Enthelpy/Entropy question. Br2 liquid to 2Br gas

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The reaction Br2 (l) to 2Br (g) indicates an increase in entropy (S is positive) due to the transition from liquid to gas, which allows for more microstates. It is also suggested that the reaction is exothermic, meaning that enthalpy (H) is negative as heat is released. The confusion arises from the presence of two options (B and D) that both indicate H is negative and S is positive. The discussion questions whether this duplication is an error or if it suggests a deeper misunderstanding. The conclusion is that the reaction is characterized by increasing entropy and decreasing enthalpy.
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Homework Statement


Br2 (l) --> 2Br (g)

the options are:

a. H is positive and S is positive for the reaction
b. H is negative and S is positive for the reaction
c. H is positive and S is negative for the reaction
d. H is negative and S is positive for the reaction
e. G Is positive for all temperatures

Homework Equations



dG= dH - TdS

The Attempt at a Solution



The chemical reaction is going from liquid to gas, therefore the entropy is increasing because the reaction is causing more macrostates due to the greater area of distribution for the gas molecules. The reaction is exothermic, because its giving off heat.

Therefore, Entropy is increasing (S is positive) and since no heat is being absorbed Enthalpy is decreasing (H is negative).

So my answer is B... so here's the dilemma,, B is the same answer as D. I don't know if this was a mistake on the teachers part, or I AM WRONG, and she put the answer there 2x to hint that its not the answer.
 
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Why do you say it's exothermic?
 
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