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(C) In the given reaction: $Ag_2O + H_2O + 2e^- \rightarrow 2Ag + 2OH^-$$1$. The oxidation state of $Ag$ in $Ag_2O$ is $+1$,and it changes to $0$ in $

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Silver is reduced.

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(C) In the given reaction: $Ag_2O + H_2O + 2e^- \rightarrow 2Ag + 2OH^-$$1$. The oxidation state of $Ag$ in $Ag_2O$ is $+1$,and it changes to $0$ in $Ag$ metal.$2$. Since the oxidation number of $Ag$ decreases from $+1$ to $0$,it undergoes reduction.$3$. Therefore,$Ag$ is reduced.$4$. The oxidation states of $H$ $(+1)$ and $O$ $(-2)$ remain unchanged in $H_2O$ and $OH^-$,so neither oxidation nor reduction occurs for these elements.

Identify the correct statement for the reaction stated below:
$Ag_2O + H_2O + 2e^- \rightarrow 2Ag + 2OH^{-}$

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Identify the correct statement for the reaction stated below:$Ag_2O + H_2O + 2e^- \rightarrow 2Ag + 2OH^{-}$