A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is 0.960 M, this same reactant decomposes with a half-life of 77.7 s. What is the order of the reaction? 0 1 2 What is the value and unit of the rate constant for this reaction? k = Unit:
A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is 0.960 M, this same reactant decomposes with a half-life of 77.7 s. What is the order of the reaction? 0 1 2 What is the value and unit of the rate constant for this reaction? k = Unit:
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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Transcribed Image Text:A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is
0.960 M, this same reactant decomposes with a half-life of 77.7 s.
What is the order of the reaction?
0
1
2
What is the value and unit of the rate constant for this reaction?
k
Unit:
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