---
title: "A student constructs an electrolytic cell to plate pure copper onto an electrode. The cell contains an aqueous solution of \\(\\text{CuSO}_4\\) and is operated at a constant current of \\(9.65\\text{ A}\\) for \\(10.0\\text{ minutes}\\). The reduction half-reaction at the cathode is  \\[\\text{Cu}^{2+}\\text{(aq)} + 2\\,e^- \\rightarrow \\text{Cu(s)}\\]  Assuming \\(100\\%\\) current efficiency, what mass of \\(\\text{Cu(s)}\\) is deposited onto the cathode?"
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url: "https://nerd-notes.com/ubq/121440/"
date_modified: "2026-08-23T05:02:24+00:00"
---

# A student constructs an electrolytic cell to plate pure copper onto an electrode. The cell contains an aqueous solution of \(\text{CuSO}_4\) and is operated at a constant current of \(9.65\text{ A}\) for \(10.0\text{ minutes}\). The reduction half-reaction at the cathode is

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

Assuming \(100\%\) current efficiency, what mass of \(\text{Cu(s)}\) is deposited onto the cathode?

A student constructs an electrolytic cell to plate pure copper onto an electrode. The cell contains an aqueous solution of \(\text{CuSO}_4\) and is operated at a constant current of \(9.65\text{ A}\) for \(10.0\text{ minutes}\). The reduction half-reaction at the cathode is

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

Assuming \(100\%\) current efficiency, what mass of \(\text{Cu(s)}\) is deposited onto the cathode?

- **A.** \(0.0318\text{ g}\)
- **B.** \(0.191\text{ g}\)
- **C.** \(0.953\text{ g}\)
- **D.** \(1.91\text{ g}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121440/*