Abstract
In Chapter 3, the statement was made that almost all chemical reactions can proceed in both the forward and reverse directions. However, the extent of the reverse reaction for many reactions is so small that they can be regarded as going to completion. When both the forward and reverse reactions are measurable, the process is called a reversible reaction. (This definition of a reversible reaction should not be confused with the term reversible used in a thermodynamic process. In a thermodynamic reversible process the reactions occur at an infinitely slow rate, while the reactions for a chemical reaction are spontaneous and, therefore, occur at a finite rate.) Looking at a system at chemical equilibrium on a macro scale, there is no change in composition with time if there is no change in temperature or pressure. This does not mean that the system is static; in fact, it is dynamic on a micro scale. The forward and reverse reactions continue, but their rates of change are equal. Therefore, the statement can be made that a system can be considered to be standing still while in a continuous state of flux. In order to arrive at the necessary relationships describing the equilibrium constant either a kinetic (state of flux) or a thermodynamic (standing still) approach can be taken.
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Keywords
- Gibbs Free Energy
- Equilibrium Constant
- Activity Coefficient
- High Pressure Liquid Chromatography
- Weak Acid
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Streng, W.H. (2001). Equilibrium Constants. In: Characterization of Compounds in Solution. Springer, Boston, MA. https://doi.org/10.1007/978-1-4615-1345-2_4
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DOI: https://doi.org/10.1007/978-1-4615-1345-2_4
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