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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 3 5 ( 2 0 1 0 ) 4 1 3 1 – 4 1 3 7
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Effect of admixing different carbon structural variants on thedecomposition and hydrogen sorption kinetics ofmagnesium hydride
Rajesh Kumar Singh, Himanshu Raghubanshi, Sunil Kumar Pandey, O.N. Srivastava*
Hydrogen Energy Centre and Unit on Nano Science and Technology, Physics Department, Banaras Hindu University,
Varanasi 221005, U.P., India
a r t i c l e i n f o
Article history:
Received 4 October 2009
Received in revised form
1 February 2010
Accepted 1 February 2010
Available online 12 March 2010
Keywords:
Hydrogen storage materials
Thermal desorption
Kinetics
* Corresponding author. Tel.: þ91 542 368468E-mail address: [email protected] (O.N
0360-3199/$ – see front matter ª 2010 Profesdoi:10.1016/j.ijhydene.2010.02.015
a b s t r a c t
The effect of admixing catalysts comprised of carbon nanostructures, specifically planar,
helical and twisted carbon nanofibers, spherical carbon particles and multi-walled carbon
nanotubes, on the hydrogen storage properties of magnesium hydride has been investi-
gated. Optimum results were achieved with the mixture containing twisted carbon
nanofibers (TCNF) synthesized by Ni catalyst derived by oxidative dissociation of catalyst
precursor LaNi5. The desorption temperature of 2 wt.% TCNF admixed MgH2 is w65 K lower
than that of pristine MgH2 milled for the same duration. The enhancement in hydrogen
absorption capacity of MgH2 admixed with 2 wt.% TCNF has been found to be two-fold in
the first 10 minutes at 573 K and under a hydrogen pressure of 2 MPa, i.e. 4.8wt% as
compared to 2.5 wt% for MgH2 alone. The increase in capacity by a factor of about two
within the first 10 minutes as a result of the catalytic activity of TCNF is one of the exciting
results obtained for hydrogen absorption in catalyzed MgH2.
ª 2010 Professor T. Nejat Veziroglu. Published by Elsevier Ltd. All rights reserved.
1. Introduction and to increase sorption kinetics, ball-milling to reduce
Hydrogen is the most abundant element on the earth and is
a promising medium for both energy transmission and
storage. Hydrogen has to be conveniently and economically
stored before it can be used as a clean fuel in IC engines or fuel
cells. For hydrogen storage, solid state (metallic as well as
complex hydrides) has potential advantages over compressed
and liquid hydrogen storage [1–3]. The gravimetric hydrogen
densities for AB5 [4] AB2, AB and A2B type metal hydrides are
usually less than 3 wt% except for MgH2 and Mg2NiH4. Mg is
cheap and found in abundance in the earth’s crust. Magne-
sium hydride has high gravimetric (7.6 wt %) as well as volu-
metric (w110 kg H2/m3) capacity. However, MgH2 is too stable
and its absorption and desorption requires high temperature
(>573 K) [5]. In order to decrease decomposition temperature
; fax: þ91 542 2369889.. Srivastava).sor T. Nejat Veziroglu. Pu
particle size [5–7] and admixing with catalysts have been
extensively studied [8–37]. Several catalysts such as transition
metals [8–12], metal oxides [13–17], halides [18–20], interme-
tallic compounds that absorb hydrogen [21–23] and different
forms of carbon [24–33] have been used to improve sorption
kinetics and to lower the desorption temperature.
Graphite, activated carbon, carbon nanoforms (single/
multi walled carbon nano tubes (S/MWCNT), carbon nano-
fibres (CNF), fullerenes, etc.) have been used as catalysts for
MgH2, hydrides of intermetallics (e.g. LaNi5) and complex
hydrides (e.g.NaAlH4). Several studies have been carried out to
explore the catalytic effect of different carbon forms on
magnesium hydride. In these investigations S/MWCNT has
been found to show quite good catalytic property [30,32].
However, few studies have been done to evaluate the catalytic
blished by Elsevier Ltd. All rights reserved.
