AP Chemistry
9.5 Free Energy and Equilibrium
9.3 Gibbs Free Energy and Thermodynamic Favorability
The decomposition of sulfuryl chloride gas is represented by the following equation:
\[\text{SO}_2\text{Cl}_2(g) \rightleftharpoons \text{SO}_2(g) + \text{Cl}_2(g)\]
For this reaction, \(\Delta H^\circ = +90\text{ kJ/mol}_{\text{rxn}}\) and \(\Delta S^\circ = +150\text{ J/(mol}_{\text{rxn}}\cdot\text{K)}\). Which of the following correctly predicts the sign of \(\Delta G^\circ\) and the relative magnitude of the equilibrium constant, \(K\), as the temperature of the reaction system is changed from \(500\text{ K}\) to \(700\text{ K}\)?
\[\text{SO}_2\text{Cl}_2(g) \rightleftharpoons \text{SO}_2(g) + \text{Cl}_2(g)\]
For this reaction, \(\Delta H^\circ = +90\text{ kJ/mol}_{\text{rxn}}\) and \(\Delta S^\circ = +150\text{ J/(mol}_{\text{rxn}}\cdot\text{K)}\). Which of the following correctly predicts the sign of \(\Delta G^\circ\) and the relative magnitude of the equilibrium constant, \(K\), as the temperature of the reaction system is changed from \(500\text{ K}\) to \(700\text{ K}\)?
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