Low Temperature Chemical Synthesis of Intermetallic TiFe Nanoparticles for Hydrogen Absorption

Low Temperature Chemical Synthesis of Intermetallic TiFe Nanoparticles for Hydrogen Absorption | Research Square window.SnipcartSettings = { analytics: { enabled: false } }; (function() { var accessVector = localStorage.getItem('access_vector') || ''; window.dataLayer = window.dataLayer || []; if (accessVector) { window.dataLayer.push({ user: { profile: { profileInfo: { snid: accessVector } } } }); } })(); (function(w,d,s,l,i){w[l]=w[l]||[];w[l].push({'gtm.start':new Date().getTime(),event:'gtm.js'});var f=d.getElementsByTagName(s)[0],j=d.createElement(s),dl=l!='dataLayer'?'&l='+l:'';j.async=true;j.src='https://www.googletagmanager.com/gtm.js?id='+i+dl;f.parentNode.insertBefore(j,f);})(window,document,'script','dataLayer','GTM-K279D39R'); Browse Preprints In Review Journals COVID-19 Preprints AJE Video Bytes Research Tools Research Promotion AJE Professional Editing AJE Rubriq About Preprint Platform In Review Editorial Policies Our Team Advisory Board Help Center Sign In Submit a Preprint Cite Share Download PDF Research Article Low Temperature Chemical Synthesis of Intermetallic TiFe Nanoparticles for Hydrogen Absorption Yasukazu Kobayashi, Shohei Yamaoka, Shunta Yamaguchi, Nobuko Hanada, and 2 more This is a preprint; it has not been peer reviewed by a journal. https://doi.org/ 10.21203/rs.3.rs-121222/v1 This work is licensed under a CC BY 4.0 License Status: Posted Version 1 posted You are reading this latest preprint version Abstract Nanosizing of TiFe hydrogen storage alloy is conducted to facilitate its activation. Here, pure intermetallic TiFe nanoparticles (45 nm) were prepared using chemical reduction of oxide precursors at 600 °C, which is the lowest temperature ever used in chemical synthesis. This was achieved using a strong reducing agent (CaH 2 ) in a molten LiCl. When used for hydrogen absorption, the obtained nanoparticles surprisingly exhibited almost no hydrogen absorption. The results demonstrated that TiFe nanoparticles are more difficult to activate than the bulk powder because the oxidized surface layers of the nanoparticles become stabilized, which prevents the morphological change necessary for their activation. Chemical Engineering Physical Chemistry TiFe CaH2 Chemical Hydrogen Figures Figure 1 Figure 1 Figure 2 Figure 2 Figure 3 Figure 3 Figure 4 Figure 4 Figure 5 Figure 5 Introduction Intermetallic TiFe is an attractive hydrogen-storage material because of its low cost, non-toxicity, and highly reversible hydrogen absorbing/desorbing capacity (~ 1.9 wt%) 1,2 . Reilly and Wiswall reported an excellent hydrogen storage performance of intermetallic hydride forms of TiFeH and TiFeH 2 3 . However, the difficulty of TiFe activation is restricting its large-scale application. The treatment is typically conducted under harsh conditions (~ 400 °C and hydrogen pressure ~ 65 atm) because of the passive Ti oxide layer formed on the surface 4 . To improve the TiFe activation kinetics, several approaches, e.g., partial substitution of Ti and Fe by an effective third element and nanostructuring of TiFe powder, were reported. In nanosizing, the hydrogen diffusion into TiFe particles is facilitated by decreasing their size, which allows easy activation under mild conditions 5–8 . Owing to their high scalability and ease of operation, physical methods, such as mechanical alloying and ball milling, are the most common methods to synthesize nanocrystalline TiFe using Ti and Fe pure metals as starting materials 9,10 . Some researchers have investigated using chemical approaches to prepare TiFe nanoparticles from metal salt precursors 11–14 . An electrochemical synthesis, which is conducted under relatively mild conditions, was investigated. This method allows the direct preparation of nanostructured TiFe from oxide precursors, such as titanium ore (ilmenite), TiO 2 , and Fe 2 O 3 , by passing an electrical current in molten salts. Hua et al. conducted the synthesis at 700 °C by using mixed molten salts (CaCl 2 –NaCl) instead of pure CaCl 2 15–18 , which successfully generated fine and homogeneous microstructures of pure TiFe with a particle size of 2–8 µm. However, at 600 °C, the titanium oxide reduction was incomplete, causing impurities, such as Fe 2 Ti and CaTiO 3 , to form. Thus, chemical synthesis of TiFe nanoparticles under mild conditions is still a highly challenging subject. Here, intermetallic TiFe nanoparticles were prepared by a chemical method using inexpensive Fe(NO 3 ) 2 and TiO 2 as precursors in molten LiCl–CaH 2 mixture. The proposed method does not require electricity. The reduction was achieved at 600 °C, which is lower than all temperatures used in previous chemical methods, allowing for a simple experimental setup. This peocess was achieved using calcium hydride as a reducing agent in molten LiCl, where highly oxygen-/vapor-free conditions were maintained. These conditions promoted the reduction of hard-reducible oxides 19–24 . The hydrogen absorption performance of the prepared TiFe nanoparticles was then evaluated. Experimental Preparation of the intermetallic TiFe nanoparticles The intermetallic TiFe nanoparticles were chemically prepared by direct reduction of Ti and Fe oxide precursors. The reduction was conducted in a molten LiCl using H 2 flow with CaH 2 as the reducing agent 19–24 . First, Fe(NO 3 ) 2 .6H 2 O was dissolved in distilled water. The solution was then mixed, and TiO 2 nanoparticles (Degussa P25 obtained from the Catalysis Society of Japan as JRC-TIO-4(2)) were suspended in the solution at a molar ratio of Fe/Ti = 1/1. The suspension was stirred and heated overnight at 110 °C until dry. The dried powder was then calcined at 500 °C for 2 h under air atmosphere to obtain Fe oxide-covered TiO 2 precursor denoted TiFe(Pre). Next, the precursor was mixed with CaH 2 and LiCl in a mortar in a weight ratio of precursor/CaH 2 /LiCl = 0.2/0.8/0.4. The mixed powder was then loaded in a stainless steel reactor connected to an H 2 gas flow system and heated at 600 °C for 2 h under the gas flow. Finally, the treated precursor was crushed in a mortar and rinsed with NH 4 Cl aqueous solution (0.1 M) and then distilled water to obtain the final product denoted TiFe(Nano), which was a relatively shiny fine black powder ( Figure S1 ). For comparison, TiFe bulk powder, i.e., TiFe(Bulk), was synthesized by conventional arc melting of pure Ti and Fe (NEV-AD 03, Nisshin Giken Co.) under an argon atmosphere. The obtained ingot was crushed and sieved to obtain a powder with a diameter of 300 µm to 2 mm in air before the characterization and measurements of hydrogen absorption and desorption. Figures S2–S4 show that the bulk powder exhibited