The following equations are balanced atom wise and charge wise.
(p) ${Cr}_{2} O_{7}^{2 -} + 8 H^{+} + 3 H_{2} O_{2} \to 2 {Cr}^{3 +} + 7 H_{2} O + 3 O_{2}$
(q) ${Cr}_{2} O_{7}^{2 -} + 8 H^{+} + 5 H_{2} O_{2} \to 2 {Cr}^{3 +} + 9 H_{2} O + 4 O_{2}$
(r) ${Cr}_{2} O_{7}^{2 -} + 8 H^{+} + 7 H_{2} O_{2} \to 2 {Cr}^{3 +} + 11 H_{2} O + 5 O_{2}$
The precise equation/equations representing the oxidation of $H_{2} O_{2}$ is/are :

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(P) only

{Q) only

(R) only

all the three

answer is C.

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Detailed Solution

The reactions are as follows:

$\begin{array}{l} 6 e^{-} + 14 H^{+} + {Cr}_{2} O_{7}^{2 -} \to 2 {Cr}^{3 +} + 7 H_{2} O \\ 3 H_{2} O_{2} \to 3 O_{2} + 6 H^{+} + 6 e^{-} \\ {Cr}_{2} O_{7}^{2 -} + 8 H^{+} + 3 H_{2} O_{2} \to 2 {Cr}^{3 +} + 7 H_{2} O + 3 O_{2} \end{array}$

The precise equation/equations representing the oxidation of $H_{2} O_{2}$ is

${Cr}_{2} O_{7}^{2} + 8 H^{+} + 3 H_{2} O_{2} \to 2 {Cr}^{3 +} + 7 H_{2} O + 3 O_{2}$ .

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