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  Characteristics of Free energy

Characteristics of Free energy ‘G’:

1) G is stated as (H - TS) where H and S are the enthalpy and entropy of the system correspondingly. T = temperature. As H and S are state functions, G is a state function.

2) G is an extensive property whereas ΔG = (G2 - G1) that is the free energy change among the initial (1) and final (2) states of the system becomes the intensive property whenever mass remains constant among initial and final states or if the system is a closed system.

3) G contains single value for the thermodynamic state of the system.

4) G and ΔG values communicate to the system only. There are three conditions of ΔG in predicting the nature of the process. When, ΔG < 0 (i.e., negative), the process is spontaneous and feasible; when ΔG = 0, the process is in equilibrium and when ΔG > 0 (i.e., positive), the process is non-spontaneous and not feasible.

5) ΔG = ΔH – TΔS. However according to I law of thermodynamics,

ΔH = ΔE + PΔV and ΔE = q – w.
∴   ΔG = q – w + PΔV – TΔS

Though, ΔS = q/ T and TΔS = q = heat included in the process.

∴   ΔG = q – w + PΔV – q = –w + PΔV
Or –ΔG = w – PΔV = network.

The reduction in free energy –ΔG, accompanying a process occurring at constant temperature and pressure is equivalent to the maximum accessible work from the system other than work of expansion.

This quantity is termed as the “net work” of the system and it is equivalent to (w – PΔV).

∴ Net work = –ΔG = w – PΔV.

–ΔG symbolizes all others forms of work accessible from the system like electrical, chemical or surface work and so on other than P-V work.

 

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