Calculating delta G degree\' and delta C. Like reaction 5-23, the conversion of

Question

Calculating delta G degree' and delta C. Like reaction 5-23, 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 2-phosphoglycerate 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 (a) 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. (b) Answer part a assuming that 0.01 M FADH_2 is also present initially. (c) 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 AC for succinate oxidation at -1.5 kcal/mol? Protein Folding. In Chapter 2, we learned that a polypeptide in solution usually folds into its proper three-dimensional shape spontaneously. The driving force for this folding is the tendency to achieve the most favored thermodynamic conformation. A folded polypeptide can be induced to unfold (i.e., will undergo denaturation) if the solution is heated or made acidic or alkaline. The denatured polypeptide is a random structure, with many

Explanation / Answer

WE know that

G0 =-RTlnK

Where R= gas constant=8.314 J/mol K

T= temperature =25 0C =25+273.15=298.15 K

K = 0.165

G0 =-RTlnK =-8.314*273.15*ln0.165=4091.8 J/mol=4.09 kJ/mol

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