CH3-CH2-CH3+CL2-
The reaction you've written appears to involve propane (CH₃-CH₂-CH₃) reacting with chlorine (Cl₂). This is a halogenation reaction, where chlorine reacts with an alkane (in this case, propane) to form alkyl chlorides.
When propane reacts with chlorine in the presence of light or heat, it can undergo free radical substitution. The overall reaction can be represented as follows:
Initiation: Cl₂ dissociates into two chlorine radicals (Cl·) under UV light or heat.
\( \text{Cl}_2 \rightarrow 2 \text{Cl} \cdot \)
Propagation: A chlorine radical abstracts a hydrogen from propane, forming a propane radical and HCl.
\( \text{C}_3\text{H}_8 + \text{Cl} \cdot \rightarrow \text{C}_3\text{H}_7 \cdot + \text{HCl} \)
The propane radical can then react with another chlorine molecule, forming an alkyl chloride and regenerating the chlorine radical.
\( \text{C}_3\text{H}_7 \cdot + \text{Cl}_2 \rightarrow \text{C}_3\text{H}_7\text{Cl} + \text{Cl} \cdot \)
Termination: Eventually, free radicals combine to terminate the reaction.
The products of the reaction could include:
- 1-chloropropane (CH₃-CH₂-CH₂Cl)
- 2-chloropropane (CH₃-CHCl-CH₃)
- Additional chlorinated by-products, depending on the extent of the reaction and the conditions.
Keep in mind that chlorination is not very selective, and you can expect a mixture of products if the reaction is allowed to proceed for a longer time.
