---
title: "A galvanic cell operates under standard conditions at \\(298\\text{ K}\\) according to the following balanced equation:  \\[\\text{Zn}(s) + \\text{Cu}^{2+}(aq) \\rightarrow \\text{Zn}^{2+}(aq) + \\text{Cu}(s)\\]  Standard reduction potentials for the relevant half-reactions are provided in the table below.  | Half-reaction | \\(E^\\circ\\text{ (V)}\\) | | :— | :— | | \\(\\text{Cu}^{2+}(aq) + 2\\,e^- \\rightarrow \\text{Cu}(s)\\) | \\(+0.34\\) | | \\(\\text{Zn}^{2+}(aq) + 2\\,e^- \\rightarrow \\text{Zn}(s)\\) | \\(-0.76\\) |  What is the value of the standard Gibbs free energy change, \\(\\Delta G^\\circ\\), for the reaction? (Faraday’s constant \\(F = 96{,}500\\text{ J}/(\\text{V}\\cdot\\text{mol } e^-)\\))"
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date_modified: "2026-08-21T08:18:08+00:00"
---

# A galvanic cell operates under standard conditions at \(298\text{ K}\) according to the following balanced equation:

\[\text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s)\]

Standard reduction potentials for the relevant half-reactions are provided in the table below.

| Half-reaction | \(E^\circ\text{ (V)}\) |
| :— | :— |
| \(\text{Cu}^{2+}(aq) + 2\,e^- \rightarrow \text{Cu}(s)\) | \(+0.34\) |
| \(\text{Zn}^{2+}(aq) + 2\,e^- \rightarrow \text{Zn}(s)\) | \(-0.76\) |

What is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the reaction? (Faraday’s constant \(F = 96{,}500\text{ J}/(\text{V}\cdot\text{mol } e^-)\))

A galvanic cell operates under standard conditions at \(298\text{ K}\) according to the following balanced equation:

\[\text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s)\]

Standard reduction potentials for the relevant half-reactions are provided in the table below.

| Half-reaction | \(E^\circ\text{ (V)}\) |
| :--- | :--- |
| \(\text{Cu}^{2+}(aq) + 2\,e^- \rightarrow \text{Cu}(s)\) | \(+0.34\) |
| \(\text{Zn}^{2+}(aq) + 2\,e^- \rightarrow \text{Zn}(s)\) | \(-0.76\) |

What is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the reaction? (Faraday's constant \(F = 96{,}500\text{ J}/(\text{V}\cdot\text{mol } e^-)\))

- **A.** \(-425\text{ kJ/mol}_{\text{rxn}}\)
- **B.** \(-212\text{ kJ/mol}_{\text{rxn}}\)
- **C.** \(-106\text{ kJ/mol}_{\text{rxn}}\)
- **D.** \(+212\text{ kJ/mol}_{\text{rxn}}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119921/*