General Chemistry 4th Edition University Science Books presented by Sapling Leam
ID: 1046887 • Letter: G
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 [o,[NO] Given that k continuous production from separate sources. k - 4.68 x 10° M-1. s-1 at a certain temperature, calculate the initial reaction rate when [OJl and n essentially constant at the values (Olo 5.19 10- M and NO),- 5.79 *10-s M, owing to Number M-s Calculate the number of moles of NO2(g) produced per hour per liter of air. mol h.L. solulian @ Check Answer ONext Exit HintExplanation / Answer
Answer:
Given reaction is O3(g) + NO(g) -------> O2(g) + NO2(g)
The rate law is Rate =k[O3][NO]
The order of the reaction with respect to O3=1 and with respect to NO=1, the overall order is 2.
where k=rate constant=4.68x106 M-1 s-1.
[O3]=5.19x10-6 M and [NO]=5.79x10-5 M
Therefore initial reaction rate=k[O3][NO]
Initial rate= (4.68x106 M-1 s-1)x(5.19x10-6 M)x(5.79x10-5 M)=1.406x10-3 M/s
Initial rate=1.406x10-3 M s-1.
From the given equation rate=d[NO2]/dt
1.406x10-3 M/s=d[NO2]/dt
d[NO2]/dt=(1.406x10-3 M/s)(60 s/1min)(60min/1h)
d[NO2]/dt=1.406x10-3 mol/L x3600/h
d[NO2]/dt=5.063 mol/L/h.
d[NO2]/dt~5 (mol/h/L) mol per hour per L.
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