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The activation energy for the gas phase decomposition of t-butyl propionate is 164 kJ/mol. C₂H5COOC(CH3)3—(CH3)₂C=CH₂ + C₂H5COOH The rate constant for this reaction is 4.35x10-4 s¹ at 530 K. What is the rate constant at 576 K? S:1

The activation energy for the gas phase decomposition of t-butyl propionate is 164 kJ/mol. C₂H5COOC(CH3)3—(CH3)₂C=CH₂ + C₂H5COOH The rate constant for this reaction is 4.35x10-4 s¹ at 530 K. What is the rate constant at 576 K? S:1

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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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 propionate is 164 kJ/mol. C₂H5COOC(CH3)3-(CH3)₂C=CH₂ + C₂H5COOH The rate constant for this reaction is 4.35x10-4 s¹ at 530 K. What is the rate constant at 576 K? S1
Transcribed Image Text:The activation energy for the gas phase decomposition of t-butyl propionate is 164 kJ/mol. C₂H5COOC(CH3)3-(CH3)₂C=CH₂ + C₂H5COOH The rate constant for this reaction is 4.35x10-4 s¹ at 530 K. What is the rate constant at 576 K? S1
For the gas phase isomerization of dimethyl maleate, cis-CH300CCH=CHCOOCH3-trans-CH300CCH=CHCOOCH3 the rate constant at 663 K is 2.43x10-4 s¹ and the rate constant at 703 K is 7.64×10-4 S-¹. What is the activation energy for this reaction? kJ/mol
Transcribed Image Text:For the gas phase isomerization of dimethyl maleate, cis-CH300CCH=CHCOOCH3-trans-CH300CCH=CHCOOCH3 the rate constant at 663 K is 2.43x10-4 s¹ and the rate constant at 703 K is 7.64×10-4 S-¹. What is the activation energy for this reaction? kJ/mol
Expert Solution
Step 1

#Q.1:

Given activation energy, Ea = 164 kJ.mol-1 

Initial state:

Temperature, T1 = 530 K

Rate constant, k1 = 4.35*10-4 s-1 

Final state:

Temperature, T2 = 576 K

Rate constant, k2 = ?? (To be calculated) 

 

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