Chemistry - Electrochemistry Question with Solution | TestHub

The given reduction reaction is ${\mathrm{Cu}}_{(\mathrm{aq})}^{+2}+2{\mathrm{e}}^{-}\to {\mathrm{Cu}}_{(\mathrm{s})}$ with $E^{\circ }=+0.34\mathrm{V}$.

The required reaction is the reverse of the given reaction, multiplied by 2: $2{\mathrm{Cu}}_{(\mathrm{s})}\to 2{\mathrm{Cu}}_{(\mathrm{aq})}^{+2}+4{\mathrm{e}}^{-}$.

When a reaction is reversed, the sign of its standard potential is reversed. Thus, the potential becomes $-0.34\mathrm{V}$.

Standard electrode potential is an intensive property, meaning it is independent of the amount of substance or the stoichiometric coefficients in the balanced equation. Multiplying the reaction by 2 does not change the value of $E^{\circ }$.

Therefore, the standard potential of the required reaction is $-0.34\mathrm{V}$.

Answer: $-0.34\mathrm{V}$