The rate constant for this second-order reaction is 0.840 M-.s at 300 °C. A products How long, in seconds, would it take for the concentration of A to decrease from 0.630 M to 0.230 M?
The rate constant for this second-order reaction is 0.840 M-.s at 300 °C. A products How long, in seconds, would it take for the concentration of A to decrease from 0.630 M to 0.230 M?
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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![The rate constant for this second-order reaction is 0.840 M⁻¹ · s⁻¹ at 300 °C.
\[ \text{A} \rightarrow \text{products} \]
**Question:**
How long, in seconds, would it take for the concentration of A to decrease from 0.630 M to 0.230 M?
**Calculation:**
To solve for the time \( t \) for a second-order reaction, the integrated rate law for second-order reactions is used:
\[
t = \frac{1}{k} \left( \frac{1}{[A]_t} - \frac{1}{[A]_0} \right)
\]
Where:
- \( [A]_0 \) is the initial concentration (0.630 M),
- \( [A]_t \) is the concentration at time \( t \) (0.230 M),
- \( k \) is the rate constant (0.840 M⁻¹ · s⁻¹).
**Input Box:**
An input field is provided to calculate and input the value of time \( t \), in seconds.
**Tools:**
A button with "x10^7" located to the left of the input box, implying the provided time may need to be adjusted by a factor of 10^7.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F04d91ec5-5dc8-475a-a219-706d13e893d1%2F5c759ffb-36ba-439f-a152-45366c86da1a%2Fceo5ysyh.jpeg&w=3840&q=75)
Transcribed Image Text:The rate constant for this second-order reaction is 0.840 M⁻¹ · s⁻¹ at 300 °C.
\[ \text{A} \rightarrow \text{products} \]
**Question:**
How long, in seconds, would it take for the concentration of A to decrease from 0.630 M to 0.230 M?
**Calculation:**
To solve for the time \( t \) for a second-order reaction, the integrated rate law for second-order reactions is used:
\[
t = \frac{1}{k} \left( \frac{1}{[A]_t} - \frac{1}{[A]_0} \right)
\]
Where:
- \( [A]_0 \) is the initial concentration (0.630 M),
- \( [A]_t \) is the concentration at time \( t \) (0.230 M),
- \( k \) is the rate constant (0.840 M⁻¹ · s⁻¹).
**Input Box:**
An input field is provided to calculate and input the value of time \( t \), in seconds.
**Tools:**
A button with "x10^7" located to the left of the input box, implying the provided time may need to be adjusted by a factor of 10^7.
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