is the particular gas constant, T {\displaystyle T}

must then be multiplied by the gas constant R that is 8.31.

P = (nRT) ÷ V, where R is the ideal gas constant.

The appropriate value of the ideal gas constant (R) depends on the units being used.

R is the perfect gas constant R = 8314,32 J/K.kmol

where R is the gas constant, T the absolute temperature and F Faraday's constant.

where R is the gas constant and T the absolute temperature.

For a so-called « perfect » gas, this relation is simply PV = RT, where R is the gas constant.

where \(n\) is the number of moles of gas and \(k\) is a constant.

where n is the number of moles of the gas and R is the ideal gas constant.

where n=N/NA is the number of moles of gas and R=NAkB is the gas constant.

where n = N/NA is the number of moles of gas and R = NAkB is the gas constant.

k = Boltzmann's constant (ideal gas constant divided by Avogadro's number)

where F is Faraday’s constant, R is the perfect gases constant, and E° is the standard potential of the Ox/Red couple corresponding to [Ox] = [Red].

where R is the ideal gas constant, T is the temperature and x2 is the solute concentration in terms of mole fraction.