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Calculate the entropy change involved in the conversion of one mole of liquid water at 373 K to vapour at the same temperature (latent heat of vaporization of water Δvap H = 2.257 kJ/g). |
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Answer» For the conversion of water→ vapour, the entropy change is given by Δvap S = ΔvapH/Tb Here, Δvap H = 2.257 kJ/g = 2.257 × 18 kJ/mol = 40.626 kJ/mol, Tb = 373 K ∴ Δvap S = 40.625KJ mol-1/373 = 0.1089 KJ K-1 mol–1 = 108.9 J K–1 mol–1 . |
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