1 atm =
760 mm Hg = 760 torr = 1.01325 • 10^5 Pa = 14.70 psi
Boyle’s Law
At a constant temperature, the volume of gas varies inversely with the pressure exerted on it
Charles’ Law
At a fixed pressure, the volume of a gas is proportional to the temperature
Gay-Lussac’s Law
Pressure is directly proportional to temperature
Avogadro’s Law
At constant temperature and pressure, the volume of a gas is proportional to the number of moles of a gas
Dalton’s Law
The total pressure of a mixture of gases is simply the sum of the partial pressures of the component gases
Kinetic Molecular Theory (KMT) Postulate #1
Molecules are in constant and random motion
Kinetic Molecular Theory (KMT) Postulate #2
Space occupied by gas molecules is small compared to volume of the container
Kinetic Molecular Theory (KMT) Postulate #3
Attractive forces between molecules are assumed to be small/negligible
Kinetic Molecular Theory (KMT) Postulate #4
Molecules collide and energy is transferred between molecules. The collisions are assumed to be completely elastic (no energy loss).
Kinetic Molecular Theory (KMT) Postulate #5
Pressure exerted by a gas is caused by collisions of gas molecules on the walls of the container.
More collisions = more pressure
Graham’s Law of Effusion
Rate of effusion of a gas is inversely proportional to the square root of the mass of the particles
At high pressure or low temperature, some assumptions of the KMT are no longer valid
- Real gases have molecules that occupy some actual volume
- Real gases may attract each other to some extent
At high pressure
The b term dominates
At low temperature
The a term dominates
