1.) A voltaic cell has a copper anode in 1 M CuSO4
and a silver cathode in 1 M AgNO3. What is Ecell for
this cell?
A. +0.270 V | |
B. -1.137 V | |
C. +1.137 V | |
D. -0.463 V | |
E. +0.463 V |
2.) Which of the following half-reactions is not correct?
A. Cu+ + e- → Cu | |
B. Mg → Mg2+ + 2e- | |
C. Fe3+ + 2e- → Fe+ | |
D. Pb2+ + e- → Pb3+ | |
E. Ag → Ag+ + e- |
1. Reduction potential of Cu2+ = 0.34 V
Reduction potential of Ag+ = 0.800 V
So, Ag+ will oxidise Cu.
Eocell = 0.80-0.34 = 0.46 V
Ecell = Eocell -0.06/n log[Cu2+]/[Ag+]2
= 0.46 - 0.06/2 log[1]/[1]2
= 0.46 V
Answer is E.
2. In all the reactions, charges are balanced on both the sides of the reaction except one reaction.
Pb2+ + e- --------> Pb3+
The reaction should be:
Pb2+ --------> Pb3+ + e-
Now the charges are balanced on both sides of the reaction.
Answer is D.
1.) A voltaic cell has a copper anode in 1 M CuSO4 and a silver cathode...
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