Li Chen*ab,
Changyi Hua and
Feng Liub
aKunming University of Science and Technology, Kunming 650093, China
bKunming Institute of Precious Metals, Kunming 650106, China. E-mail: 669282531@qq.com
First published on 5th February 2019
The present work reports the fabrication of Mg89RE11 (RE = Pr, Sm, Nd) alloys by a vacuum induction furnace. The phase analysis, structure characterization and microstructure observation of Mg89RE11 alloys were carried out by X-ray diffraction (XRD), scanning electron microscopy (SEM) and transmission electron microscopy (TEM). There exhibits a multiphase microstructure in the as-cast Mg89RE11 (RE = Pr, Nd, Sm) alloys from the comprehensive analysis made from XRD and SEM, which are containing the major phase (RE5Mg41) and several secondary phases (REMg3 and REMg12). The detections of XRD and TEM reveal that these experimental alloys turn into a MgH2 nanocrystalline composite with equably distributed RE hydride nanoparticles after hydriding and this MgH2 major phase turns into a Mg nanocrystalline after dehydriding. The determination results of the hydrogen storage kinetics show that adding the rare earth element (Pr, Sm and Nd) ameliorates the hydriding and dehydriding kinetics of the Mg-based alloys dramatically. The hydrogen desorption activation energy Ea(de) of Mg89Pr11, Mg89Nd11, Mg89Sm11 are 140.595, 139.191, 135.280 kJ mol−1 H2, respectively. Specially, the hydrogen storage capacity (wt%) of Mg89Sm11 alloy that added Sm element can reached 5 wt%. The improvement of the hydrogen storage performance of Mg89RE11 alloys can be principally ascribed to the RE hydride nanoparticles facilitating the hydriding and dehydriding reactions.
So far, a variety of chemical elements, such as In,5–7 Ni,8–10 Zr,11,12 Ag,13 Al,14,15 Ti,16,17 rare earth (RE) elements18 and their composites,19–23 have been exploited as the alloying elements for the Mg-based alloys. Among them, adding RE elements attracts extensive interest for the Mg-based alloys due to its excellent improvement of the hydriding/dehydriding rate, which may be a better choice to meet the requirements of future hydrogen energy storage systems.24–29 Therefore, the addition of rare earth elements into Mg-based alloys as alloying elements shed light on the better hydrogen storage properties for alloys. The hydrogen storage capacity of La2Mg17 reaches 6 wt% at the temperature of 350 °C.30 The Mg3La compound prepared by induction melting can absorb 2.89 wt% of hydrogen reversibly at 296 °C.31 Wu et al.32 investigated the hydrogen storage properties and phase transitions of Mg17Ba2, which has reversible hydrogen capacity of 4.0 wt% H2. Ma et al.33,34 proposed the addition of Ni to the CaMg2-based alloys resulted in room-temperature hydrogen absorption without an activation process, and a maximum hydrogen-absorption capacity of 5.65 wt%. Moreover, dual-tuning effects of the thermodynamics and kinetics for Mg-based materials is one of the key issues for hydrogen economy and hydrogen storage materials.35–37 Cao et al.35 found that the Mg85In5Al5Ti5 alloy displays both enhanced dehydriding kinetics and thermodynamics, which is prepared by plasma milling (P-milling).36 The addition of In into Mg2Ni not only greatly enhanced the dehydriding kinetics but also significantly lowered the thermodynamic stability.37
Although the research of Mg-based hydrogen storage alloys has made much substantial progress, the cost of hydrogen storage alloys has been increased by high alloying element content, and the hydrogen storage performance needs to be further improved. In this work, we report a time-saving vacuum inducing smelting method to synthesize low alloying Mg89RE11 (RE = Pr, Nd, Sm) binary alloys as new hydrogen storage materials. On the one hand, we evaluated hydrogen storage properties of the Mg89RE11 (RE = Pr, Nd, Sm) binary alloys. On the other hand, we deeply discussed the hydriding and dehydriding mechanism for the Mg89RE11 (RE = Pr, Nd, Sm) binary alloys further.
