The following questions are based on the reaction and data below. Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution this reaction takes place: 2CIO 2(aq) + 20H (aq) ClIO 2 (aq) + CIO 3 (aq) + H2O(). Based on the following data, determine the rate law and the value of the rate constant. Initial Concentrations Initial Rate [CIO2] [OH] (M/s 0.060 0.030 0.0248 0.020 0.030 0.00276 0.020 0.090 0.00828 What is the order of the reaction with respect to CIO 2? Fourth order Zero order Second order First order
The following questions are based on the reaction and data below. Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution this reaction takes place: 2CIO 2(aq) + 20H (aq) ClIO 2 (aq) + CIO 3 (aq) + H2O(). Based on the following data, determine the rate law and the value of the rate constant. Initial Concentrations Initial Rate [CIO2] [OH] (M/s 0.060 0.030 0.0248 0.020 0.030 0.00276 0.020 0.090 0.00828 What is the order of the reaction with respect to CIO 2? Fourth order Zero order Second order First order
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Question 8**
The following questions are based on the reaction and data below.
Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution, this reaction takes place:
\[ 2 \text{ClO}_2 (\text{aq}) + 2 \text{OH}^- (\text{aq}) \rightarrow \text{ClO}_2^- (\text{aq}) + \text{ClO}_3^- (\text{aq}) + \text{H}_2\text{O}(\text{l}) \]
Based on the following data, determine the rate law and the value of the rate constant.
| Initial Concentrations | Initial Rate (M/s) |
|------------------------|--------------------|
| [ClO\(_2\)] = 0.060 M | [OH\(^-\)] = 0.030 M | 0.0248 |
| [ClO\(_2\)] = 0.020 M | [OH\(^-\)] = 0.030 M | 0.00276 |
| [ClO\(_2\)] = 0.020 M | [OH\(^-\)] = 0.090 M | 0.00828 |
What is the order of the reaction with respect to ClO\(_2\)?
- Fourth order
- Zero order
- Second order
- First order
---
**Explanation:**
To determine the reaction order with respect to each reactant, observe how changes in concentration affect the rate. For example:
- Compare experiments where only one reactant concentration changes while the other remains constant.
- Calculate the rate constant from the rate law once the orders are established.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F824fa1c6-40a3-49c1-bdd2-6faa45715099%2F2b17be01-5872-4df2-8b34-4e83962821d2%2Fkkrbcjg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 8**
The following questions are based on the reaction and data below.
Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution, this reaction takes place:
\[ 2 \text{ClO}_2 (\text{aq}) + 2 \text{OH}^- (\text{aq}) \rightarrow \text{ClO}_2^- (\text{aq}) + \text{ClO}_3^- (\text{aq}) + \text{H}_2\text{O}(\text{l}) \]
Based on the following data, determine the rate law and the value of the rate constant.
| Initial Concentrations | Initial Rate (M/s) |
|------------------------|--------------------|
| [ClO\(_2\)] = 0.060 M | [OH\(^-\)] = 0.030 M | 0.0248 |
| [ClO\(_2\)] = 0.020 M | [OH\(^-\)] = 0.030 M | 0.00276 |
| [ClO\(_2\)] = 0.020 M | [OH\(^-\)] = 0.090 M | 0.00828 |
What is the order of the reaction with respect to ClO\(_2\)?
- Fourth order
- Zero order
- Second order
- First order
---
**Explanation:**
To determine the reaction order with respect to each reactant, observe how changes in concentration affect the rate. For example:
- Compare experiments where only one reactant concentration changes while the other remains constant.
- Calculate the rate constant from the rate law once the orders are established.
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