Gibbs Free Energy


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Linh Vo 2J
Posts: 61
Joined: Sat Apr 28, 2018 3:00 am

Gibbs Free Energy

Postby Linh Vo 2J » Thu Feb 21, 2019 7:33 pm

Can someone explain to me why deltaG<0 is a forward process, deltaG>0 is a reverse process, and deltaG=0 is at physical equilibrium? What is the logic behind this?

Mona Lee 4L
Posts: 60
Joined: Fri Sep 28, 2018 12:16 am

Re: Gibbs Free Energy

Postby Mona Lee 4L » Thu Feb 21, 2019 8:46 pm

If deltaG is negative, the reaction is spontaneous. That means that the reaction will proceed without the need for outside energy, therefore the forward reaction will be favored. The opposite holds for the reverse reaction.

Jennifer Su 2L
Posts: 47
Joined: Wed Nov 21, 2018 12:20 am

Re: Gibbs Free Energy

Postby Jennifer Su 2L » Thu Feb 21, 2019 9:58 pm

When deltaG is positive, it means that the free energy of the products is MORE than the free energy of the reactants. Therefore, an input of free energy is needed for the reaction to occur, so the reaction is NOT spontaneous.

When deltaG is negative, it means that the free energy of the products is LESS than the free energy of the reactants. Therefore, free energy is released during the reaction (no input needed), and so the reaction IS spontaneous.

eden tefera 2B
Posts: 39
Joined: Fri Sep 28, 2018 12:21 am

Re: Gibbs Free Energy

Postby eden tefera 2B » Fri Feb 22, 2019 10:34 am

When deltaG is positive the reactants are more thermodynamically stable, so the reaction proceeds to the left.
When deltaG is negative the products are more thermodynamically stable, so the reaction proceeds to the right.

IsabelLight2H
Posts: 34
Joined: Wed Oct 03, 2018 12:15 am

Re: Gibbs Free Energy

Postby IsabelLight2H » Fri Feb 22, 2019 10:41 am

How do we know if it's stable or not based on the spontaneity?


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