According to the kinetic molecular theory, which statement is true about gases?

The statement that gas particles are in constant and random motion aligns perfectly with the principles of the kinetic molecular theory. This theory suggests that gas particles are in relentless motion, moving freely and colliding with one another as well as with the walls of their container. This constant motion leads to behaviors characteristic of gases, such as low density and the ability to expand to fill their container.

Moreover, this random motion is a crucial aspect of how gases behave. For instance, it explains why gases can diffuse and mix rapidly, as there are no fixed positions for the particles, allowing them to move throughout the available space freely.

In contrast, the other statements do not accurately reflect the properties of gases. The idea that gas particles are stationary contradicts fundamental gas behavior, as they are never at rest in a typical situation. Similarly, stating that gas particles exert strong attractive forces is misleading; while all particles do have some interactions, the kinetic molecular theory emphasizes that the forces between gas particles are negligible compared to the energy of their motion. Finally, when it comes to gas density, particles in the gaseous state are generally much less dense than those in liquids, primarily due to the larger distances between them, reinforcing that they occupy a larger volume with lower mass.