Question #44053

Given the standard reduction potentials at $298\text{ K}$: $E^\circ_{\ce{Cu^+/Cu}} = +0.52\text{ V}$ $E^\circ_{\ce{Cu^{2+}/Cu^+}} = +0.16\text{ V}$ And the overall formation constants ($\beta$) for copper-ammonia complexes: $\beta_2 \text{ for } \ce{[Cu(NH_3)_2]^+} = 10^{11}$ $\beta_4 \text{ for } \ce{[Cu(NH_3)_4]^{2+}} = 10^{13}$ Consider the comproportionation reaction in an aqueous medium where the equilibrium concentration of free $\ce{NH_3}$ is maintained at $1.0\text{ M}$: $\ce{Cu(s) + [Cu(NH_3)_4]^{2+}(aq) \rightleftharpoons 2[Cu(NH_3)_2]^+(aq)}$ Which of the following correctly identifies the standard potential of this reaction ($E^\circ_{\text{rxn}}$) under these conditions and the thermodynamic stability of the $\ce{Cu(I)}$ state? (Take $\frac{2.303 RT}{F} = 0.06\text{ V}$)