Electrolytic cell

An electrolytic cell is an electrochemical cell that utilizes an external source of electrical energy to force a chemical reaction that would otherwise not occur.^[1]^: 64, 89^[2]^: GL7 The external energy source is a voltage applied between the cell's two electrodes; an anode (positively charged electrode) and a cathode (negatively charged electrode), which are immersed in an electrolyte solution.^[1]^: 89^[3]^{[page needed]} This is in contrast to a galvanic cell, which itself is a source of electrical energy and the foundation of a battery.^[1]^: 64 The net reaction taking place in a galvanic cell is a spontaneous reaction, i.e., the Gibbs free energy remains -ve, while the net reaction taking place in an electrolytic cell is the reverse of this spontaneous reaction, i.e., the Gibbs free energy is +ve.^[3]^{[page needed]}

^ ^a ^b ^c Murphy B, Murphy C, Hathaway B, eds. (1997). "Electrochemistry I: Galvanic Cells". A Working Method Approach for Introductory Physical Chemistry Calculations. Cambridge, United Kingdom: Royal Society of Chemistry. ISBN 0-85404-553-8 – via Internet Archive.
^ Harris, Daniel C. (2010). Quantitative Chemical Analysis (8th ed.). New York: W. H. Freeman and Company. ISBN 978-1-4292-1815-3. OCLC 540161465 – via Open Library.
^ ^a ^b Skoog, Douglas A.; West, Donald M.; Holler, F. James; Crouch, Stanley R. (2014). Fundamentals of analytical chemistry. Belmont, CA: Brooks/Cole, Cengage Learning. ISBN 978-0-495-55828-6. OCLC 824171785.