Chapter 14, Problem 14.115SP

The following mechanism has been proposed for the decomposition of dinitrogen pentoxide, which has the experimental rate law, Rate $=k{\text{[N}}_2{\text{O}}_5\text{]:}$
$N_2{O}_5\left(g\right)=\stackrel{k_1}{\to }N{O}_2\left(g\right)+N{O}_3\left(g\right)$   Faster, reversible
$N{O}_2\left(g\right)+N{O}_3\left(g\right)=\stackrel{k_2}{\to }NO\left(g\right)+N{O}_2\left(g\right)+O_2\left(g\right)$ Slow, ratedetermining
$NO\left(g\right)+N{O}_3\left(g\right)=\stackrel{k_3}{\to }2N{O}_2\left(g\right)$   Fast
Note that the first Step must be multiplied by 2 to obtain the overall reaction.
(a) Write a balanced equation for the overall reaction.
(b) Identify all reaction intermediates.
(c) Show that the proposed mechanism is consistent with the experimental rate law.
(d) Relate the rate constant k to the rate constants for the elementary reactions.