If the enthalpy of vaporisation of water is `186.5 J mol^(-1)`, then entropy of its vaporisation will be

Options

A. `0.5 JK^(-1) mol^(-1)`
B. `1.0 JK^(-1) mol^(-1)`
C. `1.5 JK^(-1) mol^(-1)`
D. `12 J K^(-1) mol^(-1)`

Answer

A

Explanation

`Delta S_("vap")=(Delta H_("vap"))/(T_(b))=(186.5)/(373) =0.5 JK^(-1) mol^(-1)`