Electrochemistry. Galvanic and electrolytic cells

Electrochemistry is a branch of chemistry that studies chemical reactions involving electron transfer, i.e. the conversion of chemical energy into electrical energy and vice versa. These reactions occur in systems called electrochemical cells, which consist of two electrodes immersed in a conductive solution called electrolyte.

In an electrochemical cell, the electrodes are composed of conductive materials, such as metals or semiconductors, and are connected through an external circuit. During the reaction, electrons are transferred from one electrode to another through the external circuit, while ions move through the electrolyte to maintain charge neutrality.

There are two main types of electrochemical cells: galvanic cells (also known as batteries) and electrolytic cells. In a galvanic cell, the spontaneous chemical reaction generates electricity. This is the principle used in common batteries, such as alkaline or lithium-ion batteries.

On the other hand, electrolytic cells are devices in which an external electric current is applied to force a non-spontaneous chemical reaction. This process is used in electrolysis, where the components of a substance can be separated by applying an electric current, as in obtaining metals from their compounds or in the production of gases such as hydrogen and oxygen from water.

Electrochemistry has applications in many fields. In industry, for example, it is used for metal production, electroplating and surface coating. In the field of energy, electrochemistry is central to the generation and storage of energy in rechargeable batteries and fuel cell technology. In addition, electrochemistry plays an essential role in the research and development of new materials and in catalysis, which is the increase in the rate of chemical reactions by involving electrochemical catalysts.