This is an old revision of this page, as edited by Event Nexus (talk | contribs) at 01:43, 16 August 2011 (grammar+style). The present address (URL) is a permanent link to this revision, which may differ significantly from the current revision.
Revision as of 01:43, 16 August 2011 by Event Nexus (talk | contribs) (grammar+style)(diff) ← Previous revision | Latest revision (diff) | Newer revision → (diff)| Names | |
|---|---|
| IUPAC name Iron(III) sulfide | |
| Other names
Iron sesquisulfide Ferric sulfide | |
| Identifiers | |
| CAS Number | |
| PubChem CID | |
| CompTox Dashboard (EPA) | |
| Properties | |
| Chemical formula | Fe2S3 |
| Molar mass | 207.90 g/mol |
| Appearance | yellow-green |
| Density | 4.3 g/cm |
| Melting point | decomposition |
| Solubility in water | very slightly soluble |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
 Y verify (what is ?)
Infobox references
| |
Iron(III) sulfide, also known as ferric sulfide or sesquisulfide, is one of the three iron sulfides besides FeS and FeS2. It is a solid, black powder but decays at ambient temperature into a yellow-green powder.
This is a relatively unstable artificial product that does not occur in nature.
Preparation and properties
Fe2S3 is prepared by addition of refrigerated iron(III) chloride dilution to also cooled sodium sulfide dilution.
- 2 FeCl3 + 3 Na2S → Fe2S3↓ + 6 NaCl
which decays at a temperature over 20°C into FeS and sulphur.
- Fe2S3 → 2 FeS + S↓
With hydrochloric acid it decays according to the following reaction equation:
- Fe2S3 + 4 HCl → 2 FeCl2 + 2 H2S↑ + S↓
References
- ^ Charles D. Hodgman, Handbook of Chemistry and Physics (1961), p.590
- Holleman, Wiberg: Inorganic Chemistry (2001), p. 1451; ISBN 0-12-352651-5
- H. Roempp, Chemie (1997), S. 1099; ISBN 3-13-734710-6