---
title: "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?"
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url: "https://nerd-notes.com/ubq/120363/"
date_modified: "2026-08-23T04:23:25+00:00"
---

# 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?

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?

- **A.** Sign of \(\Delta G^\circ\): negative (\(\Delta G^\circ < 0\)); Electrode where oxidation occurs: \(\text{Ni(s)}\)
- **B.** Sign of \(\Delta G^\circ\): positive (\(\Delta G^\circ > 0\)); Electrode where oxidation occurs: \(\text{Cu(s)}\)
- **C.** Sign of \(\Delta G^\circ\): negative (\(\Delta G^\circ < 0\)); Electrode where oxidation occurs: \(\text{Cu(s)}\)
- **D.** Sign of \(\Delta G^\circ\): positive (\(\Delta G^\circ > 0\)); Electrode where oxidation occurs: \(\text{Ni(s)}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120363/*