Will someone please answer all the parts to question 5-6 and include all of the

Question

Will someone please answer all the parts to question 5-6 and include all of the work please. Thank you

Calculating Delta G degree ' and Delta G'. Like reaction 5-25, the conversion of 3-phosphoglycerate (3PG) to 2-phosphoglycerate (2PG) is an important cellular reaction because it is one of the steps in the glycolytic pathway (see Chapter 9): 3-phosphoglycerate Equilibrium 2-phosphoglycerate (5-26) If the enzyme that catalyzes this reaction is added to a solution of 3PG at 25 degree C and pH 7.0, the equilibrium ratio between the two species will be 0.165: K'_eq = [2 - phosphoglycerate]_eq/[3 - phosphoglycerate_eq = 0.165 Cell If you start with a solution containing 0.01 M each of succinate and FAD and add an appropriate amount of the enzyme that catalyzes this reaction, will any fumarate be formed? If so, calculate the resulting equilibrium concentrations of all four species. If not, explain why not. Answer part a assuming that 0.01 M FADH_2 is also present initially. Assuming that the steady-state conditions in a cell are such that the FADH_2/FAD ratio is 5 and the fumarate concentration is 2.5 mu M, what steady-state concentration of succinate would be necessary to maintain Delta G' for succinate oxidation at -1.5 kcal/mol?

Explanation / Answer

in equilibration G= 2.303 RT log Keq.

G= 2.303* 2* 298* log (0.165)

G= 2.303*2*298* (-0.782)

G= -1073

-ve sign means favourable or spontaneous

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