Decomposition of Calcium Carbonate (Calcination)

CaCO₃ → CaO + CO₂

Visão geral

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.

Participantes

Papel	Substância	Coeficiente	Estado
Reagente	Calcium Carbonate CaCO₃	1	(s)
Produto	Calcium Oxide CaO	1	(s)
Produto	Carbon Dioxide CO₂	1	(g)

Exemplo do cotidiano

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

Importância industrial

Esta reação é fundamental para a produção de cimento (mais de 4 mil milhões de toneladas anuais). É também a maior fonte industrial única de emissões de CO₂, responsável por cerca de 8 % das emissões globais.

Propriedades

Tipo: Decomposition
Reversível: Sim
Energia: Endotérmico
ΔH: 178,3 kJ/mol

Reações relacionadas

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.