Nernst Heat Theorem
Nernst Heat Theorem
In 1906, Walther Nernst, studied the variation of enthalpy change and free energy change as a function of temperature. His results known as Nernst heat theorem.
Gibbs Helmholtz equation-
It is obvious from the above equation that the free energy change will become equal to the enthalpy change when the temperature is reduced to absolute zero i.e.
ΔF = ΔH at T = 0.
Nernst also noted that the magnitude of δ(ΔF)/δT decreases gradually and approaches the zero with the decrease of temperature.
In other words, Nernst observed that as the temperature is decreased continuously, the Gibbs free energy change was decreasing while the enthalpy change was increasing gradually with the same magnitude. Therefore, the change in slope in both curves must become zero near absolute zero. Mathematically represented as-
and graph may be plotted as-
We know that variation of free energy change with the temperature at constant pressure is equal to the negative of entropy change and Also, from the definition of change in the heat capacity, we have-
After putting the values of equation-2 and equation-3 in equation-1, we get-
(Limit T → 0), ΔS = 0 and
(Limit T → 0), ΔCP = 0
Hence, all processes should occur without entropy and heat capacity changes in the vicinity of absolute zero.
This is Nernst Heat Theorem. Since gases and liquid does not exist at absolute zero, Hence, this theorem is applicable only to solid.
