A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by: O3 +NO ---> O2 +NO2

The rate law for this reaction is: k[O3][NO]

Given that k = 4.49 × 106 M-1·s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3]0 = 7.60 × 10-6 M and [NO]0= 8.95 × 10-5 M, owing to continuous production from separate sources.

Next, Calculate the number of moles of NO2(g) produced per hour per liter of air.