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 = 4.82 times 10^6 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 = 2.23 times 10^-6 M and [NO]_0 = 8.60 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 = K [O3][NO]

substitute K , [O3] and [NO] values in above equation

rate = 4.82 x 106 [2.23 x 10-6][8.60 x 10-5]

rate = 9.24 x 10-4 M s-1

from the reaction given above

O3 and NO2 are 1:1 ratio

so rate of disaapearance = rate of apperance

so moles of NO2 produced = 9.24 x 10-4 mol . L-1 .s-1  = 3.3264 mol. L-1 . h-1

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