In complex systems of molecules, such as at the 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: Ice-melting (example by Journal of Chemical Education—subscription required); Ice-melting and Entropy Change (example by The American Heritage Book of English Usage—archive.org copy); Ice-melting and Entropy Change (discussion by Western Washington University—archive.org copy)
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In complex systems of molecules, such as at the 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: Ice-melting (example by Journal of Chemical Education—subscription required); Ice-melting and Entropy Change (example by The American Heritage Book of English Usage—archive.org copy); Ice-melting and Entropy Change (discussion by Western Washington University—archive.org copy)
