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.