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### Gibbs free energy equations

Posted: Mon Jan 22, 2018 10:22 pm
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 $\Delta G^{\circ} = \Sigma nG_{f}^{\circ}(products)- \Sigma nG_{f}^{\circ}(reactants)$)?

### Re: Gibbs free energy equations

Posted: Tue Jan 23, 2018 2:11 am
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!

### Re: Gibbs free energy equations

Posted: Fri Jan 26, 2018 12:14 am
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.

### Re: Gibbs free energy equations

Posted: Mon Jan 29, 2018 8:22 pm
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!

### Re: Gibbs free energy equations

Posted: Mon Jan 29, 2018 9:08 pm
They are essentially the same thing. The only difference is what element/molecule is part of the reaction.