Why ideal gas behavior is assumed for PV = nRT?

Question

zuko95 · Answer

PV = nRT is derived from charles, boyle's and avagadro's laws, none of which assume ideal gas behavior.

sapphiremoon · Answer

I'd like to think it's because the volume in relation to the number of moles would be different from an ideal gas because of the volume of the atoms... but I really don't know, sorry. Also possibly because gases freeze/condense at low temperatures? Idk maybe I'm making stuff up...

osprey · Answer

It MAY be that part of the problem here is a GAS versus a VAPOUR. I think that B and C's "laws" are modelled on the assumption of an ideal gas - molecules don't interact except when clunking each other etc. Also, providing you (rig ?) the experiments, you can probably squash the expt and the gas law into each other. The errors involved show how wide of the mark you are. Then, you might try things like a VAN DER WAALS gas, and there are many other models for gases, of which pvnrt is probably the "simplest" ???? Also, vapours condense at nrT temperatures, whereas gases don't. Sorry about the muddle. http://perendis.webs.com

irishboy123 · Answer

i think they are all idealised

eg if you actually do the experiments with dense or lumpy gases, none of the laws *work*