In which of the following reactions does H_2O | vedclass

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(B) To determine if $H_2O_2$ acts as an oxidising agent,we look for reactions where the oxygen in $H_2O_2$ (oxidation state $-1$) is reduced to $-2$ (

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$(i)$,$(iv)$

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(B) To determine if $H_2O_2$ acts as an oxidising agent,we look for reactions where the oxygen in $H_2O_2$ (oxidation state $-1$) is reduced to $-2$ (as in $H_2O$).$(i)$ $2Fe^{2+} + H_2O_2 \rightarrow 2Fe^{3+} + 2OH^{-}$: Here,$Fe^{2+}$ is oxidised to $Fe^{3+}$,so $H_2O_2$ acts as an oxidising agent.$(ii)$ $2MnO_4^{-} + 6H^{+} + 5H_2O_2 \rightarrow 2Mn^{2+} + 5O_2 + 8H_2O$: Here,$H_2O_2$ is oxidised to $O_2$ ($0$ oxidation state),so it acts as a reducing agent.$(iii)$ $I_2 + H_2O_2 + 2OH^{-} \rightarrow 2I^{-} + O_2 + 2H_2O$: Here,$H_2O_2$ is oxidised to $O_2$,so it acts as a reducing agent.$(iv)$ $Mn^{2+} + H_2O_2 \rightarrow Mn^{4+} + 2OH^{-}$: Here,$Mn^{2+}$ is oxidised to $Mn^{4+}$,so $H_2O_2$ acts as an oxidising agent.Thus,in reactions $(i)$ and $(iv)$,$H_2O_2$ acts as an oxidising agent.

In which of the following reactions does $H_2O_2$ act as an oxidising agent (either in acidic,alkaline,or neutral medium)?
$(i)$ $2Fe^{2+} + H_2O_2 \rightarrow$
$(ii)$ $2MnO_4^{-} + 6H^{+} + 5H_2O_2 \rightarrow$
$(iii)$ $I_2 + H_2O_2 + 2OH^{-} \rightarrow$
$(iv)$ $Mn^{2+} + H_2O_2 \rightarrow$

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In which of the following reactions does $H_2O_2$ act as an oxidising agent (either in acidic,alkaline,or neutral medium)?$(i)$ $2Fe^{2+} + H_2O_2 \rightarrow$$(ii)$ $2MnO_4^{-} + 6H^{+} + 5H_2O_2 \rightarrow$$(iii)$ $I_2 + H_2O_2 + 2OH^{-} \rightarrow$$(iv)$ $Mn^{2+} + H_2O_2 \rightarrow$