a good crystal structure of intermetallic TiFe phase and a homogeneous morphology with a stoichiometric molar ratio of Ti/Fe. It had a relatively large oxygen content, suggesting that the surface consisted of an oxide. Hydrogen Absorption Experiments The hydrogen absorption and desorption properties of TiFe(Bulk) and TiFe(Nano) were measured using a Sieverts-type apparatus constructed by our group. Each sample (200–250 mg) was loaded into a stainless-steel vessel. In the activation process, the sample was heated to 400 °C under vacuum by a rotary pump for 30–60 min. Next, hydrogen was introduced at 0.7 MPa and maintained for 30 min and then vacuumed again for 30 min. After cooling the sample to room temperature, hydrogen was introduced again at 6.5 MPa and maintained for 90–120 min. The activation process was repeated for 3 cycles. After the activation, the hydrogen desorption and absorption were repeated at 30 °C. The initial hydrogen pressure during desorption from TiFe(Bulk) and TiFe(Nano) was 0.14 and 0.26 MPa, respectively, and that of hydrogen absorption was 1.70 MPa for both samples. In the 3-cycle activation series and the following 5-cycle one, hydrogen desorption and absorption were repeated 3 times. In the first activation series of TiFe(Bulk), hydrogen desorption and absorption were repeated for only 2 cycles. Characterization The crystal structure was examined by XRD (SmartLab (3 kW), Rigaku) with CuKα radiation at 40 kV and 45 mA and XRD (Ultima III, Rigaku) with CuKα radiation at 40 kV and 40 mA. The porosity was investigated using N 2 adsorption/desorption at − 196 °C (BELLSORP mini-II, Microtrac-BEL). The sample was pretreated at 200 °C for 30 min under vacuum before the measurement. The pore size distribution was analyzed from the measured isotherms using the BJH method. The morphology was observed by SEM (JSM-7800F, JEOL Ltd.) with EDS for elemental analysis of TiFe(Nano). Some samples were observed by SEM device (Hitachi high-technologies S-4800) equipped with an energy dispersive X-ray spectroscopy (EDS, AMETEK, Genesis-APEX2) for elemental analysis. The electronic states of Ti and Fe species were examined by XPS (JEOL JPS-9010TR operating with MgKα radiation). The C 1 s peak (284.6 eV) was used to correct the binding energies. An Ar + etching ion gun (JEOL XP-HSIG, 600 V, 12 mA, 60 s) was used to remove the surface oxide layer of the sample. Results And Discussion Figure 1 a shows a synthesis process of TiFe nanoparticles. The X-ray diffraction (XRD) spectroscopy peaks observed for commercial TiO 2 (P25) nanoparticles (the Ti source) were assigned to major anatase TiO 2 and minor rutile TiO 2 ( Figure S5a ). The crystallite sizes calculated from the Scherrer equation were 22.2 and 36.0 nm, respectively (Table 1 ). The peaks of TiFe(Pre) powder were attributed to Fe 9 TiO 15 , and no peaks of TiO 2 or any other Fe oxide were observed ( Figure S5b ). Fe(NO 3 ) 2 mainly reacted with the TiO 2 surface at 500 °C to form Fe 9 TiO 15 in the calcination process, and the core–shell-structured oxide precursor nanoparticles were formed (unreacted TiO 2 and reacted Fe 9 TiO 15 were the core and shell, respectively, Fig. 1 a). Next, the precursor was reduced using CaH 2 at 600 °C in molten LiCl. The final product was obtained after rigorous rinsing by NH 4 Cl solution. No oxide peaks were observed in the XRD spectra of the final product. The XRD peaks of TiFe(Nano) mostly corresponded to intermetallic TiFe (Fig. 1 b). The peaks assigned to TiFe 39 or/and TiFe 2 were also observed around 45° but with negligible intensities compared to those of TiFe. Thus, the oxide precursors of TiO 2 and Fe 9 TiO 15 were reduced mainly to intermetallic TiFe in molten LiCl–CaH 2 at 600 °C. The crystallite size of the TiFe was calculated to be 46.2 nm, which is much larger than those of the oxides in the precursor. Therefore, the reduced metals could be sintered to grow into large intermetallic nanoparticles. Figures S6 and S7 show N 2 absorption/desorption isotherms and the corresponding pore size distributions of TiFe(Pre) and TiFe(Nano), respectively. The Brunauer-Emmett-Teller (BET) surface areas are summarized in Table 1 . Negligible hysteresis of the isotherms and very small pore volume were observed. Hence, almost non-porous nanoparticles were obtained. Assuming that the TiFe(Nano) powder consisted of non-porous spheres, the average particle size was estimated based on the surface area to be 45.2 nm (Table 1 ), which is similar to the crystallite size (46.2 nm) estimated using the Scherrer equation. The scanning electron microscopy (SEM, Figs. 2a and S8 ) and transmission electron microscopy (TEM, Figure S10 ) images show several nanosized particles with an average size close to those estimated from the BET surface area and XRD measurement (approximately 45 nm). The Ti/Fe molar ratios obtained by SEM-energy dispersive X-ray spectroscopy (SEM-EDS, Figure S9 ) and TEM-EDS ( Figure S11 ) were similar to the stoichiometric ratio (1) of intermetallic TiFe. Calcium was not detected during the EDS analysis ( Figure S9 , S11 ), indicating the efficient washing of calcium species by post-rinsing treatments. Table 1 BET surface area (SA) and the particle size calculated from nitrogen adsorption and XRD measurement. Sample SA [m 2 /g] Particle size [nm] N 2 ads 1) XRD 2) TiO 2 (P25) 50 3) 23.9 22.2 (anatase), 36.0 (rutile) TiFe(Pre) 39.1 - 21.5 (anatase), 33.4 (rutile), 21.6 (Fe 9 TiO 15 ) Fresh TiFe(Nano) 20.0 45.2 46.2 (TiFe) Used TiFe(Nano) 12.1 - 43.9 (TiFe), 10.3 (Fe) 1) Assumption: samples consisted of non-porous spheres with TiO 2 and TiFe densities of 5.01 and 6.64 g/cm 3 , respectively. 2) Calculated using the Scherrer equation with peaks observed at 25.3°, 27.4°, 33.1°, and 43.0° for anatase, rutile, Fe 9 TiO 15 , and TiFe, respectively. 