scholarly journals Studies on the Heat of Solution. I. Heats of Solution of Crystalline Pentaerythritol and Mesoerythritol

1953 ◽  
Vol 26 (2) ◽  
pp. 63-67 ◽  
Author(s):  
Syûzô Seki ◽  
Keisuke Suzuki
Keyword(s):  
Heat Of Solution ◽  
Heats Of Solution

Thermochemistry of Silver Bromate

1971 ◽  
Vol 49 (3) ◽  
pp. 523-524 ◽  
Author(s):  
L. M. Gedansky ◽  
L. G. Hepler
Keyword(s):  
Solubility Product ◽  
Standard Entropy ◽  
Heat Of Solution ◽  
Heats Of Solution ◽  
Calorimetric Measurements

Calorimetric measurements of the heat of solution of AgBrO3(c) in NH3(aq) have been combined with earlier data on heats of solution of AgNO3(c) in water and in NH3(aq) to yield ΔH0 = 11.78 ± 0.11 kcal mol–1 for AgBrO3(c) = Ag+(aq) + BrO3−(aq). Combination of this value with ΔG0 = 5.83 kcal mol–1 from the solubility product gives ΔS0°= 19.96 cal deg–1 mol–1 for the standard entropy of solution of AgBrO3(c) at 298 °K.

The heats of solution of alcohols in water

1969 ◽  
Vol 22 (2) ◽  
pp. 347 ◽  
Author(s):  
DM Alexander ◽  
DJT Hill
Keyword(s):  
Enthalpy Of Solution ◽  
Heat Of Solution ◽  
Quadratic Dependence ◽  
Heats Of Solution ◽  
Low Concentrations

A new calorimeter has been developed and the enthalpy of solution of methanol, ethanol, propan-1-ol, propan-2-ol, butan-1-ol, and 2- methylpropan-2-ol, in water to low concentrations, measured between 5� and 35�. In all cases, the results can be adequately represented by a quadratic dependence of heat of solution on temperature. The results have been compared qualitatively with the data for the hydrocarbons.

Ligand field splitting energies of the hexaamminecobalt(II) ion and the hexaamminenickel(II) ion measured by a calorimetric method

1970 ◽  
Vol 48 (14) ◽  
pp. 2177-2181 ◽  
Author(s):  
Badri Muhammad ◽  
J. W. S. Jamieson
Keyword(s):  
Close Agreement ◽  
High Energy ◽  
Calorimetric Method ◽  
Ligand Field ◽  
Maximum Difference ◽  
Kcal Mole ◽  
Heat Of Solution ◽  
Field Splitting ◽  
Heats Of Solution ◽  
Splitting Energy

Various normal lower ammines and high-energy modifications of the lower ammines of cobalt(II) sulfate and nickel(II) sulfate have been prepared and the heats of solution in dilute ammonia have been measured for both types. For each of these ammine systems the maximum difference in heat of solution, expressed as kcal/mole of each heptaammine, between the high-energy and the normal salts has been found to be in close agreement with the ligand field splitting energy of the hexaamminemetal(II) ion.

Calorimetrie an Ammoniumyttriumhalogeniden / Calorimetry of Ammonium Yttrium Halides

1997 ◽  
Vol 52 (3) ◽  
pp. 311-314 ◽  
Author(s):  
S. Ehrlich ◽  
H. Oppermann ◽  
C. Hennig
Keyword(s):  
Enthalpies Of Formation ◽  
Heat Of Solution ◽  
Heats Of Solution ◽  
Solid Phases

Abstract The heat of solution of all solid phases in the system YX3-NH4X with X = Cl, Br, I in 4n HX was investigated. The enthalpies of formation of the ammonium yttrium halides are derived from the enthalpies of formation of Y X3 and of NH4X and their heats of solution in An HX: ΔHB0(NH4Y2Cl7,f,298) = -561,5 ± 1,7 kcal/mol, ΔHB0((NH4)3 YCl6,f,298) = -474,5 ± 1,3 kcal/mol,ΔHB0((NH4)3YBr6,f,298) = -400,8 ± 2,6 kcal/mol, ΔHB0((NH4)3YI6,f,298) = -291,9 ± 3,0 kcal/mol.

The Heats of Solution and Related Thermodynamic Properties of Sodium Chlorate in Water and Water–Dioxane Mixtures

1971 ◽  
Vol 49 (2) ◽  
pp. 217-224 ◽  
Author(s):  
A. N. Campbell ◽  
O. Bhatnagar
Keyword(s):  
Free Energy ◽  
Thermodynamic Properties ◽  
Activity Coefficients ◽  
Direct Method ◽  
Sodium Chlorate ◽  
Saturated Solution ◽  
Heat Of Solution ◽  
Heats Of Solution ◽  
Tentative Explanation ◽  
A Direct Method

The heats of solution of sodium chlorate in water, and in several water-dioxane mixtures, have been determined experimentally at concentrations of salt ranging from 0.01 molal to saturation. For the dilute region, a direct method was used but for the concentrated range the method was that of diluting the saturated solution. The free energy decreases due to dilution have been calculated from previously determined activity coefficients. Using these data, the entropy changes have been evaluated.The graph of heat of solution vs. concentration of sodium chlorate passes through a minimum for the solutions more concentrated in dioxane, but not for water and weak dioxane mixtures. A tentative explanation of this is offered.

