Decomposition of Calcium Carbonate (Calcination)

CaCO₃ → CaO + CO₂

Descripción general

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

Rol	Sustancia	Coeficiente	Estado
Reactivo	Calcium Carbonate CaCO₃	1	(s)
Producto	Calcium Oxide CaO	1	(s)
Producto	Carbon Dioxide CO₂	1	(g)

Ejemplo cotidiano

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

Importancia industrial

Esta reacción es fundamental para la producción de cemento (más de 4.000 millones de toneladas al año). También es la mayor fuente industrial individual de emisiones de CO₂, responsable de aproximadamente el 8 % de las emisiones globales.

Propiedades

Tipo: Decomposition
Reversible: Sí
Energía: Endotérmico
ΔH: 178,3 kJ/mol

Reacciones 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.