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A reactant decomposes with a half-life of 179 s when its initial concentration is 0.247 M. When the initial concentration is 0.775 M, this same reactant decomposes with the same half-life of 179 s. What is the order of the reaction? 1 What is the value and unit of the rate constant for this reaction? k =

A reactant decomposes with a half-life of 179 s when its initial concentration is 0.247 M. When the initial concentration is 0.775 M, this same reactant decomposes with the same half-life of 179 s. What is the order of the reaction? 1 What is the value and unit of the rate constant for this reaction? k =

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 21PS: At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an...
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A reactant decomposes with a half-life of 179 s when its initial concentration is 0.247 M. When the initial concentration is 0.775 M, this same reactant decomposes with the same half-life of 179 s. What is the order of the reaction? 1 2 What is the value and unit of the rate constant for this reaction? k =
Transcribed Image Text:A reactant decomposes with a half-life of 179 s when its initial concentration is 0.247 M. When the initial concentration is 0.775 M, this same reactant decomposes with the same half-life of 179 s. What is the order of the reaction? 1 2 What is the value and unit of the rate constant for this reaction? k =
Expert Solution
Step 1

Given : Half life of reaction with 0.247 M initial concentration of reactant = 179 s

And half life of reaction with 0.775 M initial concentration of reactant = 179 s

 

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