The rate constant k for a certain reaction is measured at two different temperatures: temperature k 309.0 °C 8.2 x 10° 223.0 °C 6.7x 10% Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ x10 E %3D mol
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 309.0 °C 8.2 x 10° 223.0 °C 6.7x 10% Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ x10 E %3D mol
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 23P
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![The rate constant k for a certain reaction is measured at two different temperatures:
temperature
k
309.0 °C
8.2 x 10°
223.0 °C
6.7 x 108
Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction.
Round your answer to 2 significant digits.
kJ
E =
Ox10
a
mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe361a5c2-e3a6-4cd8-bee8-5dcb720cb10b%2F20963dcf-ebdf-4c20-8af7-3452ead6f1c5%2Fnu1rrkl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The rate constant k for a certain reaction is measured at two different temperatures:
temperature
k
309.0 °C
8.2 x 10°
223.0 °C
6.7 x 108
Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction.
Round your answer to 2 significant digits.
kJ
E =
Ox10
a
mol
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