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4. Determine the rate law expression of the given reaction: F2(g) +2C1O2(g) →2FCIO2(g) Experiment Initial [F₂] (M) 1 0.01 M 2 0.01 M 3 0.02 M The rate law expression of the reaction n: rate=k[F₂]*[CIO₂] solve for x and y 5. Using the rate law expression obtained in item #4 solve for the k or the rate constant. You can use the data of any experiments. (k=rate/[F2][CIO2]) Initial [CLO₂] (M) 0.01 M 0.02 M 0.01 M Initial rate of formation of FCLO₂ (M/s) 1.5X10^-6 M/s 3X10^-6 M/s 6x10^-6 M/s DO ONLY NUMBER 5

4. Determine the rate law expression of the given reaction: F2(g) +2C1O2(g) →2FCIO2(g) Experiment Initial [F₂] (M) 1 0.01 M 2 0.01 M 3 0.02 M The rate law expression of the reaction n: rate=k[F₂]*[CIO₂] solve for x and y 5. Using the rate law expression obtained in item #4 solve for the k or the rate constant. You can use the data of any experiments. (k=rate/[F2][CIO2]) Initial [CLO₂] (M) 0.01 M 0.02 M 0.01 M Initial rate of formation of FCLO₂ (M/s) 1.5X10^-6 M/s 3X10^-6 M/s 6x10^-6 M/s DO ONLY NUMBER 5

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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4. Determine the rate law expression of the given reaction: F2(g) +2C1O2(g) →2FCIO2(g) Experiment Initial [F₂] (M) 1 0.01 M 2 0.01 M 3 0.02 M The rate law expression of the reaction n: rate=k[F₂]*[CIO₂] solve for x and y 5. Using the rate law expression obtained in item #4 solve for the k or the rate constant. You can use the data of any experiments. (k=rate/[F2][CIO2]) Initial [CLO₂] (M) 0.01 M 0.02 M 0.01 M Initial rate of formation of FCLO₂ (M/s) 1.5X10^-6 M/s 3X10^-6 M/s 6x10^-6 M/s DO ONLY NUMBER 5
Transcribed Image Text:4. Determine the rate law expression of the given reaction: F2(g) +2C1O2(g) →2FCIO2(g) Experiment Initial [F₂] (M) 1 0.01 M 2 0.01 M 3 0.02 M The rate law expression of the reaction n: rate=k[F₂]*[CIO₂] solve for x and y 5. Using the rate law expression obtained in item #4 solve for the k or the rate constant. You can use the data of any experiments. (k=rate/[F2][CIO2]) Initial [CLO₂] (M) 0.01 M 0.02 M 0.01 M Initial rate of formation of FCLO₂ (M/s) 1.5X10^-6 M/s 3X10^-6 M/s 6x10^-6 M/s DO ONLY NUMBER 5
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