Define galvanic cell and its uses
Galvanic Cell and Its Uses:
- A galvanic cell, also known as a
voltaic cell, is a type of electrochemical cell that generates an
electric current through a redox reaction.
- A redox reaction is a
chemical reaction in which one species is oxidized (loses electrons) and
another species is reduced (gains electrons).
- The galvanic cell
consists of two half-cells, each containing an electrode and an
electrolyte solution.
- The two half-cells are separated by a porous
membrane, which allows ions to flow freely but prevents the mixing of
the two solutions.
- The electrodes and electrolytes are chosen so that
one electrode is an oxidizing agent and the other electrode is a
reducing agent.
- Galvanic cells have many practical applications,
including batteries, electroplating, and water treatment.
- Batteries use
galvanic cells to store and release electrical energy.
- Electroplating
uses galvanic cells to deposit a thin layer of metal onto a surface, for
example, to improve the corrosion resistance of a metal.
- In water
treatment, galvanic cells are used to disinfect water by generating
chlorine gas.
- In conclusion, Faraday's Laws of Electrolysis and
galvanic cells are important concepts in the field of electrochemistry.
- Faraday's Laws describe the relationship between the amount of electric
charge passed through a solution and the amount of product formed during
an electrolysis reaction.
- Galvanic cells use redox reactions to
generate an electric current and have many practical applications in
batteries, electroplating, and water treatment.
