The effect of temperature on the extraction of the trivalent actinides Am3+, Cm3+ and Cf3+ with the liquid cation exchanger dinonylnaphthalenesulphonic acid (HD) in toluene is studied. The different thermodynamic
functions of this system are determined from the experimental results. It is found that the free energy variation for the
extraction of these metal ions by HD is mainly determined by the entropic terms arising from the hydration-dehydration process
of the exchanged ions.
temperature dependence of the molar heat capacities of the tellurites CoTeO3,
MnTeO3 and MnTe6O13
are determined. By statistical manipulation of the values obtained, the parameters
in the equations for the corresponding compounds showing this dependence are
determined using the least-squares method. These equations and the standard
molar entropies are used to determine the thermodynamic functions for T'=298.15 K.
Low-temperature heat capacity of two polymorphs of glycine (α and γ) was measured from 5.5 to 304 K and thermodynamic functions
were calculated. Difference in heat capacity between polymorphs ranges from +26% at 10 K to -3% at 300 K. The difference indicates
the contribution into the heat capacity of piezoelectric γ polymorph, probably connected with phase transition and ferroelectricity.
Thermodynamic evaluations show that at ambient conditions γ polymorph is stable and α polymorph is metastable.
The extraction of radioactive152–154Eu by ethyl hydrogen benzyl phosphonate (HEBP) and ethyl hydrogen benzoyl phosphonate (HEBOP) in n-hexane from an aqueous solution of ionic strength 0.1M (Na+, HClO4) has been investigated at different temperatures and the thermodynamic functions evaluated. HEBOP was found to be more efficient than HEBP as extractant. In addition, the stability constant of the extracted complexes were determined.
The extraction of U(VI) with newly synthesized long chain alkyl amide, N,N-dibutyldodecanamide (DBDA), in toluene has been studied. The dependence of the extraction on nitric acid and DBDA concentrations and temperature from nitric acid solution has been considered. The extracted species has also been investigated using FT-IR spectrometry. The related thermodynamic functions were calculated. The separation factor between U(VI) and Th(IV) is higher and there is no third phase formation under the conditions studied.
The kinetics of oxidation-reduction reaction between N,N-diethylhydroxylamine (DEHAN) and nitrous acid in nitric acid solution
have been studied by spectrophotometry at 9.5°C. The rate equation is −d[HNO2]/dt=K[HNO2]·[DEHAN][HNO3] and the rate constantK=12.81 (mol/l)−2·min−1. A possible mechanism has been suggested on the basis of chemical analysis and Raman spectra. The activation energyE and the thermodynamic functions ΔH#, ΔG# and ΔS# are also calculated.
It was found that N,N,N,N-tetrabutylsuccinylamide (TBSA) in a diluent composed of 50% 1,2,3-trimethylbenzene (TMB) and 50% kerosene (OK) can extract thorium(IV) ion from a nitric acid solution. The results of the extraction study suggested the formation of a 141 thorium(IV) ion, nitrate ion and N,N,N,N-tetrabutylsuccinylamide complex as extracted species. The related thermodynamic functions were also calculated.
N,N,N,N-tetrabutylsuccinylamide (TBSA) in a diluent composed of 50% trimethylbenzene (TMB) and 50% kerosene (OK) can extract uranyl (II) ion from nitric acid solution. The results of extraction study suggested the formation of the 121 uranyl (II) ion, nitrate ion and N,N,N,N-tetrabutylsuccinylamide complex as extracted specis. The values of thermodynamic functions have been calculated.
Extraction coefficients for all lanthanides have been determined in two systems: 0.2M TBP-3M NaNCS, and 3.6M TBP-0.2M NaNCS. The data have been used for the calculation of relative changes in thermodynamic functions accompanying the investigated extraction process. The compensation of enthalpy and entropy changes is found as a result of dehydration of the lanthanide aquaions.
The molar heat capacities
of the pure samples of acetone and methanol, and the azeotropic mixture composed
of acetone and methanol were measured with an adiabatic calorimeter in the
temperature range 78–320 K. The solid–solid and solid–liquid
phase transitions of the pure samples and the mixture were determined based
on the curve of the heat capacity with respect to temperature. The phase transitions
took place at 126.160.68 and 178.961.47 K for the sample of
acetone, 157.790.95 and 175.930.95 K for methanol, which were
corresponding to the solid–solid and the solid–liquid phase transitions
of the acetone and the methanol, respectively. And the phase transitions occurred
at 126.580.24, 157.160.42, 175.500.46 and 179.740.89
K corresponding to the solid–solid and the solid–liquid phase
transitions of the acetone and the methanol in the mixture, respectively.
The thermodynamic functions and the excess thermodynamic functions of the
mixture relative to standard temperature 298.15 K were derived based on the
relationships of the thermodynamic functions and the function of the measured
heat capacity with respect to temperature.