Asked by Ceamus Angelina
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by
O3(g)+NO(g) --> O2(g)+NO2(g)
The rate law for this reaction is:
rate=k[O3][NO]
Given that k = 2.87 × 106 M–1·s–1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3]0 = 2.56 × 10–6 M and [NO]0= 7.14 × 10–5 M, owing to continuous production from separate sources.
________ M·s–1
Calculate the number of moles of NO2(g) produced per hour per liter of air.
________ mol·h-1·L-1
O3(g)+NO(g) --> O2(g)+NO2(g)
The rate law for this reaction is:
rate=k[O3][NO]
Given that k = 2.87 × 106 M–1·s–1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3]0 = 2.56 × 10–6 M and [NO]0= 7.14 × 10–5 M, owing to continuous production from separate sources.
________ M·s–1
Calculate the number of moles of NO2(g) produced per hour per liter of air.
________ mol·h-1·L-1
Answers
Answered by
DrBob222
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