Starting with the standard free energies of formation from the following table, calculate the values of ΔG° and E°cell of the following reactions. Substance ΔΔG°f (kJ/mol) FeO(s) -255.2 H2(g) 0 Fe(s) 0 H2O(l) -237.2 Pb(s) 0 O2(g) 0 H2SO4(aq) -744.5 PbSO4(s) -813.0 FeO(s)+H2(g)Fe(s)+H2O(l) ΔΔG° = kJ FeO(s)+H2(g)Fe(s)+H2O(l) E°cell = V 2Pb(s)+O2(g)+2H2SO4(aq)2PbSO4(s)+2H2O(l) ΔΔG° = kJ Pb(s)+O2(g)+2H2SO4(aq)2PbSO4(s)+2H2O(l) E°cell = V
Starting with the standard free energies of formation from the following table, calculate the values of ΔG° and E°cell of the following reactions. Substance ΔΔG°f (kJ/mol) FeO(s) -255.2 H2(g) 0 Fe(s) 0 H2O(l) -237.2 Pb(s) 0 O2(g) 0 H2SO4(aq) -744.5 PbSO4(s) -813.0 FeO(s)+H2(g)Fe(s)+H2O(l) ΔΔG° = kJ FeO(s)+H2(g)Fe(s)+H2O(l) E°cell = V 2Pb(s)+O2(g)+2H2SO4(aq)2PbSO4(s)+2H2O(l) ΔΔG° = kJ Pb(s)+O2(g)+2H2SO4(aq)2PbSO4(s)+2H2O(l) E°cell = V
General Chemistry - Standalone book (MindTap Course List)
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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
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Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.105QP
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Starting with the standard free energies of formation from the following table, calculate the values of ΔG° and E°cell of the following reactions.
| Substance | ΔΔG°f (kJ/mol) |
| FeO(s) | -255.2 |
| H2(g) | 0 |
| Fe(s) | 0 |
| H2O(l) | -237.2 |
| Pb(s) | 0 |
| O2(g) | 0 |
| H2SO4(aq) | -744.5 |
| PbSO4(s) | -813.0 |
FeO(s)+H2(g)Fe(s)+H2O(l)
FeO(s)+H2(g)Fe(s)+H2O(l)
2Pb(s)+O2(g)+2H2SO4(aq)2PbSO4(s)+2H2O(l)
Pb(s)+O2(g)+2H2SO4(aq)2PbSO4(s)+2H2O(l)
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