important of electrolysis
TRANSCRIPT
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Important Of ElectrolysisElectrolysis is a hugely important process
- it is used industrially in a number of
ways:
(1)The extraction of metals, notably
aluminium, magnesium, and sodium..
(2) The refining of metals, such as copper
and zinc.
(3) Electroplating
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Extraction of Aluminium:
Aluminium is obtained by the electrolytic reduction of its
molten oxide, (alumina). Because alumina has a very high melting point (2045
C), the mineral cryolite is added to lower the meltingpoint in order that the electrolysis may be carried out atabout 950 C.
The electrolytic cell has carbon anodes and a carboncathode (which forms the lining of the tank in which theelectrolysis takes place).
Carbon dioxide is formed at the anodes, and aluminium
at the cathode. It is heavier than the molten alumina/cryolite mixture,
and sinks to the bottom of the cell, where it is tapped off.The procedure is known as the Hall-Hroult process.
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Electrorefining of copper:
When copper is first obtained by reductionof its ores, it is cast as impure slabs oringots, called blister copper.
In the electrorefining process, the blisteringots are used as anodes in anelectrolytic cell, where an acid solution ofcopper (II) sulphate is used as electrolyte.
Initially, the cathodes consist of thin sheetsof pure copper
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During electrolysis, copper passes into solution
from the anodes, (leaving the impurities,
normally containing silver, gold and platinum)as an anode slime, which sinks to the bottom
of the cell. The anode reaction is
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At the cathode, copper (II) ions are
discharged and the pure copper sheet
becomes coated with an increasingly thick
layer of very pure copper:
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Electroplating:
Electroplating consists of depositing a thin
layer of a metal on another, either for
protection or for the sake of appearance.
a brass or nickel object is coated with a
layer of silver by making use of electrolysis
of a silver solution, using the object to be
coated as the cathode:
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Electroplating is used to:
(a) Avoid metal corrosion
(b) Prevent iron from rusting
(c) To make objects to look shiny and better
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Production Of Electrical Energy By
A Simple Cell
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The CELL
A cell is a device that transforms chemical
energy into electrical energy
It consists a piece carbon (C) and a piece
zinc (Zn) suspended in a jar that contains
a solution water and sulfuric acid
A cell is a device in which chemical energy
is converted to electrical energy.
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The current flow is the movement of
electrons from the negative electrode the
cell (zinc) and to the positive electrode
(carbon).
This causes fewer electrons in the zinc
and an excess electrons in the carbon.
The hydrogen ions (H2) from the sulfuric
acid being attracted to the carbon
electrode.
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The zinc electrode has a positive chargebecause it has lost electrons to the carbon
electrode. This positive charge attracts the negative
ions (S04) from the sulfuric acid.
The negative ions combine with the zinc toform zinc sulfate.
This action causes the zinc electrode to beeaten away. Zinc sulfate is a grayish-whitesubstance that is sometimes seen on thebattery post an automobile battery.