Formation of Iron(II) Sulfide

Fe + S → FeS

Übersicht

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.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Iron Fe 1 (s)
Reaktant Sulfur S 1 (s)

Alltägliches Beispiel

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

Industrielle Bedeutung

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

Eigenschaften

Typ
Synthesis
Reversibel
Nein
Energie
Exotherm
ΔH
-100,0 kJ/mol

Verwandte Reaktionen

Formation of Nitrogen Dioxide Formation of Potassium Chloride Formation of Sodium Bicarbonate Formation of Sodium Peroxide Formation of Silicon Dioxide Formation of Tungsten Carbide Formation of Copper(II) Sulfide Formation of Sulfur Dioxide Formation of Hydrogen Sulfide Formation of Carbon Monoxide

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.