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 3 5 ( 2 0 1 0 ) 4 1 3 1 – 4 1 3 74132
effect of carbon nanofibres. The catalytic effect of different
forms of carbon admixed with MgH2 has been investigated by
Lillo Rodenas et al. [27]. The results show that a nanofibre with
a small amount of metal (especially Ni, Fe) acts as a catalyst to
improve hydrogen storage property. The effect of carbon
supported nickel catalyst on MgH2 has also been studied [31].
These studies have shown that the interaction between
carbon and nanometric nickel lead to a decrease in decom-
position temperature.
Here, we have synthesized different carbon nano-
structures (CNSs) and studied their catalytic effect on the
absorption kinetics and decomposition temperature of MgH2.
It has been found that a small amount of (2wt%) CNS admixed
with MgH2 exhibits improved hydrogen storage properties. In
particular MgH2 admixed with 2 wt% twisted CNF (MgH2-
2TCNF) exhibited the optimum hydrogenation/dehydrogena-
tion among all admixed samples tested.
2. Experimental details
2.1. Synthesis of different carbon structures
Synthesis of CNF was performed by employing the catalytic
chemical vapor deposition (CCVD) method involving thermal
decomposition of carbon-rich acetylene (C2H2) gas. For an
effective thermal cracking, fine particles of catalyst precursor
of LaNi5 and ZrFe2 were used. The silica tube was evacuated
up to 10�4 torr in order to avoid oxidation of catalyst at high
temperature. Hydrogen and acetylene gas in the ratio 1:4 was
admitted to the silica tube at a total pressure of w450 torr (90
torr for H2 and 360 torr for C2H2). Thermal cracking of the
gases was achieved by heating in the presence of the above-
mentioned catalyst powders at different temperatures for
2 hours in a resistance heated furnace. At this stage the
carbon gets deposited inside the tube where the catalyst
precursor was located. TEM investigations have confirmed
that carbon nanofibres get formed on nano nickel catalyst
formed by oxidative dissociation of LaNi5.
X-ray diffraction analysis of sample was carried out with
an Xpert Pro (Panalytical) diffractometer employing CuKa
radiation (l¼ 1.54 A). The microstructural features were
monitored by Scanning Electron Microscopy (SEM) (Philips,
XL-20) using secondary electron imaging. Transmission elec-
tron microscopy (TEM) observations were performed using
a Technai 20 G2 microscope.
Planar, helical and twisted CNFs were formed by using
LaNi5 alloy as catalyst precursor. At 550 �C, by the interaction
of acetylene gas, LaNi5 produces spherical particles of Ni
which were decisive for the growth of planar CNFs (PCNFs).
The length of these CNFs was in the range of 6–7 mm and
average diameter was 300 nm (Fig. 1(a)). The diffraction
pattern in the TEM image shown in the inset on the upper
right corner of Fig. 1(a) confirms that the structures formed
were CNFs having platelet morphology. However, at 650 �C, by
the interaction of acetylene gas, LaNi5 produces faceted
polygonal particles of Ni which were decisive for the growth of
Helical and Twisted CNFs (HCNFs and TCNFs). HCNFs were
synthesized by using LaNi5 as a catalyst precursor at 650 �C for
30 minutes in the flowing gas environment. Average length of
these CNFs was 15 mm and average diameter was 2 mm
(Fig. 1(b)). TCNFs were synthesized by employing Ni as catalyst
derived through oxidative dissociation of LaNi5 at 650 �C for
2 hours. The length of these CNFs was in the range of 6–7 mm
and average diameter was 200 nm (Fig. 1(c)). The diffraction
patterns shown in the insets in the upper right corners of
Fig. 1(b) and (c) shows that the CNFs have herringbone
morphology. Spherical carbon particles (SCPs) were synthe-
sized by using ZrFe2 as a catalyst at 650 �C for 30 minutes in
the flowing gas environment (Fig. 1(d)). The details of the
synthesis of various forms of CNF are being studied and will be
published elsewhere.
The MWCNTs used in the present investigation were
synthesized by chemical vapor deposition technique using
ferrocene dissolved in benzene precursor. Details of the
synthesis process of CNTs have already been described by our
group on carbon nanomaterials [34,35]. The optimum flow
rate and concentration of ferrocene in benzene were found to
be w2 ml/min and 50 mg/ml. The SEM micrographs of as-
grown CNTs are shown in Fig. 2(a). The as-grown CNTs are
multi-walled as seen from the TEM image (Fig. 2(b)). The inset
in Fig. 2(b) shows HRTEM image of MWCNTs clearly showing
the multi-walled structure.
