CAS 1317-37-9 Iron(II) sulfide - Catalysts / Alfa Chemistry

Synonyms

Iron(II) sulfide; Iron(II) sulfide, 99.9%, (trace metal basis), -100 mesh; Iron sulfide (FeS); Ferrous sulfide (FeS); Iron(II) sulfide, 29.0%; EC 215-268-6; Iron(II) sulfide (99.9%-Fe); Iron sulfide, troilite; Iron(II) sulfide, sticks, >=95% FeS basis; 8658AF;

IUPAC Name

sulfanylideneiron;

Molecular Weight

87.905g/mol

Molecular Formula

FeS;FeS;

Canonical SMILES

S=[Fe];

InChI

InChI=1S/Fe.S;

InChI Key

MBMLMWLHJBBADN-UHFFFAOYSA-N;

Melting Point

1194 deg C;

Density

4.75;

Solubility

0.00062 G/100 CC WATER AT 18 DEG C; INSOL IN NITRIC ACID; SOL IN ACIDS WITH EVOLUTION OF HYDROGEN SULFIDE;

Storage

Storage temperature: no restrictions.

Color Form

Colorless hexagonal crystals when pure; usually gray to brownish-black lumps, rods or granular powder; trimorphic with transition points @ 135 and 325 deg C;Dark-brown or black metallic pieces, sticks, or granules;

Complexity

Covalently-Bonded Unit Count

Decomposition

When heated to decomposition it emits toxic fumes of /sulfur oxides/.;

EC Number

215-268-6

Exact Mass

87.907g/mol

H-Bond Acceptor

Heavy Atom Count

Monoisotopic Mass

87.907g/mol

Other Experimental

Decomposes in hot water;Oxidized by moist air to S and Fe3O4.;Standard molar enthalpy (heat) of formation at 298.15 deg K is -100.0 kJ/mol (crystal); Standard molar Gibbs energy of formation at 298.15 deg K is -100.4 kJ/mol (crystal); Standard molar entropy at 298.15 deg K is 60.3 J/mol/K (crystal); Molar heat capacity at constant pressure at 298.15 deg K is 50.5 J/mol/K (crystal);Molar enthalpy (heat) of fusion 31.5 kJ/mol at 1188 deg C;Sugar, glycerin, & many organic hydroxy acids hinder precipitation. In neutral solution, soluble carbonates, phosphates, & oxalates produce precipitation. /Ferrous salts/;

Stability

Oxidized by moist air to sulfur and iron oxide.;

Topological Polar Surface Area

32.1A^2

Application

Iron(II) sulfide, appearing as grey to brown-black lumps or powder, serves crucial roles in various industries and scientific applications. It primarily finds use in Kipp's apparatus for preparing hydrogen sulfide in laboratories. This compound reacts with hydrochloric acid to quickly produce hydrogen sulfide, which is essential in many experimental setups. Additionally, iron(II) sulfide acts as a re-sulphurizing and alloying agent, helps remove heavy metal impurities from phosphoric acid, and is involved in controlling hydrogen embrittlement within the alloy and stainless steel industries. Beyond these applications, it is utilized in the production of paints, pigments, and ceramics, and serves as a component in lubricant coatings. When exposed to moist air, iron(II) sulfide oxidizes to form triiron tetroxide and elemental sulfur, an exothermic reaction, and it decomposes into iron and sulfur at temperatures above 1,100°C. Furthermore, when heated with boiled water, it can yield sulfuric acid and hydrogen. In its natural state, iron(II) sulfide is found in minerals such as magnetkies, troillite, and pyrrhotine, illustrating its widespread occurrence and industrial significance.

January 3, 2025

Reliable Source for Hydrogen Sulfide in Research

Iron(II) sulfide was invaluable in our lab for generating hydrogen sulfide using Kipp's apparatus. Its consistent performance facilitated our experiments on heavy metal reduction in phosphoric acid. Highly recommend for any industrial research needs.