Decomposition of Calcium Carbonate (Calcination)

CaCO₃ → CaO + CO₂

Aperçu

Calcium carbonate (limestone) decomposes when heated above 840 C into calcium oxide (quicklime) and carbon dioxide gas. This is one of the oldest known industrial chemical reactions, used for thousands of years in cement and mortar production. It is a key process in the cement industry.

Participants

Rôle	Substance	Coefficient	État
Réactif	Calcium Carbonate CaCO₃	1	(s)
Produit	Calcium Oxide CaO	1	(s)
Produit	Carbon Dioxide CO₂	1	(g)

Exemple du quotidien

Lime kilns that have operated for centuries use this reaction to convert limestone into quicklime for building materials.

Importance industrielle

This reaction is fundamental to cement production (over 4 billion tonnes annually). It is also the largest single industrial source of CO2 emissions, responsible for about 8% of global emissions.

Propriétés

Type: Decomposition
Réversible: Oui
Énergie: Endothermique
ΔH: 178,3 kJ/mol

Réactions associées

Decomposition of Ammonium Nitrate Decomposition of Calcium Hypochlorite Decomposition of Carbonic Acid Decomposition of Iron(II,III) Oxide (Direct Reduction) Decomposition of Nitrous Oxide (Laughing Gas) Decomposition of Barium Peroxide Decomposition of Sodium Bicarbonate Decomposition of Water (Electrolysis) Thermal Decomposition of Copper(II) Carbonate Cracking of Octane (Thermal Cracking)

Frequently Asked Questions

What is the equation for Decomposition of Calcium Carbonate (Calcination)?

The balanced equation is: CaCO₃ → CaO + CO₂.

What type of reaction is Decomposition of Calcium Carbonate (Calcination)?

Decomposition of Calcium Carbonate (Calcination) is a decomposition reaction. It is reversible under certain conditions.

Is Decomposition of Calcium Carbonate (Calcination) exothermic or endothermic?

Decomposition of Calcium Carbonate (Calcination) is endothermic (absorbs energy). The enthalpy change (ΔH) is 178.3 kJ/mol.