The enthalpy change for the transition of liquid to steam is `40.8kJ mol^(-1)` at 373 K. What is the entropy of vaporization of water in J/mol K?

Explanation

The entropy change for the vapourization of water is given by `Delta S=(Delta H_(vap.))/(T_(vap.))`
Given `Delta H_(vap.)=40.8 kJ mol^(-1) = 40.8xx1000 J mol^(-1)` and T = 373 K
`therefore Delta S=(40.8xx100 Jmol^(-1))/(373 K)=109.38 JK^(-1)mol^(-1)`