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,
Graham's law involve the movement of more than one gas. In the same conditions of temperature and pressure, the molar mass is proportional to the mass density. Therefore the rate of diffusion of different gases is inversely proportional to the square root of their mass densities. Let gas 1 be H and gas 2 be O. (This example is solving for the ratio between the rates of the two gases) Therefore, hydrogen molecules effuse four times faster than those of oxygen. Using the formula of gaseous diffusion, the ratio of rate of diffusion of NH and HCl gas was obtained practically as