Their mass is much more less. Area scales with length2, mass with length3.adjacent said:The area of each molecule is very less ...
Pressure is a macroscopic concept, which is not useful for atomic level interactions.since the pressure is force/area
The kinetic theory of matter states that all matter is made up of tiny particles in constant motion. This motion is known as kinetic energy and it is influenced by factors such as temperature and pressure.
According to the kinetic theory, gas molecules are in constant, random motion. They collide with each other and with the walls of their container, exerting pressure. The average kinetic energy of gas molecules is directly proportional to the temperature of the gas.
An increase in temperature causes gas molecules to move faster and collide more frequently. This results in an increase in the pressure of the gas. On the other hand, a decrease in temperature causes gas molecules to move slower and collide less frequently, resulting in a decrease in pressure.
An ideal gas is a theoretical gas that follows all the assumptions of the kinetic theory. These assumptions include that the gas molecules have no volume, there are no intermolecular forces between the molecules, and all collisions are perfectly elastic.
According to the kinetic theory, the volume of a gas is directly proportional to its pressure. This means that if the volume of a gas is decreased, the molecules will collide more frequently with the walls of the container, resulting in an increase in pressure. Similarly, if the volume is increased, the pressure will decrease due to less frequent collisions.