Difference between revisions of "Advancement"
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:::# 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:147 pp. - [[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 | ||
{{Keywords: Force and membrane potential}} | {{Keywords: Force and membrane potential}} | ||
{{Template:Keywords: Normalization}} | {{Template:Keywords: Normalization}} | ||
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|mitopedia concept=MiP concept, Ergodynamics | |||
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Revision as of 06:26, 18 May 2020
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 [MUās-1], e.g., ampere for electric flow or current, Iel = delĪ¾/dt [Aā”Cās-1], watt for thermal or heat flow, Ith = dthĪ¾/dt [Wā”Jās-1], and for chemical flow of reaction, Ir = drĪ¾/dt, the unit is [molās-1] (extent of reaction per time). The corresponding motive forces are the partial exergy (Gibbs energy) changes per advancement [JāMU-1], expressed in volt for electric force, ĪelF = āG/āelĪ¾ [Vā”JāC-1], dimensionless for thermal force, ĪthF = āG/āthĪ¾ [JāJ-1], and for chemical force, ĪrF = āG/ārĪ¾, the unit is [Jāmol-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],
Abbreviation: dtrĪ¾ [MU]
Reference: Gnaiger (1993) Pure Appl Chem
Communicated by Gnaiger E (last update 2018-11-02)
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, Ītrc, in contrast to a difference of concentrations calculated between difference states, Ītrc.
- Ā» Advancement per volume, dtrY = dtrĪ¾āV-1
References
- 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. - Ā»Bioblast linkĀ«
- Prigogine I (1967) Introduction to thermodynamics of irreversible processes. Interscience New York, 3rd ed:147 pp. - Ā»Bioblast linkĀ«
- Bioblast links: Force and membrane potential - >>>>>>> - Click on [Expand] or [Collapse] - >>>>>>>
- Fundamental relationships
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