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]

it should be all of them because it asks if you included all of those in your answer

explanation:

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.