AP Chemistry Concepts ELECTROCHEMISTRY contained in Big Ideas 3 and 6 – – 1. oxidation / reduction balancing equations (review) – 2. galvanic {positive, Red Cat} – 3. electrolytic cells 4. cathode 5. anode 6. current, charge, Faradays, (voltage / EMF) (amps, coulombs and unit problem) – 7. cell notation 8. salt bridge not electron balance, – “balance of charge” Good salt bridge materials are soluble salts, not easily oxidized or reduced, doesn’t interfere with given redox reaction, ie complex ion formation or precipitation 9. and spontaneity Eo 10. = - n F Eo ΔGo 11. = (0.059 / log E Eo n) Kc – 12. Vocabulary – Galvanic Voltaic Free Response Questions 2007 #3. An external direct-current supply is connected to two platinum electrodes immersed in a beaker containing 1.0 M CuSO4(aq) at 25oC, as shown in the diagram above. As the cell operates, copper metal is deposited onto one electrode and O2(g) is produced at the other electrode. The two reduction for the overall reaction that occurs in the cell are shown in the table below. half-reaction Eo(V) O2(g) + 4 H+(aq) + 4 e- 2H2O(l) +1.23 Cu2+(aq) + 2e- Cu(s) +0.34 a. On the diagram, indicate the direction of electron flow in the wire.
AP Chemistry Concepts – ELECTROCHEMISTRY – contained in Big Ideas 3 and 6 1. oxidation / reduction – balancing equations (review) 2. galvanic – {positive, Red Cat} 3. electrolytic cells 4. cathode 5. anode 6. current, charge, Faradays, (voltage / EMF) (amps, coulombs and – unit problem) 7. cell notation 8. salt bridge – “balance of charge” not electron balance, Good salt bridge materials are soluble salts, not easily oxidized or reduced, doesn’t interfere with given redox reaction, ie complex ion formation or precipitation 9. Eo and spontaneity 10. ΔGo = - n F Eo 11. E = Eo – (0.059 / n) log Kc 12. Vocabulary – Galvanic Voltaic Free Response Questions 2007 #3. An external direct-current supply is connected to two platinum electrodes immersed in a beaker containing 1.0 M CuSO4(aq) at 25oC, as shown in the diagram above. As the cell operates, copper metal is deposited onto one electrode and O2(g) is produced at the other electrode. The two reduction for the overall reaction that occurs in the cell are shown in the table below. half-reaction Eo(V) O2(g) + 4 H+(aq) + 4 e- 2H2O(l) +1.23 Cu2+(aq) + 2e- Cu(s) +0.34 a. On the diagram, indicate the direction of electron flow in the wire.