Beginning with the untransformed Gibbs energies of formation, document the intermediate calculations for the value of apparent Gibbs energy of formation of ADP at the conditions of Example 18.10, using the extended Debye-Hückel activity coefficient model and transformed Gibbs energies. Also calculate the distribution of each species.

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Example 18.10 ATP hydrolysis (a) Calculate the transformed standard state Gibbs energy of reaction and equilibrium constant K' for hydrolysis of ATP at pH=7, pMg = 3, 298.15 K, ionic strength, I = 0.25 m, where the following data apply. (b) Show whether the reaction is endergonic or exergonic at the above conditions when the apparent concentrations are [ATP] = 0.00185 M. [ADP] = 0.0014 M, [P;] = 0.001 M. If the reac- tion is exergonic, at what concentration of ADP does it reach equilibrium if the concentration of phosphate and ATP are constant? Gibbs energies of formation at pH = 7, pMg = 3, 298.15K, I = 0.25 mol/kg ATP H₂O ADP -2298 -156 -1426 AG'O f.i (kJ/mol) P₁ -1060