---
title: "The kinetics of the reaction between nitrogen monoxide gas and chlorine gas was investigated at \\(300\\text{ K}\\): \\[ 2\\text{NO}(g) + \\text{Cl}_2(g) \\rightarrow 2\\text{NOCl}(g) \\] The reaction was determined to obey the rate law \\(\\text{rate} = k[\\text{Cl}_2][\\text{NO}]^2\\), with a rate constant of \\(k = 3.0 \\times 10^2\\text{ M}^{-2}\\text{s}^{-1}\\) at this temperature. If an experiment is initiated with \\([\\text{Cl}_2] = 0.050\\text{ M}\\) and \\([\\text{NO}] = 0.040\\text{ M}\\), what is the initial rate of the reaction?"
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url: "https://nerd-notes.com/ubq/119958/"
date_modified: "2026-08-21T08:28:15+00:00"
---

# The kinetics of the reaction between nitrogen monoxide gas and chlorine gas was investigated at \(300\text{ K}\):
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
The reaction was determined to obey the rate law \(\text{rate} = k[\text{Cl}_2][\text{NO}]^2\), with a rate constant of \(k = 3.0 \times 10^2\text{ M}^{-2}\text{s}^{-1}\) at this temperature. If an experiment is initiated with \([\text{Cl}_2] = 0.050\text{ M}\) and \([\text{NO}] = 0.040\text{ M}\), what is the initial rate of the reaction?

The kinetics of the reaction between nitrogen monoxide gas and chlorine gas was investigated at \(300\text{ K}\):
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
The reaction was determined to obey the rate law \(\text{rate} = k[\text{Cl}_2][\text{NO}]^2\), with a rate constant of \(k = 3.0 \times 10^2\text{ M}^{-2}\text{s}^{-1}\) at this temperature. If an experiment is initiated with \([\text{Cl}_2] = 0.050\text{ M}\) and \([\text{NO}] = 0.040\text{ M}\), what is the initial rate of the reaction?

- **A.** \(2.4 \times 10^{-2}\text{ M s}^{-1}\)
- **B.** \(3.0 \times 10^{-2}\text{ M s}^{-1}\)
- **C.** \(9.6 \times 10^{-2}\text{ M s}^{-1}\)
- **D.** \(6.0 \times 10^{-1}\text{ M s}^{-1}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119958/*