The gas laws are a set of fundamental principles that describe the behavior of gases. They include Boyle's law, Charles's law, Gay-Lussac's law, and Avogadro's law.
Boyle's law states that at a constant temperature, the pressure and volume of a gas are inversely proportional. This means that as the pressure on a gas decreases, its volume increases, and vice versa.
Charles's law states that at a constant pressure, the volume of a gas is directly proportional to its absolute temperature. This means that as the temperature of a gas increases, its volume also increases, and vice versa.
The kinetic theory of gases explains the behavior of gases in terms of the motion of their particles. It states that gas particles are in constant, random motion and that their kinetic energy is directly proportional to their temperature.
The ideal gas law, PV = nRT, combines the gas laws and the kinetic theory into one equation. It describes the relationship between pressure, volume, temperature, and the number of moles of an ideal gas. It is based on the assumptions that gas particles have no volume and do not interact with each other.