Next Article in Journal
Thermochromic Polymeric Films for Applications in Active Intelligent Packaging—An Overview
Next Article in Special Issue
Suppressed Transmission of Long-Range Surface Plasmon Polariton by TE-Induced Edge Plasmon
Previous Article in Journal
A Computational Fluid Dynamic Study on Efficiency of a Wavy Microchannel/Heat Sink Containing Various Nanoparticles
Previous Article in Special Issue
Macro-Modeling for N-Type Feedback Field-Effect Transistor for Circuit Simulation
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Micromachines
Volume 12
Issue 10
10.3390/mi12101194
micromachines-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Improvement in Hydriding and Dehydriding Features of Mg–TaF5–VCl3 Alloy by Adding Ni and x wt% MgH2 (x = 1, 5, and 10) Together with TaF5 and VCl3

by
Young-Jun Kwak
and
Myoung-Youp Song
*
Division of Advanced Materials Engineering, Jeonbuk National University, 567 Baekje-daero Deokjin-gu, Jeonju 54896, Korea
*
Author to whom correspondence should be addressed.
Micromachines 2021, 12(10), 1194; https://doi.org/10.3390/mi12101194
Submission received: 28 July 2021 / Revised: 14 September 2021 / Accepted: 27 September 2021 / Published: 30 September 2021
(This article belongs to the Special Issue Nano Korea 2021)
Browse Figures
Versions Notes

Abstract

:
In our previous work, TaF5 and VCl3 were added to Mg, leading to the preparation of samples with good hydriding and dehydriding properties. In this work, Ni was added together with TaF5 and VCl3 to increase the reaction rates with hydrogen and the hydrogen-storage capacity of Mg. The addition of Ni together with TaF5 and VCl3 improved the hydriding and dehydriding properties of the TaF5 and VCl3-added Mg. MgH2 was also added with Ni, TaF5, and VCl3 and Mg-x wt% MgH2-1.25 wt% Ni-1.25 wt% TaF5-1.25 wt% VCl3 (x = 0, 1, 5, and 10) were prepared by reactive mechanical milling. The addition of MgH2 decreased the particle size, lowered the temperature at which hydrogen begins to release rapidly, and increased the hydriding and dehydriding rates for the first 5 min. Adding 1 and 5 wt% MgH2 increased the quantity of hydrogen absorbed for 60 min, Ha (60 min), and the quantity of hydrogen released for 60 min, Hd (60 min). The addition of MgH2 improved the hydriding–dehydriding cycling performance. Among the samples, the sample with x = 5 had the highest hydriding and dehydriding rates for the first 5 min and the best cycling performance, with an effective hydrogen-storage capacity of 6.65 wt%.

1. Introduction

Metal hydride storage has advantages over pressure storage and cryogenic storage, as metal hydrides have higher volumetric capacity and metal hydride storage is safer due to the low pressures involved in hydrogen uptake and release [1].
To increase the hydrogen uptake and release rates of magnesium, magnesium (Mg), or magnesium hydride (MgH2) was alloyed [2,3,4,5,6,7,8,9,10] with Ni and Y [11], V [12], and Nb [13]. In addition, Mg or MgH2 was mixed with compounds such as LaNi5 [14], FeTi and FeTiMn [15], Nb2O5 [16], and La2O3 [17]. Mg-containing compounds [18,19,20,21,22] such as La2Mg16Ni [23], LaMg12 and La2Mg17 [24], Mg3Mm (Mm: misch-metal) [25], and Mg17Al12 [26] were synthesized for the same purposes.
Malka et al. [27] reported that certain metal halide additives, especially ZrF4 and NbF5 halides, could significantly influence the sorption properties of MgH2. They reported that the presence of the F anion, which weakened Mg–H bonding, led to the formation of MgF2 and provided an electron-rich center to trap transition metal atoms. They showed that NbF5, TaF5, and particularly TiCl3, took part in the disproportionation reactions that created a significant number of structural defects. Kumar et al. [28] reported that VCl3 was reduced to metallic vanadium during ball milling along with MgH2, and this in situ-formed metallic vanadium doped over the MgH2 surface and showed an excellent catalytic effect on hydrogenation–dehydrogenation of the Mg-MgH2 system. They also reported that a microstructural analysis showed an excellent grain refinement property of VCl3 which reduced the crystallite size of MgH2. Liang et al. [13] improved the hydrogen-storage properties of Mg by adding transition metals such as Ti, V, Mn, Fe, and Ni. In order to find a new route toward improving hydrogen sorption kinetics of Mg nanoparticles, Liu et al. [29] coprecipitated a Mg–Ni nanocomposite from a homogeneous tetrahydrofuran solution containing anhydrous MgCl2, NiCl2, and lithium naphthalide as the reducing agent.
In the present work, we tried to improve the hydriding and dehydriding properties of Mg by adding halides, transition metal, and metal hydride by preparing alloys via reactive mechanical milling. Selected were TaF5 and VCl3 as halides, Ni as a metal, and MgH2 as a metal hydride. Reactive mechanical milling is milling in an atmosphere in which a reaction can occur during that milling. In the present work, milling was performed in a hydrogen atmosphere. In the hydrogen atmosphere, Mg hydride can form during milling through a reaction of Mg with hydrogen.
In our previous work [30], TaF5 and VCl3 were added to Mg. In this work, Ni was added together with TaF5 and VCl3; Ni, TaF5, and VCl3 were added to Mg at the same time. MgH2 was also added to Mg together with Ni, TaF5, and VCl3 at the same time, and Mg-x wt% MgH2-1.25 wt% Ni-1.25 wt% TaF5-1.25 wt% VCl3 (x = 0, 1, 5, and 10) were prepared by reactive mechanical milling. We designated these samples as Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10). The hydriding and dehydriding properties of the prepared samples were then examined. It is thought that the materials developed in our work can be used for motive power fuel and portable appliances as mobile applications, transport and distribution as semi-mobile applications, and industrial off-peak power H2-generation, hydrogen-purifying systems, and heat pumps as stationary applications.

