Gibbs free energy equations

$\Delta G^{\circ}= \Delta H^{\circ} - T \Delta S^{\circ}$

$\Delta G^{\circ}= -RT\ln K$

$\Delta G^{\circ}= \sum \Delta G_{f}^{\circ}(products) - \sum \Delta G_{f}^{\circ}(reactants)$

OliviaShearin2E
Posts: 37
Joined: Fri Sep 29, 2017 7:05 am

Gibbs free energy equations

Is there a difference between using standard molar Gibbs energies and standard Gibbs free energies of formation to calculate $\Delta G^{\circ}$ in the equation $\Delta G^{\circ} = \Sigma nG_{m}^{\circ}(products)- \Sigma nG_{m}^{\circ}(reactants)$ (or $\Delta G^{\circ} = \Sigma nG_{f}^{\circ}(products)- \Sigma nG_{f}^{\circ}(reactants)$)?

Yashaswi Dis 1K
Posts: 56
Joined: Fri Sep 29, 2017 7:04 am

Re: Gibbs free energy equations

I think they are essentially the same when we do the computation. The delta G of formation is the energy it takes to make the molecule you want to find from its base elements, which is different from molar Gibbs' free energy which is for molecules in their standard states at 1 mole (it's not necessarily the energy it takes to form that molecule from its base elements).

I hope this helps!

MSkye Goldwater 2K
Posts: 19
Joined: Fri Sep 29, 2017 7:05 am

Re: Gibbs free energy equations

They are two ways to find the standard gibbs free energy of a reaction. However, depending on the information you are given to start with and what you are trying to solve for, you may want to use one over the other.

OliviaShearin2E
Posts: 37
Joined: Fri Sep 29, 2017 7:05 am

Re: Gibbs free energy equations

Sorry, is there any way you could clarify what the molar Gibbs free energy is further? I am still slightly confused. Thank you for your response!

Leanne Wong 1H
Posts: 50
Joined: Tue Oct 10, 2017 7:13 am
Been upvoted: 1 time

Re: Gibbs free energy equations

They are essentially the same thing. The only difference is what element/molecule is part of the reaction.

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