
Heterogeneous Kinematics Handbook
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"Soustelle (emeritus, heterogenous kinetics, Ecole NationaleSupérieure des Mines, France) offers an extensive overview ofthe theoretical and experimental basis of heterogenous kinetics andits application to the study of solids reactivity. The fieldintegrates physical, theoretical, and computational elements ofchemistry and materials science. The book's contents are based oncourses given for undergraduates and master's students in chemicalengineering." (Book News, September 2010)Weitere Details
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Inhalt
- Cover
- Handbook of Heterogenous Kinetics
- Title Page
- Copyright Page
- Table of Contents
- Preface
- List of Symbols
- Chapter 1. Definitions and Experimental Approach
- 1.1. Thermal transformations of solids
- 1.2. Classification of transformations
- 1.2.1. Transformation without formation of a new solid phase
- 1.2.2. Transformation with formation of a new solid phase
- 1.3. Speed and rate of reaction
- 1.3.1. Speed of reaction
- 1.3.2. Fractional extent and rate of a reaction
- 1.3.3. Volumes of the phases and coefficient of expansion of the reaction
- 1.4. Reaction zones of a transformation
- 1.4.1. Definition
- 1.4.2. Classification
- 1.4.3. Sizes of a reaction zone
- 1.5. Chemical characterizations
- 1.5.1. Analyses of the gas phases
- 1.5.2. Elementary analyses of the solids
- 1.6. Structural characterizations of the solids
- 1.7. Textural characterizations of the solids
- 1.7.1. The marker method
- 1.7.2. The cavity method
- 1.8. Characterization of the evolution of the systems
- 1.8.1. Curves of evolution: definitions
- 1.8.2. Curves of evolution: experimental obtaining
- 1.8.3. Curves of evolution: obtained laws
- 1.9. Influence of various variables on speed
- 1.9.1. Influence of temperature
- 1.9.2. Influence of partial pressures of gases
- 1.9.3. Influence of the shapes and sizes of solid particles
- Chapter 2. The Real Solid: Structure Elements and Quasi-Chemical Reactions
- 2.1. Structure elements of a solid
- 2.1.1. Definition of a structure element
- 2.1.2. Binary solids
- 2.1.3. Symbolic notation of structure elements
- 2.1.4. Building unit of a solid
- 2.1.5. Description and composition of a solid
- 2.2. Structure elements of a stoichiometric binary solid
- 2.2.1. Schottky disorder
- 2.2.2. Frenkel disorder
- 2.2.3. Antistructure disorder
- 2.2.4. S.A. disorder
- 2.3. Structure elements of a non-stoichiometric binary solid
- 2.3.1. Distance from stoichiometry and structure element
- 2.3.2. The approximation of Wagner of the prevalent defect for ionic solids
- 2.3.3. More complex binary compounds
- 2.4. Extension to non-binary compounds
- 2.4.1. The pseudo-binary approximation
- 2.4.2. Generalization of the approximation of the prevalent defect
- 2.5. Quasi-chemical reactions
- 2.5.1. Definition and characteristics of quasi-chemical reactions
- 2.5.2. Homogenous quasi-chemical reactions in the solid
- 2.5.3. The interphase reactions
- 2.5.4. Reactions of solid destruction
- 2.6. Introduction of foreign elements into a solid
- 2.6.1. Concepts of impurity and doping agent
- 2.6.2. The controlled atomic imperfection in stoichiometric solids
- 2.6.3. The controlled electronic imperfection in non-stoichiometric solids
- 2.6.4. Concept of induced valence
- Chapter 3. Thermodynamics of Heterogenous Systems
- 3.1. Introduction: aims of thermodynamics
- 3.2. General survey of thermodynamics of equilibrium
- 3.2.1. Chemical potential of a component in a phase
- 3.2.2. Variance of a system at equilibrium
- 3.2.3. Associated extensive properties of a transformation, partial molar properties
- 3.2.4. Chemical potential of an ion or a structure element
- 3.2.5. Feasibility of chemical reactions: De Donder inequality
- 3.2.6. Law of mass action for equilibriums
- 3.3. Phenomena leading to solid-gas equilibriums
- 3.3.1. Systems with variance p - 1
- 3.3.2. Systems with variance p
- 3.3.3. Systems with variance p + 1
- 3.4. Thermodynamic approach of solid-gas systems
- 3.4.1. Univariant systems
- 3.4.2. Divariant systems
- 3.4.3. Trivariant systems
- 3.5. Thermodynamics of systems containing solid phases only
- 3.5.1. Non-variant systems
