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All the following are examples of disproportionation reactions except.

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$2 H_{2} O_{2} \to 2 H_{2} O + O_{2}$

$4 H_{3} {P O}_{3} \to 3 H_{3} {P O}_{4} + {P H}_{3}$

$3 K_{2} {MnO}_{4} + 4 HCl \to 2 {KMnO}_{4} + {MnO}_{2} + 4 KCl + 2 H_{2} O$

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

answer is C.

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Detailed Solution

$2 K \overset{+ 7}{M} n {\overset{- 2}{O}}_{4} ⟶ K_{2} \overset{+ 6}{M} n O_{4} + \overset{+ 4}{M} n O_{2} + {\overset{0}{O}}_{2}$

‘Mn’ undergoes reduction.
‘O’ undergoes oxidation.
It is not a disproportionation reaction

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