Galvanic Cell Vs Electrolytic. Electrolytic cells are non-spontaneous and require an external power source to drive the chemical reaction. Imagine a world where chemistry powers your gadgets and drives industrial processes
from
Galvanic cells generate electrical energy through spontaneous redox reactions, while electrolytic cells require an external source of electrical energy to drive non-spontaneous redox reactions. In other words, cells can either be used to produce an electric current from chemical compounds or to apply electric current for the completion of a chemical reaction
Electrodes: Similar to galvanic cells, electrolytic cells employ two electrodes; however, the anode is connected to the positive terminal of the power source and the cathode to the negative terminal Imagine a world where chemistry powers your gadgets and drives industrial processes A galvanic cell is an electrochemical cell in which spontaneous redox processes occur allowing the continuous flow of electrons through the conductor, whereas, in an electrolytic cell, the redox reactions are influenced by an external source of current
Galvanic Cell Vs Electrolytic Cell. Imagine a world where chemistry powers your gadgets and drives industrial processes Two electrodes (anode and cathode) and an electrolyte make up the three main components of a typical electrolytic cell
Difference Between Electrochemical Cell and Electrolytic Cell Definition, Properties, How it Works. In physical chemistry, a cell is a system that is used to relate chemicals with electricity The electrolytic cell uses an electric current for the propagation of a chemical reaction