A procedure is described for the theoretical study of chemical reactions in solution by means of molecular dynamics simulation, with solute-solvent interaction potentials derived from ab initio quantum calculations. We apply the procedure to the case of neutral hydrogen isocyanate hydrolysis, HNCO + 2 H2O -> H2NCOOH + H2O, in aqueous solution, via the assisted-concerted mechanisms and the two-water model. We used the solvent as a reaction coordinate and the free-energy curves for the calculation of the properties related to the reaction mechanisms, with a particular focus on the reaction and activation energies. The results showed that the mechanism with two water molecules attacking the C=N bond is preferred to the mechanism with three waters forming a ring of eight members. In addition, the aqueous medium significantly reduces the activation barrier (Delta G(not equal) = 13.9 kcal/mol) and makes the process more exothermic (Delta G = -11.1 kcal/mol) relative to the gas-phase reaction, increasing the rate constant of the process to k = 4.25 x 10(5) s(-1).