
a simplified model gas where the particles do not interact 


pressure (P) is inversely proportional to volume (V) 

Charles’ law (and GayLussac’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 


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 Latm/mol•K = 8.314 J/mol•K) 


proportionality constant for the ideal gas law
0.082 Latm/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) 

“P_{total} = ? P_{i}” where P_{i} = X_{i} P_{total} is the partial pressure of gas “i” 


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 
