The rate constant of the elementary reaction C4Hs (9)→2C₂H4 (9) is k=1.23 x 10 sat 427 °C, and the reaction has an activation energy of 261 kJ/mol. Compute the rate constant of the reaction at a temperature of 464 °C. k: 8-1 for this question. At a temperature of 427 °C, 5.64 x 10³ s is required for half of the C4H8 originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 464 °C? t= S
The rate constant of the elementary reaction C4Hs (9)→2C₂H4 (9) is k=1.23 x 10 sat 427 °C, and the reaction has an activation energy of 261 kJ/mol. Compute the rate constant of the reaction at a temperature of 464 °C. k: 8-1 for this question. At a temperature of 427 °C, 5.64 x 10³ s is required for half of the C4H8 originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 464 °C? t= S
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 23P
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![The rate constant of the elementary reaction
C4H8 (9)→2C2H₁ (9)
is k=1.23 x 10 s¹ at 427 °C, and the reaction has an activation energy of 261 kJ/mol.
Compute the rate constant of the reaction at a temperature of 464 °C.
k=
8
Values if needed for this question.
At a temperature of 427 °C,
5.64 x 10³ s is required for half of the
C4H8 originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 464 °C?
t=
S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe8ae2ce9-f5e0-4f1a-8f27-6b600e36e8ad%2Fbd460ae3-ed29-418f-b0f8-0cb4b56f7e6e%2F4xpi8lr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The rate constant of the elementary reaction
C4H8 (9)→2C2H₁ (9)
is k=1.23 x 10 s¹ at 427 °C, and the reaction has an activation energy of 261 kJ/mol.
Compute the rate constant of the reaction at a temperature of 464 °C.
k=
8
Values if needed for this question.
At a temperature of 427 °C,
5.64 x 10³ s is required for half of the
C4H8 originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 464 °C?
t=
S
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