Which type of gas has some attractive forces between its particles?

The correct answer is Real Gas, as it accurately reflects the behavior of gases in systems where intermolecular forces come into play. In the ideal gas model, it is assumed that gas particles do not interact with each other beyond elastic collisions, meaning there are no attractive or repulsive forces between them. This simplification holds true under conditions of low pressure and high temperature.

However, in real gases, particularly at high pressures or low temperatures, the presence of attractive forces becomes significant. These forces can lead to deviations from ideal behavior, such as compressibility and changes in pressure and temperature conditions. Real gases experience slight attractive forces (such as van der Waals forces) that affect their physical properties and behavior, distinguishing them from the theoretical ideal gas which assumes that no such forces exist.

Understanding this distinction is crucial when studying gas laws and thermodynamics, as it helps predict how gases will behave in various situations encountered in real-world applications.