Final answer:
A real gas behaves like an ideal gas at low pressure and high temperature, where the effects of molecular volume and intermolecular forces become negligible.
Step-by-step explanation:
A real gas approaches the behavior of an Ideal Gas under certain conditions. Specifically, the behavior of a real gas aligns more closely with that of an ideal gas at low pressure and high temperature. At low pressures, the gas molecules are sufficiently far apart that their individual volumes do not significantly contribute to the overall volume of the gas.
At high temperatures, the kinetic energy of the gas particles is high enough that intermolecular attractions are relatively insignificant.
Conversely, at high pressures or low temperatures, the behavior of real gases tends to deviate from the ideal because the volume of the gas molecules becomes more significant and intermolecular forces become more apparent.