Chemistry - Electrochemistry Question with Solution | TestHub

The given standard reduction potential for ${\text{Ag}}_{(aq)}^{+}+e^{-}\to {\text{Ag}}_{(s)}$ is $E^{\circ }=0.79$ V.

The required reaction is $2{\text{Ag}}_{(s)}\to 2{\text{Ag}}_{(aq)}^{+}+2e^{-}$, which is the reverse of the given reaction multiplied by $2$.

When a reaction is reversed, the sign of its standard potential is reversed. Thus, the oxidation potential is $-0.79$ V.

Standard electrode potential is an intensive property, meaning it does not depend on the stoichiometric coefficients of the reaction. Multiplying the reaction by $2$ does not change the value of the potential.

Therefore, the standard potential for the given reaction is $-0.79$ V.

Answer: $-0.79$ V