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8. A reaction has AH° = 100 kJ/mol and AS°=250 J/mol-K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?

8. A reaction has AH° = 100 kJ/mol and AS°=250 J/mol-K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?

General Chemistry - Standalone book (MindTap Course List)
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
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.132QP
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5. Given the following reactions: P:(8s) + 502(9) - PĄO10 (s) = -2697.0 kJ/mol AG° = -457.18 kJ/mol AG° = -428.66 kJ/mol AG 2H2(9) + O2(9) - 2H2O(g) 6H2O(g) + P4O10(s) → 4H3PO4(1) (a) Determine the standard free energy of formation, AG°F, for phosphoric acid. (b) How does your calculated result compare to the constant thermodynamic value from the table? Explain. 6. Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it is converted to sulfur by the reaction: 2H2S(g) + SO2(g) Ss(s, rhombic) + 2H2O(1) What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic? 7. Determine the standard free energy change, AGfº, for the formation of S (aq) given that the AGF° for Ag*(ag) and Ag:S(s) are 77.1 kJ/mole and -39.5 kJ/mole respectively, and the solubility product for A92S(s) is 8 xx 10-51. 8. A reaction has AH° = 100 kJ/mol and AS°=250 J/mol-K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?
Transcribed Image Text:5. Given the following reactions: P:(8s) + 502(9) - PĄO10 (s) = -2697.0 kJ/mol AG° = -457.18 kJ/mol AG° = -428.66 kJ/mol AG 2H2(9) + O2(9) - 2H2O(g) 6H2O(g) + P4O10(s) → 4H3PO4(1) (a) Determine the standard free energy of formation, AG°F, for phosphoric acid. (b) How does your calculated result compare to the constant thermodynamic value from the table? Explain. 6. Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it is converted to sulfur by the reaction: 2H2S(g) + SO2(g) Ss(s, rhombic) + 2H2O(1) What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic? 7. Determine the standard free energy change, AGfº, for the formation of S (aq) given that the AGF° for Ag*(ag) and Ag:S(s) are 77.1 kJ/mole and -39.5 kJ/mole respectively, and the solubility product for A92S(s) is 8 xx 10-51. 8. A reaction has AH° = 100 kJ/mol and AS°=250 J/mol-K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?
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