The enthalpy and entropy of vaporization of ammonia at its normal boiling point,-33.34 $\circ$ C,are approximately 23.35 kJ/mol and 97.4 J/mol . K,respectively.What would the entropy change of the universe be if one mole of ammonia vapor were to condense in a large room maintained at 30.0 $\circ$ C?

Question

Quizplus · Accepted Answer

The entropy change of the universe is the sum of the entropy change of the system and the surroundings. When ammonia condenses, the system loses entropy (-97.4 J/K). The surroundings gain entropy, calculated as ΔH/T = 23350 J / 303.15 K = 77.0 J/K. The total change is -97.4 + 77.0 = -20.4 J/K.

The Enthalpy and Entropy of Vaporization of Ammonia at Its ∘\circ∘

The Enthalpy and Entropy of Vaporization of Ammonia at Its $\circ$