Decomposition of Calcium Carbonate (Calcination)

CaCO₃ → CaO + CO₂

Overview

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

Role	Substance	Coefficient	State
Reactant	Calcium Carbonate CaCO₃	1	(s)
Product	Calcium Oxide CaO	1	(s)
Product	Carbon Dioxide CO₂	1	(g)

Everyday Example

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

Industrial Importance

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.

Properties

Type: Decomposition
Reversible: Yes
Energy: Endothermic
ΔH: 178.3 kJ/mol

Related Reactions

Cracking of Octane (Thermal Cracking) Decomposition of Ammonium Nitrate Decomposition of Barium Peroxide Decomposition of Calcium Hypochlorite Decomposition of Carbonic Acid Decomposition of Hydrogen Peroxide Decomposition of Iron(II,III) Oxide (Direct Reduction) Decomposition of Nitroglycerin Decomposition of Nitrous Oxide (Laughing Gas) Decomposition of Ozone

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.