Identify oxidant and reductant in the following redox reactions.
$2 M n O_{4}^{2 -} + 2 H_{2} O c u r r e n t - --- \to 2 M n O_{4}^{-} + 2 {O H}^{-} + H_{2}$

Oxidant:

H_{2} O

; Reductant:

M n O_{4}^{2 -}

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Oxidant:

H_{2} O

; Reductant:

H_{2}

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Oxidant:

M n O_{4}^{2 -}

; Reductant:

H_{2} O

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None of these

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Solution

The correct option is C Oxidant: $H_{2} O$ ; Reductant: $M n O_{4}^{2 -}$
The balanced redox reaction is as follows:
$2 M n O_{4}^{2 -} + 2 H_{2} O c u r r e n t - --- \to 2 M n O_{4}^{-} + 2 {O H}^{-} + H_{2}$
The oxidation number of H changes from +1 to 0. Thus, hydrogen is reduced.
The oxidant is $H_{2} O$ .
The oxidation number of Mn changes from +6 to +7. Thus, Mn is oxidized.
The reductant is $M n O_{4}^{2 -}$ .

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