Entropy vs. enthelpy in chemical reactions.

[sghan]

Hello,
I am learning about using Free energy change /delta G to determine if a chemical reaction will occur spontaneously. /delta G = /delta H + T*/delta S. Now, enthalpy change can drive a reaction which leads to a decrease in entropy (multiple reactants => single product). My Question: can the entropy component /delta S drive a reaction to occur where the outcome is of higher energy? Do such reactions exist and are the products stable?

 

[BvU]

Hello sghan, (there is no 'welcome back' sign yet )

You are also rlearning about $\LaTeX$ I suppose.

In PF enclose source with $\#\#$ for in-line $\TeX$ and $\$\$$ for diplsayed equations (bigger, centered) and use a backslash, not a forward slash:

$\#\#$ \Delta G = \Delta H + T \Delta S $\#\#$ gives $\Delta G = \Delta H - T \Delta S$ (Note the minus sign)

For examples, google "endothermic spontaneous reactions examples"

Dissolving kitchen salt in water appears to be one example...