2. Materials and Methods

Pure Mg powder (particle size 74–149 μm, purity 99.6%, Alfa Aesar), Ni (APS 2.2–3.0 μm, purity 99.9% metal basis, C typically < 0.1%, Alfa Aesar, Haverhill, MA, USA), TaF5 (Tantalum (V) fluoride, purity 98%, Aldrich, St. Louis, MI, USA), VCl3 (Vanadium (III) chloride, purity 97%, Aldrich), and pure MgH2 powder (hydrogen storage grade, Aldrich) were used as starting materials.
The compositions of mixtures for reactive mechanical grinding were 96.25 wt% Mg + 1.25 wt% Ni + 1.25 wt% TaF5 + 1.25 wt% VCl3 and (96.25-x) Mg + x wt% MgH2 + 1.25 wt% Ni + 1.25 wt% TaF5 + 1.25 wt% VCl3 (x = 0, 1, 5, and 10). A planetary ball mill (Planetary Mono Mill; Pulverisette 6, Fritsch, Kastl, Germany) with a mill container of 250 mL in volume was used for reactive mechanical grinding. The sample (total weight = 8 g) to ball weight (105 hardened steel balls, total weight = 360 g) ratio was 1:45. All sample handling was performed in an Ar atmosphere. The disc revolution speed was 250 rpm. Reactive mechanical milling was performed in high purity hydrogen gas (≈12 bar) for 6 h by repeating the 20 min cycle of 15 min milling and 5 min rest. Hydrogen was refilled every two hours.
The absorbed and released hydrogen quantity were measured as a function of time by the volumetric method using a Sieverts’ type hydrogen uptake and release apparatus that was previously described [31]. The hydrogen pressure in the sample-containing reactor was maintained to be nearly constant (under 12 bar for the hydrogen uptake reaction and under 1.0 bar for the hydrogen release reaction) using a back-pressure regulator. The back-pressure regulator enables an appropriate amount of hydrogen to be taken from the standard reservoir (with a known volume) and dosed to the reactor during the hydrogen uptake reaction and an appropriate amount of hydrogen to be removed from the reactor to the standard reservoir during the hydrogen release reaction. From the temperature of the standard reservoir and the variation in hydrogen pressure in the standard reservoir (with a known volume) as a function of time, the variation in the absorbed or released hydrogen quantity was calculated as a function of time. The quantity of the samples used to measure the amount of absorbed or released hydrogen as time passed was 0.5 g. The standard deviations of the amount of absorbed and released hydrogen were ±0.07 wt% H.
Samples after reactive mechanical milling were characterized via X-ray diffraction (XRD) with Cu Kα radiation at a scan speed of 4°/min, using a Rigaku D/MAX 2500 powder diffractometer. The MDI JADE 5.0 program was used to analyze the XRD patterns. Scanning electron microscope (SEM) micrographs of the powders were obtained using a JSM-5900 SEM operated at 20 kV. Particle size distributions of the samples after reactive mechanical milling were analyzed by dynamic light scattering in a particle size analyzer (PSA, ASAP2010 Micrometrics, Norcross, GA, USA).

