Answer:
The change in entropy in the system is -231.5 J/K
Explanation:
Step 1: Data given
The normal boiling point of ethanol (C2H5OH) is 78.3 °C = 351.45 K
The molar enthalpy of vaporization of ethanol is 38.56 kJ/mol = 38560 J/mol
Mass of ethanol = 97.2 grams
Pressure = 1 atm
Step 2: Calculate the entropy change of vaporization
The entropy change of vaporization = molar enthalpy of vaporization of ethanol / temperature
The entropy change of vaporization = 38560 J/mol / 351.45 K
The entropy change of vaporization = -109.72 J/k*mol
Step 3: Calculate moles of ethanol
Moles ethanol = mass / molar mass ethanol
Moles ethanol = 97.2 grams / 46.07 g/mol
Moles ethanol = 2.11 moles
Step 4: Calculate change in entropy
For 1 mol = -109.72 J/K*mol
For 2.11 moles = -231.5 J/K
The change in entropy in the system is -231.5 J/K
