Abstract
Vapour pressure measurements may be undertaken for a variety of reasons, for example, the nature of a surface and its influence on evaporation and condensation may be studied as may also the diffusion coefficient of the evaporated species in air. Also information on differential vapour pressures is used to calculate molecular weights and the thermodynamic functions of solutions. From the point of view of the thermochemist, however, the temperature variation of a vapour pressure is measured so as to obtain indirectly an enthalpy of vaporisation (ΔHv) or sublimation (ΔHs). This may be combined with a standard enthalpy of formation to give a gas phase enthalpy of formation, which since it does not contain energy terms for the cohesive forces within the material, may be used to calculate bond enthalpies. Also vapour pressure measurements may be used to calculate Kp for a reaction and from Kp and its temperature variation, the standard free energy, enthalpy and entropy changes accompanying the reaction may be found. Further, if free energy functions or partition functions for the constituents are available from heat capacity or spectroscopic data, then an enthalpy change may be calculated from a single value of Kp. The two ways of handling Kp are often referred to as the “second law” and “third law” methods respectively.
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Carson, A.S. (1984). The Measurement of Vapour Pressure. In: Ribeiro da Silva, M.A.V. (eds) Thermochemistry and Its Applications to Chemical and Biochemical Systems. NATO ASI Series, vol 119. Springer, Dordrecht. https://doi.org/10.1007/978-94-009-6312-2_7
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DOI: https://doi.org/10.1007/978-94-009-6312-2_7
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