When the Gibbs free energy for a reaction is greater than zero, the reaction is "disfavored" - won't proceed in that direction - in fact it may try go in the reverse direction if possible.
When the Gibbs free energy for a reaction is less than zero, the reaction is "favored" - it should proceed as written spontaneously.
When the Gibbs free energy for a reaction is exactly zero - it is in equilibrium, with the forward and back ward reactions occurring at the same rate.
kokluot es e louktos Delta G <> Delta H
Spontaneous reaction
it depends on the entropy and enathalpy of the reaction
B
δg = (-992.0) - (298)(-294.6)(1/1000)
Exergonic reactions indicate a negative change in Gibbs free energy, which in English means that the reactions are spontaneous and do not require addition of energy. The exchange of oxygen and carbon dioxide in blood and lungs is an example. It is the concentration gradient that runs these exchanges passively, without additional energy from the cells.
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Fundamentally, because the Gibbs free energy of elemental hydrogen and oxygen is substantially greater than the Gibbs free energy of the water formed by their chemical reaction, and the activation energy for the reaction is not excessively high.
Spontaneous reaction
It predicts whether or not a reaction will be spontaneous.
it depends on the entropy and enathalpy of the reaction
it depends on the entropy and enathalpy of the reaction
If G < 0, the reaction is spontaneous.
Positive (greater than 0).
B
Gibbs free energy -- symbol G. If the change in Gibbs free energy for a reaction is negative, the reaction is spontaneous. If it is zero, you are at equilibrium. If it is positive, the reaction is NOT spontaneous.G ≡ H -TS (or in another useful form dG = dH -TdS)whereH is enthalpyT is absolute temperatureS is entropy
If the Gibbs free energy is close to zero, the reaction is close to equilibrium.
Yes, as long as the entropy of the universe increases.