3) Obtained from ref. 25 . The surface states of fresh TiFe(Bulk) and TiFe(Nano) were investigated using X-ray photoelectron spectroscopy (XPS, Fig. 3 ). The obtained spectra were calibrated with C 1 s at 284.6 eV ( Figure S13 ) and the peak identification was based on a previous report 26 . Before etching, peaks of both samples were assigned to oxidation states of Ti and Fe, suggesting that the surfaces of fresh TiFe(Bulk) and TiFe(Nano) were oxidized. After etching, peaks of metallic Ti (Ti 0 ) and Fe(Fe 0 ) were observed for both samples, indicating the presence of Ti–Fe metals/alloys below the oxide layers, which is consistent with the elemental mapping results using TEM-EDS (Fig. 2b, Figure S11 and S12 ). Thus, highly crystalline intermetallic TiFe nanoparticles covered with surface oxide layers were successfully synthesized. This method is better than electrochemical methods that require higher reduction temperature 11–18 . Moreover, the particle size (45.2–46.2 nm) obtained here is much smaller than the micron sizes reported in previous works, which can be attributed to the inhibition of grain sintering by the low temperature. Figure S14 shows hydrogen absorption properties of TiFe(Bulk) after each activation. In the 1st and 2nd absorption cycles after the 1st activation series, similar absorption properties were obtained with the total hydrogen absorption of 0.14 wt%. After the 2nd series, this value increased to approximately 0.3 wt% and the absorption rate increased with the cycle time. After the 3rd series, absorption increased to approximately 0.67 wt% during the 5th cycle, and the rate increased with the cycle time. This indicates that hydrogen absorption increases by repeating the activation process at high temperature and hydrogen pressure because the passive surface oxide layer breaks. This surface oxide was converted into a mixture of Fe, which facilitated the dissociation of physisorbed hydrogen molecules, and TiO 2 through activation, allowing hydrogen atoms to penetrate the surface and diffuse in the bulk 27 . The increase in the hydrogen absorption rate with cycling time can be attributed to the pulverization of the particles by the volume change during the hydrogen absorption and desorption cycles because of the shortening of the hydrogen diffusion path in the bulk and the increase in the surface area 27 . Figure 4 shows a comparison between the hydrogen absorption properties of TiFe(Nano) and TiFe(Bulk) after the 5th absorption cycle conducted after each activation series. In TiFe(Bulk), the absorption increased with repeating the activation process, while that in TiFe(Nano) was only 0.06 wt% in the 5th cycle after the 1st activation series. Similar properties were obtained during the 1st to 5th cycles. Those after the 5th cycle of the 2nd and 3rd activation series were similar to that obtained after the 1st one, indicating that the activation and hydrogen sorption-cycling process did not improve the hydrogen absorption properties of TiFe(Nano). The non-activated TiFe(Nano) was compared to TiFe(Bulk) powders by characterization using XRD ( Figure S15 ) and SEM (Figs. 5 a, b and Figure S16 ). N 2 adsorption ( Figure S17 ) and TEM-EDS ( Figures S18, S19 ) were also conducted. XRD measurements showed that the used TiFe(Nano) partially decomposed to form TiFe 39 or/and Fe, but a TiFe phase remained. However, no extra phases were observed in the used TiFe(Bulk). Clear cracks were observed in the used TiFe(Bulk) (Fig. 5 a, Figure S16a ), which is often observed in activated TiFe alloys 4 , while no cracks were observed in the used TiFe(Nano) (Fig. 5 b, Figure S16b ). The morphology and particle size of the used TiFe(Nano) were similar to those of the fresh TiFe(Nano) because they were maintained through the surface oxide layers. This can be attributed to the followings: First, the breakdown of the passive oxide layer was not facilitated because its large surface oxygen ratio due to the high surface area compared to TiFe(Bulk). Second, no particle pulverization by volume change occurred during hydrogen sorption because the hardness of TiFe(Nano) is six times larger than that of TiFe(Bulk) due to the Hall-Petch contribution 28,29 ( Table S1 ). Thus, it was too difficult to fracture TiFe(Nano) that was composed of non-porous spheres. Therefore, the oxidized surface nanoparticles of alloys, such as TiFe, that exhibit surface activation difficulty, hardly absorb hydrogen by conventional activation treatments. To improve the hydrogen absorption properties of TiFe(Nano), future studies may investigate adding a third element to TiFe(Nano) nanoparticles to increase the catalytic active surface, promoting hydrogen diffusion, and decrease the fracture toughness of the alloy 4 . Conclusions Intermetallic TiFe nanoparticles were chemically prepared at 600 °C in a molten LiCl–CaH 2 mixture. The prepared nanopowder exhibited the highly crystalline structure of intermetallic TiFe and a high BET surface area of 20.0 m 2 /g. The BET, XRD, and SEM results confirmed the formation of nanosized particles of 45.2–46.2 nm. Compared to previous electrochemical methods, the proposed method allowed a lower temperature reduction, resulting in smaller nanoparticles. This was achieved using CaH 2 as a superior reducing agent in molten LiCl. It was also demonstrated that TiFe nanoparticles were difficult to activate compared to the bulk powder, since the oxidized surface layers of the nanoparticles were stabilized, which prevents the morphological change necessary for the activation. Declarations Acknowledgements We acknowledge the Advanced Characterization Nanotechnology Platform of the University of Tokyo and the Center for Instrumental Analysis Ibaraki University for sample characterization. The authors thank Prof. Noda at Waseda University for his support in SEM-EDS measurement. Author contributions statement Y.K. designed the study, performed the experiments for TiFe synthesis. S.Y., S.Y. and N.H. conducted the hydrogen absorption experiments. 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Also discoverable on Platform About Our Team In Review Editorial Policies Advisory Board Help Center Resources Author Services Accessibility API Access RSS feed Manage Cookie Preferences © Research Square 2026 | ISSN 2693-5015 (online) Privacy Policy Terms of Service Do Not Sell My Personal Information {"props":{"pageProps":{"initialData":{"identity":"rs-121222","acceptedTermsAndConditions":true,"allowDirectSubmit":true,"archivedVersions":[],"articleType":"Research Article","associatedPublications":[],"authors":[{"id":5869547,"identity":"76afdf3a-dcf1-4bf3-8f03-8c9f51ed0a55","order_by":0,"name":"Yasukazu 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TiFe(Nano).","description":"","filename":"Fig1.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/b485cda5627443634d7ce459.JPG"},{"id":4160183,"identity":"11f5dc0d-7fc4-4c0f-971b-7af4449eca63","added_by":"auto","created_at":"2020-12-10 15:53:25","extension":"jpg","order_by":1,"title":"Figure 1","display":"","copyAsset":false,"role":"figure","size":66334,"visible":true,"origin":"","legend":"(a) TiFe nanoparticle synthesis and (b) XRD patterns of TiFe(Nano).","description":"","filename":"Fig1.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/5fcbf88c626d022990f8bf1e.JPG"},{"id":4160191,"identity":"dd644364-a50a-4b80-b1a0-f2ca4b223349","added_by":"auto","created_at":"2020-12-10 15:53:31","extension":"jpg","order_by":2,"title":"Figure 2","display":"","copyAsset":false,"role":"figure","size":71602,"visible":true,"origin":"","legend":"(a) SEM images of fresh TiFe(Nano) and (b) elemental mapping by TEM-EDS (Ti: blue, Fe: purple, O: red).","description":"","filename":"Fig2.