Answer : The value of
of this reaction is, ![5.51\times 10^{-6}](https://tex.z-dn.net/?f=5.51%5Ctimes%2010%5E%7B-6%7D)
At equilibrium, [L-malate] > [oxaloacetate]
Explanation :
The relation between the equilibrium constant and standard Gibbs free energy is:
![\Delta G^o=-RT\times \ln K_{eq}](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo%3D-RT%5Ctimes%20%5Cln%20K_%7Beq%7D)
where,
= standard Gibbs free energy = +30 kJ/mol = +30000 J/mol
R = gas constant = 8.314 J/K.mol
T = temperature = ![25^oC=273+25=298K](https://tex.z-dn.net/?f=25%5EoC%3D273%2B25%3D298K)
= equilibrium constant = ?
The given reaction is:
![\text{L-malate}+NAD^+\rightleftharpoons \text{oxaloacetate}+NADH+H^+](https://tex.z-dn.net/?f=%5Ctext%7BL-malate%7D%2BNAD%5E%2B%5Crightleftharpoons%20%5Ctext%7Boxaloacetate%7D%2BNADH%2BH%5E%2B)
![\Delta G^o=-RT\times \ln K_{eq}](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo%3D-RT%5Ctimes%20%5Cln%20K_%7Beq%7D)
![+30000J/mol=-(8.314J/K.mol)\times (298K)\times \ln K_{eq}](https://tex.z-dn.net/?f=%2B30000J%2Fmol%3D-%288.314J%2FK.mol%29%5Ctimes%20%28298K%29%5Ctimes%20%5Cln%20K_%7Beq%7D)
![K_{eq}=5.51\times 10^{-6}](https://tex.z-dn.net/?f=K_%7Beq%7D%3D5.51%5Ctimes%2010%5E%7B-6%7D)
Therefore, the value of
of this reaction is, ![5.51\times 10^{-6}](https://tex.z-dn.net/?f=5.51%5Ctimes%2010%5E%7B-6%7D)
As, the value of
< 1 that means the reaction mixture contains reactants.
At equilibrium, [L-malate] > [oxaloacetate]