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 3.88 times10^6 M^-1 middot 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 = 7.72 times 10^-6 M and [NO]0 = 3.15 times10^-5 M, owing to continuous production from separate sources. Number M middot S^-1 Calculate the number of moles of NO_2(g) produced per hour per liter of air. Number mol middot h^-1 midddot L^-1

Explanation / Answer

Rate = k [O3] [NO]

   = 3.88 x 10^6 ( 7.72 x 10^-6) ( 3.15 x 10^-5)

       = 9.435 x 10^- 4M/s

2) Rate = d[NO2] /dt

d[NO2] /dt = 9.435 x 10^-4 M/s

hence moles of NO2 per liter per sec = 9.435 x10^- 4

per 1 hour ( 3600 s) number of moles of NO2 = 9.435 x 10^-4 x 3600 = 3.397 mol

Hence NO2 produced = 3.397 mol h-1 L-1

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