The heat of vaporization for 1.0 mole of water at 100.°C and 1.0 atm is 40.56 kJ/mol.Calculate $\Delta$S for the process H₂O(l)$\to$ H₂O(g)at 100.°C.

Question

Quizplus · Accepted Answer

The entropy change (ΔS) for vaporization can be calculated using ΔS = ΔH/T, where ΔH is the heat of vaporization and T is the temperature in Kelvin. ΔS = 40.56 kJ/mol / 373 K = 0.1087 kJ/K mol = 109 J/K mol.

The Heat of Vaporization for 1 Δ\DeltaΔ S for the Process H2O(l)

The Heat of Vaporization for 1 $\Delta$ S for the Process H₂O(l)