Explain the microscopic model of gases.

(N/A) The microscopic model of gases is based on the postulates of the Kinetic Molecular Theory of Gases:
$1$. $Particles$ $as$ $point$ $masses$: Gases consist of a large number of identical particles (atoms or molecules) that are so small and so far apart that the actual volume of the molecules is negligible compared to the empty space between them. This explains the high compressibility of gases.
$2$. $No$ $intermolecular$ $forces$: There is no force of attraction between gas particles at ordinary temperature and pressure. This explains why gases expand to occupy all available space.
$3$. $Constant$ $random$ $motion$: Gas particles are in constant,random,straight-line motion. If they were at rest,gases would have a fixed shape,which is not observed.
$4$. $Pressure$ $exertion$: Gas particles collide with each other and with the walls of the container. The pressure exerted by a gas is the result of these collisions with the container walls.
$5$. $Elastic$ $collisions$: Collisions between gas molecules are perfectly elastic. While individual energies may change during collisions,the total kinetic energy of the system remains constant at a given temperature.
$6$. $Distribution$ $of$ $speeds$: At any given temperature,although individual particles have different and constantly changing speeds due to collisions,the overall distribution of speeds remains constant.