Here's why:
* Photolysis involves the breaking of chemical bonds using light energy.
* Decomposition reactions break down a single reactant into two or more products.
* Chlorination of methane involves the reaction of methane (CH4) with chlorine gas (Cl2) in the presence of UV light. This process produces chloromethane (CH3Cl) and hydrogen chloride (HCl).
Reaction:
CH4 + Cl2 → CH3Cl + HCl
Explanation:
1. Initiation: UV light breaks the chlorine molecule (Cl2) into two chlorine radicals (Cl•).
2. Propagation: A chlorine radical reacts with methane (CH4) to form a methyl radical (CH3•) and HCl.
3. Propagation: The methyl radical reacts with another chlorine molecule to form chloromethane (CH3Cl) and another chlorine radical.
This process continues until all the methane or chlorine is consumed. This reaction is not a decomposition reaction because it involves two reactants (methane and chlorine) forming two products (chloromethane and hydrogen chloride).
Therefore, chlorination of methane is a photolytic reaction that is not a decomposition reaction.
