In the field of thermodynamics, the gibbs function is classified as a thermodynamic potential, in short, it is a long-state function, which provides the condition of stability and spontaneity for a chemical reaction. The second law of thermodynamics maintains that a natural chemical reaction makes it possible for the energy present in the universe to increase and at the same time, it is a function of the entropy of the environment and the system.
The purpose of the gibbs function is to determine if a reaction arises naturally, taking into account only the variables of the system. This function is symbolized with the letter G.
The calculation of this function is based on the following: on the increase or decrease of the entropy that is linked to the reaction and the maximum heat that it requires or that which has been released by it. Its creator was the physicist Josiah Willard Gibbs, who gave his first contributions through the theoretical foundation of thermodynamics.
The fixed formula for the calculation of the Gibbs function is: G = H-TS
Where the T represents the total temperature. Within a process that is carried out at constant temperature, the change in the free energy of the system (ΔG) is symbolized by the expression: ΔG = ΔH - T.ΔS.
ΔG = represents the existing difference of free energy.
ΔH = represents the enthalpy difference.
T = represents the absolute temperature
ΔS = represents the entropy difference
If you want to know whether or not the function G is associated with the spontaneity of the reaction, it is important to bear in mind that the temperature and the pressure remain constant. Now, within chemical reactions, the valuation that yields ΔG can be translated in this way:
- When ΔG is equal to 0, the reaction is stable or in equilibrium.
- When ΔG is greater than 0, the reaction was not natural.
- When ΔG is less than 0, the reaction is natural.
The importance of this function resides, in that through it the technological world can know the amount of available energy. It is important to remember that the natural inclination of free energy is its progressive decline, which indicates the fact that less usable energy will be available each day.
