The following data were obtained for the reaction 2 CIO2(aq) + 2 OH (aq) → CIO3(aq) + ClO₂ (aq) + H₂O(l) [CIO₂]0 [OH-]o Initial Rate (mol/L) (mol/L) (mol L-¹ s-¹) 0.054 0.108 6.21X10-2 0.108 0.108 2.48X10-¹ 0.108 0.054 1.24X10-1 What is the numerical value for the rate constant?
The following data were obtained for the reaction 2 CIO2(aq) + 2 OH (aq) → CIO3(aq) + ClO₂ (aq) + H₂O(l) [CIO₂]0 [OH-]o Initial Rate (mol/L) (mol/L) (mol L-¹ s-¹) 0.054 0.108 6.21X10-2 0.108 0.108 2.48X10-¹ 0.108 0.054 1.24X10-1 What is the numerical value for the rate constant?
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![### Reaction Rate Data:
The following data were obtained for the reaction:
\[ 2 \text{ClO}_2(aq) + 2 \text{OH}^-(aq) \rightarrow \text{ClO}_3^-(aq) + \text{ClO}_2^-(aq) + \text{H}_2\text{O}(l) \]
#### Table of Initial Conditions and Rates:
The table below presents the initial concentrations of \(\text{ClO}_2\) and \(\text{OH}^-\) and their corresponding initial reaction rates:
| \([ \text{ClO}_2]_0\) (mol/L) | \([ \text{OH}^-]_0\) (mol/L) | Initial Rate (mol L\(^{-1}\) s\(^{-1}\)) |
|------------------------------|-----------------------------|-------------------------------------------|
| 0.054 | 0.108 | \(6.21 \times 10^{-2}\) |
| 0.108 | 0.108 | \(2.48 \times 10^{-1}\) |
| 0.108 | 0.054 | \(1.24 \times 10^{-1}\) |
#### Question:
- **What is the numerical value for the rate constant?**
### Explanation of the Data Table:
The table showcases three sets of experiments where different initial concentrations of \(\text{ClO}_2\) and \(\text{OH}^-\) were used to determine how these concentrations affect the initial rate of the reaction.
- **First row:** When \([ \text{ClO}_2]_0\) is 0.054 mol/L and \([ \text{OH}^-]_0\) is 0.108 mol/L, the initial reaction rate is \(6.21 \times 10^{-2}\) mol L\(^{-1}\) s\(^{-1}\).
- **Second row:** When \([ \text{ClO}_2]_0\) is 0.108 mol/L and \([ \text{OH}^-]_0\) remains at 0.108 mol/L, the initial reaction rate increases to \(2.48 \times 10^{-1}\) mol L\(^{-1}\) s\(^{-1}\).
- **Third row:** When](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbcb18ee9-04f5-44c4-b37d-c38609e517a7%2F3b880a04-fef2-49a5-beb3-636a005e6880%2F9a7jedc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Reaction Rate Data:
The following data were obtained for the reaction:
\[ 2 \text{ClO}_2(aq) + 2 \text{OH}^-(aq) \rightarrow \text{ClO}_3^-(aq) + \text{ClO}_2^-(aq) + \text{H}_2\text{O}(l) \]
#### Table of Initial Conditions and Rates:
The table below presents the initial concentrations of \(\text{ClO}_2\) and \(\text{OH}^-\) and their corresponding initial reaction rates:
| \([ \text{ClO}_2]_0\) (mol/L) | \([ \text{OH}^-]_0\) (mol/L) | Initial Rate (mol L\(^{-1}\) s\(^{-1}\)) |
|------------------------------|-----------------------------|-------------------------------------------|
| 0.054 | 0.108 | \(6.21 \times 10^{-2}\) |
| 0.108 | 0.108 | \(2.48 \times 10^{-1}\) |
| 0.108 | 0.054 | \(1.24 \times 10^{-1}\) |
#### Question:
- **What is the numerical value for the rate constant?**
### Explanation of the Data Table:
The table showcases three sets of experiments where different initial concentrations of \(\text{ClO}_2\) and \(\text{OH}^-\) were used to determine how these concentrations affect the initial rate of the reaction.
- **First row:** When \([ \text{ClO}_2]_0\) is 0.054 mol/L and \([ \text{OH}^-]_0\) is 0.108 mol/L, the initial reaction rate is \(6.21 \times 10^{-2}\) mol L\(^{-1}\) s\(^{-1}\).
- **Second row:** When \([ \text{ClO}_2]_0\) is 0.108 mol/L and \([ \text{OH}^-]_0\) remains at 0.108 mol/L, the initial reaction rate increases to \(2.48 \times 10^{-1}\) mol L\(^{-1}\) s\(^{-1}\).
- **Third row:** When
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