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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]
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 ...
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 ...
At standard temperature and pressure (100 kPa and 273.15 K), we can use Avogadro's law to find the molar volume of an ideal gas: V m = V n = R T P ≈ 8.3145 J m o l ⋅ K × 273.15 K 100 k P a ≈ 22.711 L / m o l {\displaystyle V_{\text{m}}={\frac {V}{n}}={\frac {RT}{P}}\approx {\frac {\mathrm {8.3145\ {\frac {J}{mol\cdot K}}\times 273.15\ K ...
The Boltzmann constant (k B or k) is the proportionality factor that relates the average relative thermal energy of particles in a gas with the thermodynamic temperature of the gas. [2] It occurs in the definitions of the kelvin (K) and the gas constant , in Planck's law of black-body radiation and Boltzmann's entropy formula , and is used in ...
Until 1982, STP was defined as a temperature of 273.15 K (0 °C, 32 °F) and an absolute pressure of 101.325 kPa (1 atm). Since 1982, STP is defined as a temperature of 273.15 K (0 °C, 32 °F) and an absolute pressure of 100 kPa (1 bar). Conversions between each volume flow metric are calculated using the following formulas: Prior to 1982,
R is the gas constant, 8.314 J·K −1 mol −1; T is the absolute temperature; To simplify, a volume of gas may be expressed as the volume it would have in standard conditions for temperature and pressure, which are 0 °C (32 °F) and 100 kPa. [2]