If the equation below is correct [itex]n = PV / (R/T)[/itex] where : n = gas density in mole / m³ P = pressure in Pascal V = volume in m³ R = ideal (individual) gas constant T = temperature in Kelvin Given that the individual gas constant - R for H_{2} = 4124 J / kg K Then 1 m³ of H_{2} at 101325 Pa and 273.15 K should have a molar density of 0.089949 and 1 m³ of H_{2} at 5 x 10^{-18} Pa and 2.7 K should have a molar density of 4.49 x 10^{-22} are these calculated results correct? .
There is an algebra error in your starting equation... See http://en.wikipedia.org/wiki/Ideal_gas_law
Thanks.. I see that now [itex]PV=nRT[/itex] Then [itex]n=PV/(RT)[/itex] however it looks like the calculations were made correctly according to the proper equation .