What is the difference between a galvanic cell (such as a Daniell cell) and an electrolytic cell?

A Galvanic cell (or voltaic cell) is a device that uses a chemical reaction to generate electrical energy. It consists of two half-cells, each containing a different electrode immersed in an electrolyte. The two half-cells are connected externally through a wire and internally through a salt bridge. In a galvanic cell, the redox reaction happens spontaneously and by this reaction, chemical energy is converted into electrical energy.

An electrolytic cell is a type of electrochemical cell that uses electrical energy to drive a non-spontaneous redox reaction. The construction of this cell is similar to a galvanic cell, but the purpose is to use electrical energy from an external source to cause a chemical change, like in the process of electrolysis.

Now, let's outline the differences between these two forms of cells: \n\n1. Energy Conversion: In a galvanic cell, chemical energy is converted into electrical energy. In an electrolytic cell, electrical energy is used to produce a chemical change.\n\n2. Reaction Spontaneity: The redox reaction in a galvanic cell proceeds spontaneously, while the reaction in an electrolytic cell is non-spontaneous and requires an external energy source.\n\n3. Flow of Electrons: In a galvanic cell, electrons flow from the anode to the cathode via the external circuit, while in an electrolytic cell, the direction of electron flow is from the positive electrode (anode) to the negative electrode (cathode), driven by an external power source.