The rate constant k for a certain reaction is measured at two different temperatures: temperature k 156.0 °C 7.6 × 1012 282.0 °C |5.7 × 1014 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E = a mol
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 156.0 °C 7.6 × 1012 282.0 °C |5.7 × 1014 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E = a mol
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 5QRT
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![The rate constant k for a certain reaction is measured at two different temperatures:
temperature
k
156.0 °C
7.6 x 1012
282.0 °C 5.7 × 1014
Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction.
a
Round your answer to 2 significant digits.
kJ
E =
x10
a
mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa63ba14e-5906-4aef-8a62-ee741ddacc25%2Ffaa23dc6-881a-4742-b3c1-1c264dc19103%2F3ild8uj_processed.png&w=3840&q=75)
Transcribed Image Text:The rate constant k for a certain reaction is measured at two different temperatures:
temperature
k
156.0 °C
7.6 x 1012
282.0 °C 5.7 × 1014
Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction.
a
Round your answer to 2 significant digits.
kJ
E =
x10
a
mol
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