What's the difference between ideal gas and real gas?

Question

wolfe8 · Answer

http://www.chemguide.co.uk/physical/kt/realgases.html

anonymous · Answer

So an ideal gas is any gases that behave as if they were ideal at ordinary working conditions (e.g. low pressure and high temperature).

wolfe8 · Answer

I think so. They work as the gas laws state.

anonymous · Answer

The KMT recalls that an ideal gas has no volume and do not exert forces on each other but real gas do in fact have a volume and exert forces on each other.

anonymous · Answer

So basically, an ideal gas's behaviour/properties can come fairly close to a real gas at low pressure and high temperature only.

wolfe8 · Answer

An ideal gas has the following properties:
1. An ideal gas is considered to be a "point mass". A point mass is a particle so small, its mass is very nearly zero. This means an ideal gas particle has virtually no volume.
2. Collisions between ideal Gases are "elastic". This means that no attractive or repulsive forces are involved during collisions. Also, the kinetic energy of the gas molecules remains constant since theses interparticle forces are lacking.

So I think what you said is correct, and that the collisions are completely elastic.

anonymous · Answer

Alright! Thanks~ =D

wolfe8 · Answer

You're welcome. Hope it's right.