Heat of vaporization
The heat of vaporization, (Hv or Hvap) 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 (LHv or Lv) and the enthalpy of vaporization (ΔHv or ΔHvap or ΔvH) 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
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
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 any of a large number of different methods. Four of the commonly used methods are discussed in the following sections.
 Using the Clausius-Clapeyron equation
which can be re-arranged to obtain:
where: Hv = Heat of vaporization, in J/mol R = 8.3144 = Universal gas constant, in J/(K mol) loge = Logarithm on base e p1 = The liquid's vapor pressure at T1, in atm p2 = The liquid's vapor pressure at T2, in atm T1 = Temperature, in K T2 = 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
As an example of using the Clausius-Clapeyron equation, given that the vapor pressure of benzene is 1 atm at 353 K and 2 atm at 377 K, benzene's heat of vaporization is obtained as 32,390 J/mol within that temperature range.
 Using Riedel's equation
where: Hv = Heat of vaporization, in J/mol R = 8.3144 = Universal gas constant, in J/(K mol) Tn = The liquid's normal boiling point, in K Tc = The liquid's critical temperature, in K loge = Logarithm on base e pc = The liquid's critical pressure at Tn, in bar 
For an empirical expression, equation (3) is surprisingly accurate and its error rarely exceeds 5 %. For example, using water data (see Table 1) of Tn = 373.2 K,
Tc = 647.3 K and Pc = 221.2 bar (218.3 atm), the heat of vaporization is obtained as 42,060 J/mol. That is within 3 percent of the 40,660 J/mol in Table 1.
 Using Trouton's rule
Troutons's rule, dating back to 1883, is a relation between a liquid's heat of vaporization and it's normal boiling point Tn. It provides a good approximation of the heat of vaporization at the normal boiling point of many pure substances, and it may be expressed as:
Table 2 provides some examples of the application of Trouton's rule.
Trouton's rule fails for liquids with boiling points below 150 K. It also fails for water, alcohols, amines and liquid ammonia.
 Using Watson's equation
which can be re-arranged to obtain:
where: Hv1 = Heat of vaporization of the liquid at T1, in J/mol Hv2 = Heat of vaporization of the liquid at T2, in J/mol T1 = Temperature, in K T2 = Temperature, in K Tc = Critical temperature of the liquid, in K
Watson's equation has achieved wide acceptance and is simple and reliable.
- ↑ 1.0 1.1 Dortmund Data Bank Online Search
- ↑ Carl L. Yaws (1998). Chemical properties Handbook, 1st Edition. McGraw-Hill. ISBN 0-07--073401-1.
- ↑ Václav Svoboda and Henry V. Kehiaian (1985). Enthalpies of Vaporization of Organic Compounds: A Critical Review and Data Compilation, IUPAC Chemical Data Series 32. Blackwell Scientific. ISBN 0-632-01529-2.
- ↑ Perry, R.H. and Green, D.W. (Editors) (2007). Perry's Chemical Engineers' Handbook, Eighth Edition. McGraw-Hill. ISBN 0-07-142294-3.
- ↑ 5.0 5.1 5.2 5.3 Jean Vidal (2003). Thermodynamics: Applications in Chemical Engineering and the Petroleum Industry. Editions Technip. ISBN 2-7108-0800-5. (Equation 2.10, page 38)
- ↑ 6.0 6.1 6.2 Amir Faghri and Yuwen Zhang (2006). Transport Phenomena in Multiphase Systems, 1st Edition. Academic Press. ISBN 0-12-370610-6. (Equation 2.168, Chapter 2)
- ↑ 7.0 7.1 7.2 J.M. Smith, H.C. Van Ness and M.M. Abbot (2004). Introduction to Chemical Engineering Thermodynamics, 7th Edition. McGraw-Hill. ISBN 0-07-310445-0.
- ↑ Robert C. Weast (Editor) (1976). Handbook of Chemistry and Physics=56th Edition. CRC Press. ISBN 0-87819-455-X.
- ↑ L. Riedel, Chem. Ing. Tech., 26, pp. 679-683, 1954
- ↑ M.M. Abbott and H.C. Van Ness (1989). Schaum's Outline of Thermodynamics With Chemical Applications, 2nd Edition. McGraw-Hill. ISBN 0-07-000042-5.
- ↑ 1 bar = 0.98692 atm
- ↑ F.T. Trouton, Nature, 27, p. 292, 1883
- ↑ F.T. Trouton, Phil. Mag., 18, pp.54-57, 1884
- ↑ 14.0 14.1 Bimalendu Narayan Roy (2002). Fundamentals of Classical and Statistical Thermodynamics. John Wiley & Sons. ISBN 0-470-84316-0.
- ↑ K.M. Watson, Thermodynamics of the Liquid States, Generalized Prediction of Properties, Ind. Eng. Chem., 35, pp.398-406, 1943
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