Calculate the entropy change of 73.8 g of steam that condenses to liquid water a

Question

Calculate the entropy change of 73.8 g of steam that condenses to liquid water at 373.15 K. (Enter your answer in J/K).

-448

Without doing further calculations, which of the following statements apply to the entropy change of the surroundings for the problem above?


True False  ?Ssurroundings < ?Ssteam
True False  ?Ssurroundings will be positive.
True False  ?Ssurroundings = -?Ssteam
True False  ?Ssurroundings > -?Ssteam
True False  ?Ssurroundings will be negative.
True False  ?Ssurroundings will not change.

Explanation / Answer

delta S sys (or delta S steam) = -448 J/K

delta S sys + delta S surr = delta S universe > 0

Therefore,

delta S surr > 448 J/K

Statement 1: delta S surr < delta S steam is false

Statement 2: delta S surr positive is true

Statement 3: delta S surr = - delta S steam is false

Statement 4: delta S surr > - delta S steam is true

Statement 5: delta S surr negative is false

Statement 6: S surr will not change is false

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.