1. Electrolysis Electrolysis: Forcing a current through a cell to produce a chemical change for which the cell potential is negative. A Galvanic Cell in Reverse!!! (Used in Electrolytic Cells)

2. 1M Al 3+ 1 M Fe 3+ Al→ Al 3+ + 3e - 3(Fe 3+ + 1e - → Fe 2+ ) Al voltmeter KNO 3 Al Al 3+ Fe 3+, Fe 2+ C C e- → anode → (oxidation) (negative electrode) ← cathode (reduction) (positive electrode) Al + 3 Fe 3+ → Al 3+ + 3 Fe 2+ 1 M Fe 2+ E°= 1.66 VE°= 0.77 V 2.43 V

3. 1.90 M Al 3+ 0.10 M Fe 3+ Al→ Al 3+ + 3e - 3(Fe 3+ + 1e - → Fe 2+ ) Al KNO 3 C e- → anode → (oxidation) ← cathode (reduction) Al + 3 Fe 3+ → Al 3+ + 3 Fe 2+ 0.70 M Fe 2+ 2.37 V (These go up as the reaction proceeds) (This goes down as the reaction proceeds)

4. E = E° - [0.0592/n] log Q Becomes zero at Eq. Becomes K at Eq. E° = [0.0592/n] log K

5. 1 M Al 3+ 1 M Fe 3+ Al 3+ + 3e - → Al3(Fe 2+ → Fe 3+ + 1e - ) Al KNO 3 C ← e- cathode → (reduction) ← anode (oxidation) Al 3+ + 3 Fe 2+ → Al + 3 Fe 3+ 1 M Fe 2+ Power Supply - + Supply a voltage in the opposite way greater than 2.43 V

6. If a current of 1.5 A was made to flow through the cell for 15.0 minutes… how much Al would plate out? 0.13 grams Al