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title: "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?"
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url: "https://nerd-notes.com/ubq/123934/"
date_modified: "2026-09-28T12:32:18+00:00"
---

# 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?

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?

- **A.** \(\Delta G^\circ_1 > \Delta G^\circ_2\) and \(K_1 < K_2\), because the positive cell potential of Process 1 indicates that work must be done on the system, making products less thermodynamically favored.
- **B.** \(\Delta G^\circ_1 > \Delta G^\circ_2\) and \(K_1 > K_2\), because a positive cell potential increases the activation energy barrier, shifting the equilibrium position toward the products.
- **C.** \(\Delta G^\circ_1 < \Delta G^\circ_2\) and \(K_1 > K_2\), because \(\Delta G^\circ = -nFE^\circ_{\text{cell}}\) means the positive \(E^\circ_{\text{cell}}\) of Process 1 results in \(\Delta G^\circ < 0\), which corresponds to \(K > 1\) through \(\Delta G^\circ = -RT\ln K\).
- **D.** \(\Delta G^\circ_1 < \Delta G^\circ_2\) and \(K_1 < K_2\), because although Process 1 is thermodynamically favored, the external voltage applied in Process 2 increases the value of the equilibrium constant such that \(K_2 > 1\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123934/*