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.

Thermische Zersetzung und Lösungskalorimetrie von Ammoniumsamariumchloriden/Thermal Decomposition and Solution Calorimetry of Ammonium Samarium Chlorides

1997 ◽  
Vol 52 (12) ◽  
pp. 1517-1525 ◽  
Author(s):  
C. Hennig ◽  
H. Oppermann
Keyword(s):  
Thermal Decomposition ◽  
Pressure Measurement ◽  
Total Pressure ◽  
Solution Calorimetry ◽  
Enthalpies Of Formation ◽  
Pressure Measurements ◽  
Heats Of Solution ◽  
Solid Phases

Abstract We determined the decomposition equilibria of ammonium samarium chlorides (NH4)2SmCl5 and NH4Sm2Cl7 by total pressure measurements and derived their thermody­ namical data from the decomposition functions. The enthalpies of formation were compared with the results of the solution calorimetry. The heats of solution of all solid phases in the system SmCl3-NH4Cl and of Sm2O3 were measured in 4n HCl. The enthalpies of formation of ammonium samarium chlorides were derived from the enthalpies of formation of SmCl3 and of NH4Cl and their heats of solution.Data by total pressure measurementΔH°B((NH4)2SmCl5,f,298) =-407,7 ± 2,9 kcal/mol;S0((NH4)2SmCl5,f,298) = 84,0 ± 4,5 cal/K-mol;ΔH°B((NH4)Sm2Cl7,f,298) = -576,8 ± 3,4 kcal/mol;S°(NH4Sm2Cl7,f,298) = 98,1 ± 5,5 cal/K-mol.Data by solution calorimetryΔH°B(SmCl3,f,298) = -248,1 ± 0,8 kcal/mol;ΔH°B((NH4),SmCl5,f,298) = -404 ,3 ± 1,1 kcal/mol;ΔH°B(NH4Sm9Cl7,f,298)= -572,3 ± 1,8 kcal/mol.

Thermische Zersetzung und Lösungskalorimetrie von Ammoniumneodymchloriden/Thermal Decomposition and Solution Calorimetry of Ammonium Neodymium Chlorides

1998 ◽  
Vol 53 (2) ◽  
pp. 175-183 ◽  
Author(s):  
C. Hennig ◽  
H. Oppermann
Keyword(s):  
Thermal Decomposition ◽  
Pressure Measurement ◽  
Total Pressure ◽  
Solution Calorimetry ◽  
Enthalpies Of Formation ◽  
Heats Of Solution

Abstract The thermodynamical data of ammonium neodymium chlorides (NH4)2NdCl5 and NH4Nd2Cl7 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 NdCl3 and NH4Cl.Data by total pressure measurement:ΔH°B((NH4)2NdCl5,f,298) = - 412,5 ± 3,6 kcal/mol;S°((NH4)2NdCl5 f 298) = 80,1 ± 5,8 cal/K · mol;ΔH°B(NH4Nd2Cl7,f,298) = -579,5 ± 3,5 kcal/mol;S°(NH4Nd2Cl7,f,298) 101,8 ± 5,6 cal/K mol.Data by solution calorimetry:ΔH°B(NdCl3,f,298) = -251,2 ± 0,7 kcal/mol;ΔH°B((NH4)2NdCl5,f,298) = -405,5 ± 1,0 kcal/mol;ΔH°B(NH4Nd2Cl7,f, 298) = -576,8 ± 1,7 kcal/mol.

