Click here to load reader
Upload
teza-nur-firlyansyah
View
215
Download
0
Embed Size (px)
Citation preview
8/9/2019 1-s2.0-S0360319915003377-main
http://slidepdf.com/reader/full/1-s20-s0360319915003377-main 1/7
The microstructure and stability of a Ni-nano-CaO/
Al2O3 reforming catalyst under
carbonationecalcination cycling conditions
Xiaochong Xue a, Sufang Wu a,b,*
a College of Chemical and Biological Engineering, Zhejiang University, Hangzhou 310027, Zhejiang, Chinab Key Laboratory of Biomass Chemical Engineering, Zhejiang University, Hangzhou 310027, Zhejiang, China
a r t i c l e i n f o
Article history:
Received 27 May 2014
Received in revised form
14 November 2014
Accepted 5 February 2015
Available online 20 March 2015
Keywords:
Hydrogen
Steam methane reforming
CatalystCarbonationecalcination cycles
Calcium aluminate
Stability
a b s t r a c t
The paper investigated the effect of carbonationecalcination cycling conditions on the
microstructure and CO2 sorption property of a sorption complex catalyst. The carbonation
operation condition consisted of temperature of 600 C with 20% CO2e80% N2 and 20% CO2
e80% steam atmosphere to simulate the methane reforming reaction conditions; the
calcination condition was 800 C with 100% N2. The BrunauereEmmereTeller (BET) surface
area and thermogravimetric analysis (TGA) were measured to investigate the microstruc-
ture and variation in sorption property of the catalyst after multiple cycles under each
condition. Results showed that the microstructure and CO2 sorption capacity of the sorp-
tion complex catalyst decayed significantly in the initial carbonationecalcination cycles,
especially under a steam atmosphere. X-ray diffraction analysis revealed that a stable
compound Ca12Al14O33 formed gradually during the initial carbonatione
calcination cycleseven at a temperature of 800 C. A model is proposed to explain the observed effect of
carbonationecalcination cycling on Ca12Al14O33 formation. Furthermore, based on our
findings, a new sorption complex catalyst was prepared by pretreating at a high temper-
ature of 900 C. Evaluation of the catalyst prepared by the ReSER hydrogen production
process through 10 circulations revealed significant improvement instability.
Copyright © 2015, Hydrogen Energy Publications, LLC. Published by Elsevier Ltd. All rights
reserved.
Introduction
Hydrogen is an environmentally friendly energy source with a
wide array of applications in the chemical and petroleum in-
dustries. Among various feedstock, natural gas is the major
source for production of hydrogen via steam methane
reforming (referred to as SMR) [1,2]. In recent years, an
improved SMR-based method for hydrogen production called
sorption enhanced reaction process (referred to as SERP) hasattracted strong attention. SERP involves the use of a CO2
adsorbent to enhance the methane reforming process by in
situ removal of CO2. It has advantages of low reaction tem-
perature, high concentration hydrogen outlet and controllable
emission of the greenhouse gas CO2 [3e5].
In a traditional SERP process, the CO2 adsorbent and nickel
reforming catalyst are mixed together mechanically, and CaO
wastypicallyselected as the CO2 adsorbent because of its high
* Corresponding author. College of Chemical and Biological Engineering, Zhejiang University, Hangzhou 310027, Zhejiang, China.
Tel.: þ86 571 87953138; fax: þ86 571 87953735.
E-mail address: [email protected] (S. Wu).
Available online at www.sciencedirect.com
ScienceDirect
j o u r n a l h o m e p a g e : w w w . e l s e v i er . c o m / l o c a t e / h e
i n t e r n a t i o n a l j o u r n a l o f h y d r o g e n e n e r g y 4 0 ( 2 0 1 5 ) 5 6 1 7 e5 6 2 3
http://dx.doi.org/10.1016/j.ijhydene.2015.02.032
0360-3199/Copyright © 2015, Hydrogen Energy Publications, LLC. Published by Elsevier Ltd. All rights reserved.
