World Library  
Flag as Inappropriate
Email this Article

Biological thermodynamics

Article Id: WHEBN0002747470
Reproduction Date:

Title: Biological thermodynamics  
Author: World Heritage Encyclopedia
Language: English
Subject: WikiProject Molecular and Cell Biology/Help/Archive 2, Thermodynamics, Energetics, Hans Westerhoff, Phosphorylation
Collection: Biology, Thermodynamics
Publisher: World Heritage Encyclopedia
Publication
Date:
 

Biological thermodynamics

Biological thermodynamics is the quantitative study of the energy transductions that occur in and between living organisms, structures, and cells and of the nature and function of the chemical processes underlying these transductions. Biological thermodynamics may address the question of whether the benefit associated with any particular phenotypic trait is worth the energy investment it requires.

Contents

  • History 1
  • The focus of thermodynamics in biology 2
    • Energy Transformation in Biological Systems 2.1
    • Energy and Dieting 2.2
  • Examples 3
    • First Law of Thermodynamics 3.1
    • Second Law of Thermodynamics 3.2
    • Gibbs Free Energy 3.3
  • See also 4
  • References 5
  • Further reading 6
  • External links 7

History

German-British medical doctor and biochemist Hans Krebs' 1957 book Energy Transformations in Living Matter (written with Hans Kornberg)[1] was the first major publication on the thermodynamics of biochemical reactions. In addition, the appendix contained the first-ever published thermodynamic tables, written by Kenneth Burton, to contain equilibrium constants and Gibbs free energy of formations for chemical species, able to calculate biochemical reactions that had not yet occurred.

Ilya Prigogine developed methods for the thermodynamic treatment of such systems. He called these systems dissipative systems, because they are formed and maintained by the dissipative processes that exchange energy between the system and its environment, and because they disappear if that exchange ceases. It may be said that they live in symbiosis with their environment. Energy transformations in biology are dependent primarily on photosynthesis. The total energy captured by photosynthesis in green plants from the solar radiation is about 2 x 1023 joules of energy per year.[2] Annual energy captured by photosynthesis in green plants is about 4% of the total sunlight energy that reaches Earth. The energy transformations in biological communities surrounding hydrothermal vents are exceptions; they oxidize sulfur, obtaining their energy via chemosynthesis rather than photosynthesis.

The focus of thermodynamics in biology

The field of biological thermodynamics is focused on principles of chemical thermodynamics in biology and biochemistry. Principles covered include the first law of thermodynamics, the second law of thermodynamics, Gibbs free energy, statistical thermodynamics, reaction kinetics, and on hypotheses of the origin of life. Presently, biological thermodynamics concerns itself with the study of internal biochemical dynamics as: ATP hydrolysis, protein stability, DNA binding, membrane diffusion, enzyme kinetics,[3] and other such essential energy controlled pathways. In terms of thermodynamics, the amount of energy capable of doing work during a chemical reaction is measured quantitatively by the change in the Gibbs free energy. The physical biologist Alfred Lotka attempted to unify the change in the Gibbs free energy with evolutionary theory.

Energy Transformation in Biological Systems

The sun is the primary source of energy for living organisms.Some living organisms like plants need sunlight directly while other organisms like humans can acquire energy from the sun indirectly.[4] There is however evidence that some bacteria can thrive in harsh environments like Antarctica as evidence by the blue-green algae beneath thick layers of ice in the lakes. No matter what the type of living species, all living organisms must capture, transduce, store, and use energy to live.

The energy can be represented by the following mathematical model:

E=hc/λ=hv

Where h is Planck's constant (6.63x10−34Js) and c is the speed of light (2.998x108 m/s). Plants trap this energy from the sunlight and undergo photosynthesis, effectively converting solar energy into chemical energy. To transfer the energy once again, animals will feed on plants and use the energy of digested plant materials to create biological macromolecules.

Energy and Dieting

Dieters can exploit the laws of thermodynamics by counting calories. This is the conservation of energy principle in that a person who consumes more calories than his body burns will gain weight whereas a person who consumes less calories than his body burns will lose weight.

