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Gas laws are a set of physical laws that describe the behavior of gases in relation to pressure, volume, and temperature. The main gas laws include:
Boyle's Law: At constant temperature, the pressure of a gas is inversely proportional to its volume. (P1V1 = P2V2) Charles's Law: At constant pressure, the volume of a gas is directly proportional to its absolute temperature. (V1/T1 = V2/T2) Avogadro's Law: At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of the gas. (V1/n1 = V2/n2) Ideal Gas Law: Combines the previous laws into one equation: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. These laws help us understand how gases behave under different conditions. The raws describing the behavior of gases under fixed pressure, volume, amount of gas, and absolute temperature conditions are called gas laws. The basic gas laws were discovered by the end of the 18th century when scientists found out that relationships between pressure, volume and temperature of a sample of gas could be obtained which would hold to approximation for all gases. The combination of several empirical gas laws led to the development of the ideal gas law.
The ideal gas law was later found to be consistent with atomic and kinetic theory.