Using the given data, calculate the change in Gibbs free energyfor each of the following reactions. In each case indicate whetherthe reaction is spontaneous at 298 K under standard conditions.
Part A: 2Ag (s) + Cl2 (g) --> 2AgCl (s) Gibbs free energy forAgCl (s) is -109.70 kJ/mol
Part B: spontaneous or nonspontaneous
Part C: P4O10 (s) + 16H2 (g) --> 4PH3 (g) + 10H2O (g)
Gibbs free energy for P4O10 (s) is -2675.2 kJ/mol
Gibbs free energy for PH3 (g) is 13.4 kJ/mol
Gibbs free energy for H2O (g) is -228.57 kJ/mol
Part D: spontaneous or nonspontaneous
Part E: CH4 (g) + 4F2 (g) --> CF4 (g) + 4HF (g)
Gibbs free energy for CH4 (g) is -50.8 kJ/mol
Gibbs free energy for CF4 (g) is -635.1 kJ/mol
Gibbs free energy for HF (g) is -270.70 kJ/mol
Part F: spontaneous or nonspontaneous
Part G: 2H2O2 (l) --> 2H2O (l) + O2 (g)
Gibbs free energy for H2O2 (l) is -120.4 kJ/mol
Gibbs free energy for H2O (l) is -237.13 kJ/mol
Part H: spontaneous or nonspontaneous
