Student Worksheet
Voltaic Cells, Extra Exercises
For each of the following cells, use the given cell notation to identify the strongest oxidizing and
reducing agents. Write chemical equations to represent the cathode, anode, and net cell reactions.
Label electrodes, electrolytes, electron flow, and ion movement. Predict the cell potential.
1. Cd(s) | Cd(NO3)2(aq) || AgNO3(aq) | Ag(s)
2. Pt(s) | IO3–(aq), H+(aq) || Zn2+(aq) | Zn(s)
Student Worksheet
Cell Potentials, Extra Exercises
1. Assume that the reference half-cell is changed to a standard mercurymercury(II) half-cell.
(a) What would be the reduction potential of a standard chlorine half-cell?
(b) What would be the reduction potential of a standard nickel half-cell?
(c) What would be the net cell potential of a standard chlorinenickel cell?
(d) Why is the answer to part c the same as the answer obtained using the standard hydrogen
half-cell as the reference?
2. For each of the following standard cells, write the cell notation, label electrodes, and
determine the cell potential.
(a) cobalthydrogen standard cell
(b) zincaluminium standard cell
(c) tin(IV)zinc standard cell
3. For each of the following cell notations, write the cathode, anode, and net cell reaction
equations and calculate the cell potential.
(a) Pb(s) | Pb2+(aq) || Ni2+(aq) | Ni(s)
(b) Pt(s) | SO42–(aq), H+(aq), H2SO3(aq) || Ag+(aq) | Ag(s)
(c) Cd(s) | Cd2+(aq) || ClO4–(aq), H+(aq), Cl–(aq) | C(s)
4. Use the standard cell described below to determine the standard reduction potential of the
gallium half-cell.
Cu(s) | Cu2+(aq) || Ga3+(aq) | Ga(s)
cathode
anode
E° = +0.90 V
Student Worksheet
Electrolytic Cells, Extra Exercises
1. Write the equations for the anode, cathode, and net reactions for the electrolysis of molten
aluminium oxide. One half-reaction will involve conversion of liquid oxide ions into oxygen
gas.
2. Write equations for the anode, cathode, and net reactions for the electrolysis of molten
potassium bromide.
3. For the following electrolytic cells, write equations for half-reactions and the net cell
reaction, and calculate the minimum electrical potential difference that would be required to
cause the electrolysis to occur.
(a) an aqueous solution of nickel (II) chloride is electrolyzed
(b) an aqueous solution of potassium sulfate is electrolyzed
(c) an aqueous solution of lead (II) nitrate is electrolyzed