What is the overall order of the following reaction, given the rate law? NO(3) + O3ls) → NO23) + O23) Rate = k[NO|[03) O 15 order O 3rd order O 1st order Oth order O 2nd order

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Need help it’s not zero order
### Determining the Overall Order of a Reaction

**Question:**

What is the overall order of the following reaction, given the rate law?

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

\[ \text{Rate} = k[\text{NO}][\text{O}_3] \]

**Options:**
1. \( \frac{1}{2} \) order
2. 3rd order
3. 1st order
4. 0th order
5. 2nd order

**Explanation:**

To determine the overall order of a reaction, we sum the exponents of the concentration terms in the rate law. 

From the given rate law:

\[ \text{Rate} = k[\text{NO}][\text{O}_3] \]

The exponent of \([\text{NO}]\) is 1 and the exponent of \([\text{O}_3]\) is also 1. 

Therefore, the overall order of the reaction is:

\[ 1 + 1 = 2 \]

**Correct Answer:**
- 2nd order
Transcribed Image Text:### Determining the Overall Order of a Reaction **Question:** What is the overall order of the following reaction, given the rate law? \[ \text{NO}(g) + \text{O}_3(g) \rightarrow \text{NO}_2(g) + \text{O}_2(g) \] \[ \text{Rate} = k[\text{NO}][\text{O}_3] \] **Options:** 1. \( \frac{1}{2} \) order 2. 3rd order 3. 1st order 4. 0th order 5. 2nd order **Explanation:** To determine the overall order of a reaction, we sum the exponents of the concentration terms in the rate law. From the given rate law: \[ \text{Rate} = k[\text{NO}][\text{O}_3] \] The exponent of \([\text{NO}]\) is 1 and the exponent of \([\text{O}_3]\) is also 1. Therefore, the overall order of the reaction is: \[ 1 + 1 = 2 \] **Correct Answer:** - 2nd order
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