A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O3(g)+NO(g)O2(g)+NO2(g) The rate law for this reaction is rateofreaction=k[O3][NO] Given that k=3.59106M1s1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3]0=5.61106M and [NO]0=5.16105M, owing to continuous production from separate sources. initial reaction rate: 4s1 Calculate the number of moles of NO2(g) produced per hour per liter of air. NO2 produced 10lh1L1