- 3.5.2. Univariant systems
- 3.6. Specific study of quasi-chemical equilibriums
- 3.6.1. Equilibrium between an oxide and oxygen: the Wagner prevalent defect approximation
- 3.6.2. General equilibrium of an oxide with oxygen in the Brouwer approximation of majority defects
- 3.6.3. Doping a solid with foreign elements: quantitative aspect
- 3.7. Thermodynamics of systems: water vapor-hydrated salts
- 3.7.1. Experimental approach of equilibriums between water vapor and hydrated salts
- 3.7.2. Study of the equilibriums with variance 1
- 3.7.3. Study of hydrates with variance 2
- 3.8. Sequence of transformations, juxtaposition of stability area
- 3.9. Equilibrium of the formation of a solid from a solution
- 3.9.1. Solubility product and supersaturation
- 3.9.2. Extension to formation of a real solid
- 3.9.3. Extension to the transformation of a solid into another solid
- 3.10. Variations in the equilibrium conditions with sizes of solid phases
- 3.10.1. Variation in equilibrium constant with curvature radii
- 3.10.2. Influence of curvature radii on tension of vapor
- 3.10.3. Influence of curvature radii on point defect concentrations
- Chapter 4. Elementary Steps in Heterogenous Reactions
- 4.1. Nature of elementary steps
- 4.1.1. The postulate of the activated jump
- 4.1.2. Voluminal speed of an elementary jump
- 4.1.3. Total voluminal speed of an elementary step
- 4.2. Elementary reactions at solid-solid interfaces
- 4.2.1. The phenomenon of epitaxy
- 4.2.2. Creation of an M interstitial cation in MG
- 4.2.3. Creation of a G vacancy anion in MG
- 4.2.4. Consumption of a G interstitial anion of MG
- 4.2.5. Consumption of an M vacancy cation of MG
- 4.2.6. Creation of the point defects created in the initial solid
- 4.3. Elementary reactions at gas-solid interfaces
- 4.3.1. Consumption of an M interstitial cation of MG
- 4.3.2. Consumption of a G vacancy anion of MG
- 4.3.3. Creation of a G interstitial anion in MG
- 4.3.4. Creation of an M vacancy cation in MG
- 4.4. The apparent energies of activation of interface reactions
- 4.5. The areal speed of an interface reaction
- Chapter 5. Chemical Diffusion
- 5.1. Introduction: nature of diffusing particles in a solid
- 5.1.1. Origin of the diffusion in a solid
- 5.1.2. Mechanisms of diffusion in a solid
- 5.2. Flux of diffusion and velocity of diffusing particles
- 5.3. The laws of Fick
- 5.3.1. First law of Fick
- 5.3.2. Second law of Fick
- 5.3.3. Expression of the laws of Fick in various axes systems
- 5.3.4. Solutions of the laws of Fick
- 5.3.5. Self-diffusion and diffusion of the associated defect
- 5.4. Steady state obstructed diffusion
- 5.5. Diffusion under electric field
- 5.5.1. Expression of flux
- 5.5.2. Electric conductivity and diffusion
- 5.5.3. Diffusion in a semiconductor with electronic conduction under null current and without accumulation
- 5.6. Diffusion in two mediums separated by a mobile interface
- 5.6.1. Danckwerts solution
- 5.6.2. Example of application
- 5.6.3. Wagner pseudo-steady state approximation
- Chapter 6. Chemical Adsorption
- 6.1. Definitions: physical adsorption and chemical adsorption
- 6.2. Adsorption thermodynamics and chemisorption equilibrium
- 6.2.1. Experimental results on adsorption equilibrium
- 6.2.2. The Langmuir model of chemisorption equilibrium
- 6.2.3. Dissociative adsorption and the Langmuir model
- 6.2.4. Chemisorption of gas mixtures in the Langmuir model
- 6.2.5. Adsorption isotherms that do not follow the Langmuir model
- 6.3. Kinetics of chemisorption
- 6.3.1. Velocity equation
- 6.3.2. Role of temperature on the kinetics of adsorption
- 6.4. Chemisorption and structure elements
- 6.4.1. Ways of chemisorption modeling
- 6.4.2. The concepts used in the quasi-chemical description of adsorption
- 6.4.3. Modes of adsorption
- 6.4.4. Modifications of the properties of adsorption of a solid
- Chapter 7. Mechanisms and Kinetics of a Process
- 7.1. Speeds and reactivities of reactions taking place in only a single zone
- 7.1.1. Voluminal speed in a zone
- 7.1.2. Reactivity of a transformation in a given zone
- 7.2. Transformations with several zones
- 7.2.1. Postulate of the decomposition of a reaction in elementary steps
- 7.2.2. Reaction mechanism
- 7.2.3. Material balance in a reaction zone
