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The Enthalpy of vaporization, also called the latent heat of vaporization is the change in the enthalpy needed to change an amount of liquid into a gas. It happens at a given pressure. The enthalpies of vaporization are usually measured at the normal boiling point for that substance. The units are usually J/mol.
An example is when the cooling effects of vaporization controls the body temperature of humans. Warm weather or exercise creates heat in the body. This causes the body to sweat (or perspire). The body feels cooler when the liquid sweat evaporates. As the humidity increases, the rate of evaporation decreases. This determines the body's comfort level.
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Temperature-dependency of the heats of vaporization for water, methanol, benzene, and acetone.
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Molar enthalpy of zinc above 298.15 K and at 1 atm pressure, showing discontinuities at the melting and boiling points. The enthalpy of melting (ΔH°m) of zinc is 7323 J/mol, and the enthalpy of vaporization (ΔH°v) is 115 330 J/mol.
