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) right arrow O_2(g) + NO_2(g) The rate law for this reaction is rate of reaction = k[O_3][NO] Given that k = 4.62 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]_o = 2.31 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

1. rate = 0.000668 M/s

2. moles = 2.40 mol /h*L

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