Thermische Zersetzung und Lösungskalorimetrie von Ammoniumneodymbromiden / Thermal Decomposition and Solution Calorimetry of Ammonium Neodymium Bromides

1999 ◽  
Vol 54 (10) ◽  
pp. 1283-1294 ◽  
Author(s):  
C. Hennig ◽  
H. Oppermann
Keyword(s):  
Thermal Decomposition ◽  
Pressure Measurement ◽  
Total Pressure ◽  
Solid Phase ◽  
Solution Calorimetry ◽  
Enthalpies Of Solution ◽  
Pressure Measurements ◽  
Tabulated Data

The thermal decomposition equilibria of ammonium neodymium bromides (NH4)3NdBr6, (NH4)2NdBr5 and NH4Nd2Br7 have been investigated by total pressure measurements. The thermodynamical data of these solid phase complexes have been derived from the decomposition functions. The standard enthalpies of solution in 4N HBr (aq.) of (NH4)3NdBr6, (NH4)2NdBr5, NH4Nd2Br7, NdBr3 and Nd2O3 were measured. On the basis of these values and tabulated data, the standard enthalpies at 298 K of the ammonium neodymium bromides were derived and compared with the results obtained from the total pressure measurements.Data by total pressure measurement: ΔH°B((NH4)3 NdBr6,f,298) = -399,1 ± 4,9 kcal/mol; S°((NH4)3NdBr6,f,298) = 153,4 ± 7,4 cal/K.mol; ΔH°B((NH4)2NdBr5,f,298) = -343,0 ± 4,4 kcal/mol; S°((NH4)2,NdBr5,f,298) = 109,9 ± 6,8 cal/K.mol; ΔH°B(NH4Nd2Br7,f,298) = -484,0 ± 5,1 kcal/mol; S°(NH4Nd2Br7,f,298) = 127,9 ± 6,6 cal/K.mol.Data by solution calorimetry: ΔH°B(NdBr3,f,298) = -208,7 ± 1,6 kcal/mol; ΔH°B((NH4)3- NdBr6,f,298) = -404,8 ± 2,7 kcal/mol; ΔH°B((NH4)2NdBr5,f,298) = -344,2 ± 2,4 kcal/mol; ΔH°B(NH4Nd2Br7,f,298) = -482,7 ± 3,7 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.

Thermochemische Untersuchungen zum ternären System Bi/Se/O. II. Das Teilsystem Bi2O3– SeO2/Thermochemical Investigations on the Ternary System Bi/Se/O.II.The Binary System Bi2O3–SeO2

1999 ◽  
Vol 54 (2) ◽  
pp. 239-251 ◽  
Author(s):  
H . Oppermann ◽  
H . Göbel ◽  
H . Schadow ◽  
P. Schmidt ◽  
C. Hennig ◽  
...  
Keyword(s):  
Phase Diagram ◽  
Total Pressure ◽  
Room Temperature ◽  
Solution Calorimetry ◽  
Enthalpies Of Formation ◽  
Standard Entropy ◽  
Pressure Measurements ◽  
Standard Enthalpies Of Formation ◽  
Higher Temperature ◽  
The Enthalpy Of Formation

We describe the existence of six thermodynamically stable phases on the binary line Bi2O3- SeO2 at room temperature: Bi12SeO20, Bi10Se2O19, Bi16Se5O34, Bi2SeO5, Bi2Se3O9 and Bi2Se4O11. At higher temperature we optained evidence for Bi20Se3O36 and Bi4SeO8. The decomposition pressures were measured for all phases in a membrane zero manometer and the enthalpy of formation and the standard entropy was determined. The phase barogram and phase diagram followed from total pressure measurements and differential thermoanalysis. The standard enthalpies of formation of all phases were also derived from solution calorimetry. The necessary data of transitions on molar enthalpies were obtained by DSC- and Cp-measurements.

Thermische Zersetzung und Lösungskalorimetrie von Ammoniumeuropiumchloriden / Thermal Decomposition and Solution Calorimetry of Ammonium Europium Chlorides

1998 ◽  
Vol 53 (10) ◽  
pp. 1169-1179 ◽  
Author(s):  
C. Hennig ◽  
H. Oppermann ◽  
A. Blonska
Keyword(s):  
Thermal Decomposition ◽  
Thermodynamic Data ◽  
Total Pressure ◽  
Solution Calorimetry ◽  
Enthalpies Of Solution ◽  
Pressure Measurements ◽  
Solid Phases ◽  
Tabulated Data

