I was reading about Dalton's Law of Partial Pressures in a textbook and the proposition is that under ideal conditions, the relevant factors are the pressures of the individual gases and their number of moles. The identity of the gas particles, however, does not matter, and the amount of volume each gas takes up is irrelevant.
But why isn't it relevant? Isn't pressure inversely proportional to volume? I'm missing something here, and I would appreciate help.