Question

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by The rate law for this reaction is rate of reaction -o, [NO] Given that k = 4.40 × 10° MA, S-1 at a certain temperature, calculate the initial reaction rate when [01 and INO] remain essentially constant at the values [Oslo 2.16 x10-6 M and [NOlo- 7.84 x10-5 M, owing to continuous production from separate sources Number M.s Calculate the number of moles of NO g) produced per hour per liter of air. Number molh.L-

Answer 1

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

O3(g)+NO(g)⟶O2(g)+NO2(g)OX3(g)+NO(g)⟶OX2(g)+NOX2(g)

the rate law for this reaction is:

rate of reaction=k[O3][NO]

Given that k=4.40×106 M–1⋅s–1 at a certain temperature, the initial reaction rate when [O3][OX3] and [NO][NO] remain essentially constant at the values

initial rate constant = 4.40 × 10⁶ M ^-1 S^-1 × 2.16× 10^-6 M × 7.84 ×10^-5 M

= 74.512 × 10^-5 MS

the amount of substance of NO2(g) produced per hour per liter of air.

= 74.512 × 10^-5 MS × 60s / 1 min × 60 min / 1 hour

=