Chapter 17, Problem 34E

Interpretation Introduction

Introduction:

The entropy change of system increases with increase in the disorders. For example, increase in the number of moles of gaseous products over the number of moles of gaseous reactants increases the entropy of the system and, thus, $\Delta S_{sys}$ will be positive. The entropy change of surroundings $\left(\Delta S_{surr} \right)$ is negative of the ratio of enthalpy change of system $\left(\Delta H_{sys} \right)$ to absolute temperature (T).

$\begin{array}{l}\Delta S_{\text{surr}}=-\frac{\Delta H_{\text{rxn}}or\Delta H_{\text{sys}}}{T}\mathrm{......}\left(1\right)\\ \Delta S_{\text{univ }}=\Delta S_{\text{surr}}+\Delta S_{\text{sys}}\end{array}$