Effects of CNTs on the hydrogen storage properties of MgH 2 and MgH 2BCC composite
-
Upload
independent -
Category
Documents
-
view
3 -
download
0
Transcript of Effects of CNTs on the hydrogen storage properties of MgH 2 and MgH 2BCC composite
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 en e r g y 3 5 ( 2 0 1 0 ) 7 8 2 1e7 8 2 6
Avai lab le a t www.sc iencedi rec t .com
journa l homepage : www.e lsev ier . com/ loca te /he
Effects of CNTs on the hydrogen storage properties of MgH2
and MgH2-BCC composite
A. Ranjbar a, M. Ismail a, Z.P. Guo a,b,c,*, X.B. Yu a,b,d, H.K. Liu a,b
a Institute for Superconducting & Electronic Materials, University of Wollongong, Wollongong, NSW 2522, AustraliabCSIRO National Hydrogen Materials Alliance, CSIRO Energy Centre, 10 Murray Dwyer Circuit, Steel River Estate, Mayfield West,
NSW 2304, AustraliacSchool of Mechanical, Materials & Mechatronics Engineering, University of Wollongong, NSW 2522, AustraliadDepartment of Materials Science, Fudan University, Shanghai 200433, China
a r t i c l e i n f o
Article history:
Received 18 December 2009
Received in revised form
14 May 2010
Accepted 14 May 2010
Available online 17 June 2010
Keywords:
Hydrogen storage
Magnesium hydride
Body centred cubic (BCC) alloys
Carbon nanotubes (CNTs)
* Corresponding author at: Institute for SupAustralia. Fax: þ61 2 4221 5731.
E-mail address: [email protected] (Z.P. G0360-3199/$ e see front matter ª 2010 Profedoi:10.1016/j.ijhydene.2010.05.080
a b s t r a c t
MgH2 with 10 wt.% Ti0.4Mn0.22Cr0.1V0.28 alloy (termed the BCC alloy for its body centred
cubic structure) and 5 wt.% carbon nanotubes (CNTs) were prepared by planetary ball
milling, and its hydrogen storage properties were compared with those of the pure MgH2
and the binary mixture of MgH2 and the BCC alloy. The sample with CNTs showed
considerable improvement in hydrogen sorption properties. Its temperature of desorption
was 125 �C lower than for the pure sample and 59 �C lower than for the binary mixture. In
addition, the gravimetric capacity of the ternary sample was 6 wt.% at 300 �C and 5.6 wt.%
at 250 �C, and it absorbed 90% of this amount at 150 s and 516 s at 300 �C and 250 �C,
respectively. It can be hypothesised from the results that the BCC alloy assists the disso-
ciation of hydrogen molecules into hydrogen atoms and also promotes hydrogen pumping
into the Mg/BCC interfaces, while the CNTs facilitate access of H-atoms into the interior of
Mg grains.
ª 2010 Professor T. Nejat Veziroglu. Published by Elsevier Ltd. All rights reserved.
1. Introduction catalysts, such as transition metals [8e10], metal oxides
The storage of hydrogen in solids seems to be the most effi-
cient and safestmethod for application in fuel cells and hybrid
vehicles [1]. Among the different solids,magnesiumhydride is
a very promising material for this purpose because of its high
capacity (7.6 wt.%), good reversibility, and low cost [2].
However, its practical application is greatly hindered by its
sluggish hydrogenation/dehydrogenation kinetics and high
operation temperature [3]. Over the last decade intensive
investigations has been dedicated to overcoming these
barriers. These efforts include surface activation and reduc-
tion of grain size by ball milling [4e7], as well as the use of
erconducting & Electron
uo).ssor T. Nejat Veziroglu. P
[11,12], body centred cubic alloys [13,14], and different kind of
carbons [15,16].
In our previous work [17], it was demonstrated that ball
millingmagnesiumwithTi0.4Mn0.22Cr0.1V0.28 alloy improvedthe
hydrogenstoragepropertiesofMgH2.On theotherhand, carbon
nanotubes (CNTs) exhibited excellent catalytic effects on the
hydrogen sorption properties of magnesium based composites
[18]. A combination of CNTs with transition metals has been
found to lead to an especially great enhancement of hydrogen
dissociation and diffusion into Mg nanoparticles [19e21].
