An electrolytic cell, also known as an electrochemical cell, is a device that utilizes electrical energy to drive a non-spontaneous redox reaction.
This process facilitates the decomposition of chemical compounds through electrolysis.
Electrolysis involves the passage of a direct electric current through a liquid containing ions, causing the compounds to disintegrate.
Electrolytic cells are essential in various applications, including the decomposition of water into hydrogen and oxygen, the extraction of metals like aluminium from bauxite, and electroplating metals such as copper, silver, nickel, and chromium.
5 Key Points Explained
Definition and Function of Electrolytic Cells
An electrolytic cell is an electrochemical device that drives a non-spontaneous redox reaction by applying electrical energy.
The primary function of an electrolytic cell is to decompose chemical compounds through electrolysis, a process where electrical energy is converted to chemical energy.
Components of an Electrolytic Cell
Typically, an electrolytic cell consists of two inert electrodes, usually made of graphite or platinum wire, which pass electric current into the electrolyte.
The electrolyte is a conducting liquid, either a molten ionic compound or an ionic solution, that allows the movement of ions necessary for the electrolytic process.
The power source, symbolized by a short fat line (negative) and a long thin line (positive), provides the necessary electrical energy to drive the reaction.
Processes Occurring in an Electrolytic Cell
Oxidation occurs at the positive electrode (anode), where negative ions lose electrons.
Reduction occurs at the negative electrode (cathode), where positive ions gain electrons.
Positive ions in the electrolyte migrate to the cathode, combining with electrons to become new ions or neutral particles.
Negative ions migrate to the anode, transferring electrons and becoming new ions or neutral particles.
Applications of Electrolytic Cells
Electrolytic cells are used to decompose water into hydrogen and oxygen.
They are employed in the extraction of metals like aluminium from bauxite.
Electrolytic cells facilitate the electroplating of metals such as copper, silver, nickel, and chromium.
They are used in the production of caustic soda and other chemicals through electrolysis.
Comparison with Galvanic Cells
Galvanic Cells, also known as voltaic cells, generate electrical energy from spontaneous redox reactions.
In contrast, electrolytic cells use electrical energy to drive non-spontaneous redox reactions, converting electrical energy into chemical energy.
In summary, an electrolytic cell, or electrochemical cell, is a crucial device in various industrial and scientific processes.
It enables the decomposition of compounds and the transformation of electrical energy into chemical energy through the controlled application of electric current.
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