Heats of Solution and Heats of Reaction on Liquid Ammonia1

1936 ◽  
Vol 58 (12) ◽  
pp. 2509-2510 ◽  
Author(s):  
Frederic C. Schmidt ◽  
Joseph Sottysiak ◽  
Herman D. Kluge
Keyword(s):  
Heats Of Solution ◽  
Heats Of Reaction

Heats of Solution and Heats of Reaction in Liquid Ammonia. I

1934 ◽  
Vol 56 (1) ◽  
pp. 79-86 ◽  
Author(s):  
Charles A. Kraus ◽  
John A. Ridderhof
Keyword(s):  
Liquid Ammonia ◽  
Heats Of Solution ◽  
Heats Of Reaction

Heats of Solution and Heats of Reaction in Liquid Ammonia. VII

1947 ◽  
Vol 69 (5) ◽  
pp. 1025-1027 ◽  
Author(s):  
E. Hennelly ◽  
D. K. Stevens ◽  
M. Warren ◽  
H. Zuhr ◽  
J. Sottysiak ◽  
...  
Keyword(s):  
Liquid Ammonia ◽  
Heats Of Solution ◽  
Heats Of Reaction

STUDIES OF RDX AND RELATED COMPOUNDS: VIII. THERMOCHEMISTRY OF RDX REACTIONS

1952 ◽  
Vol 30 (10) ◽  
pp. 743-748 ◽  
Author(s):  
V. Gilpin ◽  
C. A. Winkler
Keyword(s):  
Heats Of Solution ◽  
Heats Of Reaction ◽  
Related Compounds

The following heats of reaction have been determined, where the subscripts "c" and "s" refer to solid and solution respectively:Hexamine(c) + HNO3 (97.5%) = RDX(s); ΔH = −88.0 kcal. per mole.Hexamine mononitrate(c) + HNO3 (97.5%) = RDX(s); ΔH = −69.2 kcal. per mole.Hexamine dinitrate(c) + HNO3 (97.5%) = RDX(s); ΔH = −41.7 kcal. permole.Hexamine(s) + Bachmann reagents = RDX(s); ΔH = −140 kcal. per mole.Hexamine mononitrate(s) + Bachmann reagents = RDX(s); ΔH = −126 kcal. per mole.Hexamine dinitrate(c) + Bachmann reagents = RDX(s); ΔH = −118 kcal. per mole.These measurements, together with some on heats of solution of the reagents, indicate that hexamine dinitrate is an intermediate in the direct nitrolysis of hexamine to RDX, but that hexamine mononitrate is a probable intermediate in the Bachmann conversion of hexamine to RDX.

Heats of Solution and Heats of Reaction in Liquid Ammonia. II

1934 ◽  
Vol 56 (1) ◽  
pp. 86-88 ◽  
Author(s):  
Charles A. Kraus ◽  
Ralph F. Prescott
Keyword(s):  
Liquid Ammonia ◽  
Heats Of Solution ◽  
Heats Of Reaction

Heats of Solution and Heats of Reaction in Liquid Ammonia. III

1934 ◽  
Vol 56 (11) ◽  
pp. 2297-2300 ◽  
Author(s):  
Charles A. Kraus ◽  
Frederic C. Schmidt
Keyword(s):  
Liquid Ammonia ◽  
Heats Of Solution ◽  
Heats Of Reaction

Properties and Reactivity of First and Second Row Hydrides. IV. Interactions Between Hydrides and Their Radical Ions

1993 ◽  
Vol 58 (1) ◽  
pp. 1-10 ◽  
Author(s):  
Rudolf Zahradník
Keyword(s):  
Radical Cations ◽  
Stabilization Energy ◽  
Hydrogen Atom Abstraction ◽  
Type Ii ◽  
Radical Ions ◽  
Reaction Products ◽  
Ion Molecule Reactions ◽  
Heats Of Reaction ◽  
Experimental Values ◽  
Easy Differentiation

The energies and heats of ion-molecule reactions have been calculated (MP4/6-31G**//6-31G** or better level) and compared with the experimental values obtained from the heats of formation. Two main types of reactions have been studied: (i) AHn + AHn+• ↔ AHn+1+ + AHn-1• (A = C to F and Si to Cl), (ii) AHn + BHm+• ↔ AHn+1+ + BHm-1• or AHn-1+• + BHm+1+ (A and B = C to F). In contrast to (i), processes of type (ii) permit easy differentiation between the proton transfer and hydrogen atom abstraction mechanisms. A third type of interaction involves reactions with radical anions (A = Li to F); comparison was made with analogous processes with radical cations. A brief comment is made about the influence of the level of computational sophistication on the energies and heats of reaction, as well as on the stabilization energy of a hydrogen bonded intermediate, a structure which is similar to that of the reaction products.

Heats of Solution of Some Sodium and Potassium Salts in Water and in Water-Methanol Mixtures

1992 ◽  
Vol 57 (11) ◽  
pp. 2227-2234 ◽  
Author(s):  
Ján Benko ◽  
Oľga Vollárová
Keyword(s):  
Transfer Functions ◽  
Enthalpies Of Solution ◽  
Potassium Salts ◽  
Solvent Interactions ◽  
Heats Of Solution ◽  
Solvent Molecules ◽  
Sodium And Potassium

The enthalpies of solution ∆Hs0 were determined for NaSCN, KSCN, NaBrO3, KBrO3, NaClO3, KClO3, NaIO4, KMnO4, KNO2 and NaNO2 in water-methanol mixtures. The transfer functions ∆Ht0 of the salts and anions were calculated based on the extrathermodynamic TPTB assumption. The ∆Ht0 values of the anion obtained from the sodium and potassium salts were compared. The differences observed, particularly at higher concentrations of the cosolvent, are discussed with respect to the interactions between the solvent molecules and the solute-solvent interactions.

The Molar Heats of Solution of Boric Oxide and Boric Acid1

1951 ◽  
Vol 73 (2) ◽  
pp. 579-581 ◽  
Author(s):  
Ervin R. Van Artsdalen ◽  
Keith P. Anderson
Keyword(s):  
Boric Oxide ◽  
Heats Of Solution
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