[[FileBerkas:Ice water.jpg|thumb|Es yang meleleh pada suhu ruangan merupakan [[Entropi#Es melebur|contoh]] dari naiknya entropi,<ref group="note">In complex systems of molecules, such as at the [[critical point (thermodynamics)|critical point]] of water or when salt is added to an ice-water mixture, entropy can either increase or decrease depending on system parameters, such as temperature and pressure. For example, if the spontaneous crystallization of a supercooled liquid takes place under adiabatic conditions the entropy of the resulting crystal will be greater than that of the supercooled liquid (Denbigh, K. (1982). ''The Principles of Chemical Equilibrium'', 4th Ed.). In general, however, when ice melts the entropy of the adjoined hot and cold bodies increases. Some further tutorials: [http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA3/MAIN/ENTROPY/PAGE1.HTM Ice-melting] (example by ''[[Journal of Chemical Education]]''—subscription required); [http://web.archive.org/web/20090222060701/http://www.bartleby.com/64/C004/024.html Ice-melting and Entropy Change] (example by ''The American Heritage Book of English Usage''—archive.org copy); [http://web.archive.org/web/20091015043726/http://www.ac.wwu.edu/~vawter/PhysicsNet/Topics/ThermLaw2/Entropy/InterptEntropy.html Ice-melting and Entropy Change] (discussion by [[Western Washington University]]—archive.org copy)</ref> dijelaskan pada tahun 1862 oleh [[Rudolf Clausius]] sebagai kenaikan [[disgregasi]] molekul air pada es.<ref>Clausius, Rudolf (1862). Communicated to the Naturforschende Gesellschaft of Zurich, January 27, 1862; published in the Vierteljahrschrift of this Society, vol. vii. p. 48; in Poggendorff’s Annalen, May 1862, vol. cxvi. p. 73; in the Philosophical Magazine, S. 4. vol. xxiv. pp. 81, 201; and in the Journal des Mathematiques of Paris, S. 2. vol. vii. p. 209.
