Stability
Moderators: Chem_Mod, Chem_Admin
Stability
I need help thinking through how a raise in temperature affects the stability of compounds with respect to their elements. I know you can use the Gf and Hf of the compound to solve for the -TdeltaSf term in the gibbs free energy equation, and that if T increases than the whole -TdeltaSf term increases but then I get confused with what to do with that information and how to make a claim about stability. Can someone clarify this concept?
Re: Stability
It all depends first on whether the equation represents an exothermic or endothermic reaction.
If G is negative, it is said to be a spontaneous reaction.
If G is negative, it is said to be a spontaneous reaction.
-
- Posts: 61
- Joined: Fri Sep 28, 2018 12:17 am
Re: Stability
If the reaction is exothermic, heat is a product and increasing the temperature would cause the reaction to shift toward the reactant side, making reactants more stable and products less stable.
If the reaction is endothermic, heat is a reactant and increasing the temperature would cause the reaction to shift toward the product side, making products more stable and the reactants less stable.
If the reaction is endothermic, heat is a reactant and increasing the temperature would cause the reaction to shift toward the product side, making products more stable and the reactants less stable.
-
- Posts: 63
- Joined: Fri Sep 28, 2018 12:16 am
Re: Stability
For a specific compound, if it's gibbs free energy of formation is negative, then it's relatively stable.
Return to “Gibbs Free Energy Concepts and Calculations”
Who is online
Users browsing this forum: No registered users and 2 guests