Na+ & OH- Dissociation: Energy Absorbed yet Heat Liberated

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The discussion revolves around the dissociation of Na+ and OH- ions, which initially absorbs energy but results in an overall exothermic reaction. The key points highlight the concept of enthalpy of dissolution, where energy is required to break the lattice structure of the ions. However, the process ultimately releases heat due to the increased order from solvation, demonstrating the interplay between enthalpic and entropic factors in chemical reactions. This understanding clarifies why a reaction can absorb energy initially yet still be exothermic overall.
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Nevermind!

My heads going crazy when I think about this PLEASE HELP!

In a reaction, Na+ ions are separated from OH- ions, a process of dissociation that absorbs energy, yet, in the end, heat was liberated by the overall process... WHY? :bugeye:
 
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Never Mind I Figured It Out Thanks For Looking Though :)
 
It may still be instructive (to yourself) and others to post whatever it is that you have figured out.
 
enthalpy of dissolution heh? It takes energy to break apart the lattice energy, yet the increased order associated with the solvation suffices for the overall reaction to be exothermic. The one has to take into account both enthalpy and entropical factors.
 

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