Consider the following electrochemical cell: a. If silver metal is a product of the reaction, is the cell a galvanic cell or electrolytic cell? Label the cathode and anode, and describe the direction of the electron flow. b. If copper metal is a product of the reaction, is the cell a galvanic cell or electrolytic cell? Label the cathode and anode, and describe the direction of the electron flow. c. If the above cell is a galvanic cell, determine the standard cell potential. d. If the above cell is an electrolytic cell, determine the minimum external potential that must be applied to cause the reaction to occur.

a. If silver metal is a product, then the cell is a galvanic cell. The cathode is the silver electrode where Ag+ is reduced to Ag(s), and the anode is the copper electrode where Cu(s) is oxidized to Cu2+. Electrons flow from the anode (copper) to the cathode (silver). b. If copper metal is a product, then the cell is an electrolytic cell. The cathode is the copper electrode where Cu2+ is reduced to Cu(s), and the anode is the silver electrode where Ag(s) is oxidized to Ag+. Electrons flow from the anode (silver) to the cathode (copper) due to the external potential applied. c. For the galvanic cell, the standard cell potential is: \[E_{cell} = 0.80 - 0.34 = +0.46V\] d. For the electrolytic cell, the minimum external potential required is: \[|E_{cell}| = |{-0.46}| = 0.46V\]