Spontaneity

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

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

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

Moderators: Chem_Mod, Chem_Admin

Mahir_Hasan2C
Posts: 60
Joined: Fri Sep 28, 2018 12:25 am

Spontaneity

How does G relate to a reaction being spontaneous?

Hovik Mike Mkryan 2I
Posts: 95
Joined: Fri Sep 28, 2018 12:25 am

Re: Spontaneity

Hello, if delta G is negative it results in the reaction being spontaneous because the forward reaction is favorable and happens naturally without extra needed energy. Hope this helped!

Jaira_Murphy_2D
Posts: 31
Joined: Fri Apr 06, 2018 3:00 am

Re: Spontaneity

Can someone explain this from the textbook? "At constant temperature and pressure, the direction of spontaneous change is the direction of decreasing Gibbs free energy."

Isabelle Fontanilla 1I
Posts: 60
Joined: Fri Sep 28, 2018 12:19 am

Re: Spontaneity

"At constant temperature and pressure, the direction of spontaneous change is the direction of decreasing Gibbs free energy."
The more negative the Gibbs Free Energy value is, the more spontaneous a process becomes.

taryn_baldus2E
Posts: 62
Joined: Fri Sep 28, 2018 12:24 am

Re: Spontaneity

When delta G is negative, the reaction is spontaneous because this means that it does not need energy to proceed and will naturally follow the second law of thermodynamics by increasing in entropy.

Return to “Gibbs Free Energy Concepts and Calculations”

Who is online

Users browsing this forum: No registered users and 1 guest