Answer:
ΔS°fus = 48.88 J/K*mol
ΔS°vap =74.01 J/K*mol
Explanation:
Step 1: Data given
The molar heats of fusion of ethanol = 7.61 kJ/mol = 7610 J/mol
The molar heats of vaporization of ethanol = 26.0 kJ/mol = 26000 J/mol
Pressure = 1 atm
Ethanol melts at −117.3°C and boils at 78.3°C.
Step 2: Calculate the molar entropy changes for the solid-liquid and liquid-vapor transitions for ethanol.
ΔS°fus = 7610 / (273−117.3)
ΔS°fus = 48.88 J/K*mol
ΔS°vap = 26000/(273+78.3)
ΔS°vap =74.01 J/K*mol
