A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O 3 ( g ) + NO ( g ) ⟶ O 2 ( g ) + NO 2 ( g ) The rate law for this reaction is rate of reaction = k [ O 3 ] [ NO ] Given that k = 3.91 × 10 6 M − 1 ⋅ s − 1 at a certain temperature, calculate the initial reaction rate when [ O 3 ] and [ NO ] remain essentially constant at the values [ O 3 ] 0 = 2.35 × 10 − 6 M and [ NO ] 0 = 7.74 × 10 − 5 M, owing to continuous production from separate sources. initial reaction rate: M ⋅ s − 1 Calculate the number of moles of NO 2 ( g ) produced per hour per liter of air. NO 2 produced: mol ⋅ h − 1 ⋅ L − 1