The rate constant for the reaction below was determined to be 3.241×10-5 s–1 at 800 K. The activation energy of the reaction is 265 kJ/mol. What would be the value of the rate constant at 9.70×102 K? $$N2O(g)N2(g)+O(g) s-1

The rate constant for the reaction below was determined to be 3.241×10-5 s–1 at 800 K. The activation energy of the reaction is 265 kJ/mol. What would be the value of the rate constant at 9.70×102 K? $$N2O(g)N2(g)+O(g) s-1

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 116QRT

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Question

The rate constant for the reaction below was determined to be 3.241×10^-5 s^–1 at 800 K. The activation energy of the reaction is 265 kJ/mol. What would be the value of the rate constant at 9.70×10² K?

$$N2O(g)N2(g)+O(g)

s^-1

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