& beltramini, jorge n. file... · 1 low-temperature hydrogen desorption from mg(bh 4) 2...
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This is the author’s version of a work that was submitted/accepted for pub-lication in the following source:
Wahab, Mohammad A, Young, David J., Karim, Azharul, Fawzia, Sabrina,& Beltramini, Jorge N.(2016)Low-temperature hydrogen desorption from Mg(BH4)2 catalysed by Ultra-fine Ni nanoparticles in a Mesoporous Carbon Matrix.Low-temperature hydrogen desorption from Mg(BH4)2 catalysed by Ultra-fine Ni nanoparticles in a Mesoporous Carbon Matrix, 41(45), pp. 20573-20582.
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https://doi.org/http://dx.doi.org.ezp01.library.qut.edu.au/10.1016/j.ijhydene.2016.09.098
1
Low-temperature hydrogen desorption from
Mg(BH4)2 catalysed by Ultrafine Ni nanoparticles
in a Mesoporous Carbon Matrix
Mohammad A. Wahab*abc
, David J. Youngc, Azharul Karim
b, Sabrina Fawzia
d, and Jorge
N. Beltraminia
aARC Centre for Functional Nanomaterials, Australian Institute for Bioengineering and
Nanotechnology, The University of Queensland, Brisbane, St Lucia, QLD 4072, Australia
*E-mail: [email protected]; [email protected]
bChemistry, Physics and Mechanical Engineering, Science and Engineering Faculty, Queensland
University of Technology, 2 George Street, QLD 4001 Australia and
*Email: [email protected]
c Faculty of Science, Health, Education and Engineering, University of the Sunshine Coast,
Maroochydore DC, Queensland 4558, Australia.
*Email: [email protected]
dScience and Engineering Faculty, Civil Engineering and Built Environmental Science.
Queensland University of Technology, 2 George Street, QLD 4001 Australia.
2
Abstract: Homogenously dispersed, ultrafine Ni nanoparticles (Ni NPs) have been grown in a
mesoporous carbon (MC) matrix (MC-Niinsitu) and efficiently catalyze low-temperature hydrogen
desorption from Mg(BH4)2. The onset desorption temperature (Tonset) of this MC-Niinsitu-
Mg(BH4)2 system is 44 oC compared to 275
oC (Tonset) for pure Mg(BH4)2. This is the lowest
value reported for hydrogen desorption from this metal hydride. The activation energy (Ea) of
MC-Niinsitu-Mg(BH4)2 was determined to be 21.3 kJ/mol which is less than half the value of 45.9
kJ/mol for pure Mg(BH4)2. We ascribe this reduction to the synergistic effects of
nanoconfinement and the homogeneously dispersed, ultrafine Ni NPs active sites in the
mesoporous carbon.
Keywords: Hydrogen storage, Mg(BH4)2, Porous carbon, Nanoconfinement, Catalysis,
Synergistic effects
3
Introduction
Utilizing hydrogen (H2) as a clean energy source has been intensively investigated because of the
adverse environmental effects of burning fossil fuels [1-9]. Various hydrogen storage systems
have been demonstrated, but the realization of an efficient catch-release system is elusive [1-15].
Magnesium borohydride (Mg(BH4)2) is a promising hydrogen storage material with a high
gravimetric capacity of 14.8 wt% H2 and volumetric capacity of 112.5 kgm-3
[5-14], which can
meet the targets of 7.5 wt% and 50 kg m-3
set by the US Department of Energy (DoE). However,
its slow kinetics and unfavorably high onset H2 desorption temperature (Tonset) (270 OC - 280
OC)
currently limits its potential for this application [7-14]. Mixing Mg(BH4)2 with other
compounds/dopants has been investigated as a possible solution [7-17]. For example, the
Mg(BH4)2 - LiNH2 system released hydrogen at 170-180 OC due to the combined reaction of
[BH4]- and [NH2]
- but unfortunately the formation of poisonous NH3 during the decomposition
reactions limits its practical application [11]. A mixture of LiBH4 and Mg(BH4)2 also prepared by
ball-milling exhibited fewer decomposition steps but the first Tonset of this mixture was 235 OC,
exhibiting no significant reduction compared to pure Mg(BH4)2 [12]. Previous studies involving
extensive ball-milling of Mg(BH4)2 with TiO2, TiH2 or Ti for 2h produced material that mostly
desorbed hydrogen from a temperature of 227 oC.
10 Similarly, the ball-milling of Mg(BH4)2 with
Al was found to desorb H2 at 150 OC with a total desorption of 3.6 wt.% H2 at 300
OC in 2 h
[13]. These desorption temperatures are still too high for Mg(BH4)2 to be a practical hydrogen
reservoir. Additionally, several strategies including doping catalysts, the use of binary mixtures
of two hydrides, creating reactive composites, employing gas-solid reactions, forming
ammoniates, nanoconfinement of hydrogen precursors, exploiting dual-tuning effects of metal
hydrides and their dopants with high energy ball-milling and post-addition methods have been
4
reported to improve the hydrogen storage properties of mostly magnesium hydride-based
systems [14-18].
Recently, it has been reported that the nanoconfinement of a metal hydride within a porous
scaffold (e.g. mesoporous carbon, carbon aerogel or catalyst functionalized porous carbon) with
high surface area can reduce the Tonset, improving desorption kinetics because the porous scaffold
can contribute to the efficiency of the catalytic system [6, 8, 14, 19 - 32]. The encapsulation of
LiBH4 in pure porous carbon, for example, decreased the Tonset to 100-150 OC from 400
OC for
bulk LiBH4 [19]. The Tonset for Mg(BH4)2 confined in a disordered activated carbon reduced the
Tonset to 170 OC
and was further reduced to 75
OC when Mg(BH4)2 was incorporated into Ni
particles containing mesoporous carbon [14]. The latter study incorporated Ni nanoparticles into
the pores of a mesoporous carbon framework post-synthesis, yielding Ni NPs in the range 10 -
20 nm in size [14]. No impurities were observed during the desorption process which is
consistent with other mesoporous carbon-based nanoconfined systems [14, 26, 50]. Liu et al, for
example, evaluated the decomposition behavior of eutectic LiBH4−Mg(BH4)2 confined in
ordered porous carbon [31]. The decomposition temperatures of this system were in the range
270 to 350 OC, essentially falling between that of pure LiBH4 and Mg(BH4)2. Nanoconfinement
of these hydride materials did not produce diborane and triborane impurities. Javadian et al [27]
have described the melt-infiltration of a mixture of LiBH4 and Mg(BH4)2 in an activated carbon
aerogel with the resulting Tonset of 115-125 OC, still well short of the target working temperatures
for hydrogen storage applications [7-14]. In-situ, nanoconfined growth allows ultrafine Ni
nanoparticle catalysts to be finely dispersed, in mesoporous carbon for better performance. These
Ni nanoparticles are found to be well-distributed in mesoporous channels and to be of uniform
5
size [22,23,25-30]. The use of this material could bring metal hydrides and catalysts into more
intimate contact than is possible with other scaffolds.
