ThermodynamicsMedium
Question
What is the entropy change when 3.6 g of liquid water is completely converted into vapours at 373 K? The molar heat of vaporization is 40.85 kJ/mol.
Options
A.219.0 J/K
B.2.190 J/K
C.21.90 J/K
D.109.5 J/K
Solution
$\Delta S = \frac{\Delta H_{vap}}{B.P.} = \frac{\frac{40.85}{18} \times 3.6 \times 1000}{373} = 21.9\text{ J/K}$
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