A. Using the following standard reduction potentials: Ag* (aq) +e = Ag (s) Pb2* (aq) + 2e= Pb (s) E° = +0.80 V E° = -0.13 V Write a balanced redox reaction that represents the overall cell reaction for the feasible galvanic cell. i. ii. Calculate the standard cell potential. iii. Draw a fully labelled galvanic cell for this redox system. Your labels should show (but not limited to): the electron and ion flow; the anode and cathode, the half cells where oxidation and reduction take place.

The reaction 2Ag+(aq) + Cu(s) → 2Ag(s) + Cu2+(aq) was used in a galvanic cell. E°=0.46 V for this reaction. What is the cell potential, E, at 298K if the concentrations are [Cu2+] = 1.0M and [Ag+] = 0.10M?

Consider an electrochemical cell made up of Au Au* and Co²+ | Co³+ half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 E = ローロ V 00 Calculate the standard emf of a cell that uses the Au Au and Co²+ | Co³+ half-cell reaction at 25 °C. Round your answer to 2 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. 09 S

Sn(s) | Sn2+ (aq, 1.8 M) || Agt(aq, 0.055 M) | Ag(s) Consider the cell notation of a galvanic cell given above and the following reduction potentials: Sn- (aq) + 2e- → Sn(s) E° = -0.14 V Ag (aq) + e- → Agis) ED=0.80 V 1. The number of electron transferred in the net reaction is [Select] 2. The E is [Select] 3. The value for Q is (Select] 4. The cell potential for the cell is [Select] V.