Question

Which one of the following reactions involves disproportionation?

• A. $ 2{{H}_{2}}S{{O}_{4}}+Cu\xrightarrow{{}}CuS{{O}_{4}}+2{{H}_{2}}O+S{{O}_{2}} $
• B. $ A{{s}_{2}}{{O}_{3}}+3{{H}_{2}}S\xrightarrow{{}}A{{s}_{2}}{{S}_{3}}+3{{H}_{2}}O $
• C. $ 2KOH+C{{l}_{2}}\xrightarrow{{}}KCl+KOCl+{{H}_{2}}O $
• D. $ C{{a}_{3}}{{P}_{2}}+6{{H}_{2}}O\xrightarrow{{}}3Ca{{(OH)}_{2}}+2P{{H}_{3}} $
• E. $ 4N{{H}_{3}}+3{{O}_{2}}\xrightarrow{{}}2{{N}_{2}}+6{{H}_{2}}O $

Answer 1

Answer: (C)

The reactions, in which the same element is oxidized as well as reduced, are called disproportionation reactions.
In this reaction, the same element, ie, $ C{{l}_{2}} $ is oxidized as well as reduced, so it is an example of disproportionation reaction.