Spontaneity
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Re: Spontaneity
Negative delta G is spontaneous because free energy goes from a higher energy state to a lower energy state which is favorable.
Re: Spontaneity
A negative delta G is spontaneous because there is a lost in free energy, and going from high free energy to low free energy is favorable. A positive delta G is nonspontaneous because there is a gain in free energy. For that to happen, energy would have to be added, making the reaction nonspontaneous.
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Re: Spontaneity
A negative delta G indicates that a reaction/process is spontaneous or favorable. This is due to the fact that a negative delta G indicates a loss of free energy (going from a higher free energy of the reactants to a lower free energy of the products), which is a favorable process.
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Re: Spontaneity
Negative delta G signifies spontaneity while positive delta G reactions are not spontaneous.
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Re: Spontaneity
A -ΔG indicates that the reaction is spontaneous and exothermic, while a +ΔG indicates that the reaction is non spontaneous and endothermic. However, when dealing with a +ΔG we can say that the reverse reaction is favored since it is spontaneous in the reverse direction
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Re: Spontaneity
When delta G is negative, the process is spontaneous. When delta G is positive, the forward process is not spontaneous, but the reverse process is spontaneous.
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Re: Spontaneity
On page 348 of the textbook, there is a helpful diagram that shows that a negative change in Gibbs free energy is spontaneous.
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