My textbook shows that pressure fraction is equal to mole fraction because the same volume cancels:
But it violates (if I am not mistaken) the law in this example it gives:
the main components of dry air, by volume, are N2, 78.08%, O2, 20.95%, Ar, 0.93%, and CO2, 0.04%. What is the partial pressure of each gas in a sample of air at 1atm.
The strategy it gives for solving this problem is by treating the volume percent as mole percent, and in turn as pressure percent. But obviously, each gas occupies a different volume, the law of partial pressure doesn't apply. does it?
Also, is it possible for different components of air to occupy different amounts of space in atmosphere? If atmosphere is a container, doesn't all components just occupy the same amount of space-the size of container?