Decomposition of Calcium Carbonate (Calcination)

CaCO₃ → CaO + CO₂

نظرة عامة

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.

المشاركون

الدور	المادة	المعامل	الحالة
متفاعل	Calcium Carbonate CaCO₃	1	(s)
منتج	Calcium Oxide CaO	1	(s)
منتج	Carbon Dioxide CO₂	1	(g)

مثال من الحياة اليومية

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

الأهمية الصناعية

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.

الخصائص

النوع: Decomposition
قابل للعكس: نعم
الطاقة: ماص للحرارة
ΔH: 178,3 kJ/mol

التفاعلات ذات الصلة

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.