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/32cc242d8333a7441af76948.JPG"},{"id":4160184,"identity":"062b7168-ab7e-4197-9c98-4269d48e1adc","added_by":"auto","created_at":"2020-12-10 15:53:25","extension":"jpg","order_by":2,"title":"Figure 2","display":"","copyAsset":false,"role":"figure","size":71602,"visible":true,"origin":"","legend":"(a) SEM images of fresh TiFe(Nano) and (b) elemental mapping by TEM-EDS (Ti: blue, Fe: purple, O: red).","description":"","filename":"Fig2.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/e37b654374dc26b70ed22b01.JPG"},{"id":4160193,"identity":"b12f4bb7-7d24-4905-b839-74252fb39588","added_by":"auto","created_at":"2020-12-10 15:53:32","extension":"jpg","order_by":3,"title":"Figure 3","display":"","copyAsset":false,"role":"figure","size":160156,"visible":true,"origin":"","legend":"XPS spectra of (a) Ti 2p and (b) Fe 2p for fresh TiFe(Nano) and TiFe(Bulk).","description":"","filename":"Fig3.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/55d6f9bb9567d62eaf39244e.JPG"},{"id":4160186,"identity":"4c441b5a-7d5c-4670-b7ed-155bca57afa4","added_by":"auto","created_at":"2020-12-10 15:53:26","extension":"jpg","order_by":3,"title":"Figure 3","display":"","copyAsset":false,"role":"figure","size":160156,"visible":true,"origin":"","legend":"XPS spectra of (a) Ti 2p and (b) Fe 2p for fresh TiFe(Nano) and TiFe(Bulk).","description":"","filename":"Fig3.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/c6f2592a0ba3d2d38890084d.JPG"},{"id":4160194,"identity":"6709aab0-5034-4705-851f-9649d3d2fe99","added_by":"auto","created_at":"2020-12-10 15:53:32","extension":"jpg","order_by":4,"title":"Figure 4","display":"","copyAsset":false,"role":"figure","size":69995,"visible":true,"origin":"","legend":"Hydrogen absorption properties of TiFe(Bulk) and TiFe(Nano) after the 2nd and 5th absorption cycles after activation. ","description":"","filename":"Fig4.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/8ae288882ee64e52157412b9.JPG"},{"id":4160187,"identity":"00c9f866-0c71-4d59-bed7-20a23677350d","added_by":"auto","created_at":"2020-12-10 15:53:26","extension":"jpg","order_by":4,"title":"Figure 4","display":"","copyAsset":false,"role":"figure","size":69995,"visible":true,"origin":"","legend":"Hydrogen absorption properties of TiFe(Bulk) and TiFe(Nano) after the 2nd and 5th absorption cycles after activation. ","description":"","filename":"Fig4.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/3cb43aa1343036aef8fa3ca3.JPG"},{"id":4160195,"identity":"004dbe64-6d27-4c22-b9a0-20e1d87ca421","added_by":"auto","created_at":"2020-12-10 15:53:32","extension":"jpg","order_by":5,"title":"Figure 5","display":"","copyAsset":false,"role":"figure","size":90660,"visible":true,"origin":"","legend":"SEM images of (a) used TiFe(Bulk) and (b) used TiFe(Nano).","description":"","filename":"Fig5.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/04ffd4a94b412c8f54fe8142.JPG"},{"id":4160188,"identity":"892020f3-d876-4a6a-b608-7ac698d5cc1a","added_by":"auto","created_at":"2020-12-10 15:53:26","extension":"jpg","order_by":5,"title":"Figure 5","display":"","copyAsset":false,"role":"figure","size":90660,"visible":true,"origin":"","legend":"SEM images of (a) used TiFe(Bulk) and (b) used TiFe(Nano).","description":"","filename":"Fig5.JPG","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/25848da73ff6e6bb8a32d421.JPG"},{"id":13631911,"identity":"1c51ed17-aeec-4127-aa71-1b4f7bd42e41","added_by":"auto","created_at":"2021-09-17 08:18:50","extension":"pdf","order_by":0,"title":"","display":"","copyAsset":false,"role":"manuscript-pdf","size":953832,"visible":true,"origin":"","legend":"","description":"","filename":"manuscript.pdf","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/d8b58853-a942-463d-94a1-791ccce39f48.pdf"},{"id":4160192,"identity":"8d2afdb7-e1d4-4c13-b8da-55c85c9fab17","added_by":"auto","created_at":"2020-12-10 15:53:32","extension":"docx","order_by":1,"title":"","display":"","copyAsset":false,"role":"supplement","size":13700450,"visible":true,"origin":"","legend":"","description":"","filename":"11262020SuppInfSciRep.docx","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/99bd38fc93845c8f01ea7715.docx"},{"id":4160185,"identity":"85a1a661-86e4-4292-87ca-4b2c8569d204","added_by":"auto","created_at":"2020-12-10 15:53:25","extension":"docx","order_by":1,"title":"","display":"","copyAsset":false,"role":"supplement","size":13700450,"visible":true,"origin":"","legend":"","description":"","filename":"11262020SuppInfSciRep.docx","url":"https://assets-eu.researchsquare.com/files/rs-121222/v1/e90c100151172526866f4d48.docx"}],"financialInterests":"","formattedTitle":"Low Temperature Chemical Synthesis of Intermetallic TiFe Nanoparticles for Hydrogen Absorption","fulltext":[{"header":"Introduction","content":" \u003cp\u003eIntermetallic TiFe is an attractive hydrogen-storage material because of its low cost, non-toxicity, and highly reversible hydrogen absorbing/desorbing capacity (~\u0026thinsp;1.9\u0026nbsp;wt%)\u003csup\u003e\u003cb\u003e1,2\u003c/b\u003e\u003c/sup\u003e. Reilly and Wiswall reported an excellent hydrogen storage performance of intermetallic hydride forms of TiFeH and TiFeH\u003csub\u003e2\u003c/sub\u003e\u003csup\u003e\u003cb\u003e3\u003c/b\u003e\u003c/sup\u003e. However, the difficulty of TiFe activation is restricting its large-scale application. The treatment is typically conducted under harsh conditions (~\u0026thinsp;400\u0026nbsp;\u0026deg;C and hydrogen pressure\u0026thinsp;~\u0026thinsp;65\u0026nbsp;atm) because of the passive Ti oxide layer formed on the surface\u003csup\u003e\u003cb\u003e4\u003c/b\u003e\u003c/sup\u003e. To improve the TiFe activation kinetics, several approaches, e.g., partial substitution of Ti and Fe by an effective third element and nanostructuring of TiFe powder, were reported. In nanosizing, the hydrogen diffusion into TiFe particles is facilitated by decreasing their size, which allows easy activation under mild conditions\u003csup\u003e\u003cb\u003e5\u0026ndash;8\u003c/b\u003e\u003c/sup\u003e. Owing to their high scalability and ease of operation, physical methods, such as mechanical alloying and ball milling, are the most common methods to synthesize nanocrystalline TiFe using Ti and Fe pure metals as starting materials\u003csup\u003e\u003cb\u003e9,10\u003c/b\u003e\u003c/sup\u003e. Some researchers have investigated using chemical approaches to prepare TiFe nanoparticles from metal salt precursors\u003csup\u003e\u003cb\u003e11\u0026ndash;14\u003c/b\u003e\u003c/sup\u003e. An electrochemical synthesis, which is conducted under relatively mild conditions, was investigated. This method allows the direct preparation of nanostructured TiFe from oxide precursors, such as titanium ore (ilmenite), TiO\u003csub\u003e2\u003c/sub\u003e, and Fe\u003csub\u003e2\u003c/sub\u003eO\u003csub\u003e3\u003c/sub\u003e, by passing an electrical current in molten salts. Hua et al. conducted the synthesis at 700\u0026nbsp;\u0026deg;C by using mixed molten salts (CaCl\u003csub\u003e2\u003c/sub\u003e\u0026ndash;NaCl) instead of pure CaCl\u003csub\u003e2\u003c/sub\u003e\u003csup\u003e\u003cb\u003e15\u0026ndash;18\u003c/b\u003e\u003c/sup\u003e, which successfully generated fine and homogeneous microstructures of pure TiFe with a particle size of 2\u0026ndash;8\u0026nbsp;\u0026micro;m. However, at 600\u0026nbsp;\u0026deg;C, the titanium oxide reduction was incomplete, causing impurities, such as Fe\u003csub\u003e2\u003c/sub\u003eTi and CaTiO\u003csub\u003e3\u003c/sub\u003e, to form. Thus, chemical synthesis of TiFe nanoparticles under mild conditions is still a highly challenging subject.