8/9/2019 1-s2.0-S0360319915003377-main
http://slidepdf.com/reader/full/1-s20-s0360319915003377-main 2/7
CO2 sorption capacity and natural abundance [6,7]. Recently,
Wu etal. [8] proposed a concept of reactive sorption-enhanced
methane reforming (referred to as ReSER)process based on the
use of a sorption complex catalyst that is a composite of a
nano-particulate CaO adsorbent and a Ni-based catalyst in a
single micro-spherical particle. Compared with mechanically
mixed adsorbent and catalyst, this sorption complex catalyst
can reduce resistance to heat and CO2 diffusion transfer dur-ing the reforming process and also offers other advantages
such as increased efficiency for enhanced reforming and
convenient handling in a fluidized bed reactor [9e11].
Despite the advantages of the sorption complex catalyst,
previous studies showed that its catalytic activity decreased
after several ReSER cycles [8]. Various methods have been
proposed to improve its stability and activity. Wang and Feng
[12,13] used ZrO2 and La2O3 as additives to improve the sta-
bility of the catalyst by increasing dispersion of nickel and
inhibiting the formation of NiAl2O4 spinel. Zhang and Tang
[14] used polyethylene glycol (PEG-6000) as a template to
expand the pore size and thereby enhance the dispersion of
nickel to increase the activity. All of the aforementioned so-lutions mainly focused on improving the stability and activity
of nickel catalyst, but ignored the influence of nano-
particulate CaO on the sorption catalyst. Since the
embedded CaO needs undergo multiple carbonationecalci-
nation cycles to keep its sorption activity, this process may
have a negative influence on the sorption complex catalyst.
The effect of carbonationecalcination cycles on the sta-
bility of the catalyst is not clear, and the deactivation mech-
anisms of the catalyst are not well understood. Numerous
studies have found structural destruction and decline in
sorption activity of CaO-based absorbent after multiple car-
bonationecalcination cycles [15e18]. In addition, steam in the
carbonation process has been reported to accelerate the CaOsintering rate, resulting in a rapid decline in its sorption
property [19e21]. However, no study has been undertaken to
understand structural destruction of CaO in the complex
sorption catalyst and its influence on catalyst activity during
carbonationecalcination cycles.
In this study, we prepared Ni-nano-CaO/Al2O3 sorption
complex catalyst and subjected it to three different carbo-
nationecalcination cycling conditions to determine the
mechanism of micro-structural changes and activity decline.
Then, a Ni-nano-CaO/Ca12Al14O33 sorption complex catalyst
was prepared based on our findings in order to improve the
stability of the complex catalyst.
Experiment
Preparation of catalyst
Preparation of Ni-nano-CaO/Al2O3 sorption complex catalyst
The Ni-nano-CaO/Al2O3complex catalyst was prepared by
impregnating Ni(NO3)2 solution on the nano-CaO/Al2O3 sup-
port as described in the literature [13]. The support was pre-
pared by mixing nano-CaCO3 (70 nm, >95% purity, Hu Zhou
LingHua Co., Ltd., China) with alumina sol (10%, Zibo Longao
Co. Ltd., China). The mixed slurry was dried and extruded into
a cylinder with a diameter of approximately 2 mm. The final
Ca/Al molar ratio in the slurry was 1:1.4. The support was
calcined at 550 C f o r 2e4 h and groundto 1.3e1.5 mm. A 0.2 M
Ni(NO3)2 solution (98% purity, Shanghai HengXin Chemical
Reagent Co., Ltd., China) was prepared and infused into the
nano-CaCO3 /Al2O3 support, and the catalyst was dried at
100e150 C and calcined at 500e800 C. The final Ni content
was about 15%, and the catalyst was named “CA-cat1”.
