In which of the following reactions does H_2O | vedclass

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(D) reducing agent is a substance that loses electrons and undergoes oxidation.In reaction $(II)$,$H_2O_2 	o O_2 + 2H^{+} + 2e^-$,$H_2O_2$ loses elec

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$II$ and $IV$

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(D) reducing agent is a substance that loses electrons and undergoes oxidation.In reaction $(II)$,$H_2O_2 	o O_2 + 2H^{+} + 2e^-$,$H_2O_2$ loses electrons and is oxidized,thus acting as a reducing agent.In reaction $(IV)$,$H_2O_2 + 2OH^{-} 	o O_2 + 2H_2O + 2e^-$,$H_2O_2$ loses electrons and is oxidized,thus acting as a reducing agent.In reactions $(I)$ and $(III)$,$H_2O_2$ gains electrons and is reduced,acting as an oxidizing agent.Therefore,$H_2O_2$ acts as a reducing agent in reactions $(II)$ and $(IV)$.

In which of the following reactions does $H_2O_2$ act as a reducing agent?
$(I)$ $H_2O_2 + 2H^{+} + 2e^- \to 2H_2O$
$(II)$ $H_2O_2 \to O_2 + 2H^{+} + 2e^-$
$(III)$ $H_2O_2 + 2e^- \to 2OH^{-}$
$(IV)$ $H_2O_2 + 2OH^{-} \to O_2 + 2H_2O + 2e^-$

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In which of the following reactions does $H_2O_2$ act as a reducing agent?$(I)$ $H_2O_2 + 2H^{+} + 2e^- \to 2H_2O$$(II)$ $H_2O_2 \to O_2 + 2H^{+} + 2e^-$$(III)$ $H_2O_2 + 2e^- \to 2OH^{-}$$(IV)$ $H_2O_2 + 2OH^{-} \to O_2 + 2H_2O + 2e^-$