RESPECTED SIR,
WHAT IS THE DIFFERENCE BETWEEN SIMPLE ADIABATIC EXPANSION OF GASES AND JOULE THOMSON EXPERIMENT.BOTH OCCUR IN ADIABATIC CONDITION AND INVOLVE EXPANSION OF GASES.........BUT IN THE FORMER CASE IDEAL GASES SHOW DROP IN TEMPERATURE WHILE IN LATTER THEY CASE DONT?
PLEASE ANSWER THIS QUESTION
as far as i know
in adiabatic expansion....in the initial conditions there is considerable volume ........which means ...the attractions between molecules of gas is negligible....in fact zero(ideal gas)
where as in joule thomson cooling .....the initial conditions are ...."the gas is compressed to a very little volume "......due to which molecules come closer to each other .......and as a result attractions between molecules increase very much compared to earlier case (adiabatic expansion)...after which the gas is suddenly allowed to expand in order to increase volume ....it has to overcome attractions ......for which it requires energy......which it takes from surroundings temperature...as a result surroundings are cooled
i dont think ideal gas shows joule thomson cooling be cause ideal gas is which has no attractions between molecules unlike real gas
hope i am clear