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
Can't you plug and chug?
To calculate the initial reaction rate, we can use the rate law equation:
rate = k [O3]^m [NO]^n
Given that the rate law is rate = k [O3][NO], this means m = 1 and n = 1 in this case.
Now let's substitute the values given into the equation to find the initial reaction rate.
rate = k [O3]0 [NO]0
= (2.87 × 10^6 M^–1·s^–1) (2.56 × 10^–6 M) (7.14 × 10^–5 M)
Calculating this expression, we find:
rate ≈ 0.413 M·s^–1
So, the initial reaction rate is approximately 0.413 M·s^–1.
To calculate the number of moles of NO2(g) produced per hour per liter of air, we need to use stoichiometry and conversion factors.
From the balanced equation, we can see that the stoichiometric coefficient for NO2(g) is 1. This means that for every 1 mole of NO2(g) produced, 1 mole of the reactants (O3(g) and NO(g)) are consumed.
To find the number of moles of NO2(g) produced per hour per liter of air, we need to calculate the number of moles of NO2(g) produced per hour and divide it by the volume of air in liters.
To calculate the number of moles of NO2(g) produced per hour, we can use the initial reaction rate calculated previously:
moles of NO2(g) produced per hour = rate × volume of air in liters
Given that the volume of air is not provided, we cannot calculate the exact value. However, using a hypothetical volume of 1 liter of air:
moles of NO2(g) produced per hour = (0.413 M·s^–1) × (3600 s)
Calculating this expression, we find:
moles of NO2(g) produced per hour ≈ 1.4848 moles/hour
So, the number of moles of NO2(g) produced per hour per liter of air is approximately 1.4848 mol/hour·L.