Where can I find the gas constant R for hydrogen? How much is it?

This post was last edited by ylb913 on 2016-8-2 at 15:52. Isn’t the ideal gas constant R=0.082 fixed? If the pressure is at atmospheric pressure and the volume is in liters, then R = 0.082 atm·L/mol·K. If pressure, temperature, and volume are all in international units, R=8.314 Pa·m3/mol·K. The ideal gas law is PV = nRT, and R = PV/(nt). It is known that under standard conditions (note: 0°C, 1 standard atmosphere), the volume of 1 mole of an ideal gas is 22.4 L. By substituting p = 1 atm, T = 273 K, n = 1 mol, and V = 22.4 L, we get R ≈ 0.082 atm·L/mol·K. Using PV = nRT, we have R = PV/(nt); thus, 1*22.4/(1*273) = 0.082. When P = 101325 Pa, T = 273 K, n = 1 mol, and V = 22.4 L = 0.0224 m³ are substituted, we obtain R ≈ 8.314 Pa·m³/mol·K. Again using PV = nRT, we get R = PV/(nt); hence, 101325*0.0224/(1*273) = 8.314

The pressure is 4.0 MPa and the temperature is 313 K

Under this pressure, it is fine for hydrogen to obey the ideal gas law PV=nRT.

Rg=R/M, where Rg is the gas constant of the gas in question. R is known as the universal gas constant, or universal gas constant, and it does not change with the molecular weight of the gas ； M is the molar mass of the gas in question. For example, for hydrogen, M=0.002016 kg/mol, then . Rg=R/M=8.314/0.002016=4214