Question

I have a question on Thermodynamics/Kinetics in chemical reactions, basic entropy/Gibbs stuff, posted below in a second.

Answer 1

"Sodium reacts violently with water according to the equation:
2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g)
The resulting solution has a higher temperature than the water prior to the addition of
sodium. What are the signs of ΔH° and ΔS° for this reaction?"

Answer 2

What I'm confused about-well, no, I wouldn't say I'm confused, I just want to reinforce my conclusions. The answer is that ΔH° is negative and ΔS° is positive, and I believe that that's the case because an increase in entropy can be seen because of a solid dissolving into an aqueous state and gas moles being produced, and I'd say that Delta-H is negative because you have a reaction giving off heat to the system and is exothermic. Does this all make sense/sound right as an explanation?

@aaronq

Answer 3

yep that's exactly it.