The standard-state free energy of hydrolysis of acetyl phosphate is - 42.3 kJ/mol. a) Calculate the free energy for acetyl phosphate hydrolysis in a solution containing 2 mM acetate, 2 mM phosphate , and 3 nM acetyl phosphate. b) What ratio of concentrations of reactants to that of the products will make the reverse reaction (formation of acetyl phosphate from phosphate and acetate ion) energetically favorable?
My attempt...please tell me if my thinking is correct
a) deltaG = -42300 + 8.314(298)ln[(2x10^-3)(2x10^-3)/(3x10^-9)]
b) 42300 = 8.314(298)ln(?), ? = 25988554.67
so... reactants:products < 25988554.67