- 7.2.4. Setting in the equation of mechanism - example
- 7.3. Linear reaction mechanisms
- 7.3.1. Definition and classification of the linear mechanisms
- 7.3.2. Multiplying coefficients of a linear mechanism
- 7.4. Linear mechanisms in pseudo-steady state modes
- 7.4.1. Definitions
- 7.4.2. Theorem of "the equality of rates" of a linear mechanism in pseudo-steady state modes
- 7.4.3. Relations between various forms of the rates (speed) of reactions with a linear mechanism in pseudo-steady state modes
- 7.4.4. Volumes of the phases and coefficient of expansion of a reaction with a linear mechanism in pseudo-steady state modes
- 7.4.5. Setting in equation of a linear mechanism in pseudo-steady state modes
- 7.5. Pure modes or modes with a rate-determining step
- 7.5.1. Definition
- 7.5.2. Theorem of the concentrations in pure mode
- 7.5.3. Reactivity of the rate-determining step in pure mode
- 7.5.4. Application of the method of the pure modes
- 7.5.5. Rate of the reaction in pure modes
- 7.5.6. Examples of resolutions of pure modes
- 7.5.7. Pure modes far from equilibrium
- 7.6. Mixed modes
- 7.6.1. Definition: pseudo-steady state mixed modes
- 7.6.2. Solving a pseudo-steady state mixed mode
- 7.7. Generalization, rate of a linear mechanism in pseudo-steady state mode
- 7.8. Mixed non-pseudo-steady state modes
- 7.9. Equivalent reaction of a linear subset in local pseudo-steady state mode
- 7.9.1. Local pseudo-steady state modes
- 7.9.2. Application to the "elementary" steps
- 7.10. Reactions with separable rates
- 7.11. Influence of intensive variables on the kinetic laws
- 7.11.1. The first kind of changes of laws
- 7.11.2. The second kind changes of laws
- 7.11.3. The third kind changes of laws
- 7.12. Distance from equilibrium for a reaction
- 7.12.1. Distance of an elementary step from equilibrium
- 7.12.2. Pseudo-steady state mode with a rate-determining step
- 7.13. Processes concerned in a heterogenous reaction
- Chapter 8. Nucleation of a New Solid Phase
- 8.1. Clusters
- 8.2. Examples of nucleation diagram
- 8.3. Interfacial energy
- 8.3.1. Definition of interfacial energy
- 8.3.2. Microscopic interpretation
- 8.3.3. Effective interfacial energy
- 8.3.4. Relation between energy and the interfacial area
- 8.4. Formation molar Gibbs energy of clusters
- 8.4.1. Assumptions
- 8.4.2. Homogenous nucleation within a liquid phase: Volmer approach
- 8.4.3. Homogenous nucleation within a solid phase
- 8.4.4. Heterogenous primary nucleation starting from a fluid phase
- 8.4.5. Heterogenous primary nucleation starting from a solid phase
- 8.5. Kinetics of nucleation
- 8.5.1. Reaction pathway and localization of the phenomena
- 8.5.2. Rate and frequency of nucleation
- 8.5.3. Various considered modes
- 8.5.4. Kinetics of pseudo-steady state modes of condensation
- 8.5.5. Kinetics of pseudo-steady state modes of condensation on potential nuclei
- 8.5.6. Intervention of diffusion in the process of nucleation
- Chapter 9. Growth of a Solid Phase
- 9.1. Description of the zones of growth
- 9.1.1. The initial solid is a single reactant
- 9.1.2. The initial solid reacts with another phase
- 9.2. Direction of the development of phase B during the growth
- 9.2.1. The initial solid is a single reactant
- 9.2.2. The initial solid reacts with another phase
- 9.3. Modes and models for growth
- 9.3.1. Modes of the growth of a crystal of B on support A
- 9.3.2. Modeling the growth
- 9.4. Relationship between the motion velocities of the interfaces and the chemical growth rate
- 9.4.1. Inward development of formed solid
- 9.4.2. Outward development of the formed solid
- 9.5. Methodology to model growth
- 9.5.1. Modeling the space function of growth
- 9.5.2. Modeling the reactivity of growth
- 9.6. Expressions of the space functions for the growth of a grain
- 9.6.1. Space functions in isotropic growth
- 9.6.2. Space functions in radial anisotropic growth
- 9.6.3. Introduction of a dimensionless time
- Chapter 10. Transformation by Surface Nucleation and Growth
- 10.1. Nucleation, growth, and experimental rate
- 10.2. One-process model with instantaneous nucleation and slow growth
- 10.2.1. Reaction of a single grain (or massive material)
- 10.2.2. Case of a monodispersed powder
