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for å first order decomposition reaction, → products, given the time needed to decrease the initial concentration by one half, which equation should b- t 1/2 = 1/(k[A].) Rate = k[A] t1/2 = In2/k [A] t= -kt + [A]o 1/[A] t= kt + 1/[A]o

for å first order decomposition reaction, → products, given the time needed to decrease the initial concentration by one half, which equation should b- t 1/2 = 1/(k[A].) Rate = k[A] t1/2 = In2/k [A] t= -kt + [A]o 1/[A] t= kt + 1/[A]o

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 16PS: The decomposition of N2O5 in CCl4 is a first-order reaction. If 2.56 mg of N2O5 is present initially...
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In general, to calculate the rate constant for a first order decomposition reaction, A products, given the time needed to decrease the initial concentration by one half, which equation should be used? O t 1/2 = 1/(k[A].) O Rate = k[A] O t1/2 = In2/k O [A] t = -kt + [A]. O 1/[A] t= kt+ 1/[A]o
Transcribed Image Text:In general, to calculate the rate constant for a first order decomposition reaction, A products, given the time needed to decrease the initial concentration by one half, which equation should be used? O t 1/2 = 1/(k[A].) O Rate = k[A] O t1/2 = In2/k O [A] t = -kt + [A]. O 1/[A] t= kt+ 1/[A]o
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