(a) $H_{2} O_{2} + O_{3} \to H_{2} O + 2 O_{2}$
(b) $H_{2} O_{2} + A g_{2} O \to 2 A g + H_{2} O + O_{2}$
Role of hydrogen peroxide in the above reactions is respectively:

Oxidizing in (a) and reducing in (b)

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Reducing in (a) and oxidizing in (b)

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Reducing in (a) and (b)

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Oxidizing in (a) and (b)

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Solution

The correct option is D Reducing in (a) and (b)
(a) $H_{2} O_{2} + O_{3} \to H_{2} O + 2 O_{2}$
In this reaction, $O_{3}$ is reduced into $O^{- 2}$ ion .
(b) $H_{2} O_{2} + A g_{2} O \to 2 A g + H_{2} O + O_{2}$
In this reaction, $A g_{2} O$ is reduced to Ag .
Hence, $H_{2} O_{2}$ acts as reducing agent in both the reactions.

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Similar questions

(I) H_{2} O_{2} + O_{3} \to H_{2} O + 2 O_{2}

(I I) H_{2} O_{2} + A g_{2} O \to 2 A g + H_{2} O + O_{2}

(I) H_{2} O_{2} + O_{3} \to H_{2} O + 2 O_{2}

(I I) H_{2} O_{2} + A g_{2} O \to 2 A g + H_{2} O + O_{2}

In the reaction $A g_{2} O + H_{2} O_{2} \to 2 A g + H_{2} O + O_{2} . H_{2} O_{2}$ acts as :

(i) H_{2} O_{2} + O_{3} \to H_{2} O + 2 O_{2} (i i) H_{2} O_{2} + A g_{2} O \to 2 A g + H_{2} O + O_{2}

H_{2} O_{2}

A g_{2} O + H_{2} O_{2} \to 2 A g + H_{2} O + O_{2}

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