A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is 0.960 M, this same reactant decomposes with a half-life of 77.7 s. What is the order of the reaction? 0 1 2 What is the value and unit of the rate constant for this reaction? k = Unit:
A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is 0.960 M, this same reactant decomposes with a half-life of 77.7 s. What is the order of the reaction? 0 1 2 What is the value and unit of the rate constant for this reaction? k = Unit:
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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![**Problem Statement:**
A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is 0.960 M, this same reactant decomposes with a half-life of 77.7 s.
**Questions:**
1. What is the order of the reaction?
- 0
- 1
- 2
2. What is the value and unit of the rate constant for this reaction?
- \( k = \) [Text Box for Input]
- Unit: [Dropdown for Unit Selection]
**Explanation:**
This exercise involves determining the reaction order and rate constant based on provided half-life and concentration data. The change in half-life with changing concentration suggests the reaction order. By comparing the half-lives at different concentrations, the order affecting the decomposition rate can be determined, leading to calculations for the rate constant \( k \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fba6b20c3-fc3b-431b-838d-7e0f9d5cfa41%2F19ca88db-4490-49e0-8287-90494b59283a%2F4igl1kr_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is 0.960 M, this same reactant decomposes with a half-life of 77.7 s.
**Questions:**
1. What is the order of the reaction?
- 0
- 1
- 2
2. What is the value and unit of the rate constant for this reaction?
- \( k = \) [Text Box for Input]
- Unit: [Dropdown for Unit Selection]
**Explanation:**
This exercise involves determining the reaction order and rate constant based on provided half-life and concentration data. The change in half-life with changing concentration suggests the reaction order. By comparing the half-lives at different concentrations, the order affecting the decomposition rate can be determined, leading to calculations for the rate constant \( k \).
Expert Solution
Step 1
We have to find order of reaction .
Given initial concentrations
And half lifes .
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