Values of R |
Units (V·P·T ^{-1}·n^{-1}) |
---|---|

8.314472 | J·K^{-1}·mol^{-1} |

0.0820574587 | L·atm·K^{-1}·mol^{-1} |

8.20574587 × 10^{-5} |
m^{3}·atm·K^{-1}·mol^{-1} |

8.314472 | cm^{3}·MPa·K^{-1}·mol^{-1} |

8.314472 | L·kPa·K^{-1}·mol^{-1} |

8.314472 | m^{3}·Pa·K^{-1}·mol^{-1} |

62.36367 | L·mmHg·K^{-1}·mol^{-1} |

62.36367 | L·Torr·K^{-1}·mol^{-1} |

83.14472 | L·mbar·K^{-1}·mol^{-1} |

1.987 | cal·K^{-1}·mol^{-1} |

6.132440 | lbf·ft·K^{-1}·g-mol^{-1} |

10.73159 | ft^{3}·psi· °R^{-1}·lb-mol^{-1} |

0.7302413 | ft^{3}·atm·°R^{-1}·lb-mol^{-1} |

998.9701 | ft^{3}·mmHg·K^{-1}·lb-mol^{-1} |

8.314472 × 10^{7} |
erg·K^{-1}·mol^{-1} |

The **gas constant** (also known as the **molar**, **universal**, or **ideal gas constant**) is a physical constant that is featured in a number of fundamental equations in the physical sciences, such as the ideal gas law and the Nernst equation. It is expressed in units of energy (that is, the pressure-volume product) per kelvin per *mole.* It is equivalent to the Boltzmann constant, except that the latter is expressed in units of energy per kelvin per *particle.*

Denoted by the symbol * R*, the value of the gas constant is:

*R*= 8.314472(15) J · K^{-1}· mol^{-1}

The two digits in parentheses indicate the uncertainty (standard deviation) in the last two digits of the value.

## Contents |

An **ideal gas** (or "perfect" gas) is a hypothetical gas consisting of a very large number of identical particles, each of zero volume, uniformly distributed in density, with no intermolecular forces. Additionally, the molecules or atoms of the gas have complete randomness of direction and velocity, and they undergo perfectly elastic collisions with the walls of the container. The molecules of an ideal gas are often compared to rigid but elastic billiard balls.

The gas constant occurs in the ideal gas law (the simplest equation of state) as follows:

- <math>P = \frac{nRT}{V} = \frac{RT}{V_{\rm m}}</math>

where:

- <math>P\,\!</math> is the absolute pressure
- <math>T\,\!</math> is absolute temperature
- <math>V\,\!</math> is the volume the gas occupies
- <math>n\,\!</math> is the amount of gas (in terms of the number of moles of gas)
- <math>V_{\rm m}\,\!</math> is the molar volume

This equation does not exactly apply to real gases, because each molecule of a real gas does occupy a certain volume and the molecules are subject to intermolecular forces. Nonetheless, this equation is used as an approximation when describing the behavior of a real gas, except when the gas is at high pressures or low temperatures.

The Boltzmann constant *k _{B}* (often abbreviated

- <math>\qquad R=N_A k_B\,\!</math>,

where <math>N_A</math> is Avogadro's number (= 6.022 x 10^{23} particles per mole).

In terms of Boltzmann's constant, the ideal gas law may be written as:

- <math>PV=Nk_BT\,\!</math>

where *N* is the number of particles (atoms or molecules) of the ideal gas.

Given its relationship with the Boltzmann constant, the ideal gas constant also appears in equations unrelated to gases.

The **specific gas constant** or **individual gas constant** of a gas or mixture of gases (*R _{gas}* or just

The equation to calculate the specific gas constant for a particular gas is as follows:

- <math> R_{\rm gas} = \frac{\bar{R}}{M} </math>

where:

- <math>R_{\rm gas}\,\!</math> is the specific gas constant
- <math>\bar{R}</math> is the universal gas constant
- <math>M\,\!</math> is the molar mass (or molecular weight) of the gas

In the SI system, the units for the specific gas constant are J·kg^{-1}·K^{-1}; and in the imperial system, the units are ft·lb·°R^{-1}·slug^{-1}.^{[2]}

The specific gas constant is often represented by the symbol *R*, and it could then be confused with the universal gas constant. In such cases, the context and/or units of *R* should make it clear as to which gas constant is being referred to. For example, the equation for the speed of sound is usually written in terms of the specific gas constant.

The values of the individual gas constant for air and some other common gases are given in the table below.^{[1]}

Gas | Individual Gas Constant SI Units (J·kg ^{-1}·K^{-1}) |
Individual Gas Constant Imperial Units (ft·lb·°R ^{-1}·slug^{-1}) |
---|---|---|

Air | 286.9 | 1,716 |

Carbon dioxide (CO_{2}) |
188.9 | 1,130 |

Helium (He) | 2,077 | 12,420 |

Hydrogen (H_{2}) |
4,124 | 24,660 |

Methane (CH_{4}) |
518.3 | 3,099 |

Nitrogen (N_{2}) |
296.8 | 1,775 |

Oxygen (O_{2}) |
259.8 | 1,554 |

Water vapor (H_{2}O) |
461.5 | 2,760 |

The US Standard Atmosphere, 1976 (USSA1976) defines the Universal Gas Constant as:^{[3]}^{[4]}

- <math>\bar{R} = 8.31432\times 10^3 \frac{\mathrm{N \cdot m}}{\mathrm{kmol \cdot K}} </math>

The USSA1976 does recognize, however, that this value is not consistent with the cited values for the Avogadro constant and the Boltzmann constant.^{[4]} 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 pascals at 11,000 meters (the equivalent of a difference of only 0.174 meters, or 6.8 inches) and an increase of 0.292 pascals at 20,000 meters (the equivalent of a difference of only 0.338 meters, or 13.2 inches).

- Earth's atmosphere
- Gas
- Mole (unit)
- Pressure
- Temperature
- Volume

- ↑
^{1.0}^{1.1}The Individual and Universal Gas Constant.*The Engineering ToolBox*. Retrieved July 15, 2008. - ↑ To calculate the value of the specific gas constant of a gas in SI units, one should divide the value of the universal gas constant (in SI units) by the molar mass (or molecular weight) of the gas in kilograms per mole.
- ↑ Standard Atmospheres. Retrieved July 15, 2008.
- ↑
^{4.0}^{4.1}U.S. Standard Atmosphere, 1976. National Oceanic and Atmospheric Administration; National Aeronautics and Space Administration; United States Air Force. Retrieved July 15, 2008.

- American Institute of Chemical Engineers. 1984.
*Ideal Gas Law, Enthalpy, Heat Capacity, Heats of Solution and Mixing.*New York: American Institute of Chemical Engineers. ISBN 0816902607.

- Atkins, Peter, and Loretta Jones. 2008.
*Chemical Principles: The Quest for Insight,*4th ed. New York: W.H. Freeman. ISBN 0716799030.

- Chang, Raymond. 2006.
*Chemistry,*9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031.

- Cotton, F. Albert, and Geoffrey Wilkinson. 1980.
*Advanced Inorganic Chemistry,*4th ed. New York: Wiley. ISBN 0471027758.

- McMurry, J., and R.C. Fay. 2004.
*Chemistry,*4th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 0131402080.

All links retrieved December 5, 2013.

- The Individual and Universal Gas Constant. The Engineering ToolBox.
- The Ideal Gas Constant.

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