Gas Laws: Why is PV directly proportional to mT?

The relationship for physicists is: $$PV=NkT,$$ where $N$ is is the number of gas molecules/atoms, and $k$ is Boltzmann's constant. In chemistry they normally convert the $Nk$ to $nR$, where $n$ is measured in moles instead of being a simple count, and $R$ is the universal gas constant.

So, the proportionality from pressure to mass is incidental and depends on what the gass is made of, since, for a particular pure type of gas, you can convert from mass to number and back.

The reason that pressure is proportional to the number of atoms is because pressure is the average force per unit area exerted on the walls of the container. That force is cause by individual collisions of gas molecules with the walls, and the force is directly proportional to the collision rate. Naturally, if you double the number of molecules, all other things being equal, you'll double the collision rate, doubling the pressure. Thus pressure is proportional to particle number.

The interesting question is that when you have a collision the impulse, and thus the force, depends on both the mass and velocity of the colliding particle. So why is it proportional to number and not mass? Well, the reason is because temperature in gasses is a measure of the kinetic energy of the molecules. So, if you have two different gases at a given temperature, volume, and number of molecules, the one with more massive molecules will be moving slower in such a way that they have the same pressure.