Why Does the Human Body Maintain a Constant
37-Degree Temperature?: Thermodynamic Switch
Controls Chemical Equilibrium in Biological Systems
Paul W. Chun (pwchun@biochem.med.ufl.edu)
Professor of Biochemistry and Molecular Biology
University of Florida College of Medicine
Gainesville, Florida 32610-0245
INTRODUCTION
Shortly after T.H. Benzinger published an article in 1971 in Nature entitled “Thermodynamics,
Chemical Reactions and Molecular Biology,” the question arose whether thermochemical descriptions of
biochemical systems that existed in the literature were inadequate or wrong or both. Benzinger did not
formulate the problem in a way that would readily permit its general testing, and sufficient experimental
data bases of adequate range and accuracy for such tests did not exist at that time. Thus, for some three
decades, his conclusions were ignored.
In discussions with Dr. Benzinger, I became intrigued by the question of how the basic laws of
thermodynamics could and should be applied to the interacting biological systems I had studied for some
30 years.
Lack of a fitting function for the Gibbs free energy change as a function of temperature has
certainly hampered any understanding of thermodynamic behavior in biological systems ( Gibbs free
[available] energy = Total heat − Bound unavailable energy). However, my subsequent studies have
revealed many details of the thermodynamic and equilibrium properties of living systems.
One of the most interesting discoveries and the subject of my presentation at the 48th Biophysical
Society meeting in Baltimore, concerns the way in which the thermal set-point of a biological system is
established and maintained on a molecular level. In the human body, that set-point is 37o Celsius or 98.6o
Fahrenheit. Although it is has been recognized by generations of scientists that most warm-blooded
animals maintain a constant body temperature, few bothered to ask why. I believe I have found the
answer.
Based on the analysis of available and highly precise data for a number of interacting protein
systems, I have reached a number of overarching conclusions about their thermodynamic behavior.
In all biological interactions, ∆Ho(T) and ∆So(T) are positive at low temperature. As reaction
temperature increases, both ∆Ho(T) and ∆So(T) become negative, creating a negative minimum of Gibbs
free energy change at
. Here the balance of ∆Ho(TS)(−) = ∆Go(TS)(−)minimum and T∆So(T) = 0 at
, as seen in the accompanying figures. The change of sign in ∆Cpo(T)reaction leads to true negative
minimum in the Gibbs free energy of reaction, that is ∆Cpo(T)(+) → ∆Cpo(T)(−), designated as a
thermodynamic molecular switch.
It is known that living systems can survive and operate optimally only at a sharply defined
temperature, or over a limited temperature range where the balance of energy and entropy demands is
favorable at best. The implication is that basic macromolecular interactions exhibit a well-defined
negative free energy minimum as a function of temperature. Such a situation is not common in simple
chemical systems where a monotonic change of ∆Go, ∆Ho, and Keq over an experimental temperature
range is typical.
In a succession of publications, I have defined a thermodynamic molecular switch for various
biological systems. At a well-defined stable temperature − 37o C. in the human body − there will be a
negative minimum of free energy change and the maximum work can be accomplished for such essential
life processes as transpiration, digestion, reproduction or locomotion.
It is my contention that the thermodynamic molecular switch is a universal feature of living
systems, one in which a change in sign of the specific heat capacity change (the capacity to hold heat) of
reaction leads to a negative minimum in the Gibbs free energy change of reaction and a maximum in the
related equilibrium constant.
In assessing my thermodynamic work, Robert J. Hanrahan, professor of chemistry at the
University of Florida, said, “ Professor Chun has provided a detailed and elegant description of how the
body’s thermostat works, published in more than 20 papers in significant scientific journals. But because
of the fragmentation of modern science, few chemists are aware of this work − although the arguments
are based on straightforward (if detailed) thermodynamics.”
I have applied the Planck-Benzinger methodology I have developed to protein folding; protein-
protein, protein-nucleic acid or protein-membrane interactions, and protein self-assembly, and have found
that all these interacting biological systems exhibit a thermodynamic molecular switch at a molecular
level.
It seems apparent that the existence of a thermodynamic molecular switch may be universal in
living systems. Researchers who fail to consider it in their analysis of energy differences in biological
systems risk a conclusion that is inadequate, inaccurate − or both.
THERMODYNAMIC MOLECULAR SWTICH
Applying the Planck-Benzinger methodology to numerous biological systems, I have
established that the negative Gibbs free energy minimum at a well-defined stable temperature, ,
where the bound unavailable energy T∆So = 0, has its origin in the sequence-specific hydrophobic
interactions. Each such system examined confirms the existence of a thermodynamic molecular switch
wherein a change of sign in [∆Cpo]reaction leads to a true negative minimum in the Gibbs free energy
change of reaction, and hence a maximum in the related equilibrium constant, Keq.
