---
title: "In the atmosphere, nitrogen monoxide reacts with ozone according to the following elementary process:  \\[ \\text{NO}(g) + \\text{O}_3(g) \\rightarrow \\text{NO}_2(g) + \\text{O}_2(g) \\]  Because the reaction proceeds via a single bimolecular collision, the rate of successful collisions is directly proportional to the concentration of each reactant. Which of the following is the rate law for this elementary reaction?"
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url: "https://nerd-notes.com/ubq/119642/"
date_modified: "2026-08-21T08:11:54+00:00"
---

# In the atmosphere, nitrogen monoxide reacts with ozone according to the following elementary process:

\[ \text{NO}(g) + \text{O}_3(g) \rightarrow \text{NO}_2(g) + \text{O}_2(g) \]

Because the reaction proceeds via a single bimolecular collision, the rate of successful collisions is directly proportional to the concentration of each reactant. Which of the following is the rate law for this elementary reaction?

In the atmosphere, nitrogen monoxide reacts with ozone according to the following elementary process:

\[ \text{NO}(g) + \text{O}_3(g) \rightarrow \text{NO}_2(g) + \text{O}_2(g) \]

Because the reaction proceeds via a single bimolecular collision, the rate of successful collisions is directly proportional to the concentration of each reactant. Which of the following is the rate law for this elementary reaction?

- **A.** \(\text{Rate} = k[\text{NO}]\)
- **B.** \(\text{Rate} = k[\text{NO}]^2[\text{O}_3]\)
- **C.** \(\text{Rate} = k\dfrac{[\text{NO}_2][\text{O}_2]}{[\text{NO}][\text{O}_3]}\)
- **D.** \(\text{Rate} = k[\text{NO}][\text{O}_3]\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119642/*