Chapter 20, Problem 20.69E

Nitric oxide, $\text{NO}$, is known to break down ozone, ${\text{O}}_{\text{3}}$, by the following bimolecular reaction:

$\text{NO}\left(\text{g}\right)+{\text{O}}_3\left(\text{g}\right)\to {\text{NO}}_{\text{2}}\left(\text{g}\right)+{\text{O}}_{\text{2}}\left(\text{g}\right)$

If the activation energy of this reaction is $10.5\text{kJ}/\text{mol}$ and the pre-exponential factor is $7.9\times {10}^{11}{\text{cm}}^3/\left(\text{mol}\cdot \text{s}\right)$, (a) what is the rate constant of this reaction at $298\text{K}$? (b) If the ozone concentration were $5.4\times {10}^{-12}\text{mol}/{\text{cm}}^{\text{3}}$ and the $\text{NO}$ concentration were $2.0\times {10}^{-12}\text{mol}/{\text{cm}}^3$ (conditions that might exist in a high-pollution area), what is the rate of this reaction?