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

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    Entropy Reaction
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The reaction Ag(l) to Ag(s) indicates a decrease in entropy, as it transitions from a less ordered liquid state to a more ordered solid state, confirming that ΔSsys < 0 is correct. The change in entropy of the universe, ΔSuniv, is generally expected to be greater than zero for spontaneous processes, but the specific sign cannot be determined without additional context. The participant initially expressed uncertainty about ΔSuniv but later realized the question was misclassified as a Physics problem. Ultimately, the focus remains on understanding the relationship between entropy changes in the system and the universe. The discussion highlights the importance of correctly identifying the nature of the reaction in thermodynamic terms.
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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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