## Ideal Gas Law

 ideal gas
 a simplified model gas where the particles do not interact
 Boyle’s law
 pressure (P) is inversely proportional to volume (V)
 Charles’ law (and Gay-Lussac’s law)
 the volume (V) of a gas is directly proportional to its absolute temperature (T)
 states that at the same temperature and pressure, equal volumes of different gases contain an equal number of particles
 ideal gas law
 the “equation of state” for an ideal gas, which combines all of the empirical gas laws above-relates the thermodynamic proper ties of an ideal gas to each other
 equation for ideal gas law
 “P V = n R T”, where P is pressure, V is volume, n is moles, T is absolute temperature, and R is the gas law constant (0.082 L-atm/mol•K = 8.314 J/mol•K)
 gas law constant
 proportionality constant for the ideal gas law 0.082 L-atm/mol•K = 8.314 J/mol•K
 Dalton’ law (of partial pressures)
 each gas in a mixture exerts a “partial pressure” which adds to the others to give the total pressure
 equation for Dalton’ law (of partial pressures)
 “Ptotal = ? Pi” where Pi = Xi Ptotal is the partial pressure of gas “i”
 gas phase stoichiometry
 stoichometry where one of the reactants and/or products is a gas
 gas phase stoichiometry uses this instead of mass or moles
 uses partial pressures instead of usual mass or mole units to describe the amount of gaseous species
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