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=?[O3][NO] Given that ?=2.26×106 M−1⋅s−1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3]0=7.82×10−6 M and [NO]0=7.71×10−5 M, owing to continuous production from separate sources.

initial reaction rate: M⋅s−1

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

NO2 produced: mol⋅h−1⋅L−1

Answer 1

Here is the Solution:

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