---
title: "An electrolytic cell is operated at a constant current of \\(1.93\\text{ A}\\) to electrolyze water. The oxidation half-reaction occurring at the anode is shown below.  \\[ 2\\text{H}_2\\text{O}(l) \\rightarrow \\text{O}_2(g) + 4\\text{H}^+(aq) + 4e^- \\]  Assuming the oxygen gas behaves ideally, how many minutes of electrolysis are required to produce \\(67.2\\text{ mL}\\) of \\(\\text{O}_2(g)\\) at standard temperature and pressure (STP)? (Assume that \\(1\\text{ mol}\\) of gas occupies \\(22.4\\text{ L}\\) at STP and \\(1\\text{ F} = 96{,}500\\text{ C/mol } e^-\\).)"
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url: "https://nerd-notes.com/ubq/120355/"
date_modified: "2026-08-23T04:23:21+00:00"
---

# An electrolytic cell is operated at a constant current of \(1.93\text{ A}\) to electrolyze water. The oxidation half-reaction occurring at the anode is shown below.

\[ 2\text{H}_2\text{O}(l) \rightarrow \text{O}_2(g) + 4\text{H}^+(aq) + 4e^- \]

Assuming the oxygen gas behaves ideally, how many minutes of electrolysis are required to produce \(67.2\text{ mL}\) of \(\text{O}_2(g)\) at standard temperature and pressure (STP)? (Assume that \(1\text{ mol}\) of gas occupies \(22.4\text{ L}\) at STP and \(1\text{ F} = 96{,}500\text{ C/mol } e^-\).)

An electrolytic cell is operated at a constant current of \(1.93\text{ A}\) to electrolyze water. The oxidation half-reaction occurring at the anode is shown below.

\[ 2\text{H}_2\text{O}(l) \rightarrow \text{O}_2(g) + 4\text{H}^+(aq) + 4e^- \]

Assuming the oxygen gas behaves ideally, how many minutes of electrolysis are required to produce \(67.2\text{ mL}\) of \(\text{O}_2(g)\) at standard temperature and pressure (STP)? (Assume that \(1\text{ mol}\) of gas occupies \(22.4\text{ L}\) at STP and \(1\text{ F} = 96{,}500\text{ C/mol } e^-\).)

- **A.** \(10.0\text{ min}\)
- **B.** \(20.0\text{ min}\)
- **C.** \(40.0\text{ min}\)
- **D.** \(600\text{ min}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120355/*