Calculate the entropy change of 41.4 g of steam that condenses to liquid water at 373.15 K. (Enter your answer in J/K). Answer to part 1 is -251 J/K I need the second question answered. Thanks! Without doing further calculations, which of the following statements apply to the entropy change of the surroundings for the problem above? True False  ΔSsurroundings will be positive. True False  ΔSsurroundings > -ΔSsteam True False  ΔSsurroundings will be negative. True False  ΔSsurroundings will not change. True False  ΔSsurroundings = -ΔSsteam True False  ΔSsurroundings < ΔSsteam

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