AG can also be calculated from tabulated values of AG Work through Example 12.8a. Then use the data below to calculate A

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AG can also be calculated from tabulated values of AG Work through Example 12.8a. Then use the data below to calculate AG using free energies of formation. NO(g) + O₂(g) → NO₂(g) Compound AG /mol) 87.6 0 51.3 NO(g) O₂(g) NO₂(g)
Using Standard Free Energies of Formation to Calculate AG Consider the decomposition of yellow mercury(II) oxide. HgO(s, yellow) 02(8) Calculate the standard free energy change at room temperature, AG, using (a) standard free energies of formation and (b) standard enthalples of formation and standard entropies. Do the results indicate the reaction to be spontaneous or nonspontaneous under standard conditions? Solution The required data are available in Appendix G and are shown here. AG; (kJ/mol) Compound HgO (s, yellow) Hg() O₂(g) (a) Using free energies of formation: -58.43 0 0 Hg(1) + AH; (kJ/mol) -90.46 0 0 S° (J/K-mol) 71.13 75.9 205.2
(a) Using free energies of formation: AG=VG (products) - VAG;(reactants) = [1AGHg() + AG0₂(8)] - IAG;HgO(s, yellow) = [1 mol(0 kJ/mol) +mol(0 kJ/mol)] - 1 mol(-58.43 kJ/mol) = 58.43 kJ/mol (b) Using enthalpies and entropies of formation: AH = VAH; (products) - VAH; (reactants) = [1AH;Hg(1) + AH;0₂(8)] AH;02(8)] - 1AH;HgO(s, yellow) = [10 1 mol(0 kJ/mol) +mol(0 kJ/mol) 2 - - 1 mol(-90.46 kJ/mol) = 90.46 kJ/mol AS = VAS (products) - VAS (reactants)
= [1AS Hg() + AS O₂(g)] - 1AS HgO(s, yellow) K)] K)] - 1 mol(71.13 J/mol K) = 107.4 J/mol K =1₁ 1 mol (75.9 J/mol K) +mol(205.2 J/mol AG° = AH° - TAST = 90.46 kJ - 298.15 K × 107.4 J/K-mol x 1 kJ 1000 J AG (90.46 32.01) kJ/mol = 58.45 kJ/mol Both ways to calculate the standard free energy change at 25 °C give the same numerical value (to three significant figures), and both predict that the process is nonspontaneous (not spontaneous) at room temperature. Check Your Learning Calculate AG using (a) free energies of formation and (b) enthalpies of formation and entropies (Appendix G). Do the results indicate the reaction to be spontaneous or nonspontaneous at 25 °C? C₂H4(8) - H₂(g) + C₂H₂(g)