1. Suppose we have a voltaic cell that uses this reaction, which has a standard potential of +0.816 V: Se + H2SO3 → SeO3

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1. Suppose we have a voltaic cell that
uses this reaction, which has a standard potential of +0.816 V:
Se + H2SO3 →
SeO32- + S + 2H+
a. Write the
balanced half reactions.
b. Use the
information above and in Appendix E to calculate E˚red
for the reaction involving selenium.
c. Make a sketch of
the cell, and label the anode and cathode.
d. In your sketch
from part c, draw an arrow indicating the direction in which
electrons flow during the reaction.
2- Suppose we have a voltaic cell that
uses the reaction:
Al3+(aq) +
3Cu+(aq) → Al(s) + 3Cu2+(aq)
a. What is the
standard potential of this cell?
b. What is the emf
of this cell if [Al3+] = 0.805M, [Cu+] =
1.10M, and [Cu2+] = 1.25M?
c. What is the emf
of this cell if [Al3+] = 0.120M, [Cu+] =
0.0750M, and [Cu2+] = 3.15M?
d. What is the emf
of this cell if [Al3+] = 2.75M, [Cu+] =
2.15M, and [Cu2+] = 0.0870M?