You have an initial solution in which you added quantities of “A” and “B” such that there is 4.5 M “A” and 2.5 M “B” and no complex (“AB”) at time 0. After equilibrium, you are able to isolate and quantitate the “AB” complex, and find its concentration is 1.5 M. Given that RT is 0.59 kcal/mol, what is the delta Go’ for the association reaction?
You have an initial solution in which you added quantities of “A” and “B” such that there is 4.5 M “A” and 2.5 M “B” and no complex (“AB”) at time 0. After equilibrium, you are able to isolate and quantitate the “AB” complex, and find its concentration is 1.5 M. Given that RT is 0.59 kcal/mol, what is the delta Go’ for the association reaction?
Since conditions inside the cell are different than standard temperature and pressure, biochemists use a different set of standards called the biochemical standard state: at pH =7 and [H2O] = 55.5 M and for reactions that require Magnesium [Mg2+] = 1M
Standard free energy change calculated at biochemical standards is called biochemical standard free energy change and is denoted by ΔG'° (delta G prime knot).
K'eq is the equilibrium constant at biochemical standards, K'eq = [product]/[reactants] and is related to biochemical standard free energy change:
ΔG'° = -R T ln K'eq
Where R is the universal gas constant equal to 8.314 J mol-1 K-1, T is the standard temperature of 298 K.
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