---
title: "The kinetics of the reaction between nitrogen monoxide gas and oxygen gas were investigated at \\(298\\text{ K}\\):  \\[2\\text{NO(g)} + \\text{O}_2\\text{(g)} \\rightarrow 2\\text{NO}_2\\text{(g)}\\]  Initial rate data were collected across three experimental trials and recorded in the table below.  | Trial | \\([\\text{NO}]_0\\text{ (M)}\\) | \\([\\text{O}_2]_0\\text{ (M)}\\) | Initial rate of reaction \\(\\text{(M}\\cdot\\text{s}^{-1}\\text{)}\\) | |—|—|—|—| | 1 | \\(0.10\\) | \\(0.10\\) | \\(2.0 \\times 10^{-3}\\) | | 2 | \\(0.20\\) | \\(0.10\\) | \\(8.0 \\times 10^{-3}\\) | | 3 | \\(0.30\\) | \\(0.20\\) | \\(3.6 \\times 10^{-2}\\) |  Based on the data in the table, which of the following is the correct rate law and specific rate constant, \\(k\\), for the reaction?"
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/121491/"
date_modified: "2026-08-23T05:04:49+00:00"
---

# The kinetics of the reaction between nitrogen monoxide gas and oxygen gas were investigated at \(298\text{ K}\):

\[2\text{NO(g)} + \text{O}_2\text{(g)} \rightarrow 2\text{NO}_2\text{(g)}\]

Initial rate data were collected across three experimental trials and recorded in the table below.

| Trial | \([\text{NO}]_0\text{ (M)}\) | \([\text{O}_2]_0\text{ (M)}\) | Initial rate of reaction \(\text{(M}\cdot\text{s}^{-1}\text{)}\) |
|—|—|—|—|
| 1 | \(0.10\) | \(0.10\) | \(2.0 \times 10^{-3}\) |
| 2 | \(0.20\) | \(0.10\) | \(8.0 \times 10^{-3}\) |
| 3 | \(0.30\) | \(0.20\) | \(3.6 \times 10^{-2}\) |

Based on the data in the table, which of the following is the correct rate law and specific rate constant, \(k\), for the reaction?

The kinetics of the reaction between nitrogen monoxide gas and oxygen gas were investigated at \(298\text{ K}\):

\[2\text{NO(g)} + \text{O}_2\text{(g)} \rightarrow 2\text{NO}_2\text{(g)}\]

Initial rate data were collected across three experimental trials and recorded in the table below.

| Trial | \([\text{NO}]_0\text{ (M)}\) | \([\text{O}_2]_0\text{ (M)}\) | Initial rate of reaction \(\text{(M}\cdot\text{s}^{-1}\text{)}\) |
|---|---|---|---|
| 1 | \(0.10\) | \(0.10\) | \(2.0 \times 10^{-3}\) |
| 2 | \(0.20\) | \(0.10\) | \(8.0 \times 10^{-3}\) |
| 3 | \(0.30\) | \(0.20\) | \(3.6 \times 10^{-2}\) |

Based on the data in the table, which of the following is the correct rate law and specific rate constant, \(k\), for the reaction?

- **A.** \(\text{Rate} = k[\text{NO}][\text{O}_2]\), with \(k = 0.20\text{ M}^{-1}\cdot\text{s}^{-1}\)
- **B.** \(\text{Rate} = k[\text{NO}][\text{O}_2]^2\), with \(k = 2.0\text{ M}^{-2}\cdot\text{s}^{-1}\)
- **C.** \(\text{Rate} = k[\text{NO}]^2[\text{O}_2]\), with \(k = 2.0\text{ M}^{-1}\cdot\text{s}^{-1}\)
- **D.** \(\text{Rate} = k[\text{NO}]^2[\text{O}_2]\), with \(k = 2.0\text{ M}^{-2}\cdot\text{s}^{-1}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121491/*