Question

When does a real gas behave like an ideal gas?

Answer 1

Let us first understand that an ideal gas is one which follows all the gas laws. And, real gases are those that have different behavior from ideal gases due to the assumptions taken in the kinetic theory of gases. The assumptions include that the volume of gases in a molecule is not negligible. It was also assumed that there are no intermolecular forces between the gases molecules. Hence, there is a need for volume and pressure correction.

Complete answer:
An ideal gas is one that obeys gas laws under all pressure and temperature conditions. Ideal gases have mass and velocity.
They are devoid of volume.
The volume filled by the gas is minimal when compared to the entire volume of the gas.
It has no triple point and does not condense.
A real gas is one that defies gas laws under all standard pressure and temperature circumstances. The gas deviates from its ideal behavior when it becomes large and voluminous.
Velocity, volume, and mass are characteristics of real gases.
They liquefy when cooled below their boiling point.
The volume occupied by the gas is not insignificant when compared to the entire volume of the gas.
At low pressure and high temperature, real gases behave similarly to ideal gases.

Note:
We must note that this is because the potential energy owing to intermolecular forces diminishes in comparison to the kinetic energy of the particles, and the size of the molecules diminishes in comparison to the empty space between them. And thus, under low pressure and high temperature, the real gases start to fulfill the behavior of ideal gases and start behaving similarly to the ideal gases.