The latent energy in cold-worked iron and copper as estimated by determination of heats of solution

1934 ◽  
Vol 30 ◽  
pp. 450 ◽  
Author(s):  
R. W. France
Keyword(s):  
Latent Energy ◽  
Heats Of Solution ◽  
Cold Worked

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.

Determination of dislocation pinning and depinning stages in cold-worked copper

1978 ◽  
Vol 12 (7) ◽  
pp. 627-631 ◽  
Author(s):  
S.M.Seyed Reihani ◽  
C Esnouf ◽  
G Fantozzi
Keyword(s):  
Dislocation Pinning ◽  
Cold Worked

Was Native Copper used in Transcaucasia in Eneolithic Times?

1964 ◽  
Vol 30 ◽  
pp. 66-74 ◽  
Author(s):  
I. R. Selimkhanov
Keyword(s):  
Copper Alloys ◽  
Pure Copper ◽  
Native Copper ◽  
Cold Worked

The majority of scientists hold the opinion that mankind first knew metal in the form of native copper. In particular, at this period the malleability of native copper was realized, and its brittleness when cold worked, as well as the need of annealing to cold forge the necessary tools. The melting of copper was discovered later when native copper was met with in association with ores.These opinions are shared by H. H. Coghlan and H. Otto and W. Witter, though the first mentioned also pointed out that in some regions artifacts made from copper alloys existed in early periods while artifacts made of pure copper might be met with in the latest periods.V. I. Vernadski also had some doubt about the unconditional validity of this theory. However, he did not deny that where native copper was distributed it was the first metal replacing (although only partly) stone and bone for making tools. In certain cases such an assertion has been supported by old and unreliable analyses of ancient artifacts, as well as by some mistakes in the determination of their age.

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.

Sign in / Sign up

Export Citation Format

Share Document