D9.1 Standard Entropy Values
Consider the entropy of a pure, perfectly crystalline solid possessing no kinetic energy (that is, at a temperature of absolute zero, 0 K). This system may be described by a single microstate, as its purity, perfect crystallinity and complete lack of motion means there is but one possible energy configuration (W = 1). Therefore, the entropy of this system is zero:
This limiting condition for a system’s entropy represents the third law of thermodynamics: the entropy of a pure, perfect crystalline substance at 0 K is zero.
) to determine the temperature dependence of a substance’s entropy and to derive absolute entropy values at higher temperatures. (Note that, unlike enthalpy values, the third law of thermodynamics identifies a zero point for entropy. Therefore, there is no need for formation entropy, and all substances, including elements in their most stable states, have an absolute entropy.)Standard entropy (S°) values are the absolute entropies per mole of substance at a pressure of 1 bar. For aqueous ions, where the ions also influence the entropy of nearby water molecules, the standard entropy values are reported at 1 M concentrations relative to that of H+(aq), which is set to S° = 0 by convention.
The standard entropy change (ΔrS°) for any chemical process may be computed from the standard entropy of its reactant and product species:
The thermodynamics table in the appendix lists standard entropies of select elements and compounds at 298.15 K.
Exercise: Standard Entropy Change
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