A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more simpler substances. These products can be elements or smaller compounds.
This reaction is usually the opposite of a synthesis (or combination) reaction. Decomposition often requires an input of energy, such as heat, light, or electricity, to break the chemical bonds.
Examples of decomposition reactions:
- Heating calcium carbonate (CaCO₃) produces calcium oxide (CaO) and carbon dioxide (CO₂).
- Electrolysis of water (H₂O) produces hydrogen gas (H₂) and oxygen gas (O₂).
Key points about decomposition reactions:
- They start with one reactant and produce two or more products.
- They often need energy to proceed.
- They are important in processes like respiration, photosynthesis breakdown steps, and industrial reactions.
In simple terms, a decomposition reaction is when one substance splits into simpler substances.