A 0.207 g sample of an alloy containing lead is dissolved in nitric acid to produce an aqueous solution of lead(II) ions. This acidic solution is titrated with a 0.0136 M solution of KMnO4, forming lead(IV) and manganese(II) ions. If the titration requires 16.53 mL of the KMnO4 solution to reach the equivalence point. a. Calculate moles of permanganate required. b. Show a balanced redox equation i. oxidation ii. reduction iii. overall c. How many moles of lead are present? d. how many grams of lead does this represent? e. What is the percent lead by mass in the alloy? f. Construct a galvanic cell in contact with Pb+4 /Pb+2 in contact with a lead electrode as the anode half-cell and MnO4- / Mn2+ in contact with a pt electrode as the cathode half reaction. g. What E°cell cell for this reaction?