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The gas constant R is defined as the Avogadro constant N A multiplied by the Boltzmann constant k (or k B): = = 6.022 140 76 × 10 23 mol −1 × 1.380 649 × 10 −23 J⋅K −1 = 8.314 462 618 153 24 J⋅K −1 ⋅mol −1. Since the 2019 revision of the SI, both N A and k are defined with exact numerical values when expressed in SI units. [2]
The ideal gas equation can be rearranged to give an expression for the molar volume of an ideal gas: = = Hence, for a given temperature and pressure, the molar volume is the same for all ideal gases and is based on the gas constant: R = 8.314 462 618 153 24 m 3 ⋅Pa⋅K −1 ⋅mol −1, or about 8.205 736 608 095 96 × 10 −5 m 3 ⋅atm⋅K ...
a (L 2 bar/mol 2) b (L/mol) Acetic acid: 17.7098 0.1065 Acetic anhydride: 20.158 0.1263 Acetone: 16.02 0.1124 Acetonitrile: 17.81 0.1168 Acetylene: 4.516 0.0522 Ammonia: 4.225 0.0371 Aniline [2] 29.14 0.1486 Argon: 1.355 0.03201 Benzene: 18.24 0.1193 Bromobenzene: 28.94 0.1539 Butane: 14.66 0.1226 1-Butanol [2] 20.94 0.1326 2-Butanone [2] 19.97 ...
Where: R is the Ideal gas constant (8.314 Pa·m 3 /mol·K); T is the absolute temperature (K); H is the Henry's law constant for the target chemical (Pa/m 3 mol); K ow is the octanol-water partition coefficient for the target chemical (dimensionless ratio); P s is the vapor pressure of the target chemical (Pa); and v is the molar volume of the ...
Therefore, an alternative form of the ideal gas law may be useful. The chemical amount, n (in moles), is equal to total mass of the gas (m) (in kilograms) divided by the molar mass, M (in kilograms per mole): =. By replacing n with m/M and subsequently introducing density ρ = m/V, we get:
J/(mol K) Enthalpy of combustion –473.2 kJ/mol Δ c H o: Heat capacity, c p: 114.25 J/(mol K) Gas properties Std enthalpy change of formation, Δ f H o gas –103.18 kJ/mol Standard molar entropy, S o gas: 295.6 J/(mol K) at 25 °C Heat capacity, c p: 65.33 J/(mol K) at 25 °C van der Waals' constants [4] a = 1537 L 2 kPa/mol 2 b = 0.1022 ...
The standard Gibbs free energy of formation of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of that substance from its component elements, in their standard states (the most stable form of the element at 25 °C and 100 kPa).
Further comprehensive authoritative data can be found at the NIST Chemistry WebBook page on thermophysical properties of ... a = 553.6 L 2 kPa/mol 2 b = 0.03049 L/mol