I was recently taught about the three gas laws: 1)Boyle's Law, which stated that pressure is inversely proportional to volume and vice-versa at a constant temperature. 2)Charle's Law, which stated that volume is directly proportional to temperature at a a constant pressure 3)Amonton Law, which stated that pressure is directly proportional to temperature at a constant volume. I have no confusion regarding the first two laws, but, I don't understand how increasing temperature would increase pressure (Amonton's Law) unless the gas is in an enclosed container (so that when it's temp. is increased, it's volume increases too, which will cause it's molecules to collide with the container more often to produce more pressure). If we consider Amonoton's Law to be in the context of a closed container, then Boyle's Law and Charle's Law would also be in the context of a closed container (because the three laws are used together to derive the gas equation PV=nRT). But, then Boyle's Law would make no sense. So, the three laws are not intercompatible, which means the gas equation is wrong .... but ... how??