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 o,(g) + NO(g) O2(g) + NO2(g) The rate law for this reaction is rate of reaction =k|0,|NO Given that k 3.02 x 109 M-1 s-1 at a certain temperature, calculate the initial reaction rate when (Osl and [NOI remain essentially constant at the values [O10-8.43 x 10-6 M and [NO] continuous production from separate sources 2.59 10-5 M, owing to Number M- s-I Calculate the number of moles of NO2(g) produced per hour per liter of air. Number mol h1. L- O Previous e Check Answer Next -I Exi > Hint

Explanation / Answer

Given data

Rate constant k = 3.02 x 10^6 M-1 s-1

Initial concentration of O3, [O3]0 = 8.43*10^-6 M

Initial concentration of NO, [NO]0 = 2.59*10^-5 M

Part a

Initial rate of reaction = k[O3]0 [NO]0

= 3.02 x 10^6 x 8.43*10^-6 x 2.59*10^-5

= 6.59 x 10^-4 M s-1

Part b

Moles of O3 < moles of NO

8.43*10^-6 < 2.59*10^-5

O3 is limiting reactant

Moles of NO2 produced = 8.43*10^-6 mol h-1 L-1

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