In this work, the effect of the combination of 10 wt.% of
Ti0.4Mn0.22Cr0.1V0.28 alloy, hereafter referred to as the BCC
ic Materials, University of Wollongong, Wollongong, NSW 2522,
ublished by Elsevier Ltd. All rights reserved.
i n t e rn a t i o n a l j o u r n a l o f h y d r o g e n en e r g y 3 5 ( 2 0 1 0 ) 7 8 2 1e7 8 2 67822
alloy due to its body centred cubic structure, with a small
amount of CNTs (5 wt.%) on the hydrogen storage properties
of MgH2 has been investigated and compared with the
performance of pure MgH2 and MgH2 þ 10 wt.%
Ti0.4Mn0.22Cr0.1V0.28.
2. Experimental details
The BCC alloy sample was prepared by magnetic levitation
melting of the constituent metals (Beijing YiTianhui Institute
of Metallic Materials, all with purity of more than 99.9%). A
50 g ingot was turned over and remelted four times to ensure
higher homogeneity, and then it was quenched on a water-
cooled rotating molybdenum disc that was spinning at the
rate of 20 m/s. After preparation of the BCC alloy, 0.9 g of pure
MgH2 (SigmaeAldrich, H-storage grade powders) and 0.1 g of
the BCC alloy were introduced into stainless steel vials of
a QM-3SP2 planetary ball-milling instrument. The samples
were ball milled under Ar atmosphere for 24 h with a ball to
powder weight ratio of 20 and a speed of 400 rpm. In the last
step, the MgH2 þ 10 wt.% BCC þ 5 wt.% CNT (termed Mg-BCC-
CNT) was prepared by adding 5 wt.% multiwall carbon nano-
tubes (MWCNTs, SigmaeAldrich,> 99.9%) into the ball milling
vial with MgH2 þ 10 wt.% BCC composite and milling the
mixture for 2 h. For comparison, pure MgH2 andMgH2 þ 10 wt.
% BCC (termedMg-BCC) samples were also prepared using the
same ball-milling technique for 26 h. All handling of the
powders, before and after ball milling, was performed in an
argon filled glove box (with oxygen and water content each
below 1 ppm) in order to prevent any oxidation of the samples.
X-ray diffraction (XRD) patterns of the as-prepared and
dehydrogenated samples were obtained with a GBC-MMA
X-Ray diffractometer using Cu Ka radiation (l¼ 0.15418 nm) at
40 kV and 20 mA. The morphology of the composites and the
distribution of the elements were characterized by using
scanning electronmicroscopy (SEM; JEOL JSM-6460A) followed
by energy dispersive spectroscopy (EDS). Backscattered elec-
tron composition (BEC) images were also obtained on this
instrument. The desorption temperature and hydrogen
capacity of the as-prepared composites were determined by
using an AMC gas reactor controller in profile releasemode, in
which the samples were heated up from room temperature to
a maximum of 500 �C with a heating rate of 10 �C/min and
a pressure of 1 atm. The onset temperature (Tonset), the
temperature at which hydrogen starts to be released from the
sample, the desorption temperature (Tdes), the temperature at
which the hydrogen is completely released from the sample,
and the hydrogen content were measured and graphed using
the software package supplied with the instrument. The
hydriding kinetics, under a hydrogen pressure of 30 atm, and
the dehydriding kinetics, under a hydrogen pressure of
0.1 atm, were studied by Sievert’s method at 250 �C and 300 �Cusing the AMC gas reactor controller.
3. Results and discussion
XRD patterns of the as-milled samples are shown in Fig. 1. The
main peaks match b-MgH2 (JCPDS-12-0697), but there are
small peaks corresponding to g-MgH2 (JCPDS 351184), the BCC
alloy, MgO, and even Mg. The presence of the orthorhombic
g-phase is a result of alteration in the microstructure because
of the ball milling [22]. Despite the low quantity of the BCC
alloy in the composite, this phase could be observed as is in
agreement with Reference [13]. However, there are no peaks
which indicate formation of any new alloy phase as a result of
reaction between MgH2 and the BCC alloy. The existence of
the weak Mg peak indicates that the commercial magnesium
hydride was partially dehydrogenated during ball milling.
