TOJC

Hunter M (maferaja@PLU.edu)
Tue, 24 Sep 1996 20:43:46 -0800 (PST)

Here's something to contemplate...
In Ch.3 it mentions Free Energy, entropy and enthalpy- OK cool, but so
what right? Well this stuff can be useful in predicting things about
reactions (like wheather or not they will take place). But how can this
be??? I'm glad you asked...
Consider that a (-) value for G favors the formation of products, as
does a (-) value for H right? Well right off the bucket folks this
indicates 2 things about the reaction: 1) That it is EXOTHERMIC (provided
that H is indeed negative.) and B: That the reaction is SPONTANEOUS.
(remember, if a reaction is spontaneous, then we don't have to help much-
but if it's non-spontaneous then we have to give it a kick; this requires
Energy. Recall, that (qualitatively) if the bonds in the products are
stronger than the bonds in the reactants, then the reaction is
exothermic, releases Energy and increases the Entropy of the universe and
there was much rejoicing.
Because every spontaneous change increases the entropy of the universe-
acc. to the 2nd law of thermodynamics.. pretty cool huh??