@DrDreams
Lol after thinking about this for another 30 minutes, I'm not sure if what I wrote is correct. I think vapor pressure is only dependent on the mole FRACTIONS - and has NOTHING to do with the total amount of gas in it.

Here's my though experiment:

Let's say you have an equal-molar mixture Gas X and Gas Y. Gas X is more volatile than gas Y.

1) Now if you add Gas X, the fraction of Gas X increases and the vapor pressure of both Gas X and the total vapor pressure (which approaches the vapor pressure of pure Gas X) increases.

2) If you add Gas Y, the fraction of Gas Y increases and the VP of gas Y increases. Here, would the total vapor pressure decrease (since you have more of Gas Y - the less volatile gas)?

If you think that the total vapor pressure would decrease in scenario 2, how can you reconcile that with the fact that whenever you add a gas, the total pressure intuitively seems like it should increase? For example, if I added 10000 moles of Gas Y, I'd expect the pressure to increase overall.

Thus, I'm not sure if I can establish a relationship between total pressure and total vapor pressure.