\u003c/p\u003e \u003cp\u003eHere, intermetallic TiFe nanoparticles were prepared by a chemical method using inexpensive Fe(NO\u003csub\u003e3\u003c/sub\u003e)\u003csub\u003e2\u003c/sub\u003e and TiO\u003csub\u003e2\u003c/sub\u003e as precursors in molten LiCl\u0026ndash;CaH\u003csub\u003e2\u003c/sub\u003e mixture. The proposed method does not require electricity. The reduction was achieved at 600\u0026nbsp;\u0026deg;C, which is lower than all temperatures used in previous chemical methods, allowing for a simple experimental setup. This peocess was achieved using calcium hydride as a reducing agent in molten LiCl, where highly oxygen-/vapor-free conditions were maintained. These conditions promoted the reduction of hard-reducible oxides\u003csup\u003e\u003cb\u003e19\u0026ndash;24\u003c/b\u003e\u003c/sup\u003e. The hydrogen absorption performance of the prepared TiFe nanoparticles was then evaluated.\u003c/p\u003e "},{"header":"Experimental","content":" \u003cdiv id=\"Sec3\" class=\"Section2\"\u003e \u003ch2\u003ePreparation of the intermetallic TiFe nanoparticles\u003c/h2\u003e \u003cp\u003eThe intermetallic TiFe nanoparticles were chemically prepared by direct reduction of Ti and Fe oxide precursors. The reduction was conducted in a molten LiCl using H\u003csub\u003e2\u003c/sub\u003e flow with CaH\u003csub\u003e2\u003c/sub\u003e as the reducing agent\u003csup\u003e\u003cb\u003e19\u0026ndash;24\u003c/b\u003e\u003c/sup\u003e. First, Fe(NO\u003csub\u003e3\u003c/sub\u003e)\u003csub\u003e2\u003c/sub\u003e.6H\u003csub\u003e2\u003c/sub\u003eO was dissolved in distilled water. The solution was then mixed, and TiO\u003csub\u003e2\u003c/sub\u003e nanoparticles (Degussa P25 obtained from the Catalysis Society of Japan as JRC-TIO-4(2)) were suspended in the solution at a molar ratio of Fe/Ti\u0026thinsp;=\u0026thinsp;1/1. The suspension was stirred and heated overnight at 110\u0026nbsp;\u0026deg;C until dry. The dried powder was then calcined at 500\u0026nbsp;\u0026deg;C for 2\u0026nbsp;h under air atmosphere to obtain Fe oxide-covered TiO\u003csub\u003e2\u003c/sub\u003e precursor denoted TiFe(Pre). Next, the precursor was mixed with CaH\u003csub\u003e2\u003c/sub\u003e and LiCl in a mortar in a weight ratio of precursor/CaH\u003csub\u003e2\u003c/sub\u003e/LiCl\u0026thinsp;=\u0026thinsp;0.2/0.8/0.4. The mixed powder was then loaded in a stainless steel reactor connected to an H\u003csub\u003e2\u003c/sub\u003e gas flow system and heated at 600\u0026nbsp;\u0026deg;C for 2\u0026nbsp;h under the gas flow. Finally, the treated precursor was crushed in a mortar and rinsed with NH\u003csub\u003e4\u003c/sub\u003eCl aqueous solution (0.1\u0026nbsp;M) and then distilled water to obtain the final product denoted TiFe(Nano), which was a relatively shiny fine black powder (\u003cb\u003eFigure S1\u003c/b\u003e). For comparison, TiFe bulk powder, i.e., TiFe(Bulk), was synthesized by conventional arc melting of pure Ti and Fe (NEV-AD 03, Nisshin Giken Co.) under an argon atmosphere. The obtained ingot was crushed and sieved to obtain a powder with a diameter of 300\u0026nbsp;\u0026micro;m to 2\u0026nbsp;mm in air before the characterization and measurements of hydrogen absorption and desorption. \u003cb\u003eFigures S2\u0026ndash;S4\u003c/b\u003e show that the bulk powder exhibited a good crystal structure of intermetallic TiFe phase and a homogeneous morphology with a stoichiometric molar ratio of Ti/Fe. It had a relatively large oxygen content, suggesting that the surface consisted of an oxide.\u003c/p\u003e \u003c/div\u003e \n\u003ch2\u003eHydrogen Absorption Experiments\u003c/h2\u003e\n \u003cp\u003eThe hydrogen absorption and desorption properties of TiFe(Bulk) and TiFe(Nano) were measured using a Sieverts-type apparatus constructed by our group. Each sample (200\u0026ndash;250\u0026nbsp;mg) was loaded into a stainless-steel vessel. In the activation process, the sample was heated to 400\u0026nbsp;\u0026deg;C under vacuum by a rotary pump for 30\u0026ndash;60\u0026nbsp;min. Next, hydrogen was introduced at 0.7\u0026nbsp;MPa and maintained for 30\u0026nbsp;min and then vacuumed again for 30\u0026nbsp;min. After cooling the sample to room temperature, hydrogen was introduced again at 6.5\u0026nbsp;MPa and maintained for 90\u0026ndash;120\u0026nbsp;min. The activation process was repeated for 3 cycles. After the activation, the hydrogen desorption and absorption were repeated at 30\u0026nbsp;\u0026deg;C. The initial hydrogen pressure during desorption from TiFe(Bulk) and TiFe(Nano) was 0.14 and 0.26\u0026nbsp;MPa, respectively, and that of hydrogen absorption was 1.70\u0026nbsp;MPa for both samples. In the 3-cycle activation series and the following 5-cycle one, hydrogen desorption and absorption were repeated 3 times. In the first activation series of TiFe(Bulk), hydrogen desorption and absorption were repeated for only 2 cycles.\u003c/p\u003e \n\u003ch2\u003eCharacterization\u003c/h2\u003e\n \u003cp\u003eThe crystal structure was examined by XRD (SmartLab (3\u0026nbsp;kW), Rigaku) with CuKα radiation at 40\u0026nbsp;kV and 45\u0026nbsp;mA and XRD (Ultima III, Rigaku) with CuKα radiation at 40\u0026nbsp;kV and 40\u0026nbsp;mA. The porosity was investigated using N\u003csub\u003e2\u003c/sub\u003e adsorption/desorption at \u0026minus;\u0026thinsp;196\u0026nbsp;\u0026deg;C (BELLSORP mini-II, Microtrac-BEL). The sample was pretreated at 200\u0026nbsp;\u0026deg;C for 30\u0026nbsp;min under vacuum before the measurement. The pore size distribution was analyzed from the measured isotherms using the BJH method. The morphology was observed by SEM (JSM-7800F, JEOL Ltd.) with EDS for elemental analysis of TiFe(Nano). Some samples were observed by SEM device (Hitachi high-technologies S-4800) equipped with an energy dispersive X-ray spectroscopy (EDS, AMETEK, Genesis-APEX2) for elemental analysis. The electronic states of Ti and Fe species were examined by XPS (JEOL JPS-9010TR operating with MgKα radiation). The C 1\u0026nbsp;s peak (284.6\u0026nbsp;eV) was used to correct the binding energies. An Ar\u003csup\u003e+\u003c/sup\u003e etching ion gun (JEOL XP-HSIG, 600\u0026nbsp;V, 12\u0026nbsp;mA, 60\u0026nbsp;s) was used to remove the surface oxide layer of the sample.