1. Making Galvanic Cells Lab
No bridge
Voltage
Points to
Deposit
Cu – Al
0 V
2.0 V Cu
Cu – Zn
1.1 V
Al – Zn
0.9 V Zn
3) The salt bridge allows the cell to continue to function. K+ or NO3– can move into one of the half cells to balance the charge created by + metal ions forming or leaving solution.
4) No. We did not get the same values in the lab

2. Cu – Zn cell Electron flow Cu (+) Salt bridge Zn (–) Cu2+ Zn2+
Zn  Zn2+ + 2e– (oxidation - LEO)
Cu2+ + 2e–  Cu (reduction - GER)
Cu2+ + Zn  Cu + Zn2+

3. Al – Zn cell Electron flow Al (–) Salt bridge Zn (+) Al3+ Zn2+
Zn2+ + 2e–  Zn (reduction - GER)
Al  Al3+ + 3e– (oxidation - LEO)
2Al + 3Zn2+  2Al3+ + 3Zn

4. Making Galvanic Cells Lab
Cu-Zn
voltage
Al-Zn
voltage
No bridge
No bridge
0 sec
 0.9
0 sec
 0.5
30 sec
 0.9
30 sec
 0.5
Deposit Cu
Deposit Al
Points to Cu
Points to Al
3) The salt bridge allows the cell to continue to function. K+ or NO3– can move into one of the half cells to balance the charge created by + metal ions forming or leaving solution.
4) No. We did not get the same values in the lab
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