Chapter 12, Problem 12.94PAE

12.100 A reaction important in smog formation is

   ${\text{O}}_3\left(g\right)+\text{NO}\left(g\right)\rightleftarrows {\text{O}}_2\left(g\right)+{\text{NO}}_2\left(g\right)K=6.0\times {10}^{34}$

(a) If the initial concentrations are $\left[{\text{O}}_3\right]=1.0\times {10}^{-6}\text{M,}\left[\text{NO}\right]=1.0\times {10}^{-5}\text{M,}\left[{\text{NO}}_2\right]=2.5\times {10}^{-4}\text{M,}$ and $\left[{\text{O}}_2\right]=8.2\times {10}^{-3}\text{M}$ , is the system at equilibrium? If not, in which direction does the reaction proceed?

(b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)