E cell Table 1: The electrochemical series (abridged) Half-cell reaction Fe³+ (aq) + e→→ Fe²+ (aq) Cu²+ (aq) + 2e →→ Cu(

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E Cell Table 1 The Electrochemical Series Abridged Half Cell Reaction Fe Aq E Fe Aq Cu Aq 2e Cu 1 (110.92 KiB) Viewed 44 times

Build the followingelectrochemical cells as shown in Figure 1, andcomplete Table 2 in the Data andCalculations section. To build a galvanic cell, you onlyneed enough liquid reagent (less than 50mL in each half-cell) tomake sure that there is sufficient electrical contact between them.It does not matter which half-cell is in the porous pot and whichhalf-cell is in the plastic beaker. Change the solutions for eachgalvanic cell, even if the same solution is used for two subsequentcells.
1)Zn|Zn2+(0.100M)||Pb2+(0.100M)|Pb
2)Zn|Zn2+(0.100M)||Fe2+(0.100M)|Fe
3)Pb|Pb2+(0.100M)||Cu2+(0.100M)|Cu
4)Fe|Fe2+(0.100M)||Cu2+(0.100M)|Cu
5) Cu|Cu2+(0.100M)||Fe3+(0.0500M), Fe2+(0.0500M)|C
6) Zn|Zn2+(0.100M)||Fe3+(0.0500M), Fe2+(0.0500M)|C
7) Fe|Fe2+(0.100M)||Fe3+(0.0500M), Fe2+(0.0500M)|C

E Cell Table 1 The Electrochemical Series Abridged Half Cell Reaction Fe Aq E Fe Aq Cu Aq 2e Cu 2 (63.21 KiB) Viewed 44 times

E cell Table 1: The electrochemical series (abridged) Half-cell reaction Fe³+ (aq) + e→→ Fe²+ (aq) Cu²+ (aq) + 2e →→ Cu(s) Pb²+ (aq) + 2e →→ Pb(s) Ni²+ (aq) + 2e →→ Ni(s) Cd²+ (aq) + 2e →→ Cd(s) Fe²+ (aq) + 2e → Fe(s) Zn²+ (aq) + 2e → Zn(s) Eº cathode - anode EO Standard potential Eº, V 0.771 0.3419 -0.1262 -0.257 -0.4030 -0.447 -0.7618

Data and Calculations # 1 2 3 4 5 6 Table 2: Galvanic cells and cell potential (voltage) data Cell Diagram ZnZn²+ (0.100M)||Pb²+(0.100M)|Pb ZnZn²+ (0.100M)||Fe²+ (0.100M) Fe PbPb²+ (0.100M)||Cu²+ (0.100M)|Cu FelFe²+ (0.100M)||Cu²+ (0.100M)|Cu Cul Cu²+ (0.100M)|| Fe³+ (0.0500M), Fe²+ (0.0500M)|C ZnZn²+ (0.100M)|| Fe³+ (0.0500M), Fe²+ (0.0500M)|C Calculated Voltage 0.900 0.400 0.490 0.200 0.510 Observed Voltage