Step 1: Identify the type of reaction:
The given reaction is:
\[\text{CaCO}_3 \xrightarrow{\text{heat}} \text{CaO} + \text{CO}_2\]
This is a thermal decomposition reaction, where a single compound breaks down into two or more simpler substances when heated.
Step 2: Understand the reactant – Calcium Carbonate (CaCO3):
- Calcium carbonate is a white solid commonly found in limestone, chalk, and marble.
- It is widely used in construction and manufacturing processes.
Step 3: Apply heat to initiate decomposition:
When calcium carbonate is heated strongly, it decomposes into:
- Calcium oxide (CaO): Also known as quick lime, it is a white, caustic, alkaline solid.
- Carbon dioxide (CO2): A colorless gas released during the decomposition.
Step 4: Balanced chemical equation:
\[
\text{CaCO}_3 \xrightarrow{\text{heat}} \text{CaO} + \text{CO}_2
\]
This equation is already balanced, with one calcium (Ca), one carbon (C), and three oxygen (O) atoms on both sides.
Step 5: Uses of quick lime (CaO):
- Used in the manufacture of cement and mortar in the construction industry.
- Acts as a flux in steel manufacturing to remove impurities.
- Used in the production of slaked lime by adding water.
Step 6: Conclusion:
Heating calcium carbonate results in the formation of calcium oxide (quick lime) and carbon dioxide. This thermal decomposition is important in several industrial applications, especially in construction and metallurgy.
