Electrolytic cell Electrolytic cell An electrolytic cell is an electrochemical cell that drives a non-spontaneous redox reaction through the application of electrical energy. They are often used to decompose chemical compounds, in a process called electrolysis—the Greek word lysis means "to break up". Important examples of electrolysis are the decomposition of water into hydrogen and oxygen, and bauxite into aluminium and other chemicals. Electroplating (e.g. of copper, silver, nickel or chromium) is done using an electrolytic cell. Electrolysis is a technique that uses a direct electric current (DC). An electrolytic cell has three component parts: an electrolyte and two electrodes (a cathode
SAL electrolytic capacitor 31, 2015 these are now end-of-life and have ceased production. Basic anode material of solid aluminum capacitors exists of highly purified aluminum with a purity of at least 99.99%. In an electrochemical process the anode material is etched (roughened) to increase the effective electrode surface. After that the roughened aluminum becomes oxidized or formed by an anodic oxidizing process. Thereby an electrical insulating oxide layer AlO is formed on the aluminum surface by applying an electric current in correct polarity in an electrolytic bath. This process of oxide formation is carried out into two reaction steps: The aluminum oxide layer