Iron(II) molybdate
Iron(II) molybdate is an inorganic compound with the chemical formula FeMoO4.[1]
| Names | |
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| IUPAC name
Iron(II) molybdate | |
| Identifiers | |
3D model (JSmol) |
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PubChem CID |
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CompTox Dashboard (EPA) |
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| Properties | |
| FeMoO4 | |
| Molar mass | 215.78 g/mol |
| Appearance | Light yellow powder |
| Density | 5.6 g/cm3 (20 °C) |
| Melting point | 1,115 °C (2,039 °F; 1,388 K) |
| 0.00766 g/100 mL (20 °C) 0.038 g/100 mL (100 °C) | |
| Thermochemistry | |
Heat capacity (C) |
118.5 J/mol K |
Std enthalpy of formation (ΔfH⦵298) |
-1075 KJ/mol |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Formation
Iron(II) molybdate is created by the reaction of iron(II) chloride or iron(II) sulfate[2] and sodium molybdate.
Applications
FeMoO4 has been used as relatively stable active material for anodes in Li-ion batteries for conversion reaction,[3] as anode material in aqueous supercapacitors due to fast redox reactions[2] and as catalyst for oxygen evolution in alkaline solutions.[4]
Safety
Iron(II) molybdate is toxic and may cause irritation. It should not be released into the environment. Inhalation of dusts should be avoided.
References
- University of Akron Chemical Database
- Senthilkumar, Baskar; Kalai Selvan, Ramakrishnan (2014-07-15). "Hydrothermal synthesis and electrochemical performances of 1.7 V NiMoO4⋅xH2O||FeMoO4 aqueous hybrid supercapacitor". Journal of Colloid and Interface Science. 426: 280–286. doi:10.1016/j.jcis.2014.04.010. PMID 24863794.
- Zhang, Zhenyu; Li, Wenyue; Ng, Tsz-Wai; Kang, Wenpei; Lee, Chun-Sing; Zhang, Wenjun (2015-10-13). "Iron(ii) molybdate (FeMoO4) nanorods as a high-performance anode for lithium ion batteries: structural and chemical evolution upon cycling". J. Mater. Chem. A. 3 (41): 20527–20534. doi:10.1039/c5ta05723j. ISSN 2050-7496.
- Singh, R. N.; Singh, J. P.; Singh, A. (2008-08-01). "Electrocatalytic properties of new spinel-type MMoO4 (M = Fe, Co and Ni) electrodes for oxygen evolution in alkaline solutions". International Journal of Hydrogen Energy. 33 (16): 4260–4264. doi:10.1016/j.ijhydene.2008.06.008.
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