I am confusing about the delta G(free-energy change). Could any one

[quynhchi0907]

I am confusing about the delta G(free-energy change). Could anyone explain me more about the sign of delta G. wat the exergonic and endergonic process mean? also, wat is the relation between the delta G and delta S(entropy)? I know the formula between them, but I don't quite understand

Thank you,

 

[spectre101]

Free energy is essentially the ability to do work. A reaction where free energy is absorbed from the environment has work being done on the reactants (this is endergonic, delta G is positive). When free energy is release by a reaction, the reactants have done work on the environment (this is exergonic, delta G is negative). The entropy of a system represents the amount of disorder when a reaction occurs. It will determine how much of the available energy in a system can do work. Change in entropy alone, however, does not influence delta G. The change in enthalpy (H) must also be known.

 

[quicknote]

for reaching out for clarification on the concept of delta G (free-energy change). Delta G is a measure of the thermodynamic potential of a system to do work. The sign of delta G indicates the direction of a spontaneous reaction, with negative values indicating an exergonic (energy-releasing) process and positive values indicating an endergonic (energy-consuming) process.

Exergonic processes occur spontaneously and release energy, while endergonic processes require energy input to occur. An example of an exergonic process is the breakdown of glucose during cellular respiration, which releases energy for the cell to use. An example of an endergonic process is the synthesis of glucose from smaller molecules, which requires energy input from the cell.

The relationship between delta G and delta S (entropy) is described by the equation delta G = delta H - T*delta S, where delta H is the change in enthalpy (heat energy) and T is the temperature in Kelvin. This equation shows that delta G is influenced by both the change in enthalpy and the change in entropy. A negative delta G value indicates that the reaction is spontaneous and that the system is becoming more ordered (decreasing in entropy), while a positive delta G value indicates a non-spontaneous reaction and an increase in disorder (increase in entropy).

I hope this explanation helps clarify your confusion about delta G and its relationship to delta S. If you have any further questions or need additional clarification, please don't hesitate to ask. As a scientist, it is important to fully understand these concepts in order to accurately interpret and analyze data related to thermodynamics and chemical reactions.