dehydrogenation activities of decalin over bimetallic
catalysts with different Pt/Ni molar ratios were discussed in
light of Fig. 5. The yield for naphthalene first increased and
then decreased with the addition of Ni, while the byproduct
tetralin remained nearly unchanged after the Pt/Ni ratio ex‐
ceeded 0.5. The 1Ni‐1Pt/C catalyst exhibited the best activity
and naphthalene yield; its enhanced catalytic activity likely
benefits from the formation of the Pt‐Ni bimetallic bonds.
However, excessive Ni atoms may block the Pt active sites and
lead to a decline of the catalytic activity.
4. Conclusions
In previous work, the hydrogenation activity of Pt‐Ni bime‐
tallic catalysts has been correlated to weaker HBEs on bimetal‐
lic surfaces [28,30]. Herein, DFT calculations were performed
to explore whether such correlation can be extended to dehy‐
The catalytic dehydrogenation of decalin was investigated
using a combination of experimental methods and DFT calcula‐
tions. Supported Pt‐Ni bimetallic and Ni and Pt monometallic
catalysts on active carbon were prepared by incipient wetness
impregnation and evaluated using a batch reactor for decalin
dehydrogenation. The results showed that Pt‐Ni bimetallic cat‐
alysts had higher dehydrogenation activities than the corre‐
sponding monometallic catalysts. The 1Ni‐1Pt/C bimetallic
catalyst exhibited the highest activity among all the prepared
catalysts toward decalin hydrogenation, which was mostly
attributed to the Pt‐Ni bimetallic formation. The observed
highest activity over 1Ni‐1Pt/C agrees well with DFT results,
which predict that the Ni‐Pt‐Pt(111) surface structures bind
hydrogen more strongly than Pt(111) and Pt‐Ni‐Pt(111).
5
4
3
2
1
0
Naphthalene
Tetralin
Acknowledgments
0.0
0.5
1.0
1.5
2.0
Pt/Ni molar ratio
We would like to acknowledge the technical assistance on
computing platform from Professor Xiangdong Ding's Group at
Xi'an Jiaotong University.
Fig. 5. Effect of the Pt/Ni ratio on product yield of decalin dehydro‐
genation over Ni‐Pt/C catalysts. Reaction conditions: 290 °C, decalin 1
mL, catalyst 0.3 g, Pt first impregnated, 0.5 h.

Suitao Qi et al. / Chinese Journal of Catalysis 35 (2014) 1833–1839
1837
Graphical Abstract
Chin. J. Catal., 2014, 35: 1833–1839 doi: 10.1016/S1872‐2067(14)60178‐9
Hydrogen production from decalin dehydrogenation over Pt‐Ni/C bimetallic
catalysts
Suitao Qi*, Yingying Li, Jiaqi Yue, Hao Chen, Chunhai Yi, Bolun Yang
Xi’an Jiaotong University
The correlation of experimental results with density functional theory calculations
confirmed that bimetallic surfaces with stronger hydrogen binding energies exhibited
higher dehydrogenation activity for decalin.
[19] Suttisawat Y, Horikoshi S, Sakai H, Abe M. Int J Hydrogen Energy,
2010, 35: 6179
References
[20] Yolcular S, Olgun Ö. Catal Today, 2008, 138: 198
[21] Nagaraja B M, Shin C H, Jung K D. Appl Catal A, 2013, 467: 211
[22] Patil S P, Pande J V, Biniwale R B. Int J Hydrogen Energy, 2013, 38:
15233
[23] Alhumaidan F, Tsakiris D, Cresswell D, Garforth A. Int J Hydrogen
Energy, 2013, 38: 14010
[1] Eberle U, Felderhoff M, Schüth F. Angew Chem Int Ed, 2009, 48:
6608
[2] David E. J Mater Process Technol, 2005, 162‐163: 169
[3] Biniwale R B, Rayalu S, Devott S, Ichikawa M. Int J Hydrogen Ener‐
gy, 2008, 33: 360
[4] Zhu G L, Yang B L. Progr Chem, 2009, 21: 2760
[5] Ninomiya W, Tanabe Y, Sotowa K I, Yasukawa T, Sugiyama S. Res
Chem Intermed, 2008, 34: 663
[24] Aboul‐Fotouh S M K, Aboul‐Gheit N A K. Chin J Catal, 2012, 33:
697
[6] Pande J V, Shukla A, Biniwale R B. Int J Hydrogen Energy, 2012, 37:
6756
[7] Kariya N, Fukuoka A, Ichikawa M. Appl Catal A, 2002, 233: 91
[8] Saito Y, Aramaki K, Hodoshima S, Saito M, Shono A, Kuwano J,
Otake K. Chem Eng Sci, 2008, 63: 4935
[9] Wang Y G, Shah N, Huffman G P. Energy Fuels, 2004, 18: 1429
[10] Tien P D, Satoh T, Miura M, Nomura M. Fuel Process Technol, 2008,
89: 415
[11] Du J P, Zhao R H, Jiao G R. Int J Hydrogen Energy, 2013, 38: 5789
[12] Chen A B, Zhang W P, Li X Y, Tan D L, Han X W, Bao X H. Catal Lett,
2007, 119: 159
[13] Shukla A A, Gosavi P V, Pande J V, Kumar V P, Chary K V R, Bi‐
niwale R B. Int J Hydrogen Energy, 2010, 35: 4020
[14] Shinohara C, Kawakami S, Moriga T, Hayashi H, Hodoshima S,
Saito Y, Sugiyama S. Appl Catal A, 2004, 266: 251
[15] Tien P D, Satoh T, Miura M, Nomura M. Energy Fuels, 2005, 19: 731
[16] Tien P D, Satoh T, Miura M, Nomura M. Energy Fuels, 2005, 19:
2110
[25] Gao X F, Chen C L, Ren S Y, Zhang J, Su D S. Chin J Catal, 2012, 33:
1069
[26] Biniwale R B, Kariya N, Ichikawa M. Catal Lett, 2005, 105: 83
[27] Qi S T, Yu W T, Lonergan W W, Yang B L, Chen J G. Chin J Catal,
2010, 31: 955
[28] Qi S T, Yu W T, Lonergan W W, Yang B L, Chen J G. ChemCatChem,
2010, 2: 625
[29] Chen J G, Qi S T, Humbert M P, Menning C A, Zhu Y X. Acta
Phys‐Chim Sin, 2010, 26: 869
[30] Chen J G, Menning C A, Zellner M B. Surf Sci Rep, 2008, 63: 201
[31] Skoplyak O, Barteau M A, Chen J G. ChemSusChem, 2008, 1: 524
[32] Hansgen D A, Vlachos D G, Chen J G. Nat Chem, 2010, 2: 484
[33] Shu Y Y, Murillo L E, Bosco J P, Huang W, Frenkel A I, Chen J G. Appl
Catal A, 2008, 339: 169
[34] Lima F H B, Zhang J, Shao M H, Sasaki K, Vukmirovic M B, Ticianelli
E A, Adzic R R. J Phys Chem C, 2007, 111: 404
Page numbers refer to the contents in the print version, which include
both the English and Chinese versions of the paper. The online version
only has the English version. The pages with the Chinese version are only
available in the print version.
[17] Wang Y G, Shah N, Huggins F E, Huffman G P. Energy Fuels, 2006,
20: 2612
[18] Jiang N Z, Rao K S R, Jin M J, Park S E. Appl Catal A, 2012, 425‐426:
62