please help with both parts of the question :) A reaction of importance in the f

Question

please help with both parts of the 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 = 3.39 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 = 7.06 times 10^-6 M and [NO]_0 = 2.83 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]

Rate = (3.39x10^6 M-1s-1)(7.06x10^-6 M)(2.83x10^-5 M) = 6.773 x10^-4 M/s

d[NO2]/dt = Rate = (6.773 x10^-4 M/s) x [(3600 s)/(1 h)] = =2.438 M/h

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