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Ch.19 - Chemical Thermodynamics
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.19 - Chemical ThermodynamicsProblema 104b
Capitolo 19, Problema 104b

The reaction SO2(g) + 2 H2S(g) ⇌ 3 S(s) + 2 H2O(g) is the basis of a suggested method for removal of SO2 from power-plant stack gases. The standard free energy of each substance is given in Appendix C. (b) In principle, is this reaction a feasible method of removing SO2?

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1
Identify the standard free energy of formation (\( \Delta G^\circ_f \)) for each substance involved in the reaction from Appendix C.
Write the balanced chemical equation: \( \text{SO}_2(g) + 2 \text{H}_2\text{S}(g) \rightleftharpoons 3 \text{S}(s) + 2 \text{H}_2\text{O}(g) \).
Calculate the standard free energy change (\( \Delta G^\circ \)) for the reaction using the formula: \( \Delta G^\circ = \sum \Delta G^\circ_f(\text{products}) - \sum \Delta G^\circ_f(\text{reactants}) \).
Determine the sign of \( \Delta G^\circ \). If \( \Delta G^\circ < 0 \), the reaction is spontaneous under standard conditions, suggesting feasibility.
Discuss the implications of the \( \Delta G^\circ \) value in terms of the reaction's feasibility for removing \( \text{SO}_2 \) from power-plant stack gases.

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Gibbs Free Energy

Gibbs Free Energy (G) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. A negative change in Gibbs Free Energy (ΔG) indicates that a reaction is spontaneous and can occur without external energy input. Understanding ΔG is crucial for assessing the feasibility of chemical reactions, such as the removal of SO₂ in this context.
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Gibbs Free Energy of Reactions

Equilibrium Constant

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. It provides insight into the position of equilibrium and the extent to which a reaction proceeds. For the reaction in question, analyzing K can help determine whether the formation of products (S and H₂O) is favored over the reactants (SO₂ and H₂S), indicating the feasibility of SO₂ removal.
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Equilibrium Constant K

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle is essential for understanding how changes in concentration, pressure, or temperature can affect the reaction's direction and feasibility, particularly in the context of removing SO₂ from stack gases.
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Le Chatelier's Principle
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Domanda del libro di testo

The reaction SO2(g) + 2 H2S(g) ⇌ 3 S(s) + 2 H2O(g) is the basis of a suggested method for removal of SO2 from power-plant stack gases. The standard free energy of each substance is given in Appendix C. (a) What is the equilibrium constant for the reaction at 298 K? (c) If PSO2 = PH2S and the vapor pressure of water is 25 torr, calculate the equilibrium SO2 pressure in the system at 298 K.

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Consider the following equilibrium: N2O4(g) ⇌ 2 NO2(g) Thermodynamic data on these gases are given in Appendix C. You may assume that ΔH° and ΔS° do not vary with temperature. (a) At what temperature will an equilibrium mixture contain equal amounts of the two gases?

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Domanda del libro di testo

The reaction SO2(g) + 2 H2S(g) ⇌ 3 S(s) + 2 H2O(g) is the basis of a suggested method for removal of SO2 from power-plant stack gases. The standard free energy of each substance is given in Appendix C. (d) Would you expect the process to be more or less effective at higher temperatures?

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At what temperatures is the following reaction, the reduction of magnetite by graphite to elemental iron, spontaneous? Fe3O4(s) + 2 C(s, graphite) → 2 CO2(g) + 3 Fe(s)

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Domanda del libro di testo

When most elastomeric polymers (e.g., a rubber band) are stretched, the molecules become more ordered, as illustrated here:

Suppose you stretch a rubber band. (a) Do you expect the entropy of the system to increase or decrease?

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