Preparation of Ni-nano-CaO/Ca12Al14O33 sorption complex
catalyst
Preparation of the sorption complex catalyst was similar to
that of the catalyst described in section Preparation of Ni-
nano-CaO/Al2O3 sorption complex catalyst. The nano-
CaCO3 /Al2O3 support was obtained in the same way and
calcined at 900 C for 2 h to form nano-CaO/Ca12Al14O33. Then
impregnated the same Ni(NO3)2 solution as described above.
The catalyst was named ‘CA-cat2’.
Characterization of the sorption complex catalyst
Surface area and pore structures of the sorption complex cata-
lyst were characterized by nitrogen physical sorption in liquid
N2 at 77 K using an apparatus (BELII-mini Japan). Surface area
wascalculatedaccordingtotheBrunauereEmmetteTeller(BET)
formula, and pore size distribution was calculated using the
Barrette JoynereHalenda (BJH) model. Micro-crystallinity of the
samples wasmeasured by X-raydiffraction (XRD) on a Rigaku D/
MAX-RA X-ray diffractometer (Japan) equipped with a copper
anode. The measurement conditions were: voltage 40 kV, cur-
rent 40 mA, and diffraction angle 2q with a range of 10 to 80.
Thermogravimetric analysis (Pyris1, PerkineElmer, USA)
was used to measure the sorption property of the samples.
The sorption process was conducted at 600 C under 0.02 MPa
ofCO2 in N2. Regeneration was performed at 750 C in pure N2.
The sorption capacity was calculated according to Equa-
tion (1):
Sorption capacity ¼CO2 sorption mol amount
Mass of catalyst
1000ðmol=kg Þ (1)
Evaluation of catalyst
Evaluation of ‘CA-cat1’ by carbonationecalcination cycling
A fixed-bed reactor was used for the carbonationecalcination
cycling test. Further details of the fixed-bed are provided
elsewhere [12,13]. Mass flow controllers and water pump wereutilized to achieve the desired inlet gas concentrations. Two
cyclic carbonation conditions were employed: 600 C for 1 h
with 20% CO2e80%N2, and 20% CO2e80% H2O respectively. All
calcinations were carried out at 800 C with 100%N2 for1h.To
determine the effect of temperature variation, a cyclic con-
dition in which the temperature was varied between 600 C
and 800 C with100%N2 for the sametime was used. A total of
30 carbonationecalcination cycles were performed and 10 g of
catalyst was used to obtain different samples that were tested
after the 1st, 3rd, 7th, 15th, and 30th cycles. The samples were
designated as ‘Sn-m’ where ‘n’ represents the carbonation
condition and ‘m’ represents the number of cycle. The con-
dition with pure N2 without carbonation was defined as ‘S1-m’
i n t e r n a t i o n a l j o u r n a l o f h y d r o g e n e n e r g y 4 0 ( 2 0 1 5 ) 5 6 1 7 e5 6 2 35618
8/9/2019 1-s2.0-S0360319915003377-main
http://slidepdf.com/reader/full/1-s20-s0360319915003377-main 3/7
for comparison. The carbonation condition with 20%
CO2e80%N2 was defined as ‘S2-m’. The carbonation condition
with 20% CO2e80% H2O was defined as ‘S3-m’.
Evaluation of ‘CA-cat2’ by the ReSER hydrogen production
process
Evaluation of the ‘CA-cat2’ complex catalysts was carried out
in the same fixed-bed as described in section 2.2.1. The con-
dition for ReSER hydrogen production was as follows: 5 g
sorption complex catalyst, 45 mL/min CH4, 180 mL/min H2O,
reaction at 600 C and calcination at 800 C with 100% N2.
Before the reaction, the sorption catalyst was calcined at
800 C with 100% N2 and then reduced under 20%H2, 80%N2
with total gas flow of 100 mL/min. GC analysis was used to
detect the outlet production mixtures. The conversion of
methane was calculated according to Equation (2), where
XCH4 ð%Þ is the conversion of methane, FCH4 ðmL=minÞ is theflow rate of methane, FoutðmL=minÞ is the effluent flow rate of
the product gas, and yCH4 (%) is the methane content.
