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Spontaneity

Posted: Fri Feb 22, 2019 2:24 pm
by Jessica Helfond 2F
How does Gibbs free energy relate to the spontaneity of a reaction?

Re: Spontaneity

Posted: Fri Feb 22, 2019 2:32 pm
by Bruce Chen 2H
When delta G is negative, it is spontaneous. When it is positive, it is not.

Re: Spontaneity

Posted: Fri Feb 22, 2019 8:55 pm
by Carissa Young 1K
Gibbs free energy can be used to determine the "spontaneity" of a reaction due to the fact Gibbs free energy change is the total energy change of the system.

Re: Spontaneity

Posted: Sat Feb 23, 2019 6:40 pm
by Xingzheng Sun 2K
△G determines whether a reaction can happen spontaneously. Negative △G is spontaneous, and positive △G is not. It is also related to which way of reaction can be more stable. The lower △G is, the more stable it is.

Re: Spontaneity

Posted: Sat Feb 23, 2019 11:01 pm
by Henry Dudley 1G
What does it mean if delta G is 0?

Re: Spontaneity

Posted: Sun Feb 24, 2019 1:24 am
by Danny Zhang 4L
I believe that the reaction is at equilibrium if delta G is zero.

Re: Spontaneity

Posted: Sun Feb 24, 2019 12:47 pm
by Anmol_cheema_2F
When change in Gibbs free energy is negative, the reaction is spontaneous; when delta G is positive, the reaction is not spontaneous.

Re: Spontaneity

Posted: Sun Feb 24, 2019 2:27 pm
by Desiree1G
If Gibbs is at 0 it is at equilibrium, if it is negative then it is exergonic meaning it is also spontaneous. If it is positive it is endergonic which means it is non-spontaneous. The lower the delta G is the more stable it is.

Re: Spontaneity

Posted: Sun Feb 24, 2019 2:30 pm
by Erin Kim 2G
delta G= 0 is at equilibrium
delta G >0 is not spontaneous
delta G < 0 spontaneous