The enthalpy and entropy of vaporization of water at 100.00$\degree$C are 40.66 kJ/mol and 109.0 J/mol . K, respectively.What is the entropy change of the universe when one mole of steam condenses in a large room maintained at 25.00$\degree$C? Assume the final temperature of the water is 100.00$\degree$C.

Question

Quizplus · Accepted Answer

The entropy change of the universe is the sum of the entropy change of the system and the surroundings. The entropy change of the system is -109.0 J/K (since steam condenses). The surroundings gain heat at 25°C, so the entropy change of the surroundings is 40660 J / 298 K = 136.4 J/K. The total change is 136.4 J/K - 109.0 J/K = 27.4 J/K.

The Enthalpy and Entropy of Vaporization of Water at 100 °\degree°

The Enthalpy and Entropy of Vaporization of Water at 100 $\degree$