Balance the following redox reaction:

$C l O_{2} + O_{2}^{2 -} ⟶ C l O_{2}^{-} + O_{2}$

2 C l O_{2} + O_{2}^{2 -} ⟶ 2 C l O_{2}^{-} + O_{2}

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4 C l O_{2} + O_{2}^{2 -} ⟶ 2 C l O_{2}^{-} + O_{2}

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2 C l O_{2} + O_{2}^{2 -} ⟶ 3 C l O_{2}^{-} + O_{2}

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None of these

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Solution

The correct option is A $2 C l O_{2} + O_{2}^{2 -} ⟶ 2 C l O_{2}^{-} + O_{2}$
The unbalanced redox equation is as follows:
$C l O_{2} + O_{2}^{2 -} ⟶ C l O_{2}^{-} + O_{2}$

All atoms other than H and O are balanced.

The oxidation number of Cl changes from 4 to 3. The change in the oxidation number of Cl is 1.

The oxidation number of O changes from -1 to -2. The change in the oxidation number per O atom is 1. Total change in the oxidation number for 2 O atoms is 2.

The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying $C l O_{2}$ and $C l O_{2}^{-}$ with 2.

$2 C l O_{2} + O_{2}^{2 -} ⟶ 2 C l O_{2}^{-} + O_{2}$

This is the balanced chemical equation.

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