@X@user.full_name@X@ @GMU: What is the standard free energy change for the ionization of HF acid, if its Ka is 6.60e-4.

@X@user.full_name@X@ @GMU: What is the pOH of 9.35e-4 M HNO3 ?

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3709 M A, 0.2658 M B, and 0.1997 M C. Which change will cause the equilibrium to shift from left to right if the reaction is exothermic? Use the reaction below.4A(aq) → 3B(aq) +4C(aq) K = 0.600

John Schreifels @GMU: What is the total entropy change at 25oC for the reaction below, if the standard entropies of reactants and products are So (C(gr)) = 5.74 J/mol*K, So (H2(g)) = 130.68 J/mol*K, and So (C9H16(g)) = 484.8200 J/mol*K and the heat of formation of C9H16(g)) is 61.8300 kJ/mol.9C(gr) + 8H2(g) → C9H16(g)

@X@user.full_name@X@ @GMU: What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C4H6(g)) = 283.4000J/mol*K and the heat of formation of C4H6(g)) is 148.0700 kJ/mol?4C(gr) + 3H2(g) → C4H6(g)

@X@user.full_name@X@ @GMU: What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C5H12(g)) = 349.0000J/mol*K and the heat of formation of C5H12(g)) is -146.4400 kJ/mol?C5H12(g) → 5C(gr) + 6H2(g)

@X@user.full_name@X@ @GMU: Which base listed below would be the best to creat a buffer having a pH of 6.2299?

@X@user.full_name@X@ @GMU: What is the standard free energy change for the following cell?3Ag+(aq) + Al(s) → 3Ag(s) + Al3+(aq) Ecoell = 2.459V

@X@user.full_name@X@ @GMU: What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 3.26e-5?5C2H2(g) + 4 H2(g) → C10H18(g) ΔGo = -793.710 kJ.

@X@user.full_name@X@ @GMU: What must the reaction quotient Q be, if the free energy is -961.941 kJ at 25.0oC?5C2H2(g) + 5 H2(g) → C10H20(g) ΔGo = -925.150 kJ.