Humid Air vs. the Ideal Gas Law
Pressure, temperature and volume in a perfect ideal gas like moist air (air with water vapor).
In a perfect or ideal gas the correlations between pressure, volume, temperature and quantity of gas can be expressed by the Ideal Gas Law.
The Universal Gas Constant, _{ Ru } is independent of the particular gas and is the same for all "perfect" gases, and is included in of The Ideal Gas Law:
p V = n R _{ u } T (1)
where
p = absolute pressure (N/m^{2}, lb/ft^{2})
V = volume (m ^{ 3, } ft^{3} )
n = is the number of moles of the gas present
R _{ u } = universal gas constant (J/mol ^{ o } K, lb_{f} ft/(lb mol ^{ o } R) = 8.3145 J/mol K = 0.08206 L atm/mol K = 62.37 torr /mol K
T = absolute temperature ( ^{ o } K, ^{ o } R)
For a given quantity of gas, both n and R _{ u } are constant, and Equation (1) can be modified to
p_{1} V_{1} / T_{1} = p_{2}V_{2}/ T_{2}(2)
expressing the relationship between different states for the given quantity of the gas.
Equation (1) can also be expressed as
p V = N k T (3)
N =number of molecules
k = Boltzmann constant = 1.38066 10 ^{ 23 } J/K = 8.617385 10 ^{ 5 } eV/K
 One mole of an ideal gas at STP occupies 22.4 liters.
The Ideal Gas Law express the relation between pressure, temperature and volume in an ideal or perfect gas.
The Ideal Gas Law expessed by the Induvidual Gas Constant
The Ideal Gas Law can be expressed with the Individual Gas Constant as
p V = m R T (4)
where
p = absolute pressure (N/m^{2}, lb/ft^{2})
V = volume of gas (m ^{ 3, } ft^{3} )
m = mass of gas (kg, slugs )
R = individual gas constant (J/kg ^{ o } K, ft lb/slugs ^{ o } R)
T = absolute temperature ( ^{ o } K, ^{ o } R)
Density can be expressed as
ρ = m / V (4b)
where
ρ = density (kg/m^{3}, slugs/ft^{3} )
and equation (4) can be modified to
p = ρ R T (4c)
The Individual and Universal Gas Constant
The Individual Gas Constant can be expressed with the Universal Gas Constant and the molecular weight of a gas like
R = R _{ u } / M _{ gas } (2)
where
M _{ gas } = molecular weight of the gas
R _{ u } = universal gas constant ( 8314.47 J/(kmol K))
The Molecular weight and the Individual Gas Constants for air and water vapor are listed below:
Gas  Individual Gas Constant  R  Molecular Weight ( kg/kmole ) 

Imperial Units ( ft lb/slug ^{ o } R ) 
SI Units ( J/kg K ) 

Air  1716  286.9  28.97 
Water vapor  2760  461.4  18.02 
Air Pressure
Daltons Law states that
 the total pressure exerted by a mixture of gases is the sum of the partial pressures of the individual gases
The total pressure in moist air can therefore be expressed as
p _{ t } = p _{ a } + p _{ w } (3)
where
p _{ t } = total pressure (kPa)
p _{ a } = partial pressure dry air (kPa)
p _{ w } = partial pressure water vapor (kPa)
Dry Air Partial Pressure
By using (1) and (2) , the dry air partial pressure can be expressed as
p _{ a } = ρ _{ a } (286.9 J/kg K) T (4)
Water Vapor Partial Pressure
The water vapor partial pressure can be expressed as
p _{ w } = ρ _{ w } ( 461.5 J/kg K) T (4b)
Unlike other gases in air , water vapor may condense under common conditions. Since the boiling point of water at normal atmospheric pressure ( 101.3 kPa) is 100 ^{o}C, the vapor partial pressure of water is low compared to dry air partial pressure in moist air. Common values for vapor pressure in moist air are in the range 0.5 to 3.0 kPa .
Maximum vapor pressure before water vapor start to condense at an actual temperature is called saturation pressure  p _{ ws } .
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