Enthalpy and the Second Law of Thermodynamics
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David Keifer [1]
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[1] Salisbury University
Salisbury University
Estados Unidos
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- Localización: Journal of chemical education, ISSN 0021-9584, Vol. 96, Nº 7, 2019, págs. 1407-1411
- Idioma: inglés
- Texto completo no disponible (Saber más ...)
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Resumen
The change in enthalpy of a chemical reaction conducted at constant pressure is equal to the heat of the reaction plus the nonexpansion work of the reaction, ΔH = qP + wadditional. After deriving that relationship, most general and physical chemistry textbooks set wadditional = 0 to arrive at the claim that ΔH = qP, and nearly all further discussion of enthalpy assumes that ΔH = qP. Setting wadditional = 0 is viable for spontaneous reactions, but for nonspontaneous reactions, wadditional ≠ 0 as a consequence of the second law of thermodynamics. Therefore, ΔH ≠ qP for nonspontaneous reactions. Moreover, nonexpansion work is important for many interesting and important spontaneous reactions in biology (e.g., muscular movement, nerve signal transmission) and in modern society (e.g., batteries); incorporating wadditional into ΔH allows for a more accurate discussion of the energy flow in these reactions. In this paper, I show that ΔH ≠ qP for nonspontaneous reactions, and I discuss how ΔH must be partitioned between qP and wadditional for several kinds of reactions according to the second law of thermodynamics. Finally, I suggest how the discussion of enthalpy could be corrected in general and physical chemistry textbooks.
