I have two questions, so if anyone could answer them it would be very helpful: 1) How can you cool a gas by increasing the volume, even though PV=nRT indicates otherwise. I thought if you increase volume, you also increase temperature? 2) High pressure and low temperature cause deviations from ideal gas behavior, so gases deviate from ideal behavior when pressure is >10atm and temperatures near the boiling points. Shouldn't we decrease temperature? From PV=nRT if we increase temperature we can increase pressure (and decrease volume), creating intermolecular forces. But if this is true, gases deviate at extremely high temperature and extremely low temperatures, since gases come together when temperature decreases. please help!