Which of the following is not an example of disproportionation reaction

4 K C l O_{3} \to 3 K C l O_{4} + K C l

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C l_{2} + K I O_{3} + 2 K O H \to K I O_{4} + 2 K C l + H_{2} O

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3 C l_{2} + 6 N a O H \to 5 N a C l + N a C l O_{3} + 3 H_{2} O

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4 P + 3 N a O H + 3 H_{2} O \to 3 N a H_{2} P O_{2} + P H_{3}

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Solution

The correct option is B $C l_{2} + K I O_{3} + 2 K O H \to K I O_{4} + 2 K C l + H_{2} O$
In all the above reactions, at least one element undergoes both oxidation and reduction. These are example of disproportionation reactions.
But in option B there are no elelment or species with undergo both oxidation and reduction.

$0 C l_{2} + + 1 + 5 - 2 K I O_{3} + 2 + 1 - 1 K O H \to + 1 - 1 - 2 K I O_{4} + 2 + 1 - 1 K C l + + 1 - 2 H_{2} O$

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Similar questions

$P_{4} + 3 N a O H + 3 H_{2} O ⟶ 3 N a (H_{2} P O_{2}) + P H_{3}$ is an example of:

3 {C l}_{2} + 6 N a O H ⟶ 5 N a C l + N a C l O_{3} + 3 H_{2} O

$P_{4} + 3 N a O H + 3 H_{2} O ⟶ 3 N a (H_{2} P O_{2}) + P H_{3}$ is an example of:

3 C l_{2} + 6 N a O H ⟶ 5 N a C l + N a C l O_{3} + 3 H_{2} O

3 C l_{2} + 6 N a O H \to 5 N a C l + N a C l O_{3} + 3 H_{2} O

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