8.2 Ideal Gases Flashcards
Ideal gas
a hypothetical gas with molecules that have no intermolecular forces and occupy no volume
Many real gases demonstrate behaviour close to ideal
ideal gas law
PV = nRT
P = pressure
V = volume
N = number of moles
R = ideal gas constant = 8.21 x 10-2 L*atm / mol*K; or 8.314 J/mol*K
ideal gas constant (R)
- 314 J / mol K
- 0821 atm*L / mol*K
Note: for any ideal gas, 1 mole of gas takes up a volume of approx:
22.4 L
Density (ρ)
mass / volume
combined gas law
Avogadro’s principles
if the pressure and temperature of a gas are held constant, the Volume and number of Moles are directly proportional
Boyle’s law
if the temperature and number of moles are held constant, the volume is inversely proportional to the pressure
- (boyle → popping pimple → volume and pressure)*
- (Can These Girls Possibly Be Virgins)*
Charles’s law
if the pressure and number of moles are held constant, the Volume is directly proportional to the absolute Temperature
(Can These Girls Possibly Be Virgins)
Gay-Lussac’s Law
if the volume and number of moles held constant, the Temperature and Pressure are directly proportional
(Can These Girls Possibly Be Virgins)
Dalton’s law of partial pressures
the total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual components
(where Pa, Pb, and Pc are the partial pressures of gases A, B, and C, respectively)
how to calculate the partial pressure of a gas
Henry’s Law
a gas law that states that the amount of dissolved gas in a liquid/solution is proportional to its partial pressure above the liquid (at the surface of the solution)
Vapor pressure
the pressure exerted by evaporated particles above the surface of a liquid
Evaporation
a dynamic process that requires the molecules at the surface of a liquid to gain enough energy to escape into the gas phase
