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Electrochemistry
Module: General and Organic Chemistry (AOC106DI)
26 Documents
Students shared 26 documents in this course
University: Coventry University
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Electrochemistry
The oxidised reducing agent is known as the reductant (loses electrons).
The oxidant is an oxidising agent that has been reduced (gains electrons).
In a redox reaction, electrons are transported. An electric potential (E) is formed as a result
of their charge.
A half reaction is the name given to each component. Reduction and oxidation are required
half processes. An oxidation half reaction is the inverse of a reduction half reaction.
The half reactions are all represented as reduction potentials in the standard reduction
potential table. Simply invert the half equation and the sign of the reduction potential to
discover the oxidation potential.
Chemical energy is converted into electrical energy by a galvanic cell. To generate electricity,
it employs a spontaneous redox process.
The oxidation and reduction components of the galvanic cell are separated and carried in
two distinct containers. Copper is put in a CuSO4 solution while zinc is put in a ZnSO4
solution.
Electrodes are the metallic rods in a galvanic cell.
By releasing electrons, Zn metal dissolves in zinc sulphate solution, which climb up through
the external wire, pass through the voltmeter to register the voltage, enter the copper
sulphate solution through the copper electrode, and then reduce the Cu+2 ions to copper
metal. As a result, the Zn electrode undergoes oxidation whereas the Cu electrode
undergoes reduction.
Anode refers to the Zn electrode. The cathode is the Cu electrode. The anode is where
oxidation (the loss of electrons) occurs, while the cathode is where reduction (the gain of
electrons) occurs. Each reaction is half of the total cell reaction, therefore the name half-cell
reaction.
A spontaneous redox reaction is utilised to produce current in a galvanic cell, whereas
current is used to drive a non-spontaneous reaction in an electrolytic cell.