3. Results

The quantities of absorbed and released hydrogen, Ha and Hd, respectively, were defined using sample weight as a criterion. Ha and Hd were expressed in the unit of wt% H. The quantities of hydrogen absorbed and released from the start for x min are expressed by Ha (x min) and Hd (x min), respectively. The hydriding rate for the first 5 min (wt% H/min) was calculated by dividing Ha (5 min) by 5 and the dehydriding rate for the first 5 min (wt% H/min) was calculated by dividing Hd (5 min) by 5.
Figure 1 shows the Ha vs. time t curves at 593 K under 12 bar H2 at the number of cycles, n, of one (n = 1) for Mg-1.25TaF5-1.25VCl3 and Mg-1.25Ni-1.25TaF5-1.25VCl3. Mg-1.25Ni-1.25TaF5-1.25VCl3 has a lower hydriding rate for the first 5 min, but a larger quantity of hydrogen absorbed for 60 min than Mg-1.25TaF5-1.25VCl3. Mg-1.25Ni-1.25TaF5-1.25VCl3 absorbs 2.28 wt% H for 5 min, 3.17 wt% H for 10 min, 5.04 wt% H for 30 min, and 6.12 wt% H for 60 min.
The Hd vs. time t curves at 593 K under 1.0 bar H2 at n = 1 for Mg-1.25TaF5-1.25VCl3 and Mg-1.25Ni-1.25TaF5-1.25VCl3 are shown in Figure 2. Mg-1.25TaF5-1.25VCl3 shows a maximum dehydriding rate after about 20 min. On the other hand, Mg-1.25Ni-1.25TaF5-1.25VCl3 shows a maximum dehydriding rate after about 15 min. Mg-1.25Ni-1.25TaF5-1.25VCl3 has a higher maximum dehydriding rate and a larger quantity of hydrogen released for 60 min than Mg-1.25TaF5-1.25VCl3. Mg-1.25Ni-1.25TaF5-1.25VCl3 releases 0.11 wt% H for 5 min, 0.53 wt% H for 10 min, 4.11 wt% H for 30 min, and 5.70 wt% H for 60 min.
Figure 1 shows that the addition of Ni together with TaF5 and VCl3 increases the quantity of hydrogen absorbed for 60 min of the TaF5 and VCl3-added Mg. Figure 2 shows that the addition of Ni together with TaF5 and VCl3 increases the maximum dehydriding rate and the quantity of hydrogen released for 60 min of the TaF5 and VCl3-added Mg.
X wt% MgH2 (x = 1, 5, and 10) was added together with Ni, TaF5, and VCl3 at the same time with a goal of preparing materials with better hydriding and dehydriding properties.
Figure 3 shows the desorbed hydrogen quantity versus time t curves for the as-milled Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) when the sample was heated with a heating rate of 5–6 K/min. The ranges of temperature where hydrogen is released rapidly are 648–688 K, 579–643 K, 608–625 K, and 570–626 K, respectively. The addition of MgH2 lowers the temperature at which hydrogen begins to release rapidly. The curves of the samples with x = 0 and x = 10 show two stages. The total desorbed hydrogen quantities of the as-milled Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) were 2.24, 2.56, 4.24, and 3.50 wt% H, respectively.
The Ha versus t curves at 593 K under 12 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) are shown in Figure 4. The sample with x = 0 has a quite high hydriding rate for the first 5 min, and the samples with x = 1, 5, and 10 have higher hydriding rates for the first 5 min than the sample with x = 0. The addition of MgH2 increases the hydriding rate for the first 5 min. The sample with x = 1 has the highest hydriding rate for the first 5 min, followed in order by the samples with x = 5, 10, and 0. The sample with x = 1 has the largest quantity of hydrogen absorbed for 60 min, Ha (60 min), followed in order by the samples with x = 5, 0, and 10. The addition of 1 and 5 wt% MgH2 increases Ha (60 min) to 6.72 wt% H (x = 1) and 6.65 wt% H (x = 5) from 6.12 wt% H (x = 0). Mg-1MgH2-1.25Ni-1.25TaF5-1.25VCl3 absorbs 3.20 wt% H for 2.5 min, 5.69 wt% H for 10 min, and 6.72 wt% H for 60 min. We define the effective hydrogen-storage capacity as the quantity of hydrogen absorbed for 60 min. The sample with x = 5 absorbs 5.58 wt% H for 10 min and has an effective hydrogen-storage capacity of 6.65 wt%.
Table 1 presents the variations of the Ha with time and hydriding rates for the first 5 min at 593 K under 12 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
The sample with x = 0 has quite a high hydriding rate for the first 5 min, and the samples with x = 1, 5, and 10 have higher hydriding rates for the first 5 min than the sample with x = 0. The addition of MgH2 increases the hydriding rate for the first 5 min. The samples with x = 1 and 5 have the highest hydriding rate for the first 5 min, followed in order by the samples with x = 10 and 0. The sample with x = 1 has the largest quantity of hydrogen absorbed for 60 min, Ha (60 min), followed in order by the samples with x = 5, 0, and 10. The addition of 1 and 5 wt% MgH2 increases Ha (60 min).
The Hd versus t curves at 593 K under 1.0 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) are shown in Figure 5. The sample with x = 0 exhibits an incubation period of about 2.5 min, and then the dehydriding rate increases gradually. After 15 min, the dehydriding rate of the sample with x = 0 is quite high and becomes very low after 45 min. Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 1, 5, and 10) have quite high dehydriding rates from the start. The addition of MgH2 increases the dehydriding rate for the first 5 min. The sample with x = 5 has the highest dehydriding rate for the first 5 min, followed in order by the samples with x = 10, 1, and 0. The sample with x = 1 has the largest quantity of hydrogen released for 60 min, Hd (60 min), followed in order by the samples with x = 5, 0, and 10. The addition of 1 and 5 wt% MgH2 increases Hd (60 min).
Table 2 presents the variations of Hd with time and the dehydriding rates for the first 5 min at 593 K under 1.0 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
The sample with x = 0 has a very low dehydriding rate for the first 5 min, and the samples with x = 1, 5, and 10 have much higher dehydriding rates for the first 5 min than the sample with x = 0. The sample with x = 5 has the highest dehydriding rate for the first 5 min, followed in order by the samples with x = 10, 1, and 0. The addition of MgH2 increases the dehydriding rate for the first 5 min. The sample with x = 1 has the largest quantity of hydrogen released for 60 min, Hd (60 min), followed in order by the samples with x = 5, 0, and 10. The addition of 1 and 5 wt% MgH2 increases Hd (60 min).
Figure 6 presents the XRD patterns of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) after reactive mechanical milling. The samples contain Mg, β-MgH2, γ-MgH2, Ta, V, Ni, and MgF2. β-MgH2 and γ-MgH2 are formed by a reaction of Mg with hydrogen during reactive mechanical milling. Ta and MgF2 are formed due to a reaction of TaF5 with Mg. V is believed to be formed from a reaction of VCl3 with Mg. The reaction of VCl3 with Mg is reported to form MgCl2 together with V [32]. Ni remains unreacted after reactive mechanical milling. The intensity of the Mg peaks decrease in the samples containing MgH2. This is believed to be due to the decrease in Mg content in MgH2-added samples. Larger decrease in particle size due to reactive mechanical milling with the MgH2 mix is thought to have made the Mg peaks wider.
The SEM micrographs of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) after reactive mechanical milling are presented in Figure 7. Particle sizes are not homogeneous, but Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 1 and 10) exhibit more homogeneous particle sizes than Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0 and 5). The sample with x = 5 has the smallest particle size, followed in order by the samples with x = 1, 10, and 0. The samples with x = 5 and 1 have similar particle sizes. The sample with x = 0, not containing MgH2, has quite large particles, and the particles of this sample form agglomerates. The addition of MgH2 decreases the particle size.
The variations of Ha values for 5 min and 60 min at 593 K under 12 bar H2 with the number of cycles for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) are shown in Figure 8a. The variations of Hd values for 5 min and 60 min at 593 K under 1.0 bar H2 with the number of cycles for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) are shown in Figure 8b. The samples with x = 1, 5, and 10 have better hydriding and dehydriding cycling performance than the sample with x = 0, showing that the addition of MgH2 improves the cycling performance. The sample with x = 5 has the largest value of the quantity of hydrogen absorbed for 5 min, Ha (5 min), at each cycle and the best cycling performance. At n = 1, the sample with x = 1 has the largest value of the quantity of hydrogen absorbed for 60 min, Ha (60 min), and a slightly larger value of Ha (60 min) than the sample with x = 5. At n = 2−4, the sample with x = 5 has the largest values of Ha (60 min). However, the sample with x = 5 has the best cycling performance. The sample with x = 5 has the largest value of the quantity of hydrogen released for 5 min, Hd (5 min), at each cycle, and the best cycling performance. At n = 1, the sample with x = 1 has the largest value of the quantity of hydrogen released for 60 min, Hd (60 min), and a slightly larger value of Hd (60 min) than the sample with x = 5. However, the sample with x = 5 has the best cycling performance.
Figure 9 shows the SEM micrographs of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 5 and 10) after four hydriding and dehydriding cycles. Compared with the particles of these samples after reactive mechanical milling, those of the samples after four hydriding and dehydriding cycles are more agglomerated.

