The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 58.0 kJ/mol. If the rate constant of thisreaction is 1.3 × 10³ M¹s -1at 348.0 °C, what will the rate constant be at 445.0 °C?Round your answer to 2 significant digits.k=M-1 -1SExplanationCheckJUL16X8tvWXMacBook AirⒸ2023 McGraw Hill LLC. All Rights Reserved. Terms of UsePPrivacy Center | Accessil The rate constant k for a certain reaction is measured at two different temperatures:temperaturek233.0 °C 5.3 x 10¹02.8 × 10¹1Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction.Round your answer to 2 significant digits.324.0 °CE =molExplanationCheckJULS 160x10XStvW© 2023 McGraw Hill LLC. All Rights Reserved. Ter70P

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The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 58.0 kJ/mol. If the rate constant of this reaction is 1.3 x 105 M¹s -1 at 348.0 °C, what will the rate constant be at 445.0 °C? Round your answer to 2 significant digits. k=M -1 -1 'S Explanation Check JUL 16 ☐ x10 X e tv W X 70 MacBook Air Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessib

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 58.0 kJ/mol. If the rate constant of this reaction is 1.3 x 105 M¹s -1 at 348.0 °C, what will the rate constant be at 445.0 °C? Round your answer to 2 significant digits. k=M -1 -1 'S Explanation Check JUL 16 ☐ x10 X e tv W X 70 MacBook Air Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessib

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Hello I need help with these question: based on the example I included, what other trials and different concentrations could I have used to end up with the same overall reaction order of 2, and what would be the rate law formula.
Use the Arrhenius equation to calculate Ea from the k versus T data.
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