2.2. Ball-milling and hydrogen sorption measurement
The commercial MgH2 (Alfa Aesar 98%) was used as received.
Admixing was done by mechanical milling using a locally
fabricated miller. This consisted of a chrome steel vial with
a volume of 110 cm3. This contained two steel balls of
12.5 mm diameter and one steel ball with 4 mm diameter.
The miller was kept in an argon-filled glove box. All material
handling (including weighing and loading) was performed in
an argon (high purity)-filled glove box. Through several trial
runs employing varying concentration of CNS, it was found
that optimum admixing occurred for 1gm of as-obtained
MgH2 and 2wt% of CNS admixed through milling at 500 rpm
for 10 minutes. For comparison MgH2 was also milled alone
for 10 minutes under similar conditions and then used for
analysis. Henceforth this milled MgH2 will be referred to
simply as MgH2.
Hydrogenation/dehydrogenation properties were measured
through P–C–T system (Advanced Materials Corporation,
Pittsburgh, PA, USA) attached to a Furnace controlled to within
an accuracy of �2 K. A 300-mg sample was loaded in a cylin-
drical SS reactor for each measurement. The hydrogen
desorption behaviour was monitored under a primary vacuum
of 10�3 torr. Thermal desorption of the ball-milled samples was
performed using a computer-programmed furnace under
dynamic heating condition (5 K/min). After loading the sample,
the system was first evacuated by a rotary pump. The absorp-
tion was carried out under 2 MPa pressure of high purity
hydrogen gas at an operating temperature of 573 K.
3. Results and discussions
All CNSs were synthesized and admixed without purification
since. as stated earlier, carbon and metal particle interaction
also plays a positive catalytic effect in MgH2.
Fig. 1 – SEM images of different carbon structures (a) planar CNF (b) helical CNF (c)twisted CNF and (d) spherical carbon
particles. Inset of (a), (b) and (c) shows the diffraction pattern obtained by transmission electron microscope.
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 3 5 ( 2 0 1 0 ) 4 1 3 1 – 4 1 3 7 4133
3.1. SEM analysis results
The morphologies of the as-received MgH2 sample and
10-minute ball-milled TCNF admixed MgH2 as revealed by
SEM are presented in Fig. 2(c) and (d). Particle size of as-
Fig. 2 – (a). SEM images of MWCNT (b) TEM image of MWCNT (Ins
as-received MgH2 and ball-milled MgH2.
received MgH2 observed from Fig. 2(c) seems to be in the
range of w 50-100 mm. After milling of MgH2 and CNS admixed
MgH2 the particle size of MgH2 is reduced to w5-10 mm and it
seems to be flattened. The microstructure of CNS is not
discernible since it is present in very small quantity (2% of the
et shows HRTEM image of MWCNT) (c) and (d) SEM image of
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 3 5 ( 2 0 1 0 ) 4 1 3 1 – 4 1 3 74134
weight of MgH2). Analysis of SEM micrographs of ball-milled
MgH2 and different CNS admixed samples show no signifi-
cant difference in the particle morphology and hence are not
presented here.
Fig. 4 – Hydrogen absorption curve of 2-wt% CNS admixed
Mg at 573 K and an applied pressure of 2 MPa.
3.2. Hydrogen desorption/absorption on CNS-catalyzedMgH2
Fig. 3 shows the temperature programmed desorption curve of
MgH2 and different catalytic CNS-MgH2 admixtures at a heat-
ing rate of 5 K/min in a closed chamber. To avoid the effect of
increased pressure on desorption temperature, equal weights
of each sample were taken for comparison. As seen from the
figure the starting H -desorption temperature is 695 K for
MgH2, 653 K for SCP and MWCNT, 623 K for HCNF, 613 K for
PCNF and 603 K for TCNF admixed MgH2 respectively. It can
also be seen from the figure that there is a temperature shift in
the starting H-desorption temperature of about 90 K for 2wt%
TCNF admixed sample as compared to MgH2. The hydrogen
desorption temperature gets lowered by w65 K in the case of
optimum catalyst.
