Question

5 differences b/w galvanic cell and electrolytic cell.

Answer 1

A Galvanic cell is an electrochemical cell that can produce electricity with the help of a chemical reaction. This chemical reaction is a redox reaction which includes an oxidation reaction and a reduction reaction that occur at the same time. An electrolytic cell is a cell that uses an electric current for the progression of a chemical reaction. An electrical current is used in these cells to obtain a non-spontaneous reaction. This is the opposite of the Galvanic cell.

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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