Difference between revisions of "Mitocondrial pyruvate metabolism"
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*The rate law is defined as <center><math>v = K_1[Pyruvate][ADP]^{13}[Pi]^{13}\left(1-\frac{\frac{[ATP]^{13}}{[Pyruvate][ADP]^{13}[Pi]^{13}}}{K_{eq}}\right)</math></center><br> | *The rate law is defined as <center><math>v = K_1[Pyruvate][ADP]^{13}[Pi]^{13}\left(1-\frac{\frac{[ATP]^{13}}{[Pyruvate][ADP]^{13}[Pi]^{13}}}{K_{eq}}\right)</math></center><br> | ||
− | *The <math>\Delta G^ | + | *The <math>\Delta G^o'</math> for the reaction that converts Pyruvate to Acetyl-CoA is <math>\Delta G^{\circle}'= -33.4 Kj/Mol</math>. Therefore, the overall standard free-energy change for Pyruvate metabolism is <math>\Delta G^{\circle}'= -63.9 Kj/Mol</math>. |
Revision as of 12:45, 12 May 2014
Mitocondrial pyruvate metabolism(MPM) is an enzyme that generates ATP form pyruvate.
Chemical reaction
![Pyruvate + 13ADP + 13Pi \rightarrow 13ATP](/wiki/images/math/8/c/1/8c1f1d258edc09e0bf6a00a60726ecc6.png)
Rate equation
- Chemical reactions proceed to equilibrium within closed systems. For a simple reaction
it is defined as
where forward and reverse rates are equal.
- Equilibrium is not reached in open system due to influx and outflux. Mass action ratio[1]
for
reaction is defined as
where subscript ob represents observable at a given point.
- Deviation from equilibrium is measured with Disequilibrium constant
as
- Given the simple uni molecular reaction
the mass action equation can be modified as
![v=K_1A-K_2B](/wiki/images/math/4/f/9/4f987b54432b9936018bfd10963d900c.png)
![v=K_1A \left(1-\frac{K_2B}{K_1A} \right)](/wiki/images/math/0/3/7/037f9459550126e5cd2441ef1640a0a0.png)
Considering and
we have,
![v=K_1A \left(1-\frac{\tau}{K_{eq}} \right)](/wiki/images/math/3/f/9/3f943c876067cef366aa637f2c84b76c.png)
- The generalized arbitrary mass action ratio gives us
![v = K_1A^{n_1}B^{n_2} \ldots \left(1-\frac{\tau}{K_{eq}} \right)](/wiki/images/math/c/b/8/cb8c7324e3da3f18cc6db89df26713fe.png)
![v = K_1A^{n_1}B^{n_2} \ldots (1 - \rho)](/wiki/images/math/1/8/5/185e5a66573702fc1d0b17b55b30ecac.png)
For eg. for the reaction , the rate law would be
- This equation demonstrates how a rate expression can be divided into parts that include both kinetics and thermodynamic properties [2].
- Given the net rate of reaction
, we have
![v = v_f \left(1 - \rho \right)](/wiki/images/math/f/6/a/f6a215a344f21d60a655289cb93408d4.png)
In this model
- The rate law is defined as
- The Failed to parse (PNG conversion failed; check for correct installation of latex and dvipng (or dvips + gs + convert)): \Delta G^o' for the reaction that converts Pyruvate to Acetyl-CoA is Failed to parse (unknown function "\circle"): \Delta G^{\circle}'= -33.4 Kj/Mol . Therefore, the overall standard free-energy change for Pyruvate metabolism is Failed to parse (unknown function "\circle"): \Delta G^{\circle}'= -63.9 Kj/Mol .
![K_{eq}](/wiki/images/math/9/b/8/9b86a46f8d5d72f82284b40ef5232a5b.png)
![Pyruvate Keq.png](/wiki/images/thumb/3/32/Pyruvate_Keq.png/550px-Pyruvate_Keq.png)
- The Flux of pyruvate consumed by mitochondria measured for AS_30D is
[4].
- The steady state concentrations for substrates and products are
,
,
and
.
- The
value calculated from the above mentioned values are Failed to parse (Cannot store math image on filesystem.): 2.20E-018
Parameter values
Parameter | Value | Organism | Remarks |
---|---|---|---|
![]() |
Failed to parse (Cannot store math image on filesystem.): 2.20E^{-018} |
References
- ↑ Hess B. and Brand K. (1965), Enzymes and metabolite profiles. In Control of energy metabolism. III. Ed. B. Chance, R. K. Estabrook and J. R. Williamson. New York: Academic Press
- ↑ Sauro H M, Enzyme Kinetics for Systems Biology, Second Edition, Ambrosius Publishing (2013), ISBN-10: 0-9824773-3-3
- ↑ Owusu-Apenten R. Introduction to Food Chemistry, First Edition, CRC Press (2004), ISBN-10: 084931724X
- ↑ Marín-Hernández A, Gallardo-Pérez JC, Rodríguez-Enríquez S et al (2011) Modeling cancer glycolysis. Biochim Biophys Acta 1807:755–767 (doi)