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 is described as: O3(g) + NO(g) ---> O2(g) + NO2(g) The rate law for this reaction= k[O3][NO] & k= 2.42 x 10-6 M-1*s-1 at a certain temperature, calculate the initial reaction rate when [O3] & [NO] remain essentially constant at the values [O3]0= 7.48 x 10-6 M & [NO]0= 3.26 x 10-5M, owing to continuous production from separate sources. & Calculate the number of moles of NO2(g) produced per hour per liter of air.

Explanation / Answer

initial rate = 5.9 * 10 ^-16 njumber of moles of ozone in 1 litre air = 1.72e-8 moles of ozone per litre air number of moles of NO2(g) produced per hour per liter of air = 1.72e-8

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