An electrolytic cell is a device that uses electrical energy to force a chemical reaction to happen that would not occur on its own, a process called electrolysis.

Quick Scoop

Simple definition

An electrolytic cell is an electrochemical cell in which an external power source (like a battery or DC supply) pushes electrons through a solution or molten salt, driving a non‑spontaneous redox reaction.

In other words, it converts electrical energy into chemical change.

Main parts

  • Electrolyte: An ionic medium (aqueous solution or molten salt) that contains mobile ions.
  • Cathode: The negatively charged electrode where reduction (gain of electrons) takes place in an electrolytic cell.
  • Anode: The positively charged electrode where oxidation (loss of electrons) takes place.
  • External power source: Provides the voltage needed to push the non‑spontaneous reaction.

How it works (story-style)

Imagine a tank of molten sodium chloride connected to a battery.
The battery pulls electrons from the positive electrode (anode) and pushes them onto the negative electrode (cathode).
Positive sodium ions in the melt travel toward the cathode, gain electrons, and become sodium metal, while negative chloride ions travel to the anode and lose electrons to form chlorine gas.

None of this would happen on its own at room conditions; it occurs only because the external source keeps supplying electrical energy.

Key features (quick bullets)

  • Drives non‑spontaneous reactions (ΔG ≥ 0) using electricity.
  • Has negative cathode and positive anode (opposite sign convention to a galvanic cell).
  • Performs electrolysis: breaking or transforming chemical compounds using electric current.
  • Amount of product formed is proportional to the charge passed (linked to moles of electrons).

Common uses today

  • Electroplating metals like copper, silver, nickel, and chromium onto objects for protection or decoration.
  • Extracting or purifying metals (for example, producing sodium or aluminum from molten salts).
  • Producing gases such as hydrogen and oxygen by water electrolysis.

In many modern batteries, the same physical cell can behave as a galvanic cell when discharging and as an electrolytic cell when being recharged, depending on whether it is supplying current or being driven by an external charger.

Tiny comparison (for context)

  • Galvanic cell: spontaneous reaction makes electricity (like a battery).
  • Electrolytic cell: electricity is used to force a reaction that is not spontaneous.

TL;DR: An electrolytic cell is an electrochemical setup with a power source, two electrodes, and an electrolyte that uses electricity to drive a chemical reaction that would not happen on its own.

Information gathered from public forums or data available on the internet and portrayed here.