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The enthalpy of vaporization of water at 100.0°C is 40.68 kJ/mol. What is the entropy change in the surroundings when one mole of water vapor condenses at 100.0°C in a large room maintained at a temperature of 25.00°C? A.−136.4 J/ K . D.+109.0J / K B.−109.0J/ K . E.+136.4 J / K . C.−40.68 J / K