Well i know real gases behave as ideal gas (almost) when pressure is low and temperature is high. I want to understand this - When pressure is low attractive forces in the gas moelcules will be stronger(as compared to high pressure) but the fast movement due to high temperature compensates it? Am i right? Why can't it be high pressure and low temperature? Because of high pressure repulsive forces dominate ( because molecules will be very close) but then you lower the temperature and moelcules don't move very fast and that compensates for the repulsive forces Anything wrong in my reasoning. Please help!