In which one of the following conditions is a real gas expected to behave like an ideal gas ?

A real gas behaves most like an ideal gas under conditions of low pressure and high temperature. According to the Kinetic Molecular Theory, ideal gases are assumed to have no intermolecular forces and their particles occupy negligible volume. In real gases, these assumptions fail at high pressures (where molecules are forced close together, making their volume significant) and low temperatures (where molecules move slowly enough for intermolecular attractions to take effect). At lower pressure, the gas molecules are far apart, making the volume of the particles negligible compared to the total container volume and minimizing intermolecular interactions. Conversely, high pressure and low temperature (Option D) cause the greatest deviation from ideal behavior, often leading to liquefaction.