XCH4 ¼FCH4
Fout yCH4
FCH4
100% (2)
Multiple reactions and regeneration runs were conducted
to evaluate the stability of the sorption complex catalyst.
Results and discussions
Effect of carbonationecalcination cycles on microstructure
and sorption property of the catalyst
The specific surface area of all carbonationecalcination
cycling test samples was shown in Fig. 1. The results showed
that the ‘S1’ condition of use N2 as the environmental gas has
a little change of surface area. Temperature variation between
600 C and 800 C had little effect on the catalyst microstruc-
ture with a slightly specific surface area fluctuation at
20 m2 g 1. Alternatively, conditions of ‘S2’ and ‘S3’ which all
contain CO2 as the environmental gas have an obvious
Fig. 1 e Variation of specific surface area of CA-cat1 under
S1, S2, S3 conditions.
Fig. 2 e
Pore size distribution of CA-cat1 under S1, S2, S3 conditions. (a) 1st cycle, (b) 7th cycle, (c) 15th cycle, (d) 30th cycle.
i n t e r n a t i o n a l j o u r n a l o f h y d r o g e n e n e r g y 4 0 ( 2 0 1 5 ) 5 6 1 7 e5 6 2 3 5619
8/9/2019 1-s2.0-S0360319915003377-main
http://slidepdf.com/reader/full/1-s20-s0360319915003377-main 4/7
decrease of surface area. And contain the steam and CO2 both
of ‘S3’ condition has a big decrease of surface area. The rapiddecay of ‘S2’ and‘S3’ in the initial three cycles indicates that
the catalyst microstructure changes strongly during the initial
carbonationecalcination cycles, while the presence of steam
during carbonation appeared to accelerate the decay rate. No
significant variation was observed in the later cycles, which
implies that the catalyst structure was stable.
Fig. 2(a), (b), (c), (d) show a comparison of the evolution of
pore size distribution of the catalyst under S1, S2, S3 three
different test conditions after 1, 7, 15, 30 cycles respectively.
Two types of meso-pores were found with the main part
around 8e10 nm and the subordination part around 35 nm,
and we defined them as ‘SPs’ and ‘LPs’, respectively. The ‘LPs’
appeared stable during the 30 carbonatione
calcination cyclesat all cycling conditions while the ‘SPs’varied significantly
with changes in the cycling conditions. The maximum in the
curve of dV p /drp vs. rp shifted slightly from 8 nm to 13 nm in
the comparison cycles,which indicated expansion of the pore.
The structure of ‘SPs’ decayed strongly during the carbo-
nationecalcination cycles in the initial 15 cycles with the
presence of steam accelerating the decay rate, while a stable
trend was observed in subsequent 15 cycles. The pore vol-
umes of pores with a diameter of about 13 nm appeared
relatively stable at all cyclic conditions after 30 cycles. These
results show that apart from the influence of high tempera-
ture variation, the carbonationecalcination process has a
major effect on pore evolution, with the small pores decaying during the initial cycles.
To investigate the influence of cycles on CO2 sorption ca-
pacity, each sample obtained under S1, S2, S3 conditions was
tested by thermogravimetric analysis, and the results are
shown in Fig. 3. The declining trend in sorption capacity was
similar to the decrease in the specific surface area, suggesting
that they are related; higher specific surface area could pro-
vide more sorption reactive sites and thereby increase the CO2
sorption capacity. In the cyclic condition of ‘S1’, the CO2
sorption capacity declined from 3.3 mol/kg to 2.5 mol/kg
during 30 cycles, and the decline of ‘S2’, ‘S3’ was significant in
the initial 15 cycles, but only modest in the subsequent 15
cycles. Sintering of CaO during the cycles may have caused
decay of the catalyst's microstructure and sorption capacity,
but further detailed investigation should be conducted to
determine the exact relationship between decay rate and
carbonationecalcination cycles.
