scholarly journals THE ADIABATIC DETERMINATION OF THE HEATS OF SOLUTION OF METALS IN ACIDS.

1910 ◽  
Vol 32 (4) ◽  
pp. 431-460 ◽  
Author(s):  
Theodore William Richards ◽  
Laurie Lorne Burgess
Keyword(s):  
Heats Of Solution

Untersuchungen zum ternären System Bi/Te/O, III. Bestimmung thermodynamischer Daten der ternären Verbindungen/Investigations on the Ternary System Bi/Te/O,III. Determination of Thermodynamic Data of Ternary Compounds

1999 ◽  
Vol 54 (2) ◽  
pp. 252-260 ◽  
Author(s):  
P. Schmidt ◽  
C. Hennig ◽  
H. Oppermann
Keyword(s):  
Solid State ◽  
Ternary System ◽  
Thermodynamic Data ◽  
Phase Relations ◽  
Solid State Reactions ◽  
Enthalpies Of Formation ◽  
Ternary Compounds ◽  
Heats Of Solution

The phase relations in the ternary system Bi/Te/O have been determined in previous studies by solid state reactions. Thermodynamical data have now been obtained for the pertinent equilibria. The heats of solution of Bi2O3, Bi12TeO20, Bi10Te2O19, Bi16Te5O34, Bi2TeO5, Bi2Te2O7, Bi2Te4O11 and TeCl4 were determined in 4N HCl. From these the enthalpies of formation of bismuth tellurites at 298 K have been derived:⊿H°b (Bi12TeO20, f, 298) = -901,6 ± 8 kcal/mol,⊿H°b (Bi10Te2O19, f, 298) = -856,1 ± 9 kcal/mol,⊿H°b (Bi16Te5O34, f, 298) = -1519,5 ± 17 kcal/mol,⊿H°b (Bi2TeO5, f, 298)= -222,8 ± 3 kcal/mol,⊿H°b (Bi2Te2O7, f, 298)= -299,4 ± 4 kcal/mol,⊿H°b (Bi2Te4O11, f, 298)= -448,2 ± 7 kcal/mol.

Thermochemisches und kalorisches Verhalten von NdAl3Cl12 / Thermochemical and Calorical Behaviour of NdAl3Cl12

1998 ◽  
Vol 53 (11) ◽  
pp. 1343-1351 ◽  
Author(s):  
H. Oppermann ◽  
M. Zhang ◽  
C. Hennig
Keyword(s):  
Total Pressure ◽  
Solid Phase ◽  
Chemical Transport ◽  
Solution Calorimetry ◽  
Enthalpies Of Formation ◽  
Melting Diagram ◽  
Heats Of Solution ◽  
Neodymium Chloride ◽  
The Enthalpy Of Formation

The thermodynamical data of solid and gaseous aluminium neodymium chloride have been obtained by determination of the decomposition equilibria (of solid) from total pressure measurements and chemical transport reactions (gaseous). The melting diagram was determined by DTA. The enthalpy of formation of the solid phase was calculated from their heats of solution and from the enthalpies of formation and the heats of solution of NdCl3 and AlCl3. Data by total pressure measurement: ΔH°B |(NdAl3Cl12,f,298) = -749,6 ± 2,5 kcal/mol; S°(NdAl3Cl12,f,298) = 118,2 ± 3,0 cal/K·mol. Data by solution calorimetry: ΔH°B(NdAl3Cl12,f,298) = -748,6 ± 1,3 kcal/mol. Data by chemical transport:ΔH°B(NdAl3Cl12,g,298) = -701,5 ± 3,0 kcal/mol; S°(NdAl3Cl12,g,298) = 215,0 ± 4,0 cal/K-mol.

Thermische Zersetzung und Lösungskalorimetrie von Ammoniumneodymiodiden / Thermal Decomposition and Solution Calorimetry of Ammonium Neodymium Iodides

2000 ◽  
Vol 55 (1) ◽  
pp. 65-73 ◽  
Author(s):  
C. Hennig ◽  
H. Oppermann
Keyword(s):  
Thermal Decomposition ◽  
Pressure Measurement ◽  
Total Pressure ◽  
Solution Calorimetry ◽  
Enthalpies Of Formation ◽  
Pressure Measurements ◽  
Heats Of Solution

The thermodynamical data of ammonium neodymium iodides (NH4)3NdI6 and (NH4)2NdI5 were derived by the determination of their decomposition equilibria by total pressure measurements. Moreover, solution calorimetry was applied. The enthalpies of formation of these phases were calculated from their heats of solution and from the enthalpies of formation and the heats of solution of N dl3 and NH4I in 4n HI (aq.) at 298 K.Data by total pressure measurement:⊿H°B(NH4)3NdI6,f,298) = -306,7 ± 4,9 kcal/mol;S°((NH4)3NdI6,f,298) = 152,8 ± 5,7 cal/K·mol;⊿H°B(NH4)2NdI5,f,298) = -260,9 ± 4,2 kcal/mol;S°((NH4)2NdI3,f,298) = 114,3 ± 4,7 cal/K·mol.Data by solution calorimetry:⊿H°B(NdI3,f,298) = -154,3 ± 2,0 kcal/mol;⊿H°B((NH4)3NdI6,f,298) = -299,6 ± 3,2 kcal/mol;⊿H°B((NH4)2NdI5,f,298) = -255,2 ± 2,8 kcal/mol.

AN EXPERIMENTAL DETERMINATION OF THE SURFACE ENTHALPY OF SODIUM CHLORIDE

1956 ◽  
Vol 34 (11) ◽  
pp. 1553-1556 ◽  
Author(s):  
G. C. Benson ◽  
H. P. Schreiber ◽  
F. Van Zeggeren
Keyword(s):  
Sodium Chloride ◽  
Specific Surface ◽  
Experimental Determination ◽  
Special Care ◽  
Heats Of Solution ◽  
Surface Areas ◽  
Specific Surface Areas ◽  
Surface Enthalpy ◽  
Excess Sodium

The surface enthalpy of NaCl has been redetermined from heats of solution of salt samples of different specific surface areas. Special care was taken in the preparation of these samples to avoid contamination by nitrate and excess sodium. The value obtained, 276 ergs/cm.2, differs from that reported by Benson and Benson, viz. 305 ergs/cm.2, for samples containing some nitrate impurity.

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