Question 28 of 28 Ma General Chemistry 4th Edition . University Science Books pr

Question

Question 28 of 28 Ma General Chemistry 4th Edition . University Science Books presented by Sapling Learning cQuarrie Rock ly A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by 03(g) + NO(g) O2(g)+NO2(g) The rate law for this reaction is =k[O3][NO] rate of reaction Given that k = 4.34 x 106 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [O3lo 8.66 x10-6 M and [NOlo- 2.52 x 10-5 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.h1.L-1

Explanation / Answer

The rate of the reaction = k[O3][NO]
                       = (4.34 x 106 M-1 S-1) x (8.66 x 10-6 M) x (2.52 x 10-5 M)
                       = 9.471 x 10-4 M.S-1
      
Therefore, the rate of the reaction = 9.47 x 10-4 M.S-1

No. of moles NO2(g) produced per hour per liter of air:

d[NO2]/dt = rate of reaction = 9.47 x 10-4 M.S-1

But, the reaction rate is in M.S-1 = mol.S-1.L-1
we need to convert into mol.h-1.L-1
d[NO2]/dt = rate of reaction = 9.47 x 10-4 mol.S-1. L-1 x (3600 S/1h)
                           = 3.41 mol.h-1.L-1
                          
Therefore, no. of moles NO2(g) produced per hour per liter of air = = 3.41 mol.h-1.L-1

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