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 0_3(g) + No(g) rightarrow O_2(g) + NO_2(g) The rate law for this reaction is rule of reaction = k[o_3][No] Given that k = 4 74 times 10^6 M^1 s^1 at a certain temperature, calculate the initial reaction rate when (O.J and [NO] remain essentially constant at the values [O_3]o = 83 times 10^-6 M and [NO]_o" 39 times 10^-6 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] =(4.74x10^6 M-1s-1)(5.83x10^-6 M)(5.39x10^-5 M) = 1.48x10^-3 M/s

d[NO2]/dt = Rate = (1.4x10^-3 M/s) x [(3600 s)/(1 h)] = 5.328 M/h

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