Answer:
The change in entropy is -1.66 kJ/K.
Explanation:
Heat of vaporization of acetic acid = 41.0 kJ/mol
Heat of condensation of acetic acid = -41.0 kJ/mol
Mass of acetic acid = 954 g
Condensing temperature of acetic acid =118.1 °C = 391.25 K
Moles of acetic acid = [tex]\frac{954 g}{60.05 g/mol}=15.8867 mol[/tex]
Heat evolved during condensation of 15.8867 moles of acetic acid:
[tex] -41.0 kJ/mol\times 15.8867 mol=-651.35 kJ[/tex]
Entropy change = ΔS = [tex]\frac{Heat}{Temperature}[/tex]
[tex]\Delta S=\frac{-651.35 kJ}{391.25 K}=-1.664 kJ/K\approx -1.66 kJ/K[/tex]
The change in entropy is -1.66 kJ/K.
