effect of rare earth elements on electrochemical properties of la–mg–ni-based hydrogen storage...
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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 4 ( 2 0 0 9 ) 1 3 9 9 – 1 4 0 4
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Effect of rare earth elements on electrochemical propertiesof La–Mg–Ni-based hydrogen storage alloys
Yuan Lia,b, Da Hanc, Shumin Hana,b,*, Xilin Zhub, Lin Hub, Zhong Zhanga, Yuwen Liub
aState Key Laboratory of Metastable Materials Science and Technology, Yanshan University, Qinhuangdao 066004, ChinabCollege of Environmental and Chemical Engineering, Yanshan University, Qinhuangdao 066004, ChinacDepartment of Chemistry, Xiamen University, Xiamen 361005, China
a r t i c l e i n f o
Article history:
Received 26 March 2008
Received in revised form
23 July 2008
Accepted 14 November 2008
Available online 23 December 2008
Keywords:
Hydrogen storage alloys
Rare earth elements
Electrochemical properties
Phase structure
Kinetics
* Corresponding author. College of Environm066004, Hebei Province, China. Tel./fax: þ86
E-mail address: [email protected] (S. H0360-3199/$ – see front matter ª 2008 Interndoi:10.1016/j.ijhydene.2008.11.049
a b s t r a c t
La0.60R0.20Mg0.20(NiCoMnAl)3.5 (R¼ La, Ce, Pr, Nd) alloys were prepared by inductive melting.
Variations in phase structure and electrochemical properties due to partial replacement of
La by Ce, Pr and Nd, were investigated. The alloys consist mainly of LaNi5 phase, La2Ni7
phase and LaNi3 phase as explored by XRD and SEM. The maximum discharge capacity
decreases with Ce, Pr and Nd substitution for La. However, the cycling stability is improved
by substituting Pr and Nd at La sites, capacity retention rate at the 100th cycle increases by
13.4% for the Nd-substituted alloy. The electrochemical kinetics measurements show that
Ce and Pr substitution improves kinetics and thus ameliorates the high rate discharge-
ability (HRD) and low temperature dischargeability. The HRD at 1200 mA g�1 increases from
22.1% to 61.3% and the capacity at 233 K mounts up from 90 mAh g�1 to 220 mAh g�1 for the
Ce-substituted alloy.
ª 2008 International Association for Hydrogen Energy. Published by Elsevier Ltd. All rights
reserved.
1. Introduction these methods elemental substitution was found to be an
Metal hydride/Nickel (MH/Ni) batteries are widely used in
portable electronic devices, electric hand tools and even
electric vehicles owing to their high energy density, long cycle
life and environmental friendliness [1]. R–Mg–Ni-based
(R¼ rare earths, Y and Ca) alloys are considered as promising
negative electrode materials due to their higher capacity than
commercial AB5-type alloys in recent years [2,3]. However,
they are subject to poor cycling stability, failing to meet the
need of practical applications [4].
Several methods have been applied to improve hydrogen
storage properties of R–Mg–Ni-based alloys, such as elemental
substitution in alloy composition [5–7], rapid quenching [8],
composite alloying [9], and surface modification [10]. Among
ental and Chemical En335 807 4648.an).
ational Association for H
effective way to improve cycling stability of R–Mg–Ni-based
alloys. A lot of research has been focused on B-elements up to
now. Mn, Co, Al, Mo, Cr, Cu, Fe, etc were adopted in B-sites. In
LaNi3�xMnx alloys, Mn entered the Ni sites and changed the
structure from PuNi3-type to CeNi3-type, decreasing stability
of the hydride against amorphisation on hydrogenation [5].
