13. Write the oxidation half reaction, the reduction half reaction, and the overall cell reaction for the following galvanic cell. Identify the anode and the cathode and state why you labeled the metals that way. (4) Zn (s) | Zn²+ (aq) || Cu²+ (aq) | Cu (s)

An electrochemical cell is made of two electrodes: (Zn2+/Zn) and (Ag+/Ag). Use the standard reduction potentials to answer the following questions. What is the standard potential of the cell and which electrode is the cathode and which one is the anode? Write a net redox equation for this electrochemical cell.

Historically, the first true battery was the Leclanché cell, named after its discoverer, Georges Leclanché. It was based on the following reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Identify what is being oxidized, what is being reduced, and the respective reducing and oxidizing agents.

Questions 20 and 21 refer to the following information. Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg2(1.0 M) || Pb*2(1.0 M) | Pb 1 2.24 Zn | Zn(1.0 M) || Pb*2(1.0 M) | Pb 2 0.63 Mg | Mg*(1.0 M) || Zn*2(1.0 M) | Zn 3 The chemical reaction occurring in first galvanic cell is: Mg + Pb*2 → Mg+2 + Pb 21. If the concentration of Mg+2 is changed from 1.0 M to 3.0 M in the galvanic cells above, what will happen to the observed cell voltages in galvanic cells 1 and 3? (A) The voltage in both galvanic cells 1 and 3 will increase. (B) The voltage will decrease in both galvanic cells 1 and 3. (C) The voltage in galvanic cell 1 will increase and will decrease in galvanic cell 3 (D) The voltage in galvanic cell 3 will increase and will decrease in galvanic cell 1. 22. Consider a voltaic cell based on these half-cells. Ag (aq) +e → Ag/s) Cd (aq) + 2e → Cd¢s) E* = +0.80 V E = -0.40 V Identify the anode and give the voltage of this cell under standard conditions. (A) Ag; Ecell = 0.40 V (B) Ag;…