🙁 Expiramental cell potential: 1.093V Transcribed Image Text: Ered. V
+1.50
Reduction Half-Reaction
Aud: (aq) + 3e → Au (s)
Pt2 (ag) + 2e → Pt (s)
Ag (aq) + e -→ Ag (s)
Cu2 (ag) + 2e → Cu (s)
+1.20
+0.80
+0.34
0.000
2H (ag) + 2e → H2 (s)
Pb2 (ag) + 2e→ Pb (s)
Sn? (ag) + 2e→ Sn (s)
-0.13
-0.14
Ni? (ag) + 2e Ni (s)
-0.28
Fe? (ag) + 2e→Fe (s)
Zn2: (aq) + 2e→Zn (s)
AP (ag) + 3e → Al (s)
Mg2 (aq) + 2e → Mg (s)
-0.44
-0.76
-1.66
-2.37
Na (ag) + e Na (s)
-2.71 Transcribed Image Text: Part A: Constructlon of Voltalc Cells and Measurement of Cell Potentlals
Cll
Cell
Cu/ Zn
4
Zn/Pb
Cu/ Pb
Zn/Ag
3
Cu/Ag
6
Pb/Ag
Prepare and complete the tollowing table tor each of your six voltaic cells
Example for Cell 1:
Copper/Zinc cell
Oxidation half-reaction
Reduction half-reaction
Balanced Net reaction
Metal at the anode
Metal at the cathode
Experimental cell potential
Calculated standard cell potential,
% difference
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