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 (a) FeO (s) + H2 (g) -----> Fe (s) + H2O (l)
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 (a) FeO (s) + H2 (g) -----> Fe (s) + H2O (l)
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Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.43QP: The free energy of formation of one mole of compound refers to a particular chemical equation. For...
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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 |
(a) FeO (s) + H2 (g) -----> Fe (s) + H2O (l)
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