The rate constant of a chemical reaction increased from 0.100 s to 3.20 s upon raising the temperature from 25.0 °C to 47.0 °C. Learning Goal: 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 Part A k = Ae-E/RT where k is the rate constant, A is the frequency factor, E, 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: Calculate the value of + -*) where Ti is the initial temperature and T, is the final temperature. Express your answer numerically. Ia (:)- (*)(* - *) E. V AEO R ? where ki is the rate constant at temperature T1, and kz is the rate constant at temperature T K- Part B Calculate the value of In | 1 where ki and kz correspond to the rate constants at the initial and the final temperatures as defined in part A. Express your answer numerically. Πν ΑΣφ. ? In Part C What is the activation energy of the reaction? Express your answer numerically in kilojoules per mole. ? E, = kJ/mol Submit Request Answer
The rate constant of a chemical reaction increased from 0.100 s to 3.20 s upon raising the temperature from 25.0 °C to 47.0 °C. Learning Goal: 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 Part A k = Ae-E/RT where k is the rate constant, A is the frequency factor, E, 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: Calculate the value of + -*) where Ti is the initial temperature and T, is the final temperature. Express your answer numerically. Ia (:)- (*)(* - *) E. V AEO R ? where ki is the rate constant at temperature T1, and kz is the rate constant at temperature T K- Part B Calculate the value of In | 1 where ki and kz correspond to the rate constants at the initial and the final temperatures as defined in part A. Express your answer numerically. Πν ΑΣφ. ? In Part C What is the activation energy of the reaction? Express your answer numerically in kilojoules per mole. ? E, = kJ/mol Submit Request Answer
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 of a chemical reaction increased from 0.100 s
-1
to 3.20 s
-1
upon raising the temperature from 25.0 ° C to 47.0 °C.
Learning Goal:
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
Part A
k = Ae-E/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:
1
Calculate the value of
T2
E where T is the initial temperature and T, is the final temperature.
Express your answer numerically.
m (:) - (*)(* - *)
k1
In
k2
Ea
R
T2
画]?
where ki is the rate constant at temperature T1 , and k2 is the rate constant at
temperature T2.
(*-+)-
1
K-1
%3D
T2
T1
Part B
ki
where ki and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.
k2
Calculate the value of ln
Express your answer numerically.
?
a (#) [
ki
In
k2
Part C
What is the activation energy of the reaction?
Express your answer numerically in kilojoules per mole.
ΑΣφ
圈]?
Ea =
kJ/mol
Submit
Request Answer](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4326a4d2-65b4-45a2-98ce-b76c49527a93%2Fdea07c19-c366-4c29-855c-57a70db4e0c6%2Fvism27h_processed.png&w=3840&q=75)
Transcribed Image Text:The rate constant of a chemical reaction increased from 0.100 s
-1
to 3.20 s
-1
upon raising the temperature from 25.0 ° C to 47.0 °C.
Learning Goal:
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
Part A
k = Ae-E/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:
1
Calculate the value of
T2
E where T is the initial temperature and T, is the final temperature.
Express your answer numerically.
m (:) - (*)(* - *)
k1
In
k2
Ea
R
T2
画]?
where ki is the rate constant at temperature T1 , and k2 is the rate constant at
temperature T2.
(*-+)-
1
K-1
%3D
T2
T1
Part B
ki
where ki and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.
k2
Calculate the value of ln
Express your answer numerically.
?
a (#) [
ki
In
k2
Part C
What is the activation energy of the reaction?
Express your answer numerically in kilojoules per mole.
ΑΣφ
圈]?
Ea =
kJ/mol
Submit
Request Answer
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