Final answer:
The correct statement is that real gas particles exert intermolecular forces on each other, while ideal gas particles do not. Option D is correct.
Step-by-step explanation:
The statement that correctly describes real and ideal gases among the choices provided is: d) Real gas particles exert intermolecular forces (IMFs) on each other; ideal gas particles do not.
Ideal gases are hypothetical gases that perfectly follow the kinetic-molecular theory, meaning they occupy no volume and exhibit no attractive forces whatsoever toward each other. Real gases, on the other hand, do not completely abide by these assumptions.
While at normal laboratory conditions of temperature and pressure, real gases behave sufficiently like ideal gases, at high pressures and low temperatures, the behaviors diverge due to the volume of real gas particles and the presence of intermolecular forces.
Ideal gases are theoretical constructs that perfectly follow the kinetic-molecular theory, whereas real gases have volume and exert intermolecular forces, particularly at high pressures and low temperatures.