NO2(g) + CO(g) NO(g) + CO2(g)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)00.4401.55×1030.4183.88×1030.3895.81×1030.3681.16×1040.3172.32×1040.248Which of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data. ln([NO2]/[NO2]0) = -kt [NO2] = [NO2]0 - kt d[NO]/dt = k[NO2] k[NO2]2 = d[CO2]/dt 1/[NO2] - 1/[NO2]0 = ktCalculate the rate constant (k).Enter the numerical value and corresponding units.

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Answered: Time (s) [NO2] (mol/L) 0 0.440…

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 37E: The decomposition of hydrogen peroxide was studied, and the following data were obtained at a...

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NO₂(g) + CO(g) NO(g) + CO₂(g)

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	0.440
1.55×10³	0.418
3.88×10³	0.389
5.81×10³	0.368
1.16×10⁴	0.317
2.32×10⁴	0.248

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

    ln([NO₂]/[NO₂]₀) = -kt

    [NO₂] = [NO₂]₀ - kt

    d[NO]/dt = k[NO₂]

    k[NO₂]² = d[CO₂]/dt

    1/[NO₂] - 1/[NO₂]₀ = kt

Calculate the rate constant (k).

Enter the numerical value and corresponding units.

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