Advancement

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 [MU∙s^-1], e.g., ampere for electric flow or current [A≡C∙s^-1], watt for heat flow [W≡J∙s^-1], and for chemical flow the unit is [mol∙s^-1] (extent of reaction per time). The corresponding motive forces are the partial exergy (Gibbs energy) changes per advancement [J∙MU^-1], expressed in volt for electric force [V≡J∙C^-1], dimensionless for thermal force [J∙J^-1], and for chemical force the unit is [J∙mol^-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, ν_i, associated with each motive component i (transformant [2]).

In a chemical reaction, r, the motive entity is the stoichiometric amount of reactant, d_rn_i, with stoichiometric number ν_i. The advancement of the chemical reaction, d_rξ [mol], is then defined as

d_rξ = d_rn_i·ν_i^-1

The flow of the chemical reaction, I_r [mol·s^-1], is advancement per time,

I_r = d_rξ·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: d_trξ

Reference: Gnaiger (1993) Pure Appl Chem

Communicated by Gnaiger E 2018-11-01, 2018-10-16

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.

» Advancement per volume, d_trY = d_trξ∙V^-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. - »Bioblast link«

Prigogine I (1967) Introduction to thermodynamics of irreversible processes. Interscience New York, 3rd ed:147pp. - »Bioblast link«

MitoPedia concepts: MiP concept, Ergodynamics