This may be helpful to improve cycling stability. Co substitu-
tion and combining annealing treatment was believed to
improve cycling stability. The capacity retention rate at the
100th cycle increased from 65.5% for La0.7Mg0.3Ni2.45Co0.75
Mn0.1Al0.2 electrode to 80.5% for La0.7Mg0.3Ni2.15Co1.05Mn0.1Al0.2
electrode [6]. Moreover, the combination of Al and Mo
ameliorated high rate dischargeability, low temperature dis-
chargeability and cycle life [7]. Reports on A-site substitution
gineering, Yanshan University, 438# Hebei Street, Qinhuangdao
ydrogen Energy. Published 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 4 ( 2 0 0 9 ) 1 3 9 9 – 1 4 0 41400
were not enough although investigation on B-site substitution
was systematic. Pan et al. [12] reported Pr substitution for La in
R–Mg–Ni-based alloys La0.7�xPrxMg0.3Ni2.45Co0.75Mn0.1Al0.2 and
found improvement in cycling stability. Zhang et al. [11]
prepared (La, Ce, Pr, Nd)2MgNi9 alloys through an orthogonal
design, and the results showed that Mishmetal composition
has great influence on the La2MgNi9-type alloys. Under the
work typified above, overall electrochemical properties of R–
Mg–Ni-based alloys have been greatly improved; however,
cycling stability is still unsatisfactory. In our previous work,
we have found that low-Mg and B-site multi-component
design was beneficial for improving cycling stability, and we
have also obtained alloys with higher capacity retention rate
by substituting La-rich mishmetal for elemental La [13,14]. But
the effect of each component in the mishmetal (La, Ce, Pr and
Nd) was not clear.
This paper will focus on the effect of rare earth elements on
electrochemical properties of La–Mg–Ni-based hydrogen
storage alloys. The low-Mg and B-site multi-component
La0.60R0.20Mg0.20(NiCoMnAl)3.5 (R¼ La, Ce, Pr, Nd) alloys were
prepared. Phase structure and electrochemical properties of
the alloys will be studied as a part of our systematic work.
10 20 30 40 50 60 70 80
o**
oo+
****
o
o*
+o*o
*o+ *
+
o
o*
+
* LaNi5o La2Ni7+ LaNi3
R = Nd
R = Pr
R = Ce
R = La
Inte
nsit
y (a
.u.)
2 Theta (degree)
Fig. 1 – XRD patterns of La0.60R0.20Mg0.20(NiCoMnAl)3.5
alloys.
2. Experimental
La0.60R0.20Mg0.20(NiCoMnAl)3.5 (R¼ La, Ce, Pr, Nd) alloys were
prepared by inductive melting constituent metals (La, Ce, Pr,
Nd, Ni, Co, Mn, Al) with a purity of 99.5% and Mg–Ni inter-
metallic alloy under argon atmosphere. A Mg–Ni intermetallic
alloy was used instead of Mg and a slight excess of Mg was
used to compensate for evaporative Mg loss during the
melting for the purpose of reducing Mg loss. Then the five-
kilogram ingots were annealed at 1173 K for 8 h. Chemical
composition of the alloys was examined by ICP analysis. The
prepared ingots were mechanically crushed and ground into
fine powders in the air. Powders of 200–300 mesh were used
for electrochemical test and those below 300 mesh for XRD
analysis.
X-ray diffraction (XRD) patterns were obtained on a D/Max-
2500/PC X-ray diffractometer (Cu Ka radiation). Phase identi-
fication and lattice parameters calculation have been carried
out using Jade-5.0 software. Morphology of the alloys was
observed by S-3400 scanning electron microscopy.
A testing electrode was prepared by cold pressing a mixture
of 0.15 g alloy powders and 0.75 g carbonyl nickel powders into
a pellet of 10 mm in diameter under 20 MPa. Electrochemical
measurements were performed in a tri-electrode system con-
sisting of MH electrode (working electrode), Ni(OH)2/NiOOH
electrode (counter electrode) and Hg/HgO electrode (reference
electrode). All the tests were performed at 298 K except for low
temperature dischargeability measurement. The electrodes
were fully charged (the over-charged ratio was approximately
30–50%) at current density of 60 mA g�1, and then discharged at
the same current density during charge/discharge tests.
Discharge capacities were measured at different discharge
current densities when high rate dischargeabilty (HRD) was
measured. Low temperature dischargeability was measured
after laying the tri-electrode system at constant temperature for
8 h using a low-temperature-equipment (WGD701). The
electrodes were discharged to cut-off potential of�0.6 V (vs. Hg/
HgO electrode) in all the discharge process.