THE HEATS OF SOLUTION AND SPECIFIC HEATS OF RHOMBIC SULPHUR IN CARBON DISULPHIDE: THE SURFACE ENERGY OF SOLID RHOMBIC SULPHUR

1935 ◽  
Vol 13b (5) ◽  
pp. 280-288 ◽  
Author(s):  
A. R. Williams ◽  
F. M. G. Johnson ◽  
O. Maass
Keyword(s):  
Particle Size ◽  
Surface Energy ◽  
Carbon Disulphide ◽  
Heat Of Solution ◽  
Specific Heats ◽  
Heats Of Solution

The heats of solution of rhombic sulphur in carbon disulphide were measured over the concentration range 6 to 17% of sulphur and at 20° and 25 °C., and the specific heats of these solutions were calculated. The apparatus designed for these measurements is described. By measuring the heat of solution of finely divided sulphur and its particle size, the surface energy of solid rhombic sulphur is estimated.

Heats of Solution and Swelling of Some Synthetic High-Molecular Compounds

1951 ◽  
Vol 24 (4) ◽  
pp. 773-776 ◽  
Author(s):  
A. Tager ◽  
V. Sanatina
Keyword(s):  
Mechanical Behavior ◽  
Polymer Chain ◽  
High Polymer ◽  
Heat Of Solution ◽  
Barrier Potential ◽  
Heats Of Solution ◽  
Molecular Compounds

Abstract 1. The heat of solution of a high polymer depends on the nature of the solvent as well as on the nature of the polymer. 2. The value and sign of the heat of solution of a polymer are related to the structure of the polymer and its mechanical behavior. For polymers which have relatively flexible chains, the heats of solution are negative ; for polymers which have relatively rigid chains, the heats of solution are positive. 3. The value and sign of the heat of solution indicate to a certain degree the change of the barrier potential of the polymer chain in any given solvent.

scholarly journals Basicity of N-substituted anilines and pyridine in dimethylsulfoxide

1981 ◽  
Vol 59 (10) ◽  
pp. 1501-1504 ◽  
Author(s):  
Robert L. Benoit ◽  
Moyra J. Mackinnon ◽  
Léon Bergeron
Keyword(s):  
Gas Phase ◽  
Aromatic Amines ◽  
Ionization Constants ◽  
Heat Of Solution ◽  
Substituted Anilines ◽  
Heat Of Vaporization ◽  
Heats Of Solution ◽  
Phase Data

The ionization constants of the conjugated acids BH+ of aniline, N-methyl- and N,N-dimethylaniline, and pyridine have been determined potentiometrically in Me2SO. The heats of neutralization of the amines B and their heats of solution have been obtained by calorimetry. The pK's and enthalpies of ionization of these BH+ ions and alkylammonium ions are linearly related. Comparisons with gas phase data show that the abnormal basicity order of the amines B in Me2SO is mainly due to the decreasing exothermicity of the heat of solution of the BH+ ions with the number of N—H protons available for H-bonding to Me2SO. The large increase in basicity difference between equally substituted aromatic and alkylamines, when passing from the gas phase to Me2SO, is linked to the larger heat of vaporization of the aromatic amines.

Thermochemistry of the aqueous manganous ion

1969 ◽  
Vol 47 (4) ◽  
pp. 699-701 ◽  
Author(s):  
L. M. Gedansky ◽  
L. G. Hepler
Keyword(s):  
Kcal Mole ◽  
Heat Of Solution ◽  
Standard Heat ◽  
Heats Of Solution ◽  
Heats Of Dilution

Heats of solution of MnSO4(c) have been measured and combined with heats of dilution to yield ΔH0 = −15.3 kcal/mole for the standard heat of solution. This value leads to ΔHf0 = −52.9 kcal/mole for Mn2+(aq). Calculations with data from the literature give ΔGf0 = −55.1 kcal/mole for Mn2+(aq). Combination of this value with our ΔHf0 gives [Formula: see text] for Mn2+(aq). Our ΔHf0 value for Mn2+(aq) is compared with other values derived from calculations based on data taken from the literature.

scholarly journals Heats of Solution of Liquid Solutes in Various Solvents

2013 ◽  
Vol 2013 ◽  
pp. 1-3 ◽  
Author(s):  
Vladimir D. Kiselev ◽  
Ilzida I. Shakirova ◽  
Lubov N. Potapova ◽  
Helen A. Kashaeva ◽  
Dmitry A. Kornilov
Keyword(s):  
Heat Of Mixing ◽  
Heat Of Solution ◽  
Limit Values ◽  
Heats Of Solution ◽  
Wide Range

The values of the heats of solution (2131 solutions) of different liquid solutes in organic and inorganic solvents were obtained from the literature data on the heat of mixing (ΔmixH) in the wide range of concentrations. The limit values of the heat of solution of a solute (i) in a solvent (j) (ΔsolnHi/j) were calculated from the limit data of the dependence ΔmixH/xi  versus  xi at xi→0 and the values of that of a solute (j) in a solvent (i) (ΔsolnHj/i) from the limit data of the dependence ΔmixH/xj  versus  xj at xj→0, respectively.

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