Spontaneity and the Direction of a Reaction






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Kathleen Vidanes 1E
Posts: 62
Joined: Fri Sep 29, 2017 7:07 am

Spontaneity and the Direction of a Reaction

Postby Kathleen Vidanes 1E » Tue Feb 06, 2018 2:07 pm

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!

Laura Riccardelli
Posts: 49
Joined: Fri Sep 29, 2017 7:04 am

Re: Spontaneity and the Direction of a Reaction

Postby Laura Riccardelli » Tue Feb 06, 2018 2:32 pm

My understanding is that if the delta G is negative then it is a spontaneous favorable reaction and will proceed toward the products.

Lindsay Kester 2L
Posts: 29
Joined: Thu Jul 27, 2017 3:00 am

Re: Spontaneity and the Direction of a Reaction

Postby Lindsay Kester 2L » Tue Feb 06, 2018 3:08 pm

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.


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