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) -----> O2(g) + NO2(g)

The rate law for this reaction is:

rate of reaction= k[O3][NO]

Given that k=3.58*10^6M^-1*S^-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3]0=2.76*10^-6M and [NO]0=4.80*10^-5M, owing to continuous production from separate sources.

______ M*s^-1

Calculate the number of moles of NO2(g) produced per hour per liter of air.

_______mol*h^-1*L^-1

Explanation / Answer

O3 + NO(g) --- > O2 (g) + NO2 (g)

Rate : k [ O3][NO]

We use above rate law, rate constant and equilibrium constant and concentration.

Rate = (3.58 E6) (2.76 E-6)(4.80 E-5) = 4.74 E-4 Ms-1

Calculation of number of moles of NO2 (g)

Rate of product of moleso of NO2 = rate of decomposition of O3

Rate of formation of NO2 = 4.74 E-4

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