The pressure–composition isotherms were obtained
through an electrochemical method. The fully charged elec-
trodes were discharged for 0.5 h, followed by a 0.5 h rest until
cut-off potential was �0.6 V (vs. Hg/HgO electrode). The
equilibrium potential (Eeq) was recorded and converted to
equilibrium pressure (Peq) of hydrogen on basis of the Nernst
equation [15].
EeqðV vs: Hg=HgOÞ ¼ �0:925� 0:03 log�Peq
�The micropolarization curves of the electrodes were
measured on a ZF-9 potentiostat by scanning electrode
potential at the rate of 5 mV min�1 from �5 to 5 mV (vs. open-
circuit potential) at 50% depth of discharge (DOD). For the
potentialstatic step discharge, the fully charged electrode was
discharged at þ500 mV step for 3000 s.
3. Results and discussion
3.1. Phase structure
The XRD patterns of La0.60R0.20Mg0.20(NiCoMnAl)3.5 (R¼ La, Ce,
Pr, Nd) alloys are shown in Fig. 1. The alloys consist mainly of
LaNi5 phase, La2Ni7 phase and minor LaNi3 phase from Jade-
5.0 analysis. The lattice parameters and cell volume of the
above phases are listed in Table 1. It is noticed that Ce-
substituted alloy has the smallest cell volume although rare
earth atoms’ radii decrease in the order La>Ce> Pr>Nd. This
may be ascribed to particular 4f electron structure of Ce
atoms, which makes Cerium be compacted more tightly by
other atoms, such as Ni atoms [16].
The back scattered electron (BSE) image of La0.60Nd0.20-
Mg0.20(NiCoMnAl)3.5 and EDX spectra for phases are shown
in Fig. 2. Three main areas with different colors can be seen
in Fig. 2(a). The EDX analyses in Fig. 2(b)–(d) show that the
light grey (a), dark grey (b) and black area (g) correspond to
AB3 (La0.62Nd0.16Mg0.22Ni2.58Mn0.09Co0.19Al0.11) phase, A2B7
(La0.72Nd0.17Mg0.11Ni3.04Mn0.12Co0.23Al0.26) phase and AB5
Table 1 – Lattice parameters and cell volume of LaNi5phase and La2Ni7 phase.
Samples LaNi5 phase La2Ni7 phase
a (A) c (A) V (A3) a (A) c (A) V (A3)
R¼ La 5.032 4.015 88.05 5.057 24.71 547.2
R¼Ce 5.012 3.986 86.68 5.043 24.68 543.5
R¼ Pr 5.013 3.994 86.90 5.059 24.54 543.9
R¼Nd 5.017 4.009 87.37 5.071 24.55 546.8
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 4 ( 2 0 0 9 ) 1 3 9 9 – 1 4 0 4 1401
(La0.78Nd0.18Mg0.03Ni3.99Mn0.19Co0.36Al0.33) phase, respectively.
The results are consistent with those obtained from XRD.
3.2. P–C isotherms
The electrochemical pressure–composition isotherms that
examine the discharge level of hydrogen in an anode at 298 K
are presented in Fig. 3. The plateaus of the hydrogen desorp-
tion isotherms increase by substituting Ce, Pr and Nd at La
sites. This is closely related with decrease in cell volume after
Fig. 2 – BSE image and EDX analysis of La0.60Nd0.20Mg0.20(NiCoMn
substitution. The Ce-substituted alloy exhibits much sloppier
plateau and higher equilibrium pressure in desorption PCT
owing to the smallest cell volume. The hydrogen storage
capacity (H/M ) obtained from desorption PCT is also shown in
Table 2. The capacity decreases after La is substituted by Ce, Pr
and Nd, which results mainly from decreasing cell volumes.
Among the four alloys, Ce-substituted alloy has the lowest
hydrogen storage capacity.
3.3. Electrochemical properties
The discharge capacities of La0.60R0.20Mg0.20(NiCoMnAl)3.5
(R¼ La, Ce, Pr, Nd) alloys at different cycle numbers are shown
in Fig. 4. It can be seen that the Ce- and Pr-substituted alloys
can be activated in 2 cycles; the Nd-substituted alloy and the
original alloy need 3 cycles to be activated. The maximum
discharge capacity (Cmax) listed in Table 2 decreases with Ce,
Pr and Nd substitution. The capacity of Ce-substituted alloy
decreases from 372 mAh g�1 to 340 mAh g�1, decreasing by
8.6%, however, the capacity of Nd-substituted alloy decreases
slightly, from 372 mAh g�1 to 370 mAh g�1.