4. Discussion

The weight percentages of additives were relatively small (2.5 and 3.75 wt%) not to sacrifice the hydrogen-storage capacity of the samples. The addition of Ni together with TaF5 and VCl3 increases the quantity of hydrogen absorbed for 60 min of the TaF5 and VCl3-added Mg, as shown in Figure 1. Figure 2 shows that the addition of Ni together with TaF5 and VCl3 increases the maximum dehydriding rate and the quantity of hydrogen released for 60 min of the TaF5 and VCl3-added Mg.
Metallic hydrides are more brittle than their parent metals [33]. MgH2 is brittle [34]. The addition of MgH2 was expected to increase hydriding and dehydriding rates, as MgH2 may be pulverized during milling. To prepare materials with better hydriding and dehydriding properties, x wt% MgH2 (x = 1, 5, and 10) was added together with Ni, TaF5, and VCl3 at the same time.
Figure 3 shows that the as-milled Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 5) has the largest total desorbed hydrogen quantity of 4.24 wt%. Figure 4 shows that the samples with x = 1, 5, and 10 have higher hydriding rates for the first 5 min than the sample with x = 0. The samples with x = 1 and 5 have larger quantities of hydrogen absorbed for 60 min, Ha (60 min) than the sample with x = 0. Figure 5 shows that the samples with x = 1, 5, and 10 have higher dehydriding rates for the first 5 min than the sample with x = 0. The samples with x = 1 and 5 have larger quantities of hydrogen released for 60 min, Hd (60 min), than the sample with x = 0. These results show that the addition of MgH2 increases the hydriding and dehydriding rates for the first 5 min and the additions of 1 and 5 wt% MgH2 increase the quantity of hydrogen absorbed and released for 60 min, Ha (60 min) and Hd (60 min). This proves that the addition of MgH2 made the effects of reactive mechanical milling, which are explained in the following, stronger.
Figure 7 shows that after reactive mechanical milling, the sample with x = 5 has the smallest particle size, followed in order by the samples with x = 1, 10, and 0. Figure 7 also shows that the samples with x = 5 and 1 have similar particle sizes. A comparison of the results in Figure 4 and Figure 5 with the particle sizes in the SEM micrographs in Figure 7 shows that the smaller the particle size, the higher the hydriding rate for the first 5 min and the dehydriding rate for the first 5 min.
The reactive mechanical milling of Mg with Ni, TaF5, and VCl3 is thought to increase the hydriding and dehydriding rates by forming defects [35,36,37,38] (leading to easier nucleation) [39,40,41], making new clean surfaces (leading to an increase in the reactivity of Mg particles with hydrogen) [30,42], and decreasing the particle size of Mg (leading to a decrease in the diffusion distances of hydrogen atoms) [9,10,36,37,38,43]. Especially, the added Ni is believed to form the Mg2Ni phase, which has higher hydriding and dehydriding rates than Mg at the same conditions [36,44], contributing greatly to the increases in the reaction rates. The formed phases (β-MgH2, γ-MgH2, Ta, V, and MgCl2) are believed to help the reactive mechanical milling occur more effectively. The result that the addition of MgH2 increases the hydriding and dehydriding rates for the first 5 min and the result that the additions of 1 and 5 wt% MgH2 increase Ha (60 min) and Hd (60 min) show that the addition of MgH2 makes the effects of reactive mechanical milling stronger. Figure 8 shows that Ha (60 min) values decrease as n increases for all the samples. It is believed that the reason of this behavior is that particles coalesce more and more as n increases. The result that the addition of MgH2 improves the cycling performance, shown in Figure 8, indicates that the added MgH2 prevents particle from coalescing. The formed phases are also believed to help the sample have better cycling performance. After conducting many studies to improve the reaction kinetics of magnesium with hydrogen, researchers reported as the following. The dissociation rate of hydrogen molecules can be improved by adding catalytic metals, for example, Pd [45] and Co, Ni, or Fe [46]. Nucleation can be facilitated by creating active nucleation sites by mechanical treatment and/or alloying with additives [39]. The diffusion distance of hydrogen can be decreased by the mechanical treatment and/or alloying of Mg with additives, thereby reducing the magnesium particle size [43]. In addition, the hydrogen mobility can be improved by additives that create microscopic paths of hydrogen [43]. A rough surface of magnesium having many cracks and defects is thus considered more advantageous for hydrogen absorption [35].
Compared with the microstructures of these samples after reactive mechanical milling (shown in Figure 7), particles after four hydriding and dehydriding cycles are more agglomerated (shown in Figure 9). Agglomeration is believed to have led to the decreases in the absorbed and released hydrogen quantities of the samples.
Among Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10), the samples with x = 1 and 5 have the highest hydriding rate for 5 min at n = 1, but the sample with x = 5 has the highest dehydriding rate for 5 min at n = 1. Among all the samples, the sample with x = 5 has the best cycling performance. The sample with x = 5 absorbs 5.58 wt% H for 10 min and has an effective hydrogen storage capacity of 6.65 wt%.
Table 3 presents the hydrogen-storage capacities of several Mg-based alloys. Conditions of sample preparation and reaction are given. The sample Mg-5MgH2-1.25Ni-1.25TaF5-1.25VCl3 has quite a high hydrogen-storage capacity. It has a higher hydrogen-storage capacity than Ni and Ti-added Mg alloys.

