| Identification | More | [Name]
Ferrous sulfide | [CAS]
1317-37-9 | [Synonyms]
FERROUS SULFIDE
FERROUS SULPHIDE
IRON(+2)SULFIDE
IRON(II) SULFIDE
IRON(II) SULPHIDE
IRON MONOSULFIDE
IRON SULFIDE
blackironsulfide
ci77540
ferrousmonosulfide
ferroussulfide(fes)
ferroussulfide(iron(ii)
ferroussulfide(iron(ii)sulfide)
ironmonosulfide(fes)
ironprotosulfide
ironsulfide(fes)
ironsulfide[fes]
ironsulfuret
iron sulphide
Iron(Ⅱ) sulfide | [EINECS(EC#)]
215-268-6 | [Molecular Formula]
FeS | [MDL Number]
MFCD00011013 | [Molecular Weight]
87.91 | [MOL File]
1317-37-9.mol |
| Chemical Properties | Back Directory | [Appearance]
grey to brown-black lumps or powder | [Melting point ]
1195 °C
| [Boiling point ]
decomposes [HAW93] | [bulk density]
1500-2000kg/m3 | [density ]
4.84 g/mL at 25 °C(lit.)
| [vapor pressure ]
0Pa at 25℃ | [storage temp. ]
Storage temperature: no restrictions. | [solubility ]
insoluble in H2O; reacts with acid solutions | [form ]
Sticks | [color ]
Grayish-black | [Specific Gravity]
4.84 | [Odor]
Odorless | [Stability:]
Stable. Incompatible with strong acids, strong bases, metal oxides. Avoid moisture. | [Water Solubility ]
Soluble in water(0.0062g/L ), in acids with evolution of hydrogen sulfide. Insoluble in nitric acid. | [Specific Heat Capacity]
Cp(crystal):0.574451J/(g·K),at 25℃ | [Crystal Structure]
NiAs type | [Sensitive ]
Moisture Sensitive | [crystal system]
Six sides | [Merck ]
14,4058 | [Solubility Product Constant (Ksp)]
pKsp: 17.2 | [Space group]
P63/mmc | [Lattice constant]
| a/nm | b/nm | c/nm | α/o | β/o | γ/o | V/nm3 | | 0.345 | 0.345 | 0.567 | 90 | 90 | 120 | 0.0584 |
| [InChI]
1S/Fe.S | [InChIKey]
MBMLMWLHJBBADN-UHFFFAOYSA-N | [SMILES]
S=[Fe] | [CAS DataBase Reference]
1317-37-9(CAS DataBase Reference) | [EPA Substance Registry System]
1317-37-9(EPA Substance) |
| Hazard Information | Back Directory | [Chemical Properties]
grey to brown-black lumps or powder | [Physical properties]
Colorless hexagonal or tetragonal crystals; density 4.7g/cm3; melts at 1188°C; insoluble in water; soluble in acids (reacts). | [Flammability and Explosibility]
Nonflammable | [reaction suitability]
reagent type: catalyst
core: iron |
| Safety Data | Back Directory | [Symbol(GHS) ]
GHS07 | [Signal word ]
Warning | [Hazard statements ]
H315-H319-H335 | [Precautionary statements ]
P280-P302+P352-P304+P340 | [Hazard Codes ]
N | [Risk Statements ]
R31:Contact with acids liberates toxic gas.
R50:Very Toxic to aquatic organisms. | [Safety Statements ]
S60:This material and/or its container must be disposed of as hazardous waste .
S61:Avoid release to the environment. Refer to special instructions safety data sheet . | [RIDADR ]
UN 3077 9/PG 3
| [WGK Germany ]
3
| [F ]
13 | [TSCA ]
Yes | [REACH Registrations]
Active | [HazardClass ]
4.1 | [PackingGroup ]
III | [HS Code ]
28309011 | [Storage Class]
11 - Combustible Solids | [Hazardous Substances Data]
1317-37-9(Hazardous Substances Data) |
| Questions And Answer | Back Directory | [Uses]
Iron(II) sulfide occurs in nature as the minerals magnetkies, troillite and pyrrhotine. The most important application of this compound is in Kipp’s apparatus as a source for laboratory preparation of hydrogen sulfide. It also is used in paints, pigments, and ceramics and lubricant coatings.
| [Preparation]
Iron(II) sulfide may be synthesized from the elements but the product is contaminated with iron. The reaction is exothermic and the heat of reaction melts iron. Pure sulfide may be obtained by using a slight excess of sulfur: the excess then is distilled off.
The compound also may be precipitated by treating an aqueous solution of an alkali metal sulfide with that of iron(II) chloride or any iron(II) salt solution:
S2– (aq) + Fe2+ (aq) → FeS(s)
Another method of preparation involves passing a mixture of hydrogen sulfide and hydrogen over iron(III) oxide at about 1,000°C:
Fe2O3 + 2H2S + H2 → 2FeS + 3H2O
| [Reactions]
Iron(II) sulfide reacts with acids evolving hydrogen sulfide:
FeS + 2HCl → H2S + FeCl2
The compound is readily oxidized under moist condition by action of air, forming triiron tetroxide and elemental sulfur:
3FeS + 2O2 → Fe3O4 + 3S
The above reaction is exothermic.
Iron(II) sulfide decomposes to its elements when heated above 1,100°C:
FeS → Fe + S
When heated with boiled water, it generates sulfuric acid and hydrogen:
4FeS + 8H2O + 7O2 → 4H2SO4 + 4H2 + Fe2O3
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