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of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data.     [NO2] - [NO2]0 = -kt     [NO2] = 1/(kt + 1/[NO2]0)     k[NO2]2 = d[CO2]/dt     d[CO2]/dt = k[NO2]     -d[NO2]/dt = k[NO2]2 b) Calculate the rate constant (k). Enter the numerical value and corresponding

of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data.     [NO2] - [NO2]0 = -kt     [NO2] = 1/(kt + 1/[NO2]0)     k[NO2]2 = d[CO2]/dt     d[CO2]/dt = k[NO2]     -d[NO2]/dt = k[NO2]2 b) Calculate the rate constant (k). Enter the numerical value and corresponding

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 78GQ
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NO2(g) + CO(g)  NO(g) + CO2(g)


1a) The rate of the above reaction depends only on the concentration of nitrogen dioxide at temperatures below 225°C.
At a temperature below 225°C the following data were obtained:

 Time
(s) 		 [NO2]
(mol/L)
0 0.740
1.60×103 0.663
4.00×103 0.574
6.00×103 0.516
1.20×104 0.396
2.40×104 0.270



Which of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data.


    [NO2] - [NO2]0 = -kt

    [NO2] = 1/(kt + 1/[NO2]0)

    k[NO2]2 = d[CO2]/dt

    d[CO2]/dt = k[NO2]

    -d[NO2]/dt = k[NO2]2

b) Calculate the rate constant (k).
Enter the numerical value and corresponding

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