Electrochemistry is a branch
of chemistry that deals with the study of chemical reactions that involve the
transfer of electrons between reactants. It involves the study of the
relationship between electricity and chemical reactions, and the application of
this knowledge in various fields such as energy storage, corrosion prevention,
and the production of metals and chemicals.
In electrochemical
reactions, the transfer of electrons occurs between two species, typically an
oxidizing agent (also called an oxidant or electron acceptor) and a reducing
agent (also called a reductant or electron donor). This transfer of electrons
leads to the formation of ions or molecules with different charges and is
accompanied by a flow of electrical current.
Electrochemical cells are
devices that utilize electrochemical reactions to convert chemical energy into
electrical energy or vice versa. They are made up of two half-cells, each
containing an electrode immersed in an electrolyte solution. The electrodes can
be made of different materials and can be either anodic (positive electrode) or
cathodic (negative electrode).
In a galvanic cell, also
known as a voltaic cell, the chemical energy is converted into electrical
energy as a result of a spontaneous redox reaction. This reaction causes
electrons to flow from the anode to the cathode through an external circuit,
generating an electric current. In contrast, in an electrolytic cell,
electrical energy is used to drive a non-spontaneous redox reaction. This
involves applying a voltage to the cell that is greater than the voltage
generated by the redox reaction to drive the reaction in the opposite
direction.
Electrochemistry has many
practical applications, including the production of electricity in batteries
and fuel cells, the corrosion prevention of metals, and the extraction and
refining of metals. It is also used in the production of various chemicals,
such as chlorine and sodium hydroxide, through the process of electrolysis.
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