- 10.2.3. Shapes of kinetic and rate curves
- 10.2.4. One-process model with slow nucleation and instantaneous growth
- 10.2.5. Reaction of a single grain
- 10.2.6. Reaction of a powder
- 10.3. Two-process models: nucleation and growth
- 10.3.1. General expression for the rate
- 10.3.2. Influence of the past on the transformation rate
- 10.4. Two-process model with surface nucleation-radialanisotropic growth
- 10.4.1. Reaction of a single grain
- 10.4.2. Construction of the model of evolution of a powder
- 10.4.3. Calculation of the free area (space function) for nucleation
- 10.4.4. Calculation of the rates and the fractional extents according to time
- 10.4.5. Dimensionless rate
- 10.4.6. Conclusion on the surface nucleation and radial anisotropic growth model
- 10.5. Two-process model with surface nucleation and isotropic growth
- 10.5.1. Qualitative approach
- 10.5.2. Quantitative approach
- 10.5.3. Modeling the evolution of a grain
- 10.5.4. Modeling the evolution of a collection of grains
- 10.5.5. Application to the spherical grains: model of Johnson-Mehl and Mampel
- 10.6. Non-isobaric and/or non-isothermal kinetics
- 10.6.1. One-process models
- 10.6.2. Two-process models
- 10.7. Powders with granular distributions
- 10.8. Return to the first and second kind of changes of laws
- 10.8.1. First kind of changes of laws
- 10.8.2. Second kind of changes of laws
- 10.9. Conclusion
- Chapter 11. Modeling and Experiments
- 11.1. The adequacy between the experimental conditions and modeling
- 11.2. Expressions of experimental speeds
- 11.2.1. Thermogravimetry
- 11.2.2. Microcalorimetry
- 11.2.3. Manometry
- 11.2.4. Measurement of the amounts of solids A with X-ray diffraction
- 11.2.5. Measurement of the amounts of the formed solid B
- 11.2.6. Thickness of the layer of a planar sample of B
- 11.2.7. Relationships between experimental speeds
- 11.3. Derivation of the kinetic curves
- 11.4. The experimental verification of the assumptions
- 11.4.1. The pseudo-steady state mode test
- 11.4.2. The test of the separable rate or the f? test
- 11.5. Determination of the morphological model for growth
- 11.5.1. Choice of the category of models: one-process or two-process model?
- 11.5.2. Determination of the model and its parameters
- 11.6. Calculations of the reactivity of growth and the specific frequency of nucleation
- 11.7. Variations of the kinetic properties with the intensive variables
- 11.7.1. Determination of the variation in the reactivity of growth starting from the morphological model
- 11.7.2. Direct determination of the variation in the reactivity of growth starting from the experiment
- 11.7.3. Comparison of the two obtained variations: new verification of the morphological model
- 11.8. Methodology of a study
- 11.8.1. Identification of the reaction
- 11.8.2. The separation of the models
- 11.8.3. Methodical approach of a study
- Chapter 12. Granular Coalescence
- 12.1. Qualitative description of the model
- 12.2. Morphological modeling
- 12.2.1. Assumptions
- 12.2.2. Geometry of the neck
- 12.2.3. Relation between the fractional extent and the radius x of the bridge
- 12.3. Structure of the coalescence mechanism
- 12.3.1. Transport phenomenon and groups of elementary steps
- 12.3.2. Various kinetic modes with rate-determining steps
- 12.3.3. Definition of the reactivity of coalescence
- 12.4. Determination of the space functions
- 12.4.1. Mode with an interface reaction as the rate-determining step
- 12.4.2. Modes with diffusion as rate-determining step
- 12.4.3. Recapitulation of the space functions
- 12.5. Rate constants and radius of curvature
- 12.6. Reactivity of coalescence of a solid with a single component
- 12.6.1. Case of vacancies diffusion in the solid
- 12.6.2. Case of gas diffusion
- 12.6.3. Summary of the reactivities
- 12.7. Extensions to the coalescence of solids with several components
- 12.7.1. Coalescence of anatase in the presence of water vapor
- 12.7.2. Coalescence of anatase in the presence of oxygen and hydrogen chloride with or without water vapor
- 12.7.3. Coalescence of ceria in presence of oxygen and water vapor
- 12.8. Relations between experiments and modeling
- 12.8.1. Experimental measurement of coalescence
- 12.8.2. Determination of the variations of the reactivity with intensive quantities