We herein report the in-situ growth of nanoconfined and highly dispersed Ni nanoparticles
throughout a mesoporous carbon framework (MC-Niinsitu) and compare the catalytic
dehydrogenation of Mg(BH4)2 in this matrix to that of the same metal hydride in mesoporous
carbon alone. Nanoconfinement not only limits particle growth and aggregation of particles, but
also creates a shorter diffusion path with a lower energy barrier between Mg(BH4)2 and the
homogeneously dispersed Ni NPs. We have found that this confined MC-Niinsitu-Mg(BH4)2
system releases hydrogen at ~ 44 oC with a peak temperature (Tmax) at 141
OC, a remarkable
reduction of about 226 OC relative to previously reported systems. The activation energy (Ea) of
MC-Niinsitu-Mg(BH4)2 and kinetics of dehydrogenation are also reported.
Experimental
Methods and materials: Tetraethylorthosilicate (TEOS), pluronic surfactant P123
(EO20PPO70EO20), magnesium borohydride (Mg(BH4)2), sucrose, and Ni(NO3)2·6H2O from
Sigma-Aldrich were used without further purification. Hydrofluoric acid (HF), tetrahydrofuran
(THF), diethyl ether, ethanol, 2M NaOH and sulphuric acid (H2SO4) were also used as received.
Preparation of mesoporous SBA15 silica template: A surfactant solution containing 2 g of
P123 in 60 ml of 2M HCl was stirred vigorously at 38 OC for 2 h. TEOS (4.2 g) was slowly
added to the surfactant solution and stirring was continued for another 6 - 8 min and then the
solution left without stirring for 24 h at 38 OC [14,23,33-35]. The mixture was then put into an
autoclave for 48 h at 100 OC, filtered and the precipitate dried. Finally, as-prepared SBA15 silica
was calcined at 550 OC for 6 h in air for producing pure SBA15 silica template (Fig.1a).
6
Synthesis of mesoporous carbon (MC): A mixture of sucrose (1.25 g), water (5.0 mL) and
H2SO4 (0.14 g) was prepared and mesoporous SBA15 silica (1.0 g) was added slowly with
continual stirring for 5-6 h. Thermal polymerization was conducted at 100 OC for 6 h and then at
160 OC for another 6 h. Another 5.0 mL of aqueous solution containing 0.8 g of sucrose and 0.09
g of conc. H2SO4 was added to the above polymerized sample. Thermal polymerization was
repeated using the same conditions [14,23]. Finally, mesoporous SBA-15 silica/carbon
nanocomposite was carbonized in a conventional furnace at 850 OC under a nitrogen flow. The
carbonized nanocomposite sample was stirred in an aqueous solution of 7-wt% hydrogen
fluoride (HF) to dissolve the SBA15 silica template, thereby creating the mesoporous carbon
(MC) framework.
Synthesis of MC-Niinsitu: A Ni source Ni(NO3)2·6H2O was added to SBA15 using a two-step
procedure. Sucrose (1.25 g) and a predetermined amount of Ni(NO3)2·6H2O precursor was added
into 7 mL of H2O containing 0.14 g of conc. H2SO4. The mixture was stirred for several hours
and then 1 g of SBA15 was added and the mixture stirred for another 6 h. Thermal
polymerisation was carried out at 100 oC for 6 h and then at 160
oC for 6 h. This procedure was
then repeated with the addition of a solution containing 0.8 g sucrose and a pre-determined
amount of Ni(NO3)2·6H2O precursor in 5 mL of H2O with 0.1 g of conc. H2SO4. Thermal
polymerization was repeated using the same conditions. The polymerized sample was carbonized
at 850 OC for 5 h under a nitrogen flow. The carbonized MC-Niinsitu sample was washed with 2
M NaOH solution for 7-8 h (Fig. 1e) to remove the SBA15 silica template. The final, dried Ni-
containing MC samples (MC-Niinsitu) were reduced by exposure to a 5% H2/N2 gas mixture at
500 oC for 2 h.
7
Synthesis of MC-Nipost: Ni(NO3)2·6H2O solution (10 wt%) was added slowly to the desired
amount of previously synthesized dried mesoporous carbon, followed by drying the slurry at
120-130 OC overnight. The final dried Ni-containing MC samples (MC-Nipost) were reduced by
by exposure to a 5% H2/N2 gas mixture at 500 oC for 2 h.
Infiltration of Mg(BH4)2 into MC (MC-Mg(BH4)2), MC-Nipost (MC-Nipost-Mg(BH4)2), and
MC-Niinsitu (MC-Niinsitu-Mg(BH4)2): All mesoporous carbon and Ni-containing mesoporous
carbon materials were thoroughly dried dried at 200 oC, cooled in a desiccator and transferred to
a glovebox. Mg(BH4)2 (45 wt%) solution (THF and diethyl ether) was slowly impregnated into
the MC, MC-Niinsitu, and MC-Nipost samples inside the glovebox [14,23,32]. The Mg(BH4)2
confined samples were dried again for 24 h at room temperature using a freeze-dryer at -77 - 80
oC with a pressure of 0.3 mbar to remove solvent and loosely bound materials from the surface.
All samples were stored inside the glove box.
