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The rearrangement of cyclopropane to propene at 500 °C is first order (k = 6.70x10-4s ¹). (CH₂)3(9) CH₂CH=CH₂(g) How much time is required for 89.9% of the (CH₂)3 intially present in a reaction flask to be converted to product at this temperature? S

The rearrangement of cyclopropane to propene at 500 °C is first order (k = 6.70x10-4s ¹). (CH₂)3(9) CH₂CH=CH₂(g) How much time is required for 89.9% of the (CH₂)3 intially present in a reaction flask to be converted to product at this temperature? S

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
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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Use the integrated rate law to calculate time for percent reacted. The rearrangement of cyclopropane to propene at 500 °C is first order (k = 6.70x10-4s-¹). (CH₂)3(9) CH3CH=CH₂(g) How much time is required for 89.9% of the (CH₂)3 intially present in a reaction flask to be converted to product at this temperature? S
Transcribed Image Text:Use the integrated rate law to calculate time for percent reacted. The rearrangement of cyclopropane to propene at 500 °C is first order (k = 6.70x10-4s-¹). (CH₂)3(9) CH3CH=CH₂(g) How much time is required for 89.9% of the (CH₂)3 intially present in a reaction flask to be converted to product at this temperature? S
Use the integrated rate law to determine the rate constant. The rearrangement of cyclopropane to propene at 500 °C is first order in (CH₂)3. (CH₂)3(9) CH3CH=CH₂(g) During one experiment it was found that the (CH₂)3 concentration dropped from 0.211 M at the beginning of the experiment to 7.62x10-2 M in 1.365x10³ seconds. What is the value of the rate constant for the reaction at this temperature? s-1
Transcribed Image Text:Use the integrated rate law to determine the rate constant. The rearrangement of cyclopropane to propene at 500 °C is first order in (CH₂)3. (CH₂)3(9) CH3CH=CH₂(g) During one experiment it was found that the (CH₂)3 concentration dropped from 0.211 M at the beginning of the experiment to 7.62x10-2 M in 1.365x10³ seconds. What is the value of the rate constant for the reaction at this temperature? s-1
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