Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Calculating the Rate Constant of a Reaction**
In order to calculate the rate constant (\( k \)) for a reaction, follow the given parameters:
- **Given Parameters:**
- Concentration of reactant (\([X]\)) = 0.27 M (molarity)
- Rate of the reaction = 0.0050 M/s (molarity per second)
The task involves calculating the value of \( k \) using the given data.
**Equation to Use:**
The rate law for a reaction of the form \(\text{Rate} = k[X]\) can be rearranged to solve for \( k \):
\[ k = \frac{\text{Rate}}{[X]} \]
Where:
- Rate = 0.0050 M/s
- \([X]\) = 0.27 M
Using these values, you can calculate \( k \):
\[ k = \frac{0.0050 \, \text{M/s}}{0.27 \, \text{M}} \]
Make sure to plug in the values correctly and perform the arithmetic to find the value of \( k \).
**Graphical Section:**
There is also a space provided for entering the rate constant value ( \( k \)) and its units. Here is a detailed view of the provided space:
- **Entry Box for \( k \):**
- A box labeled 'k =' where you should enter the calculated value of the rate constant.
- **Units:**
- A field to enter the units of \( k \) which is \( \text{M}^{-1} \text{s}^{-1} \).
Additionally, there is an input tool labeled 'TOOLS' right beneath the rate constant entry box that helps to input scientific values, providing the notation \( \times 10^x \) for easier data entry representation for any scientific calculations.
Follow the steps and perform the required calculations to determine the rate constant accurately.](https://content.bartleby.com/qna-images/question/58420377-1b68-412b-9b13-d1652dd3ab6a/cc65fba3-b009-481b-b090-a56ad4d9289a/3deer3yh_processed.jpeg)
Transcribed Image Text:**Calculating the Rate Constant of a Reaction**
In order to calculate the rate constant (\( k \)) for a reaction, follow the given parameters:
- **Given Parameters:**
- Concentration of reactant (\([X]\)) = 0.27 M (molarity)
- Rate of the reaction = 0.0050 M/s (molarity per second)
The task involves calculating the value of \( k \) using the given data.
**Equation to Use:**
The rate law for a reaction of the form \(\text{Rate} = k[X]\) can be rearranged to solve for \( k \):
\[ k = \frac{\text{Rate}}{[X]} \]
Where:
- Rate = 0.0050 M/s
- \([X]\) = 0.27 M
Using these values, you can calculate \( k \):
\[ k = \frac{0.0050 \, \text{M/s}}{0.27 \, \text{M}} \]
Make sure to plug in the values correctly and perform the arithmetic to find the value of \( k \).
**Graphical Section:**
There is also a space provided for entering the rate constant value ( \( k \)) and its units. Here is a detailed view of the provided space:
- **Entry Box for \( k \):**
- A box labeled 'k =' where you should enter the calculated value of the rate constant.
- **Units:**
- A field to enter the units of \( k \) which is \( \text{M}^{-1} \text{s}^{-1} \).
Additionally, there is an input tool labeled 'TOOLS' right beneath the rate constant entry box that helps to input scientific values, providing the notation \( \times 10^x \) for easier data entry representation for any scientific calculations.
Follow the steps and perform the required calculations to determine the rate constant accurately.
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