Which of the following conditions represents the closest approach to an ideal gas behavior for a real gas?
Correct: D
Real gases behave most like ideal gases when the intermolecular forces between molecules are minimized and the volume occupied by the gas molecules themselves is negligible compared to the total volume of the container. These conditions are best met at low pressure (molecules are far apart, reducing interactions) and high temperature (high kinetic energy overcomes attractive forces, and the overall volume of the gas is large, making molecular volume relatively insignificant).