Using given data, calculate the change in Gibbs free energy for each of the following reactions. In each case indicate whether the reaction is spontaneous at 298K under standard conditions.

Part A: 2Ag (s) + Cl2 (g) --> 2AgCl (s) Gibbs free energy for AgCl (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