Molar gas constant

Values of R	Units
8.3144621	J·K-1·mol-1
0.082057	L·atm·K-1·mol-1
8.205745 × 10-5	m3·atm·K-1·mol-1
8.3144621	L·kPa·K-1·mol-1
8.3144621	m3·Pa·K-1·mol-1
62.36367	L·mmHg·K-1·mol-1
62.36367	L·torr·K-1·mol-1
83.144621	L·mbar·K-1·mol-1
10.7316	ft3·psi· °R-1·lb-mol-1
0.73024	ft3·atm·°R-1·lb-mol-1

In chemistry, chemical engineering and physics, the molar gas constant (also called universal gas constant) R is a fundamental physical constant which appears in a large number of fundamental equations in the physical sciences, such as the ideal gas law and other equations of state and the Nernst equation. It is equivalent to the the Boltzmann constant (k_B) times Avogadro's constant (N): R = k_BN_A.

Currently its most accurate value is:

R = 8.3144621 J · K^-1 · mol^-1

The gas constant occurs in the ideal gas law as follows:

$P={\frac {nRT}{V}}={\frac {RT}{V_{\rm {m}}}}$

where:

P is the gas absolute pressure

T is the gas absolute temperature

V is the volume the gas occupies

n is the number of moles of gas

V_m is the molar volume

The specific gas constant

The gas constant of a specific gas, as differentiated from the above universal molar gas constant which applies for any ideal gas, is designated by the symbol R_s and is equal to the molar gas constant divided by the molecular mass (M) of the gas:

R_s = R ÷ M

The specific gas constant for an ideal gas may also be obtained from the following thermodynamics relationship:[2]

R_s = c_p – c_v

where c_p and c_v are the gas's specific heats at constant pressure and constant volume respectively.

Some example values of the specific gas constant are:

• Ammonia (molecular mass of 17.032 g · mol^–1) : R_s = 0.4882 J · K^–1 · g^–1
• Hydrogen (molecular mass of 2.016 g · mol^–1) : R_s = 4.1242 J · K^–1 · g^–1
• Methane (molecular mass of 16.043 g · mol^–1) : R_s = 0.5183 J · K^–1 · g^–1

Unfortunately, many authors in the technical literature sometimes use R as the specific gas constant without designating it as such or stating that it is the specific gas constant. This can and does lead to confusion for many readers.

The specific gas constant

The gas constant of a specific gas, as differentiated from the above universal molar gas constant which applies for any ideal gas, is designated by the symbol R_s and is equal to the molar gas constant divided by the molecular mass (M) of the gas:

R_s = R ÷ M

The specific gas constant for an ideal gas may also be obtained from the following thermodynamics relationship:[2]

R_s = c_p – c_v

where c_p and c_v are the gas's specific heats at constant pressure and constant volume respectively.

Some example values of the specific gas constant are:

• Ammonia (molecular mass of 17.032 g · mol^–1) : R_s = 0.4882 J · K^–1 · g^–1
• Hydrogen (molecular mass of 2.016 g · mol^–1) : R_s = 4.1242 J · K^–1 · g^–1
• Methane (molecular mass of 16.043 g · mol^–1) : R_s = 0.5183 J · K^–1 · g^–1

Unfortunately, many authors in the technical literature sometimes use R as the specific gas constant without designating it as such or stating that it is the specific gas constant. This can and does lead to confusion for many readers.