Final answer:
In an electrolytic cell, oxidation occurs at the anode with a positive voltage, due to its connection to the positive terminal of the battery. The cell requires an external electrical current to drive the nonspontaneous redox reactions, with a minimum requirement exceeding the cell's negative standard potential.
Step-by-step explanation:
Electrolytic cells facilitate a chemical reaction through the application of an external electrical current, making them examples of nonspontaneous redox reactions. Within these cells, oxidation occurs at the anode, and this is associated with a positive voltage because the anode is connected to the positive terminal of the external power source. Conversely, reduction occurs at the cathode, which has a negative voltage in the context of electrolytic cells. This is because the cathode is connected to the negative terminal of the power source, making electrons flow from the anode to the cathode.
The voltage required to drive an electrolytic reaction must surpass the cell's standard potential, which is typically negative. This indicates that electrical energy is needed to force the reaction to proceed, distinguishing electrolytic cells from voltaic (galvanic) cells where the reaction is spontaneous and generates electrical energy.