Chapter 15, Problem 39E

The reaction

$\text{NO}\left(g\right){\text{ + O}}_3\left(g\right){\text{ NO}}_2\left(g\right){\text{ + O}}_2\left(g\right)$

was studied by performing two experiments. In the first experiment (results shown in following table), the rate of disappearance of NO was followed in a large excess of ${\text{O}}_3.$ (The $\left[{\text{O}}_3\right]$ remains effectively constant at $\text{1}{\text{.0×10}}^4{\text{ molecules/cm}}^3\text{.)}$

In the second experiment, [NO] was held constant at $2.0\times {10}^{14}{\text{molecules/cm}}^3.$ The data for the disappearance of ${\text{O}}_3$ were as follows:

1. What is the order with respect to each reactant?
2. What is the overall rate law?
3. What is the value of the rate constant obtained from each set of experiments? $\text{Rate}=k\text{'}{\left[\text{NO}\right]}^x\text{ Rate}=k"{\left[{\text{O}}_3\right]}^y$
4. What is the value of the rate constant for the overall rate law?
   $\text{Rate}=k{\left[\text{NO}\right]}^x{\left[{\text{O}}_3\right]}^y$