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where <math>R</math> is the [[molar gas constant]] (also known as the [[Universal gas constant]]). This equation can be re-a

|align=left|= the [[molar gas constant|universal gas law constant]] of 8.314472 m³·Pa·mol<sup>-1</su

...8.314472 J mol^&minus;1 T^{&thinsp;&minus;1} ) is the [[molar gas constant]]. A mole of a real gas will deviate from this volume, but for many real ga

|align=left|= the [[Molar gas constant|universal gas law constant]] = 8314.5 Pa·m³/(kmole·[[kelvin|K]

where ''R'' is the [[molar gas constant]], defined as the product of the [[Boltzmann constant]] ''k''_B a ...t accurate value of R is:<ref>[http://physics.nist.gov/cgi-bin/cuu/Value?r Molar gas constant] Obtained from the [[NIST]] website. [http://www.webcitation.org/query?url=

|align=left|= [[Molar gas constant|Universal gas constant]] in atm·m³/(kmol·K)

...'', and Avogadro’s constant through ''k'' = ''N''_A/''R''. The [[molar gas constant]] ''R'' was already known in 1908 with high precision. Perrin in his first ...'h'' and [[Boltzmann's constant]] ''k''. From the ratio of ''k'' and the [[molar gas constant]] ''R'' Avogadro’s constant could be determined. Planck's estimate was

|align=left|= [[Molar gas constant|Universal gas constant]] in atm·m³/(kmol·K)

|align=left|= the [[Molar gas constant|universal gas law constant]] = 8314.5 Pa·m³/(kmole·[[kelvin|K]

|align=left|= the [[Molar gas constant|universal gas law constant]] = 8314.5 Pa·m³/(kmole·[[kelvin|K]

...he order of 10²³&times;''k''_B &asymp; ''R'', the [[molar gas constant]]. where ''R'' is the [[molar gas constant]], ''p'' the pressure, and ''V'' the volume of the gas.

|align=left|= the [[molar gas constant]], 8.314 J '''·''' K^&ndash;1 '''·''' mol^&ndash;1

|align=left|= the [[molar gas constant]], 8.314 J '''·''' K^&ndash;1 '''·''' mol^&ndash;1

...ssibility factor (gases)|compressibility factor]], <math>R</math> is the [[molar gas constant]], <math>P</math> is the [[pressure]], <math>M</math> is the [[molecular ma

...d 6 for a gas of arbitrarily shaped molecules. The quantity ''R'' is the [[molar gas constant]]. For the present discussion it is important to notice that ''U'' is a fun

|align=left|= [[Molar gas constant|Universal gas constant]]

|align=left|= [[Molar gas constant|Universal gas constant]]

...ulation. The energy of one mole of such gas is 3''RT''/2, with ''R'' the [[molar gas constant]] and ''T'' the absolute [[temperature]]. The entropy of one mole is ''S''(

...ulation. The energy of one mole of such gas is 3''RT''/2, with ''R'' the [[molar gas constant]] and ''T'' the absolute [[temperature]]. The entropy of one mole is ''S''(