Unit 6B - Pressure and Gas Laws - AP Chemistry

ideal gas

ideal gas

a gas that behaves according to KMT (i.e. sufficiently far from the boundaries of the gas region of the phase diagram)

ideal gas conditions

• elastic collisions

• temperature

• constant motion of particles

• size/spacing is insignificant

non-ideal gas conditions

• inelastic collisions

• temperature (phase changes)

• small volume (size/spacing becomes significant)

real gas

a gas that is deviating from KMT in some way (usually at low temperatures and/or high pressures, which would cause it to be close to its condensation or deposition point)

van der waals forces

intermolecular forces

van der waals equation

(P + n²a/V²)(V-nb) = nRT

constant “a” - pressure correction term

related to the attractions between the particles and must be determined experimentally

constant “b” - volume correction term

related to the volume excluded by a mole of particles and must be determined experimentally