Consider the malate dehydrogenase reaction from the citric acid cycle. Given the listed concentrations, calculate the free energy change for this reaction at energy change for this reaction at 37.0 ∘C37.0 ∘C (310 K). ΔG∘′ΔG∘′ for the reaction is +29.7 kJ/mol+29.7 kJ/mol . Assume that the reaction occurs at pH 7. [malate]=1.37 mM [malate]=1.37 mM [oxaloacetate]=0.130 mM [oxaloacetate]=0.130 mM [NAD+]=490 mM [NAD+]=490 mM [NADH]=2.0×102 mM

The Gibbs free energy of the reaction is 21.32 kJ/mol

Explanation:

The chemical equation follows:

The equation used to Gibbs free energy of the reaction follows:

where,

= free energy of the reaction

= standard Gibbs free energy = 29.7 kJ/mol = 29700 J/mol  (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314J/K mol

T = Temperature =

= Ratio of concentration of products and reactants =

Putting values in above expression, we get:

Hence, the Gibbs free energy of the reaction is 21.32 kJ/mol

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

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