Diffraction peaks of the composites are considerably broad-
ened as a consequence of reduction of particle size, as well as
the increase in defects and the mechanical strains created
within the lattice by the ball milling [14].
Fig. 2 shows SEM images of all the as-prepared samples. It
can be explicitly seen that the particle size of the samples
decreases in the following order: pure MgH2 (Fig. 2(a)), MgH2-
BCC (Fig. 2(b)), and MgH2-BCC-CNT (Fig. 2(c)). The particle size
distribution of the pure MgH2 sample is concentrated in the
range of 10 mme30 mm, but from 2 mm to 20 mm for the MgH2-
BCC and from a few hundred nanometres to 5 mm for the
MgH2-BCC-CNT.
In addition, agglomeration is lower for the samples with
CNTs than in the samples without them, which is because of
the lubricant effect of the carbon as reported in the literature
[23,24]. To monitor the dispersion of the BCC alloy particles,
EDSwas conducted, and a backscattered electron composition
(BEC) image of the Mg-BCC sample with the EDS element
analysis (inset) is shown in Fig. 3. The larger gray particles
(between 5 mm and 30 mm) are MgH2, and the white particles,
with sizes of several hundred nanometres, are the BCC alloy. It
can be clearly observed that the BCC alloy particles are
distributed uniformly among the MgH2 particles. Although by
BEC it is possible to see only the surface of the powders, it can
be hypothesized that the BCC phase is distributed both on the
surface of the Mg hydride grains and in the interior of the
particles. Therefore, based on the morphology, it is predict-
able that the hydrogen sorption properties of the samples
with the BCC alloy and CNTs will be improved as a result of
a clearly smaller particle size, less agglomeration, and
homogeneous dispersion of the catalysts among the MgH2.
Fig. 4 shows the hydrogen capacity and both Tonset and
Tdes for the as-milled samples, which were measured by
hydrogen release with the gas reactor controller in profile
mode. Before the measurement, the sample holder was
evacuated at room temperature for 30 min. Based on the
graphs, Tdes for both doped sample was reduced significantly.
The onset temperature of hydrogen release, Tonset, for the
pure sample is 350 �C, while for the MgH2-BCC and MgH2-
BCC-CNT samples, Tonset is 280 �C and 245 �C, respectively.Moreover Tdes for the pure MgH2 is 430 �C, but it is 361 �C for
the binary sample and 301 �C for the ternary one. Therefore,
Tdes was reduced by 125 �C and 66 �C for the MgH2-BCC-CNT
and MgH2-BCC samples, respectively, in comparison with the
pure MgH2. In addition the differences between Tdes and
Tonset show that hydrogen release from the sample including
CNTs was much easier. Moreover, based on the figure, the
hydrogen contents for all samples are almost the same and
approximately 6 wt.%. It was expected that the gravimetric
capacity would decrease in the order of pure MgH2,
25 30 35 40 45 50 55 60 65 70 75 802θ (degree)
In
ten
sity (a. u
.)
MgH2-BCC
MgH2-BCC-CNT
MgH2
&
&
##
# #
Δ Δ× × O
# β-MgH2
× γ-MgH2
& BCC
O MgO
Δ Mg
Fig. 1 e XRD patterns for as-milled samples.
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 en e r g y 3 5 ( 2 0 1 0 ) 7 8 2 1e7 8 2 6 7823
MgH2 þ BCC, and MgH2þBCC þ CNT because the BCC phase is
a hydrogen active phase with mass higher than that of
magnesium hydride and a lower gravimetric capacity, and
CNTs have not been demonstrated to absorb/adsorb
hydrogen under these experimental conditions. Therefore,
the common value of the hydrogen capacity of these samples
indicates that the hydrogen sorption efficiency is increased in
the presence of the additives.
Fig. 2 e SEM images of all samples: a) pu
After dehydrogenation under profile mode and for each
sample, the temperature of the sample holder was set at
300 �C (and then 250 �C), and the sample chamber was
evacuated for 1 h to remove any remaining hydrogen des-
orbed by the sample and to fix the temperature. Then, the
hydriding/dehydriding kinetics were studied at these
temperatures at a hydrogen pressure of 30 atm and 0.1 atm,
respectively.
re MgH2, b) Mg-BCC, c) Mg-BCC-CNT.
