Gas laws are a set of fundamental principles that describe the behavior of gases under different conditions of pressure, temperature, and volume. The three most important gas laws are:

1. Boyle’s law: This law states that the volume of a gas is inversely proportional to its pressure, provided that the temperature and number of gas molecules remain constant. Mathematically, this can be expressed as PV = constant, where P is the pressure, V is the volume, and the constant is the product of the initial pressure and volume.
2. Charles’s law: This law states that the volume of a gas is directly proportional to its absolute temperature, provided that the pressure and number of gas molecules remain constant. Mathematically, this can be expressed as V/T = constant, where V is the volume, T is the absolute temperature, and the constant is the ratio of the initial volume to the initial temperature.
3. Gay-Lussac’s law: This law states that the pressure of a gas is directly proportional to its absolute temperature, provided that the volume and number of gas molecules remain constant. Mathematically, this can be expressed as P/T = constant, where P is the pressure, T is the absolute temperature, and the constant is the ratio of the initial pressure to the initial temperature.

These laws can be combined to form the ideal gas law, which relates the pressure, volume, temperature, and number of gas molecules of an ideal gas. The ideal gas law is expressed as PV = nRT, where P is the pressure, V is the volume, n is the number of gas molecules, R is the universal gas constant, and T is the absolute temperature.