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(GNU) Diagram: Wilfried Cordes
Figure 1: Heats of vaporization versus temperature.

The heat of vaporization, ($H_{v}$ or $H_{vap}$) is the amount of thermal energy required to convert a quantity of liquid into a vapor. It can be thought of as the energy required to break the intermolecular bonds within the liquid.

It is also often referred to as the latent heat of vaporization ($LH_{v}$ or $L_{v}$) and the enthalpy of vaporization ($\Delta H_{v}$ or $\Delta H_{vap}$ or $\Delta _{v}H$) and is usually measured and reported at the temperature corresponding to the normal boiling point of the liquid. Sometimes reported values have been corrected to a temperature of 298 K.

Measurement units

Heat of vaporization values are usually reported in measurement units such as J/mol or kJ/mol and referred to as the molar heat of vaporization, although J/g or kJ/kg are also often used. Older units such as kcal/mol, cal/g, Btu/lb and others are still used sometimes.

Temperature dependency

The heat of vaporization is not a constant. It is temperature dependent as shown in Figure 1 by the example graphs of temperature versus heat of vaporization for acetone, benzene, methanol and water.

As shown by the example graphs, the heat of vaporization of a liquid at a given temperature (other than the normal boiling point temperature) may vary significantly from the value reported at the normal boiling point of the liquid.

Estimating heat of vaporization values

Heat of vaporization, normal boiling point and critical temperature and pressure of various liquids Name Formula Hv Tn Tc pc ( J/mol ) ( °C ) ( K ) ( K ) ( atm ) Acetic acid C2H4O2 23,700 117.9 391.1 594.8 57.1 Acetone C3H6O 29,100 56.2 329.4 508.7 47.0 Benzene C6H6 30,720 80.0 353.2 562.1 48.6 Butane C4H10 22,440 – 0.5 272.7 425.2 37.5 Carbon tetrachloride CCl4 29,820 76.6 349.8 556.3 45.0 Chloroform CHCl3 29,240 61.1 334.3 536.2 54.0 Cyclohexane C6H12 29,970 80.7 353.9 553.6 40.0 Cyclopentane C5H10 27,300 49.2 322.4 511.8 44.6 Decane C10H22 38,750 174.1 447.3 617.6 20.8 Ethanol C2H6O 38,560 78.2 351.4 516.2 63.0 Hexane C6H14 28.850 68.7 341.9 507.4 29.9 Isobutane C4H10 21,300 – 11.9 261.3 408.2 36.0 Methanol CH4O 35,210 64.7 337.9 513.2 78.5 Octane C8H18 34,410 125.6 398.8 569.2 24.8 Water H20 40,660 100 373.2 647.3 218.3 Notes: (1) Hv = heat of vaporization at the normal boiling point (2) Tn = normal boiling point (3) Tc = critical temperature (4) pc = absolute critical pressure

Heats of vaporization can be measured calorimetrically and measured values are available from a number of sources. However, data is not always available for certain liquids or at certain temperatures. In such cases, estimation of heats of vaporization can be made by the three methods (among others) discussed in the following sections.

Using the Clausius-Clapeyron equation

This integrated form of the Clausius-Clapeyron equation can be used to provide a good approximation of the heat of vaporization for many pure liquids:

(1)     $\log _{e}\left({\frac {\;p_{2}}{p_{1}}}\right)={\frac {\;H_{v}}{R}}\left({\frac {1}{T_{2}}}-{\frac {1}{T_{1}}}\right)$

which can be re-arranged to obtain:

(2)     $H_{v}=R\cdot \log _{e}\left({\frac {\;p_{2}}{p_{1}}}\right)\left({\frac {\;T_{1}\cdot T_{2}}{T_{2}-T_{1}}}\right)$

where:
$H_{v}$	= Heat of vaporization, in J/mol
$R$	= 8.3144 = Universal gas constant, in J/(K $\cdot$ mol)
$log_{e}$	= Logarithm on base $e$
$p_{1}$	= The liquid's vapor pressure at $T_{1}$, in atm
$p_{2}$	= The liquid's vapor pressure at $T_{2}$, in atm
$T_{1}$	= Temperature, in K
$T_{2}$	= Temperature, in K

The primary Clausius-Clapeyron equation is exact. However, the above integrated form of the equation is not exact because it is necessary to make these assumptions in order to perform the integration:

• The molar volume of the liquid phase is negligible compared to the molar volume of the vapor phase
• The vapor phase behaves like an ideal gas
• The heat of vaporization is constant over the temperature range as defined by T₁ and T₂

Using Trouton's rule

Troutons's equation, often referred to as Trouton's rule, also provides good approximations for many pure substances. It may be expressed as:

(3)     ${\frac {H_{v}}{T_{n}}}\approx 87-88$