Characterization and properties evaluation: Samples were prepared for XRD analysis by
smearing on a glass slide in an argon glove box and then being covered with Parafilm tape to
exclude moisture. X-ray diffraction (XRD) patterns were recorded on a Rigaku Miniflex
diffractometer (Japan) with Cu Kα radiation at a scanning rate of 2 degree/min in the 2θ range
from 10 to 80° under identical conditions. An automated adsorption analyzer (Autosorb-1C,
Quantachrome, USA) was used to record the BET surface areas, pore volume and pore size
distribution (PSD) curves [36,37]. Porous carbon and related samples were ultrasonically
dispersed in ethanol for 10-15 mins. These samples were cast on carbon-coated Cu grids using a
dropper. TEM (FEI Tecnai 20, 200kV) was performed using a F20 microscope with an
accelerating voltage 200 kV. Hydrogen desorption behaviour of pure Mg(BH4)2 and Mg(BH4)2
confined samples was investigated using TPD data recorded by a Brooks 5850E mass flow
8
controller attached to a glass tube furnace. The temperature was varied from room temperature to
500 oC at a rate of 5
oC/min, with He flowing at a rate of 50 mL/min. An automated Sieverts’
apparatus (Suzuki Shokan PCT H2 Absorption Rig) was used to record hydrogen desorption
studies. Solid-state NMR spectroscopy was carried out on a Bruker Avance III spectrometer
fitted with a 300 MHz magnet. The solid-state 11
B NMR spectra were recorded using magic
angle spinning (9kHz), a single 2.5µs pulse and 10s relaxation delay, with high-power 1H
decoupling employing the tppm 15 sequence. Spectra are referenced to BF3OEt2 (δ = 0 ppm).
Other solid-state NMR spectra were also obtained on an Avance III spectrometer (Bruker),
operating at 300.1300 MHz for 1H, 59.627 MHz for
29Si and 75.468 MHz for
13C. Powdered
material was placed in the 4 mm zirconium rotor and rotated at the magic angle with 7 kHz
frequency. 13
C NMR spectra were recorded using the SP-hpdec technique (single pulse with
high-power proton decoupling) and CPMAS. The parameters included 42 ms acquisition time
with sweep width of 50 kHz; 2K data points were collected. High-power decoupling utilized the
tppm15 scheme at 100 kHz. Between 200 and 1000 scans were collected. The recycle times
ranged from 30s to 100s and were verified to be sufficient for relaxation without signal
saturation. 29
Si NMR spectra were recorded after a single pulse to allow for quantification of the
Si species. The 90° pulse was followed be high-power decoupling using the tppm15 scheme at
87 kHz.
Results and Discussion
The porous carbon used for this research was a highly ordered mesoporous carbon scaffold
characterized by large surface area, uniform pore size, ordered and interconnected pore structure,
with good thermal and mechanical stability [14,21-24,27-32, 34,35]. These characteristics
facilitated both high dispersion and high loading of hydrogen with fine control of the particles
9
within the pore channels. Figure 1 illustrates the synthesis of three types of ordered mesoporous
carbon scaffolds: (i) mesoporous carbon (MC), (ii) post-incorporated Ni NPs in MC (MC-Nipost),
and (iii) in-situ grown, nanoconfined Ni NPs in MC (MC-Niinsitu). In this work, Mg(BH4)2 was
slowly impregnated into the nanopores of previously well-dried MC, MC-Niinsitu, and MC-Nipost
matrices. All materials were thoroughly characterized by XRD and BET (supplementary
information, SI). The presence of three well-defined XRD reflections (100), (110), and (200)
(Fig. 1a, SI) confirmed the formation of a 2D hexagonal mesoporous structure (p6mm) for the
SBA15 silica template and it’s corresponding mesoporous carbon (MC) replica [14, 19-24,33-
35]. A small shift in the XRD diffraction for MC (Fig. 1a, SI) can be ascribed to the contraction
of both the mesoporous carbon framework and the silica template during the high-temperature
(850 OC) carbonization. The presence of broad peaks at higher angles (Fig. 1a, SI) for MC
supports the graphitic nature of the mesoporous carbon framework [14, 19-24,33-35]. Moreover,
the N2 isotherms and PSD curves (Figs. 1b and 1c, SI) for both the SBA15 silica template and
MC are in good agreement with previous reports on the formation of mesoporous structures [14,
19-24,34-37]. The structure of these matrices were also investigated by solid-state 29
Si and 13
C
NMR spectroscopy (Fig. 2, SI) which demonstrated that the structural composition was
dependent on the experimental conditions and final framework [38-42]. The absence of ‘Q sites’
(right side, Fig. 2, SI) confirmed the efficient removal of the silica template by HF washing. The
13C CP-MAS NMR spectra of carbonized mesoporous carbon samples (before (a) and after
removing silica template (b) (right side, Fig. 2, SI) clearly show the formation of mesoporous
carbon structures. NMR signals in the range 0 - 80 ppm are characteristic of sp3 carbon atoms,
while signals ranging from 100 - 160 ppm arise from sp2 carbon atoms, Signals between 140 and
10
160 ppm are assigned to oxygen bound, O-C=C sp2 carbons and those in the region of 165 - 200
ppm were ascribed to the C=O groups of the mesoporous carbon framework [38-42].
The incorporation of Ni NPs into the mesoporous carbon was observed in the XRD patterns and
TEM-EDX (Fig. 2) of MC-Nipost and MC-Niinsitu. The surface areas, pore sizes, and pore
volumes of the studied samples are given in Table 1 [14,19-24,43-52]. Incorporation of Ni NPs
into the MC framework post-synthetically decreased the pore size of MC-Nipost (Fig. 3, SI and
Table 1) whereas the pore size of MC-Niinsitu in Table 1 was slightly larger (by 0.85 nm) due to
the consumption of carbon during the nickel oxide/nickel nitrate reduction by surrounding
carbon [14,19-30,43]. The shapes of N2 isotherms and PSD curves (Fig. 3, SI) for MC-Nipost and
MC-Niinsitu are consistent with previous results [14,19-24,43-48]. The XRD peak intensities of
MC-Nipost-Mg(BH4)2 and MC-Niinsitu-Mg(BH4)2 in Fig. 2b are remarkably reduced due to the X-
ray scattering contrast between the mesoporous pore walls and the guest Mg(BH4)2 molecules
inside the pores of the mesoporous scaffold. Further, proof of confinement is provided by the
decrease in the surface areas, pore volumes and pore sizes of the impregnated matrices (Table 1),
consistent with previous reports on confinement-based systems [6,8,14,19-31,49-57]. TEM (Fig.
