Calculate the entropy change of 47.7 g of steam that condenses to liquid water at 373.15 K. The heat of condensation for water is - 40.79 kJ/mol. (Enter your answer in J/K). Without doing further calculations, which of the following statements apply to the entropy change of the surroundings for the problem above?     ΔSsurroundings will not change.     ΔSsurroundings will be positive.     |ΔSsurroundings| = |ΔSsteam|     |ΔSsurroundings| < |ΔSsteam|     ΔSsurroundings will be negative.     |ΔSsurroundings| > |ΔSsteam|

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