Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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 for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.53PAE: Silicon forms a series of compounds analogous to the al-kanes and having the general formula...
See similar textbooks
icon
Related questions
Question

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.
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.
Expert Solution
steps

Step by step

Solved in 2 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Rate Laws
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning
Physical Chemistry
Physical Chemistry
Chemistry
ISBN:
9781133958437
Author:
Ball, David W. (david Warren), BAER, Tomas
Publisher:
Wadsworth Cengage Learning,
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS