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On the early thermodynamic and kinetic deductions of the equilibrium constant equation

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Abstract

After briefly presenting the first formulation of the equilibrium constant stated by Guldberg and Waage, this study examines the early thermodynamic and kinetic deductions of the equilibrium law. Firstly, it is discussed how Horstmann applied the concept of entropy to chemical equilibrium reactions, which meant the first thermodynamic explanation of the Guldberg-Waage law of mass action proposed in 1864. A different theoretical derivation of the equilibrium constant came from the works of van’t Hoff. This study analyses the first accurate kinetic treatment of equilibrium reactions as well as van’t Hoff’s imaginative thermodynamic foundation of the constant ratios in chemical equilibrium systems.

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Notes

  1. Page 1046.

  2. Page 10.

  3. Page 74.

  4. Page 555.

  5. Page 46.

  6. Page 550.

  7. Page 282.

  8. Page 21.

  9. Page 205.

  10. Page 77.

  11. Page 77.

  12. Page 81.

  13. Page 78.

  14. A point of clarification must be made in the presentation of Eq. (7). In this case, Q stands for the reaction quotient corresponding to the equilibrium equation that represents the chemical equilibrium system. Thus, in this expression, Q does not represent the heat of reaction.

  15. Page 240.

  16. Page 144.

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  19. Pages 223–224.

  20. Page 254.

  21. Page 228.

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  1. Department of Education, University Jaume I, 12071, Castelló de la Plana, Spain

    Juan Quílez

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Quílez, J. On the early thermodynamic and kinetic deductions of the equilibrium constant equation. Found Chem 23, 85–103 (2021). https://doi.org/10.1007/s10698-020-09376-2

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