For the following thermodynamic equilibrium chemical reaction shown below determine the overall ΔH° of the reaction first and then determine if it is endothermic, exothermic, or neither. Next determine the overall S° of the reaction then decide if the entropy (disorder) is increasing, decreasing, or no change . Next determine the Gibbs free energy ΔG° of the reaction at 1234.56°C and determine if the reaction is spontaneous, non-spontaneous, or at equilibrium. Finally calculate the equilibrium constant (K) for the reaction and determine if the equilibrium will shift to left, right, or is at equilibrium.
For the following thermodynamic equilibrium chemical reaction shown below determine the overall ΔH° of the reaction first and then determine if it is endothermic, exothermic, or neither. Next determine the overall S° of the reaction then decide if the entropy (disorder) is increasing, decreasing, or no change . Next determine the Gibbs free energy ΔG° of the reaction at 1234.56°C and determine if the reaction is spontaneous, non-spontaneous, or at equilibrium. Finally calculate the equilibrium constant (K) for the reaction and determine if the equilibrium will shift to left, right, or is at equilibrium.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.103QP
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Question
- For the following
thermodynamic equilibriumchemical reaction shown below determine the overall ΔH° of the reaction first and then determine if it is endothermic, exothermic, or neither. Next determine the overall S° of the reaction then decide if the entropy (disorder) is increasing, decreasing, or no change . Next determine the Gibbs free energy ΔG° of the reaction at 1234.56°C and determine if the reaction is spontaneous, non-spontaneous, or at equilibrium. Finally calculate the equilibrium constant (K) for the reaction and determine if the equilibrium will shift to left, right, or is at equilibrium.
PbS(s) + 4H2O2(aq) ↔ PbSO4(s) + 4H2O(L)
|
Chemical species |
ΔH (kJ/mole) |
S (J*mole/K) |
|
PbS(s) |
-98.32 |
91.34 |
|
H2O2(aq) |
-191.2 |
143.9 |
|
PbSO4(s) |
-919.9 |
148.6 |
|
H2O(L) |
-285.8 |
69.95 |
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