AbstractThe thermal decomposition equilibria of ammonium europium chlorides (NH4)3EuCl6, (NH4)2EuCl5 and NH4Eu2Cl7 have been investigated by total pressure measurements in a membrane zero manometer. The thermodynamic data of these solid phases have been derived from the decomposition functions. The standard enthalpies of solution in 4n HCl (aq.) of (NH4)3EuCl6, (NH4)2EuCl5, NH4Eu2Cl7, EuCl3 and Eu2O3 were measured. On the basis of these values and tabulated data, the standard enthalpies at 298 K of the ammonium europium chlorides were derived and compared with the obtained results from the total pressure measurements.

Untersuchungen zur thermischen Zersetzung von Ammoniumlanthanhalogeniden/Investigation on the Thermal Decomposition of Ammonium Halides

1997 ◽  
Vol 52 (6) ◽  
pp. 696-706 ◽  
Author(s):  
A. Morgenstern ◽  
H. Oppermann
Keyword(s):  
Thermal Decomposition ◽  
Total Pressure ◽  
Enthalpies Of Formation ◽  
Pressure Measurements ◽  
Ammonium Halides ◽  
One Step

Abstract The decomposition equilibria of Ammonium Lanthanum Halides (NH4)2LaX5 were determined by total pressure measurements in a membrane zero manometer. The phases (NH4)2LaX5 decompose in one step to give solid LaX3 and gaseous NH3 and HX. From the decomposition functions the enthalpies of formation and the standard entropies of the phases are derived.ΔH°B (NH4)2LaCl5,f,298) = -411 ,7 ± 2,2 kcal/mol; S°((NH4)2LaCl5,f,298) = 86,7 ± 2,3cal/Kmol;ΔH°B (NH4)2LaBr5,f,298) = -351,6 ± 3,8 kcal/mol; S°((NH4)2LaBr5,f,298) = 101,1 ± 1,8 cal/Kmol;ΔH°B (NH4)2LaI5,f,298)= -268 ,9 ± 3,9 kcal/mol; S°((NH4)2LaI5,f,298) = 115,5 ± 4,3 cal/Kmol.

Thermisches Verhalten von festem LaAlCl6 und chemischer Transport von LaCl3 mit AlCl3/Thermical Behaviour of Solid LaAlCl6 and Chemical Transport of LaCl3 with AlCl3

1999 ◽  
Vol 54 (11) ◽  
pp. 1410-1416 ◽  
Author(s):  
H. Oppermann ◽  
H. Dao Quoc ◽  
A. Morgenstern
Keyword(s):  
Total Pressure ◽  
Chemical Transport ◽  
Lanthanum Chloride ◽  
Pressure Measurements ◽  
Melting Diagram

The thermodynamical data of solid aluminium lanthanum chloride LaAlCl6 have been obtained by determination of the decomposition equilibria from total pressure measurements. The melting diagram was determined by DTA. The chemical transport of LaCl3 with AlCl3 is suggesting the existence of the gaseous complex LaAl3Cl12. The data are:ΔH(LaAlCl6f,298) =-427,1 ±2,5 kcal/mol, S°(LaAlCl6,f,298) = 61 ±2,5 cal/K-mol,Δ(LaAl3Cl12,g ,298) =-712 ± 7 kcal/mol, S°(LaAl3Cl12,g,298) = 205 ± 3 cal/K-mol.

scholarly journals Determination of Vapor-Liquid Equilibrium from Total Pressure Measurement

1971 ◽  
Vol 14 (4) ◽  
pp. 252-256 ◽  
Author(s):  
Kunio Nagahama ◽  
Seijiro Suda ◽  
Toshikatsu Hakuta ◽  
Mitsuho Hirata
Keyword(s):  
Pressure Measurement ◽  
Total Pressure ◽  
Liquid Equilibrium ◽  
Vapor Liquid Equilibrium ◽  
Vapor Liquid

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.

Sign in / Sign up

Export Citation Format

Share Document