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Electrochemistry (Ch 11)

Electrochemistry (Ch 11). 1. Define: a. galvanic (voltaic) cell b. electrolytic cell. Electrochemistry (Ch 11). 2. Draw the galvanic cells based on the following reactions in a diagram and in line notation. Give the overall reaction, label the anode and cathode and calculate E ˚ cell .

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Electrochemistry (Ch 11)

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  1. Electrochemistry (Ch 11) 1. Define: a. galvanic (voltaic) cell b. electrolytic cell

  2. Electrochemistry (Ch 11) 2. Draw the galvanic cells based on the following reactions in a diagram and in line notation. Give the overall reaction, label the anode and cathode and calculate E˚cell. a. Fe3+ + 3e- → Fe 0.036 V Cu2+ + 2e- → Cu 0.34 V b. MnO4- + 8H+ + 5e- → Mn2+ + 4H2O 1.51 V Al3+ + 3e- → Al -1.66 V

  3. Electrochemistry (Ch 11) F2 + 2e- 2F- 2.87 Au3+ + 3e- Au 1.50 Cl2 + 2e- 2Cl- 1.36 ClO2 + e- ClO2- 0.954 I2 + 2e- 2I- 0.54 2H+ + 2e- H2 0.00 Pb2+ + 2e- Pb -0.13 Al3+ + 3e- Al -1.66 Li+ + e- Li -3.05

  4. Electrochemistry (Ch 11) 3. Use the reduction potential table to answer the following: a. pick the strongest oxidizing agent Al3+ Au ClO2 F2 b. pick the strongest reducing agent Au H2 Al Pb2+ c. will gold dissolve in acid? what about aluminum? d. which species can oxidize Pb but not Cl-? Li+ F- H+ Au3+

  5. Electrochemistry (Ch 11) 4. Calculate E˚, ΔG˚ and K at 25 ˚C for the following reaction Cl2 (g) + 2NaI (aq)  2NaCl (aq) + I2 (s)

  6. Electrochemistry (Ch 11) 5. Calculate the potential of the following galvanic cell at 25 ˚C after the concentration of Pb2+ has changed by 0.60 M. Pb | Pb2+ (1.0 M) || Au3+ (1.0 M) | Au

  7. Electrochemistry (Ch 11) 6. What mass of chromium can be produced from the electrolysis of a solution of CrCl3 with a current of 15 A for 1 hr?

  8. Electrochemistry (Ch 11) 7. An aqueous solution of an unknown salt of manganese ion is electrolyzed by a current of 4.20 A passing for 35 minutes. If 1.00 g of Mn is produced at the cathode, what is the charge on the manganese ions in solution?

  9. Electrochemistry (Ch 11) 8. In the electrolysis of water to form hydrogen and oxygen gases, which is correct? a. hydrogen is produced at the anode b. hydrogen is produced at the cathode c. oxygen is produced at the cathode d. both gases are produced at the anode e. both gases are produced at the cathode

  10. Electrochemistry (Ch 11) 9. What volume of hydrogen gas at STP is produced from the electrolysis of water by a current of 3.5 amps in 15 minutes?

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