---
title: "Hydrogen gas reacts with oxygen gas in a closed container at a constant temperature according to the balanced chemical equation below:  \\[ 2\\,\\text{H}_2(g) + \\text{O}_2(g) \\rightarrow 2\\,\\text{H}_2\\text{O}(g) \\]  If the rate of formation of \\(\\text{H}_2\\text{O}(g)\\) is \\(0.080\\text{ M}\\cdot\\text{s}^{-1}\\), what is the rate of disappearance of \\(\\text{O}_2(g)\\) under the same conditions?"
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url: "https://nerd-notes.com/ubq/119675/"
date_modified: "2026-08-21T08:12:01+00:00"
---

# Hydrogen gas reacts with oxygen gas in a closed container at a constant temperature according to the balanced chemical equation below:

\[ 2\,\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\,\text{H}_2\text{O}(g) \]

If the rate of formation of \(\text{H}_2\text{O}(g)\) is \(0.080\text{ M}\cdot\text{s}^{-1}\), what is the rate of disappearance of \(\text{O}_2(g)\) under the same conditions?

Hydrogen gas reacts with oxygen gas in a closed container at a constant temperature according to the balanced chemical equation below:

\[ 2\,\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\,\text{H}_2\text{O}(g) \]

If the rate of formation of \(\text{H}_2\text{O}(g)\) is \(0.080\text{ M}\cdot\text{s}^{-1}\), what is the rate of disappearance of \(\text{O}_2(g)\) under the same conditions?

- **A.** \(0.040\text{ M}\cdot\text{s}^{-1}\)
- **B.** \(0.080\text{ M}\cdot\text{s}^{-1}\)
- **C.** \(0.16\text{ M}\cdot\text{s}^{-1}\)
- **D.** \(0.32\text{ M}\cdot\text{s}^{-1}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119675/*