16.3 Exercise 8

By calculating ΔS_univ at each temperature, determine if the melting of 1 mole of NaCl(s) is spontaneous at 500 °C and at 700 °C.
$S_{\text{NaCl} \left(s\right)}^{\circ} = 72.11 \frac{\text{J}}{\text{mol}\cdot\text{K}} S_{\text{NaCl} \left(l\right)}^{\circ} = 95.06 \frac{\text{J}}{\text{mol}\cdot\text{K}} \Delta H_{\text{fusion}}^{\circ} = \text{27}.\text{95 kJ}/\text{mol}$

What assumptions are made about the thermodynamic information (entropy and enthalpy values) used to solve this problem?