Electrolytic cell

An electrolytic cell is an electrochemical cell that uses an external source of electrical energy to drive a non-spontaneous chemical reaction, a process known as electrolysis.[1]: 64, 89 [2]: GL7  In the cell, a voltage is applied between the two electrodes—an anode (positively charged) and a cathode (negatively charged)—immersed in an electrolyte solution.[1]: 89 [3] This contrasts with a galvanic cell, which produces electrical energy from a spontaneous chemical reaction and forms the basis of batteries.[1]: 64  The net reaction in an electrolytic cell is a non-spontaneous (Gibbs free energy is positive), whereas in a galvanic cell, it is spontaneous (Gibbs free energy is negative).[3]

  1. ^ 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.
  2. ^ 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.
  3. ^ 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.
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