A student constructs two separate electrochemical cells using standard \(\text{Ni(s)}\mid\text{Ni}^{2+}\text{(aq)}\) and \(\text{Cu(s)}\mid\text{Cu}^{2+}\text{(aq)}\) half-cells at \(298\text{ K}\).

In Setup 1, the half-cells are connected through a wire and a salt bridge, allowing the system to operate as a galvanic cell.

In Setup 2, a \(\text{DC}\) power supply providing \(1.5\text{ V}\) is connected to the electrodes to reverse the direction of electron flow, forcing the system to operate as an electrolytic cell.

The standard reduction potentials are given below.
\[\text{Ni}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Ni(s)} \quad E^\circ = -0.25\text{ V}\]
\[\text{Cu}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Cu(s)} \quad E^\circ = +0.34\text{ V}\]

Which of the following correctly identifies the sign of \(\Delta G^\circ\) for the net chemical reaction occurring in Setup 2 and the identity of the electrode at which oxidation occurs?