At high temperatures, low pressures, and relatively low densities, real gases behave similarly to ideal gases.
The molecules of the gas have sufficient kinetic energy to overcome intermolecular forces at high temperatures; at low temperatures, however, the gas has less kinetic energy, making the intermolecular forces more noticeable. There is a lot of room between molecules at low gas densities and low pressures, but at high densities, the molecules are packed together, making the volume of the gas particles no longer insignificant. It is easier to think of those interactions as elastic collisions because there are fewer interactions at lower pressures.
D is therefore the right choice.
At high temperatures, low pressures, and relatively low densities, real gases behave similarly to ideal gases.
The molecules of the gas have sufficient kinetic energy to overcome intermolecular forces at high temperatures; at low temperatures, however, the gas has less kinetic energy, making the intermolecular forces more noticeable. There is a lot of room between molecules at low gas densities and low pressures, but at high densities, the molecules are packed together, making the volume of the gas particles no longer insignificant. It is easier to think of those interactions as elastic collisions because there are fewer interactions at lower pressures.
D is therefore the right choice.