The rate constant k for a certain reaction is measured at two different temperatures: temperature k 311.0 °C 1.3 x 10¹1 421.0 °C 1.6 x 1011 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ 0 E = 0 mol x10 Xx
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 311.0 °C 1.3 x 10¹1 421.0 °C 1.6 x 1011 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ 0 E = 0 mol x10 Xx
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
311.0 °C
1.3 x 10¹1
421.0 °C
1.6 x 1011
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 =
x10
mol
X
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe361a5c2-e3a6-4cd8-bee8-5dcb720cb10b%2F4914f488-d04b-498d-b363-44edc46c4387%2F4iq3ls_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
311.0 °C
1.3 x 10¹1
421.0 °C
1.6 x 1011
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 =
x10
mol
X
?
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