Decomposition of Calcium Carbonate (Calcination)

CaCO3 → CaO + CO2

概要

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.

参加者

役割 物質 係数 状態
反応物 Calcium Carbonate CaCO₃ 1 (s)
生成物 Calcium Oxide CaO 1 (s)
生成物 Carbon Dioxide CO₂ 1 (g)

日常の例

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

産業上の重要性

この反応はセメント生産(年間40億トン以上)の基本です。世界排出量の約8%を占める、最大の単一工業CO₂排出源でもあります。

特性

タイプ
Decomposition
可逆的
はい
エネルギー
吸熱性
ΔH
178.3 kJ/mol

関連する反応

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.