Problem: A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide describe by:O3(g) + NO(g) → O2(g) + NO2(g)The rate law for this reaction is:rate of reaction = k[O3][NO]a. Given that k = 3.66x10 6 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O 3]0 = 2.25x10-6 M and [NO]0 = 4.37x10-5 M, owing to continuous production from separate sources. (M s-1)b. Calculate the number of moles of NO2(g) produced per hour per liter of air. (mol h -1  L-1) 

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Problem Details

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide describe by:

O3(g) + NO(g) → O2(g) + NO2(g)

The rate law for this reaction is:

rate of reaction = k[O3][NO]

a. Given that k = 3.66x10 6 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O 3]0 = 2.25x10-6 M and [NO]0 = 4.37x10-5 M, owing to continuous production from separate sources. (M s-1)






b. Calculate the number of moles of NO2(g) produced per hour per liter of air. (mol h -1  L-1)

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