\u003c/p\u003e "},{"header":"Results And Discussion","content":"\u003cp\u003eFigure \u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003ea shows a synthesis process of TiFe nanoparticles. The X-ray diffraction (XRD) spectroscopy peaks observed for commercial TiO\u003csub\u003e2\u003c/sub\u003e (P25) nanoparticles (the Ti source) were assigned to major anatase TiO\u003csub\u003e2\u003c/sub\u003e and minor rutile TiO\u003csub\u003e2\u003c/sub\u003e (\u003cstrong\u003eFigure S5a\u003c/strong\u003e). The crystallite sizes calculated from the Scherrer equation were 22.2 and 36.0\u0026nbsp;nm, respectively (Table\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003e). The peaks of TiFe(Pre) powder were attributed to Fe\u003csub\u003e9\u003c/sub\u003eTiO\u003csub\u003e15\u003c/sub\u003e, and no peaks of TiO\u003csub\u003e2\u003c/sub\u003e or any other Fe oxide were observed (\u003cstrong\u003eFigure S5b\u003c/strong\u003e). Fe(NO\u003csub\u003e3\u003c/sub\u003e)\u003csub\u003e2\u003c/sub\u003e mainly reacted with the TiO\u003csub\u003e2\u003c/sub\u003e surface at 500\u0026nbsp;\u0026deg;C to form Fe\u003csub\u003e9\u003c/sub\u003eTiO\u003csub\u003e15\u003c/sub\u003e in the calcination process, and the core\u0026ndash;shell-structured oxide precursor nanoparticles were formed (unreacted TiO\u003csub\u003e2\u003c/sub\u003e and reacted Fe\u003csub\u003e9\u003c/sub\u003eTiO\u003csub\u003e15\u003c/sub\u003e were the core and shell, respectively, Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003ea). Next, the precursor was reduced using CaH\u003csub\u003e2\u003c/sub\u003e at 600\u0026nbsp;\u0026deg;C in molten LiCl. The final product was obtained after rigorous rinsing by NH\u003csub\u003e4\u003c/sub\u003eCl solution. No oxide peaks were observed in the XRD spectra of the final product. The XRD peaks of TiFe(Nano) mostly corresponded to intermetallic TiFe (Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003eb). The peaks assigned to TiFe\u003csub\u003e39\u003c/sub\u003e or/and TiFe\u003csub\u003e2\u003c/sub\u003e were also observed around 45\u0026deg; but with negligible intensities compared to those of TiFe. Thus, the oxide precursors of TiO\u003csub\u003e2\u003c/sub\u003e and Fe\u003csub\u003e9\u003c/sub\u003eTiO\u003csub\u003e15\u003c/sub\u003e were reduced mainly to intermetallic TiFe in molten LiCl\u0026ndash;CaH\u003csub\u003e2\u003c/sub\u003e at 600\u0026nbsp;\u0026deg;C. The crystallite size of the TiFe was calculated to be 46.2\u0026nbsp;nm, which is much larger than those of the oxides in the precursor. Therefore, the reduced metals could be sintered to grow into large intermetallic nanoparticles. \u003cstrong\u003eFigures S6\u003c/strong\u003e and \u003cstrong\u003eS7\u003c/strong\u003e show N\u003csub\u003e2\u003c/sub\u003e absorption/desorption isotherms and the corresponding pore size distributions of TiFe(Pre) and TiFe(Nano), respectively. The Brunauer-Emmett-Teller (BET) surface areas are summarized in Table\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003e. Negligible hysteresis of the isotherms and very small pore volume were observed. Hence, almost non-porous nanoparticles were obtained. Assuming that the TiFe(Nano) powder consisted of non-porous spheres, the average particle size was estimated based on the surface area to be 45.2\u0026nbsp;nm (Table\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003e), which is similar to the crystallite size (46.2\u0026nbsp;nm) estimated using the Scherrer equation. The scanning electron microscopy (SEM, \u003cstrong\u003eFigs.\u0026nbsp;2a\u003c/strong\u003e and \u003cstrong\u003eS8\u003c/strong\u003e) and transmission electron microscopy (TEM, \u003cstrong\u003eFigure S10\u003c/strong\u003e) images show several nanosized particles with an average size close to those estimated from the BET surface area and XRD measurement (approximately 45\u0026nbsp;nm). The Ti/Fe molar ratios obtained by SEM-energy dispersive X-ray spectroscopy (SEM-EDS, \u003cstrong\u003eFigure S9\u003c/strong\u003e) and TEM-EDS (\u003cstrong\u003eFigure S11\u003c/strong\u003e) were similar to the stoichiometric ratio (1) of intermetallic TiFe. Calcium was not detected during the EDS analysis (\u003cstrong\u003eFigure S9\u003c/strong\u003e, \u003cstrong\u003eS11\u003c/strong\u003e), indicating the efficient washing of calcium species by post-rinsing treatments.\u003c/p\u003e\n\u003ctable id=\"Tab1\" border=\"1\"\u003e\u003ccaption\u003e\n\u003cdiv class=\"CaptionNumber\"\u003eTable 1\u003c/div\u003e\n\u003cdiv class=\"CaptionContent\"\u003e\n\u003cp\u003eBET surface area (SA) and the particle size calculated from nitrogen adsorption and XRD measurement.\u003c/p\u003e\n\u003c/div\u003e\n\u003c/caption\u003e\n\u003cthead\u003e\n\u003ctr\u003e\n\u003cth rowspan=\"2\" align=\"left\"\u003e\n\u003cp\u003eSample\u003c/p\u003e\n\u003c/th\u003e\n\u003cth rowspan=\"2\" align=\"left\"\u003e\n\u003cp\u003eSA [m\u003csup\u003e2\u003c/sup\u003e/g]\u003c/p\u003e\n\u003c/th\u003e\n\u003cth colspan=\"2\" align=\"left\"\u003e\n\u003cp\u003eParticle size [nm]\u003c/p\u003e\n\u003c/th\u003e\n\u003c/tr\u003e\n\u003ctr\u003e\n\u003cth align=\"left\"\u003e\n\u003cp\u003eN\u003csub\u003e2\u003c/sub\u003e ads\u003csup\u003e1)\u003c/sup\u003e\u003c/p\u003e\n\u003c/th\u003e\n\u003cth align=\"left\"\u003e\n\u003cp\u003eXRD\u003csup\u003e2)\u003c/sup\u003e\u003c/p\u003e\n\u003c/th\u003e\n\u003c/tr\u003e\n\u003c/thead\u003e\n\u003ctbody\u003e\n\u003ctr\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eTiO\u003csub\u003e2\u003c/sub\u003e (P25)\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e50\u003csup\u003e3)\u003c/sup\u003e\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e23.9\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e22.2 (anatase), 36.0 (rutile)\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003ctr\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eTiFe(Pre)\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e39.1\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e-\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e21.5 (anatase), 33.4 (rutile), 21.6 (Fe\u003csub\u003e9\u003c/sub\u003eTiO\u003csub\u003e15\u003c/sub\u003e)\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003ctr\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eFresh TiFe(Nano)\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e20.0\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e45.2\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e46.2 (TiFe)\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003ctr\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eUsed TiFe(Nano)\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e12.1\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e-\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e43.9 (TiFe), 10.3 (Fe)\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003c/tbody\u003e\n\u003ctfoot\u003e\n\u003ctr\u003e\n\u003ctd colspan=\"4\"\u003e1) Assumption: samples consisted of non-porous spheres with TiO\u003csub\u003e2\u003c/sub\u003e and TiFe densities of 5.01 and 6.64\u0026nbsp;g/cm\u003csup\u003e3\u003c/sup\u003e, respectively.