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

N_{2}O_{4} → 2 NO_{2}

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

Given that N_{2}O_{4} is 2nd order for the reaction: N_{2}O_{4} → 2 NO_{2} , what is the concentration of N_{2}O_{4 }at 5 min when the rate constant is 0.50 min^{-1} M^{-1} and the initial [N_{2}O_{4}] is 0.24 M

A. 0.15 M

B. 6.7 M

C. 0.056 M

D. 0.22 M

E. 0.19 M

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Our tutors rated the difficulty of*Given that N2O4 is 2nd order for the reaction: N2O4 → 2 NO2 ...*as medium difficulty.