A student measures the potential of a cell made up with 1M CuSO4 in one solution

Question

A student measures the potential of a cell made up with 1M CuSO4 in one solution and 1 M AgNO3 in the other. There is a Cu electrode in the CuSO4 and an Ag electrode in the AgNO3, and the cell is set up as in Figure 32.1. She finds that the potential, or voltage, of the cell, Ecell standard, is 0.45V, and that the Cu electrode is negative. A) At which electrode is oxidation occurring? B)Write the equation for the oxidation reaction. C) Write the equation for the reduction reaction. D) If the potential of the silver, silver ion electrode, E standard sub Ag+, Ag is taken to be 0.000V in oxidation or reduction, what is the value of the potential for the oxidation reaction, E standard sub Cu, Cu2+oxid?

Explanation / Answer

in an electrochemical cell, electrons spontaneously flow from the negative electrode to the positive electrode (the opposite situation applies in an electrolytic cell).

a) since oxidation is a loss of electrons, it occurs at the negative electrode (Cu).

b) Cu -> Cu2+ + 2e-

c) Ag+ + e- -> Ag

d) E0cell = 0.45 V, and E0red has been defined to be zero, so E0oxid = 0.45 V

e) 0.45 = E0oxid + 0.80; rearranging E0oxid = -0.35 V

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