|A section from the original Lewis (1923) free energy of formation of chemical substances table (see: free energy table), showing, e.g., that table salt (NaCl) has a free energy of formation, from the elements, at STP, of -91.8 kJ of free energy (Gibbs energy); the basics of which can be extrapolated up to the human level (see: human free energy of formation), to the effect that, e.g., Bill Gates (see: Gates model), in 2016, has a free energy of formation of so many kJ, a quantification of his "existence state" or "becoming" so to say.|
“Values obtained for the increase in free energy, at 25°C, in the formation of a substance (at unit activity) form the elements in their standard reference states.”
These values are listed in free energy tables, the first of which were made by Gilbert Lewis and Merle Randall in 1914.
Human free energies of formation
See main: Human free energy of formation; See also: Human free energyOne of the more complex subjects in human chemical thermodynamics, is the subject of scaling up the Lewis-Randall model of calculating "standard Gibbs free energies of formation" for any and all atoms and molecular entities to that of the human reaction level, namely of calculating a standard Gibbs free energy of formation for each existing human molecule (person), defined at the point of formation or synthesis, or point of detachment, whether physical (umbilical severing) or orbital (adulthood detachment), from the parental structure.
As to whether or not there exists a "standard" Gibbs free energy of formation, for a general human, the question remains open, being that there seem to be many underlying puzzling issues to this definition. 
Historically, the first to state that a mouse has a free energy of formation was American chemist Martin Goldstein in 1993. 
1. Lewis, Gilbert N. and Randall, Merle. (1923). Thermodynamics and the Free Energy of Chemical Substances (pg. 596). McGraw-Hill Book Co., Inc.
2. Lewis, Gilbert and Randall, Merle. (1914). “The Free Energy of Oxygen, Hydrogen, and the Oxides of Hydrogen”, Journal of American Chemical Society, 35:1964.
3. (a) Thims, Libb. (2007). Human Chemistry (Volume One). Morrisville, NC: LuLu.
(b) Thims, Libb. (2007). Human Chemistry (Volume Two). Morrisville, NC: LuLu.
4. Goldstein, Martin and Goldstein, Inge F. (1993). The Refrigerator and the Universe: Understanding the Laws of Energy. Cambridge, Massachusetts: Harvard University Press.
● Brezonik, Patrick L. and Arnold, William A. (2011). Water Chemistry (table: Free Energies and Enthalpies of Formation of Common Chemical Species in Water, pgs. 758-). Oxford University Press.
● Standard Gibbs function of formation – Wikipedia.