CO(g) + NO2(9) → CO2(9) + NO(g) Reaction Initial Rate Trial Concentration (mol/L-h) (mol/L) [CO) (NO: 5.0 x 10 0.36 x 10 5.0 x 10 0.18 x 10 1.0 x 10 0.36 x 10 1.5 x 10 0.72 x 10 3.4 x 10 1.7 x 10 3 6.8 x 10 ? a Which two reaction trials can be used to determine the order of the reaction in [CO]? v and

CO(g) + NO2(9) → CO2(9) + NO(g) Reaction Initial Rate Trial Concentration (mol/L-h) (mol/L) [CO) (NO: 5.0 x 10 0.36 x 10 5.0 x 10 0.18 x 10 1.0 x 10 0.36 x 10 1.5 x 10 0.72 x 10 3.4 x 10 1.7 x 10 3 6.8 x 10 ? a Which two reaction trials can be used to determine the order of the reaction in [CO]? v and

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5RQ

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The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
A reaction of the form aAProducts gives a plot of ln[A] versus time (in seconds), which is a straight line with a slope of 7.35 X 103. Assuming [A]0 = 0.0100 M, calculate the time (in seconds) required for the reaction to reach 22.9% completion.
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