The third law of thermodynamics has two important consequences: it defines the sign of the entropy of any substance at temperatures above absolute zero as positive, and it provides a fixed reference point that allows us to measure the absolute entropy of any substance at any temperature.In practice, chemists determine the absolute entropy of a substance by measuring the molar heat capacity (Cp) as a function of temperature and then plotting the quantity Cp/T versus T. The area under the curve between 0 K and any temperature T is the absolute entropy of the substance at T. In contrast, other thermodynamic properties, such as internal energy and enthalpy, can be evaluated in only relative terms, not absolute terms. One way of calculating ΔS for a reaction is to use tabulated values of the standard molar entropy (S°), which is the entropy of 1 mol of a substance at a standard temperature of 298 K; the units of S° are J/(mol•K). The entropy for a phase change is just the heat (which is the reversible heat) divided by the phase transition temperature. \\ &=[1.194\;\mathrm{J/(mol\cdot K)}]+[4.434\;\mathrm{J/(mol\cdot K)}]+\Delta S_3+[-1.303\;\mathrm{J/(mol\cdot K)}]\end{align}\). Similarly, the absolute entropy of a substance tends to increase with increasing molecular complexity because the number of available microstates increases with molecular complexity. with latent heat of fusion= 339.92 kJ/kg. 1) you know delta G = delta H - TdeltaS = 0 for phase transition(ie during condensation and freezing), so at that point, delta S = deltaH/T where T is temperature in K, and T(in K) = T(in degree C) + 273. If there is heat absorbed by the reservoir at temperature , the change in entropy of the reservoir is .In general, reversible processes are accompanied by heat exchanges that occur at different temperatures. The change in entropy that accompanies the conversion of liquid sulfur to Sβ (−ΔSfus(β) = ΔS3 in the cycle) cannot be measured directly. Finally, substances with strong hydrogen bonds have lower values of S°, which reflects a more ordered structure. Unlike enthalpy or internal energy, it is possible to obtain absolute entropy values by measuring the entropy change that occurs between the reference point of 0 K [corresponding to S = 0 J/(mol•K)] and 298 K. Figure $$\PageIndex{2}$$: A Generalized Plot of Entropy versus Temperature for a Single Substance. Legal. isothermal process), �������������������� �� =� Cp ln(T2/T1) Only a perfectly ordered, crystalline substance at absolute zero would exhibit no molecular motion and have zero entropy. 19.3: Evaluating Entropy and Entropy Changes, $$\mathrm{C_8H_{18}(l)}+\dfrac{25}{2}\mathrm{O_2(g)}\rightarrow\mathrm{8CO_2(g)}+\mathrm{9H_2O(g)}$$, 19.4: Criteria for Spontaneous Change: The Second Law of Thermodynamics, Calculating ΔS from Standard Molar Entropy Values. change at constant temperature and pressure. The contents of a large change if 1kg of water at 300 C is heated to 800C at 1 Because entropy is a state function, however, ΔS3 can be calculated from the overall entropy change (ΔSt) for the Sα–Sβ transition, which equals the sum of the ΔS values for the steps in the thermodynamic cycle, using Equation 18.20 and tabulated thermodynamic parameters (the heat capacities of Sα and Sβ, ΔHfus(α), and the melting point of Sα.). Using the equation, Change in S = qrev/T, to calculate the entropy change for a substance undergoing a transition from one phase to another at its transition temperature, we need to note three facts: 1. The entropy of a reaction refers to the positional probabilities for each reactant. DSº = -50 g  333 J/g/(0 + 273.15)K = -61.0 J/K.