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The rate constant k for a certain reaction is measured at two different temperatures: temperature k 311.0 °C 1.3 x 10¹1 421.0 °C 1.6 x 1011 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ 0 E = 0 mol x10 Xx

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 311.0 °C 1.3 x 10¹1 421.0 °C 1.6 x 1011 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ 0 E = 0 mol x10 Xx

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 311.0 °C 1.3 x 10¹1 421.0 °C 1.6 x 1011 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 mol X ?
Transcribed Image Text:The rate constant k for a certain reaction is measured at two different temperatures: temperature k 311.0 °C 1.3 x 10¹1 421.0 °C 1.6 x 1011 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 mol X ?
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