2d) confirmed the presence of homogeneously distributed, ultrafine Ni NPs of less than 5 nm
diameter compared to the post-synthesis incorporated Ni NPs (Fig. 2c) with average particle
sizes of about 20 nm that appear more aggregated, non-uniform and non-homogenously
distributed. TEM-EDX analysis of MC-Niinsitu (Fig. 2e) clearly indicates the presence of various
elements with a negligible amount of oxygen, consistent with previous studies [14,23,55-57].
The recorded small oxygen peak in Fig. 2e could be due to the adsorption of oxygen during the
dispersion of the samples in ethanol and/or by sample handling. Similar kinds of observations
have been reported previously [14,23].
11
Table 1 outlines the surface and structural properties before and after confining Mg(BH4)2 into
the various porous carbon matrices. Figures 3a and 3b show the XRD patterns of crystalline
Mg(BH4)2 [9] and graphitic MC, respectively, consistent with previous reports [41-43,48]. The
new diffraction peaks at 43.5°, 52°, 60°, and 74.08° in Fig. 3c confirm the incorporation of Ni
NPs [42,43,48]. Importantly, broadening of these Ni peaks also suggests the formation of small
Ni NPs as confirmed by the TEM image (Fig. 2d). Interestingly, a broad and weak XRD peak is
observed for Mg(BH4)2 in the confined sample MC-Niinsitu-Mg(BH4)2 (Fig. 3d) and for the pure
Mg(BH4)2 (Fig. 3a) in which peaks for the dehydrogenated MC-Niinsitu-Mg(BH4)2 sample at 350
oC (Fig. 3e) are even weaker and almost indistinguishable. These observations suggest that when
a guest molecule such as Mg(BH4)2 is confined within the pores of mesoporous carbon, there is a
change to the structure of the ordered pore channels. This is consistent with previous reports of
the nanoconfinement of metal hydride mixtures in porous scaffolds [14, 19-31,45-52]. An almost
negligible hump found at ~ 49.2o with evidence from the TEM-EDX (Fig. 3g) suggests the
formation of a small amount of MgO due to the presence of surface absorbed oxygen [14, 52].
The three broad hump peaks at 66, 68 and 75.8o could be consistent with the presence of MgH2.
The TEM (Fig. 3f) and TEM-EDS (Energy Dispersive Spectroscopy, Fig. 3g) images of sample
MC-Niinsitu-Mg(BH4)2 after desorption at 350 oC clearly show the presence of various elements
including a major signal for Mg.
The dehydrogenation behavior of pure Mg(BH4)2, MC-Mg(BH4)2, MC-Nipost-Mg(BH4)2, and
MC-Niinsitu-Mg(BH4)2 was systematically investigated by TPD analysis (Fig. 4).
Dehydrogenation of Mg(BH4)2, began at 270 oC (Fig. 4a) with a few additional peaks at higher
temperatures consistent with previous TPD studies [7-10,14,23]. By contrast, nanoconfinement
of Mg(BH4)2 in pure mesoporous carbon desorbed hydrogen at 150 oC (Tonset) (Fig. 4b) [26-32],
12
and the addition of Ni NPs in MC-Nipost-Mg(BH4)2 further reduced the Tonset to at ~ 76 oC with a
Tpeak at ~ 161 oC (Fig. 4c). The in-situ grown and highly dispersed Ni NPs (≤ 5 nm) in
mesoporous carbon exhibited a significant reduction of the Tonset to ~ 44 oC with a Tpeak at ~ 141
oC (Fig. 4d). This remarkably low value for Tonset is the lowest reported for Mg(BH4)2. [14]
These results indicate that the size, distribution, and aggregation of Ni NPs in mesoporous
carbon can remarkably influence the dehydrogenation kinetics of metal hydrides. These results
also suggest that synergistic effects between nanoconfinement, NP particle size, and dispersion
of catalyst throughout the mesoporous carbon (MC) is responsible for creating favorable
conditions that enable release of hydrogen at low temperatures. In addition,
compartmentalization by highly ordered porous carbon scaffolds also destabilizes the metal
hydride to release hydrogen at a significantly lower temperature with faster dehydrogenation
kinetics [14, 19-32,49-57]. However, the broad TPD curve profiles in Fig. 4 for the confined
systems, particularly at > 240-250 oC indicate slow release of H2. The formation of some large
metal hydride particles outside of the mesoporous carbon scaffold could be responsible for
producing such broad TPD profiles and Mg(BH4)2 particles buried in the deeper inside pores
may also be responsible for the slow release of hydrogen at higher temperatures.
The desorption profiles, the quantity of desorbed hydrogen (wt%) versus time (min), for the pure
Mg(BH4)2 and nanoconfined (MC-Mg(BH4)2, MC-Nipost-Mg(BH4)2 and MC-Niinsitu-Mg(BH4)2)
are compared in Fig. 5. The differences in hydrogen releasing behavior indicate that the size and
distribution of Ni NPs has a profound catalytic effect on hydrogen desorption from Mg(BH4)2
[14,23,48]. These results are consistent with previous reports in which the thermal hydrogen
desorption from MgH2 nanoparticles with primary particle size of <10 nm occurred at 350 K for
the Mg-based system [14, 19-31, 56-58]. These improvements were associated with the large
13
grain boundary and surface area achieved by small nanoparticle sizes, which also provides a
larger surface for reactions with the hydrogen [14, 19-31, 56-58]. Our results indicate that the
order of catalytic efficiency was MC-Niinsitu-Mg(BH4)2 > MC-Nipost-Mg(BH4)2 > (MC-
Mg(BH4)2. We also measured the dehydrogenation kinetics of the MC-Niinsitu-Mg(BH4)2 system
at different temperatures (Fig. 6). Confinement system MC-Niinsitu-Mg(BH4)2 delivered 7.21 wt%
of hydrogen at 350 OC (Fig. 6a), indicating that the higher the temperature, the higher the
capacity and the faster the kinetics of hydrogen release. An activation energy Ea of 21.3 kJ/mol
for this process (Figure 6b) was calculated using an Arrhenius plot (K = Aexp(-Ea/RT). This value
is less than half of the corresponding value of 45.9 kJ/mol for pure, bulk Mg(BH4)2 [14]. The
present results are consistent with those previously reported for nanoconfinement by porous
carbon scaffolds [22-32, 49-54].
