1. An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.8 ampere current. What mass of nickel is produced?

2. How many liters of F2 at STP could be liberated from the electrolysis of molten NaF under a 2.16 ampere current for 60.0 minutes?

3. How long would a constant current of 18.0 amperes be required to flow in order for 9000 coulombs of charge to pass through a cell?

4. Molten AlCl3 is electrolyzed for 5.0 hours with a current of 0.40 ampere. Metallic aluminum is produced at one electrode and chlorine gas, Cl2, is produced at the other. How many liters of Cl2 measured at STP are produced at the other electrode.

5. How many minutes would a 5.00 ampere current have to be applied to plate out 8.00 grams of copper metal from aqueous copper(II) sulfate solution?

6. Calculate the cell potential for the following voltaic cell. Cr/Cr3+(1.0x10^-2 M)//Co2+(1.0x10^-5 M)/Co

7. Calculate the [H+] for the hydrogen half-cell of the following voltaic cell if the observed cell voltage is 2.02 V. Mg/Mg2+(1.00 M)//H+(? M), H2(1.00 atm)/Pt

8. Calculate the pH for the hydrogen half-cell of the following voltaic cell if the observed cell voltage is 1.00 V. Mn/Mn2+(1.00 M)/H+(pH=?), H2(1.00 atm)/Pt