Question

write any four differences between Galvanic cell and electrolytic cell

Answer 1

Galvanic cells are devices where the two half reactions of a redox reaction are happening in different chambers, and the electrons flow from one to the other chamber through wires. Galvanic cells are exergonic, with a negative free energy change; the reaction "wants" to happen. Batteries are galvanic cells. Electrolytic cells are the same thing except that they have a positive free energy change. They use electrical energy to drive chemistry. Usually they are used to reduce metal ions to metal on something that we want a new metal plated on.

Answer 2

Hey !!

DIFFERENCES BETWEEN ''Galvanic cell and electrolytic cell''

GALVANIC CELL

• It is a device to convert chemical energy into electrical energy, i.e electrical energy is produced as result of the redox reaction taking place. Hence, free energy change (ΔG) is negative.
• It is based upon the redox reaction which is spontaneous.
• Two electrodes are usually set up in two separate beakers.
• The electrolytes taken in the two beakers are different.
• The electrodes taken are of different materials.
• To set up this cell, a salt bridge/porous pot is used.

ELECTROLYTIC CELL

• It is a device to convert electrical energy into chemical energy, electrical energy is supplied to the electrolyte solution to bring about the redox reaction (i.e electrolysis). Hence free energy change (ΔG) is positive.
• The redox reaction is non-spontaneous and takes place only when electrical energy is supplied.
• Both the electrodes are suspended in the solution or melt of the electrolyte in the same beaker.
• Only one electrolyte is taken.
• The electrodes taken may be of the same or different materials.
• No salt bridge is used in this case.

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