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The rate constant k for a certain reaction is measured at two different temperatures: temperature k 6.2 × 10¹1 X 3.8 x 1013 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. 132.0 °C 242.0 °C Round your answer to 2 significant digits. 4-0 E = kJ mol x10

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 6.2 × 10¹1 X 3.8 x 1013 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. 132.0 °C 242.0 °C Round your answer to 2 significant digits. 4-0 E = kJ mol x10

Chemistry & Chemical Reactivity
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 k 132.0 °C E Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. a 242.0 °C = 6.2 × 10¹1 3.8 × 10¹3 kJ mol x10
Transcribed Image Text:The rate constant k for a certain reaction is measured at two different temperatures: temperature k 132.0 °C E Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. a 242.0 °C = 6.2 × 10¹1 3.8 × 10¹3 kJ mol x10
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