Fig. 4 presents a comparative study of hydrogen absorption
behaviour of desorbed MgH2 and different CNS admixed des-
orbed MgH2 samples at 300 �C and an applied pressure of
2 MPa. It was observed that the absorption kinetics of MgH2
are considerably improved by admixing different CNSs. It can
also be seen from the figure that MgH2-2TCNF shows 4.8 wt%
absorption as compared to 2.5 wt% for MgH2 alone in the first
10 minutes. The absorption rate for the first 10 minutes for
MgH2 -2TCNF is 0.48 wt%/min which is w200% higher
compared to some of the recently reported rates for catalyzed
MgH2, for example Nb2O5-catalyzed MgH2 ball-milled for
40 hours by V.V. Bhat et al. [36]. In the work of C.Z. Wu et al.
[30,32] absorption kinetics were higher than in our case, which
may be due to longer ball-milling time, which has an effect on
absorption rate. However, the decomposition temperature in
these studies is still higher than that in the present investi-
gation. Some other workers have also reported absorption
Fig. 3 – Thermal desorption of hydrogen from 2-wt% CNS
admixed MgH2 heating @ 5 K/min.
rates better than our results but these are for samples ball-
milled for more than 5 hours.
The X-ray diffractograms of as-received MgH2, 10-minute
milled MgH2 with 2 wt% TCNF and MgH2 after 5th cycle of
hydrogenation/dehydrogenation are shown in Fig. 5(a)–(c)
respectively. After milling the main phases of the sample
remained b MgH2. A change in intensity and peak width of the
samples after the 5th cycle was observed which is due to an
increase in crystallite size of MgH2 due to crystallization.
A small amount of unhydrided Mg is also present; this leads to
a decrease in storage capacity. This unhydrided Mg may be
present due to high energy impact of balls during milling. It is
possible to hydrogenate unhydrided Mg by applying pressure
higher than 5 MPa at 300 �C for 2 hours.
Fig. 5 – XRD patterns of (a) as-received MgH2 (b) 10-minute
ball-milled MgH2 (c) MgH2 after five dehydriding/hydriding
cycles.
Fig. 7 – Plot of ln[Lln(1 L a)] vs ln(t) of Mg-2TCNF at
553 K,573 K and 593 K. Inset shows ln k vs 1/T plot of Mg
and Mg-2TCNF.
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 3 5 ( 2 0 1 0 ) 4 1 3 1 – 4 1 3 7 4135
Fig. 6 shows the XRD of as-synthesized TCNF without
purification. The presence of a graphitic carbon peak arising
from CNF, and La2O3 and Ni peaks from chemical decompo-
sition of native catalyst particles (LaNis) [37] can be clearly
seen. Ni particles are known to have better catalytic activity
for dissociation of hydrogen molecules to atoms [9,11] and
carbon facilitates the diffusion of H in MgH2 [30,32]. Several
workers found that the interaction of carbon and Ni enhances
hydrogen storage behaviour [38,39] and act as a better catalyst
also [27,31]. Therefore, enhancement in the hydrogen storage
properties of MgH2-TCNF can be taken to be the combined
interactive effect of Ni and carbon. In order to confirm this we
have admixed 2 wt% of purified TCNF and 2 wt% of Ni sepa-
rately as catalyst in MgH2. In both cases hydrogen storage
properties were enhanced as compared to milled MgH2 but
less than that of MgH2 catalyzed through TCNF with Ni cata-
lyst which stands as impurity in the CNF matrix. HCNF and
PCNF have also been synthesized mainly by Ni but the catalyst
used is in the micrometer range which, on synthesis, breaks
into smaller size particles w >250 nm.