Karger et al [50] have recently reported the altered reaction pathway of a nanoconfined mixture
of LiBH4–Mg(BH4)2 in which the formation of intermediate species such as [B12H12]2 was
inhibited by the influence of the porous carbon scaffold [50]. This altered reaction pathway
might be the origin of the enhanced desorption kinetics observed by us. Compartmentalization
not only limits the particle growth and aggregation of particles but also creates close contact
between Mg(BH4)2 and homogeneously dispersed ultrafine Ni NPs in mesoporous carbon
[14,19-32,54-58]. The enhanced desorption kinetics of MC-Niinsitu-Mg(BH4)2 is presumably the
synergy of (i) confinement/compartmentalization, (ii) homogeneously dispersed ultrafine
nanocatalyst with high surface area, (iii) the carbon matrix playing a catalytic role and (iv)
intimate contract between Mg(BH4)2 and MC-Niinsitu.
Conclusion
14
We have successfully demonstrated an in-situ growth nanoconfinement approach that has
reduced the Tonset of dehydrogenation of Mg(BH4)2 to an unprecedented 44 OC. MC-Niinsitu-
Mg(BH4)2) exhibited a superior dehydrogenation performance compared to pure Mg(BH4)2 or
confined Mg(BH4)2 without Ni catalyst. The activation energy (Ea) of MC-Niinsitu-Mg(BH4)2
system is 21.3 kJ/mol, less than half the value for pure Mg(BH4)2. We propose that this reduction
is due to nanoconfinement of the metal hydride with the finely divided and homogeneously
dispersed dehydrogenation catalyst within the mesoporous carbon scaffold. This approach could
be an important strategy for designing an efficient hydrogen storage system. The latter, of course
also requires modified thermodynamics to permit rehydrogenation/ reversibility and that will be
a major direction for future research.
Acknowledgements
The authors thank the AIBN-UQ for providing a new staff grant and research facilities at ARC
Centre for Functional Nanomaterials, AIBN UQ. We acknowledge the facilities and the scientific
and technical assistance of the Australian Microscopy and Microanalysis Research Facility at the
Centre for Microscopy and Microanalysis, University of Queensland, Brisbane, Australia.
Supporting information is included as attached References
[1] Schlapbach L, Zuttel A. Hydrogen-storage materials for mobile applications. Nature
2001;414:353.
[2] Chen P, Xiong Z, Luo J, Lin J, Tan KL. Interaction of hydrogen with metal nitrides and
imides. Nature 2002;420:302e4.
[3] Ritter JA, Ebner AD, Wang J, Zidan R. Implementing a hydrogen economy. Mater Today
2003;6:18-23.
15
[4] Vajo JJ, Salguero TT, Gross AF, Skeith LS, Olson GL. Thermodynamic destabilization and
reaction kinetics in light metal hydride systems. J Alloys Compd 2007;446:409.
[5] Orimo S, Nakamori Y, Eliseo JR, Zuttel A, Jensen CM. Complex hydrides for hydrogen
storage. Chem Rev 2007;107:4111.
[6] Wahab MA, Zhao H, Yao XD. Nano-confined ammonia borane for chemical hydrogen
storage. Front Chem Sci Eng 2012;6:27.
[7] Matsunaga T, Buchter F, Maurona P, Bielman M, Nakamori Y, Orimo S, Ohbad N, Miwa K,
Towata S, Zuttel A. Hydrogen storage properties of Mg[BH4]2, J. Alloys Compd. 2008; 459:
583-588.
[8] Fichtner M, Zhao-Karger Z, Hu J, Roth A, Weidler P. The kinetic properties of Mg[BH4]2
infiltrated in activated carbon, Nanotechnology 2009; 20: 204029.
[9] Rebecca JN, Vitalie S, Hwang SJ, Leonard EK, Zhang JZ. Reversibility and improved
hydrogen release of magnesium borohydride, J. Phys. Chem. C, 2010; 114: 5224.
[10] Li HW, Kikuchi K, Yuku N, Miwa K,Towata S, Orimo S. Effects of ball milling and
additives on dehydriding behaviors of well-crystallized Mg[BH4]2. Scripta Mater. 2007; 57:
679-682.
[11] David TS, Laura HR, Huang Z, Zhao JC, Tang X, Stavila V, Conradi MS.
Comprehensive NMR study of magnesium borohydride. J. Phys. Chem. C, 2011; 115 (7):
3172–3177.
[12] Nale A, Catti M, Bardaj EG, Fichtner M. On the decomposition of the 0.6LiBH4-
0.4Mg(BH4)2 eutectic mixture for hydrogen storage. Int. J. Hydrogen Energy 2010; 36:
13676.
[13] Satoshi H, Jon EF, Corno M, Zavorotynska O, Damin A, Richter B, Baricco B, Jensen
TR, Sørby MH, Hauback BC. Halide substitution in magnesium borohydride. J. Phys. Chem.
C 2012; 116 (23): 12482–12488.
[14] Wahab MA, Yi J, Yang DJ, Zhao HJ, Yao XD, Enhanced hydrogen desorption from
Mg(BH4)2 by combining nanoconfinement and a Ni catalyst. J. Mater. Chem. A 2013; 1:
3471.
[15] Huang J, Yan Y, Arndt R, Zhang Y, Daniel R, Yuen SA, Jongh Petra E. de, Fermin C,
Quyang L, Zhu M, Zuttel A, A novel method for the synthesis of solvent-free Mg(B3H8)2.
Dalton Trans. 2016; 45: 3687-3690.
16
[16] Grigorii S, Jae-Hyuk H, Stephens PW, Gao Y, Job R, Matt A, Zhao JC, Ammine
magnesium borohydride complex as a new material for hydrogen storage: structure and
properties of Mg(BH4)2·2NH3. Inorg. Chem. 2008; 47: 4290-4298.
[17] (a) Yang Y, Gao M, Liu Y, Wang J, Gu J, Pan H, Guo Z, Multi-hydride systems with
enhanced hydrogen storage properties derived from Mg(BH4)2 and LiAlH4, Intl. J. Hydrogen
Energy, 2012; 37: 10733-10742; (b) Liu Y, Yang Y, Zhou Y, Zhang Z, Gao M, Pan H.
Hydrogen storage properties and mechanisms of the Mg(BH4)2-NaAlH4 system, Intl. J.