Mechanism of the influence of carbonationecalcination on
catalysts
The experiments were designed use CA-cat1 under S1, S2, S3
conditions for 30 cyclic carbonationecalcination runs to study
the relation between the conditions and the formation of
Ca12Al14O33.
XRD was used to measure phase transformation of thesamples after different cycling operations. Data on the sample
from the 30th cycle under each cyclic condition is presented in
Fig. 4. From Fig. 4, there are obvious Ca12Al14O33 peak under S3
condition, and a few Ca12Al14O33 peak is under S2 condition,
and few Ca12Al14O33 peak appeared under S1 condition. The
result of the Ca12Al14O33 peak was the most intense of sample
S3-30 indicates the sample contained the largest amount of
Ca12Al14O33.
Fig. 3 e Sorption capacity of CA-cat1 samples treated under
S1, S2, S3 conditions.Fig. 4 e XRD test result of the 30th sample of CA-cat1 under
S1, S2, S3 conditions.
Fig. 5 e
TEM image of the sample CA-cat1.
i n t e r n a t i o n a l j o u r n a l o f h y d r o g e n e n e r g y 4 0 ( 2 0 1 5 ) 5 6 1 7 e5 6 2 35620
8/9/2019 1-s2.0-S0360319915003377-main
http://slidepdf.com/reader/full/1-s20-s0360319915003377-main 5/7
The cyclic reaction between CaO and CO2 may push thecatalyst to an unstable state, and the Al2O3 in the catalyst
support may react with CaO [22,23] according to Equation (3):
12CaO þ 7Al2O3/Ca12Al14O33 (3)
Normally, the reaction shown in Equation (3) occurs only at
temperatures greater than 900 C [22]. However, in this study,
Ca12Al14O33 was found to be formed at temperatures as low as
800 C. A possible reason for this behavior is the use of nano-
sized CaO as CO2 sorbent, and in most previous studies,
micro-sized CaO was used as the CO2 sorbent.
Fig. 5 showed the TEM image of sample of CA-cat1. The
dark point presents the NiO before reduced to Ni as a size of
5e
20 nm. And the other is the support of a mixture of CaO/Al2O3. The size is also under 100 nm. The results proved the
both NiO and CaO/Al2O3 are under a nanometer scale.
To determine the relationship between formation of
Ca12Al14O33 and cycling conditions, we characterized the
samples cycled under the S3 condition in detail s as shown in
Fig. 6. From Fig. 6, Ca12Al14O33 was not detected during the
original three cycles, but was easily detected after the 7th
cycle. This indicates that the quantity of Ca12Al14O33 formed
accumulated during cycling as the as the carbonationecalci-
nation cycles running on. The catalyst we prepared was a
complex of alumina sol and nano-CaCO3, which has a rela-
tively low decomposition temperature [24]. The nano-CaCO3
in the catalyst likely decomposed into nano-CaO at 800 C.
Hence, the reaction shown in Equation (3) must have occurred
during each calcination cycle under a temperature of 800 C.
A possible mechanism of Ca12Al14O33 formation under
different cycling conditions is proposed in Fig. 7. First, after
initial calcination at 800 C, nano CaCO3 decomposed into
nano-CaO, which immediately reacted with Al2O3 to form
Ca12Al14O33. Owing to the smaller molar volume of CaO
compared to that of CaCO3, a pore channel was simulta-
neously formed. If the channel was not filled-in during sub-
sequent cycles, it would prevent continued reaction between
CaO and Al2O3, as shown case 1 in Fig. 7. Therefore, cycling
performed under N2 atmosphere did not lead to accumulationthe quantity of Ca12Al14O33. However, if the channel became
blocked during carbonation, as shown in cases 2 and 3 in
Fig. 7, a new phase interface between CaCO3 and Al2O3 would
have formed and led to the formation of Ca12Al14O33 during
subsequent calcination. This may explain why Ca12Al14O33
accumulated as the number of cycles increased. The effect of
steam is explained as follows: since steam may accelerate
carbonation rate by forming the intermediate Ca(OH)2, the
amount of CaCO3 may have increased during carbonation in
our experiments, thereby resulting in increased amounts of
Ca12Al14O33 after calcination.
