What is the value of the rate law constant for the reaction shown below? 1. -1.9 x 10^4 2. +1.9 x 10^4 3. -5.2 x 10^-5 4. +5.2 x 10^-5 5. +6.2
What is the value of the rate law constant for the reaction shown below? 1. -1.9 x 10^4 2. +1.9 x 10^4 3. -5.2 x 10^-5 4. +5.2 x 10^-5 5. +6.2
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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What is the value of the rate law constant for the reaction shown below?
1. -1.9 x 10^4
2. +1.9 x 10^4
3. -5.2 x 10^-5
4. +5.2 x 10^-5
5. +6.2
![**Isomerization of Methylisonitrile (CH3NC) to Acetonitrile (CH3CN)**
**Reaction Overview:**
At elevated temperatures, methylisonitrile (CH3NC) undergoes isomerization to form acetonitrile (CH3CN). The chemical equation representing this reaction is:
\[ \text{CH}_3\text{NC (g)} \rightarrow \text{CH}_3\text{CN (g)} \]
**Kinetics of the Reaction:**
The isomerization reaction is first-order with respect to methylisonitrile. Experimental data for this reaction at a temperature of 198.9 °C is presented in the following graph.
**Graph Interpretation:**
*Graph Details:*
- The graph plots the natural logarithm of the pressure of CH3NC (in units of pressure) on the y-axis against time (in seconds) on the x-axis.
- The y-axis is labeled as "ln pressure, CH3NC" and ranges from 3.4 to 5.2.
- The x-axis is labeled as "Time (s)" and ranges from 0 to 30,000 seconds.
*Data Points and Observations:*
- The graph shows a linear decrease in the natural logarithm of the pressure of CH3NC over time, indicating a first-order reaction.
- This linearity confirms that the reaction follows first-order kinetics, as the natural logarithm of the concentration of a reactant in a first-order reaction decreases linearly with time.
Understanding the First-Order Reaction:
- In a first-order reaction, the rate of reaction is directly proportional to the concentration of one reactant.
- The slope of the linear plot corresponds to the negative rate constant for the reaction (k).
This information is crucial for those studying chemical kinetics as it provides a clear example of how first-order reactions behave and how their data can be represented and analyzed graphically.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8466b748-e672-4c61-893b-8156cddfafb1%2Fa356a92e-248d-4be8-aef1-e6b0ff2a2d88%2Fikzrtsk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Isomerization of Methylisonitrile (CH3NC) to Acetonitrile (CH3CN)**
**Reaction Overview:**
At elevated temperatures, methylisonitrile (CH3NC) undergoes isomerization to form acetonitrile (CH3CN). The chemical equation representing this reaction is:
\[ \text{CH}_3\text{NC (g)} \rightarrow \text{CH}_3\text{CN (g)} \]
**Kinetics of the Reaction:**
The isomerization reaction is first-order with respect to methylisonitrile. Experimental data for this reaction at a temperature of 198.9 °C is presented in the following graph.
**Graph Interpretation:**
*Graph Details:*
- The graph plots the natural logarithm of the pressure of CH3NC (in units of pressure) on the y-axis against time (in seconds) on the x-axis.
- The y-axis is labeled as "ln pressure, CH3NC" and ranges from 3.4 to 5.2.
- The x-axis is labeled as "Time (s)" and ranges from 0 to 30,000 seconds.
*Data Points and Observations:*
- The graph shows a linear decrease in the natural logarithm of the pressure of CH3NC over time, indicating a first-order reaction.
- This linearity confirms that the reaction follows first-order kinetics, as the natural logarithm of the concentration of a reactant in a first-order reaction decreases linearly with time.
Understanding the First-Order Reaction:
- In a first-order reaction, the rate of reaction is directly proportional to the concentration of one reactant.
- The slope of the linear plot corresponds to the negative rate constant for the reaction (k).
This information is crucial for those studying chemical kinetics as it provides a clear example of how first-order reactions behave and how their data can be represented and analyzed graphically.
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