If the reaction proceeds at second order kinetics and has half-life of 100.0 seconds. If the reaction is carried out at some temperature, and the initial concentration of NO₂ is 1.225 M, what is the rate constant for the reaction? What will the NO₂ concentration be after 35.4 s? At 175 s? At 865 s?
If the reaction proceeds at second order kinetics and has half-life of 100.0 seconds. If the reaction is carried out at some temperature, and the initial concentration of NO₂ is 1.225 M, what is the rate constant for the reaction? What will the NO₂ concentration be after 35.4 s? At 175 s? At 865 s?
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
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Transcribed Image Text:A substance decays with second order kinetics. What is the half-life given a rate constant that is 0.37 M⁻¹ s⁻¹ and an initial concentration of 0.75 M? How much of the substance remains after 13.9 seconds? After 55.2 seconds?
(Note: Any scribbled out section seems to be irrelevant to the core text.)
![**Problem Statement:**
If the reaction proceeds at second-order kinetics and has a half-life of 100.0 seconds, what is the rate constant for the reaction when the initial concentration of NO₂ is 1.225 M? Additionally, what will the NO₂ concentration be after:
- 35.4 seconds?
- 175 seconds?
- 865 seconds?
**Solution Explanation:**
1. **Rate Constant Calculation:**
For a second-order reaction, the relationship between half-life (\( t_{1/2} \)) and the rate constant (\( k \)) is given by the equation:
\[
t_{1/2} = \frac{1}{k \cdot [A]_0}
\]
Where \( [A]_0 \) is the initial concentration.
2. **Concentration Over Time:**
The concentration at any time \( t \) for a second-order reaction can be determined using:
\[
\frac{1}{[A]} = \frac{1}{[A]_0} + k \cdot t
\]
Apply this formula to find the concentration at each specified time.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe8e7ecd1-00b2-4f87-97f4-1e990180b5ce%2F4ba25a70-dd29-46ae-96f1-1c69b32ba758%2Fdaqmf4q_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
If the reaction proceeds at second-order kinetics and has a half-life of 100.0 seconds, what is the rate constant for the reaction when the initial concentration of NO₂ is 1.225 M? Additionally, what will the NO₂ concentration be after:
- 35.4 seconds?
- 175 seconds?
- 865 seconds?
**Solution Explanation:**
1. **Rate Constant Calculation:**
For a second-order reaction, the relationship between half-life (\( t_{1/2} \)) and the rate constant (\( k \)) is given by the equation:
\[
t_{1/2} = \frac{1}{k \cdot [A]_0}
\]
Where \( [A]_0 \) is the initial concentration.
2. **Concentration Over Time:**
The concentration at any time \( t \) for a second-order reaction can be determined using:
\[
\frac{1}{[A]} = \frac{1}{[A]_0} + k \cdot t
\]
Apply this formula to find the concentration at each specified time.
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