Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 5 - Thermochemistry - Exercises: 5.45c


60.6 Joules

Work Step by Step

The dissolution of AgCl in water would be the reverse of the reaction shown so we must multiply the $\Delta H$ by negative 1 as follows; AgCl --> Ag+ + Cl- $\Delta H$ = 65.5 kJ This means one mole of AgCl dissolving into its constituent ions has a $\Delta H $ of 65.5kJ so then 9.25 x 10^-4 mol would release 9.25 x 10^-4 * 65.5kJ = 0.0606 kJ or 60.6 Joules
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