I am trying to determine the density of a gas (oxygen). As the gas is a compressible fluid a modified version of the ideal gas equation is required. I have been given the following equation and I am struggling to interpret it. I would like advice on the unit conversions and whether this is the correct equation at all.
\rho=\frac{(P+1.01325).10^5.MW}{z.8314.(T+273)}
where:
\rho = density (Kg/m3)
P = pressure (bar(g))
MW = molecular weight (in kg/kmol)
z = compressibility factor (dimensionless)
T = temperature (deg. C)
I think that the 1.01325 converts the bar.g. to bar.a. then to pascals using the 100,000 multiplier?
Has the universal gas constant 8.314 J/( ) been converted to J/(K.kmol) ?
