Pb | PbSO4 (s) | SO4 2- (1.00 M) || H+ (2.00 M), SO4 2- (1.00 M) | PbSO4 (s) | PbO2 (s) Where PbSO4 (s) + 2 e- = Pb(s) + SO4 2- (aq) EPb/PbSO4 = -0.355 V PbO2 (s) + 4 H+ (aq) + SO4 2- (aq) + 2 e- = PbSO4 (s) + 2 H2O(l) EPbO2/PbSO4 =+1.685 V (a) Identify which half reaction occurs at the anode and which one occurs at the cathode. (b) Calculate the potentials of the half-reactions, given the concentrations above. (c) What are the oxidation numbers (oxidation states) of the lead in all three of the leadcontaining species (PbSO4, Pb, and PbO2). (d) Write the balanced, overall chemical reaction of the cell. (e) In the overall chemical reaction, which one of the reactants serves as the oxidant? (f) Calculate the potential of the cell (Ecell) and state whether the cell is galvanic, electrolytic, or neither. (g) Is the overall cell reaction spontaneous or not?