A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by

Question

O3(g)+NO(g) --> O2(g)+NO2(g)
The rate law for this reaction is:
rate=k[O3][NO]
Given that k = 2.87 × 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 = 2.56 × 10–6 M and [NO]0= 7.14 × 10–5 M, owing to continuous production from separate sources.
________ M·s–1
Calculate the number of moles of NO2(g) produced per hour per liter of air.
________ mol·h-1·L-1

Answer 1

i know how to do the first part, I just need the second part of the problem.

Answer 2

M,s-1 is a zero order; i.e., it is mols/L/s = mols/Ls.
Let's call your answer for the first part y, then
y mols/Ls x (60 s/min) x (60 min/hr) = 3600(y) mols/L.hr. Check my thinking