Gas Compressibility is the ability of a gas to be compressed.
Boyle's Law is a set of rules that governs how things are done.
The impact of a gas's molecules on the container's walls causes pressure to be exerted by it.
The number of molecule collisions with the walls every second, or collision rate, is proportional to the gas's number density.
When the volume of a gas is reduced, the number density rises, and the collision rate rises as well.
As a result, a gas's pressure is inversely proportional to the volume it takes up; as volume drops, pressure rises, and vice versa.
The Law of Charles.
The average kinetic energy of gas molecules is proportional to the absolute temperature of the sample, hence increasing the temperature increases the average kinetic energy.
As a result, if the gas is heated, molecules will collide with the container's walls more frequently and with more force, increasing the pressure.
The volume of gas expands until the pressure of the gas is balanced by the constant external pressure.
The Law of Avogadro is related to both its density and its temperature.
The Law of Partial Pressures by Dalton, The pressure generated by one type of molecule is unaffected by the presence of another gas if molecules do not attract or repel one another.
Diffusion, the slow mixing of molecules of one gas with molecules of another due to their kinetic properties, provides direct evidence of gaseous random motion.
Thomas Graham, a Scottish scientist, discovered in 1832 that rates of diffusion for gases are inversely proportional to the square roots of their molar weights under the same conditions of temperature and pressure.