A student compares two electrochemical processes involving cadmium and copper electrodes in \(1.0 \text{ M}\) aqueous solutions at \(298 \text{ K}\).

Process 1 occurs in a galvanic cell:
\[\text{Cd}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Cd}^{2+}(aq) + \text{Cu}(s) \quad E^\circ_{\text{cell}} = +0.74 \text{ V}\]

Process 2 occurs in an electrolytic cell connected to an external power source:
\[\text{Cu}(s) + \text{Cd}^{2+}(aq) \rightarrow \text{Cu}^{2+}(aq) + \text{Cd}(s) \quad E^\circ_{\text{cell}} = -0.74 \text{ V}\]

Which of the following correctly compares \(\Delta G^\circ\) and \(K\) for Process 1 to those for Process 2, and provides the correct thermodynamic reasoning?