 Gas constant

Values of R
^{[1]}Units
(V P T ^{−1} n^{−1})8.3144621(75)^{[2]} J K^{−1} mol^{−1} 5.189×10^{19} eV K^{−1} mol^{−1} 0.08205746(14) L atm K^{−1} mol^{−1} 1.9858775(34) cal K^{−1} mol^{−1} 8.314472(15)×10^{7} erg K^{−1} mol^{−1} 8.314472(15) L kPa K^{−1} mol^{−1} 8.314472(15) m^{3} Pa K^{−1} mol^{−1} 8.314472(15) cm^{3} MPa K^{−1} mol^{−1} 8.314472×10^{−5} m^{3} bar K^{−1} mol^{−1} 8.205746×10^{−5} m^{3} atm K^{−1} mol^{−1} 82.05746 cm^{3} atm K^{−1} mol^{−1} 84.78402×10^{−6} m^{3} kgf/cm^{2} K^{−1} mol^{−1} 8.314472×10^{−2} L bar K^{−1} mol^{−1} 62.36367(11) L mmHg K^{−1 } mol^{−1} 62.36367(11) L Torr K^{−1 } mol^{−1} 6.132440(10) ft lbf K^{−1} gmol^{−1} 1,545.34896(3) ft lbf °R^{−1} lbmol^{−1} 10.73159(2) ft^{3} psi °R^{−1} lbmol^{−1} 0.7302413(12) ft^{3} atm °R^{−1} lbmol^{−1} 1.31443 ft^{3} atm K^{−1} lbmol^{−1} 998.9701(17) ft^{3} mmHg K^{−1} lbmol^{−1} 1.986 Btu lbmol^{−1} °R^{−1} The gas constant (also known as the molar, universal, or ideal gas constant, denoted by the symbol R or R) is a physical constant which is featured in many fundamental equations in the physical sciences, such as the ideal gas law and the Nernst equation. It is equivalent to the Boltzmann constant, but expressed in units of energy (i.e. the pressurevolume product) per temperature increment per mole (rather than energy per temperature increment per particle). The constant is also a combination of the constants from Boyle's Law, Charles' Law, Avogadro's Law, and GayLussac's Law.
Its value is
 ^{[2]}
The two digits in parentheses are the uncertainty (standard deviation) in the last two digits of the value. The relative uncertainty is 9.1×10^{−7}.
The gas constant occurs in the ideal gas law, as follows:
where P is the absolute pressure (SI units Pascals), V is the volume of gas (SI units m^{3}), n is the chemical amount of gas (SI units mole), and T is thermodynamic temperature (SI units Kelvin). The gas constant has the same units as molar entropy.
Contents
Relationship with the Boltzmann constant
The Boltzmann constant k_{B} (often abbreviated k) may be used in place of the gas constant by working in pure particle count, N, rather than amount of substance, n, since
where N_{A} is the Avogadro constant. For example, the ideal gas law in terms of Boltzmann's constant is
where N is the number of particles (atoms or molecules).
Measurement
As of 2006, the most precise measurement of R is obtained by measuring the speed of sound c_{a}(p, T) in argon at the temperature T of the triple point of water (used to define the kelvin) at different pressures p, and extrapolating to the zeropressure limit c_{a}(0, T). The value of R is then obtained from the relation
where:
 γ_{0} is the heat capacity ratio (5/3 for monatomic gases such as argon);
 T is the temperature, T_{TPW} = 273.16 K by definition of the kelvin;
 A_{r}(Ar) is the relative atomic mass of argon and M_{u} = 10^{−3} kg mol^{−1}.^{[1]}
Specific gas constant
R_{specific}
for dry airUnits 287.04 J kg^{−1} K^{−1} 53.3533 ft lbf lb^{−1} °R^{−1} 1716.59 ft lbf slug^{−1} °R^{−1} Based on a mean molar mass
for dry air of 28.9645 g/mol.The specific gas constant of a gas or a mixture of gases (R_{specific}) is given by the molar gas constant, divided by the molar mass (M) of the gas/mixture.
Just as the ideal gas constant can be related to the Boltzmann constant, so can the specific gas constant by dividing the Boltzmann constant by the molecular mass of the gas.
Another important relationship comes from thermodynamics. This relates the specific gas constant to the specific heats for a calorically perfect gas and a thermally perfect gas.
where c_{p} is the specific heat for a constant pressure and c_{v} is the specific heat for a constant volume.^{[3]}
It is common, especially in engineering applications, to represent the specific gas constant by the symbol R. In such cases, the universal gas constant is usually given a different symbol such as R to distinguish it. In any case, the context and/or units of the gas constant should make it clear as to whether the universal or specific gas constant is being referred to.^{[4]}
U.S. Standard Atmosphere
The U.S. Standard Atmosphere, 1976 (USSA1976) defines the gas constant R* as:^{[5]}^{[6]}
The USSA1976 does recognize, however, that this value is not consistent with the cited values for the Avogadro constant and the Boltzmann constant.^{[6]} This disparity is not a significant departure from accuracy, and USSA1976 uses this value of R* for all the calculations of the standard atmosphere. When using the ISO value of R, the calculated pressure increases by only 0.62 pascal at 11 kilometers (the equivalent of a difference of only 0.174 meter or 6.8 inches) and an increase of 0.292 Pa at 20 km (the equivalent of a difference of only 0.338 m or 13.2 in).^{[citation needed]}
References
 ^ ^{a} ^{b} Mohr, Peter J.; Taylor, Barry N.; Newell, David B. (2008). "CODATA Recommended Values of the Fundamental Physical Constants: 2006". Rev. Mod. Phys. 80: 633–730. Bibcode 2008RvMP...80..633M. doi:10.1103/RevModPhys.80.633. http://physics.nist.gov/cuu/Constants/codata.pdf. Direct link to value.
 ^ ^{a} ^{b} http://physics.nist.gov/constants
 ^ Anderson, Hypersonic and HighTemperature Gas Dynamics, AIAA Education Series, 2nd Ed, 2006
 ^ Moran and Shapiro, Fundamentals of Engineering Thermodynamics, Wiley, 4th Ed, 2000
 ^ "Standard Atmospheres". http://www.sworld.com.au/steven/space/atmosphere/. Retrieved 20070107.
 ^ ^{a} ^{b} U.S. Standard Atmosphere, 1976, U.S. Government Printing Office, Washington, D.C., 1976 (Linked file is 17 MiB).
Categories: Ideal gas
 Physical constants
 Amount of substance
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