The Arrhenius equation shows how the rate constant (k) for a reaction is related to various factors, as follows. k = Ae−(Ea/RT) In this equation, k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant, and T is the temperature in kelvin. (The frequency factor is associated with the frequency and orientation of molecular collisions.) Calculate the activation energy for a reaction that has a rate constant of 0.242 s−1 and a frequency factor of 1.13 ✕ 1011 s−1 at 43.0°C. The gas constant, R, is 8.314472 _______J/K·mol.
The Arrhenius equation shows how the rate constant (k) for a reaction is related to various factors, as follows. k = Ae−(Ea/RT) In this equation, k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant, and T is the temperature in kelvin. (The frequency factor is associated with the frequency and orientation of molecular collisions.) Calculate the activation energy for a reaction that has a rate constant of 0.242 s−1 and a frequency factor of 1.13 ✕ 1011 s−1 at 43.0°C. The gas constant, R, is 8.314472 _______J/K·mol.
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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The Arrhenius equation shows how the rate constant (k) for a reaction is related to various factors, as follows.
k = Ae−(Ea/RT)
In this equation, k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant, and T is the temperature in kelvin. (The frequency factor is associated with the frequency and orientation of molecular collisions.)
Calculate the activation energy for a reaction that has a rate constant of 0.242 s−1 and a frequency factor of 1.13 ✕ 1011 s−1 at 43.0°C. The gas constant, R, is 8.314472
_______J/K·mol.
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