As can be seen from Figs. 3 and 4 all the three types of
fibres, namely PCNF, TCNF and HCNF, were found to signifi-
cantly catalyze the sorption characteristics of Mg/MgH2. The
diameter of the CNF depends on the size of the catalyst
formed during the synthesis process. The typical SEM micro-
graphs of TCNF and PCNF as shown in Fig. 1(a) and (c) reveal
that the diameter of PCNF (>300 nm) is larger than that of
TCNF (<200 nm). Since the size of the catalyst particle decides
the diameter of the CNF, the nickel catalyst particle leading to
growth of PCNF can be taken to be>300 nm while that of TCNF
<200 nm. The larger size Ni particle is expected to have
a lower degree of carbon-nickel interaction than that of
smaller particles as in the case of TCNF. This will lead to
higher catalytic activity for TCNF. The interaction of catalyst
with carbon in the CNF is mainly at tip on which it grows. In
the case of HCNF the length of the fibre is much larger as
compared to PCNF and TCNF. Due to this, carbon-nickel
interaction is of lower degree. This is most probably the
Fig. 6 – XRD pattern of as-synthesized TCNF prepared by
employing LaNi5 as catalyst.
reason for the less effective catalytic behaviour of HGNF as
compared to PCNF and TCNF. The catalyst used in case of
MWCNT and SCP is Fe based and hence does not show
prominent effect.
We have also calculated the activation energy for hydrogen
absorption in MgH2 as well as the optimum catalyzed material
MgH2-2TCNF. The activation energies Ea, for the hydrogen
absorption of samples MgH2-2TCNF and MgH2 were estimated
from an Arrehenius plot, which can be derived from the
equation:
k ¼ Ae�Ea=RT
The absorption curves in Fig. 4 are not linear. Therefore the
rate constant k was obtained by the kinetic model for nucle-
ation and crystal growth in solids formulated by John-Mehl-
Avrami [40] outlined in the following equation:
½ � lnð1� aÞ�1=n¼ kt
where, a is the extent of the reaction which can be identified
with a normalized hydrogen wt% (range: from 0 to 1), t is the
time and k and n are constants (at constant temperature).
The logarithmic transform of the above equation has
been used to construct a graph of ln [�ln(1� a)] vs. ln(t) in
which isothermal experimental data are linear. The loga-
rithmic transforms of the equation as calculated from
hydrogenation curves at (a) 553 K, (b) 573 K and (c) 593 K for
Mg-2TCNF are shown in Fig. 7. The dependence of ln k on the
inverse temperature is shown in the inset of Fig. 7 for
hydrogenation of MgH2 and MgH2-2TCNF. From the slope of
the Arrhenius plot of ln k vs 1/T, the activation energy has
been calculated. The activation energy Ea, obtained from the
curve for absorption of hydrogen in Mg-2TCNF is 66 kJ/mol
H2 and 98 kJ/mol H2 for pure MgH2 (milled). This value is
lower than that for the formation of MgH2 calculated in
earlier studies.
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 3 5 ( 2 0 1 0 ) 4 1 3 1 – 4 1 3 74136
4. Conclusions
The starting H-desorption temperature is 695 K for pure MgH2,
653 K for SCP and MWCNT, 623 K for HCNF, 613 K for PCNF and
the least 603 K (the lowest) for TCNF admixed MgH2 respec-
tively. For the first 10 minutes Mg-2TCNF shows 4.8 wt%
absorption as compared to 2.5 wt% for pure Mg H2. This shows
about a two-fold enhancement in the absorption rate. The
activation energy for the absorption comes out to be 66 kJ/mol
H2 for twisted CNF admixed MgH2 as compared to 98 kJ/mol H2
for pure MgH2.
Acknowledgements
The authors are grateful to Prof. T.N. Veziroglu (President, IAHE
Florida USA) and Prof. M. Groll (Stuttgart, Germany) for helpful
discussions. Financial assistance from CSIR (New Delhi, India),
UNANST (DST) and Ministry of New and Renewable Energy
(New Delhi, India) is gratefully acknowledged.
r e f e r e n c e s
[1] Schlapbach L, Zuttel A. Hydrogen-storage materials formobile applications. Nature 2001;414:353–8.
[2] Zuttel A. Materials for hydrogen storage. Mater Today 2003;6:24–33.
[3] Hudson MSL, Dubey PK, Pukazhselvan D, Pandey SK,Singh RK, Raghubanshi H, et al. Hydrogen energy in changingenvironmental scenario: Indian context. Int J HydrogenEnergy 2009;34:7358–67.
