When calculating the entropy of vaporization of water at 25 $\circ$ C, the dominant contribution is
A) the molar heat capacity of liquid water.
B) heating the water from 25 $\circ$ C to 100 $\circ$ C.
C) cooling the water from 100 $\circ$ C to 25 $\circ$ C.
D) the entropy of vaporization of water at its normal boiling point.

Question

Quizplus · Accepted Answer

The dominant contribution to the entropy of vaporization of water at 25°C is the entropy of vaporization at its normal boiling point. This is because the process of phase transition from liquid to vapor is associated with a significant increase in entropy, and this dominates over the contributions from heating or cooling the liquid water.

When Calculating the Entropy of Vaporization of Water at 25 ∘\circ∘

When Calculating the Entropy of Vaporization of Water at 25^$\circ$