A reaction of importance in the formation of smog is that between ozone and nitr

Question

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O_3(g) + NO(g) rightarrow O_2(g) + NO_2(g) The rate law for this reaction is rate of reaction = k[O_3][NO] Given that k = 2.42 times 10^6 M^-1, s^-1 at a certain temperature, calculate the initial reaction rate when [O_3] and [NO] remain essentially constant at the values [O_3]_0 = 7.84 times 10^-6 M and [NO]_0 = 5.11 times 10^-5 M, owing to continuous production from separate sources. M middot s^-1 Calculate the number of moles of NO_2(g) produced per hour per liter of air. mol middot h^-1 middot L^-1

Explanation / Answer

Rate of reaction , r = K [O3][NO]

=(2.42 x 106 M-1s-1)(7.841 x 10-6M)(5.11 x 10-5M)

=96.95 x 10-5

= 9.695 x 10-4 M/s

d[NO2]/dt = Rate = (9.695 x 10-4 M/s) x [(3600 s)/(1 hour)] = 34902 x 10-4 M/h =3.4902 M/h =3.4902 mol.h-1.L-1

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