Question

difference between ideal gas and real gas ....

Answer 1

Ideal gas:-
1. Ideal gases obeys all gas laws under all conditions of temperature and pressure.
2. The volume occupied by the molecules is negligible as compared to the total volume occupied by gas.
3. Obeys ideal gas equation PV=nRT.
Real gas:-
1. Real gases obeys gas laws only at low pressures and high temperatures.
2. The volume occupied by the molecules is not negligible as compared to the total volume of the gas.
3.Obeys Van Der Waals equation (P+ an^2/V^2)(V-nb)=nRT.


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Answer 2

Real gases differ from ideal gases such that,

Real gases have small attractive and repulsive forces between particles and ideal gases do not.

Real gas particles have a volume and ideal gas particles do not.

Real gas particles collide in-elastically (loses energy with collisions) and ideal gas particles collide elastically.

The most “ideal” real gas would be helium owing to its size and inert nature. The next one is probably hydrogen.

Generally speaking, a real gas approaches ideal behavior in high temperatures and low pressures. At high temperatures, kinetic energy of gas particles are much higher and the potential energy due to inter-molecular interactions becomes less and less significant. At low pressures, the volume of the gas is so high that individual volume of a gas particle becomes less significant compared to the total volume. The reverse is also true. Real gases deviate from ideal behavior at high pressures and low temperatures.

We can look at the ideal gas law, PV = nRT.

Since PV = nRT, for an ideal gas PV/nRT must be equal to 1. We call this the compression factor. Let us look at the compression factor of some real gases.

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