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Unformatted text preview: n potential of the cathode half cell reaction and
E°anode is the standard reduction potential of the anode half cell reaction. Q is the reaction
quotient, for the overall cell reaction, using the concentrations given in the cell diagram.
Note that at equilibrium when Q = K then Ecell is equal to zero.
For the cell discussed in the introduction this equation becomes:
Ecell = (E°Ag+/Ag - E°Cu++/Cu) - 0.0129 ln[ (0.10M) / (0.10M)2 ]
= (0.799-0.337) - 0.0297
= + 0.432 V
The numerical values of the standard reduction potentials used in this example were
taken from a table in the Appendix of your textbook.
In part I you measured the voltages of three cells, each containing a different metal,
against a common Cu(II)/Cu reference electrode. The standard reduction potential of the
Cu(II)/Cu(s) redox couple is known to be 0.34V. This value is used as the "known"
standard reduction potential in the following calculations.
For each of the three cells whose voltages you measured in Part I of this experiment write
the corresponding redox reaction in the spontaneous direc...
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This note was uploaded on 04/09/2013 for the course CHE CHE 2C taught by Professor Nasiri during the Spring '07 term at UC Davis.
- Spring '07