General Chemistry 4th Edition University Science Books presented by Sapling Leam

Question

General Chemistry 4th Edition University Science Books presented by Sapling Leaming A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by The rate law for this reaction is rate of reaction kO, INO Given that k 2.26x10 M-1 s-at a certain temperature, calculate the initial reaction rate when (Osl and [NO] remain essentially constant at the values (Oslo-1.94*10- 5 M and [NOo- 8.92x10-5 M, owing to continuous production from separate sources. Number M-s Calculate the number of moles of NO2(g) produced per hour per liter of air Number mol h.L

Explanation / Answer

rate = k*[O3]*[NO]
= 2.26*10^6*1.94*10^-6*8.92*10^-5
= (3.91*10^-4) M.s^-1

Answer : (3.91*10^-4) M.s^-1

d[O2]/dt = rate
= (3.91*10^-4) M.s^-1
= (3.91*10^-4)*(3600) M.h^-1
= 1.41 M.h^-1
= 1.41 mol.h^-1.L^-1

Answer : 1.41 mol.h^-1.L^-1

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