Temperature Dependence of Henry's Law Constant

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Henry's law was originally formulated by William Henry in 1803. This law describes the solubility of gases in liquids. Henry's law states that at constant temperature, the mole fraction of a given gas dissolved in the liquid is directly proportional to the partial pressure of that gas (i.e., , where is the total pressure, is the Henry's law constant, and is the vapor-phase mole fraction).

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The constant in Henry's law changes with the system's temperature . This is why it is preferable to name it Henry's coefficient. Multiple equations take into account the effect of temperature on this constant. Here, the following relationship is adopted [1]:

, where is in Kelvin, and , , , and are constants that depend on the chemical species considered.

The present Demonstration plots for different gaseous species in water ( is expressed in atm).

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Contributed by: Housam Binous and Ahmed Bellagi (June 2015)
Open content licensed under CC BY-NC-SA


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Reference

[1] R. H. Perry, Perry’s Chemical Engineers’ Handbook, 4th ed., New York: McGraw–Hill, 1963.



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