Hydrogen peroxide acts both as an oxidizing and as a reducing agent depending upon the reacting species. In which of the following cases $H_{2} O_{2}$ acts as a reducing agent in acid medium?

{M n O}_{4}^{-}

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{S O}_{3}^{2 -}

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K l

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{C r}_{2} O_{7}^{2 -}

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Solution

The correct option is C ${M n O}_{4}^{-}$
$H_{2} O_{2}$ when act as reducing agent, oxygen is reduced to $H_{2} O$
(from $- 1$ to $- 2$ )
$H_{2} O_{2} + {2 H}^{+} + 2 e ⟶ 2 H_{2} O$
When $H_{2} O_{2}$ acts as oxidizing agent, oxygen is oxidized to $O_{2}$ (from $- 1$ to $0$ ) and bubbles are noticed.
${2 M n O_{4}}^{-} + 5 H_{2} O_{2} + {6 H}^{+} ⟶ 5 O_{2} + 2 M n^{2 +} + 8 H_{2} O$

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