Answer: The entropy change of the process is [tex]2.0\times 10^2J/K[/tex]
Explanation:
To calculate the entropy change for different phase at same temperature, we use the equation:
[tex]\Delta S=n\times \frac{\Delta H_{f}}{T}[/tex]
where,
[tex]\Delta S[/tex] = Entropy change
n = moles of acetone = 6.3 moles
[tex]\Delta H_{f}[/tex] = enthalpy of fusion = 5.7 kJ/mol = 5700 J/mol (Conversion factor: 1 kJ = 1000 J)
T = temperature of the system = [tex]-94.7^oC=[273-94.7]=178.3K[/tex]
Putting values in above equation, we get:
[tex]\Delta S=\frac{6.3mol\times 5700J/mol}{178.3K}\\\\\Delta S=201.4J/K=2.0\times 10^2J/K[/tex]
Hence, the entropy change of the process is [tex]2.0\times 10^2J/K[/tex]
