Question 19.1: Calculating the Entropy Change for a Phase Transition The he...
Calculating the Entropy Change for a Phase Transition
The heat of vaporization, \Delta H_{\text {vap }}, of carbon tetrachloride, \mathrm{CCl}_{4}, at 25^{\circ} \mathrm{C} is 39.4 \mathrm{~kJ} / \mathrm{mol}.
\mathrm{CCl}_{4}(l) \longrightarrow \mathrm{CCl}_{4}(g) ; \Delta H_{\text {vap }}=43.0 \mathrm{~kJ} / \mathrm{mol}
If 1 \mathrm{~mol} of liquid carbon tetrachloride at 25^{\circ} \mathrm{C} has an entropy of 216 \mathrm{~J} / \mathrm{K}, what is the entropy of 1 \mathrm{~mol} of the vapor in equilibrium with the liquid at this temperature?
PROBLEM STRATEGY
The entropy change for this equilibrium vaporization is \Delta H_{v a p} / T. The entropy of the vapor equals the entropy of the liquid plus the entropy change.
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