H_2O_2 reacts as a reducing agent with:(I) KM | vedclass

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(C) $H_2O_2$ acts as a reducing agent when it reacts with strong oxidizing agents,where it gets oxidized to $O_2$.$1$. With $KMnO_4$ in acidic medium:

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$I, II, III$

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(C) $H_2O_2$ acts as a reducing agent when it reacts with strong oxidizing agents,where it gets oxidized to $O_2$.$1$. With $KMnO_4$ in acidic medium: $2KMnO_4 + 3H_2SO_4 + 5H_2O_2 \rightarrow K_2SO_4 + 2MnSO_4 + 8H_2O + 5O_2$.$2$. With $K_2Cr_2O_7$ in acidic medium: $K_2Cr_2O_7 + 4H_2SO_4 + 3H_2O_2 \rightarrow K_2SO_4 + Cr_2(SO_4)_3 + 7H_2O + 3O_2$.$3$. With $Ag_2O$: $Ag_2O + H_2O_2 \rightarrow 2Ag + H_2O + O_2$.$HNO_3$ is an oxidizing agent,but $H_2O_2$ does not typically act as a reducing agent against it in standard conditions; rather,it is often used to reduce higher oxidation states. However,in the context of common textbook examples for $H_2O_2$ as a reducing agent,$I, II,$ and $III$ are the standard reactions.

$H_2O_2$ reacts as a reducing agent with:
$(I)$ $KMnO_4$
$(II)$ $K_2Cr_2O_7$
$(III)$ $Ag_2O$
$(IV)$ $HNO_3$

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$H_2O_2$ reacts as a reducing agent with:$(I)$ $KMnO_4$$(II)$ $K_2Cr_2O_7$$(III)$ $Ag_2O$$(IV)$ $HNO_3$