Al)3.5 alloy (a) BSE image (b) a phase (c) b phase (d) g phase.
0.0 0.2 0.4 0.6 0.8 1.01E-4
1E-3
0.01
0.1
1
10
R = LaR = CeR = PrR = Nd
p eq(
MP
a)
H/M
Fig. 3 – Electrochemical desorption P–C isotherms of
La0.60R0.20Mg0.20(NiCoMnAl)3.5 alloy electrodes.
0 20 40 60 80 100100
150
200
250
300
350
400
0 2 4 6 8150
200
250
300
350
400
R = La
R = Ce
R = Pr
R = Nd
Dis
char
ge c
apac
ity
(mA
h g-1
)
Cycle number (n)
Fig. 4 – Discharge capacity of La0.60R0.20Mg0.20(NiCoMnAl)3.5
alloy electrodes vs. cycle number.
60
80
100 R = La
R = Ce
R = Pr
R = Nd
%)
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 4 ( 2 0 0 9 ) 1 3 9 9 – 1 4 0 41402
Cycling stability of metal hydride electrode is an important
factor to cycle life of MH/Ni batteries. It can be seen from Fig. 4
that slope of cycle life profiles becomes smaller with Pr and Nd
substitution for La, indicating that the cycle life is improved.
In order to illustrate cycling stability, capacity retention rate at
the 100th cycle (S100) is calculated as the ratio of C100/Cmax, and
is listed in Table 2. Table 2 shows that Pr- and Nd-substitution
causes an increase in S100. Nd substitution improves cycle life
significantly with S100 increasing from 79.8 to 93.2%.
It has been proved that discharge capacity degradation is
caused by serious pulverization and oxidation of alloy elec-
trodes. Structure of LaNi3 and La2Ni7 phases are both
described as a stacking of [LaNi5] and [La2Ni4] slabs, and
volume expansion of [La2Ni4] slabs can reach up to 59–63% on
hydriding [17]. Moreover, in the anisotropic hydride, expan-
sion of La2Ni7 phase and LaNi3 phase in c-axis direction is
larger than that in a-axis direction [18], causing serious inner
stress and thus easy pulverization. Therefore, pulverization is
an important factor to capacity degradation of R–Mg–Ni-based
alloys. Meanwhile, pulverization accelerates oxidation and
diffusion of rare earth elements towards the surface. During
charge/discharge process, rare earth elements tend to diffuse
towards alloy surface, and the disproportion is determined by
atom concentration, melting point and cell volume. Among
the four elements Ce diffuses to surface more quickly because
of low melting point and small volume, however, Nd diffuses
slowly due to its much higher melting point [19]. That is Nd
substitution can suppress oxidation of the alloy elements and
Table 2 – Electrochemical properties ofLa0.60R0.20Mg0.20(NiCoMnAl)3.5 alloy electrodes.
Samples H/M Cmax
(mAh g�1)Na HRD1200
(%)C233
(mAh g�1)S100
(%)
R¼ La 0.972 372 3 22.1 90 79.8
R¼Ce 0.907 340 2 61.3 220 79.6
R¼ Pr 0.957 363 2 49.6 141 81.5
R¼Nd 0.968 370 3 44.3 60 93.2
help to keep original structure of the alloys. As a result, the
Nd-substituted alloy has better cycling stability.
The high rate dischargeability (HRD) of La0.60R0.20Mg0.20
(NiCoMnAl)3.5 (R¼ La, Ce, Pr, Nd) alloys is shown in Fig. 5. The
HRD can be calculated by the following expression:
HRDð%Þ ¼ Cd
C60� 100
where Cd is discharge capacity at the discharge current
density Id (mAh g�1) and C60 is the discharge capacity at
60 mA g�1 (mAh g�1).
Ce, Pr and Nd substitutions for La are beneficial to HRD of
the alloys. High rate dischargeability at discharge current
density of 1200 mA g�1 (HRD1200) is listed in Table 2. Ce
substitution brings prominent improvement in HRD, and
HRD1200 of Ce-substituted alloy reaches 61.3%, which is 177%
higher than that of the original alloy (22.1%).
