How does an electrolytic cell differ from a cell that produces electricity?

The primary difference between an electrolytic cell and a cell that produces electricity (often called a voltaic or galvanic cell) lies in the direction of energy conversion.12

• Electrolytic Cell: This device consumes electrical energy to drive a non-spontaneous chemical reaction. By applying an external source of direct electric current, electrical energy is converted into chemical energy. This process, known as electrolysis, is commonly used for tasks such as metal plating or refining.12
• Cell that Produces Electricity: Also known as a voltaic cell, this device converts chemical energy directly into electrical energy. It utilizes spontaneous chemical reactions that are separated into oxidation and reduction processes at different electrodes. This separation creates a potential difference (voltage) that drives an electric current through an external circuit.132

While both systems involve electrochemical reactions and rely on electrodes and electrolytes to facilitate electron transfer, they operate in opposite directions regarding energy flow. Some devices, such as storage batteries, can function as both: they act as electrolytic cells when being charged and as electricity-producing cells when discharging.124