The cell shown above is a concentration cell. Both cells contain a copper solution and have copper electrodes. The only driving force for this cell is the difference in the concentration of the copper solutions. The system will react to equalize the concentration of the ions in both cells.
Oxidation: Cu (s) → Cu2+ (aq) + 2 e– Reduction: Cu 2+ (aq) + 2 e– → Cu (s)
Determine if the following statements are True or False.
True False The half-cell with the higher concentration of copper (II) ions must be the anode. True False The cell that has the lower ion concentration acts as the cathode. True False When the cathode dissolves, copper (II) ions are formed. True False At the anode, the concentration of copper (II) ions is decreasing.
Hint: Reduction occurs at the cathode and oxidation occurs at the anode. Copper (II) ions will be a reactant in the half-cell where they are present at the highest concentration.
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