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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: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section11.7: Reaction Mechanisms
Problem 11.12E
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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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