[qwerty12321]

Hi everyone,

There is one major concept I am struggling with, and that is why acids dissociate more at higher temperatures. How can this be explained in terms of molecular energy levels becoming accessible at higher temperature, and the fact that the spacing between adjacent energy levels id closer for the products (more molecules). That is, the products do not have as much kinetic energy as the reactants, but can promote particles to high levels more easily.
This is sort of explained better here:http://www.chem1.com/acad/webtext/thermeq/TE1.html

What I am struggling with is how this relates to the Gibbs free energy equation? The aforementioned facts would suggest the the entropy changes, but people say that the entropy is assumed to stay the same for Gibbs, with only temperature changing (thus attributing for increased dissociation).

I would really appreciate any feedback or clarification on any of these issues,
Many thanks.