Question

Why are gases not ideal?

Answer 1

1. Gas molecules are present in large numbers and they perform random motion.
2. Gases obey Newton's laws of motion.
3. An ideal gas is a gas in which the gas molecules collide elastically and so there is no intermolecular force of attraction present between the molecules.
4. The volume of the gas is negligible compared with the volume occupied by the gas molecules.
5. No gas can even behave ideally but theoretically, the gas is composed of many random moving particles.
6. They behave ideally at standard temperature and pressure.
7. The kinetic energy of gas molecules is very high at higher temperatures, and so they move very fast.
8. The kinetic energy of gas molecules is very low at lower temperatures, so they come closer to one another, and so they do not behave ideally.
9. Therefore, we conclude that the real gases behave ideally at higher temperatures and lower pressure.