---
title: "A student electrolyzes an aqueous solution of \\(\\text{CuSO}_4\\text{(aq)}\\) to deposit copper metal onto a cathode. To deposit \\(0.635 \\text{ g}\\) of \\(\\text{Cu(s)}\\) in \\(965 \\text{ s}\\), what constant electrical current, in amperes, must be passed through the cell? (Faraday’s constant = \\(96,500 \\text{ C/mol } e^-\\); molar mass of \\(\\text{Cu} = 63.5 \\text{ g/mol}\\))"
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url: "https://nerd-notes.com/ubq/119300/"
date_modified: "2026-08-19T12:39:42+00:00"
---

# A student electrolyzes an aqueous solution of \(\text{CuSO}_4\text{(aq)}\) to deposit copper metal onto a cathode. To deposit \(0.635 \text{ g}\) of \(\text{Cu(s)}\) in \(965 \text{ s}\), what constant electrical current, in amperes, must be passed through the cell? (Faraday’s constant = \(96,500 \text{ C/mol } e^-\); molar mass of \(\text{Cu} = 63.5 \text{ g/mol}\))

A student electrolyzes an aqueous solution of \(\text{CuSO}_4\text{(aq)}\) to deposit copper metal onto a cathode. To deposit \(0.635 \text{ g}\) of \(\text{Cu(s)}\) in \(965 \text{ s}\), what constant electrical current, in amperes, must be passed through the cell? (Faraday's constant = \(96,500 \text{ C/mol } e^-\); molar mass of \(\text{Cu} = 63.5 \text{ g/mol}\))

- **A.** 0.500 A
- **B.** 1.00 A
- **C.** 2.00 A
- **D.** 4.00 A

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119300/*