What is the purpose of an electrolytic cell?

An electrolytic cell is designed specifically to use electrical energy to drive a non-spontaneous chemical reaction, which is essentially a redox reaction. In an electrolytic cell, electrical energy is supplied from an external source, allowing the cell to facilitate a process where oxidation and reduction occur simultaneously. This is contrary to a galvanic cell, which generates electrical energy from a spontaneous reaction.

An example of an electrolytic cell is the electrolysis of water, where electrical energy is applied to split water molecules into hydrogen and oxygen gases. This illustrates the core function of electrolytic cells: they convert electrical energy into chemical energy, facilitating reactions that would not occur under standard conditions without the external energy input.

The other options relate to different aspects of electrochemistry but do not correctly describe the specific purpose of an electrolytic cell. While measuring half-cell potentials is related to understanding redox reactions, it does not involve influencing a reaction via electrical input. Maintaining a constant temperature is a concern in many chemical processes, but it is not a direct function of electrolytic cells.