# How can I calculate for the theoritical potential needed to precipitate a metal in an electrolytic cell?

We were given a problem where we are to calculate the theoretical potential needed to initiate the deposition of $$\ce{Cu^2+}$$ in a solution buffered to $$\mathrm{pH} = 4.00$$ and the IR drop associated with $$\pu{0.15 A}$$ of applied current. Oxygen is evolved from the anode at a partial pressure of $$\pu{730 torr}$$ and the measured resistance of the cell at $$\pu{298 K}$$ is $$\pu{3.60 Ω}.$$

I know that I should reverse the reaction of the most spontaneous half cell reaction to favor the reduction of $$\ce{Cu^2+}$$ in the cathode. However, I do not know if I should just add the standard cell potential of the electrolytic cell just like how it will be if this was an electrochemical cell.

\begin{align} \ce{Cu^2+ + 2 e- &<=> Cu} &\quad E^\circ &= \pu{0.337 V} \\ \ce{O2(g) + 4 H+ + 4 e- &<=> 2 H2O} &\quad E^\circ &= \pu{1.229 V} \end{align}