\u003c/td\u003e\n\u003c/tr\u003e\n\u003c/tfoot\u003e\n\u003c/table\u003e\n\u003cp\u003e2) Calculated using the Scherrer equation with peaks observed at 25.3\u0026deg;, 27.4\u0026deg;, 33.1\u0026deg;, and 43.0\u0026deg; for anatase, rutile, Fe\u003csub\u003e9\u003c/sub\u003eTiO\u003csub\u003e15\u003c/sub\u003e, and TiFe, respectively.\u003c/p\u003e\n\u003cp\u003e3) Obtained from \u003cstrong\u003eref. 25\u003c/strong\u003e.\u003c/p\u003e\n\u003cp\u003eThe surface states of fresh TiFe(Bulk) and TiFe(Nano) were investigated using X-ray photoelectron spectroscopy (XPS, \u003cstrong\u003eFig.\u0026nbsp;3\u003c/strong\u003e). The obtained spectra were calibrated with C 1\u0026nbsp;s at 284.6\u0026nbsp;eV (\u003cstrong\u003eFigure S13\u003c/strong\u003e) and the peak identification was based on a previous report\u003csup\u003e\u003cstrong\u003e26\u003c/strong\u003e\u003c/sup\u003e. Before etching, peaks of both samples were assigned to oxidation states of Ti and Fe, suggesting that the surfaces of fresh TiFe(Bulk) and TiFe(Nano) were oxidized. After etching, peaks of metallic Ti (Ti\u003csup\u003e0\u003c/sup\u003e) and Fe(Fe\u003csup\u003e0\u003c/sup\u003e) were observed for both samples, indicating the presence of Ti\u0026ndash;Fe metals/alloys below the oxide layers, which is consistent with the elemental mapping results using TEM-EDS (Fig.\u0026nbsp;2b, \u003cstrong\u003eFigure S11 and S12\u003c/strong\u003e). Thus, highly crystalline intermetallic TiFe nanoparticles covered with surface oxide layers were successfully synthesized. This method is better than electrochemical methods that require higher reduction temperature\u003csup\u003e\u003cstrong\u003e11\u0026ndash;18\u003c/strong\u003e\u003c/sup\u003e. Moreover, the particle size (45.2\u0026ndash;46.2\u0026nbsp;nm) obtained here is much smaller than the micron sizes reported in previous works, which can be attributed to the inhibition of grain sintering by the low temperature.\u003c/p\u003e\n\u003cp\u003e\u003cstrong\u003eFigure S14\u003c/strong\u003e shows hydrogen absorption properties of TiFe(Bulk) after each activation. In the 1st and 2nd absorption cycles after the 1st activation series, similar absorption properties were obtained with the total hydrogen absorption of 0.14\u0026nbsp;wt%. After the 2nd series, this value increased to approximately 0.3\u0026nbsp;wt% and the absorption rate increased with the cycle time. After the 3rd series, absorption increased to approximately 0.67\u0026nbsp;wt% during the 5th cycle, and the rate increased with the cycle time. This indicates that hydrogen absorption increases by repeating the activation process at high temperature and hydrogen pressure because the passive surface oxide layer breaks. This surface oxide was converted into a mixture of Fe, which facilitated the dissociation of physisorbed hydrogen molecules, and TiO\u003csub\u003e2\u003c/sub\u003e through activation, allowing hydrogen atoms to penetrate the surface and diffuse in the bulk\u003csup\u003e\u003cstrong\u003e27\u003c/strong\u003e\u003c/sup\u003e. The increase in the hydrogen absorption rate with cycling time can be attributed to the pulverization of the particles by the volume change during the hydrogen absorption and desorption cycles because of the shortening of the hydrogen diffusion path in the bulk and the increase in the surface area\u003csup\u003e\u003cstrong\u003e27\u003c/strong\u003e\u003c/sup\u003e.\u003c/p\u003e\n\u003cp\u003eFigure \u003cspan class=\"InternalRef\"\u003e4\u003c/span\u003e shows a comparison between the hydrogen absorption properties of TiFe(Nano) and TiFe(Bulk) after the 5th absorption cycle conducted after each activation series. In TiFe(Bulk), the absorption increased with repeating the activation process, while that in TiFe(Nano) was only 0.06\u0026nbsp;wt% in the 5th cycle after the 1st activation series. Similar properties were obtained during the 1st to 5th cycles. Those after the 5th cycle of the 2nd and 3rd activation series were similar to that obtained after the 1st one, indicating that the activation and hydrogen sorption-cycling process did not improve the hydrogen absorption properties of TiFe(Nano).\u003c/p\u003e\n\u003cp\u003eThe non-activated TiFe(Nano) was compared to TiFe(Bulk) powders by characterization using XRD (\u003cstrong\u003eFigure S15\u003c/strong\u003e) and SEM (Figs.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e5\u003c/span\u003ea, b and \u003cstrong\u003eFigure S16\u003c/strong\u003e). N\u003csub\u003e2\u003c/sub\u003e adsorption (\u003cstrong\u003eFigure S17\u003c/strong\u003e) and TEM-EDS (\u003cstrong\u003eFigures S18, S19\u003c/strong\u003e) were also conducted. XRD measurements showed that the used TiFe(Nano) partially decomposed to form TiFe\u003csub\u003e39\u003c/sub\u003e or/and Fe, but a TiFe phase remained. However, no extra phases were observed in the used TiFe(Bulk). Clear cracks were observed in the used TiFe(Bulk) (Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e5\u003c/span\u003ea, \u003cstrong\u003eFigure S16a\u003c/strong\u003e), which is often observed in activated TiFe alloys\u003csup\u003e\u003cstrong\u003e4\u003c/strong\u003e\u003c/sup\u003e, while no cracks were observed in the used TiFe(Nano) (Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e5\u003c/span\u003eb, \u003cstrong\u003eFigure S16b\u003c/strong\u003e). The morphology and particle size of the used TiFe(Nano) were similar to those of the fresh TiFe(Nano) because they were maintained through the surface oxide layers. This can be attributed to the followings: First, the breakdown of the passive oxide layer was not facilitated because its large surface oxygen ratio due to the high surface area compared to TiFe(Bulk). Second, no particle pulverization by volume change occurred during hydrogen sorption because the hardness of TiFe(Nano) is six times larger than that of TiFe(Bulk) due to the Hall-Petch contribution\u003csup\u003e\u003cstrong\u003e28,29\u003c/strong\u003e\u003c/sup\u003e (\u003cstrong\u003eTable S1\u003c/strong\u003e). Thus, it was too difficult to fracture TiFe(Nano) that was composed of non-porous spheres. Therefore, the oxidized surface nanoparticles of alloys, such as TiFe, that exhibit surface activation difficulty, hardly absorb hydrogen by conventional activation treatments. To improve the hydrogen absorption properties of TiFe(Nano), future studies may investigate adding a third element to TiFe(Nano) nanoparticles to increase the catalytic active surface, promoting hydrogen diffusion, and decrease the fracture toughness of the alloy\u003csup\u003e\u003cstrong\u003e4\u003c/strong\u003e\u003c/sup\u003e.