[4] Singh RK, Lototsky MV, Srivastava ON. Thermodynamical,structural, hydrogen storage properties and simulationstudies of P–C isotherms of (La, Mm) Ni5-yFey. Int J HydrogenEnergy 2007;32:2971–6.
[5] Imamura H, Masanari K, Kusuhara M, Katsumoto H, Sumi T,Sakata Y. High hydrogen storage capacity of nanosizedmagnesium synthesized by high energy ball-milling. J AlloysCompds 2005;386:211–6.
[6] Zaluska A, Zaluski L, Strom-Olsen JO. Nanocrystallinemagnesium for hydrogen storage. J Alloys Compds 1999;288:217–25.
[7] Gross KJ, Spatz P, Zuttel A. Mechanically milled Mgcomposites for hydrogen storagedthe transition to a steadystate composition. J Alloys Compds 1996;240:206–13.
[8] Denis A, Sellier E, Aymonier C, Bobet JL. Hydrogen sorptionproperties of magnesium particles decorated with metallicnanoparticles as catalyst. J Alloys Compds 2009;e476:152–9.
[9] Liang G, Huot J, Boily S, Nestea AV, Schulz R. Catalytic effectof transition metals on hydrogen sorption in nanocrystallineball milled MgH2–Tm (Tm ¼ Ti, V, Mn, Fe and Ni) systems.J Alloys Compds 1999;292(1–2):247–52.
[10] Shang CX, Bououdina M, Song Y, et al. Mechanical alloyingand electronic simulations of (MgH2 þ M) systems (M-Al, Ti,Fe, Ni, Cu and Nb) for hydrogen storage. Int J HydrogenEnergy 2004;29:73–80.
[11] Hanada N, Ichikawa T, Fuji H. Catalytic effect of nanoparticle3dtransition metals on hydrogen storage properties inmagnesium hydride MgH2 prepared by mechanical milling.J Phys Chem B 2005;109:7188–94.
[12] Barkhordarian G, Klassen T, Bormann R. Catalyticmechanism of transition-metal compounds on Mg hydrogensorption reaction. J Phys Chem B 2006;110:11020–4.
[13] Song MY, Kwon IH, Kwon SN, Park CG, Park HR, Bae J- S.Preparation of hydrogen-storage alloy Mg–10 wt% Fe2O3
under various milling conditions. Int J Hydrogen Energy 2006;31:43–7.
[14] Dehouche Z, Klassen T, Oelerich W, Goyette J, Bose TK,Schulz R. Cycling and thermal stability of nanostructuredMgH2–Cr2O3 composite for hydrogen storage. J AlloysCompds 2002;347:319–23.
[15] Song MY, Bobet JL, Darriet B. Improvement in hydrogensorption properties of Mg by reactive mechanical grindingwith Cr2O3, Al2O3 and CeO2. J Alloys Compds 2002;340:256–62.
[16] Barkhordarian G, Klassen T, Bormann R. Fast hydrogensorption kinetics of nanocrystalline Mg using Nb2O5 ascatalyst. Scr Mater 2003;49:213–7.
[17] Aguey-Zinsou KF, Fernandez JRA, Klassen T, Bormann R.Effect of Nb2O5 on MgH2 properties during mechanicalmilling. Int J Hydrogen Energy 2007;32:2400–7.
[18] Xie L, Liu Y, Wang YT, Zheng J, Li XG. Superior hydrogenstorage kinetics of MgH2 nanoparticles doped with TiF3. ActaMater 2007;55:4585–91.
[19] Reule Yavari AR, LeMoulec A, de Castro FR, Deledda S,Friedrichs O, Botta WJ, et al. Improvement in H-sorptionkinetics of MgH2 powders by using Fe nanoparticles generatedby reactive FeF3 addition. Scr Mater 2005;52:719–24.
[20] Jin SA, Shim JH, Cho YW, Yi KW. Dehydrogenation andhydrogenation characteristics of MgH2 with transition metalfluorides. J Power Sources 2007;172:859–62.
[21] RamanSai SS, Srivastava ON. Hydrogenation behaviour ofthe new composite storage material Mg–x wt% CFMmNi5.J Alloys Compds 1996;241:167–74.
