Here's the breakdown:
Decomposition Reaction:
* Definition: A single reactant breaks down into two or more products.
* General form: AB → A + B
* Example: The decomposition of water into hydrogen and oxygen: 2H₂O → 2H₂ + O₂
Synthesis Reaction:
* Definition: Two or more reactants combine to form a single product.
* General form: A + B → AB
* Example: The synthesis of water from hydrogen and oxygen: 2H₂ + O₂ → 2H₂O
Key Differences:
* Reactants and Products: Decomposition reactions start with one reactant and end with multiple products, while synthesis reactions start with multiple reactants and end with one product.
* Energy Change: Decomposition reactions typically require energy input (endothermic), while synthesis reactions often release energy (exothermic).
In summary, decomposition is the reverse of synthesis. They are not the same, but rather two opposite types of chemical reactions.
