The solubility property of Zn(NO 3) 2 Try H 2O system at 25 ℃ in whole concentration range has been investigated by the semi micro phase equilibrium method. The corresponding phase diagrams and refractive index...The solubility property of Zn(NO 3) 2 Try H 2O system at 25 ℃ in whole concentration range has been investigated by the semi micro phase equilibrium method. The corresponding phase diagrams and refractive index diagrams were constructed. Under the guidance of the phase equilibrium results, the incongruently soluble compounds of Zn(Try)(NO 3) 2·2H 2O (F) and Zn^(Try) 2(NO 3) 2·H 2O (G), which have not been reported previously, were synthesized and characterized by IR, XRD, TG DTG, as well as chemical and elemental analyses. The constant volume combustion energies of the compounds, Δ c E , determined by a precision rotating bomb calorimeter at 298 15 K, were (-13518 98±4 99) J·g -1 and (-17690 85±4 88) J·g -1 , respectively. The standard enthalpies of combustion for these compounds, Δ c H , were calculated to be (-5802 36±2 14) kJ· mol -1 and (-10891 59±3 01) kJ·mol -1 when the standard enthalpies of formation, Δ f H m were (-1161 18±2 61) kJ·mol -1 and (-1829 71±4 20) kJ·mol -1 . The enthalpies of solution in condition of simulating human gastric juice (37 ℃, pH=1, the solution of hydrochloric acid), which were also measured by a microcalorimeter, were (14 55±0 04) kJ·mol -1 and (10 58±0 06) kJ·mol -1 , respectively.展开更多
文摘The solubility property of Zn(NO 3) 2 Try H 2O system at 25 ℃ in whole concentration range has been investigated by the semi micro phase equilibrium method. The corresponding phase diagrams and refractive index diagrams were constructed. Under the guidance of the phase equilibrium results, the incongruently soluble compounds of Zn(Try)(NO 3) 2·2H 2O (F) and Zn^(Try) 2(NO 3) 2·H 2O (G), which have not been reported previously, were synthesized and characterized by IR, XRD, TG DTG, as well as chemical and elemental analyses. The constant volume combustion energies of the compounds, Δ c E , determined by a precision rotating bomb calorimeter at 298 15 K, were (-13518 98±4 99) J·g -1 and (-17690 85±4 88) J·g -1 , respectively. The standard enthalpies of combustion for these compounds, Δ c H , were calculated to be (-5802 36±2 14) kJ· mol -1 and (-10891 59±3 01) kJ·mol -1 when the standard enthalpies of formation, Δ f H m were (-1161 18±2 61) kJ·mol -1 and (-1829 71±4 20) kJ·mol -1 . The enthalpies of solution in condition of simulating human gastric juice (37 ℃, pH=1, the solution of hydrochloric acid), which were also measured by a microcalorimeter, were (14 55±0 04) kJ·mol -1 and (10 58±0 06) kJ·mol -1 , respectively.