5. Conclusions

The addition of Ni together with TaF5 and VCl3 increased the quantity of hydrogen absorbed for 60 min and increased the maximum dehydriding rate and the quantity of hydrogen released for 60 min of the TaF5 and VCl3-added Mg. MgH2 was added together with Ni, TaF5, and VCl3, and Mg-x wt% MgH2-1.25 wt% Ni-1.25 wt% TaF5-1.25 wt% VCl3 (x = 0, 1, 5, and 10) were prepared by reactive mechanical milling. The addition of MgH2 increased the hydriding and dehydriding rates for the first 5 min, and the additions of 1 and 5 wt% MgH2 increased the quantities of hydrogen absorbed and released for 60 min, denoted Ha (60 min) and Hd (60 min), respectively. The comparison of Hd versus t and Ha versus t curves with SEM micrographs after reactive mechanical milling showed that the smaller the particle size, the higher the hydriding rate for the first 5 min, and the dehydriding rate for the first 5 min. The reactive mechanical milling of Mg with Ni, TaF5, and VCl3 is thought to increase the hydriding and dehydriding rates by forming defects, making new clean surfaces, and decreasing the particle size of Mg. The addition of MgH2 made the effects of reactive mechanical milling stronger. The formed phases (β-MgH2, γ-MgH2, Ta, V, and MgCl2) are also believed to have made these effects stronger. The addition of MgH2 improved cycling performance by preventing particles from coalescing. The formed phases are also believed to have helped the sample have the better cycling performance. Among Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10), the sample with x = 5 had the highest hydriding and dehydriding rates for the first 5 min and the best cycling performance. The sample with x = 5 absorbed 5.58 wt% H for 10 min and had an effective hydrogen-storage capacity of 6.65 wt%.

