# Gas Density Equation

by kinogram
Tags: density, equation
 P: 24 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? .
 Quote by 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? .
 P: 24 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 .