In the citric acid cycle, malate is dehydrogenated to oxaloacetate in a highly endergonic reaction with a ΔG’o of +30 kJ mol-1: L‐malate + NAD+ ⇌ oxaloacetate + NADH + H+ Calculate the equilibrium constant K’eq of this reaction. What is the implication of this result?

Answer :  The value of of this reaction is,

At equilibrium, [L-malate] > [oxaloacetate]

Explanation :

The relation between the equilibrium constant and standard Gibbs free energy is:

where,

= standard Gibbs free energy  = +30 kJ/mol = +30000 J/mol

R = gas constant = 8.314 J/K.mol

T = temperature =

 = equilibrium constant  = ?

The given reaction is:

Therefore, the value of of this reaction is,

As, the value of < 1 that means the reaction mixture contains reactants.

At equilibrium, [L-malate] > [oxaloacetate]

increased stability in the completion of fluorine's outer shell.