The rate constant for the reaction of hydrogen with iodine is 2.45 x 10-4 M-1s-1 at 302°C and 0.950 M-1 s1 at 508°C. Calculate the activation energy and Arrhenius preexponential factor for this reaction. OA= 9.50 x 108 M1s1 O A = 1.02 x 1010 M:1 5-1 OA=5.26 x 105 M-1 s1 O E, = 2.58 x 10o5 J/mol O E, = 1.50 x 105 J/mol O E, = 1.2 x 1015 J/mol

The rate constant for the reaction of hydrogen with iodine is 2.45 x 10-4 M-1s-1 at 302°C and 0.950 M-1 s1 at 508°C. Calculate the activation energy and Arrhenius preexponential factor for this reaction. OA= 9.50 x 108 M1s1 O A = 1.02 x 1010 M:1 5-1 OA=5.26 x 105 M-1 s1 O E, = 2.58 x 10o5 J/mol O E, = 1.50 x 105 J/mol O E, = 1.2 x 1015 J/mol

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.56PAE: The table below presents measured rate constants for the reaction of NO with ozone at three...

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