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 O3(g) + NO(g) rightarrow O2(g) + NO2(g) The rate law for this reaction is rate of reaction = k[O3][NO] Given that k = 2.53 Times 106 M- 1.s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values owing to continuous production from separate sources. Calculate the number of moles of N02(g) produced per hour per liter of air.

Explanation / Answer

a. Rate of reaction = k O3 x NO = 2.593 x 10^-4 M.s^-1 b. all stoichiometric co-efficient are equal to 1 first see the units in which rate is expressed = "M.s^-1" M means mol/liter so the rate is essentially expressed in units mol.L^-1.s^-1 to find answer for part (b) you simple need to convert the units from mol.L^-1.s^-1 to mol.L^-1.h^-1 which can be done by multiplying answer of part(a) by 3600 hence the answer for part (b) is 0.93348 mol.L^-1.h^-1 hope u got the answer and concept right :D

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