In which one of the following reactions does ozone act as a reducing agent?

B a O_{2} + O_{3} \to B a O + 2 O_{2}

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

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P b S + 4 O_{3} \to {P b S O}_{4} + 4 O_{2}

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

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Solution

The correct option is A $B a O_{2} + O_{3} \to B a O + 2 O_{2}$
The reaction is as follows:
$+ 4$ $+ 2$
$B a O_{2} + O_{3} ⟶ B a O + 2 O_{2}$
The oxidation state of $B a$ in the above reaction changes from $+ 4$ to $+ 2$ . Hence, $B a$ is being reduced by $O_{3}$ . So. in the above reaction, $O_{3}$ acts as a reducing agent.

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