Chapter 18, Problem 136CWP

An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag⁺] = 1.00 M separated by a porous disk from a compartment with a copper metal electrode immersed in a solution of 10.00 M NH₃ that also contains 2.4 × 10⁻³ M Cu(NH₃)₄²⁺. The equilibrium between Cu²⁺ and NH₃ is:

$\begin{array}{cc}{\text{Cu}}^{2+}\left(aq\right)+4{\text{NH}}_3\left(aq\right)\rightleftharpoons \text{Cu}{\left(\text{N}\text{}{\text{H}}_{\text{3}}\right)}_4{}^{2+}\left(aq\right)& K=1.0\times {10}^{13}\end{array}$

and the two cell half-reactions are:

Assuming Ag⁺ is reduced, what is the cell potential at 25°C?