The discharge capacities of La0.60R0.20Mg0.20(NiCoMnAl)3.5
(R¼ La, Ce, Pr, Nd) electrodes at low temperature are
0 200 400 600 800 1000 1200 1400 16000
20
40
HR
D (
Discharge current density (mA g-1)
Fig. 5 – HRD of La0.60R0.20Mg0.20(NiCoMnAl)3.5 alloy
electrodes.
230 240 250 260 270 280 290 3000
100
200
300
400
R = La
R = Ce
R = Pr
R = Nd
Dis
char
ge c
apac
ity
(mA
h g-1
)
Temperature (K)
Fig. 6 – Discharge capacity of La0.60R0.20Mg0.20(NiCoMnAl)3.5
alloy electrodes at low temperature.
Table 3 – Electrochemical kinetics parameters ofLa0.60R0.20Mg0.20(NiCoMnAl)3.5 alloy electrodes.
Samples Polarizationresistance,
Rp (mU)
Exchangecurrent density,
I0 (mA g�1)
Hydrogendiffusion
coefficient, D(�10�11 cm2 s�1)
R¼ La 152.1 168.8 3.68
R¼Ce 129.2 198.7 12.1
R¼ Pr 119.5 214.8 6.55
R¼Nd 138.0 186.0 3.23
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 4 ( 2 0 0 9 ) 1 3 9 9 – 1 4 0 4 1403
presented in Fig. 6. The discharge capacity decreases with
decreasing temperature. The discharge capacities at 233 K
(C233) listed in Table 2 are 90 mAh g�1, 220 mAh g�1,
141 mAh g�1 and 60 mAh g�1, and they are 25.6%, 68.8%, 42.5%
and 16.5% of the capacities at 298 K in the order of La, Ce, Pr
and Nd, respectively.
Iwakura et al. [20] have pointed out that high rate dis-
chargeability and low temperature dischargeability are
controlled by kinetics, including charge transfer rate at
surface and hydrogen diffusion rate in bulk. The micro-
polarization curves of La0.60R0.20Mg0.20(NiCoMnAl)3.5 (R¼ La,
Ce, Pr, Nd) alloy electrodes are plotted in Fig. 7. From Fig. 7
polarization resistance (Rp) can be obtained and consequently
exchange current density (I0) can be calculated according to
equation [21]
I0 ¼RTFRp
where I0 is the exchange current density (mA g�1); R is the gas
constant (J mol�1 K�1); T is the absolute temperature (K); F is
-6 -5 -4 -3 -2 -1 0 1 2 3 4 5 6-50
-40
-30
-20
-10
0
10
20
30
40
50
R = La
R = Ce
R = Pr
R = NdCur
rent
den
sity
(m
A g
-1)
Overpotential (mV)
Fig. 7 – Micropolarization curves of La0.60R0.20Mg0.20-
(NiCoMnAl)3.5 alloy electrodes at 50% DOD.
the Faraday constant (C mol�1) and Rp is the polarization
resistance (mU).
The polarization resistance and the exchange current
density are both presented in Table 3. The Ce- and Pr-
substituted alloys have much larger exchange current density
I0, indicating their higher charge transfer rate at electrode
surface.
For the hydrogen diffusion coefficient test, potentialstatic
step method was used. It can be seen from Fig. 8 that each
semilogarithmic curve of anode current density vs. time can
be divided into two time regions. In the first time domain, the
current decreases rapidly due to consumption of hydrogen on
the surface; while in the second time domain, the current
decreases slowly with a linear tendency. In this case,
hydrogen is supplied from the bulk alloy proportionally to the
concentration gradient of hydrogen and the current is
controlled by the diffusion rate of hydrogen atom. From slope
of the liner region in Fig. 8, hydrogen diffusion coefficient D
can be calculated by the following equation [22].
log i ¼ lg
�6FDda2ðC0 � CsÞ
�� p2
2:303Da2
t
where i is the anode current density (mA g�1), D is the
hydrogen diffusion coefficient (cm2 s�1), d is the density of the
alloy (g cm�3), a is the average radius of the alloy particles, C0
is the initial hydrogen concentration in the alloy (mol cm�3),
Cs is the surface hydrogen concentration of the alloy
0 500 1000 1500 2000 2500 3000-2.8
-2.4
-2.0
-1.6
-1.2
-0.8
-0.4
0.0
log(
i(A
g-1))
Time (s)
R = La
R = Ce
R = Pr
R = Nd
Fig. 8 – Correspondence of anode current density vs. time
of La0.60R0.20Mg0.20(NiCoMnAl)3.5 alloy electrodes at
D500 mV.
