How do you measure Gibbs free energy?
1 Answer
You can't measure it directly, and
SCENARIO 1: DISSOLVING SOLUTE INTO SOLVENT
One way to measure it indirectly is through the chemical potential at constant temperature.
Let's say we had a solvent
#mu_j = mu_j^"*" + RTlnchi_j# where:
#chi_j = (n_j)/(n_(t ot))# is the mol fraction of solvent#j# in solution.#mu_j = G_j/n_j# is the chemical potential, or the molar Gibbs' free energy of substance#j# .#mu_j^"*"# is the chemical potential for some reference point. In this case, it is for an unmixed solvent#j# .
We define the change in molar Gibbs' free energy as:
#Deltamu_j = mu_j - mu_j^"*" = RTlnchi_j#
#= DeltabarG_j = barG_j - barG_j^"*" = (DeltaG_j)/n_j# ,where the bar signifies molar quantities.
So, the change in the Gibbs' free energy of the solvent for adding solute into solution (starting with no solute) would be given by:
#barul(|stackrel(" ")(" "DeltaG_j = n_jRTlnchi_j" ")|)#
SCENARIO 2: MEASUREMENT OF NATURAL VARIABLES
Let's attempt to derive a functional form using only natural variables (
#dG = -SdT + VdP# #" "bb((1))#
Now, if we write the total differential of
#dG = ((delG)/(delT))_PdT + ((delG)/(delP))_TdP# #" "bb((2))#
We know the second term to be
But unfortunately the first term has no physical meaning in thermodynamics, as the entropy at absolute zero is arbitrarily defined (Physical Chemistry by Levine). This is referring to...
#DeltaG = DeltaH - Delta(TS)#
#= DeltaH - T_1DeltaS - S_1DeltaT - DeltaSDeltaT#
However,
#barul(|stackrel(" ")(" "DeltaG = DeltaH - TDeltaS" ")|)#
Otherwise, it cannot be measured.