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Equation de Nernst

Equation de Nernst. BUT: Calculer pour chaque ion les conditions d ’équilibre connaissant les concentrations intra et extracellulaires. Travail à fournir pour transporter une mole d ’ion x contre les forces électriques W Ex = Z F Em W Ex travail en KJ/mole, Z valence, F faraday (96500C/mole).

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Equation de Nernst

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  1. Equation de Nernst BUT: Calculer pour chaque ion les conditions d ’équilibre connaissant les concentrations intra et extracellulaires Travail à fournir pour transporter une mole d ’ion x contre les forces électriques W Ex = Z F Em W Ex travail en KJ/mole, Z valence, F faraday (96500C/mole) Travail à fournir pour transporter une mole d ’ion x contre le gradient de concentration W Cx = RT ln [x]i / [x]e W Cx travail en KJ/mole, R = 8.31J/mole/°K, T Température en °Kelvin (273+°C), [x]i et [x]e concentrations de x intra et extracellulaires La ddp électrochimique agissant sur x est la somme algébrique de ces 2 composantes D µx = W Ex + W Cx Dµx = ZFEm + RT ln [x]i / [x]e A l ’équilibre Le potentiel Em est entièrement déterminé par x donc = à Ex et Dµx =0 D ’où…. Ex = RT /ZF ln ( [x]e /[x]i )

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