Hydrogen Energy, 2012; 37: 17137-17145; (c) Li Y, Liu Y, Yang Y, Gao M, Pan H,
Thermal dehydrogenation behaviors and mechanisms of Mg(BH4)2∙6NH3-xLiH
combination systems, Intl. J. Hydrogen Energy, 2014; 39: 11999-12006; (d) Yang Y, Liu Y,
Li Y, Gao M, Pan H, Synthesis and thermal decomposition behaviors of magnesium
borohydride ammoniates with controllable composition as hydrogen storage materials,
Chem. Asian J. 2013; 8: 476 – 481.
[18] (a) Ouyang LZ, Cao ZJ, Li LL, Wang H, Liu JW, Min D, Chen YW, Xiao FM, Tang RH,
Zhu M, Enhanced high-rate discharge properties of La11.3Mg6.0Sm7.4Ni61.0Co7.2Al7.1 with
added graphene synthesized by plasma milling, Intl. J. Hydrogen Energy, 2014; 39: 12765-
12772; (b) Ouyang LZ, Cao ZJ, Wang H, Liu JW, Sun DL, Zhang QA, Zhu M, Enhanced
dehydriding thermodynamics and kinetics in Mg(In)–MgF2 composite directly synthesized
by plasma milling, J. Alloys Compd. 2014; 586: 113–117; (c) Cao Z, Ouyang L, Wu Y,
Wang H, Liu J, Fang F, Sun D, Zhang Q, Zhu M, Dual-tuning effects of In, Al, and Ti on the
thermodynamics and kinetics of Mg85In5Al5Ti5 alloy synthesized by plasma milling. J.
Alloys Compd. 2015; 623: 354–358; (d) Ouyang LZ, Cao ZJ, Wang H, Liu JW, Sun DL,
Zhang QA, Zhu M, Dual-tuning effect of In on the thermodynamic and kinetic properties of
Mg2Ni dehydrogenation. Intl. J. Hydrogen Energy, 2013; 38: 8881-8887; (e) Cao Z, Ouyang
L, Wang H, Liu J, Sun L, Michael F, Zhu M, Development of Zr-Fe-V alloys for hybrid
hydrogen storage system. Intl. J. Hydrogen Energy, 2016; 41: 11242-11253; (f) Minghong H,
Ouyang L, Wang H, Jiangwen L, Zhu M, Hydrogen generation by hydrolysis of MgH2 and
enhanced kinetics performance of ammonium chloride introducing. Intl. J. Hydrogen Energy,
2015; 40: 6145-6150; (g) Ouyang LZ, Yang XS, Zhu M, Liu JW, Dong HW, Sun DL, Zou J,
Yao XD, Enhanced hydrogen storage kinetics and stability by synergistic effects of in situ
formed CeH2.73 and Ni in CeH2.73-MgH2‑Ni nanocomposites. J. Phys. Chem. C. 2014; 118:
17
7808−7820; (h) Ouyang LZ, Cao ZJ, Yao L, Wang H, Liu JW, Zhu M, Comparative
investigation on the hydrogenation/dehydrogenation characteristics and hydrogen storage
properties of Mg3Ag and Mg3Y. Intl. J. Hydrogen Energy, 2014; 118: 13616-13621; (i) Cao
Z, Quyang L, Li L, Lu Y, Wang H, Liu J, Min D, Chen Y, Xiao F, Sun T, Tang R, Zu Min,
Enhanced discharge capacity and cycling properties in high-samarium, praseodymium/
neodymium-free, and low-cobalt A2B7 electrode materials for nickel-metal hydride battery,
Intl. J. Hydrogen Energy, 2015; 40: 451-455; (j) Huang JM, Duan RM, Quyang LZ, Wen YJ,
Wang H, Zhu M, The effect of particle size on hydrolysis properties of Mg3La hydrides, Intl.
J. Hydrogen Energy, 2014; 39: 13564-568; (k) Huang JM, Quyang LZ, Wen YJ, Wang H,
Liu JW, Chen ZL, Zhu M, Improved hydrolysis properties of Mg3RE hydrides alloyed with
Ni, Intl. J. Hydrogen energy, 2014; 39: 6813-6818.
[19] Gross AF, Vajo JJ, Atta VSL, Olson G. Enhanced hydrogen storage kinetics of LiBH4 in
nanoporous carbon scaffolds. J. Phys. Chem. C 2008; 112: 5651.
[20] Gutowska A, Li L, Shin Y, Wang M, Li S, Linehan J, Smith R, Kay B, Schmid B, Shaw
W, Gutowski M, Autrey T. Nanoscaffold mediates hydrogen release and the reactivity of
ammonia borane. Angew. Chem. Int. Edn. 2005; 44: 3578.
[21] Jongh PEde, Wagemans RWP, Eggenhuisen MT, Dauvillier BS, Radstake PB, Meeldijk
JD, Geus JW, Jong KP, The Preparation of carbon-supported magnesium nanoparticles using
melt infiltration. Chem. Mater. 2007; 19: 6052.
[22] Li L, Yao XD, Sun C, Du A, Cheng L, Zhu Z, Yu C, Zou J, Sean S, Wang P, Cheng HM,
Frost RL, Max Lu GQ. Lithium-catalyzed dehydrogenation of ammonia borane within
mesoporous carbon framework for chemical hydrogen storage. Adv. Funct. Mater. 2009; 19:
265.
[23] Wahab MA, Beltramini J. Catalytic nanoconfinement effect of in-situ synthesized Ni-
containing mesoporous carbon scaffold (Ni-MCS) on the hydrogen storage properties of
LiAlH4. Intl. J. Hydrogen Energy 2014; 39: 18280.
[24] Yi J, Sun C, Lina C, Wahab MA, Cheng L, Cui J, Zou J, Zhu M, Yao XD,
Destabilization of Mg–H-bonding through nano-interfacial confinement by unsaturated
carbon for hydrogen desorption from MgH2. Phys. Chem. Chem. Phys. 2013; 15: 5814.
18
[25] Nielsen TK, Polanski M, Zasada M, Javadian P, Besenbacher F, Bystrzycki J, Jorgen S,
Jensen TR. Improved hydrogen storage kinetics of nanoconfined NaAlH4 catalyzed with
TiCl3 nanoparticles. ACS Nano 2011; 5: 4056.
[26] Liu X, Pealee D, Jost CZ, Baumann F, Majzoub EH. Decomposition behavior of eutectic
LiBH4−Mg(BH4)2 and its confinement effects in ordered nanoporous carbon. J. Phys. Chem.
