---
title: "In an electroplating experiment, a constant current of \\(9.65\\text{ A}\\) is passed through an electrolytic cell containing an aqueous \\(\\text{CuSO}_4\\) solution for \\(1000\\text{ s}\\). Assuming that all the current is used in the reduction of \\(\\text{Cu}^{2+}\\text{(aq)}\\) to deposit \\(\\text{Cu(s)}\\) on the cathode, what is the mass of copper deposited?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/119919/"
date_modified: "2026-08-21T08:18:08+00:00"
---

# In an electroplating experiment, a constant current of \(9.65\text{ A}\) is passed through an electrolytic cell containing an aqueous \(\text{CuSO}_4\) solution for \(1000\text{ s}\). Assuming that all the current is used in the reduction of \(\text{Cu}^{2+}\text{(aq)}\) to deposit \(\text{Cu(s)}\) on the cathode, what is the mass of copper deposited?

In an electroplating experiment, a constant current of \(9.65\text{ A}\) is passed through an electrolytic cell containing an aqueous \(\text{CuSO}_4\) solution for \(1000\text{ s}\). Assuming that all the current is used in the reduction of \(\text{Cu}^{2+}\text{(aq)}\) to deposit \(\text{Cu(s)}\) on the cathode, what is the mass of copper deposited?

- **A.** \(3.18\text{ g}\)
- **B.** \(6.36\text{ g}\)
- **C.** \(12.7\text{ g}\)
- **D.** \(63.6\text{ g}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119919/*