Example of a disproportionation reaction is

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$2 N a B r + {C l}_{2} \to 2 N a C l + {B r}_{2}$

$2 C u B r \to {C u B r}_{2} + C u$

$2 {M n O}_{4}^{-} + 10 I^{-} + 16 H^{+} \to 2 {M n}^{2 +} + 5 I_{2} + 8 H_{2} O$

$2 {K M n O}_{4} \to K_{2} {M n O}_{4} + {M n O}_{2} + O_{2}$

answer is A.

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Detailed Solution

Disproportionation reaction is a reaction in which one element undergoes both oxidation and reduction simultaneously.

Here in reaction A manganese only undergoes reduction i.e from +7 to +6 and +4.

In the reaction B, Copper undergoes both oxidation and reduction since it goes from +1 to +2 and 0 thus this is a disproportionation reaction.

In the reaction C ,all elements attains only one kind of ox state in product side hence cannot be a disproportionation reaction

In the reaction D, all elements attains only one kind of ox state in product side hence cannot be a disproportionation reaction

Hence option (B) is the correct answer.

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