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Spontaneity and the Direction of a Reaction

Posted: Tue Feb 06, 2018 2:07 pm
by Kathleen Vidanes 1E
Hi,

I am still a bit confused on the relationship between spontaneity and the direction of a reaction. For example, for 11.15, why is it that if delta G of the reaction is positive, that means the spontaneous reaction is proceeding towards the reactants? Does the rxn proceed towards the products if delta G is negative?

Thank you!

Re: Spontaneity and the Direction of a Reaction

Posted: Tue Feb 06, 2018 2:32 pm
by Laura Riccardelli
My understanding is that if the delta G is negative then it is a spontaneous favorable reaction and will proceed toward the products.

Re: Spontaneity and the Direction of a Reaction

Posted: Tue Feb 06, 2018 3:08 pm
by Lindsay Kester 2L
When delta G is negative, it means that the products are at a lower energy level than the reactants, and thus the reaction moves toward them. When it's positive, however, the reactants are at a lower energy level than the products, and so the reaction moves toward them.