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Ch.18 - Free Energy and Thermodynamics
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.18 - Free Energy and ThermodynamicsProblema 55d
Capitolo 18, Problema 55d

Use data from Appendix IIB to calculate ΔS°rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°rxn. d. 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g)

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1
Identify the standard entropy values (S°) for each reactant and product from Appendix IIB.
Write the balanced chemical equation: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g).
Calculate the total standard entropy of the reactants: (2 * S°(H2S)) + (3 * S°(O2)).
Calculate the total standard entropy of the products: (2 * S°(H2O)) + (2 * S°(SO2)).
Determine the change in standard entropy (ΔS°rxn) using the formula: ΔS°rxn = ΣS°(products) - ΣS°(reactants).

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Standard Entropy (ΔS°)

Standard entropy (ΔS°) is a measure of the disorder or randomness in a system at standard conditions (1 atm, 25°C). It quantifies the amount of energy that is unavailable to do work due to the dispersal of energy among the particles in a substance. Higher entropy values indicate greater disorder, while lower values suggest more order.
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Standard Molar Entropy

Entropy Change in Reactions

The change in entropy (ΔS°rxn) for a chemical reaction is calculated by considering the difference in standard entropies of the products and reactants. It is given by the equation ΔS°rxn = ΣS°(products) - ΣS°(reactants). A positive ΔS°rxn indicates an increase in disorder, while a negative value suggests a decrease in disorder during the reaction.
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Entropy in Phase Changes

Rationalizing the Sign of ΔS°rxn

Rationalizing the sign of ΔS°rxn involves analyzing the physical states and the number of moles of reactants and products. Generally, reactions that produce gases from solids or liquids, or increase the number of gas molecules, tend to have a positive ΔS°rxn. Conversely, reactions that produce fewer gas molecules or convert gases to liquids or solids typically exhibit a negative ΔS°rxn.
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Spontaneity of Reactions
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