By J. Moreno-Pirajan
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8), EPH of a standard electrode reaction can be determined provided that S* of the reaction is known. mol-1. 15K are given in table 4. (20). Like this, the second problem mentioned in introduction, that is, how to seek a feasible method to calculate or predict the “real” heat effect of a standard reversible electrode reaction, is also resolved. 2 Table 4. 15K. From Ref. [1], but recalculating a part of data according to Ref. 3 Determination of the electric potentials of the standard electrode by H (c→0) The standard electrode potential of an electrode is a very important electrochemical quantity.
The thermodynamic parameter values obtained are shown in Table 3. As it can be observed, the thermodynamic parameter values are very similar, the main difference being the absolute ΔCp values, which were considerably larger (approximately twice as large) for the binding to the Y108V mutant when compared to the wt enzyme. These results might be used to make an assessment on the predilection of the Y108V mutant to adopt a particular 3D structure, when it is complexed with EASG, where there is a high drop in the centroid distance between the ligand EA moiety and Phe 8.
On this scale, the entropy change for a single-electrode reaction, S*T will be characterized as: S*T = z F (∂*T / ∂T) P, (6) When integrating Eq. (6), the integral constant, S*0 is appointed to zero at T→0 based on the third law of thermodynamics. The resultant EPH of the electrochemical reaction, is defined as = z F T ( ∂*/∂T) P, i→0, (7) or = -T (∂ (G*)/∂T) P =T(S*)p, i→0 , (8) where i→0 indicates that the considered electrode reaction progresses in the reversible manner. It should be noted that in this scale, the electronic entropy is specified to be zero.
