d. Il and III only 13. If the reaction 2A +B+C→2D+E is first order overall, which of these could be the units of its rate constant, k? 1/s a. b. Mls C. 1/Ms d. 1/Ms? e. Ms 14. In a first order reaction, the initial concentration of A is 0.40 M. What is the concentration of A after 15
d. Il and III only 13. If the reaction 2A +B+C→2D+E is first order overall, which of these could be the units of its rate constant, k? 1/s a. b. Mls C. 1/Ms d. 1/Ms? e. Ms 14. In a first order reaction, the initial concentration of A is 0.40 M. What is the concentration of A after 15
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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![**Educational Resource: Reaction Rate Constants**
**Question 13:**
"If the reaction 2A + B + C → 2D + E is first order overall, which of these could be the units of its rate constant, k?"
- a. \(1/\text{s}\)
- b. \(M/\text{s}\)
- c. \(1/Ms\)
- d. \(1/M^2s\)
- e. \(Ms\)
**Explanation:**
Each chemical reaction's rate law has a specific order and corresponding units for the rate constant, \(k\). For a first-order reaction, the overall order of the reaction is one. The units for the rate constant, \(k\), in a first-order reaction are typically \(s^{-1}\) (1/s).
To determine the correct units for \(k\), one must consider the general form of the rate law, which is rate = \(k[A]^m[B]^n\).... For a first-order reaction, the sum of the exponents (m, n, ...) in the rate law must equal 1.
For first-order reactions, the units of the rate are concentration/time (such as M/s).
So, if the reaction is first order overall, the units of its rate constant, \(k\), would be \(1/\text{s}\).
Therefore, the correct answer is:
- **a. \(1/\text{s}\)**
**Question 14:**
"In a first-order reaction, the initial concentration of A is 0.40 M. What is the concentration of A after 15 seconds if the half-life of the reaction is 81 seconds?"
To solve this problem, additional details such as the rate constant and further steps of the calculation might be presented in other parts of the educational material not included in this extract. Here, the purpose is to determine the remaining concentration of A after a given period, based on its half-life in a first-order reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc31825ca-e532-4346-8c67-c6f0bc8ad95c%2Fea26ad29-c865-452a-a4c1-85bef603c511%2Fvuxlgvb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Resource: Reaction Rate Constants**
**Question 13:**
"If the reaction 2A + B + C → 2D + E is first order overall, which of these could be the units of its rate constant, k?"
- a. \(1/\text{s}\)
- b. \(M/\text{s}\)
- c. \(1/Ms\)
- d. \(1/M^2s\)
- e. \(Ms\)
**Explanation:**
Each chemical reaction's rate law has a specific order and corresponding units for the rate constant, \(k\). For a first-order reaction, the overall order of the reaction is one. The units for the rate constant, \(k\), in a first-order reaction are typically \(s^{-1}\) (1/s).
To determine the correct units for \(k\), one must consider the general form of the rate law, which is rate = \(k[A]^m[B]^n\).... For a first-order reaction, the sum of the exponents (m, n, ...) in the rate law must equal 1.
For first-order reactions, the units of the rate are concentration/time (such as M/s).
So, if the reaction is first order overall, the units of its rate constant, \(k\), would be \(1/\text{s}\).
Therefore, the correct answer is:
- **a. \(1/\text{s}\)**
**Question 14:**
"In a first-order reaction, the initial concentration of A is 0.40 M. What is the concentration of A after 15 seconds if the half-life of the reaction is 81 seconds?"
To solve this problem, additional details such as the rate constant and further steps of the calculation might be presented in other parts of the educational material not included in this extract. Here, the purpose is to determine the remaining concentration of A after a given period, based on its half-life in a first-order reaction.
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