Use general chemistry rules for significant figures. 1. (12 pts) A cell is constructed to reduce the Ag+ in AgCl(s) to Ag(s) at the cathode when
current is passed through the cell. At the anode, Cu(s) is oxidized to Cu2+.
If current of 0.500 A is passed through the cell for 101 minutes, calculate the mass of
Cu(s) dissolved and mass of Ag(s) deposited. Half-cell reactions:
Cathode: AgCl(s) + e ⇌ Ag(s) + Cl–
Anode: Cu(s) ⇌ Ce2+ + 2e