A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(aq) +2e-→→ Cu(s) +0.34 Zn2+(ag) +2e-→→→ Zn(s) -0.76 1. Identify the reduction half-reaction involved. ○a. Ag+ (aq) +e²- Ag(s) O b. Cu²+ (aq) +2e* → Cu(s) OC. Zn²+ (aq) +2e → Zn(s)

A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E E = = X

.  At 25 C, the standard hydrogen electrode (SHE) has a half-cell potential that is defined to be 0.00 volts. If the pH is increased at this electrode (keeping everything else the same), at what pH will the half-cell potential be equal to -0.521 volts?

The following spontaneous reaction occurs when metallic zinc is dipped into a solution of copper sulfate. Zn (s) +Cu^ 2+ (aq) ----> Zn^ 2+ (aq) +Cu (s) Describe a galvanic cell that could take advantage of this reaction. What are the half-cell reactions? Make a sketch of the cell and label the cathode and anode, the charges on each electrode , the direction of ion flow, and the direction of electron flow .