The reaction of nitrogen monoxide with ozone at 25 °C NO+O3 → NO2 + O2 is first order in NO and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.

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**Title: Reaction of Nitrogen Monoxide with Ozone at 25 °C**

**Reaction:**
\[ \text{NO} + \text{O}_3 \rightarrow \text{NO}_2 + \text{O}_2 \]

This reaction is first order in NO and second order overall.

**Task:**
Complete the rate law for this reaction.

**Instructions:**
Use the form \( k[\text{A}]^m [\text{B}]^n \), where '1' is assumed for \( m \) or \( n \) if applicable. Any concentration raised to the zero power does not appear in the expression. Do not input 1 for \( m \) or \( n \).

**Rate Law:**

\[ \text{Rate} = \boxed{} \]

The rate law should reflect the first order dependence on NO and the overall reaction order of two.
Transcribed Image Text:**Title: Reaction of Nitrogen Monoxide with Ozone at 25 °C** **Reaction:** \[ \text{NO} + \text{O}_3 \rightarrow \text{NO}_2 + \text{O}_2 \] This reaction is first order in NO and second order overall. **Task:** Complete the rate law for this reaction. **Instructions:** Use the form \( k[\text{A}]^m [\text{B}]^n \), where '1' is assumed for \( m \) or \( n \) if applicable. Any concentration raised to the zero power does not appear in the expression. Do not input 1 for \( m \) or \( n \). **Rate Law:** \[ \text{Rate} = \boxed{} \] The rate law should reflect the first order dependence on NO and the overall reaction order of two.
Expert Solution
Step 1: Rate law

The relation between the concentration of the reactants and the rate of reaction is expressed by the rate law. The given reaction is as follows:

table row cell NO space plus space straight O subscript 3 space end cell rightwards arrow cell NO subscript 2 space plus space straight O subscript 2 end cell end table

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