Effect of plastic flow on the kinetics of amorphous phase growth by solid state reaction in the Ni-Zr system

1990 ◽  
Vol 65 (16) ◽  
pp. 2019-2022 ◽  
Author(s):  
G. Mazzone ◽  
A. Montone ◽  
M. Vittori Antisari
Keyword(s):  
Solid State ◽  
Plastic Flow ◽  
Amorphous Phase ◽  
Solid State Reaction ◽  
Phase Growth ◽  
Kinetics Of

Amorphization of Thin Multilayer Films by Ion Mixing and Solid State Reaction

1983 ◽  
Vol 27 ◽  
Author(s):  
M. Van Rossum ◽  
U. Shreter ◽  
W. L. Johnson ◽  
M-A. Nicolet
Keyword(s):  
Solid State ◽  
Amorphous Phase ◽  
Solid State Reaction ◽  
Amorphous Alloys ◽  
Composition Range ◽  
Multilayer Films ◽  
Solid State Diffusion ◽  
State Diffusion ◽  
Thermochemical Parameters ◽  
Mixed Samples

ABSTRACTWe have compared the formation of amorphous alloys from Ni-Hf multilayer films by ion mixing and solid state diffusion. We find that ion mixing and solid state reaction produce significant differences in the composition range of the amorphous phase inside the mixed samples. Moreover, the thermochemical parameters which are of primary importance for the solid state reaction also influence the behavior of the Ni-Hf system under ion mixing.

Kinetics of the solid state reaction between zinc oxide and aluminum oxide

1980 ◽  
Vol 11 (3) ◽  
pp. 455-461 ◽  
Author(s):  
K. Nagata ◽  
K. Sato ◽  
K. S. Goto
Keyword(s):  
Zinc Oxide ◽  
Solid State ◽  
Aluminum Oxide ◽  
Solid State Reaction ◽  
Kinetics Of

Kinetic study and modeling of the solid-state reaction Y2BaCuO5 + 3BaCuO2 + 2CuO ⇉ 2YBa2Cu3O6.5−x + xO2

1990 ◽  
Vol 5 (10) ◽  
pp. 2056-2065 ◽  
Author(s):  
Nae-Lih Wu ◽  
Ta-Chin Wei ◽  
Shau-Y Hou ◽  
S-Yen Wong
Keyword(s):  
Particle Size ◽  
Solid State ◽  
Solid State Reaction ◽  
Size Dependence ◽  
Average Particle Size ◽  
Average Particle ◽  
Fractional Conversion ◽  
X Ray ◽  
Unreacted Core ◽  
Kinetics Of

The kinetics of the solid-state reaction Y2BaCuO5 + 3BaCuO2 + 2CuO ⇉ 2YBa2Cu3O6.5−x + xO2 was studied by using x-ray diffractometric and thermogravimetric analyses. Both analyses established that the reaction was well described by the kinetic equation: 1 − 3(1 − F)2/3 + 2(1 − F) = k0 exp(− E/RT)t, where F is the fractional conversion of a calcined powder, E is 520 kcal/molc and, for a rcactant mixture with an average particle size of 3 μm, k0 is 2.03 ⊠ 1092 min−1. An unreacted-core shrinking model was proposed to obtain the particle-size dependence of the reaction, and predicted that the pre-exponential constant k0 changed with reactant particle size by k0 = 2.03 ⊠ 1092(3/d)2 exp(4/d − 4/3), where d is the average reactant particle size in μm.

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