A real gas approaches ideal behaviour at

Solution:

Real gases deviate from ideal gas behaviour primarily due to two factors: the finite volume occupied by gas molecules and the presence of intermolecular forces. Ideal gas behaviour assumes that molecules have negligible volume and no intermolecular forces. These assumptions become more valid under conditions where molecules are far apart and have high kinetic energy.

At high temperatures, the kinetic energy of molecules is high, which helps overcome the attractive intermolecular forces. At low pressures, the molecules are far apart, making their own volume negligible compared to the total volume of the container and reducing the effect of intermolecular forces.

Therefore, a real gas approaches ideal behaviour at high temperature and low pressure.