To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation k=Ae−Ea/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K⋅mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: ln(k2k1)=(EaR)(1T1−1T2) where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2. The rate constant of a chemical reaction increased from 0.200 s−1 to 2.80 s−1 upon raising the temperature from 26.0 ∘C to 52.0 ∘C . Calculate the value of (1T1−1T2) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.
To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation k=Ae−Ea/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K⋅mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: ln(k2k1)=(EaR)(1T1−1T2) where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2. The rate constant of a chemical reaction increased from 0.200 s−1 to 2.80 s−1 upon raising the temperature from 26.0 ∘C to 52.0 ∘C . Calculate the value of (1T1−1T2) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 69AP
Related questions
Question
To use the Arrhenius equation to calculate the activation energy.
As temperature rises, the average kinetic energy of molecules increases. In a
k=Ae−Ea/RT
where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K⋅mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful:
ln(k2k1)=(EaR)(1T1−1T2)
where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2.
The rate constant of a chemical reaction increased from 0.200 s−1 to 2.80 s−1 upon raising the temperature from 26.0 ∘C to 52.0 ∘C .
Calculate the value of (1T1−1T2) where T1 is the initial temperature and T2 is the final temperature.
Express your answer numerically.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 3 images
Knowledge Booster
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.Recommended textbooks for you
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:
9780078746376
Author:
Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:
Glencoe/McGraw-Hill School Pub Co