C 2014; 118: 27265.
[27] Karger ZZ, Witter R, Bardaj EG, Wang D, Cossement D, Fichtnera M. Altered reaction
pathways of eutectic LiBH4–Mg(BH4)2 by nanoconfinement. J. Mater. Chem. A 2013; 1:
3379.
[28] Nielsen TK, Ulrike B, Gosalawit R, Dornheim M, Cerenius Y, Besenbacher F, Jensen
TR. A Reversible nanoconfined chemical reaction. ACS Nano 2009; 4: 3903.
[29] Nielsen TK, Besenbacher F, Jensen T R. Nanoconfined hydrides for energy storage.
Nanoscale 2011; 3: 2086.
[30] de Jongh PE, Adelhelm P. Nanosizing and nanoconfinement: new strategies towards
meeting hydrogen storage goals. ChemSusChem, 2010; 3: 1332.
[31] Javadian P, Jensen TR. Enhanced hydrogen reversibility of nanoconfined LiBH4–
Mg(BH4)2. Int. J. Hydrogen Energy 2014; 39: 9871.
[32] Xiangfeng Liu, David PT, Patrick S, Majzoub EH. Decomposition Behavior of Eutectic
LiBH4–Mg(BH4)2 and Its Confinement Effects in Ordered Nanoporous Carbon, J. Phys.
Chem. C, 2014; 118 (47): 27265–27271.
[33] Yu C, Fan J, Tian B, Zhao DY. Morphology development of mesoporous materials: a
colloidal phase separation mechanism. Chem. Mater. 2014; 16: 889.
[34] Jun S, Joo SH, Ryoo R, Kruk M, Jaroniec M, Liu Z, Ohsuna T, Terasaki O. Synthesis of
new, nanoporous carbon with hexagonally ordered mesostructure. J. Am. Chem. Soc. 2000;
122: 10712.
[35] Ji X, Kyu TL, Nazer LF. A highly ordered nanostructured carbon sulphur cathode for
lithium sulphur batteries. Nature Mater. 2009; 8: 500.
[36] Brunauer S, Emmett PH, Teller E. The determination of pore volume and area
distributions in porous substances. I. computations from nitrogen isotherms. J. Am. Chem.
Soc. 1938; 60: 309.
19
[37] Barrett EP, Joyner LG, Halenda PP, The determination of pore volume and area
distributions in porous substances. II. computations from nitrogen isotherms. J. Am. Chem.
Soc. 1951; 73: 373.
[38] Falco C, Caballero FP, Babonneau F, Gervais C, Laurent G, Titirici MM, Baccile N.
Hydrothermal carbon from biomass: structural differences between hydrothermal and
pyrolyzed carbons via 13
C solid-state NMR. Langmuir 2011; 17: 14460.
[39] Meng Y, Gu D, Zhang F, Shi Y, Cheng L, Feng D, Wu Z, Chen Z, Wan Y, Stein A, Zhao
DY. A Family of highly ordered mesoporous polymer resin and carbon structures from
organic−organic self-assembly. Chem. Mater. 2006; 18: 4447.
[40] Ghimbeu CM, Vidal L, Delmotte L, Meins JML, Guterl CV. Catalyst-free soft-template
synthesis of ordered mesoporous carbon tailored using phloroglucinol/glyoxylic acid
environmentally friendly precursors. Green Chem. 2014; 16: 3079.
[41] Hwang CC, Jin Z, Lu W, Sun Z, Alemany LB, Lomeda JR., Tour JM. In-situ synthesis of
polymer-modified mesoporous carbon CMK-3 composites for CO2 sequestration. ACS Appl.
Mater. Interfaces 2011; 3: 4782.
[42] Baccile N, Laurent G, Babonneau F, Fayon F, Titiric MG, Antonietti M. Structural
characterization of hydrothermal carbon spheres by advanced solid-state MAS 13
C NMR
investigations. J. Phys. Chem. C 2009; 113: 9644.
[43] Tian Y, Wang X, Pan Y. Simple synthesis of Ni-containing ordered mesoporous carbons
and their adsorption/desorption of methylene orange. J. Hazard. Mater. 2012; 213-214: 361.
[44] Wahab MA, Beltramini JN. Recent advances in hybrid periodic mesostructured
organosilica materials: opportunities from fundamental to biomedical applications RSC Adv.
2015; 5: 79129.
[45] Wahab MA, Yeo E, Shudhakar S, Sellinger A. Evaporation induced self-assembly of
mesoscopically ordered organic/ organosilica nanocomposite thin films with
photoluminescent properties and improved hardness. Chem. Mater. 2008; 20: 1855.
[46] Wahab MA, Imae I, Kawakami Y, Ha CS. Periodic mesoporous organosilica materials
incorporating various organic functional groups: synthesis, structural characterization, and
morphology. Chem. Mater. 2005; 17: 2165.
[47] Wahab MA, Ha CS. Ruthenium-functionalised hybrid periodic mesoporous
organosilicas: synthesis and structural characterization. J. Mater. Chem. 2005; 15: 508.
20
[48] Garcia A, Neito A, Vila M, Vallet-Regi MV. Easy synthesis of ordered mesoporous
carbon containing nickel nanoparticles by a low-temperature hydrothermal method. Carbon
2013; 51: 410.
[49] Fan X, Xiao X, Shao J, Zhang L, Li S, Ge HQ. Wang L., Size effect on hydrogen storage
properties of NaAlH4 confined in uniform porous carbons. Nano Energy 2013; 2: 995.
[50] Karger ZZ, Witter R, Bardajı EG, Wang D, Cossement D, Fichtner M. Altered reaction
pathways of eutectic LiBH4–Mg(BH4)2 by nanoconfinement. J. Mater. Chem. A 2013; 1:
3379.
[51] Javadiana P, Sheppardb DA, Buckleyb CE, Jensen TR., Hydrogen storage properties of
nanoconfined LiBH4–Ca(BH4)2. Nano Energ, 2015; 11: 96.
[52] Konarova M, Tanksale A, Beltramini JN, Max Lu GQ. Effects of nano-confinement on
the hydrogen desorption properties of MgH2. Nano Energy 2013; 2: 98.
[53] Metin O, Mazumder V, Ozkar S, Sun S, Monodisperse nickel nanoparticles and their
catalysis in hydrolytic dehydrogenation of ammonia borane. J. Am. Chem. Soc. 2010; 132:
1468.