At this temperature, , where ∆Ho(TS)(−) = ∆Go(TS)(−)min, the maximum work can be
accomplished in transpiration, digestion, reproduction or locomotion. In the human body, this
temperature is 37 oC. The values may vary from one living organism to another, but the fact that the
value of T∆So(T) = 0 will not.
There is a lower cutoff point, , where enthalpy is unfavorable but entropy is favorable, i.e.
∆Ho(Th)(+) = T∆So(Th)(+), and an upper limit, , above which enthalpy is favorable but entropy is
unfavorable, i.e. ∆Ho(Tm)(−) = T∆So(Tm)(−). Only between these two temperature limits, where
∆Go(T) = 0, is the net chemical driving force favorable for such biological processes as protein folding,
protein-protein, protein-nucleic acid or protein-membrane interactions, and protein self-assembly. All
interacting biological systems examined using the Planck-Benzinger methodology have shown such a
thermodynamic switch at the molecular level, suggesting that its existence may be universal.
CONCLUSION
Application of the Planck-Benzinger methodology to biological systems has demonstrated a
basic rule for life processes, in that there is a lower cutoff point, , where entropy is favorable but
enthalpy is unfavorable, i.e. ∆Ho(Th)(+) = T∆So(Th)(+), and an upper cutoff, , above which
enthalpy is favorable but entropy unfavorable, i.e. ∆Ho(Tm)(−) = T∆So(Tm)(−). Only between these two
limits, where ∆Go(T) = 0, is the net chemical driving force favorable for such biological processes as
protein folding; protein-protein, protein-nucleic acid, or protein-membrane interactions; and protein self-
assembly. The significance of a negative Gibbs free energy minimum in the equilibrium of biological
systems is simply that one is dealing with a true condition of stability, that is, maximum Keq of reaction.
The value may vary from one organism to another, but the fact that the value of T∆So(T) = 0 will
not.
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As experimentally observed in interacting biological systems such as α-chymotrypsin dimerization at low
temperature, ∆Ho and ∆So are both positive, becoming negative as temperature increases, whereas ∆Go changes
from positive to negative, then reaches a negative value of maximum magnitude at , and finally becomes
positive as temperature increases (figure on the left ). That is, process 1 goes to process 2, creating cooperative
enthalpy-entropy compensation between and , where both ∆Ho(T)(+) and T∆So(T)(+) intercept at
. Both ∆Ho(T)(−) and T∆So(T)( −) intercept at . This process is illustrated schematically at right.
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The Planck-Benzinger methodology provides a means of determining the innate temperature-
invariant enthalpy, ),T(H 0
o∆ thermal agitation energy, or the heat capacity integrals, ,dT)T(CpT
0
o∫ ∆
and allows precise determination of , , and . It is the best method for evaluating
],T(HH[ 0
oo
298 ∆−∆ the heat of reaction for biological molecules at room temperature, and provides for a
better understanding of cooperative thermodynamic compensation. It can be effectively applied to the
thermodynamic analysis of site-directed mutagenesis.
It is apparent that the critical factor driving interacting biological systems is a temperature-
dependent heat capacity change of reaction, ∆Cpo(T)reaction, which is positive at low temperature but
switches to a negative value at a temperature well below the ambient range. This change of sign of the
critically important ∆Cpo(T)reaction has such significant consequences that it is referred to as a
thermodynamic switch. It determines the behavior patterns of the Gibbs free energy change, and hence a
change in the equilibrium constant, and /or spontaneity. All interacting biological systems we have thus
far examined using with the Planck-Benzinger approach point to the universality of this thermodynamic
switch [1-10].
References
1. Chun, P. W., (2000a) Biophysical J. 78, 416.
2. Chun, P. W., (2000b) Cell Biochemistry and Biophysics, 33, 149.
3. Chun, P. W., (2000c) Int’l. J. Quantum Chem. 80, 1181.
4. Chun, P. W., (2001a) J. Colloids a and Interfacial Science, 181,183.
5. Chun, P. W., (2001b) Int’l. J. Quantum Chem. 85, 697.
6. Chun. P. W., (2002) Int’l. J. Quantum Chem. 87, 323.
7. Chun, P. W., (2003a) Biophysical Journal 84, 1352.
8. Chun, P. W., (2003b) The ScientificWorldJournal 3, 176. .
9. Chun, P. W., (2004a) Accepted in Physica Scripta.
10. Chun, P. W., (2004b) Accepted in J. Applied Physics.
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