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Nernst Heat Theorem
Additional recommended knowledge
The Nernst heat theorem says that as absolute zero is approached, the entropy change ΔS for a chemical or physical change approaches 0. This can be expressed mathematically as follows:
Another way of looking at the theorem is to start with the definition of the Gibbs free energy (G), G = H - TS, where H stands for enthalpy. For a change from reactants to products at constant temperature and pressure the equation becomes ΔG = ΔH − TΔS.
In the limit of T = 0 the equation reduces to ΔG = ΔH, as illustrated in the figure shown here, which is supported by experimental data. However, it is known from thermodynamics that the slope of the ΔG curve is -ΔS. Since the slope shown here reaches the horizontal limit of 0 as T → 0 then the implication is that ΔS → 0, which is the Nernst heat theorem.
The significance of the Nernst heat theorem is that it was later developed by Max Planck into what is now regarded as the third law of thermodynamics, that the entropy of all pure, homogeneous materials is 0 at T = 0.
For further reading
References and notes
|This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Nernst_Heat_Theorem". A list of authors is available in Wikipedia.|