Determine the change in entropy ΔS (in SI unit) of 100gm of water when it is heated to the boiling point from room temperature of T=300K , and it is transformed into vapour at the boiling temperature and atmospheric pressure. It is given that for water: the molar heat capacity C=75.4J/(mol - K) ; latent heat of vaporization :L=2.26MJ/kg [Take ln(1 .24)=0.217 ]

Question

Determine the change in entropy ΔS (in SI unit) of 100gm of water when it is heated to the boiling point from room temperature of T=300K , and it is transformed into vapour at the boiling temperature and atmospheric pressure. It is given that for water: the molar heat capacity C=75.4J/(mol - K) ; latent heat of vaporization :L=2.26MJ/kg [Take ln(1 .24)=0.217 ] (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Δ S=nCln((Tb/T))+(m L/Tb)=697JK- 1

ΔS=nCln(TTb​​)+Tb​mL​=697JK−1

$Δ S = n Cl n (\frac{T _{b}}{T}) + \frac{m L}{T _{b}} = 697 J K^{- 1}$