According to kinetic molecular theory, how are gases compared with liquids and solids?
The kinetic molecular theory of matter says that, molecules of gases undergo greater rotational, translational and vibrational motion, than the molecules solids and liquids.
That's why gases don't have fixed volumes; their molecules just move around "carelessly" for as much space is available; little or no intermolecular forces are involved, except in collision.
And we can also see that, there are many more collisions between gas molecules than there are in liquid, and none in solids.
We can also note that, the pressure of a gas is thus as a result of the collisions that the gas molecules make with the container enclosing the gas or any other object in contact.
The Kinetic Theory of Matter describes the three different states of matter.
The particles are arranged orderly and closely packed. The attractive forces between them are very strong but their kinetic energy is very low. Thus, they vibrate about fixed positions.
The particles are arranged disorderly and less closely packed than in solid. The attractive forces between particles is stronger than in gases but weaker than in solids. However, the kinetic energy of particles is low. Thus, they are able to slide over one another.
The particles are arranged disorderly and very far apart. The attractive forces between them is very weak but their kinetic energy is very high. Thus, they move about randomly at high speeds.