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5. Given the following reactions: P:(8) + 502(g) 2H2(g) + O2(g) → 2H2O(g) 6H2O(g) + P4O10(s) - P4O10 (s) -2697.0 kJ/mol AG° = -457.18 kJ/mol AG° = -428.66 kJ/mol AG + 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.

5. Given the following reactions: P:(8) + 502(g) 2H2(g) + O2(g) → 2H2O(g) 6H2O(g) + P4O10(s) - P4O10 (s) -2697.0 kJ/mol AG° = -457.18 kJ/mol AG° = -428.66 kJ/mol AG + 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.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.62QE: A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup...
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5. Given the following reactions: P:(8) + 502(g) = -2697.0 kJ/mol AG° = -457.18 kJ/mol AG° = -428.66 kJ/mol - P,O10 (s) 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?
Transcribed Image Text:5. Given the following reactions: P:(8) + 502(g) = -2697.0 kJ/mol AG° = -457.18 kJ/mol AG° = -428.66 kJ/mol - P,O10 (s) 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?
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