Some microstructures of the samples, including microscopic morphology, phase composition and crystal structure, were observed and characterized by TEM (JEM-2100F) linked with an SAED (selected area electron diffraction), SEM (FEI Quanta 400) linked with an EDS (Energy Disperse Spectroscopy, EDAX Apollo 40 silicon drift detector). For phase analysis, XRD (D/max/2400) technique was employed.
A series of tests on the kinetics of hydrogen absorption and desorption of alloys were carried out on an automatically controlled Sieverts apparatus. The alloys used in above test need to be mechanically pulverized in advance and the powder between 48–75 μm is screened for testing. The sample weighing 1 g was put into the reaction chamber and repeatedly absorbed/desorbed hydrogen until completely activated. When the initial hydrogen pressure of hydriding process was set at 3 MPa, the hydrogen absorption experiment was carried out in the temperature range of 150–380 °C. At the same temperature, the initial hydrogen pressure in hydrogen desorption was set at 1 × 10−4 MPa.
Fig. 2 displays the SEM micrographs of as-cast Mg89RE11 (RE = Pr, Nd, Sm) binary alloys. Taking as-cast Mg89Sm11 alloy as an example, the EDS patterns of A and B regions are depicted to represent the alloy content of each region. The two regions with different degrees of darkness in the as-cast alloy represent the two-phase structure of the alloy. The results combining the EDS and XRD analysis show that the white and dark gray areas are SmMg3 and Sm5Mg41, respectively.
Fig. 2 SEM micrographs and EDS of as-cast samples for Mg89RE11 (RE = Pr, Nd, Sm) alloys: (a) RE = Pr; (b) RE = Nd; (c) RE = Sm. |
Mg89Pr11 + H2 → PrH2 + Pr8H18.96 + MgH2 ↔ PrH2 + Mg + H2 | (1) |
Mg89Nd11 + H2 →Nd2H5 + MgH2 ↔ Nd2H5 + Mg + H2 | (2) |
Mg89Sm11 + H2 → Sm3H7 + MgH2 ↔ Sm3H7 + Mg + H2 | (3) |
The fundamental reason for reversible hydrogen absorption/desorption of the active Mg89RE11 (RE = Pr, Nd, Sm) binary alloys is coming from the formation and decomposition of MgH2.
Fig. 4 shows the TEM and HRTEM micrographs and SAED rings of the fully hydrogen desorption samples at 380 °C for Mg89RE11 (RE = Pr, Nd, Sm) alloy. According to the inset of Fig. 4(a)–(c), the alloys are composed of the Mg and REHx (PrH2, Nd2H5 and Sm3H7) nanocrystal phases, which conforms to the XRD detections. As the observation of the internal lattice structure from HRTEM (Fig. 4(d)), the interplanar spacing of Mg nanocrystalline on (100) crystal surface is 0.278 nm and the secondary phase Sm3H7 nanocrystal on (101) crystal surface is 0.309 nm. The hydrogen absorption alloy turns into a Mg nanocrystalline composite with equably distributed Sm3H7 nanoparticles (<100 nm) after dehydriding. The mechanism of the nucleation and growth of the formed REHx (PrH2, Nd2H5 and Sm3H7) composites is similar to CeH2.73–MgH2–Ni composites.39 It can be found that the secondary phase PrH2, Pr8H18.96, Nd2H5 and Sm3H7 served as catalysts39 affect the hydrogen absorption and desorption rates.