Fig. 3 e Backscattered electron composition (BEC) image of
the Mg-BCC sample, with its EDS element analysis shown
in the inset.
0
1
2
3
4
5
6a
b
0 500 1000 1500 2000 2500Time (s)
%)
tw
(t
ne
tn
oc
-H
Mg-BCC-CNTMg-BCCMg
-6
-5
-4
-3
-2
-1
0
0 50 100 150 200 250 300 350 400 450 500 550 600Time (s)
)%
tw
(t
ne
tn
oc
-H
MgH2-BCC-CNTMgH2-BCCMgH2
Fig. 5 e a) Hydrogen absorption at 300 �C and 30 atm, and b)
desorption at 300 �C and 0.1 atm for all samples.
i n t e rn a t i o n a l j o u r n a l o f h y d r o g e n en e r g y 3 5 ( 2 0 1 0 ) 7 8 2 1e7 8 2 67824
The absorption kinetics results at 300 �C (shown in Fig. 5(a))
indicate that both doped samples absorbed hydrogen more
rapidly than the pure one and that MgH2-BCC-CNT has the
fastest absorption rate. The maximum hydrogen absorbed
(Hmax) by pure MgH2 at this temperature and after 2500 s is
3.46 wt.%. This quantity for binary MgH2-BCC is 5.7 wt.% and
6 wt.% for ternary MgH2-BCC-CNT. MgH2-BCC-CNT soaks up
90% of itsHmax in 150 s while the times for MgH2-BCC and pure
MgH2 are 195 s and 1680 s, respectively.
The desorption kinetic curves at 300 �C (Fig. 5(b)) illustrate
that 90% ofHmax release occurs at 500 s, 179 s, and 93 s for pure
MgH2, MgH2-BCC, and MgH2-BCCeCNT, respectively. Fig. 6(a)
and (b) presents the corresponding absorption/desorption
kinetics at 250 �C.Hmax, at this temperature and after 2500 s, is
2.8 wt.% for pure MgH2, and 4.7 wt.% and 5.6 wt.% for MgH2-
BCC and MgH2-BCC-CNT, respectively. At this temperature,
the pure sample has absorbed 90% of its Hmax at 1932 s, while
this time for the binary sample is 823 s and 516 s for the
ternary one.
As both 300 �C and 250 �C are lower than Tdes of pure MgH2,
the kinetics of this phase is very sluggish at these tempera-
tures, although its kinetics are improved significantly as
a result of the addition of the BCC and BCC-CNT alloys.
-7
-6
-5
-4
-3
-2
-1
0
1
200 250 300 350 400 450
Temperature (°C)
)%
tw
(t
ne
tn
oC
-H
MgH2MgH2-BCC-CNTMgH2-BCC
245°C
280°C
346°C
301°C
361°C430°C
Fig. 4 e Initial hydrogen release of all as-prepared samples
in profile release mode.
Fig. 7 shows the XRD patterns for the dehydrogenated
samples. It can be observed that the major phase after dehy-
drogenation is magnesium, however, there are peaks corre-
sponding to the BCC alloy and MgO which overlap in the
MgH2-BCC pattern. Although all the sample handling was
done in an argon filled glove box, oxidation due to periodic
opening of the milling jar and the AMC sample holder in the
glove box could be the reason for the appearance of MgO
phase. The peaks became sharper for the dehydrided samples
in comparison with the as-milled samples, which indicates
a reduction in defects and mechanical strain through the
hydriding/dehydriding processes. In addition, there is a slight
shift in the peaks (as is shown in the Fig. 7 inset for the most
intense peak), indicating extra enlargement in the lattice
parameters of the unit cells for both MgH2-BCC and MgH2-
BCC-CNT composites. This enlargement could be due to the
formation of a solid solution between themagnesium hydride
and the additives.
