Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. What is the partial pressure of nitrogen in air at atmospheric pressure (1.0 atm)?
As you know, the partial pressure exerted by a gas that's part of a gaseous mixture depends on two things
- the total pressure of the mixture
- the mole fraction of that gas
Your equation will look like this
#color(blue)(P_"gas" = chi_"gas" xx P_"total")" "#, where
In this case, you know that the total pressure of the mixture is equal to
- the number of moles of that gas present in the mixture
- the total number of moles present in the mixture
You don't know exactly how many moles of the mixture you have, but you do know one important thing.
More specifically, you know that
As you know, a mole is simply a very large collection of molecules. In order to have one mole of a substance, you need to have
This means that the actual number of moles is not important here, because the ratio that exists between the number of molecules is equivalent to the ratio that exists between the number of moles.
So, if you have
So, let's say that you have
#chi_(N_2) = ("number of moles of N"_2)/"total number of moles"#
The number of moles of nitrogen will be
#x color(red)(cancel(color(black)("moles air"))) * "78 moles of N"_2/(100color(red)(cancel(color(black)("moles air")))) = 78/100x" moles N"_2#
The partial pressure of nitrogen will thus be
#P_(N_2) = 78/100 * "1.0 atm" = color(green)("0.78 atm")#