Question #44786

An electrolytic cell consists of two parallel Platinum electrodes, each of area $10\text{ cm}^2$, separated by a distance of $5\text{ cm}$. The cell contains an aqueous solution of $0.01\text{ M } \ce{AgNO3 (aq)}$ and $0.01\text{ M } \ce{Cu(NO3)2 (aq)}$ buffered at $pH = 2$ at $298\text{ K}$. The specific conductance of the solution is constant at $0.008\text{ S cm}^{-1}$.

During electrolysis, water is oxidized at the anode to $\ce{O2 (g)}$ (at $1\text{ bar}$) with a constant overpotential of $0.49\text{ V}$. The limiting current for the reduction of $\ce{Ag+ (aq)}$ is $0.16\text{ A}$. Cathodic overpotentials for metal deposition are negligible.

Given: $E^\circ_{\ce{Ag+ /Ag}} = 0.80\text{ V}$ $E^\circ_{\ce{Cu^{2+} /Cu}} = 0.34\text{ V}$ $E^\circ_{\ce{O2 /H2O}} = 1.23\text{ V}$ $\frac{2.303 RT}{F} = 0.06\text{ V}$

What is the minimum applied voltage ($V_{app}$) required to just initiate the deposition of Copper?