The Universal and Individual Gas Constants in fluid mechanics and thermodynamics. Individual gas constant is given for the most common gases.

• Molar Mass Of Helium In Kg/mol
• Molar Mass Of Helium In Kg/kmol
• Molar Mass Of Helium In Kg
• He Element

Helium He weighs 0.0001785 g/cm³ (0.00010318 oz/in³) weight to volume volume to weight price mole to volume and weight mass and molar concentration density Helium, liquid He weighs 160 kg/m³ (9.98847 lb/ft³) weight to volume volume to weight price mole to volume and weight mass and molar concentration density. Explanation of how to find the molar mass of H2: Hydrogen Gas.A few things to consider when finding the molar mass for H2:- make sure you have the correct ch. Molar mass of Helium = 4 g. The given mass of Helium = 5 2 g. Thus the number of moles of Helium = g i v e n m a s s / m o l a r m a s s.

The Universal and Individual Gas Constants are known from the Ideal Gas Law.

The Individual Gas Constant - R

Molar Mass Of Helium In Kg/mol

The Individual Gas Constant depends on the particular gas and is related to the molecular weight of the gas. The value is independent of temperature. The induvidual gas constant, R, for a gas can be calculated from the universal gas constant, R_u (given in several units below), and the gas molecular weight, M_gas:

R = R_u/M_gas [1]

In the imperial system the most common units for the individual gas constant are ft lb/slug ^oR. In the SI system the most common units are J/kg K.

Unit conversion: 1 J/kg K = 5.97994 ft lb/slug °R, and 1 ft lb/slug °R = 0.167226 J/kg K.

The Individual Gas Constant for gases:

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The Universal Gas Constant - R_u

The Universal Gas Constant - R_u - appears in the ideal gas law and can be expressed as the product between the Individual Gas Constant - R - for the particular gas - and the Molecular Weight - M_gas - for the gas, and is the same for all ideal or perfect gases:

R_u = M_gas R [2]

The Universal Constant defined in Terms of the Boltzmann's Constant

The universal gas constant can be defined in terms of Boltzmann's constant k as:

R_u = k N_A [3]

where
k = Boltzmann's constant = 1.381 x 10^-23 [J/K]
N_A = Avogadro Number = 6.022 x 10²³ [1/mol]

The Molecular weight of a Gas Mixture

The average molecular weight of a gas mixture is equal to the sum of the mole fractions of each gas multiplied by the molecular weight of that particular gas:

M_mixture = Σx_i*M_i = (x₁*M₁ + ......+ x_n*M_n) [4]

where

x_i = mole fractions of each gas
M_i = the molar mass of each gas

The Universal Gas Constant - R_u - in alternative Units

• atm.cm³/(mol.K) : 82.057338
• atm.ft³/(lbmol.K) : 1.31443
• atm.ft³/(lbmol.^oR) : 0.73024
• atm.l/(mol.K) : 0.082057338
• bar.cm³/(mol.K) : 83.144598
• bar.l/(mol.K) : 0.083144598
• Btu/(lbmol.^oR) : 1.9872036
• cal/(mol.K) : 1.9859
• erg/(mol.K) : 83144598
• hp.h/(lbmol.^oR) : 0.0007805
• inHg.ft³/(lbmol.^oR) : 21.85
• J/(mol.K) : 8.3144598
  
• kJ/(kmol.K) : 8.3144598
  
• J/(kmol.K) : 8314.472
• (kgf/cm²).l/(mol.K) : 0.084784
• kPa.cm³/(mol.K) : 8314.4598
• kWh/(lbmol.^oR) : 0.000582
• lbf.ft/(lbmol.^oR) : 1545.349
• mmHg.ft³/(lbmol.K) : 999
• mmHg.ft³/(lbmol.^oR) : 555
• mmHg.l/(mol.K) : 62.363577
• Pa.m³/(mol.K) : 8.3144598
• psf.ft³/(lbmol.^oR) : 1545.3465
• psi.ft³/(lbmol.^oR) : 10.73
• Torr.cm³/(mol.K) : 62364

See also:
- More material properties
- The Ideal Gas Law - Gases are highly compressible with changes in density directly related to changes in temperature and pressure.
- A Mixture of Gases - Properties of mixtures of gases.
- More about temperature

Molar Mass Of Helium In Kg/kmol

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Molar Mass Of Helium In Kg

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