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 0,(g) + NO(g) O2(g) + NO2(g) The rate law for this reaction is rate of reaction = 031[NO] Given that k = 4.40 × 106 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [Oland [NOI remain essentially constant at the values [O3lo = 4.60 x 10-6 M and [NO1OF 3.17 x 10-5 M, owing to continuous production from separate sources. Number M. s Calculate the number of moles of NO2(9) produced per hour per liter of air. Number mol. h-1.L-

Explanation / Answer

rate = k [O3][NO2]

initial rate = 4.40*10^6*(4.6*10^-6*3.17*10^-5

               = 6.416*10^-4 M.s-1

from equation, rate = +d[NO2]/Dt

No of mol of NO2(g) produced = 6.416*10^-4 M.s-1

                      = 6.416*10^-4 M.s-1

                  1 sec = 0.000278 hr

        so that,

No of mol of NO2(g) produced =   6.416*10^-4*(0.000278)^-1  

                             = 2.308 mol.L-1*h-1

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