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2.8 Thermodynamic potentials

Take-home message: Other quantities can be defined which, under common experimental conditions, are more relevant than the energy.

Let's look again at the fundamental thermodynamic relation for a hydrodynamic system: ${\rm d}E=T{\rm d}S-P{\rm d}V$.

This suggests that the natural variable in which to express $E$ are $S$ and $V$: $E=E(S,V)$. That means that energy will be unchanged for processes at constant volume and entropy--not the most common experimental conditions. It is useful to introduce other functions of state, called ``thermodynamic potentials'', which are conserved, or whose change is easily calculated, in common experimental conditions.

These are

Note that Enthalpy and Gibbs free energy are only relevant to hydrodynamic systems for which $ {}\raise0.44ex\hbox{\bf\symbol{'040}}\llap{d}W^{\rm rev}=-P{\rm d}V$. However the energy and the Helmholtz free energy is more general, with ${\rm d}E= T{\rm d}S+ {}\raise0.44ex\hbox{\bf\symbol{'040}}\llap{d}W^{\rm rev}$ and ${\rm d}F=-S{\rm d}T+ {}\raise0.44ex\hbox{\bf\symbol{'040}}\llap{d}W^{\rm rev}$

References


next up previous contents index
Next: 2.9 The approach to equilibrium Previous: 2.7 The Fundamental Thermodynamic Relation
Judith McGovern 2004-03-17