A comparison of the sintering behavior of the sorption
complex catalyst under different conditions revealed thatformation of Ca12Al14O33, which consumed the porous Al2O3
carrier, played the largest role in the evolution of micro-
structure of the catalysts. As a result, the specific surface area
of catalysts cycled under the S2 and S3 conditions decreased
Fig. 6 e XRD results of samples under the S3 condition.
Fig. 7 e Mechanism of Ca12Al14 O33formation during the carbonationecalcination cycle.
i n t e r n a t i o n a l j o u r n a l o f h y d r o g e n e n e r g y 4 0 ( 2 0 1 5 ) 5 6 1 7 e5 6 2 3 5621
8/9/2019 1-s2.0-S0360319915003377-main
http://slidepdf.com/reader/full/1-s20-s0360319915003377-main 6/7
substantially, whereas that of the catalyst cycled under the S1
conditions decreased only slightly. The reasons for these be-
haviors are similar in that the sorption capacity changes with
consumption of CaO during the carbonationecalcination
cycling process. Since Ca12Al14O33 is thermally stable at tem-
peratures less than 1000 C [25], it serves as an inert compo-
nent to maintain the skeleton of the complex catalyst and to
prevent further sintering during cycling. This may explain
why the microstructure and sorption capacity stabilized after
several cycles.
Results of ‘CA-cat2’ evaluation by the ReSER hydrogen production process
Based on our finding that formation of Ca12Al14O33led to a
more stable microstructure and sorption properties, a new
sorption catalyst Ni-nano-CaO/Ca12Al14O33 was obtained to
improve the stability of sorption complex catalyst as illus-
trated above (section Preparation of Ni-nano-CaO/Ca12Al14O33
sorption complex catalyst).
Results of stability evaluation of ‘CA-cat2’ based on ReSER
hydrogen production are presented in Fig. 8. Ten runs of the
ReSER hydrogen production were conducted. The first
reformingreaction showedthe highestactivitywith 96.2%(v/v)
hydrogen content and 86.1% methane conversion. The sorp-
tion catalyst showedan improvement in stabilityin theinitial8
reaction cycles with >90.0% (v/v) hydrogen content in theoutlet. Comparison of our results with the previous study [13]
that investigated the stability of Ni-nano CaO/Al2O3 is shown
in Fig. 9. The catalyst Ni-nano CaO/Ca12Al14O33 shows greater
stability than ‘NCA’ with improvement of six reaction cycles.
The sorption complex catalysts were characterized before
and after ReSER hydrogen production by N2 nitrogen physic-
sorption to investigate variation in the microstructure, and
by TGA testing to define the reason of sorption capacity sta-
bility. As is evident from Table 1, the surface area and pore
volume of CA-cat2-0 was much smaller than that of NCA-0,
and the average pore diameter was much larger than that of
NCA-0. However, the microstructure of NCA changed signifi-
cantly after 7 ReSER cycles while the CA-cat2 remained almostthe same after 10 ReSER cycles. This improvement in micro-
structure stability may have contributed to stability of sorp-
tion capacity, making the catalyst highly suitable for ReSER
hydrogen production.
Conclusions
In this paper, the influence of carbonationecalcination con-
ditions on microstructure of the sorption catalyst was studied.