Examples

First Law of Thermodynamics

The First Law of Thermodynamics is a statement of the conservation of energy; though it can be changed from one form to another, energy can be neither created nor destroyed.[5] From the first law, a principle called Hess's Law arises. Hess’s Law states that the heat absorbed or evolved in a given reaction must always be constant and independent of the manner in which the reaction takes place. Although some intermediate reactions may be endothermic and others may be exothermic, the total heat exchange is equal to the heat exchange had the process occurred directly. This principle is the basis for the calorimeter, a device used to determine the amount of heat in a chemical reaction. Since all incoming energy enters the body as food and is ultimately oxidized, the total heat production may be estimated by measuring the heat produced by the oxidation of food in a calorimeter. This heat is expressed in kilocalories, which are the common unit of food energy found on nutrition labels.[6]

Second Law of Thermodynamics

The Second Law of Thermodynamics is concerned primarily with whether or not a given process is possible. The Second Law states that no natural process can occur unless it is accompanied by an increase in the entropy of the universe.[7] Stated differently, an isolated system will always tend to disorder. Living organisms are often mistakenly believed to defy the Second Law because they are able to increase their level of organization. To correct this misinterpretation, one must refer simply to the definition of solvation from the components and the resulting increase in rotational and translational entropy of the solvent.[8]

Gibbs Free Energy

In biological systems, in general energy and entropy change together. Therefore, it is necessary to be able to define a state function that accounts for these changes simultaneously. This state function is the Gibbs Free Energy, G.

G = HTS

where:

The change in Gibbs Free Energy can be used to determine whether a given chemical reaction can occur spontaneously. If ∆G is negative, the reaction can occur

  • Cellular Thermodynamics - Wolfe, J. (2002), Encyclopedia of Life Sciences.
  • Bioenergetics

External links

  • Haynie, D. (2001). Biological Thermodynamics (textbook). Cambridge: Cambridge University Press.
  • Lehninger, A., Nelson, D., & Cox, M. (1993). Principles of Biochemistry, 2nd Ed (textbook). New York: Worth Publishers.
  • Alberty, Robert, A. (2006). Biochemical Thermodynamics: Applications of Mathematica (Methods of Biochemical Analysis), Wiley-Interscience.

Further reading

  1. ^  
  2. ^ Akihiko Ito and Takehisa Oikawa. "Global Mapping of Terrestrial Primary Productivity and Light-Use Efficiency with a Process-Based Model". In M. Shiyomi et al. Global Environmental Change in the Ocean and on Land. pp. 343–358. 
  3. ^ M.J. Farabee. "Reactions and Enzymes". On-Line Biology Book. Estrella Mountain Community College. 
  4. ^ Haynie, Donald T. (2001). Biological Thermodynamics. Cambridge University Press. pp. 1–16. 
  5. ^ Haynie, Donald T. (2001). Biological Thermodynamics. Cambridge UP.  
  6. ^ Stacy, Ralph W., David T. Williams, Ralph E. Worden, and Rex O. McMorris. Essentials of Biological and Medical Physics. New York: McGraw-Hill Book, 1955. Print.
  7. ^ Haynie, Donald T. Biological Thermodynamics. Cambridge: Cambridge UP, 2001. Print.
  8. ^ Edsall, John T., and H. Gutfreund. Biothermodynamics: The Study of Biochemical Processes at Equilibrium. Chichester, West Sussex: Wiley, 1983. Print.
  9. ^ Bergethon, P. R. The Physical Basis of Biochemistry: The Foundations of Molecular Biophysics. New York: Springer, 1998. Print.
  10. ^ Alberts, Bruce. Essential Cell Biology. New York: Garland Science, 2009. Print.

References

See also

[10]

This article was sourced from Creative Commons Attribution-ShareAlike License; additional terms may apply. World Heritage Encyclopedia content is assembled from numerous content providers, Open Access Publishing, and in compliance with The Fair Access to Science and Technology Research Act (FASTR), Wikimedia Foundation, Inc., Public Library of Science, The Encyclopedia of Life, Open Book Publishers (OBP), PubMed, U.S. National Library of Medicine, National Center for Biotechnology Information, U.S. National Library of Medicine, National Institutes of Health (NIH), U.S. Department of Health & Human Services, and USA.gov, which sources content from all federal, state, local, tribal, and territorial government publication portals (.gov, .mil, .edu). Funding for USA.gov and content contributors is made possible from the U.S. Congress, E-Government Act of 2002.
 
Crowd sourced content that is contributed to World Heritage Encyclopedia is peer reviewed and edited by our editorial staff to ensure quality scholarly research articles.
 
By using this site, you agree to the Terms of Use and Privacy Policy. World Heritage Encyclopedia™ is a registered trademark of the World Public Library Association, a non-profit organization.
 


Copyright © World Library Foundation. All rights reserved. eBooks from Project Gutenberg are sponsored by the World Library Foundation,
a 501c(4) Member's Support Non-Profit Organization, and is NOT affiliated with any governmental agency or department.