Van der Waals force

The molar volume, symbol V_m, is the volume occupied by one mole of a substance (chemical element or chemical compound) at a given temperature and pressure. It is equal to the molar mass (M) divided by the mass density (ρ). It has the SI unit cubic metres per mole (m³/mol), although it is more practical to use the units cubic decimetres per mole (dm³/mol) for gases and cubic centimetres per mole (cm³/mol) for liquids and solids.

The molar volume of a substance can be found by measuring its molar mass and density then applying the relation

$V_{\mathrm{m}}=\frac{M}{\rho }$.

If the sample is a mixture containing N components, the molar volume is calculated using:

$V_{\mathrm{m}}=\frac{\sum _{i=1}^N{x}_i{M}_i}{{\rho }_{\mathrm{m}\mathrm{i}\mathrm{x}\mathrm{t}\mathrm{u}\mathrm{r}\mathrm{e}}}$.

For ideal gases, the molar volume is given by the ideal gas equation: this is a good approximation for many common gases at standard temperature and pressure. For crystalline solids, the molar volume can be measured by X-ray crystallography.

Ideal gases

The ideal gas equation can be rearranged to give an expression for the molar volume of an ideal gas:

$V_{\mathrm{m}}=\frac{V}{n}=\frac{RT}{P}$.

Hence, for a given temperature and pressure, the molar volume is the same for all ideal gases and is known to the same precision as the gas constant: R = 8.314 4621(75) J mol⁻¹ K⁻¹, that is a relative standard uncertainty of 9.1×10⁻⁷, according to the 2010 CODATA recommended value. The molar volume of an ideal gas at 100 kPa (1 bar) is

22.710 980(38) dm³/mol at 0 °C

24.789 598(42) dm³/mol at 25 °C

The molar volume of an ideal gas at 1 atmosphere of pressure is

22.414 L/mol at 0 °C

24.465 L/mol at 25 °C

Crystalline solids

The unit cell volume (V_cell) may be calculated from the unit cell parameters, whose determination is the first step in an X-ray crystallography experiment (the calculation is performed automatically by the structure determination software). This is related to the molar volume by

$V_{\mathrm{m}}=\frac{N_{\mathrm{A}}{V}_{\mathrm{c}\mathrm{e}\mathrm{l}\mathrm{l}}}{Z}$

where N_A is the Avogadro constant and Z is the number of formula units in the unit cell. The result is normally reported as the "crystallographic density".

Molar volume of silicon

silicon are routinely made for the electronics industry, and the measurement of the molar volume of silicon, both by X-ray crystallography and by the ratio of molar mass to mass density, has attracted much attention since the pioneering work at NIST by Deslattes et al. (1974). The interest stems from the fact that accurate measurements of the unit cell volume, atomic weight and mass density of a pure crystalline solid provide a direct determination of the Avogadro constant. At present (2006 CODATA recommended value), the precision of the value of the Avogadro constant is limited by the uncertainty in the value of the Planck constant (relative standard uncertainty of 5×10⁻⁸).

The 2006 CODATA recommended value for the molar volume of silicon is 12.058 8349(11)×10⁻⁶ m³/mol, with a relative standard uncertainty of 9.1×10⁻⁸.

References

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See also

Interactive table of molar volumes at http://www.webelements.com/periodicity/molar_volume/

• specific volume