Electrochemistry( grade 10)

GALVANIC (VOLTAIC) CELLS

•Galvanic cell are electrochemical cells that convert chemical energy into electrical energy.

• The reaction that occurs inside the Galvanic cell is a
spontaneous redox reaction. Once the reaction starts, it
will proceed on its own without any external influence.
This enables the cell to generate electricity.

• Galvanic or voltaic cells are classified into
-› primary cells,
-›secondary cells and
-›Fuel cells.

Primary cells

• Primary cells are Galvanic cells that cannot be recharged.

This is because the electrode reaction as well as the entire
cell reaction cannot be reversed on recharging.
• Once the chemicals in the cells that serve as reactants are
completely used up, it is not possible to recover them by
charging the cells.

• Examples of primary cells include Daniel’s cell and zinc-
carbon (Le Clanche) dry cell.

• The common feature of all Galvanic cells is that they
contain two electrodes in contact with an electrolyte.
• The electrolyte in Galvanic cells can be in the form of a
solution (Daniell cell ) or a paste (Le Clanche cell).

• The cells containing electrolytes in the form of solution are called wet cells, and those containing electrolytes in the form of paste are called dry cells

• Example of a wet primary cell is the Daniell cell.

• Daniell cell is a Galvanic cell that was invented by the
British Chemist John Daniell in 1836

• Daniell cell consists of a zinc strip placed in ZnSO4
solution in one compartment and a copper strip placed in
CuSO4
solution in another compartment.
• Each compartment is called a half-cell, and the reactions
occurring in each compartment are called half-cell
reactions. The solutions in the two compartments are
joined by a salt bridge.

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