The results demonstrate that 1) the BCC alloy improves the
hydriding/dehydryding kinetics and maximum hydrogen
capacity, 2) theMg-BCC-CNT system shows superior hydrogen
storage properties, and so 3) the BCC alloy and CNTs have
synergistic effects on all aspects of hydrogen sorption prop-
erties. On the other hand, the hydriding and dehydriding
mechanisms could be the keys to insight into the reasons for
these special effects. It is accepted both theoretically [25] and
experimentally [19,26] that: 1) dissociation of H2 molecules
into H-atoms on the surface of the magnesium, 2) diffusion of
H-atoms along the grain boundaries, and 3) hydrogen
absorption/desorption of the catalyst and transformation of
0
1
2
3
4
5
6a
b
0 500 1000 1500 2000 2500Time (s)
)%
tw
(t
ne
tn
oc
-H
MgH2-BCC-CNT
MgH2
MgH2-BCC
-6.5
-5.5
-4.5
-3.5
-2.5
-1.5
-0.5
0 200 400 600 800 1000 1200 1400 1600 1800 2000 2200 2400
Time (s)
)%
tw
(t
ne
tn
oc
-H
MgH2
MgH2-BCC-CNT
MgH2-BCC
Fig. 6 e a) Hydrogen absorption at 250 �C and 30 atm, and b)
desorption at 250 �C and 0.1 atm for all samples.
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 en e r g y 3 5 ( 2 0 1 0 ) 7 8 2 1e7 8 2 6 7825
Mg atoms into MgH2 molecules at catalyst/Mg interfaces, are
the three critical steps of the hydrogenation process. The
energy barrier for H2 dissociation without any substrate is
4.52 eV, and this value reduces to 1.15 eV in the presence of
magnesium [27], which still requires more than 400 �C for
dissociation. However, this energy barrier will decrease even
more in the presence of a catalyst. For example, it is 0.201 eV
and 0.103 eV for V and Ti, respectively [28]. Although further
investigation seems to be necessary to find the exact energy
25 30 35 40 45 50
2 (de
In
ten
sit
y (
a. u
.) O
&
&
Fig. 7 e XRD patterns for the samples after dehydrogenation. The
highest intensity.
barrier for H2 dissociation on the BCC alloy’s surface, as it is
a composite of transitionmetals, the barrier could be very low.
Therefore, the main catalytic effect of the BBC could be
dissociation of hydrogen molecules at low temperature and
improvement of the first step of the hydrogenation
mechanism.
In addition, as described in our previous work [17] and
other references [13,29,30], the BCC alloy can absorb the H-
atoms at low temperature to form BCC hydride by the
following reaction:
ðBCCÞ þ x2H20ðBCCÞHx (1)
with the BCC hydride then releasing hydrogen at the Mg/BCC
interfaces. Therefore, the second effect of the BCC alloy is to
work as an atomic hydrogen bridge which facilitates the
bridge which facilitates the pumping of H atoms into the
Mg/BCC interfaces and so, improves the 3rd step of the
hydrogenation process.
On the other hand, because the outer regions of the Mg
particles and their grain boundaries are completely hydro-
genated, the centres of grains may be unreachable for
hydrogen atoms. After a 2 h ball milling, CNTs retain their
nanotube structure, and they aggregate along the grain
boundaries of magnesium particles [28], so they may facili-
tate access of H-atoms to the magnesium grains, which
increases both the absorption kinetics and the hydrogen
storage capacity. Therefore, for the MgH2-BCC-CNT sample,
the effect of the CNTs is enhancement of the 2nd step by
improvement of the diffusion path of H-atoms along the
grain boundaries.
The desorption mechanism is the reverse process to the
absorption. The H-atoms interact with the BCC alloy to form
“BCC hydride” on the magnesium particle surfaces. In addi-
tion, CNTs (for the MgH2-BCC-CNT sample) facilitate the
emergence of hydrogen from the grain boundaries. Finally,
the BCC alloy recombines the H-atoms into hydrogen mole-
cules, with a resulting improvement in the dehydriding
kinetics and desorption temperature.
