For a phase transition like melting of ice, the entropy change ($\Delta_{fus} S$) is given by the formula: $\Delta_{fus} S = \frac{\Delta_{fus} H}{T_f}$ where $\Delta_{fus} H$ is the enthalpy of fusion and $T_f$ is the freezing/melting point in Kelvin. Given: $\Delta_{fus} H = 1.435 \text{ kcal/mol} = 1435 \text{ cal/mol}$ $T_f = 0^\circ\text{C} = 273 \text{ K}$ Substituting the values: $\Delta_{fus} S = \frac{1435 \text{ cal/mol}}{273 \text{ K}} \approx 5.256 \text{ cal/(mol K)}$ This value is closest to $5.260 \text{ cal/(mol K)}$.