Gconsider 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 ∘c (310 k). δ∘′ for the reaction is +29.7 kj/mol . assume that the reaction occurs at ph 7. [malate]=1.37 mm [oxaloacetate]=0.130 mm [nad+]=460 mm [nadh]=180 mm δ:

The free energy change for malate dehydrogenase reaction is -50kJ/mol

Explanation:

The malate dehydrogenase reaction is:

Malate + NAD⁺ ⇄ Oxaloacetate + NADH + H⁺

Where equilibrium constant, k, could be expressed as:

Replacing with the listed concentrations:

K = 3,713x10⁻⁹

ΔG° is defined as:

ΔG° = RT ln K (1)

Where:

R is gas constant 8,314J/molK

T is temperature 310K

And K = 3,713x10⁻⁹

ΔG° = -50000 J/mol ≡ -50kJ/mol

I hope it helps!

catya your not at all which answer i've seen you do this on another question!