Page 282 - Thermodynamics of Biochemical Reactions

282 Mathematica Solutions to Problcms

This second program has the advantage that the standard transformed enthalpy of formation can be calculated at other
temperatures.

(b) This second program can be used to construct a plot of the standard transformed enthalpy of formation as a function of
PH.

(c) This second program can be used to calculate the standard transformed enthalpy of formation at several temperature

{-3617.28, -3616.89, -3616.681

This calculation is based on the assumption that the standard enthalpies of formation of the ions at zero ionic strength are
independent of temperature. However, at finite ionic strength there is a small electrostatic effect on the enthalpy.

4.3 (a) Calculate A, G'" in kJ mol-1 at 298.15 K, pH 7, and I = 0.25 M for ATP + H20 = ADP + P,. (b) Calculate the
corresponding A,H'" . (c) Calculate the corresponding A,S'" in J K-lmol-l. (d) Calculate IogK'. (e) Plot the values of
each of these properties versus pH at I = 0.25 M.

(BasicBiochemData2 must be loaded)

calctrGerx[e~,pHlist_,islislist~]:=Module[{energy},(*Calculates the standard transformed
Gibbs energy of reaction in kJ molA-l at specified pHs and ionic strengths for a
biochemical equation typed in the form atp+hao+de==adp+pi. The names of the reactants
call the appropriate functions of pH and ionic strength. pHlist and islist can be
lists. This program can be used to calculate the standard transformed enthalpy of
reaction by appending an h to the name of each reactant.*)
energy=Solve[eq,del;
energy[[1,1,2ll/.pH->pHlist/.is-~~sl~st]

(a) Calculate the standard transformed reaction Gibbs energy

-36.0353

(b) Append h to the name of each reactaant to obtain its standard transformed reaction enthalpy