Thermodynamics Research Center / ThermoML | Journal of Chemical and Engineering Data

ABSTRACT

The solid-liquid equilibrium for quizalofop-p-ethyl in twelve solvents (methanol, ethanol, 1-propanol, 2-propanol, 1-butanol, N,N-dimethylformamide (DMF), acetone, acetonitrile, ethyl acetate, 1,4-dioxane, toluene and 1-hexane) was measured by using a static equilibrium method at temperatures T = (273.15 to 313.15) K under pressure of 101.2 kPa. The results show that the solubility in those twelve monosolvents increases with increasing temperature. At a given temperature range, they gradually decrease in the following order: 1,4-dioxane greater than acetonitrile greater than DMF greater than toluene greater than acetone greater than ethyl acetate greater than 1-butanol greater than 1-propanol greater than 1-hexane greater than 2-propanol greater than ethanol greater than methanol. Moreover, Modified Apelblat model, Uh model, Wilson model and NRTL model were used to correlate the experiment values. Compared with the results of above models, the calculated values provided good results with the experimental data. Consequently, the values of root-mean-square deviation (RMSD) and relative average deviation (RAD) were no more than 4.57 e10-4 and 2.29 %, respectively. Furthermore, the thermodynamic properties of quizalofop-p-ethyl in monosolvents were calculated. From the analysis results, the dissolution process of quizalofop-p-ethyl was a spontaneous and entropy driven process. The experimental solubility and the models in this study could be helpful in application in the field of purification and recrystallization.