Ferrous sulfide Chemical Properties

Melting point:

1195 °C

Boiling point:

decomposes [HAW93]

Density 

4.84 g/mL at 25 °C(lit.)

vapor pressure 

0Pa at 25℃

storage temp. 

no restrictions.

solubility 

insoluble in H2O; reacts with acid solutions

form 

Sticks

Specific Gravity

4.84

color 

Grayish-black

Odor

Odorless

Water Solubility 

Soluble in water(0.0062g/L ), in acids with evolution of hydrogen sulfide. Insoluble in nitric acid.

Crystal Structure

NiAs type

Sensitive 

Moisture Sensitive

Merck 

14,4058

crystal system

Six sides

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

Stability:

Stable. Incompatible with strong acids, strong bases, metal oxides. Avoid moisture.

CAS DataBase Reference

1317-37-9(CAS DataBase Reference)

EPA Substance Registry System

Ferrous sulfide (1317-37-9)

Safety Information

Hazard Codes 

N

Risk Statements 

31-50

Safety Statements 

60-61-50

RIDADR 

UN 3077 9/PG 3

WGK Germany 

3

F 

13

TSCA 

Yes

HazardClass 

4.1

PackingGroup 

III

HS Code 

28309011

Hazardous Substances Data

1317-37-9(Hazardous Substances Data)

MSDS

• Language:English Provider:Ferrous sulfide
• Language:English Provider:ACROS
• Language:English Provider:SigmaAldrich
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Ferrous sulfide Usage And Synthesis

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

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).

Uses

Iron(II) sulfide is used to generate hydrogen sulfide instantaneously by reacting with hydrochloric acid. In laboratory, Kipp?s apparatus is utilized for this purpose. It is used as a re-sulphurizing and alloying agent, as a reducing agent to remove heavy metal impurities from phosphoric acid. It is used to control hydrogen embrittlement in alloy and stainless steel industries.

Uses

Ferrous sulfide can be used as a laboratory source of H2S; in the ceramic industry; as a paint pigment; in anodes; in lubricant coatings.

Flammability and Explosibility

Non flammable

Ferrous sulfide(1317-37-9)Related Product Information

• CARBONYL SULFIDE
• Hematite
• Hydrogen Sulfide
• Dimethyl sulfide
• Sodium sulfide
• FERROUS SULFATE
• Ferrous fumarate
• IRON SULFIDE,iron sulfide (naturally occurring mineral)
• copper iron sulfide
• MAGNESIUM SILICIDE
• Iron sulfide
• Ferrous sulfide
• Iron(Ⅲ) sulfide
• LEAD IRON SULFIDE
• COBALT IRON DISULFIDE
• Iron(III) sulfide
• Ferrous
• Ferrous Sulphide Sticks