55 60 65 70 75 80
gree)
MgH2-BCC-CNT
MgH2-BCC
MgH2
Mg
MgO
*
O
& BCC
enlarged area in the inset shows the shift of the peak with
i n t e rn a t i o n a l j o u r n a l o f h y d r o g e n en e r g y 3 5 ( 2 0 1 0 ) 7 8 2 1e7 8 2 67826
4. Conclusion
Acomparisonbetween theeffects of theadditionof 10wt.%BCC
(Ti0.4Mn0.22Cr0.1V0.28) alloyand10wt.%BCCþ5wt.%CNTsonthe
hydrogen storage properties of MgH2 were investigated. The
results showed that homogeneously distributed catalysts
significantly improve the desorption temperature, the
maximum absorbed hydrogen and the hydriding/dehydriding
kinetics. The results showed that these additives have different
catalytic effects on the hydrogenation/dehydrogenation
processesofmagnesiumhydride. Theeffectsof theBCCalloyon
the hydrogenation could be reduction of the barrier energy for
dissociation of hydrogen molecules into hydrogen atoms and
also promotion of hydrogen pumping into the Mg/BCC inter-
faces, while CNTs (for the MgH2-BCC-CNT sample) facilitate
access of H-atoms to the interior of Mg grains. Furthermore,
during dehydrogenation, the “BCC hydride” forms on the Mg/
BCC interfaces, and then the BCC alloy releases H-atoms more
rapidly thanMg,while it also facilitates the recombination ofH-
atoms into H2 molecules. CNTs facilitate the emergence of
hydrogen from the grain boundaries during desorption.
Acknowledgments
This work was financially supported by the Australian
Research Council (ARC) through Discovery project grant
DP0771193. The authors would like to thank Dr. Tania Silver
and Dr. Darren Attard for their great helps.
r e f e r e n c e s
[1] Schlapbach L, Zuttel A. Hydrogen-storage materials formobile applications. Nature 2001;414:353e8.
[2] Shang CX, Guo ZX. Effect of carbon on hydrogen desorptionand absorption of mechanically milled MgH2. J Power Sourc2004;129(1):73e80.
[3] Huot J, Liang G, Schulz R. Mechanically alloyed metal hydridesystems. Appl Phys A Mater Sci Process 2001;72(2):187e95.
[4] Zaluski L, Zaluska A, Strom-Olsen JO. Hydrogenabsorption in nanocrystalline Mg2Ni formed bymechanical alloying. J Alloys Compd 1995;217(2):245e9.
[5] Wang XL, Tu JP, Zhang PL, Zhang XB, Chen CP, Zhao XB.Hydrogenation properties of ball-milled composite. Int JHydrogen Energy 2007;32(15):3406e10.
[6] Imamura H, Kitazawa I, Tanabe Y, Sakata Y. Hydrogenstorage in carbon/Mg nanocomposites synthesized by ballmilling. Int J Hydrogen Energy 2007;32(13):2408e11.
[7] Ranjbar A, Guo ZP, Yu XB, Wexler D, Calka A, Kim CJ, et al.Hydrogen storage properties of MgH2-SiC composites. MaterChem Phys 2009;114(1):168e72.
[8] Bobet J-L, Akiba E, Darriet B. Study of Mg-M (M¼Co, Ni and Fe)mixture elaborated by reactivemechanical alloying: hydrogensorption properties. Int J Hydrogen Energy 2001;26(5):493e501.
[9] Shang CX, Bououdina M, Guo ZX. Structural stability ofmechanically alloyed (Mgþ10Nb) and (MgH2þ10Nb) powdermixtures. J Alloys Compd 2003;349(1e2):217e23.
[10] Shang CX, Bououdina M, Song Y, Guo ZX. Mechanicalalloying and electronic simulations of (MgH2þM) systems(M¼Al, Ti, Fe, Ni, Cu and Nb) for hydrogen storage. Int JHydrogen Energy 2004;29(1):73e80.
[11] Huang ZG, Guo ZP, Calka A,Wexler D, Lukey C, Liu HK. Effectsof iron oxide (Fe2O3, Fe3O4) on hydrogen storage properties ofMg-based composites. J Alloys Compd 2006;422(1e2):299e304.
[12] Patah A, Takasaki A, Szmyd JS. Influence of multiple oxide(Cr2O3/Nb2O5) addition on the sorption kinetics of MgH2. IntJ Hydrogen Energy 2009;34(7):3032e7.
[13] Song M, Kwon I, Bae J-S. Development of hydrogen-storagealloys of Mg-Fe2O3 system by reactive mechanical grinding.Int J Hydrogen Energy 2005;30(10):1107e11.
