Are these gas density calculations correct?

[kinogram]

If the equation below is correct

$n = PV / (R/T)$

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 H₂ = 4124 J / kg K

Then 1 m³ of H₂ at 101325 Pa and 273.15 K
should have a molar density of 0.089949

and

1 m³ of H₂ 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?




.

 

[berkeman]

If the equation below is correct

$n = PV / (R/T)$

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 H₂ = 4124 J / kg K

Then 1 m³ of H₂ at 101325 Pa and 273.15 K
should have a molar density of 0.089949

and

1 m³ of H₂ 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

 

[kinogram]

Thanks.. I see that now



$PV=nRT$

Then

$n=PV/(RT)$


however it looks like the calculations were made correctly according to the proper equation






.