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.
General Chemistry - Standalone book (MindTap Course List)
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Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.97QP: When 1.000 g of gaseous butane, C4H10, is burned at 25C and 1.00 atm pressure, H2O(l) and CO2(g) are...
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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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