---
title: "At 25°C, a student evaluates an electrochemical process for recovering zinc from an aqueous recycling stream. The reaction for the process is  \\(\\text{Zn}^{2+}\\text{(aq)} + \\text{Cu(s)} \\rightarrow \\text{Zn(s)} + \\text{Cu}^{2+}\\text{(aq)}\\)  The standard cell potential for the reaction as written is \\(-1.10\\text{ V}\\). Faraday’s constant is \\(96{,}500\\text{ C/mol e}^-\\). What is the standard Gibbs free-energy change, \\(\\Delta G^\\circ\\), for the reaction?"
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url: "https://nerd-notes.com/ubq/119412/"
date_modified: "2026-08-19T12:40:12+00:00"
---

# At 25°C, a student evaluates an electrochemical process for recovering zinc from an aqueous recycling stream. The reaction for the process is

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

The standard cell potential for the reaction as written is \(-1.10\text{ V}\). Faraday’s constant is \(96{,}500\text{ C/mol e}^-\). What is the standard Gibbs free-energy change, \(\Delta G^\circ\), for the reaction?

At 25°C, a student evaluates an electrochemical process for recovering zinc from an aqueous recycling stream. The reaction for the process is

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

The standard cell potential for the reaction as written is \(-1.10\text{ V}\). Faraday's constant is \(96{,}500\text{ C/mol e}^-\). What is the standard Gibbs free-energy change, \(\Delta G^\circ\), for the reaction?

- **A.** \(-212\text{ kJ/mol}\)
- **B.** \(+21.2\text{ kJ/mol}\)
- **C.** \(+106\text{ kJ/mol}\)
- **D.** \(+212\text{ kJ/mol}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119412/*