Iron(II) molybdate

Iron(II) molybdate
Names
	IUPAC name Iron(II) molybdate
Identifiers
CAS Number	13718-70-2;
3D model (JSmol)	Interactive image;
PubChem CID	16217045;
CompTox Dashboard (EPA)	DTXSID30584227 ;
	InChI InChI=1S/Fe.Mo.4O/q+2;;;;2*-1 Key: QQOCLJJWXLOEJE-UHFFFAOYSA-N;
	SMILES [O-][Mo](=O)(=O)[O-].[Fe+2];
Properties
Chemical formula	FeMoO4
Molar mass	215.78 g/mol
Appearance	Tan brown powder or crystals
Density	5.6 g/cm3 (20 °C)
Melting point	1,115 °C (2,039 °F; 1,388 K)
Solubility in water	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

Iron(II) molybdate is an inorganic compound with the chemical formula FeMoO₄.^[2]

Synthesis

Iron(II) molybdate is prepared by the reaction of iron(II) chloride or iron(II) sulfate^[3] and sodium molybdate.

Na₂MoO₄ + FeSO₄ → Na₂SO₄ + FeMoO₄

Na₂MoO₄ + FeCl₂ → 2 NaCl + FeMoO₄

Due to its very low aqueous solubility, iron(II) molybdate precipitates out as a brown powder from the above reactions, which can then be obtained by filtration.

Applications

FeMoO₄ has been used as relatively stable active material for anodes in Li-ion batteries for conversion reaction,^[4] as anode material in aqueous supercapacitors due to fast redox reactions^[3] and as catalyst for oxygen evolution in alkaline solutions.^[5]

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

^ "Iron(II) Molybdate". American Elements. Archived from the original on 2023-01-17. Retrieved 2023-01-17.
^ University of Akron Chemical Database^{[permanent dead link‍]}
^ ^a ^b 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.

[1] "Iron(II) Molybdate". American Elements. Archived from the original on 2023-01-17. Retrieved 2023-01-17.

[2] University of Akron Chemical Database^{[permanent dead link‍]}

[:0-3] 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.

[4] 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.

[5] 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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