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 [MUโs-1], e.g., ampere for electric flow or current [AโกCโs-1], watt for heat flow [WโกJโs-1], and for chemical flow the unit is [molโs-1] (extent of reaction per time). The corresponding motive forces are the partial exergy (Gibbs energy) changes per advancement [JโMU-1], expressed in volt for electric force [VโกJโC-1], dimensionless for thermal force [JโJ-1], and for chemical force the unit is [Jโmol-1], which deserves a specific acronym ([Jol]) comparable to volt. 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, ฮฝi, 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 ฮฝi. The advancement of the chemical reaction, drฮพ [mol], is defined as,
drฮพ = drniยทฮฝi-1
The flow of the chemical reaction, Ir [molยทs-1], is advancement per time,
Ir = drฮพยทdt-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: dtrฮพ
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.
- ยป Advancement per volume, dtrY = dtrฮพโV-1
References
- De Donder T (1936) Thermodynamic theory of affinity: a book of principles. Oxford, England: Oxford University Press.
- Gnaiger E (1993) Nonequilibrium thermodynamics of energy transformations. Pure Appl Chem 65:1983-2002. - ยปBioblast linkยซ
- Prigogine I (1967) Introduction to thermodynamics of irreversible processes. Interscience New York, 3rd ed:147pp. - ยปBioblast linkยซ
MitoPedia concepts: MiP concept, Ergodynamics