The rate constant k for a certain reaction is measured at two different temperatures: temperature k 3.1 × 108 9.5 × 107 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. 195.0 °C E = a 127.0 °C Round your answer to 2 significant digits. kJ mol x10
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 3.1 × 108 9.5 × 107 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. 195.0 °C E = a 127.0 °C Round your answer to 2 significant digits. kJ mol x10
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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![The rate constant k for a certain reaction is measured at two different temperatures:
temperature
195.0 °C
127.0 °C
Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction.
Round your answer to 2 significant digits.
8. - 0
E
=
a
k
3.1 x 108
9.5 × 107
kJ
mol
x10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F61ad7f72-97e8-4e38-83ab-7685cffaff26%2Fda1a54e9-8330-4ab2-8dad-80117dd2e319%2Fyxczkw_processed.png&w=3840&q=75)
Transcribed Image Text:The rate constant k for a certain reaction is measured at two different temperatures:
temperature
195.0 °C
127.0 °C
Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction.
Round your answer to 2 significant digits.
8. - 0
E
=
a
k
3.1 x 108
9.5 × 107
kJ
mol
x10
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