The results showed that microstructure and CO2 sorption
capacity of the sorption complex catalyst decayed signifi-
cantly during the carbonatione
calcination cycle, especiallyunder a steam atmosphere during the initial cycles. This was
caused not only by sintering of CaO to effectively decrease the
surface area, but also because the reaction between Al2O3 and
CaO to form Ca12Al14O33, which decreased the Al2O3 and
reactive CaO content, occurred even at 800 C. A model for
formation of Ca12Al14O33 is proposed. Meanwhile, our results
suggest that formation of Ca12Al14O33 is the main factor
contributing to stability of the subsequently cyclic process.
Based on these results, a new catalyst was prepared by
pretreatment of the nano-CaCO3 /Al2O3 support at a high
temperature to improve the stability of the sorption complex
catalyst. Ten cycles of ReSER process of hydrogen production
has proved the more stable of conversion of methane, while
Fig. 8 e Evaluation of ‘CA-cat2’ catalyst by the ReSER
hydrogen production process. (reaction temperature of
600 C, calcination temperature of 800 C, steam methane
molar ratio of 4, reaction pressure of 1 atm).
Fig. 9 e Evaluation the stability of ‘CA-cat2’ and ‘NCA’
catalysts by the ReSER hydrogen production process.
(reaction temperature of 600 C, calcination temperature of
800 C, steam methane molar ratio of 4, reaction pressure
of 1 atm).
Table 1 e Microstructure variation of CA-cat2 and NCA.
Name Surfacearea
(m2$g 1)
Average poresize(nm)
Porevolume
(cm3$g 1)
Adsorptioncapacity(mol/kg)
NCA-0 33.4 17.2 0.198 2.1
NCA-7 10.7 19.8 0.055 0.9
CA-cat2-0 5.2 49.3 0.064 1.4
CA-cat2-10 5.4 41.1 0.055 1.1
i n t e r n a t i o n a l j o u r n a l o f h y d r o g e n e n e r g y 4 0 ( 2 0 1 5 ) 5 6 1 7 e5 6 2 35622
8/9/2019 1-s2.0-S0360319915003377-main
http://slidepdf.com/reader/full/1-s20-s0360319915003377-main 7/7
the catalyst without pretreatment yielded only four cycles of
stable of conversion of methane.
Acknowledgment
We gratefully acknowledge financial supports from the Na-
tional Natural Science Foundation of China (NSFC,Grant No.
21276234).
r e f e r e n c e s
[1] Yang X, Wei YN. Research progress in methane reforming
catalyst for the production of hydrogen. Mater Rev
2007;21:49e53.
[2] Li WB, Qi ZQ. Progress on technical study for production of
hydrogen from methane. Nat Gas Ind 2005;2:165e8.
[3] Harrison DP. Sorption-enhanced hydrogen production: a
review. Ind Eng Chem Res 2008;47:6486e501.
[4] Han C, Harrison DP. Simultaneous shift reaction and carbondioxide separation for the direct production of hydrogen.
ChemEngSci 1994;49:5875e83.
[5] Carvill BT, Hufton JR, Anand M, Sircar S. Sorption-enhanced
reaction process. AIChE J 1996;42:2765e72.
[6] Johnsen K, Ryu HJ, Grace JR, Lim CJ. Sorption-enhanced
steam reforming of methane in a fluidized bed reactor with
dolomite as CO2-acceptor. ChemEngSci 2006;61:1195e202.
[7] Lopez Ortiz A, Harrison DP. Hydrogen production using
sorption-enhanced reaction. Ind Eng Chem Res
2001;40:5102e9.
[8] Wu SF, Li LB, Zhu YQ, Wang XQ. A micro-sphere catalyst
complex with nano CaCO3 precursor for hydrogen
production used in ReSER process. Eng Sci 2010;8:22e6.
[9] Kim JN, Ko CH, Yi KB. Sorption enhanced hydrogen
production using one-body CaOeCa12Al14O33eNi composite
as catalytic absorbent. Int J Hydrogen Energy 2013;38:6072e8.
