T. S. Kon'kova

Enthalpies of formation of triaminoguanidinium chloride, nitrate, and perchlorate

Conclusions1.Enthalpies of combustion and solution have been measured, and the standard enthalpy of formation calculated, for triaminoguanidinium nitrate.2.Standard enthalpies of formation have been calculated for triaminoguanidinium perchlorate and nitrate, and the enthalpy of formation of the triaminoguanidinium ion in dilute aqueous solution determined.

Enthalpy of formation of guanidinium nitrate, perchlorate, and chloride

Conclusions1.The enthalpies of combustion and dissolution of guanidinium nitrate have been measured. The standard enthalpy of formation of guanidinium nitrate has been calculated: ΔHf,298.150[C(NH2)3NO3]c=−92.47±0.17 kcal/mole.2.The enthalpy of formation of the guanidinium ion in infinitely dilute aqueous solution has been calculated: ΔHf,298.150[C(NH2)3+(∞H2O=−33.24±0.21 kcal/mole].3.The enthalpies of dissolution of guanidinium perchlorate and chloride have been measured, and the standard enthalpies of their formation have been calculated:ΔHf,298.150 [C(NH2)3ClO4]c=−74.35 ± 0.22 kcal/mole;ΔHf,298.150 [C(NH2)3Cl]c=−77.66±0.21 kcal/mole.

Combined study of thermochemical properties of nitroform and its salts

A combined method for determination of the standard enthalpies of formation of nitroform and its salts was proposed. The enthalpies of dissolution of nitroform and its ammonium, hydrazinium, guanidinium, and potassium salts in water were measured. The enthalpy of combustion of hydrazinium salt of nitroform was determined by a combustion calorimetry, and its standard enthalpy of formation was calculated. The enthalpy of formation of trinitromethyl anion in indefinitely diluted aqueous solution −24.94±0.79 kJ mol−1, was calculated on the basic of the data obtained for enthalpies of formation and dissolution of ammonium and hydrazinium salts of nitroform. Standard enthalpies of formation of nitroform and its salts were calculated.

Thermochemical properties of monoaminoguanidinium salts

Conclusions1.The enthalpies of combustion and dissolution have been determined, and the standard enthalpy of formation has been calculated, for monoaminoguanidinium nitrate: ΔHf,298.150× [H2NHNC(NH2)2]NO3(c)= −66.62±0.18 kcal/mole.2.The enthalpy of formation of the monoaminoguanidinium ion in an infinitely dilute aqueous solution has been calculated: ΔHf,298.150[H2NHNC(NH2)2+](∞H2O)=-5.48 ± 0.21 kcal/mole.3.The enthalpies of dissolution of monoaminoguanidinium chloride and perchlorate in infinitely dilute aqueous solutions have been determined, and their enthalpies of formation in the standard states have been calculated:ΔHf,298.150 [H2NHNC(NH2)2Cl](c)=-52.73±0.21 kcal/mole,ΔHf,298.150 [H2NHNC(NH2)2ClO4](c)= −45.88±0.21 kcal/mole,.

Thermochemical properties of the salts of picric and dinitrobenzoic acids

The enthalpies of formation and dissolution of the ammonium and guanidinium picrates and dinitrobenzoate were determined by precision calorimetry. On the basis of the data obtained, the enthalpies of formation of the anions of the acids in indefinitely diluted aqueous solutions were calculated and the enthalpy of formation of potassium picrate was estimated.

Integral heats of solution and enthalpies of ionization of 100% nitric acid at 298 K 3. Aqueous solutions of sulfuric acid containing 70–90% H2SO4 and ionization of HNO3 as a base

AbstractThe integral heats of solution of 100% HNO3

Calorimetric study of the esterification of cellulose by H3PO4-HNO3 mixtures

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Integral heats of dissolution and enthalpies of ionization of 100% nitric acid at 298°K. Communication 2. Concentrated aqueous solutions of sulfuric acid

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