Contrast ideal vs. nonideal/real gases, and explain why very high pressure and very low temperature gases...

Contrast ideal vs. nonideal/real gases, and explain why very high pressure and very low temperature gases behave nonideally. (6 points)

Expert Solution

Ideal Gas	NonIdeal gas
There is no attractive or repulsive force between gas molecules.	There is a little attractive or repulsive force between gas molecules.
It was assumed that ideal gas molecules do not occupy any volume.	Nonideal gas molecules occupy small volume
The collisions between ideal gas molecules are elastic collision.	The collisions between ideal gas molecules are inelastic collisions.
Ideal gas follow PV=nRT formula	Nonideal gas follow the van-der-Walls formula, (p+an2/V2) (V-nb) = nRT

At higher temperature molecular kinetic energy increases enough so the molecules can overcome the effect of intermolecular attraction or repulsion. So the term an2/V2 which arises due to intermolecular attraction of molecules can be neglected.

The 2nd term nb arise as the nonideal gas occupy a finite volume. At low pressure, the volume of gas increase so much that the effect of the finite volume was reduced.

So the van-der-Walls equation becomes PV=nRT i.e gas law of ideal gas. So at high temperature and low-pressure non-ideal gas behave ideally.

queen_honey_blossom answered 8 months ago

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