What are the correct conclusions for the change in entropy in this reaction?

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SUMMARY

The discussion centers on the change in entropy for the reaction Ag(l) → Ag(s) at 1 atm and 25°C. The correct conclusion is that ΔSsys < 0, indicating a decrease in entropy as the system transitions from a liquid to a solid state. Additionally, ΔSuniv > 0 is also a valid conclusion, reflecting the overall increase in entropy of the universe despite the system's decrease. The participant initially expressed uncertainty regarding the implications for ΔSuniv but later resolved their confusion.

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Homework Statement



Which of the following conclusions is correct for the change in entropy for this reaction? You must find all of the correct answers.
Ag(l) --> Ag(s) (1atm, 25°C)

1. ΔSsys < 0
2. ΔSuniv > 0
3. The sign of ΔSsys cannot be determined.
4. ΔSsys > 0
5. The sign of ΔSuniv cannot be determined.
7. ΔSuniv < 0

Homework Equations


liquid --> solid = ΔS< 0.

The Attempt at a Solution


The reaction is more orderly because it goes from a liquid to a solid. I am pretty positive that number 1 is, therefore, correct. However, I am unsure of what happens to ΔSuniverse. Any suggestions/hints/information are much appreciated!
***It's been quite a loooong day and I have accidentally entered this as a Physics problem when it's actually Chemistry according to the subject I'm currently working on. Agh...
 
Last edited:
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Ahh, I've figured it out. Nevermind to this question.
 

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