---
title: "An electrolytic cell is used to electroplate gold onto an electrode from an aqueous solution of gold(III) nitrate, \\(\\text{Au(NO}_3)_3\\text{(aq)}\\). The cathodic half-reaction is represented below.  \\[ \\text{Au}^{3+}\\text{(aq)} + 3\\,e^- \\rightarrow \\text{Au(s)} \\]  A constant current of \\(9.65\\text{ A}\\) is passed through the cell for \\(50.0\\text{ min}\\). Assuming that the reduction of \\(\\text{Au}^{3+}\\text{(aq)}\\) is the only process occurring at the cathode and proceeds with \\(100\\%\\) current efficiency, which of the following is closest to the mass of \\(\\text{Au(s)}\\) deposited on the electrode? (Faraday’s constant \\(F = 96{,}500\\text{ C/mol } e^-\\); molar mass of \\(\\text{Au} = 197.0\\text{ g/mol}\\))"
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url: "https://nerd-notes.com/ubq/121503/"
date_modified: "2026-08-23T05:04:52+00:00"
---

# An electrolytic cell is used to electroplate gold onto an electrode from an aqueous solution of gold(III) nitrate, \(\text{Au(NO}_3)_3\text{(aq)}\). The cathodic half-reaction is represented below.

\[ \text{Au}^{3+}\text{(aq)} + 3\,e^- \rightarrow \text{Au(s)} \]

A constant current of \(9.65\text{ A}\) is passed through the cell for \(50.0\text{ min}\). Assuming that the reduction of \(\text{Au}^{3+}\text{(aq)}\) is the only process occurring at the cathode and proceeds with \(100\%\) current efficiency, which of the following is closest to the mass of \(\text{Au(s)}\) deposited on the electrode? (Faraday’s constant \(F = 96{,}500\text{ C/mol } e^-\); molar mass of \(\text{Au} = 197.0\text{ g/mol}\))

An electrolytic cell is used to electroplate gold onto an electrode from an aqueous solution of gold(III) nitrate, \(\text{Au(NO}_3)_3\text{(aq)}\). The cathodic half-reaction is represented below.

\[ \text{Au}^{3+}\text{(aq)} + 3\,e^- \rightarrow \text{Au(s)} \]

A constant current of \(9.65\text{ A}\) is passed through the cell for \(50.0\text{ min}\). Assuming that the reduction of \(\text{Au}^{3+}\text{(aq)}\) is the only process occurring at the cathode and proceeds with \(100\%\) current efficiency, which of the following is closest to the mass of \(\text{Au(s)}\) deposited on the electrode? (Faraday's constant \(F = 96{,}500\text{ C/mol } e^-\); molar mass of \(\text{Au} = 197.0\text{ g/mol}\))

- **A.** \(0.328\text{ g}\)
- **B.** \(6.57\text{ g}\)
- **C.** \(9.85\text{ g}\)
- **D.** \(19.7\text{ g}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121503/*