A “dead” 12 V lead storage battery has 5.31 g of PbSO4 deposited on each of its anodes. It is connected to a “trickle charger” that supplies 0.120 A of current at a voltage of 13 V. The reaction for the discharge of the lead storage battery follows.

Pb(s) + 2HSO4-(aq) + PbO2(s) + 2H3O+(aq)   2PbSO4(s) + 4H2O(l)

1.To which electrode, Pb or PbO2, should the anode from the charger be connected?

2.Compute the time in hours needed to convert all 5.31 g of PbSO4 back to HSO4- ions in solution. The Faraday constant is 96485 C/mol.