Name:
Date:
Period:
Reduction Potentials Practice
1. Calculate
and write the overall cell reaction for these cells.
llPb
Snl5n
l
Pb
a. 2
—
— -b(
b
lHllBr
2
H
l
Br
—
2. In one process used to produce aluminum metal, ore containing alumInum oxide is
converted to aluminum chloride. Aluminum metal is then produced by the electrolysis
of molten aluminum chloride (AlCl
).
3
a. Write the hIf-reactions that take place at each electrode.
—
2
b. Write the equation for the overall cell reaction.
c. Identify the products produced at eac{ electrode,
/
r
3. What relationship does the voltage produced by a redox reaction have to the
spontaneity of the reaction?
4. Use the information in Table 21.2 to determine which of the following cell reactions will
proceed spontaneously.
$
a
b
c
d.
e
?
2
Zn+Pb
Cu÷Fe 2
2
?
2
Ag+Cu
H
+
2
Cu
-?
2
Fe+Pb
7,.
2
Na+C1
5. For each spontaneous reaction in #4, write the half-reaction that takes place at the
anode. Be sure to include the electrons.
6. Write the overall balanced equation for each reaction in #4 that proceeds
spontaneously.
/
7. Determine the standard cell potential for each reaction in #4 that proceeds
spontaneously.
—5
—
7_
‘
,
‘
5!
8. A voltaic cell is constructed using the following half-reactions.
2 (aq) + 2& 5 Cu (s)
Cu’
= +O.34V
At(aq)+3e-> Al(s)
813+ = —1.66V
Calculate the standard cell potential.
,vttW r2OOV
9. Calculate the standard potential of this redox reaction to determine whether the
reaction will occur spontaneously.
2At (aq) + 3Mg(s) 5 2A1 Cs) + 3M? (aq)
(..,4q,V)
ti/V