Fig. 4 TEM and HRTEM micrographs and SAED rings of the hydrogen desorption samples for Mg89RE11 (RE = Pr, Nd, Sm) alloy: (a) RE = Pr; (b) RE = Nd; (c) and (d) RE = Sm. |
ln[−ln(1 − α)] = ηlnk + ηlnt | (4) |
k = Aexp[−Ea/RT] | (5) |
Fig. 5(a) shows the hydrogen absorption curves of the Mg89Pr11 alloy, which were measured at 150 to 380 °C under the initial hydrogen pressure of 3 MPa. The increase of hydrogen absorption capacity will bring with the increase of the temperature for the alloy. It can be suggested that increasing temperature facilitates the improvement of the hydriding kinetics of the alloy. In terms of specific data, the hydrogen absorption capacity of 3.712 wt% for the alloy can be reached within 10 min at 250 °C, compared to only 2.4 wt% for pure MgH2 even if it lasts 20 min and under the same condition.42 Fig. 5(b) displays the hydrogen desorption curves of the Mg89Pr11 alloy, which were measured at 300 to 360 °C under 1 × 10−4 MPa pressure. The final hydrogen desorption capacity of 4.7 wt% for this alloy is lower than own hydrogen absorption capacity due to the lower final hydrogen pressure (<1 × 10−2 MPa) of the test system. The hydrogen desorption of the hydrogenated alloy at 320 °C, 340 °C and 360 °C have finished within 10350 s, 3195 s and 2025 s, respectively. Compared to no decomposition for the milled MgH2 at 300 °C, 3.15 wt% H for the Mg89Pr11 alloy is desorbed in 200 min, suggesting that this alloy displays a good desorption kinetics. Fig. 5(c) and (d) illustrate the Arrhenius plot of lnk vs. 1000/RT under hydrogenation and dehydrogenation conditions, respectively. The calculated activation energy for the hydrogenation (Ea(ab) = 90.35 kJ mol−1) is much lower than that of Mg powder after cyclic activation process (100 kJ mol−1).43 For the dehydrogenation, the values of activation energy are 160 and 156 kJ mol−1 for un-milled MgH2 (ref. 44 and 45) and the value of which is 158.5 kJ mol−1 for pure milled MgH2,46 which values all show larger than the calculated Ea(de) value (140.60 kJ mol−1) for the Mg89Pr11 alloy.
Fig. 5 Isothermal hydrogen absorption (a) and desorption (b) kinetic curves of Pr11Mg89 alloy at different temperatures and the corresponding Arrhenius plots ((c) and (d)). |
In the initial pressure in the 3 Mpa, the hydrogen absorption curves of the Mg89Nd11 alloy tested at temperatures ranging from 150 to 380 °C are displayed in Fig. 6(a). The hydrogen absorption capacity of the alloy increases from 2.403 wt% at 150 °C to 4.491 wt% at 380 °C. It can be found that the increase of the temperature facilitates the improvement of the hydriding kinetics of the alloy. Under the condition of 250 °C, the hydrogen absorption capacity of 3.712 wt% for the alloy could reach within 10 min. Fig. 6(b) exhibits the hydrogen desorption curves of the Mg89Nd11 alloy measured at 300 to 360 °C under 1 × 10−4 MPa pressure. The final hydrogen desorption capacity of 4.7 wt% for the alloy is also lower than the hydrogen absorption capacity. The hydrogen desorption of the hydrogenated alloy at 320 °C, 340 °C and 360 °C have finished within 8235 s, 3420 s and 1890 s, respectively. Unlike no decomposition for the milled MgH2 at 300 °C, 3.45 wt% H for the Mg89Nd11 alloy is desorbed in 200 min. Fig. 6(c) and (d) illustrate the Arrhenius plot of lnk vs. 1000/RT that is able to reflect the hydrogenation and dehydrogenation kinetics of the Mg89Nd11 alloy. The calculated Ea(ab) value (84.072 kJ mol−1) is also much lower than that of Mg powder (100 kJ mol−1). For the dehydrogenation, the Ea(de) value from calculating is 139.193 kJ mol−1 approximately.
