presentation on electrolysis

2. In chemistry, the production of
chemical changes by passing and
electric current through a solution
or molten salt (electrolyte) resulting
in the migration of ions to the
electrode: positive ions (cations) to
the negative electrode(cathode)
and negative ions (anions) to the
positive electrode (anode).

3. During electrolysis, the ions
react with the electrode, either
receiving or giving up electrons.
The resultant atoms may be
liberated as gas or deposit as a
solid on the electrode, in
amount that are proportional to
the amount of current passed.

4. If negative ions move towards
the anode they lose electrons
and become neutral, resulting
in an oxidation reaction. If
positive ion move towards the
cathode and gain electron
becoming neutral. A reduction
reaction takes place.

5. Michael Faraday (1791-1867)

6. At anode
For CuS
At cathode

7. Electrolysis is used for many
purposes, including the
extraction of metals from
ores, the cleaning of
archaeological artefacts, and
the coating of materials with
thin layers of metals.

10. Faraday’s laws of electrolysis
Michael Faraday discovered a
quantitative relationship
between the extent of
electrolysis and the quantities
of electricity passed and put
forward two laws.

11. First law
It states that the mass of a substance
liberated at the electrode is directly
proportional to the quantity of electricity
passed through the electrolyte.
Where z: is the constant called
electrochemical equivalent
I: is the current in ampere and
t: is the time in seconds.

12. Second law
It also states that, when the same
quantity of electricity is passed
through different electrolytes the
masses of substances formed at the
electrodes are proportional to their
equivalent masses.
i.e, =

13. THANK YOU