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 4 ( 2 0 0 9 ) 1 3 9 9 – 1 4 0 41404
(mol cm�3) and t is the discharge time (s). Taking a as 13 mm, D
can be calculated according to the equation, and the results
are presented in Table 3. It can be seen that the Ce-substituted
alloy has the largest hydrogen diffusion coefficient D.
4. Conclusions
The effect of rare earth elements on phase structure and
electrochemical properties of La–Mg–Ni-based hydrogen
storage alloys has been investigated in the paper present. The
main results can be summarized as follows.
(1) The XRD patterns and SEM–EDS analyses show that the
alloys consist mainly of LaNi5 phase, La2Ni7 phase and
minor LaNi3 phase. The cell volumes of LaNi5 and La2Ni7phase in the Ce-substituted alloy decrease the most.
(2) The electrochemical capacity decreases and equilibrium
pressure increases with Ce, Pr and Nd substitution for La.
However, Pr and Nd substitution improves the cycling
stability. The capacity retention rate at the 100th cycle of
Nd-substituted alloy rises by 13.4%.
(3) Ce and Pr substitution greatly improves hydrogen diffu-
sion rate in the bulk and charge transfer rate at the surface,
and thus ameliorates the high rate dischargeability and
low temperature dischargeability. The HRD at 1200 mA g�1
and capacity at 233 K reach 61.3% and 220 mAh g�1, 177%
and 154% higher than those of the original alloy for the
Ce-substituted alloy, respectively.
Acknowledgements
This work was financially supported by the National Natural
Science Foundation of China (20673093) and the Natural
Science Foundation of Hebei Province (B2007000303).
r e f e r e n c e s
[1] Ruiz FC, Castro EB, Real SG, Peretti HA, Visintin A, Triaca WE.Electrochemical characterization of AB2 alloys used fornegative electrodes in Ni/MH batteries. Int J Hydrogen Energy2008;33(13):3576–80.
[2] Kadir K, Sakai T, Uehara I. Structural investigation andhydrogen capacity of LaMg2Ni9 and (Y0.65Ca0.35)(Mg1.32Ca0.
68)Ni9 of the AB2C9 type structure. J Alloys Compd 2000;302(1–2):112–7.
[3] Kohno T, Yoshida H, Kawashima F, Inaba T, Sakai I,Yamamoto M, et al. Hydrogen storage properties of newternary system alloys: La2MgNi9, La5Mg2Ni23, La3MgNi14. JAlloys Compd 2000;311(2):L5–7.
[4] Liu YF, Pan HG, Gao MX, Zhu YF, Lei YQ, Wang QD. The effectof Mn substitution for Ni on the structural andelectrochemical properties of La0.7Mg0.3Ni2.55�xCo0.45Mnx
hydrogen storage electrode alloys. Int J Hydrogen Energy2004;29(3):297–305.
[5] Denys RV, Riabov B, Yartys VA, Delaplane RG, Sato M.Hydrogen storage properties and structure of
La1�xMgx(Ni1�yMny)3 intermetallics and their hydrides. JAlloys Compd 2007;446–447:166–72.
[6] Miao H, Pan HG, Zhang SC, Chen N, Li R, Gao MX. Influencesof Co substitution and annealing treatment on the structureand electrochemical properties of hydrogen storage alloysLa0.7Mg0.3Ni2.45�xCo0.75þxMn0.1Al0.2 (x¼ 0.00, 0.15, 0.30). Int JHydrogen Energy 2007;32(15):3387–94.
[7] Zhang XB, Sun DZ, Yin WY, Chai YJ, Zhao MS.Crystallographic and electrochemical characteristics of La0.