Author Contributions

Conceptualization, Y.-J.K. and M.-Y.S.; methodology, Y.-J.K. and M.-Y.S.; investigation, Y.-J.K. and M.-Y.S.; data analysis, Y.-J.K. and M.-Y.S.; writing—original draft preparation, Y.-J.K. and M.-Y.S.; writing—review and editing, Y.-J.K. and M.-Y.S. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Von Colbe, J.B.; Ares, J.-R.; Barale, J.; Baricco, M.; Buckley, C.; Capurso, G.; Gallandat, N.; Grant, D.; Guzik, M.N.; Jacob, I.; et al. Application of hydrides in hydrogen storage and compression: Achievements, outlook and perspectives. Int. J. Hydrog. Energy 2019, 44, 7780–7808. [Google Scholar] [CrossRef]
  2. Zhang, X.; Liu, Y.; Ren, Z.; Zhang, X.; Hu, J.; Huang, Z.; Lu, Y.; Gao, M.; Pan, H. Realizing 6.7 wt% reversible storage of hydrogen at ambient temperature with non-confined ultrafine magnesium hydrides. Energy Environ. Sci. 2020, 14, 2302–2313. [Google Scholar] [CrossRef]
  3. Liao, W.; Jiang, W.; Yang, X.-S.; Wang, H.; Ouyang, L.; Zhu, M. Enhancing (de)hydrogenation kinetics properties of the Mg/MgH2 system by adding ANi5 (A = Ce, Nd, Pr, Sm, and Y) alloys via ball milling. J. Rare Earths 2020, 39, 1010–1016. [Google Scholar] [CrossRef]
  4. Pukazhselvan, D.; Sandhya, K.; Nasani, N.; Fagg, D.P. Chemical transformation of additive phase in MgH2/CeO2 hydrogen storage system and its effect on catalytic performance. Appl. Surf. Sci. 2021, 561, 150062. [Google Scholar] [CrossRef]
  5. Paul, D.R.; Sharma, A.; Panchal, P.; Chaudhary, S.; Patidar, D.; Nehra, S. Effect of ball milling and iron mixing on structural and morphological properties of magnesium for hydrogen storage application. Mater. Today Proc. 2020, 42, 1673–1677. [Google Scholar] [CrossRef]
  6. Berezovets, V.; Denys, R.; Zavaliy, I.; Kosarchyn, Y. Effect of Ti-based nanosized additives on the hydrogen storage properties of MgH2. Int. J. Hydrog. Energy 2021. [Google Scholar] [CrossRef]
  7. Yin, Y.; Li, B.; Yuan, Z.; Qi, Y.; Zhang, Y. Enhanced hydrogen storage performance of Mg-Cu-Ni system catalyzed by CeO2 additive. J. Rare Earths 2019, 38, 983–993. [Google Scholar] [CrossRef]
  8. Liu, P.; Chen, H.; Yu, H.; Liu, X.; Jiang, R.; Li, X.; Zhou, S. Oxygen vacancy in magnesium/cerium composite from ball milling for hydrogen storage improvement. Int. J. Hydrog. Energy 2019, 44, 13606–13612. [Google Scholar] [CrossRef]
  9. Song, M.Y.; Choi, E.; Kwak, Y.J. Increase in the dehydrogenation rates and hydrogen-storage capacity of Mg-graphene composites by adding nickel via reactive ball milling. Mater. Res. Bull. 2020, 130, 110938. [Google Scholar] [CrossRef]
  10. Song, M.Y.; Lee, S.H.; Kwak, Y.J. Improvement in the hydrogenation and dehydrogenation features of Mg by milling in hydrogen with vanadium chloride. Korean J. Met. Mater. 2021, 59, 721–729. [Google Scholar] [CrossRef]
  11. Li, Z.; Liu, X.; Jiang, L.; Wang, S. Characterization of Mg–20 wt% Ni–Y hydrogen storage composite prepared by reactive mechanical alloying. Int. J. Hydrog. Energy 2007, 32, 1869–1874. [Google Scholar] [CrossRef]
  12. Liang, G.; Huot, J.; Boily, S.; Van Neste, A.; Schulz, R. Hydrogen storage properties of the mechanically milled MgH2–V nanocomposite. J. Alloy. Compd. 1999, 291, 295–299. [Google Scholar] [CrossRef]
  13. Huot, J.; Pelletier, J.; Lurio, L.; Sutton, M.; Schulz, R. Investigation of dehydrogenation mechanism of MgH2–Nb nanocomposites. J. Alloy. Compd. 2003, 348, 319–324. [Google Scholar] [CrossRef]
  14. Fu, Y.; Groll, M.; Mertz, R.; Kulenovic, R. Effect of LaNi5 and additional catalysts on hydrogen storage properties of Mg. J. Alloy. Compd. 2008, 460, 607–613. [Google Scholar] [CrossRef]
  15. Vijay, R.; Sundaresan, R.; Maiya, M.; Murthy, S.S.; Fu, Y.; Klein, H.-P.; Groll, M. Characterisation of Mg–x wt.% FeTi (x = 5–30) and Mg–40 wt.% FeTiMn hydrogen absorbing materials prepared by mechanical alloying. J. Alloy. Compd. 2004, 384, 283–295. [Google Scholar] [CrossRef]
  16. Friedrichs, O.; Klassen, T.; Sanchez-Lopez, J.C.; Bormann, R.; Fernandez, A. Hydrogen sorption improvement of nanocrystalline MgH2 by Nb2O5 nanoparticles. Scr. Mater. 2006, 54, 1293–1297. [Google Scholar] [CrossRef]
  17. Gupta, R.; Agresti, F.; Russo, S.L.; Maddalena, A.; Palade, P.; Principi, G. Structure and hydrogen storage properties of MgH2 catalysed with La2O3. J. Alloy. Compd. 2008, 450, 310–313. [Google Scholar] [CrossRef]
  18. Zhang, Y.; Zhang, W.; Wei, X.; Yuan, Z.; Gao, J.; Guo, S.; Ren, H. Catalytic effects of TiO2 on hydrogen storage thermodynamics and kinetics of the as-milled Mg-based alloy. Mater. Charact. 2021, 176, 111118. [Google Scholar] [CrossRef]
  19. Zhang, Y.; Wei, X.; Zhang, W.; Yuan, Z.; Gao, J.; Ren, H. Catalytic effect comparison of TiO2 and La2O3 on hydrogen storage thermodynamics and kinetics of the as-milled La-Sm-Mg-Ni-based alloy. J. Magnes. Alloy 2021. [Google Scholar] [CrossRef]
  20. Zhang, Y.; Wei, X.; Zhang, W.; Yuan, Z.; Gao, J.; Qi, Y.; Ren, H. Effect of milling duration on hydrogen storage thermodynamics and kinetics of Mg-based alloy. Int. J. Hydrog. Energy 2020, 45, 33832–33845. [Google Scholar] [CrossRef]
  21. Yong, H.; Wei, X.; Zhang, K.; Wang, S.; Zhao, D.; Hu, J.; Zhang, Y. Characterization of microstructure, hydrogen storage kinetics and thermodynamics of ball-milled Mg90Y1.5Ce1.5Ni7 alloy. Int. J. Hydrog. Energy 2021, 46, 17802–17813. [Google Scholar] [CrossRef]
  22. Hou, Z.; Wei, X.; Zhang, W.; Yuan, Z.; Ge, Q. Electrochemical hydrogen storage performances of Mg–Ti–Ni–Co–Al-based alloys prepared by mechanical milling. J. Phys. Chem. Solids 2021, 149, 109788. [Google Scholar] [CrossRef]
