Chemistry - Thermodynamics - II Question with Solution | TestHub

Given enthalpy of vaporization, $$\Delta \mathrm{H}=186.5\mathrm{kJ}{\mathrm{mol}}^{-1}$$ Boiling point of water $$=100^{\circ }\mathrm{C}=100+273=373\mathrm{K}$$ Entropy change, $$\begin{array}{r}\Delta \mathrm{S}=\frac{\Delta \mathrm{H}}{\mathrm{T}}=\frac{186.5\mathrm{kJ}{\mathrm{mol}}^{-1}}{373\mathrm{K}}\\ =0.5\mathrm{kJ}{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}\end{array}$$