[22] Davidson DJ, Sai Raman SS, Srivastava ON. Investigation onthe synthesis, characterization and hydrogenationbehaviour of new Mg based composite materials Mg–x wt%MmNiFe prepared through mechanical alloying. J AlloysCompds 1999;292:194–201.
[23] Kondo T, Shindo K, Sakurai Y. Dependence of hydrogenstorage characteristics of Mg-TiFe0.92Mn0.08 composite onamount of TiFe0.92Mn0.08. J Alloys Compds 2005;404:511–4.
[24] Fujii H, Orimo S. Hydrogen storage properties in nano-structured magnesium- and carbon-related materials.Physica B 2003;328:77–80.
[25] Shang CX, Guo ZX. Effect of carbon on hydrogen desorptionand absorption of mechanically milled MgH2. J PowerSources 2004;129:73–80.
[26] Imamura H, Kusuhara M, Minami S, Matsumoto M,Masanari K, Sakata Y, et al. Carbon nanocompositessynthesized by high-energy mechanical milling of graphiteand magnesium for hydrogen storage. Acta Mater 2003;51:6407–14.
[27] Lillo-Rodenas MA, Guo ZX, Aguey-Zinsou KF, Cazorla-Amoros D, Linares-Solano A. Effects of different carbonmaterials on MgH2 decomposition. Carbon 2008;46:126–37.
[28] Takasaki A, Furuya Y, Katayama M. Mechanical alloying ofgraphite and magnesium powders, and their hydrogenation.J Alloys Compds 2007;446:110–3.
[29] Narayanan DL, Lueking AD. Mechanically milled coal andmagnesium composites for hydrogen storage. Carbon 2007;45:805–20.
[30] Wu CZ, Wang P, Yao X, Liu C, Chen DM, Lu GQ, et al. Effect ofcarbon/noncarbon addition on hydrogen storage behaviorsof magnesium hydride. J Alloys Compds 2006;414:259–64.
[31] Lillo-Rodenas MA, Aguey-Zinsou KF, Cazorla-Amors D,Linares-Solano A, Guo ZX. Effects of Carbon-SupportedNickel Catalysts on MgH2 Decomposition. J Phys Chem C2008;112(15):5984–92.
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 3 5 ( 2 0 1 0 ) 4 1 3 1 – 4 1 3 7 4137
[32] Wu CZ, Wang P, Yao X, Liu C, Chen DM, Lu GQ, et al.Hydrogen storage properties of MgH2/SWNT compositeprepared by ball milling. J Alloys Compds 2006;420:278–82.
[33] Yao X, Wu CZ, Wang H, Cheng HM, Lu GQ. Effects of carbonnanotubes and metal catalysts on hydrogen storage inmagnesium nanocomposites. J Nanosci Nanotech 2006;6:494–8.
[34] Srivastava A, Srivastava ON, Talapatra S, Vajtai R,Ajayan PM. Carbon nanotube filters. Nat Mater 2004;3:610–4.
[35] Awasthi K, Srivastava AK, Srivastava ON. Synthesis ofcarbon nanotubes. J Nanosci Nanotech 2005;5:1616–36.
[36] Bhat VV, Rougier A, Aymard L, Nazri GA, Tarascon J.- M. Highsurface area niobium oxides as catalysts for improved
hydrogen sorption properties of ball milled MgH2. J AlloysCompds 2008;460:507–12.
[37] Gao XP, Qin X, Wu F, Liu H, Lan Y, Fan SS, et al. Synthesis ofcarbon nanotubes by catalytic decomposition of methaneusing LaNi5 hydrogen storage alloy as a catalyst. Chem PhysLett 2000;327:271–6.
[38] Zubizarreta L, Menendez JA, Pis JJ, Arenillas A. Improvinghydrogen storage in Ni-doped carbon nanospheres. Int JHydrogen Energy 2009;34:3070–6.
[39] Kim HS, Lee H, Han KS, Kim JH, Song MS, Park MS, et al.Hydrogen storage in Ni nanoparticle-dispersed multiwalledcarbon nanotubes. J Phys Chem B 2005;109:8983–6.
[40] Avrami M. Kinetics of phase change. III: granulation, phasechange and microstructures. J Chem Phys 1941;9:177.