  23. Wang, W.; Chen, C.; Chen, L.; Wang, Q. Change in structure and hydrogen storage properties of La2Mg16Ni alloy after modification by mechanical grinding in tetrahydrofuran. J. Alloy. Compd. 2002, 339, 175–179. [Google Scholar] [CrossRef]
  24. Sun, D.; Gingl, F.; Nakamura, Y.; Enoki, H.; Bououdina, M.; Akiba, E. In situ X-ray diffraction study of hydrogen-induced phase decomposition in LaMg12 and La2Mg17. J. Alloy. Compd. 2002, 333, 103–108. [Google Scholar] [CrossRef]
  25. Ouyang, L.; Dong, H.; Zhu, M. Mg3Mm compound based hydrogen storage materials. J. Alloy. Compd. 2007, 446-447, 124–128. [Google Scholar] [CrossRef]
  26. Yabe, H.; Kuji, T. Thermal stability and hydrogen absorption/desorption properties of Mg17Al12 produced by bulk mechanical alloying. J. Alloy. Compd. 2007, 433, 241–245. [Google Scholar] [CrossRef]
  27. Malka, I.; Pisarek, M.; Czujko, T.; Bystrzycki, J. A study of the ZrF4, NbF5, TaF5, and TiCl3 influences on the MgH2 sorption properties. Int. J. Hydrog. Energy 2011, 36, 12909–12917. [Google Scholar] [CrossRef]
  28. Kumar, S.; Singh, P.K.; Rao, G.N.; Kojima, Y.; Kain, V. Synergic effect of vanadium trichloride on the reversible hydrogen storage performance of the Mg MgH2 system. Int. J. Hydrog. Energy 2018, 43, 15330–15337. [Google Scholar] [CrossRef]
  29. Liu, Y.; Zou, J.; Zeng, X.; Wu, X.; Li, D.; Ding, W. Hydrogen storage properties of a Mg–Ni nanocomposite coprecipitated from solution. J. Phys. Chem. C 2014, 118, 18401–18411. [Google Scholar] [CrossRef]
  30. Kwak, Y.J.; Song, M.Y. Enhancement of the hydrogen uptake and release rates of Mg by the addition of TaF5 and VCl3 with reactive mechanical grinding. Nanosci. Nanotechnol. Lett. 2018, 10, 772–778. [Google Scholar] [CrossRef]
  31. Song, M.Y.; Baek, S.H.; Bobet, J.-L.; Hong, S.-H. Hydrogen storage properties of a Mg–Ni–Fe mixture prepared via planetary ball milling in a H2 atmosphere. Int. J. Hydrog. Energy 2010, 35, 10366–10372. [Google Scholar] [CrossRef]
  32. da Conceição, M.; Brum, M.; dos Santos, D. The effect of V, VCl3 and VC catalysts on the MgH2 hydrogen sorption properties. J. Alloy. Compd. 2014, 586, S101–S104. [Google Scholar] [CrossRef]
  33. Mandzhukova, T.; Bobet, J.-L.; Khrussanova, M.; Peshev, P. Hydrogen sorption properties of MgH2–NiCo2O4 composites activated mechanically under argon and hydrogen atmospheres. Mater. Res. Bull. 2009, 44, 1968–1972. [Google Scholar] [CrossRef]
  34. Metallic hydrides. Available online: https://www.toppr.com/ask/content/story/amp/metallic-hydrides-9178/ (accessed on 14 September 2021).
  35. Vigeholm, B.; Kjøller, J.; Larsen, B.; Pedersen, A. Formation and decomposition of magnesium hydride. J. Less Common Met. 1983, 89, 135–144. [Google Scholar] [CrossRef]
  36. Song, M.; Ivanov, E.; Darriet, B.; Pezat, M.; Hagenmuller, P. Hydriding and dehydriding characteristics of mechanically alloyed mixtures Mg-x wt.% Ni (x = 5, 10, 25 and 55). J. Less Common Met. 1987, 131, 71–79. [Google Scholar] [CrossRef]
  37. Song, M.Y. Effects of mechanical alloying on the hydrogen storage characteristics of Mg-x wt% Ni (x = 0, 5, 10, 25 and 55) mixtures. Int. J. Hydrog. Energy 1995, 20, 221–227. [Google Scholar] [CrossRef]
  38. Song, M.Y. Improvement in hydrogen storage characteristics of magnesium by mechanical alloying with nickel. J. Mater. Sci. 1995, 30, 1343–1351. [Google Scholar] [CrossRef]
  39. Hjort, P.; Krozer, A.; Kasemo, B. Hydrogen sorption kinetics in partly oxidized Mg films. J. Alloy. Compd. 1996, 237, 74–80. [Google Scholar] [CrossRef]
  40. Song, M.Y.; Choi, E.; Kwak, Y.J. Preparation of a Mg-based alloy with a high hydrogen-storage capacity by adding a polymer CMC via milling in a hydrogen atmosphere. Int. J. Hydrog. Energy 2019, 44, 3779–3789. [Google Scholar] [CrossRef]
  41. Song, M.Y.; Choi, E.; Kwak, Y.J. Increase in the dehydrogenation rate of Mg–CMC (Carboxymethylcellulose, Sodium Salt) by adding Ni via hydride-forming milling. Met. Mater. Int. 2018, 25, 516–527. [Google Scholar] [CrossRef]
  42. Song, M.Y.; Kwak, Y.J. Effects of Zn(BH4)2, Ni, and/or Ti doping on the hydrogen-storage features of MgH2. Korean J. Met. Mater. 2019, 57, 176–183. [Google Scholar] [CrossRef] [Green Version]
  43. Zaluska, A.; Zaluski, L.; Ström–Olsen, J. Nanocrystalline magnesium for hydrogen storage. J. Alloy. Compd. 1999, 288, 217–225. [Google Scholar] [CrossRef]
  44. Reilly, J.J.; Wiswall, R.H. Reaction of hydrogen with alloys of magnesium and nickel and the formation of Mg2NiH4. Inorg. Chem. 1968, 7, 2254–2256. [Google Scholar] [CrossRef]
  45. Krozer, A.; Kasemo, B. Equilibrium hydrogen uptake and associated kinetics for the Mg-H2 system at low pressures. J. Phys. Condens. Matter 1989, 1, 1533–1538. [Google Scholar] [CrossRef]
  46. Stillesjö, F.; Ólafsson, S.; Hjörvarsson, B.; Karlsson, E. Hydride formation in Mg/Ni-sandwiches studied by hydrogen profiling and volumetric measurements. Z. Phys. Chem. 1993, 181, 353–358. [Google Scholar] [CrossRef]
  47. Song, M.Y.; Kwak, Y.J. Enhancement of the hydrogenation and dehydrogenation characteristics of Mg by adding small amounts of nickel and titanium. Mater. Sci. 2021. [Google Scholar] [CrossRef]
Micromachines 12 01194 g001 550
Figure 1. Ha vs. t curves at 593 K under 12 bar H2 at n = 1 for Mg-1.25TaF5-1.25VCl3 and Mg-1.25Ni-1.25TaF5-1.25VCl3.
Figure 1. Ha vs. t curves at 593 K under 12 bar H2 at n = 1 for Mg-1.25TaF5-1.25VCl3 and Mg-1.25Ni-1.25TaF5-1.25VCl3.
Micromachines 12 01194 g001
Micromachines 12 01194 g002 550
