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

it is a good conductor

explanation: