You are given normal boiling points and standard enthalpies of vaporization, Calendly. the entropy of vaporization of liquids listed below.

Explanation

For ethanol :
Given :
`T_b=78.4^@C=(78.4+273)`
=351.4 K
`DeltaH_V` (ethanol)=`+42.4 "kJ mol"^(-1)`
`DeltaS_V=(DeltaH_V)/T_b`
`DeltaS_V=(+42.4 "kJ mol"^(-1))/"351.4 K"`
`DeltaS_V=(+42.400 "J mol"^(-1))/"351.4 K"`
`DeltaS_V=+120.66 J K^(-1) "mol"^(-1)`
For Toluene :
Given :
`T_b=110.6^@C`=(110.6+273)
=383.6 K
`DeltaH_V`(toluene )=+35.2 kJ `"mol"^(-1)`
`DeltaS_V=(DeltaH_V)/T_b`
`DeltaS_V=(+35.2 "kJ mol"^(-1))/(383.6 K)`
`DeltaS_V=(+35200 J mol^(-1))/(383.6 K)`
`DeltaS_V=+91.76 J K^(-1) mol^(-1)`