Everything about Ideal Gas Constant totally explained
R>
Units
(V·P·T-1·n-1) |
J·K-1·mol-1
| 0.0820574587 |
L·atm·K-1·mol-1 |
| 8.20574587 × 10-5 |
m3·atm·K-1·mol-1 |
| 8.314472 |
cm3·MPa·K-1·mol-1 |
| 8.314472 |
L·kPa·K-1·mol-1 |
| 8.314472 |
m3·Pa·K-1·mol-1 |
| 62.3637 |
L·mmHg·K-1·mol-1 |
| 62.3637 |
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 |
| 10.7316 |
ft3·psi· °R-1·lb-mol-1 |
| 0.7302 |
ft3·atm·°R-1·lb-mol-1 |
| 1716 (Air only) |
ft·lb·°R-1·slug-1 |
| 286.9 (Air only) |
N·m·kg-1·K-1 |
| 286.9 (Air only) |
J·kg-1·K-1 |
| 999 |
ft3·mmHg·K-1·lb-mol-1 |
The
gas constant (also known as the
molar,
universal, or
ideal gas constant, usually denoted by symbol
R) is a
physical constant which is featured in a large number of 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 (for example the pressure-volume product) per
kelvin per
mole (rather than energy per kelvin per
particle).
Its value is:
» R = 8.314472(15) J · K-1 · mol-1
The two digits in
parentheses are the uncertainty (
standard deviation) in the last two digits of the value.
The gas constant occurs in the simplest
equation of state, the
ideal gas law, as follows:
»
The USSA1976 does recognize, however, that this value isn't consistent with the cited values for the Avogadro constant and the Boltzmann constant.
This disparity isn't 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).
Further Information
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