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 Q_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 = 2.70 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 = 1.87 times 10^-6 M and [NO]_0 = 3.98 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]

k = 2.7*10^6 M-1 s-1

Rate of reaction at given concentrations = 2.7*10^6 * 1.87*10^-6 *3.98*10^-5 = 2*10^-4 M.s-1

Number of moles of NO2 produced per hour per litre of air is = Rate of reaction *time in hours

(2×10^-4 moles/Ls)(3600s/Hour) = 0.72 moles of NO2 mol / hr.L

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