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(i) Define Gibb's free energy. (ii) You...

(i) Define Gibb's free energy.
(ii) You are given normal boiling points and standard enthalpies of vapourisation. Calculate the entropy of vapourisation of liquids listed below.

Text Solution

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(i) Gibbs free energy is defined as the part of total energy of a system that can be converted (or) available for conversion into work.
G=H-TS, where G = Gibb.s free energy
  H enthalpy : T - temperature , S = entropy
  (ii) For ethanol,
Given: `T_(b)=78.4^(@)C=(78.4+273)=351.4K`
`DeltaH_(v)`(ethanol) = `+ 42.4 kJ mol^(-1)`
`DeltaS_(v)=(DeltaH_(v))/(T_(b))=(+42+kJ mol^(-1))/(351.4.K)=(+42400 J mol^(-1))/(351.4 K)`
`DeltaS=+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))=(+35.2 kJ mol^(-1))/(383.6 K)=(+ 35200 J mol^(-1))/(383.6K)`
`DeltaS_(v)=+91.76 J K^(-1)mol^(-1)`
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