[54] Minella CB, Lindemann I, Nolis P, Kiebling A, Baro MD, Klose M, Giebeler L,
Rellinghaus B, Eckert J, Schultz L, Gutfleisch O, NaAlH4 confined in ordered mesoporous
carbon. Int. J. Hydrogen Energy 2013; 38: 8829.
[55] Quyang LZ, Tang J, Zhao Y, Wang H, Yao XD, Liu J, Zou J, Zhu M, Expression
penetration of hydrogen on Mg(1013) along the close-packed planes, Scientific Reports, 5:
10776, DOI: 10.1038/srep10776.
[56] Ouyang LZ, Yang XS, Zhu M, Liu JW, Dong HW, Sun DL, Zou J, Yao XD, Enhanced
hydrogen storage kinetics and stability by synergistic effects of in-situ formed CeH2.73 and Ni
in CeH2.73-MgH2‑Ni Nanocomposites. J. Phys. Chem. C 2014, 118, 7808−7820.
[57] Ouyang LZ, Ye SY, Dong HW, Zhu M, Effect of interfacial free energy on hydriding
reaction of Mg–Ni thin films, Applied Phys. Lett. 2007, 90, 021917-021919.
[58] Dornheim M, Doppiu S, Barkhordarian G, Boesenberg U, Klassen T, Gutfleisch O,
Bormann R. Hydrogen storage in magnesium-based hydrides and hydride composites. Scr.
Mater. 2007; 56: 841−846.
21
Table 1. Surface and structural properties: specific surface area(SBET
), pore volume (cm3/g) and
the pore size (nm).
22
Fig. 1. Synthesis of MC/MC-Ni-insitu/MC-Ni-post using a mesoporous SBA15 silica template
followed by impregnation of Mg(BH4)2 in to MC/MC-Ni-insitu/MC-Ni-post. The structural
properties of all used materials are given in Table 1.
23
Fig. 2. (a) XRD patterns for MC-Niinsitu and MC-Nipost, (b) XRD patterns of Mg(BH4)2 confined
in MC-Niinsitu, (c) TEM image of MC-Nipost, (d) TEM image of MC-Niinsitu and (e) TEM-EDX of
(d).
24
Fig. 3. XRD patterns of (a) Pure Mg(BH4)2, (b) pure mesoporous carbon (MC), (c) MC-Niinsitu,
(d) MC-Niinsitu-Mg(BH4)2 (as-prepared and dried), (e) dehydrogenated MC-Niinsitu-Mg(BH4)2 at
350OC, (f) TEM image of MC-Niinsitu-Mg(BH4)2 at 350
OC, and (g) TEM-EDX of MC-Niinsitu-
Mg(BH4)2 at 350OC.
25
50 100 150 200 250 300 350 400 450 500
Temperature (OC)
(a) Pure Mg(BH4)2
(b) MC-Mg(BH4)2
(c) MC-Nipost
-Mg(BH4)2
(d) MC-Niinsitu
-Mg(BH4)2
(d)
(a)
(b)
(c)
Fig. 4. TPD-MS spectra of (a) Pure Mg(BH4)2, (b) MC-Mg(BH4)2, (c) MC-Ni-post-Mg(BH4)2,
and (d) MC-Niinsitu-Mg(BH4)2.
26
0 20 40 60 800
1
2
3(d)
(c)
(b)
(a) Pure Mg(BH4)
2
(b) MC-Mg(BH4)
2
(c) MC-Nipost
-Mg(BH4)
2
(d) MC-Niinsitu
-Mg(BH4)
2
H2 d
eso
rbed (
wt%
)
Time (min)
(a)
Fig. 5. PCT results of (a) Pure Mg(BH4)2, (b) MC-Mg(BH4)2, (c) MC-Ni-post-Mg(BH4)2, and (d)
MC-Niinsitu-Mg(BH4)2 at 145OC.
27
Fig. 6. (a) H2 desorption of pure Mg(BH4)2 and MC-Niinsitu-Mg(BH4)2 with temperature and (b)
activation energy from Arrhenius plot.
28
Supporting Information
Low-temperature hydrogen desorption from
Mg(BH4)2 catalysed by ultrafine Ni nanoparticles in
a mesoporous carbon matrix
Mohammad A. Wahab,*abc
David Jame Young,c Azharul Karim,
b Sabrina Fawzia
d and
Jorge N. Beltraminia
abARC Centre for Functional Nanomaterials, Australian Institute for Bioengineering and
Nanotechnology, The University of Queensland, Brisbane, St Lucia, QLD 4072, Australia
*E-mail: [email protected]; [email protected]
bChemistry, Physics and Mechanical Engineering, Science and Engineering Faculty, Queensland
University of Technology, 2 George Street, QLD 4001 Australia.
c Faculty of Science, Health, Education and Engineering, University of the Sunshine Coast,
Maroochydore DC, Queensland 4558, Australia.
d Science and Engineering Faculty, Civil Engineering and Built Environmental Science.
Queensland University of Technology, 2 George Street, QLD 4001 Australia.
29
Fig. 1. (a) XRD patterns of mesoporous SBA15 silica template and its replicate MC. Inset shows
the higher angle XRD patterns of MC. (b) N2 isotherms of mesoporous SBA15 silica template
and its replicate MC, and pore size distribution curves of mesoporous SBA15 silica template and
its replicate MC.
30
Fig. 2. (left) Solid-state 29
Si NMR spectra of (a) mesoporous SBA15 silica template and (b) its
replicate MC after removing SBA15 silica template and (right) Solid-state 13
C NMR spectra of
(a) mesoporous SBA15 silica template/carbon (carbonized) and (b) its replicate MC after
removing SBA silica template.
Fig. 3. (a) N2 isotherms of MC-Niinsitu and MC-Nipost, (b) pore size distribution curves of MC-
Niinsitu and MC-Nipost..
31
0 -25 -50
(ppm)
(a) Pure Mg(BH4)
2
(b) MC-Niinsitu
-Mg(BH4)
2
(c) MC-Niinsitu
-Mg(BH4)
2
Fig. 4. Solid-state 11
B NMR spectra of (a) Pure Mg(BH4)2, (b) MC-Niinsitu-Mg(BH4)2 (as-
confined), and (c) MC-Niinsitu-Mg(BH4)2 (dehydrogenated at 350 oC).