**Reaction Order and Rate Constant Calculation** **Multiple Choice Options:** - **c.** The reaction is second order, and k is \(2.75 \times 10^{-3} \, \text{l/Ms}\). - **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\). - **e.** The reaction is first order, and k is \(-2.75 \times 10^{-3} \, \text{s}^{-1}\). **Selected Option:** - **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\). **Problem Description:** A **first order** reaction (\(A \rightarrow B\)) starts with an initial concentration \([A]_0 = 0.400 \, \text{M}\). After 2.25 seconds, the concentration \([A]\) is measured to be 0.060 M. Calculate the rate constant for the reaction. The answer should be in \(\text{s}^{-1}\) with three significant figures. **Provided Answer:** - **6.29** --- To solve this problem, one would typically use the first order reaction formula: \[ \ln\left(\frac{[A]_0}{[A]}\right) = kt \] Plugging in the values: - \([A]_0 = 0.400 \, \text{M}\) - \([A] = 0.060 \, \text{M}\) - \(t = 2.25 \, \text{s}\) The rate constant, \(k\), can be calculated as follows: \[ k = \frac{\ln\left(\frac{0.400}{0.060}\right)}{2.25} \] This calculation yields a rate constant, \(k\), consistent with the values expected of a correctly computed first order reaction rate constant.
**Reaction Order and Rate Constant Calculation** **Multiple Choice Options:** - **c.** The reaction is second order, and k is \(2.75 \times 10^{-3} \, \text{l/Ms}\). - **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\). - **e.** The reaction is first order, and k is \(-2.75 \times 10^{-3} \, \text{s}^{-1}\). **Selected Option:** - **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\). **Problem Description:** A **first order** reaction (\(A \rightarrow B\)) starts with an initial concentration \([A]_0 = 0.400 \, \text{M}\). After 2.25 seconds, the concentration \([A]\) is measured to be 0.060 M. Calculate the rate constant for the reaction. The answer should be in \(\text{s}^{-1}\) with three significant figures. **Provided Answer:** - **6.29** --- To solve this problem, one would typically use the first order reaction formula: \[ \ln\left(\frac{[A]_0}{[A]}\right) = kt \] Plugging in the values: - \([A]_0 = 0.400 \, \text{M}\) - \([A] = 0.060 \, \text{M}\) - \(t = 2.25 \, \text{s}\) The rate constant, \(k\), can be calculated as follows: \[ k = \frac{\ln\left(\frac{0.400}{0.060}\right)}{2.25} \] This calculation yields a rate constant, \(k\), consistent with the values expected of a correctly computed first order reaction rate constant.
Chemistry
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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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![**Reaction Order and Rate Constant Calculation**
**Multiple Choice Options:**
- **c.** The reaction is second order, and k is \(2.75 \times 10^{-3} \, \text{l/Ms}\).
- **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\).
- **e.** The reaction is first order, and k is \(-2.75 \times 10^{-3} \, \text{s}^{-1}\).
**Selected Option:**
- **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\).
**Problem Description:**
A **first order** reaction (\(A \rightarrow B\)) starts with an initial concentration \([A]_0 = 0.400 \, \text{M}\). After 2.25 seconds, the concentration \([A]\) is measured to be 0.060 M. Calculate the rate constant for the reaction. The answer should be in \(\text{s}^{-1}\) with three significant figures.
**Provided Answer:**
- **6.29**
---
To solve this problem, one would typically use the first order reaction formula:
\[ \ln\left(\frac{[A]_0}{[A]}\right) = kt \]
Plugging in the values:
- \([A]_0 = 0.400 \, \text{M}\)
- \([A] = 0.060 \, \text{M}\)
- \(t = 2.25 \, \text{s}\)
The rate constant, \(k\), can be calculated as follows:
\[ k = \frac{\ln\left(\frac{0.400}{0.060}\right)}{2.25} \]
This calculation yields a rate constant, \(k\), consistent with the values expected of a correctly computed first order reaction rate constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F83487220-e3b7-46aa-96f9-171ca8a3e4b1%2F83b99a55-0b4a-41d4-85ef-91d3472dbbdd%2Fn043rwi_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Reaction Order and Rate Constant Calculation**
**Multiple Choice Options:**
- **c.** The reaction is second order, and k is \(2.75 \times 10^{-3} \, \text{l/Ms}\).
- **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\).
- **e.** The reaction is first order, and k is \(-2.75 \times 10^{-3} \, \text{s}^{-1}\).
**Selected Option:**
- **d.** The reaction is first order, and k is \(2.75 \times 10^{-3} \, \text{s}^{-1}\).
**Problem Description:**
A **first order** reaction (\(A \rightarrow B\)) starts with an initial concentration \([A]_0 = 0.400 \, \text{M}\). After 2.25 seconds, the concentration \([A]\) is measured to be 0.060 M. Calculate the rate constant for the reaction. The answer should be in \(\text{s}^{-1}\) with three significant figures.
**Provided Answer:**
- **6.29**
---
To solve this problem, one would typically use the first order reaction formula:
\[ \ln\left(\frac{[A]_0}{[A]}\right) = kt \]
Plugging in the values:
- \([A]_0 = 0.400 \, \text{M}\)
- \([A] = 0.060 \, \text{M}\)
- \(t = 2.25 \, \text{s}\)
The rate constant, \(k\), can be calculated as follows:
\[ k = \frac{\ln\left(\frac{0.400}{0.060}\right)}{2.25} \]
This calculation yields a rate constant, \(k\), consistent with the values expected of a correctly computed first order reaction rate constant.
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