Gas laws 1662 Robert Boyle studied the relationship between volume and pressure of a gas of fixed amount at constant temperature. He observed that volume of a given mass of a gas is inversely proportional to its pressure at a constant temperature. Boyle's law, published in 1662, states that, at constant temperature, the product of the pressure and volume of a given mass of an ideal gas in a closed system is always constant. It can be verified experimentally using a pressure gauge and a variable volume container. It can also be derived from the kinetic theory of gases: if a container,
Gas the volume is doubled, the pressure is halved. Given the inverse relationship between pressure and volume, the product of pressure ("P") and volume ("V") is a constant ("k") for a given mass of confined gas as long as the temperature is constant. Stated as a formula, thus is: Because the before and after volumes and pressures of the fixed amount of gas, where the before and after temperatures are the same both equal the constant "k", they can be related by the equation: formula_5 In 1787, the French physicist and balloon pioneer, Jacques Charles, found that oxygen, nitrogen, hydrogen, carbon