[14] Liu X, Huang Z, Jiang L, Wang S. Thermal stabilization andhydrogen storage properties of Mg-40 wt%Ti0.28Cr0.50V0.22
composite prepared by mechanical milling. Int J HydrogenEnergy 2007;32(8):965e8.
[15] Huang ZG, Guo ZP, Calka A, Wexler D, Liu HK. Effects ofcarbon black, graphite and carbon nanotube additives onhydrogen storage properties of magnesium. J Alloys Compd2007;427(1e2):94e100.
[16] Huang ZG, Guo ZP, Calka A, Wexler D, Wu J, Notten PHL, et al.Noticeable improvement in the desorption temperature fromgraphite in rehydrogenated MgH2/graphite composite. MaterSci Eng A 2007;447(1e2):180e5.
[17] Ranjbar A, Guo ZP, Yu XB, Calka A, Liu HK. Hydrogen storageproperties of Mg-BCC composite. Int J Green Energy 2009;6:607e15.
[18] Kiyobayashi T, Komiyama K, Takeichi N, Tanaka H, Senoh H,Takeshita HT, et al. Hydrogenation of nanostructuredgraphite by mechanical grinding under hydrogenatmosphere. Mater Sci Eng B 2004;108(1e2):134e7.
[19] Yao X, Wu C, Du A, Lu GQ, Cheng H, Smith SC, et al. Mg-basednanocomposites with high capacity and fast kinetics forhydrogen storage. J Phys Chem B 2006;110(24):11697e703.
[20] Zaluska A, Zaluski L, Strom-Olsen JO. Nanocrystallinemagnesium for hydrogen storage. J Alloys Compd 1999;288(1e2):217e25.
[21] Liang G, Huot J, Boily S, Van Neste A, Schulz R. Catalyticeffect of transition metals on hydrogen sorption innanocrystalline ball milled MgH2-Tm (Tm¼Ti, V, Mn, Fe andNi) systems. J Alloys Compd 1999;292(1e2):247e52.
[22] SchulzR,Huot J,LiangG,BoilyS,LalandeG,DenisMC,etal.Recentdevelopments in the applications of nanocrystallinematerials tohydrogen technologies. Mater Sci Eng A 1999;267(2):240e5.
[23] Imamura H, Sakasai N, Fujinaga T. Characterization andhydriding properties of Mg-graphite composites preparedby mechanical grinding as new hydrogen storage materials.J Alloys Compd 1997;253e254:34e7.
[24] Aminorroaya S, Chob Y, Liua HK, Dahleb A. Microstructureand activation characteristics of Mg-Ni alloy modified byMulti-Walled carbon nanotubes. Int J Hydrogen Energy 2010;35:4144e53.
[25] DuAJ, Smith SC, Yao XD, LuGQ. Catalytic effects of Subsurfacecarbon in the Chemisorption of hydrogen on a Mg(0001)surface: an Ab-initio Study. J Phys Chem B 2006;110(4):1814e9.
[26] RanjbarA,GuoZP,YuXB,AttardD,CalkaA, LiuHK.Effects ofSiCnanoparticles with andwithout Ni on the hydrogen storageproperties of MgH2. Int J Hydrogen Energy 2009;34(17):7263e8.
[27] Du AJ, Smith AJ, Yao XD, Lu GQ. The Role of Ti as a catalystfor the dissociation of hydrogen on a Mg(0001) surface. J PhysChem B 2005;109(38):18037e41.
[28] Yao X, Wu C, Du A, Zou J, Zhu Z, Wang P, et al. Metallic andcarbon nanotube-catalyzed Coupling of hydrogenation inmagnesium. J Am Chem Soc 2007;129(50):15650e4.
[29] Yu XB, Guo YH, Yang ZX, Guo ZP, Liu HK, Dou SX. Synthesisof catalyzed magnesium hydride with low absorption/desorption temperature. Scr Mater 2009;61(5):469e72.
[30] Yu XB, Guo YH, Yang H, Wu Z, Grant DM, Walker GS.Improved hydrogen storage in magnesium hydride catalyzedby Nanosized Ti0.4Cr0.15Mn0.15V0.3 alloy. J Phys Chem C 2009;113(13):5324e8.