Why Ideal Gas Laws Fail

Ideal gases are a complete scientific fantasy. You are taught that if you double the

pressure on a gas, the volume cuts in half perfectly. That is Boyle’s Law.

But in the real world, if you squeeze a gas too hard, the math completely

breaks. Here is why. Real gas particles actually take up physical space and

have sticky forces between them. The standard formula assumes particles are invisible ghosts

with zero volume and no attraction. So, unless you keep the pressure low

and the temperature high, your gas is going to go rogue and break the laws of

physics.