Question

If the intracellular concentrations of a metabolite (M-OH) and its phosphorylated form (M-OPO32-) were 3.2 mM and 0.1 mM, respectively, and if the intracellular concentrations of ATP and ADP were 4 mM and 0.15 mM, respectively, what would be the numerical value of \DeltaΔG (in kcal per mol to the nearest hundredth) for the following reaction: M-OH + ATP <--> M-OPO32- + ADP + H+? Assume a temperature of 37 °C and a pH of 7.4. To solve this problem, you will need to know the standard free energies of hydrolysis of the phosphorylated metabolite and of ATP. These values are –3.5 kcal/mol and –7.3 kcal/mol, respectively.

Answer 1

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