Fig. 6 Isothermal hydrogen absorption (a) and desorption (b) kinetic curves of Nd11Mg89 alloy at different temperatures and the corresponding Arrhenius plots ((c) and (d)). |
The hydrogen absorption curves of the Mg89Sm11 alloy, which were measured at 150 to 380 °C under 3 MPa hydrogen pressure, shows in Fig. 7(a). The hydrogen absorption capacity of the alloy increases from 2.803 wt% at 150 °C to 5.022 wt% at 380 °C, suggesting that the increasing temperature promotes the improvement of the hydriding kinetics. The hydrogen absorption capacity of 4.112 wt% for the alloy can achieve within 10 min at 250 °C. The hydrogen desorption curves of the Mg89Sm11 alloy tested at 300 to 360 °C under 1 × 10−4 MPa are depicted in Fig. 7(b). The final hydrogen desorption capacity of 5.0 wt% for the alloy is lower than the hydrogen absorption capacity. Length of time for the completion of hydrogen desorption of the hydrogenated alloy at 320 °C, 340 °C and 360 °C have finished within 6556 s, 2527 s and 1106 s, respectively. Compared to no decomposition for the milled MgH2 at 300 °C, 3.572 wt% H for the Mg89Sm11 alloy is desorbed in 200 min. The Arrhenius plot of lnk vs. 1000/RT for the hydrogenation and dehydrogenation kinetics are displayed in Fig. 7(c) and (d). The calculated Ea(ab) and Ea(de) values are about 77.802 kJ mol−1 135.280 kJ mol−1, respectively.
Fig. 7 Isothermal hydrogen absorption (a) and desorption (b) kinetic curves of Sm11Mg89 alloy at different temperatures and the corresponding Arrhenius plots ((c) and (d)). |
Synthesizing the above analysis, the hydrogen storage kinetics properties of Mg89RE11 (RE = Pr, Nd, Sm) alloys are listed in the Table 1. For Mg89RE11 (RE = Pr, Nd, Sm) alloys, the order of hydrogen absorption and desorption rate is Sm > Nd > Pr. However, the apparent activation energy (Ea) both absorption and desorption course are all decreased, and the order is Sm < Nd < Pr. It can be concluded that the Mg89Sm11 alloy is the highest hydrogen storage kinetics properties alloy. The results shows that the hydrogen sorption properties of Mg-based alloys can be substantially improved by forming composites having catalytic effect and proper microstructure features.47–49
Mg89RE11 alloy | 250 °C, capacity within 10 min | 320 °C, complete dehydrogenation time | Ea(ab) kJ mol−1 | Ea(de) kJ mol−1 |
---|---|---|---|---|
RE = Pr | 3.712 wt% | 10350 s | 90.35 | 140.60 |
RE = Nd | 3.895 wt% | 8235 s | 84.07 | 139.19 |
RE = Sm | 4.112 wt% | 6556 s | 77.802 | 135.28 |
MgH2 (ref. 42–45) | 2.4 wt% | Stable | 100 | 156/160 |
(1) The as-cast Mg89RE11 (RE = Pr, Nd, Sm) alloy contains a major phase RE5Mg41 (RE = Pr, Nd, Sm) as well as two kinds of secondary phase REMg3 (RE = Pr, Nd, Sm) or REMg12 (RE = Pr, Nd). After hydrogen absorption, there will form a major phase MgH2 and a secondary phase PrH2 and Pr8H18.96 for RE = Pr, Nd2H5 for RE = Nd, Sm3H7 for RE = Sm. After hydrogen desorption, there will exist the major phase Mg and a secondary phase PrH2 for RE = Pr, Nd2H5 for RE = Nd, Sm3H7 for RE = Nd.
(2) The RE hydrides (PrH2, Nd2H5 and Sm3H7) are equably distributed in the MgH2 nanocrystalline phase and possess characteristics of good thermal stability. These RE hydrides (<100 nm) served as catalysts increase the hydrogen absorption and desorption rates. In these three kinds of hydrogen storage alloys, the Mg89Sm11 alloy shows the lowest apparent activation energy both in the absorption and desorption and the fastest hydrogen absorption and desorption rates.
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