Molecules of a gas are in incessant random motion colliding against one another and  with the walls of the container

The statement you provided describes the kinetic molecular theory of gases, which is fundamental in understanding the behavior of gases. This theory states that gas molecules are in constant, random motion, and their collisions with each other and with the walls of their container explain various gas properties, such as pressure and temperature.

Here are some key points regarding this concept:

1. Molecular Motion: Gas molecules move freely and randomly within a given space. They possess kinetic energy, which is directly proportional to the temperature of the gas.

2. Collisions: The collisions between gas molecules and between molecules and the walls of the container are elastic, meaning that there is no net loss of kinetic energy in the system. This is crucial for explaining the pressure exerted by gases.

3. Pressure: The pressure exerted by a gas on the walls of its container is a result of the force applied by countless individual molecule collisions against the wall. The more frequent and forceful the collisions, the higher the pressure.

4. Temperature: The average kinetic energy of the gas molecules is a measure of the temperature of the gas. As the temperature increases, the kinetic energy increases, leading to more vigorous motion and higher pressure.

5. Volume and Temperature Relationship: According to Boyle's Law and Charles's Law, the behavior of gases is predictable in terms of volume, pressure, and temperature. For instance, at constant temperature, increasing the volume decreases the pressure (and vice versa).

Understanding these principles is key when studying gas laws and thermodynamics in chemistry and physics.