[10] Broda M, Kierzkowska AM, Baudouin D, Imtiaz Q, Coperet C,
Muller CR. Sorbent-enhanced methane reforming over a
NieCa-based, bifunctional catalyst sorbent. ACS Catal
2012;2:1635e46.
[11] Chanburanasiri N, Ribeiro AM, Rodrigues AE,
Arpornwichanop A, Laosiripojana N, Praserthdam P, et al.
Hydrogen production via sorption enhanced steam methane
reforming process using Ni/CaO multifunctional catalyst. Ind
Eng Chem Res 2011;50:13662e71.
[12] Wu SF, Wang LL. Improvement of the stability of a ZrO2-
modified Ni-nano-CaO sorption complex catalyst for ReSER
hydrogen production. Int J Hydrogen Energy
2010;35:6518e24.
[13] Feng HZ, Lan PQ, Wu SF. A study on the stability of a
NiOeCaO/Al2O3 complex catalyst by La2O3 modification for
hydrogen production. Int J Hydrogen Energy
2012;37:14161e6.
[14] Zhang F, Tang Q, Wu SF. Preparation of a mesoporoussorption complex catalyst and its evaluation in reactive
sorption enhanced reforming. J Zhejiang Univ Sci A
2013;14:915e22.
[15] Donat F, Florin NH, Anthony EJ, Fennell PS. Influence of high-
temperature steam on the reactivity of CaO sorbent for CO2
capture. Environ Sci Technol 2012;46:1262e9.
[16] Blamey J, Anthony EJ, Wang J, Fennell PS. The calcium
looping cycle for large-scale CO2 capture. Prog Energ
Combust 2010;36:260e79.
[17] Fennell PS, Pacciani R, Dennis JS, Davidson JF, Hayhurst AN.
The effects of repeated cycles of calcination and carbonation
on a variety of different limestones, as measured in a hot
fluidized bed of sand. Energy Fuel 2007;21:2072e81.
[18] Sun P, Grace JR, Lim CJ, Anthony EJ. The effect of CaO
sintering on cyclic CO2 capture in energy systems. AIChE J2007;53:2432e42.
[19] Dou B, Song Y, Liu Y, Feng C. High temperature CO2 capture
using calcium oxide sorbent in a fixed-bed reactor. J Hazard
Mater 2010;183:759e65.
[20] Manovic V, Anthony EJ. Carbonation of CaO-based sorbents
enhanced by steam addition. Ind Eng Chem Res
2010;49:9105e10.
[21] Symonds RT, Lu DY, Hughes RW, Anthony EJ, Macchi A. CO2
capture from simulated syngas via cyclic carbonation/
calcination for a naturally occurring limestone: pilot-plant
testing. Ind Eng Chem Res 2009;48:8431e40.
[22] Wu SF, Jiang MZ. Formation of a Ca12Al14O33 nanolayer and
its effect on the attrition behavior of CO2-adsorbent
microspheres composed of CaO nanoparticles. Ind Eng Chem
Res 2010;49:12269e
75.[23] Li Z, Cai N, Huang Y, Han H. Synthesis, experimental studies,
and analysis of a new calcium-based carbon dioxide
absorbent. Energy Fuel 2005;19:1447e52.
[24] Wu SF, Li QH, Kim JN, Yi KB. Properties of a nano CaO/Al2O3
CO2 sorbent. Ind Eng Chem Res 2008;47:180e4.
[25] Rivas Mercury JM, De Aza AH, Turrillas X, Pena P. The
synthesis mechanism of Ca3Al2O6 from soft
mechanochemically activated precursors studied by time-
resolved neutron diffraction up to 1000 C,. J Solid State
Chem 2004;177:866e74.
i n t e r n a t i o n a l j o u r n a l o f h y d r o g e n e n e r g y 4 0 ( 2 0 1 5 ) 5 6 1 7 e5 6 2 3 5623