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!

the child will have heterozygous dominant chromosomes as characters of his father are dominant over the characters of his mother.

the child is heterozygous

dynamic equilibrium is the answer.