Chemistry · States of Matter - Gases, Liquids and Solids

Boyle’s Law describes the inverse relationship between pressure and volume of a gas at constant temperature, which is mathematically represented as PV = K. This means as the pressure increases, the volume decreases, and vice versa, while temperature remains constant. Avogadro’s Law involves the relationship between gas volume and moles, Charles’s Law involves volume and temperature, Dalton’s Law involves partial pressures, and Graham’s Law involves the rates of diffusion, none of which are represented by PV = K.

Boyle’s Law states that the pressure of a gas is inversely proportional to its volume when temperature is held constant. This is represented by the equation PV = K. Avogadro’s Law states that the volume of a gas is directly proportional to the number of moles at constant temperature and pressure, which is not represented by PV = K. Charles’s Law describes how gases tend to expand when heated, stating that volume is directly proportional to temperature at constant pressure, not represented by PV = K. Graham’s Law relates to the rate of effusion of a gas and is not represented by PV = K. Dalton’s Law deals with the total pressure exerted by a mixture of non-reacting gases and is not represented by PV = K.