Question

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide is described as: O3(g) + NO(g) ---> O2(g) + NO2(g)The rate law for this reaction= k[O3][NO] & k= 2.13 x 10-6 M-1*s-1 at a certain temperature, calculate the initial reaction rate when [O3] & [NO] remain essentially constant at the values [O3]0= 5.25 x 10-6 M &

Answer 1

Answer:

The question is not complete, but here is the complete part ; [NO]0= 2.92 x 10-5M, owing to continuous production from separate sources. & Calculate the number of moles of NO2(g) produced per hour per liter of air

Explanation:

The step by step calculations is as shown in the attachment.