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 = 3.91 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 = 4.10 times 10^-6 M and [NO]_0= 8.32 times 10^-5 M, owing to continuous production from separate sources. Calculate the number of moles of NO_2 (g) produced per hour per liter of air.

Explanation / Answer

Rate of reaction = k [O3] [NO] = 3.91 x 106 M-1 s-1 x 4.10 x 10-6 M x 8.32 x 10-5 M = 1.33 x 10-3 M s-1

So, the number of moles of NO2 produced per litre per second = 1.33 x 10-3

Number the number of moles of NO2 produced per litre per hour = 1.33 x 10-3 x 3600 = 4.788 mol L-1 h-1

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