Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 16 - Thermodynamics: Directionality of Chemical Reactions - Problem Solving Practice 16.2 - Page 704: c



Work Step by Step

Usually when a pure solid dissolves in a solvent, entropy increases. So, KOH(aq) is expected to have greater entropy than KOH(s). We see from table 16.1 that our prediction is correct. $S^{\circ}(KOH,s)=78.9\,JK^{-1}mol^{-1}$ $S^{\circ}(KOH,aq)=91.6\,JK^{-1}mol^{-1}$
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