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Difference between revisions of "Advancement"

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== References ==
== References ==
:::# De Donder T (1936) Thermodynamic theory of affinity: a book of principles. Oxford, England: Oxford University Press.
:::# De Donder T, Van Rysselberghe P (1936) Thermodynamic theory of affinity: a book of principles. Oxford, England: Oxford University Press:144 pp.
:::# Gnaiger E (1993) Nonequilibrium thermodynamics of energy transformations. Pure Appl Chem 65:1983-2002. - [[Gnaiger 1993 Pure Appl Chem |Ā»Bioblast linkĀ«]]
:::# Gnaiger E (1993) Nonequilibrium thermodynamics of energy transformations. Pure Appl Chem 65:1983-2002. - [[Gnaiger 1993 Pure Appl Chem |Ā»Bioblast linkĀ«]]
:::# Prigogine I (1967) Introduction to thermodynamics of irreversible processes. Interscience New York, 3rd ed:147pp. - [[Prigogine 1967 Interscience |Ā»Bioblast linkĀ«]] Ā 
:::# Prigogine I (1967) Introduction to thermodynamics of irreversible processes. Interscience New York, 3rd ed:147 pp. - [[Prigogine 1967 Interscience |Ā»Bioblast linkĀ«]] Ā 
{{MitoPedia concepts
{{MitoPedia concepts
|mitopedia concept=MiP concept, Ergodynamics
|mitopedia concept=MiP concept, Ergodynamics
}}
}}

Revision as of 19:36, 27 December 2018


high-resolution terminology - matching measurements at high-resolution


Advancement

Description

In an isomorphic analysis, any form of flow is the advancement of a process per unit of time, expressed in a specific motive unit [MUāˆ™s-1], e.g., ampere for electric flow or current, Iel = delĪ¾/dt [Aā‰”Cāˆ™s-1], watt for thermal or heat flow, Ith = dthĪ¾/dt [Wā‰”Jāˆ™s-1], and for chemical flow of reaction, Ir = drĪ¾/dt, the unit is [molāˆ™s-1] (extent of reaction per time). The corresponding motive forces are the partial exergy (Gibbs energy) changes per advancement [Jāˆ™MU-1], expressed in volt for electric force, Ī”elF = āˆ‚G/āˆ‚elĪ¾ [Vā‰”Jāˆ™C-1], dimensionless for thermal force, Ī”thF = āˆ‚G/āˆ‚thĪ¾ [Jāˆ™J-1], and for chemical force, Ī”rF = āˆ‚G/āˆ‚rĪ¾, the unit is [Jāˆ™mol-1], which deserves a specific acronym [Jol] comparable to volt [V]. For chemical processes of reaction (spontaneous from high-potential substrates to low-potential products) and compartmental diffusion (spontaneous from a high-potential compartment to a low-potential compartment), the advancement is the amount of motive substance that has undergone a compartmental transformation [mol]. The concept was originally introduced by De Donder [1]. Central to the concept of advancement is the stoichiometric number, Ī½i, associated with each motive component i (transformant [2]).

In a chemical reaction, r, the motive entity is the stoichiometric amount of reactant, drni, with stoichiometric number Ī½i. The advancement of the chemical reaction, drĪ¾ [mol], is defined as,

drĪ¾ = drniĀ·Ī½i-1

The flow of the chemical reaction, Ir [molĀ·s-1], is advancement per time,

Ir = drĪ¾Ā·dt-1

This concept of advancement is extended to compartmental diffusion and the advancement of charged particles [3], and to any discontinuous transformation in compartmental systems [2],

Advancement.png

Abbreviation: dtrĪ¾

Reference: Gnaiger (1993) Pure Appl Chem

Communicated by Gnaiger E (last update 2018-11-02)
delQi (dthQi) are the changes in electric charge (heat) at the compartments of high or low electric potential (temperature) within the discontinuous system (from ref. [2]).

Advancement per volume

The advancement of a transformation in a closed homogenous system (chemical reaction) or discontinuous system (diffusion) causes a change of concentration of substances i.
The advancement causes a change of concentration due to a transformation, Ī”trc, in contrast to a difference of concentrations calculated between difference states, Ī”trc.
Ā» Advancement per volume, dtrY = dtrĪ¾āˆ™V-1


Template:Keywords Membrane potential

References

  1. De Donder T, Van Rysselberghe P (1936) Thermodynamic theory of affinity: a book of principles. Oxford, England: Oxford University Press:144 pp.
  2. Gnaiger E (1993) Nonequilibrium thermodynamics of energy transformations. Pure Appl Chem 65:1983-2002. - Ā»Bioblast linkĀ«
  3. Prigogine I (1967) Introduction to thermodynamics of irreversible processes. Interscience New York, 3rd ed:147 pp. - Ā»Bioblast linkĀ«

MitoPedia concepts: MiP concept, Ergodynamics