---
title: "A student electroplates pure copper onto an electrode using an aqueous solution of \\(\\text{CuSO}_4\\). A constant current of \\(9.65\\text{ A}\\) is passed through the electrolytic cell for \\(2{,}000\\text{ s}\\).  \\[ \\text{Cu}^{2+}\\text{(aq)} + 2\\,e^- \\rightarrow \\text{Cu(s)} \\]  Assuming that all current is consumed in the reduction of \\(\\text{Cu}^{2+}\\text{(aq)}\\) ions, what mass of \\(\\text{Cu(s)}\\) is deposited on the electrode? (Faraday’s constant \\(F = 96{,}500\\text{ C/mol } e^-\\); molar mass of \\(\\text{Cu} = 63.55\\text{ g/mol}\\))"
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url: "https://nerd-notes.com/ubq/120362/"
date_modified: "2026-08-23T04:23:24+00:00"
---

# A student electroplates pure copper onto an electrode using an aqueous solution of \(\text{CuSO}_4\). A constant current of \(9.65\text{ A}\) is passed through the electrolytic cell for \(2{,}000\text{ s}\).

\[ \text{Cu}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Cu(s)} \]

Assuming that all current is consumed in the reduction of \(\text{Cu}^{2+}\text{(aq)}\) ions, what mass of \(\text{Cu(s)}\) is deposited on the electrode? (Faraday’s constant \(F = 96{,}500\text{ C/mol } e^-\); molar mass of \(\text{Cu} = 63.55\text{ g/mol}\))

A student electroplates pure copper onto an electrode using an aqueous solution of \(\text{CuSO}_4\). A constant current of \(9.65\text{ A}\) is passed through the electrolytic cell for \(2{,}000\text{ s}\).

\[ \text{Cu}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Cu(s)} \]

Assuming that all current is consumed in the reduction of \(\text{Cu}^{2+}\text{(aq)}\) ions, what mass of \(\text{Cu(s)}\) is deposited on the electrode? (Faraday's constant \(F = 96{,}500\text{ C/mol } e^-\); molar mass of \(\text{Cu} = 63.55\text{ g/mol}\))

- **A.** \(0.100\text{ g}\)
- **B.** \(1.59\text{ g}\)
- **C.** \(3.18\text{ g}\)
- **D.** \(6.36\text{ g}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120362/*