General Chemistry 10th Edition

Published by Cengage Learning
ISBN 10: 1-28505-137-8
ISBN 13: 978-1-28505-137-6

Chapter 18 - Thermodynamics and Equilibrium - Questions and Problems - Page 770: 18.32


Please see the work below.

Work Step by Step

We know that $\Delta H=1.34 mol\times \frac{26.7Kj}{1 mol}=3.5778\times 10^4J$ Now $\Delta S=\frac{\Delta H}{T}$ We plug in the known values to obtain: $\Delta S=\frac{3.5778\times 10^{4}}{35.6+273}=115.93\frac{J}{mol.K}$
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