Calorimetric study of the entropy relation in the NaCl–KCl system

The heat capacity of one Na-rich and two K-rich samples of the NaCl–KCl (halite–sylvite) crystalline solution was investigated between 5 and 300 K. It deviated positively from ideal behaviour with a maximum at 40 K. The thereby produced excess entropy at 298.15 K was described by a symmetric Margule...

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Detalles Bibliográficos
Autores principales: Benisek, Artur, Dachs, Edgar
Formato: Online Artículo Texto
Lenguaje:English
Publicado: Academic Press 2013
Materias:
Article
Acceso en línea:https://www.ncbi.nlm.nih.gov/pmc/articles/PMC4047613/
https://www.ncbi.nlm.nih.gov/pubmed/24926102
http://dx.doi.org/10.1016/j.jct.2013.03.015
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author Benisek, Artur
Dachs, Edgar
author_facet Benisek, Artur
Dachs, Edgar
author_sort Benisek, Artur
collection PubMed
description The heat capacity of one Na-rich and two K-rich samples of the NaCl–KCl (halite–sylvite) crystalline solution was investigated between 5 and 300 K. It deviated positively from ideal behaviour with a maximum at 40 K. The thereby produced excess entropy at 298.15 K was described by a symmetric Margules mixing model yielding [Formula: see text]  = 8.73 J/mol/K. Using enthalpy of mixing data from the literature and our data on the entropy, the solvus was calculated for a pressure of 10(5) Pa and compared with the directly determined solvus. The difference between them can be attributed to the effect of Na–K short range ordering (clustering).
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spelling pubmed-40476132014-06-10 Calorimetric study of the entropy relation in the NaCl–KCl system Benisek, Artur Dachs, Edgar J Chem Thermodyn Article The heat capacity of one Na-rich and two K-rich samples of the NaCl–KCl (halite–sylvite) crystalline solution was investigated between 5 and 300 K. It deviated positively from ideal behaviour with a maximum at 40 K. The thereby produced excess entropy at 298.15 K was described by a symmetric Margules mixing model yielding [Formula: see text]  = 8.73 J/mol/K. Using enthalpy of mixing data from the literature and our data on the entropy, the solvus was calculated for a pressure of 10(5) Pa and compared with the directly determined solvus. The difference between them can be attributed to the effect of Na–K short range ordering (clustering). Academic Press 2013-07 /pmc/articles/PMC4047613/ /pubmed/24926102 http://dx.doi.org/10.1016/j.jct.2013.03.015 Text en © 2013 Elsevier Ltd. https://creativecommons.org/licenses/by-nc-nd/3.0/ Open Access under CC BY-NC-ND 3.0 (https://creativecommons.org/licenses/by-nc-nd/3.0/) license
spellingShingle Article
Benisek, Artur
Dachs, Edgar
Calorimetric study of the entropy relation in the NaCl–KCl system
title Calorimetric study of the entropy relation in the NaCl–KCl system
title_full Calorimetric study of the entropy relation in the NaCl–KCl system
title_fullStr Calorimetric study of the entropy relation in the NaCl–KCl system
title_full_unstemmed Calorimetric study of the entropy relation in the NaCl–KCl system
title_short Calorimetric study of the entropy relation in the NaCl–KCl system
title_sort calorimetric study of the entropy relation in the nacl–kcl system
topic Article
url https://www.ncbi.nlm.nih.gov/pmc/articles/PMC4047613/
https://www.ncbi.nlm.nih.gov/pubmed/24926102
http://dx.doi.org/10.1016/j.jct.2013.03.015
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