Question

You became familiar with laws describing behavior of an ideal gas. How does it differ from the real gas behavior? What approximations are taken to describe ideal gases?

Answer 1

In ideal gas we consider two big approximations which are not correct-------- 1.The gas molecules (i.e atoms of the gas) does not posses any volume    2.There is no inter molecular attraction present among the gaseous molecule.   The above two are the major approximation considered for ideal gas. But in reality the gaseous molecules have volumes and they have inter molecular attraction present among them selves. Thus ideal gas model fails at lower temperature or higher pressure where the approximations are invalid.