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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.

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

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