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Related Concept Videos

Thermodynamic Potentials01:26

Thermodynamic Potentials

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Thermodynamic potentials are state functions that are extremely useful in analyzing a thermodynamic system. They have dimensions of energy. The four important thermodynamic potentials are internal energy, enthalpy, Helmholtz free energy, and Gibbs free energy. These thermodynamic potentials can be expressed using two of the following variables: pressure, volume, temperature, and entropy. These two variables are expressed as the rate of change of the thermodynamic potential with respect to other...
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Internal Energy01:29

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The internal energy of a thermodynamic system is the sum of the kinetic and potential energies of all the molecules or entities in the system. The kinetic energy of an individual molecule includes contributions due to its rotation and vibration, as well as its translational energy. The potential energy is associated only with the interactions between one molecule and the other molecules of the system. Neither the system's location nor its motion is of any consequence as far as the internal...
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Internal Energy02:00

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The total of all possible kinds of energy present in a substance is called the internal energy (U), sometimes symbolized as E. Suppose a system with initial internal energy, Uinitial, undergoes a change in energy (transfer of work or heat), and the final internal energy of the system is Ufinal. Change in internal energy equals the difference between Ufinal and Uinitial.
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Energy Conservation
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A change in the internal energy of a system depends on the the net heat transfer into the system and the net work done by the system. The first law of thermodynamics, which is a generalized form of energy conservation, relates these three quantities mathematically. It states that the change in the internal energy equals the difference between the heat transfer and work done by the system.
The applied heat increases the internal energy of a system. Hence, conventionally heat is considered...
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First Law of Thermodynamics00:37

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The First Law of Thermodynamics states that energy cannot be created or destroyed, only transformed. This can be demonstrated within a classic food web where light energy from the sun is harnessed as radiant energy by plants, converted into chemical energy, and stored as complex carbohydrates. The vegetation is then consumed by animals and during the digestion process, the sugars release energy as heat. The sugars also produce chemical energy that either gets used up doing work, stored in...
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Spin Saturation Transfer Difference NMR SSTD NMR: A New Tool to Obtain Kinetic Parameters of Chemical Exchange Processes
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Metabolic thermodynamics: pertinent reference state and energy potentials.

Hans V Westerhoff1,2,3,4, Barbara M Bakker5, Andreas S Bommarius6

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Summary

This study introduces a novel biological reference state for chemical potentials, significantly reducing extrapolation errors in biochemical research. This new standard enhances accuracy and biological relevance for metabolic potential calculations.

Keywords:
biological energymetabolic reference statephysiological conditionsrecommendations on use of thermodynamics in biological chemistrystandard metabolic potential

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Area of Science:

  • Biochemistry
  • Chemical Thermodynamics
  • Bioenergetics

Background:

  • Standard chemical potentials require extrapolation to remote physical-chemical reference states, introducing significant errors for in vivo applications.
  • Current methods necessitate complex reverse extrapolations for biological conditions, limiting accuracy and biological interpretation.
  • Biological systems operate under specific conditions (pH, pMg, temperature, ionic strength) that differ from traditional reference states.

Purpose of the Study:

  • To propose and define a more biologically relevant reference state for chemical potentials, termed 'metabolic potentials'.
  • To reduce extrapolation errors and enhance the accuracy and biological meaning of thermodynamic data.
  • To create an accessible database of standard metabolic potentials for biochemical compounds.

Main Methods:

  • Defined a biological reference state with specific pH, pMg, water content, precursor concentrations, temperatures, and ionic strength.
  • Transformed standard chemical potentials into 'metabolic potentials' by incorporating the chemical potentials of protons, Mg2+, water, and precursor ions.
  • Calculated and collated 1360 standard metabolic potentials for 320 biochemical compounds.

Main Results:

  • Established a standardized metabolic reference state (pH 7, pMg 3, 37/25°C, 0.15 m ionic strength, 1 mM precursors).
  • Created a database of 1360 standard metabolic potentials for 320 compounds, facilitating direct use in biological contexts.
  • Developed algorithms for transforming between experimental and metabolic reference states, ensuring data interoperability.

Conclusions:

  • The proposed metabolic reference state significantly minimizes extrapolation errors, improving the accuracy of thermodynamic calculations in biology.
  • Standardized metabolic potentials enhance the biological relevance and accessibility of thermodynamic data for researchers.
  • This approach facilitates the integration of thermodynamic data across diverse biological systems and research fields.