The figure shows NCERT's standard electrode potentials for copper at $298\ \text{K}$: $E^\circ(\text{Cu}^{2+}/\text{Cu}) = 0.34\ \text{V}$ and $E^\circ(\text{Cu}^+/\text{Cu}) = 0.52\ \text{V}$. The potential of the couple $\text{Cu}^{2+}/\text{Cu}^+$ is not given. In water, copper(I) ions react with one another: $2\text{Cu}^+(aq) \rightleftharpoons \text{Cu}^{2+}(aq) + \text{Cu}(s)$. This is why most simple copper(I) salts do not last in solution. Take $\dfrac{2.303RT}{F} = 0.059\ \text{V}$. Remember that electrode potentials cannot simply be added or subtracted when the numbers of electrons differ, but Gibbs energies can. Assume the solution is ideal and the temperature stays at $298\ \text{K}$. What is the equilibrium constant of this reaction at $298\ \text{K}$?

Fig. 1: A diagram of standard electrode potentials for copper. Arrows run from Cu2+ to Cu+ and from Cu+ to Cu. The arrow from Cu2+ to Cu+ is marked with a question mark; the arrow from Cu+ to Cu is marked 0.52 V. A longer curved arrow below runs straight from Cu2+ to Cu and is marked 0.34 V.