Advancement per volume: Difference between revisions

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Advancement per volume

Description

Advancement per volume or volume-specific advancement, d_trY, is particularly introduced for chemical reactions, d_rY, where it has the dimension of a concentration. In an open system at steady-state, however, the concentration does not change as the reaction advances. Only in closed systems, specific advancement is the change in concentration divided by the stoichiometric number, Δ_rY = Δc_i/ν_i. In general, Δc_i is replaced by the partial change of concentration, Δ_rc_i, which contributes to the total change of concentration, Δc_i. In open systems at steady-state, Δ_rc_i is compensated by the external contributions, Δ_extc_i, to the total concentration change, Δc_i = Δ_rc_i + Δ_extc_i = 0.

Abbreviation: d_trY

Reference: Gnaiger_1993_Pure Appl Chem

MitoPedia concepts: Ergodynamics

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 {{MitoPedia
 |abbr=d<sub>tr</sub>''Y''
-|description='''[[Advancement]] per volume''' or volume-specific advancement, d<sub>tr</sub>''Y'', is particularly introduced for chemical reactions, d<sub>r</sub>''Y'', where it has the dimension of a [[concentration]]. In a closed system, specific advancement is the change in concentration divided by the stoichiometric number, Δ<sub>r</sub>''Y'' = Δ''c<sub>i</sub>''/''ν<sub>i</sub>''. In general, Δ''c<sub>i</sub>'' is replaced by the partial change of concentration, Δ<sub>r</sub>''c<sub>i</sub>'', which contributes to the total change of concentration, Δ''c<sub>i</sub>''.
+|description='''[[Advancement]] per volume''' or volume-specific advancement, d<sub>tr</sub>''Y'', is particularly introduced for chemical reactions, d<sub>r</sub>''Y'', where it has the dimension of a [[concentration]]. In an [[open system]] at steady-state, however, the concentration does not change as the reaction advances. Only in [[closed system]]s, specific advancement is the change in concentration divided by the stoichiometric number, Δ<sub>r</sub>''Y'' = Δ''c<sub>i</sub>''/''ν<sub>i</sub>''. In general, Δ''c<sub>i</sub>'' is replaced by the partial change of concentration, Δ<sub>r</sub>''c<sub>i</sub>'', which contributes to the total change of concentration, Δ''c<sub>i</sub>''. In open systems at steady-state, Δ<sub>r</sub>''c<sub>i</sub>'' is compensated by the external contributions, Δ<sub>ext</sub>''c<sub>i</sub>'', to the total concentration change, Δ''c<sub>i</sub>'' = Δ<sub>r</sub>''c<sub>i</sub>'' + Δ<sub>ext</sub>''c<sub>i</sub>'' = 0.
 |info=[[Gnaiger_1993_Pure Appl Chem]]
 }}