# Problem: Given that N2O4 is 2nd order for the reaction: N2O4 → 2 NO2 , what is the concentration of N2O4 at 5 min when the rate constant is 0.50 min-1 M-1 and the initial [N2O4] is 0.24 MA. 0.15 MB. 6.7 MC. 0.056 MD. 0.22 ME. 0.19 M

###### FREE Expert Solution

We’re being asked to determine the rate constant (k) of a second-order reaction:

N2O4 → 2 NO2

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

###### Problem Details

Given that N2O4 is 2nd order for the reaction: N2O4 → 2 NO2 , what is the concentration of N2Oat 5 min when the rate constant is 0.50 min-1 M-1 and the initial [N2O4] is 0.24 M

A. 0.15 M

B. 6.7 M

C. 0.056 M

D. 0.22 M

E. 0.19 M