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`"R (Gas Constant)" = 8.31446261815324 " J/Mol" * "K"`

8.3144626181532

The **Gas Constant**, R, from the Ideal Gas Law is 8.31446261815324 Joules / (moles • Kelvin). The **gas constant** (also known as the **molar**, **universal**, or **ideal gas constant**, denoted by the symbol *R* or *R*) is a physical constant which is featured in many fundamental equations in the physical sciences. The Gas Constant (R) is equivalent to the Boltzmann constant, but expressed in units of energy (i.e. the pressure-volume product) per temperature increment per *mole* (rather than energy per temperature increment per *particle*). The constant is also a combination of the constants from Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law.

The Gas Constant (R) appears in many formulas including the following:

**Ideal Gas Law**: PV = nRT (Click any Parameter)

- Clausius-Clapeyron Equation: `ln(P_2/P_1) = (DeltaH_(vap))/R * (1/T_1 - 1/T_2)`

**R - Gas Constant:**8.3144626181532 J/(K⋅mol)**Boyle's Law Calculator**: P_{1}• V_{1}= P_{2}• V_{2}**Charles Law Calculator**: V_{1}• T_{2}= V_{2}• T_{1}**Combined Gas Law Calculator**: P•V / T= k**Gay-Lussac Law:**T_{1}•P_{2}=T_{2}•P_{1}**Ideal Gas Law**: P•V = n•R•T**Bragg's Law:**n·λ = 2d·sinθ**Hess' Law:**ΔH^{0}_{rxn}=ΔH^{0}_{a}+ΔH^{0}_{b}+ΔH^{0}_{c}+ΔH^{0}_{d}**Internal Energy**: ΔU = q + ω**Activation Energy**: E_{a}= (R*T_{1}⋅T_{2})/(T_{1}- T_{2}) ⋅ ln(k_{1}/k_{2})**Arrhenius Equation**: k = Ae^{E_a/(RT)}**Clausius-Clapeyron Equation**: ln(P_{2}/P_{1}) = (ΔH_{vap})/R * (1/T_{1}- 1/T_{2})**Compressibility Factor**: Z = (p*V_{m})/(R*T)**Peng-Robinson Equation of State**: p = (R*T)/(V_{m}- b) - (a*α)/(V_{m}^{2}+ 2*b*V_{m}- b^{2})**Reduced Specific Volume**: v_{r}= v/(R* T_{cr }/ P_{c})**Van't Hoff Equation**: ΔH^{0}= R * ( -ln(K_{2}/K_{1}))/ (1/T_{1}- 1/T_{2})

- Some descriptive text in the description of the Gas constant comes from Wikipedia: wikipedia/wiki/Gas_constant