The use of a catalyst causes the rate constant for the reaction R → P to increase by a factor of exactly 450 at 298 K. Which one of the following statements best describes the effect of the catalyst? Assume that the rate constant for the reaction obeys the Arrhenius equation and that the Arrhenius pre- exponential factors are the same for both the catalyzed and uncatalyzed reactions. The catalyst decreases the activation energy by 7.02 kJ mol-1 The catalyst increases the activation energy by 15.1 k) mol1 The catalyst decreases the activation energy by 15.1 kJ mol-1 The catalyst decreases the enthalpy change by 21.3 kJ mol-1 The catalyst increases the activation energy by 7.02 kJ mol1

The use of a catalyst causes the rate constant for the reaction R → P to increase by a factor of exactly 450 at 298 K. Which one of the following statements best describes the effect of the catalyst? Assume that the rate constant for the reaction obeys the Arrhenius equation and that the Arrhenius pre- exponential factors are the same for both the catalyzed and uncatalyzed reactions. The catalyst decreases the activation energy by 7.02 kJ mol-1 The catalyst increases the activation energy by 15.1 k) mol1 The catalyst decreases the activation energy by 15.1 kJ mol-1 The catalyst decreases the enthalpy change by 21.3 kJ mol-1 The catalyst increases the activation energy by 7.02 kJ mol1

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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