My book mentions that the three informal gas laws (Boyle's, Charles', and Gay-Lussac's) can be combined into a more general relation PV ∝ mT (the precursor to the Ideal Gas Law).
Where: P is pressure, V is volume, m is mass (taken as a measure related to quantity of gas molecules), and T is temperature on the absolute scale.
- From Boyle's Law: P ∝ 1/V
- From Charles' Law: V ∝ T
- From Gay-Lussac's Law: P ∝ T
- From simple observation of a balloon being inflated: m ∝ V
All these can be surmised from PV ∝ mT by letting some of these state variables be constant. But when we let V and T be constant we get P ∝ m and this is a relationship I don't understand. It's not any law that I was able to find in my textbook or online and I don't get it conceptually.
But for PV ∝ mT to be true, P ∝ m must also be true. So my question is what is the relationship between pressure and mass?