Fundamentals of Biochemistry: Life at the Molecular Level 5th Edition

Published by Wiley
ISBN 10: 1118918401
ISBN 13: 978-1-11891-840-1

Chapter 1 - Introduction to the Chemistry of Life - Exercises - Page 21: 11

Answer

$\Delta G=\Delta H-T \Delta S$ $\Delta G=-7000 \mathrm{\ J} \cdot \mathrm{mol}^{-1}-(298 \mathrm{\ K})\left(-25 \mathrm{\ J} \cdot \mathrm{\ K}^{-1} \cdot \mathrm{mol}^{-1}\right)$ $\Delta G=-7000+7450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}=450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}$ $\text{The reaction is not spontaneous because $\Delta G>0 .$ The temperature}$ $\text{must be decreased in order to decrease the value of the $T \Delta S$ term.}$

Work Step by Step

$\Delta G=\Delta H-T \Delta S$ $\Delta G=-7000 \mathrm{\ J} \cdot \mathrm{mol}^{-1}-(298 \mathrm{\ K})\left(-25 \mathrm{\ J} \cdot \mathrm{\ K}^{-1} \cdot \mathrm{mol}^{-1}\right)$ $\Delta G=-7000+7450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}=450 \mathrm{\ J} \cdot \mathrm{mol}^{-1}$ $\text{The reaction is not spontaneous because $\Delta G>0 .$ The temperature}$ $\text{must be decreased in order to decrease the value of the $T \Delta S$ term.}$
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