Formation of Iron(II) Sulfide

Fe + S → FeS

Overview

Iron filings react with sulfur powder when heated to form iron(II) sulfide. This is a classic demonstration reaction in chemistry education, showing the difference between a mixture and a compound. Unlike the original mixture, iron sulfide cannot be separated with a magnet.

Participants

Role Substance Coefficient State
Reactant Iron Fe 1 (s)
Reactant Sulfur S 1 (s)

Everyday Example

This reaction is commonly demonstrated in school chemistry labs using iron filings and powdered sulfur with a Bunsen burner.

Industrial Importance

Iron sulfide (pyrite) is important in mining as an indicator of gold deposits. Synthetic iron sulfide is used in the production of sulfuric acid.

Properties

Type
Synthesis
Reversible
No
Energy
Exothermic
ΔH
-100.0 kJ/mol

Related Reactions

Fischer-Tropsch Synthesis (General) Formation of Aluminum Oxide Formation of Ammonia (Haber Process) Formation of Barium Oxide Formation of Barium Sulfate Formation of Beryllium Oxide Formation of Cadmium Oxide Formation of Calcium Carbonate from Oxides Formation of Calcium Hydroxide Formation of Calcium Oxide (Quicklime)

Frequently Asked Questions

What is the equation for Formation of Iron(II) Sulfide?
The balanced equation is: Fe + S → FeS.
What type of reaction is Formation of Iron(II) Sulfide?
Formation of Iron(II) Sulfide is a synthesis reaction.
Is Formation of Iron(II) Sulfide exothermic or endothermic?
Formation of Iron(II) Sulfide is exothermic (releases energy). The enthalpy change (ΔH) is -100.0 kJ/mol.