Robert N. Goldberg and Robert A. Alberty
This table contains values of the standard transformed Gibbs energies of formation ∆fG´° for 130 biochemical reactants. Values of ∆fG´° are given at pH 7.0, the temperature 298.15 K, and the pressure 100 kPa for three ionic strengths: I = 0, I = 0.1 mol/L, and I = 0.25 mol/L. The table can be used for calculating apparent equilibrium constants K´ and standard apparent reduction potentials E´° for biochemical reactions. Such a listing is more compact than tabulating the actual apparent equilibrium constants or standard apparent reduction potentials, which would require a very large number of reactant–product combinations. In the table, all reactants are in aqueous solution unless indicated otherwise.
A biochemical reactant is a sum of species. For example, ATP consists of an equilibrium mixture of the aqueous species ATP4-, HATP3-, H2ATP2-, MgATP2-, etc. Similarly, phosphate refers to the equilibrium mixture of the aqueous species PO43-, HPO42-, H2PO4-, H3PO4, MgHPO4, etc. Biochemical reactions are written using biochemical reactants in terms of an apparent equilibrium constant K´, which is distinct from the standard equilibrium constant K. This subject is discussed in an IUPAC report (see Ref. 1).
The apparent equilibrium constant K´ and the standard transformed Gibbs energy change ∆rG´° for a biochemical reaction can be calculated from the ∆fG´° values by using the relationship
-RT ln K´ = ∆rG´° = Σν´i ∆fG´°
where the summation is over all of the biochemical reactants. The quantity ν'i is the stoichiometric number of reactant i (ν'i is positive for reactants on the right side of the equation and negative for reactants on the left side); R is the gas constant. As an example, the hydrolysis reaction of ATP is
ATP + H2O(l) = ADP + phosphate
At pH 7.00 and I = 0.25 M, ∆rG´° and K´ are calculated as follows:
∆rG´° = {-1424.70 - 1059.49 - (-2292.50 –155.66)}∙(kJ mol-1) = -36.03 kJ mol-1
K´ = exp[-(-36030 J mol-1)/{(8.3145 J mol-1 K-1)∙(298.15 K)} = 2.05∙106
An example involving a biochemical half-cell reaction is
acetaldehyde(aq) + 2 e- = ethanol(aq)
At 298.15 K, pH 7.00, and I = 0, the standard apparent reduction potential E´° can be calculated as follows
E´° = -(1/nF)·{∆fG´°(ethanol) - ∆fG´°(acetaldehyde)}
where n is the number of electrons in the half-cell reaction and F is the Faraday constant. Then,
E´° = [-1/(2·9.6485·104 C mol-1)]·(58.10·103 J mol-1 - 20.83·103 J mol-1) = -0.193 V
Column definitions for the table are as follows.
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