The following data were obtained for the reaction where the rate is the following: Rate=d[CIO₂2]/dt [CIO₂] [OH-]。 Initial Rate (mol/L) (mol/L) (mol L-¹ s-¹) 0.0540 0.108 6.21X10-2 0.108 0.108 2.48×10-1 0.108 0.0540 1.24X10-1 2 CIO₂(aq) + 2 OH (aq) → CIO3 (aq) + ClO₂ (aq) + H₂O(l)
The following data were obtained for the reaction where the rate is the following: Rate=d[CIO₂2]/dt [CIO₂] [OH-]。 Initial Rate (mol/L) (mol/L) (mol L-¹ s-¹) 0.0540 0.108 6.21X10-2 0.108 0.108 2.48×10-1 0.108 0.0540 1.24X10-1 2 CIO₂(aq) + 2 OH (aq) → CIO3 (aq) + ClO₂ (aq) + H₂O(l)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Chemical Kinetics: Determination of the Rate Law
#### Reaction Data
The following data were obtained for the reaction:
\[ 2 \text{ClO}_2(aq) + 2 \text{OH}^-(aq) \rightarrow \text{ClO}_3^-(aq) + \text{ClO}_2^-(aq) + \text{H}_2O(l) \]
where the rate is given by the following expression:
\[ \text{Rate} = -\frac{d[\text{ClO}_2]}{dt} \]
#### Experimental Data
| \([\text{ClO}_2]_0\) (mol/L) | \([\text{OH}^-]_0\) (mol/L) | Initial Rate (mol L\(^{-1}\) s\(^{-1}\)) |
|-----------------------------|-----------------------------|------------------------------------------|
| 0.0540 | 0.108 | 6.21 × 10\(^{-2}\) |
| 0.108 | 0.108 | 2.48 × 10\(^{-1}\) |
| 0.108 | 0.0540 | 1.24 × 10\(^{-1}\) |
#### Objective
Determine which of the following rate laws correctly describes the reaction rate:
1. \(\text{rate} = k[\text{ClO}_2][\text{OH}^-]\)
2. \(\text{rate} = k[\text{ClO}_2]^2[\text{OH}^-]\)
3. \(\text{rate} = k[\text{ClO}_2]^3[\text{OH}^-]\)
4. \(\text{rate} = k[\text{ClO}_2]^2[\text{OH}^-]^2\)
5. \(\text{rate} = k[\text{ClO}_2][\text{OH}^-]^2\)
By analyzing the given data, you are expected to identify the correct order of the reaction with respect to each reactant and thus determine the accurate rate law for the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbcb18ee9-04f5-44c4-b37d-c38609e517a7%2F79b33683-adf2-4063-a075-a64091fe04d3%2Fqqtmag5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Kinetics: Determination of the Rate Law
#### Reaction Data
The following data were obtained for the reaction:
\[ 2 \text{ClO}_2(aq) + 2 \text{OH}^-(aq) \rightarrow \text{ClO}_3^-(aq) + \text{ClO}_2^-(aq) + \text{H}_2O(l) \]
where the rate is given by the following expression:
\[ \text{Rate} = -\frac{d[\text{ClO}_2]}{dt} \]
#### Experimental Data
| \([\text{ClO}_2]_0\) (mol/L) | \([\text{OH}^-]_0\) (mol/L) | Initial Rate (mol L\(^{-1}\) s\(^{-1}\)) |
|-----------------------------|-----------------------------|------------------------------------------|
| 0.0540 | 0.108 | 6.21 × 10\(^{-2}\) |
| 0.108 | 0.108 | 2.48 × 10\(^{-1}\) |
| 0.108 | 0.0540 | 1.24 × 10\(^{-1}\) |
#### Objective
Determine which of the following rate laws correctly describes the reaction rate:
1. \(\text{rate} = k[\text{ClO}_2][\text{OH}^-]\)
2. \(\text{rate} = k[\text{ClO}_2]^2[\text{OH}^-]\)
3. \(\text{rate} = k[\text{ClO}_2]^3[\text{OH}^-]\)
4. \(\text{rate} = k[\text{ClO}_2]^2[\text{OH}^-]^2\)
5. \(\text{rate} = k[\text{ClO}_2][\text{OH}^-]^2\)
By analyzing the given data, you are expected to identify the correct order of the reaction with respect to each reactant and thus determine the accurate rate law for the reaction.
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