## Spontaneity and the Direction of a Reaction

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

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

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

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

### Spontaneity and the Direction of a Reaction

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

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

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.