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Hydrogen Peroxide

Which of the ...

Question

Which of the following equations depict the oxidizing nature of $H_{2} O_{2}$ ?

2 M n O_{4}^{-} + 6 H^{+} + 5 H_{2} O_{2} \to 2 M n^{2 +} + 8 H_{2} O + 5 O_{2}

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2 F e^{3 +} + 2 H^{+} + H_{2} O_{2} \to 2 F e^{2 +} + 2 H_{2} O + O_{2}

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2 H I + H_{2} O_{2} \to I_{2} + 2 H_{2} O

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K I O_{4} + H_{2} O_{2} \to K I O_{3} + H_{2} O + O_{2}

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Solution

The correct option is D $2 H I + H_{2} O_{2} \to I_{2} + 2 H_{2} O$
Oxidizing nature of $H_{2} O_{2}$ means it oxidizes other substance and itself gets reduced. In such reactions $O_{2}$ is not evolved.

In (A), $M n O_{4}^{-}$ gets reduced from $M n^{7 +}$ to $M n^{2 +} .$

In (B), $F e^{3 +}$ gets reduced to $F e^{2 +}$ .

In (C), $I^{-}$ gets oxidised to $I_{2}$

In (D), $K I O_{4}$ gets reduced from $I^{7 +}$ to $I^{5 +}$

Option C is correct.

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