The kinetic theory of gases describes gases as collections of particles (atoms or molecules) in constant random motion. It assumes that these particles are point masses with negligible volume, and their collisions are perfectly elastic. Temperature is related to the average kinetic energy of these particles, and pressure arises from their collisions with the container walls. This theory helps explain gas behavior, such as pressure, temperature, and volume relationships, based on the motion and collisions of individual particles.
The Laws
1) Boyle's Law: At constant temperature, the volume of a given amount of gas is inversely proportional to its pressure.
2)Charles's Law: At constant pressure, the volume of a given amount of gas is directly proportional to its absolute temperature.
3)Avogadro's Law: Equal volumes of gases at the same temperature and pressure contain an equal number of molecules.
4) The ideal gas laws is a combination of all:
These laws, when combined, lead to the Ideal Gas Law:[PV = nRT]where (P) is pressure, (V) is volume, (n) is the number of moles of gas, (R) is the ideal gas constant, and (T) is the absolute temperature.