Identify the pair of reactions undergoing dis | vedclass

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(A) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.$1. 2 H_2\stackrel{-1}{O_2} \righ

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$2 H_2O_2 \rightarrow 2 H_2O + O_2$ and $Cl_2 + 2 NaOH \rightarrow NaCl + NaOCl + H_2O$

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(A) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.$1. 2 H_2\stackrel{-1}{O_2} \rightarrow 2 H_2\stackrel{-2}{O} + \stackrel{0}{O_2}$Here,the oxidation state of oxygen changes from $-1$ to $-2$ (reduction) and from $-1$ to $0$ (oxidation).$2. \stackrel{0}{Cl_2} + 2 OH^{-} \rightarrow \stackrel{-1}{Cl^{-}} + \stackrel{+1}{ClO^{-}} + H_2O$Here,the oxidation state of chlorine changes from $0$ to $-1$ (reduction) and from $0$ to $+1$ (oxidation).Both reactions involve the same element undergoing both oxidation and reduction,hence they are disproportionation reactions.

Identify the pair of reactions undergoing disproportionation from the following.

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