Impurity determination by thermal analysisThe melting curve of a gradually frozen sample

Wijk, H.F. Van; Smit, W. M.

doi:10.1016/s0003-2670(01)81376-3

Cited by 4 publications

(3 citation statements)

References 3 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…In conformity with Alexandrov recommendation (Alexandrov, 1975), the tp N in a binary system with solid solution formation (Van Wijk & Smit, 1960) and (Alexandrov et al, 1983):…”

Section: Determination Of Thermodynamic Properties Of the Phase Transsupporting

confidence: 68%

Thermodynamics of the Phase Equilibriums of Some Organic Compounds

Varushchenko¹,

Дружинина²

2011

Thermodynamics - Interaction Studies - Solids, Liquids and Gases

View full text Add to dashboard Cite

“…In conformity with Alexandrov recommendation (Alexandrov, 1975), the tp N in a binary system with solid solution formation (Van Wijk & Smit, 1960) and (Alexandrov et al, 1983):…”

Section: Determination Of Thermodynamic Properties Of the Phase Transsupporting

confidence: 68%

Thermodynamics of the Phase Equilibriums of Some Organic Compounds

Varushchenko¹,

Дружинина²

2011

Thermodynamics - Interaction Studies - Solids, Liquids and Gases

View full text Add to dashboard Cite

“…It is doubtful whether these dependences can be explained by the formation of the solid solution because of the high purity of the sample, 0.9994 mole fraction (Table ). Nevertheless, for the determination of the impurity content, a treatment of these experiments were carried out by the Smit–Aleksandrov method , which was applicable for the case of solid solution formation between the main compound and impurities. The T tp temperatures in these experiments were calculated by the Mastrangelo–Dornte method.…”

Section: Methodsmentioning

confidence: 99%

Heat Capacity and Thermodynamic Functions of Diphenylacetylene

et al. 2011

View full text Add to dashboard Cite

The heat capacity of diphenylacetylene was measured by vacuum adiabatic calorimetry over the temperature range from (8 to 371) K. The temperature and the enthalpy and entropy of fusion have been determined. The standard thermodynamic functions (changes of the entropy, enthalpy, and Gibbs free energy) were obtained for the crystal and liquid states in the temperature interval studied and for the ideal gas state at T = 298.15 K. The ideal gas entropies in wide temperature range were also calculated by the principle of additivity and statistical thermodynamics using molecular constants determined by the density functional theory (DFT) method on the level B3LYP/cc-pVTZ. The S m 0(g)(298.15K) values derived from the experimental and calculated data agree within (0.3 to 0.2) % which confirms their reliability. The data on thermodynamic properties of diphenylacetylene studied earlier and in this work were critically analyzed for verification of their reliability and mutual consistency.

show abstract

“…The triple point temperatures and cryoscopic constants (Table ) were determined according to the Rossini method . The mole fraction of impurities, x 2 , in the POF and PF samples were determined by the Smit−Aleksandrov method , using the equation for the equilibrium fusion temperature of the binary system with solid solution ln true( − d T i d ( 1 / F i ) true) = ln true{ x 2 A c r ( 1 − k ) 2 true} − k · ln ( 1 / F i ) where A cr is a cryoscopic constant of the compound under study and k denotes a coefficient of the impurity distribution between the solid and liquid phases of the system. Equation makes it possible to determine k directly from the experimental dependences T i = f (1/ F i ) and then to calculate the x 2 value.…”

Section: Methodsmentioning

confidence: 99%

Heat Capacities and Thermodynamic Functions of Propanoylferrocene and Propylferrocene

et al. 2008

View full text Add to dashboard Cite

The heat capacities of propanoylferrocene (POF), C 5 H 5 FeC 5 H 4 COC 2 H 5 , and propylferrocene (PF), C 5 H 5 FeC 5 -H 4 C 3 H 7 -n, were measured by vacuum adiabatic calorimetry in the temperature ranges from (10 and 7) K to 372 K. The temperatures and enthalpies of the phase transitions and the purity of the samples have been determined. The solid phase transition of PF was studied by single-crystal crystallography in the temperature range from (150 to 200) K. The thermodynamic functions (absolute entropies, changes of the enthalpy, and Gibbs energy) of POF and PF were calculated for the solid and liquid phases of the temperature intervals studied. The ideal gas thermodynamic functions were derived at T ) 298.15 K using the data on saturated vapor pressure and the enthalpies and entropies of vaporization. A reliability of the ideal gas thermodynamic functions was corroborated by the additive calculation method. A mutual congruence of the absolute entropies of alkylferrocenes and acylferrocenes studied in this work and available in the literature were critically analyzed.

show abstract

Impurity determination by thermal analysisThe melting curve of a gradually frozen sample

Cited by 4 publications

References 3 publications

Thermodynamics of the Phase Equilibriums of Some Organic Compounds

Thermodynamics of the Phase Equilibriums of Some Organic Compounds

Heat Capacity and Thermodynamic Functions of Diphenylacetylene

Heat Capacities and Thermodynamic Functions of Propanoylferrocene and Propylferrocene

Contact Info

Product

Resources

About