11th Class Chemistry Hydrocarbons

  • question_answer 15) How do you account for the formation of ethane during chlorination of methane?

    Answer:

    Chlorination of methane proceeds by free radical mechanism. Initiation step: Propagation step: Termination step: \[\underset{Methyl\,free\,radical}{\mathop{\overset{\centerdot }{\mathop{C}}\,{{H}_{3}}+\overset{\centerdot }{\mathop{C}}\,{{H}_{3}}}}\,\to \underset{Ethane}{\mathop{C{{H}_{3}}-C{{H}_{3}}}}\,\] Two \[\overset{\centerdot }{\mathop{C}}\,{{H}_{3}}\] free radicals combine together to formethane molecule. \[\overset{\centerdot }{\mathop{C}}\,{{H}_{3}}+\overset{\centerdot }{\mathop{Cl}}\,\to C{{H}_{3}}-Cl\] \[\overset{\centerdot }{\mathop{Cl}}\,+\overset{\centerdot }{\mathop{Cl}}\,\to C{{l}_{2}}\]  


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