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.

1. Understand the definitions - A galvanic cell is a spontaneous electrochemical cell in which the electrical energy is produced by a spontaneous redox reaction. - An electrolytic cell is a non-spontaneous electrochemical cell in which the electrical energy is used to drive a non-spontaneous redox reaction. - Cathode: an electrode where reduction takes place - Anode: an electrode where oxidation takes place 2. Identify the redox half-reactions If silver metal is a product of the reaction, the following half-reaction occurs: \[Ag^+ + e^- \to Ag\] Since the reduction reaction takes place, this electrode is considered as the cathode. 3. Determine the type of cell and electron flow Since reduction takes place at the cathode and oxidation takes place at the anode in a galvanic cell, this cell is most likely a galvanic cell if silver metal is a product. Electrons flow from the anode to the cathode in a galvanic cell.

1. Identify the redox half-reaction If copper metal is a product of the reaction, the following half-reaction occurs: \[Cu^{2+} + 2e^- \to Cu\] Since the reduction reaction takes place, this electrode will be considered the cathode. 2. Determine the type of cell and electron flow Since reduction takes place at the cathode and oxidation takes place at the anode in an electrolytic cell, this cell is most likely an electrolytic cell if copper metal is a product. Electrons flow from the cathode to the anode in an electrolytic cell.

1. Identify the half-reactions In a galvanic cell, the following half-reactions occur: - Anode (oxidation): \(Cu \to Cu^{2+} + 2e^-\) - Cathode (reduction): \(Ag^+ + e^- \to Ag\) 2. Determine the standard potentials The standard reduction potentials for the half-reactions are: - Anode: \(E^\circ_{Cu^{2+}/Cu} = +0.34 V\) - Cathode: \(E^\circ_{Ag^+/Ag} = +0.80 V\) 3. Calculate the standard cell potential The standard cell potential for a galvanic cell is given by the following equation: \[E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}\] Using the standard potentials, we calculate the standard cell potential: \[E^\circ_{cell} = (+0.80 V) - (+0.34 V) = +0.46 V\]

1. Determine the half-reactions In an electrolytic cell, the following half-reactions occur: - Anode (oxidation): \(Ag \to Ag^+ + e^-\) - Cathode (reduction): \(Cu^{2+} + 2e^- \to Cu\) 2. Calculate the minimum external potential The minimum external potential required for an electrolytic cell can be obtained from the standard cell potential calculated in Part C, but with the opposite sign: \[E^\circ_{ext} = -E^\circ_{cell} = -(+0.46 V) = -0.46 V\] A potential of at least -0.46 V must be applied to cause the reaction to occur in the electrolytic cell.