\u003c/p\u003e"},{"header":"Conclusions","content":" \u003cp\u003eIntermetallic TiFe nanoparticles were chemically prepared at 600\u0026nbsp;\u0026deg;C in a molten LiCl\u0026ndash;CaH\u003csub\u003e2\u003c/sub\u003e mixture. The prepared nanopowder exhibited the highly crystalline structure of intermetallic TiFe and a high BET surface area of 20.0\u0026nbsp;m\u003csup\u003e2\u003c/sup\u003e/g. The BET, XRD, and SEM results confirmed the formation of nanosized particles of 45.2\u0026ndash;46.2\u0026nbsp;nm. Compared to previous electrochemical methods, the proposed method allowed a lower temperature reduction, resulting in smaller nanoparticles. This was achieved using CaH\u003csub\u003e2\u003c/sub\u003e as a superior reducing agent in molten LiCl. It was also demonstrated that TiFe nanoparticles were difficult to activate compared to the bulk powder, since the oxidized surface layers of the nanoparticles were stabilized, which prevents the morphological change necessary for the activation.\u003c/p\u003e "},{"header":"Declarations","content":"\u003cp\u003e\u003cstrong\u003eAcknowledgements\u003c/strong\u003e\u003c/p\u003e\n\u003cp\u003eWe acknowledge the Advanced Characterization Nanotechnology Platform of the University of Tokyo and the Center for Instrumental Analysis Ibaraki University for sample characterization. The authors thank Prof. Noda at Waseda University for his support in SEM-EDS measurement.\u003c/p\u003e\n\u003cp\u003e\u003cstrong\u003eAuthor contributions statement\u003c/strong\u003e\u003c/p\u003e\n\u003cp\u003eY.K. designed the study, performed the experiments for TiFe synthesis. S.Y., S.Y. and N.H. conducted the hydrogen absorption experiments. S.T. and R.K. analysed the prepared nanoparticles and verified the results. All authors reviewed the manuscript.\u003c/p\u003e\n\u003cp\u003e\u003cstrong\u003eCompeting interests\u003c/strong\u003e\u003c/p\u003e\n\u003cp\u003eThe authors declare no competing interests.\u003c/p\u003e"},{"header":"References","content":"\u003col\u003e\u003cli\u003e\u003cspan\u003eG. Sandrock, J. Alloys Comp., 1999, 293\u0026ndash;295, 877.\u003c/span\u003e\u003c/li\u003e \u003cli\u003e\u003cspan\u003eN. A. A. Rusman and M. Dahari, Int. J. Hydrogen Energy, 2016, 41, 12108.\u003c/span\u003e\u003c/li\u003e \u003cli\u003e\u003cspan\u003eJ. J. Reilly and R. H. Wiswall Jr., Inorg. Chem., 1974, 13, 218.\u003c/span\u003e\u003c/li\u003e \u003cli\u003e\u003cspan\u003eG. K. Sujan, Z. Pan, H. Li, D. Liang and N. Alam, Crit. Rev. 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Iron Steel Inst. 1953, 174, 25.\u003c/span\u003e\u003c/li\u003e\u003c/ol\u003e"}],"fulltextSource":"","fullText":"","funders":[],"hasAdminPriorityOnWorkflow":false,"hasManuscriptDocX":true,"hasOptedInToPreprint":true,"hasPassedJournalQc":"","hasAnyPriority":false,"hideJournal":true,"highlight":"","institution":"","isAcceptedByJournal":false,"isAuthorSuppliedPdf":false,"isDeskRejected":"","isHiddenFromSearch":false,"isInQc":false,"isInWorkflow":false,"isPdf":false,"isPdfUpToDate":true,"isWithdrawnOrRetracted":false,"journal":{"display":true,"email":"[email protected]","identity":"researchsquare","isNatureJournal":false,"hasQc":true,"allowDirectSubmit":true,"externalIdentity":"","sideBox":"","snPcode":"","submissionUrl":"/submission","title":"Research Square","twitterHandle":"researchsquare","acdcEnabled":true,"dfaEnabled":false,"editorialSystem":"","reportingPortfolio":"","inReviewEnabled":false,"inReviewRevisionsEnabled":true},"keywords":"TiFe, CaH2, Chemical, Hydrogen","lastPublishedDoi":"10.21203/rs.3.rs-121222/v1","lastPublishedDoiUrl":"https://doi.org/10.21203/rs.3.rs-121222/v1","license":{"name":"CC BY 4.0","url":"https://creativecommons.org/licenses/by/4.0/"},"manuscriptAbstract":"\u003cp\u003e\tNanosizing of TiFe hydrogen storage alloy is conducted to facilitate its activation. Here, pure intermetallic TiFe nanoparticles (45 nm) were prepared using chemical reduction of oxide precursors at 600 °C, which is the lowest temperature ever used in chemical synthesis. This was achieved using a strong reducing agent (CaH\u003csub\u003e2\u003c/sub\u003e) in a molten LiCl. When used for hydrogen absorption, the obtained nanoparticles surprisingly exhibited almost no hydrogen absorption. The results demonstrated that TiFe nanoparticles are more difficult to activate than the bulk powder because the oxidized surface layers of the nanoparticles become stabilized, which prevents the morphological change necessary for their activation.\u003c/p\u003e","manuscriptTitle":"Low Temperature Chemical Synthesis of Intermetallic TiFe Nanoparticles for Hydrogen Absorption","msid":"","msnumber":"","nonDraftVersions":[{"code":1,"date":"2020-12-10 15:53:23","doi":"10.21203/rs.3.rs-121222/v1","editorialEvents":[{"type":"communityComments","content":0}],"status":"published","journal":{"display":true,"email":"[email protected]","identity":"researchsquare","isNatureJournal":false,"hasQc":true,"allowDirectSubmit":true,"externalIdentity":"","sideBox":"","snPcode":"","submissionUrl":"/submission","title":"Research Square","twitterHandle":"researchsquare","acdcEnabled":true,"dfaEnabled":false,"editorialSystem":"","reportingPortfolio":"","inReviewEnabled":false,"inReviewRevisionsEnabled":true}}],"origin":"","ownerIdentity":"2a40e57f-9f64-4b86-bd02-63783faa6e62","owner":[],"postedDate":"December 10th, 2020","published":true,"recentEditorialEvents":[],"rejectedJournal":[],"revision":"","amendment":"","status":"posted","subjectAreas":[{"id":1417464,"name":"Chemical Engineering"},{"id":1417465,"name":"Physical Chemistry"}],"tags":[],"updatedAt":"2020-12-31T10:29:10+00:00","versionOfRecord":[],"versionCreatedAt":"2020-12-10 15:53:23","video":"","vorDoi":"","vorDoiUrl":"","workflowStages":[]},"version":"v1","identity":"rs-121222","journalConfig":"researchsquare"},"__N_SSP":true},"page":"/article/[identity]/[[...version]]","query":{"redirect":"/article/rs-121222","identity":"rs-121222","version":["v1"]},"buildId":"_2-kVJe1T_tPrBINL-cwx","isFallback":false,"isExperimentalCompile":false,"dynamicIds":[84888],"gssp":true,"scriptLoader":[]}