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 >> [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.

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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:


ln[A]t = -kt +ln[A]0 


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


1[A]t=kt+1[A]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.

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