Chapter 8 - The Gas Phase Flashcards
what is an ideal gas?
hypothetical gas with no intermolecular forces, occupies no volume
when does a gas not behave like an ideal gas?
high pressures (low volume) and low temperatures
equation for ideal gas law?
PV=nRT
what is density?
ratio of mass per unit volume (g/L for gases)
what is the volume of one mole at STP?
22.4 L
equation for combined gas law?
PV/T = PV/T
how to calculate molar mass?
(density at STP)(22.4 L/mol)
what is Avagadro’s principle?
all gases at a constant temperature and pressure occupy volumes directly proportional to the number of moles present; as the number of moles of gas increases, the volume increases in direct proportion
what is the equation for Avagadro’s principle?
n/v = n/v
what is Boyle’s law?
for a given gaseous sample held at constant temperature (isothermal), the volume of the gas is inversely proportional to its pressure; as pressure increases, volume decreases
equation for Boyle’s law?
PV=PV
what is Charle’s law?
at constant pressure, the volume of a gas is proportional to its absolute temperature; as temperature increases, pressure increases
what is the equation for Charle’s law?
P/T=P/T
how do gases behave when their is more than one gas in a container?
each gas will behave independently of the others; each will behave as if it’s the only gas in the container
what is partial pressure?
pressure exerted by each individual gas
what is Dalton’s law of partial pressure?
total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual components
what is the equation for Dalton’s law?
PT=PA+PB+PC+⋯
how can you find a partial pressure of a certain gas?
find the mole fraction of the gas (moles of gas/moles of total gas) and multiply that by the total pressure
what is vapor pressure?
pressure exerted by evaporated particles above the surface of a liquid
how are solubility (concentration) and pressure related?
directly
