Unformatted text preview: of the
following is the spontaneous reaction for the copper concentration cell you measured in
Part II of the electrochemistry experiment? Three choices will be given
Part II Analysis. Because the standard potentials are the same for both the anode and the
cathode reactions for a concentration cell, the Nernst equation for a concentration cell
becomes simply Ecell = -(0.0257/n)lnQ, where Q is to be calculated for the spontaneous
cell reaction. What is the value of Q for the copper concentration cell?
Part II Analysis.
Ecell = -(0.0257/n)lnQ Now, using your value for Q calculate Ecell
from the Nernst equation for the copper concentration cell, and enter it here.
For Part II of the electrochemistry experiment, you measured the potential of some
concentration cells. The laboratory manual asked you to construct the cells
a) Cu(s)Cu(NO3)2(0.010M) || Cu(NO3)2(0.10M)|Cu(s)
b) C(graphite) | FeSO4(0.010M), Fe(NO3)3(0.10M) || Cu(NO3)2(0.10M) | Cu(s)
c) C(graphite) | FeSO4(0.010M), Fe(NO3)3(0.10M) || Cu(NO3)2(0.10M) | Cu(s) 20 When the red lead for the voltmeter was connected to t...
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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