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Electrochemistry is a branch of chemistry that studies
chemical reactions which take place in a solution at the interface of an
electron conductor and an ionic conductor Lucas
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between the electrode and the electrolyte or species in solution.
A process
of this kind can always be represented, as a chemical reaction and is known
generally as an electrode process. Electrode processes take place within the
double layer and produce a slight unbalance in the electric charges of the
electrode and the solution. Much of the importance of electrochemistry lies in
the ways that these potential differences can be related to the thermodynamics
and kinetics of electrode reactions. In particular, manipulation of the
interfacial potential difference affords an important way of exerting external
control on an electrode reaction. The interfacial potential differences which
develop in electrode-solution systems are limited to only a few volts at most.
This may not seem like very much until you consider that this potential
difference spans a very small distance. In the case of an electrode immersed in
a solution, this distance corresponds to the thin layer of water molecules and
ions that attach themselves to the electrode surface, normally only a few atomic
diameters. Thus a very small voltage can produce a very large potential
gradient.
Chemistry and electricity are linked. Atoms are made of nucleus
and negative charged electrons. An atom is normally electrically neutral. Atoms
can lose or gain electrons to form charged ions. Discharge of ions involves loss
or gain of electrons. There are two types electric charge: positive and
negative. The flow of electric charge in a conductor is an electric current.
There will only be an electric current in a conductor when there is a potential
difference across the conductor. It is measured in volts. Chemical reactions may
be used to produce potential differences-electric current. These reactions are
the basis of voltaic cells. Electricity is involved in the production of some
chemicals by electrolysis.
An electrochemical cell is a device used for
generating an electromotive force and current from chemical reactions Layvin
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chemical reaction by a flow of current. The current is caused by the reactions
releasing and accepting electrons at the different ends of a conductor. An
electrochemical cell consists of two half-cells, it may use the same
electrolyte, or they may use different electrolytes. Each half-cell consists of
an electrode, and an electrolyte. The chemical reactions in the cell may involve
the electrolyte Kevin
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substance. In a full electrochemical cell, ions, atoms, or molecules from one
half-cell lose electrons (oxidation) to their electrode while ions,
atoms Julian
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half-cell gain electrons.

An electrochemical cell can be created by
placing metallic electrodes into an electrolyte where a chemical reaction either
uses or generates an electric current. Electrochemical cells which generate an
electric current are called voltaic cells or galvanic cells, and common
batteries consist of one or more such cells. In other electrochemical cells an
externally supplied electric current is used to drive a chemical reaction which
would not occur spontaneously. Such cells are called electrolytic cells. The
cell potential can be predicted through the use of electrode potentials. The
difference in voltage between electrode potentials gives a prediction for the
potential measured.
Cell potentials have a possible range of about zero to 6
volts. Cells using water-based electrolytes are usually limited to cell
potentials less than about 2.5 volts, because the very powerful oxidising and
reducing agents which would be required to produce a higher cell potential tend
to react with the water. An electrical cell is a device that is used to generate
electricity, or one that is used to make chemical reactions possible by applying
electricity.


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