Gas Laws The Behavior of matter

Compressibility Realization: since there is usually volume around the molecules of a gas, gases are readily compressible.

Factors affecting Gas pressure Amount of gas, volume, temperature

Boyle’s Law If the temperature is constant, as pressure increases, the volume decreases. P1V1 = P2V2

Charles’ Law If pressure is constant, as temperature increases, volume increases V1/T1 = V2/T2

Gay-Lussac’s Law If volume constant, as temperature increases, pressure increases. P1/T1 = P2/T2

Combined Gas Law Single expression combining Boyle’s, Charles’, and Gay-Lussac’s Laws: P1V1/T1 = P2V2/T2 The only constant is the amount of gas (number of molecules)

Ideal Gas Law PV = nRT R: constant: 8.31 L·Pa/K·mol n is the number of moles of gas Real gases and ideal gases differ most at low temperatures and high pressures

Dalton’s law of partial pressures Ptotal = P1 + P2 + P3 + … Think parts of a whole pie

Graham’s Law of Effusion Diffusion: the tendency of molecule to move from a zone of higher conc. to a zone of lower concentration Effusion: the process of escaping through a small orifice in a container Graham’s law: the rate of effusion is inversely proportional to the square root of the gas’s molar mass…this means that the lighter gases effuse faster than a heavier gas