Which of the following reactant is oxidised in the following (unbalanced) reaction?
$C_{6} H_{5} O H + O_{3} ⟶ {C O}_{2} + H_{2} O + O_{2}$

C_{6} H_{5} O H

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O_{3}

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Both

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None

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Solution

The correct option is A $C_{6} H_{5} O H$
Phenol is oxidized to carbon dioxide. Ozone is reduced to oxygen.

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Similar questions

I^{-} + O_{3} ⟶ O_{2} + I_{2}

C_{6} H_{12} O_{6} ⟶ C_{2} H_{5} O H + C O_{2}

F e + O_{2} ⟶ {F e}_{2} O_{3}

N H_{3} + {C l}_{2} ⟶ N_{2} H_{4} + N H_{4} C l

N a + H_{2} O ⟶ N a O H + H_{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}

The reaction ; $2 O_{3}$ → $3 O_{2}$ , is assigned the following mechanism.

(I) $O_{3} ⇋ O_{2} + O (i i) O_{3} + O s l o w ⇌ 2 O_{2}$

The rate law of the reaction will therefore be

C O_{2}

H_{2} O

O_{3}

O_{2}

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