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Postby 105114680 » Thu Feb 14, 2019 3:31 pm

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?

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Re: Stability

Postby 805087225 » Thu Feb 14, 2019 3:55 pm

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.

Jessica Chen 1F
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Re: Stability

Postby Jessica Chen 1F » Thu Feb 14, 2019 6:12 pm

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.

Lorena Zhang 4E
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Re: Stability

Postby Lorena Zhang 4E » Fri Feb 15, 2019 5:18 pm

For a specific compound, if it's gibbs free energy of formation is negative, then it's relatively stable.

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