Everything about Electrochemical Cell totally explained
An
electrochemical cell is a device used for creating an
electromotive force (
voltage) and current from
chemical reactions. The current is caused by the reactions releasing and accepting
electrons at the different ends of a conductor. A common example of an electrochemical cell is a standard 1.5-volt
battery.
Overview
Each
half-cell consists of an electrode with atoms, and an electrolyte with ions that undergo either
oxidation or reduction. In a full electrochemical cell, ions from the electrolyte of one half-cell lose electrons (oxidation) to their
electrode while ions from the electrolyte of other half-cell gain electrons (reduction) from their electrode. If the atoms/ions involved in the electrode reactions are
metal, then the same metal can be used for each electrode. If the
atoms/
ions involved in the reaction at each half-cell are not metal, then no electrode can be constructed out of those ions in atomic form; nonreactive metals such as
platinum then can be used as a substitute electrode (as in the
standard hydrogen electrode). Finally, a
salt bridge is often employed to provide electrical contact between two half-cells with very different electrolytes—to prevent the solutions from mixing. This can simply be a strip of
filter paper soaked in saturated potassium nitrate (V) solution.
Each half-cell has a characteristic voltage. Different choices of substances for each half-cell give different potential differences. Each reaction is undergoing an
equilibrium reaction between different oxidation states of the ions—when equilibrium is reached the cell can't provide further voltage. In the half-cell which is undergoing oxidation, the closer the equilibrium lies to the ion/atom with the more positive oxidation state the more potential this reaction will provide. Similarly, in the reduction reaction, the further the equilibrium lies to the ion/atom with the more
negative oxidation state the higher the potential.
This potential can be predicted quantitatively through the use of
electrode potentials (the voltage measured when the substance is connected to
hydrogen). The difference in voltage between electrode potentials gives a prediction for the potential measured. Spontaneity of a chemical reaction is determined by the overall cell potential E
cell. If E
cell>0, the reaction is spontaneous and if E
cell<0, the reaction won't be spontaneous.
The
potential window is the electrochemical voltage range between which a substance doesn't get oxidized or reduced.
Cell types
Further Information
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