A solution containing 0.14M Pb2+, 1.5×10−6M Pb4+, 1.5×10−6M Mn2+, 0.14M MnO−4, and 0.83M HNO3 was prepared. For this solution, the balanced reduction half‑reactions and overall net reaction shown can occur. 5[Pb4++2e−↽−−⇀Pb2+] ∘+ = 1.690 V
2[MnO−4+8H++5e−↽−−⇀Mn2++4H2O] ∘− = 1.507 V

5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO−4+16 H+

A) Determine ∘cell , Δ∘ , and for this reaction. B) Calculate the value for the cell potential, cell , and the free energy, Δ , for the given conditions. C) Calculate the value of cell for this system at equilibrium. D) Determine the pH at which the given concentrations of Pb2+, Pb4+, Mn2+, and MnO−4 would be at equilibrium.