1. Write the following half-reactions, and include oxidation numbers on all participants

2. Write the oxidation half reaction for lithium oxidizing
Li0 (s)  Li+ (aq) + e-

3. Write the reduction half reaction for aluminum ions reducing to aluminum metal
Al3+ (aq) + 3e-  Al0 (s)

4. The following questions are about this voltaic cell.

5. Which metal is the cathode?
silver

6. Which metal is being oxidized?
zinc

7. What voltage is being measured by the voltmeter?

8. Which solution is accumulating sodium ions from the salt bridge?
The silver nitrate

9. Write the oxidation half-reaction.
Zn0 (s)  Zn+2(aq) + 2e-

10. Which metal is increasing in mass?
silver

11. Which direction are electrons flowing?
Right to left

12. Is this reaction spontaneous or nonspontaneous

13. Increasing (Zn0 is oxidized into Zn+2 ions)
Is the concentration of zinc ions in the soultion on the right increasing or decreasing?
Increasing (Zn0 is oxidized into Zn+2 ions)

14. Use the following electrolytic cell to answer the questions
Use the following electrolytic cell to answer the questions. A copper penny is submerged in iron (III) nitrate solution and connected to a DC source and a piece of iron.

15. What is the anode in this cell?
The iron

16. During this electroplating process, _____ is being coated with a thin layer of _____.
Cu, Fe

17. Write the oxidation half-reaction occuring in this cell.
Fe0 (s)  Fe3+ (aq) + 3e-

18. Write the reduction half-reaction occuring in this cell.
Fe3+ (aq) + 3e-  Fe0 (s)

19. Is the concentration of Fe3+ (aq) increasing, decreasing, or remaining constant?
(for every Fe3+ ion reduced to Fe0 metal, another metal atom is oxidized into Fe3+

20. This cell requires a DC power source because the reaction is ___________.
nonspontaneous

21. During this electroplating process, _____ is being coated with a thin layer of _____.
Cu, Zn

22. Write the oxidation half reaction
Zn0 (s)  Zn2+ (aq) + 2e-

23. Write the reduction half reaction
Ag+ (aq) + e-  Ag0 (s)

24. Write the oxidation half reaction for carbon going from oxidation state of 2+ to 4+
C+2  C e-

25. Write the reduction half reaction for pure chlorine gas becoming chloride ions
Cl2 (g) + 2e-  2 Cl- (aq)