The activation energy for the gas phase decomposition of t-butyl alcohol is 274 kJ.(CH3)3COH(CH3)2C=CH2 + H2OThe rate constant at 803.0K is 0.000710/s. The rate constant will be _______/s at 852.0K.

Answered: The activation energy for the gas phase…

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 activation energy for the gas phase decomposition of t-butyl alcohol is 274 kJ.

(CH₃)₃COH(CH₃)₂C=CH₂ + H₂O
The rate constant at 803.0K is 0.000710/s. The rate constant will be _______/s at 852.0K.

Expert Solution

Step 1

Arrhenius equation:
If we know the value of the rate constant at two different temperatures, we can calculate the activation energy by using the Arrhenius equation. The Arrhenius equation is given by:

where k₂= rate constant at the T₂ temperature

k₁ = rate constant at T₁ = 0.000710 s^-1

E_a = activation energy = 274 kJ/mol

R = gas constant = 8.314 J/K.mol

T₁ = 803.0 K

T₂ = 852.0 K

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