# Problem: The reaction NO2 + CO → NO + CO2 is found to obey the following empirical rate law: rate = k[NO2]2 For this reaction, if you start with an initial concentration of CO that is much higher than the initial concentration of NO2 ([CO]0 &gt;&gt; [NO2]0) then a plot of ln[NO2] will appearA. curved as the kinetics are 2nd order in NO2.B. linear as the kinetics are 1st order in NO2.C. linear as the kinetics are pseudo-first order in NO2.D. curved as the kinetics are 1st order in NO2.

###### FREE Expert Solution

We’re being asked to how the plot will appear if you start with an initial concentration of CO that is much higher than the initial concentration of NO2 ([CO]0 >> [NO2]0) then a plot of ln[NO2]

NO2 + CO → NO + CO2

The empirical rate law for this reaction rate = k[NO2]

The integrated rate law for a first-order reaction is as follows:

The integrated rate law for a second-order reaction is as follows:

$\overline{)\frac{\mathbf{1}}{{\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{\mathbf{t}}}{\mathbf{=}}{\mathbf{kt}}{\mathbf{+}}\frac{\mathbf{1}}{{\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{\mathbf{0}}}}$

where:

[A]t = concentration at time t

k = rate constant

t = time

[A]0 = initial concentration

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###### Problem Details

The reaction NO2 + CO → NO + CO2 is found to obey the following empirical rate law: rate = k[NO2]For this reaction, if you start with an initial concentration of CO that is much higher than the initial concentration of NO2 ([CO]0 >> [NO2]0) then a plot of ln[NO2] will appear

A. curved as the kinetics are 2nd order in NO2.

B. linear as the kinetics are 1st order in NO2.

C. linear as the kinetics are pseudo-first order in NO2.

D. curved as the kinetics are 1st order in NO2.