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The Antoine equation[1] is a vapor pressure equation and describes the relation between vapor pressure and temperature for pure components. The Antoine equation is derived from the Clausius–Clapeyron relation.

## The equation

$\log_{10} p = A-\frac{B}{C+T}.$

where p is the vapor pressure, T is temperature and A, B and C are component-specific constants.

The simplified form with C set to zero:

$\log_{10} p = A-\frac{B}{T}$

is named the August equation, after the German physicist Ernst Ferdinand August (1795–1870). The August equation describes a linear relation between the logarithm of the pressure and the reciprocal temperature. This assumes a temperature-independent heat of vaporization. The Antoine equation allows an improved, but still inexact description of the change of the heat of vaporization with the temperature.

The Antoine equation can also be transformed in a temperature-explicit form with simple algebraic manipulations:

$T = \frac{B}{A-\log_{10}\, p} - C$

## Validity range

Usually, the Antoine equation cannot be used to describe the entire saturated vapour pressure curve from the triple point to the critical point, because it is not flexible enough. Therefore, multiple parameter sets for a single component are commonly used. A low-pressure parameter set is used to describe the vapour pressure curve up to the normal boiling point and the second set of parameters is used for the range from the normal boiling point to the critical point.

## Example parameters

A B C T min.

°C

T max

°C

Water 8.07131 1730.63 233.426 1 100
Water 8.14019 1810.94 244.485 99 374
Ethanol 8.20417 1642.89 230.300 -57 80
Ethanol 7.68117 1332.04 199.200 77 243

The constants are given in °C and mmHg.

### Example calculation

The normal boiling point of ethanol is TB = 78.32 °C.

$P = 10^{(8{.}20417 - \frac{1642{.}89}{78{.}32 + 230{.}300})} = 760{.}0\ \mathrm{mmHg}$
$P = 10^{(7{.}68117 - \frac{1332{.}04}{78{.}32 + 199{.}200})} = 761{.}0\ \mathrm{mmHg}$

(760 mmHg = 101.325 kPa = 1.000 atm = normal pressure)

This example shows a severe problem caused by using two different sets of coefficients. The described vapor pressure is not continuous—at the normal boiling point the two sets give different results. This causes severe problems for computational techniques which rely on a continuous vapor pressure curve.

Two solutions are possible: The first approach uses a single Antoine parameter set over a larger temperature range and accepts the increased deviation between calculated and real vapor pressures. A variant of this single set approach is using a special parameter set fitted for the examined temperature range. The second solution is switching to another vapor pressure equation with more than three parameters. Commonly used are simple extensions of the Antoine equation (see below) and the equations of DIPPR or Wagner.[2][3]

## Units

The coefficients of Antoine's equation are normally given in mmHg—even today where the SI is recommended and pascals are preferred. The usage of the pre-SI units has only historic reasons and originates directly from Antoine's original publication.

It is however easy to convert the parameters to different pressure and temperature units. For switching from degrees Celsius to kelvin it is sufficient to subtract 273.15 from the C parameter. For switching from millimeters of mercury to pascals it is sufficient to add the common logarithm of the factor between both units to the A parameter:

$A_{\mathrm{Pa}} = A_{\mathrm{mmHg}} + \log_{10}\frac{101325}{760} = A_{\mathrm{mmHg}} + 2.124903.$

The parameters for °C and mmHg for ethanol

A B C
8.20417 1642.89 230.300

are converted for K and Pa to

A B C
10.32907 1642.89 -42.85

The first example calculation with TB = 351.47 K becomes

$\log_{10}(P) = 10{.}3291 - \frac{1642{.}89}{351{.}47 - 42{.}85} = 5{.}005727378 = \log_{10}(101328\ \mathrm{Pa}).$

A similarly simple transformation can be used if the common logarithm should be exchanged by the natural logarithm. It is sufficient to multiply the A and B parameters by ln(10) = 2.302585.

The example calculation with the converted parameters (for K and Pa):

A B C
23.7836 3782.89 -42.85

becomes

$\ln P = 23{.}7836 - \frac{3782{.}89}{351{.}47 - 42{.}85} = 11{.}52616367 = \ln(101332\,\mathrm{Pa}).$

(The small differences in the results are only caused by the used limited precision of the coefficients).

## Extension of the Antoine equations

To overcome the limits of the Antoine equation some simple extension by additional terms are used:

• $P = \exp{\left( A + \frac{B}{C+T} + D \cdot T + E \cdot T^2 + F \cdot \ln \left( T \right) \right)}$
• $P = \exp\left( A + \frac{B}{C+T} + D \cdot \ln \left( T \right) + E \cdot T^F\right).$

The additional parameters increase the flexibility of the equation and allow the description of the entire vapor pressure curve. The extended equation forms can be reduced to the original form by setting the additional parameters D, E and F to 0.

A further difference is that the extended equations use the e as base for the exponential function and the natural logarithm. This doesn't affect the equation form.

## References

1. ^ Antoine, C. (1888), "Tensions des vapeurs; nouvelle relation entre les tensions et les températures" [Vapor Pressure: a new relationship between pressure and temperature], Comptes Rendus des Séances de l'Académie des Sciences (in French) 107: 681–684, 778–780, 836–837
2. ^ Wagner, W. (1973), "New vapour pressure measurements for argon and nitrogen and an new method for establishing rational vapour pressure equations", Cryogenics 13 (8): 470–482
3. ^ Reid, R. C., Properties of Gases and Liquids (3rd ed.)
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