Figure 2. Hd vs. t curves at 593 K under 1.0 bar H2 at n = 1 for Mg-1.25TaF5-1.25VCl3 and Mg-1.25Ni-1.25TaF5-1.25VCl3.
Figure 2. Hd vs. t curves at 593 K under 1.0 bar H2 at n = 1 for Mg-1.25TaF5-1.25VCl3 and Mg-1.25Ni-1.25TaF5-1.25VCl3.
Micromachines 12 01194 g002
Micromachines 12 01194 g003a 550Micromachines 12 01194 g003b 550
Figure 3. Desorbed hydrogen quantity versus time t curves for the as-milled Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3; (a) x = 0, (b) x = 1, (c) x = 5, and (d) x = 10 when the sample was heated with a heating rate of 5–6 K/min.
Figure 3. Desorbed hydrogen quantity versus time t curves for the as-milled Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3; (a) x = 0, (b) x = 1, (c) x = 5, and (d) x = 10 when the sample was heated with a heating rate of 5–6 K/min.
Micromachines 12 01194 g003aMicromachines 12 01194 g003b
Micromachines 12 01194 g004 550
Figure 4. Ha versus t curves at 593 K under 12 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Figure 4. Ha versus t curves at 593 K under 12 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Micromachines 12 01194 g004
Micromachines 12 01194 g005 550
Figure 5. Hd versus t curves at 593 K under 1.0 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Figure 5. Hd versus t curves at 593 K under 1.0 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Micromachines 12 01194 g005
Micromachines 12 01194 g006 550
Figure 6. XRD patterns of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) after reactive mechanical milling.
Figure 6. XRD patterns of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10) after reactive mechanical milling.
Micromachines 12 01194 g006
Micromachines 12 01194 g007 550
Figure 7. SEM micrographs of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 1, 1, 5, and 10) after reactive mechanical milling; (a) x = 0, (b) x = 1, (c) x = 5, and (d) x = 10.
Figure 7. SEM micrographs of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 1, 1, 5, and 10) after reactive mechanical milling; (a) x = 0, (b) x = 1, (c) x = 5, and (d) x = 10.
Micromachines 12 01194 g007
Micromachines 12 01194 g008 550
Figure 8. Variations of (a) Ha values for 5 min and 60 min at 593 K under 12 bar H2 and (b) Hd values for 5 min and 60 min at 593 K under 1.0 bar H2 with the number of cycles for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Figure 8. Variations of (a) Ha values for 5 min and 60 min at 593 K under 12 bar H2 and (b) Hd values for 5 min and 60 min at 593 K under 1.0 bar H2 with the number of cycles for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Micromachines 12 01194 g008
Micromachines 12 01194 g009 550
Figure 9. SEM micrographs of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 5 and 10) after four hydriding and dehydriding cycles; (a) x = 5 and (b) x = 10.
Figure 9. SEM micrographs of Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 5 and 10) after four hydriding and dehydriding cycles; (a) x = 5 and (b) x = 10.
Micromachines 12 01194 g009
Table
Table 1. Variations of the Ha with time and hydriding rates for the first 5 min at 593 K under 12 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Table 1. Variations of the Ha with time and hydriding rates for the first 5 min at 593 K under 12 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3
at 593 K		Ha (wt% H)Hydriding Rate for the First 5 min
(wt% H/min)
2.5 min5 min10 min30 min60 min
x = 01.472.283.175.046.120.456
x = 13.24.595.696.526.720.917
x = 53.174.595.586.456.650.917
x = 102.773.914.665.425.570.783
Table
Table 2. Variations of the Hd with time and the dehydriding rates for the first 5 min at 593 K under 1.0 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Table 2. Variations of the Hd with time and the dehydriding rates for the first 5 min at 593 K under 1.0 bar H2 at n = 1 for Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3 (x = 0, 1, 5, and 10).
Mg-xMgH2-1.25Ni-1.25TaF5-1.25VCl3
at 593 K		Hd (wt% H)Dehydriding Rate for the First 5 min
(wt% H/min)
2.5 min5 min10 min30 min60 min
x = 0 0.050.110.534.115.700.023
x = 10.741.382.625.826.240.276
x = 50.941.682.975.876.050.336
x = 100.761.502.955.185.200.299
Table
Table 3. Hydrogen-storage capacities of several Mg-based alloys.
Table 3. Hydrogen-storage capacities of several Mg-based alloys.
CompositionBall Milling Time (h)Reaction Temperature (K)Reaction Hydrogen Pressure (Bar H2)Hydrogen- Storage Capacity (wt% H)Reference
Mg-2.5TaF5-2.5VCl36593125.86 (n = 1)[30]
Mg-1.25TaF5-1.25VCl36593125.36 (n = 1)this work
Mg-1.25Ni-1.25TaF5-1.25VCl36593126.12 (n = 1)this work
Mg-5MgH2-1.25Ni-1.25TaF5-1.25VCl36593126.65 (n = 1)this work
Mg-14Ni-6Ti6573124.98[27]
Mg-1.25Ni-1.25Ti6593125.91[47]
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Share and Cite

MDPI and ACS Style

Kwak, Y.-J.; Song, M.-Y. Improvement in Hydriding and Dehydriding Features of Mg–TaF5–VCl3 Alloy by Adding Ni and x wt% MgH2 (x = 1, 5, and 10) Together with TaF5 and VCl3. Micromachines 2021, 12, 1194. https://doi.org/10.3390/mi12101194

AMA Style

Kwak Y-J, Song M-Y. Improvement in Hydriding and Dehydriding Features of Mg–TaF5–VCl3 Alloy by Adding Ni and x wt% MgH2 (x = 1, 5, and 10) Together with TaF5 and VCl3. Micromachines. 2021; 12(10):1194. https://doi.org/10.3390/mi12101194

Chicago/Turabian Style

Kwak, Young-Jun, and Myoung-Youp Song. 2021. "Improvement in Hydriding and Dehydriding Features of Mg–TaF5–VCl3 Alloy by Adding Ni and x wt% MgH2 (x = 1, 5, and 10) Together with TaF5 and VCl3" Micromachines 12, no. 10: 1194. https://doi.org/10.3390/mi12101194

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop