where P is absolute pressure (Pa), V is volume (m3), n is amount of substance (mol), R is the universal gas constant (8.314 J·K−1·mol−1), and T is temperature (K).
Boyle’s law: at a constant temperature, the volume of an ideal gas is indirectly proportional to pressure.
Charles’s law: at a constant pressure, the volume of an ideal gas is directly proportional to absolute temperature.
Gay-Lussac’s law: at a constant volume, the pressure of an ideal gas is directly proportional to absolute temperature.
Other gas laws of relevance are as follows.
Avogadro’s hypothesis: at a constant temperature and pressure, all gases of the same volume contain an equal number of molecules.
Dalton’s law: the pressure exerted by a mixture of gases is the sum of the partial pressures of its constituents.
Henry’s law: at a constant temperature, the amount of gas dissolved in a given volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with the liquid.
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