7Mg0.3Ni3.5�x(Al0.5Mo0.5)x (x¼ 0–0.8) hydrogen storage alloys. JPower Sources 2006;154(1):290–7.
[8] Zhang YH, Dong XP, Wang GQ, Guo SH, Ren JY, Wang XL.Effect of boron additive on electrochemical cycling life of La–Mg–Ni alloys prepared by casting and rapid quenching. Int JHydrogen Energy 2007;32(5):594–9.
[9] Chu HL, Qiu SJ, Sun LX, Zhang Y, Xu F, Zhu M, et al.Electrochemical hydrogen storage properties of La0.7Mg0.3
Ni3.5–Ti0.17Zr0.08V0.35Cr0.1Ni0.3 composites. Int J HydrogenEnergy 2008;33(2):755–61.
[10] Xiao LL, Wang YJ, Liu Y, Song DW, Jiao LF, Yuan HT. Influenceof surface treatments on microstructure and electrochemicalproperties of La0.7Mg0.3Ni2.4Co0.6 hydrogen-storage alloy.Int J Hydrogen Energy 2008;33(14):3925–9.
[11] Pan HG, Ma S, Shen J, Tan JJ, Deng J, Gao MX. Effect of thesubstitution of PR for LA on the microstructure andelectrochemical properties of La0.7�xPrxMg0.3Ni2.45Co0.75Mn0.
1Al0.2 (x¼ 0.0–0.3) hydrogen storage electrode alloys. Int JHydrogen Energy 2007;32(14):2949–56.
[12] Zhang FL, Luo YC, Deng AQ, Tang ZH, Kang L, Chen JH. Astudy on structure and electrochemical properties of (La, Ce,Pr, Nd)2MgNi9 hydrogen storage electrode alloys. ElectrochimActa 2006;52(1):24–32.
[13] Li Y, Han SM, Li JH, Hu L. Study on phase structure andelectrochemical properties of Ml1�xMgxNi2.80Co0.50Mn0.10
Al0.10 (x¼ 0.08, 0.12, 0.20, 0.24, 0.28) hydrogen storage alloys.Electrochim Acta 2007;52(19):5945–9.
[14] Li M, Han SM, Li Y, Guan W, Mao LR, Hu L. Study on the phasestructure and electrochemical properties of RE0.93Mg0.07Ni2.
96Co0.60Mn0.37Al0.17 hydrogen storage alloy. Electrochim Acta2006;51(26):5926–31.
[15] Balej J. Determination of the oxygen and hydrogenovervoltage in concentrated alkali hydroxide solutions. Int JHydrogen Energy 1985;10(6):365–74.
[16] Fukuda H, Fujii H, Matsumoto Y, Suzuki T, Fujita T, Kadir K,et al. Anomalous behavior of physical properties in RMg2Ni9(R¼Ce and Pr) with a two-dimensional rare eartharrangement. Physica B 1999;259–261:894–5.
[17] Yartys VA, Riabov AB, Denys RV, Sato M, Delaplane RG. Novelintermetallic hydrides. J Alloys Compd 2006;408–412:273–9.
[18] Akiba E, Hayakawa H, Kohno T. Crystal structure of novel La–Mg–Ni hydrogen absorbing alloys. J Alloys Compd 2006;408–412:280–3.
[19] Jiang JJ, Lei YQ, Sun DL, Wu J, Wang QD. Mechanism of La, Ce,Nd and Pr on the electrochemical properties ofmulticomponents RE(NiCoMnTi)5 hydrogen storage alloys. JChin Rare Earth Soc 1997;15(4):318–24.
[20] Iwakura C, Oura T, Inoue H, Matsuoka M. Effects ofsubstitution with foreign metals on the crystallographic,thermodynamic and electrochemical properties of AB5-typehydrogen storage alloys. Electrochim Acta 1996;41(1):117–21.
[21] Notten PHL, Hokkeling P. Double-phase hydride formingcompounds: a new class of highly electrocatalytic materials.J Electrochem Soc 1991;138(7):1877–85.
[22] Zheng G, Popov BN, White RE. Electrochemicaldetermination of the diffusion coefficient of hydrogenthrough a LaNi4.25Al0.75 electrode in alkaline aqueoussolution. J Electrochem Soc 1995;142(8):2695–8.