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The rate constant k for a certain reaction is measured at two different temperatures: temperature k 190.0 °C 9.2×10¹0 316.0°C 8.5x10¹¹ Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy for this reaction. Round your answer to 2 significant digits. = mol 10 S

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 190.0 °C 9.2×10¹0 316.0°C 8.5x10¹¹ Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy for this reaction. Round your answer to 2 significant digits. = mol 10 S

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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KINETICS AND EQUILIBRIUM Using the Arrhenius equation to calculate Ea from k versus T data The rate constant k for a certain reaction is measured at two different temperatures: k 9.2×10¹0 8.5x10¹¹ temperature 190.0 °C 316.0 °C Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. mol 0 x10 X 3/5
Transcribed Image Text:KINETICS AND EQUILIBRIUM Using the Arrhenius equation to calculate Ea from k versus T data The rate constant k for a certain reaction is measured at two different temperatures: k 9.2×10¹0 8.5x10¹¹ temperature 190.0 °C 316.0 °C Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. mol 0 x10 X 3/5
Expert Solution
Step 1: Introduction to the given data
TemperatureRate constant, k
190.0degree C9.2 x 1010
316.0 degree C8.5 x 1011

straight E subscript straight a space equals space ? kJ/mol

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