- 12.8.3. Relation between experiment and space function in the model of tangential spheres
- 12.9. Oswald ripening and reduction in porosity
- Chapter 13. Decomposition Reactions of Solids
- 13.1. Classifications of decomposition reactions
- 13.1.1. Classification according to the sign of the enthalpy
- 13.1.2. Classification according to the origin of the gas molecule
- 13.2. Extent measurement with the change of the mass
- 13.2.1. Stoichiometric solids
- 13.2.2. The produced solid is not stoichiometric
- 13.2.3. The initial solid is not stoichiometric
- 13.3. Observed experimental results
- 13.3.1. Rate-time and extent-time curves
- 13.3.2. Influences of the gas pressures
- 13.3.3. Influence of temperature
- 13.3.4. Non-isothermal decomposition reactions
- 13.4. Kinetics of growth in decomposition reactions of solids
- 13.4.1. Qualitative analysis of the growth
- 13.4.2. Basic growth mechanism with gaseous diffusion
- 13.4.3. Basic mechanism of growth with diffusions of defects
- 13.4.4. Smith-Topley's Effect
- 13.5. Nucleation in decomposition reactions of solids
- 13.5.1. Experimental approach of nucleation
- 13.5.2. Example of the dehydration of kaolinite
- 13.5.3. Nucleation and Smith-Topley's effect
- 13.6. Total kinetic curves
- 13.7. Influence of the granular distribution
- 13.8. Normal and abnormal growth
- Chapter 14. Reactions Between Solids
- 14.1. Classification of the reactions between solids
- 14.1.1. Simple addition reactions
- 14.1.2. Addition reactions involving decomposition
- 14.1.3. Addition reactions involving a redox reaction
- 14.1.4. Exchange reactions or double decompositions
- 14.2. The modeling assumptions
- 14.3. The experimental measure of the extent of the reactions
- 14.4. Reactivities of reactions between solids
- 14.4.1. Position of the problem and experimental approach
- 14.4.2. Structures of the reaction mechanism of growth
- 14.4.3. Expression of the reactivities, reaction of titanium dioxide with barium carbonate
- 14.5. Rates of the reactions between powders
- 14.5.1. Problems of designs
- 14.5.2. Rates of a two-grain level
- 14.5.3. Rate of a granular cell
- 14.5.4. Rates on the scale of the powder
- 14.6. Conclusion
- Chapter 15. Gas-Solid Reactions
- 15.1. Classification of gas-solid reactions
- 15.1.1. Class 1: synthesis reactions
- 15.1.2. Class 2: double-decomposition reactions
- 15.2. Pure metal gas reactions
- 15.2.1. Experimental data of oxidation of metals
- 15.2.2. Reaction zones and elementary reactions
- 15.2.3. Pure modes with interface rate determining step
- 15.2.4. Pure diffusion modes
- 15.2.5. Mixed modes
- 15.3. Growth process in the reduction of metallic oxides by hydrogen
- 15.3.1. Mechanism with diffusion of gases through the pores
- 15.3.2. Mechanisms with diffusion of defect in the formed solid phase
- 15.3.3. Conclusion about the reduction of oxides by hydrogen
- 15.3.4. Example of the reduction of a uranium oxide
- 15.4. Growth process of oxidation of metals by water vapor
- 15.4.1. General approach of mechanism
- 15.4.2. n-type formed oxide with interstitial cations
- 15.4.3. n-type formed oxide with anion vacancies
- 15.4.4. p-type formed oxide with cation vacancies
- 15.4.5. p-type formed oxide with interstitial anions
- Chapter 16. Transformations of Solid Solutions
- 16.1. General information on transformations of solid solutions
- 16.1.1. Various types of transformations of solid solutions
- 16.1.2. Variations of concentrations in solid solution
- 16.2. Oxidation of metal alloys
- 16.2.1. Selective oxidation of single-phase binary metal alloys
- 16.2.2. Internal oxidation of single-phase binary alloys
- 16.2.3. Oxidation of single-phase binary alloys with miscibility of formed oxides
- 16.2.4. Oxidation of single-phase binary alloys with formation of two superimposed oxide layers
- 16.3. Variations of the composition of a solid solution with gas formation
- 16.3.1. Fractional extent and rate
- 16.3.2. Spatial structure of the model
- 16.3.3. Pure diffusion mode
- 16.3.4. Example: variation of stoichiometry of an oxide by reaction with hydrogen
- 16.4. Superposition of a variation of stoichiometry and decomposition
- Chapter 17. Modeling of Mechanisms
- 17.1. Non-stoichiometry of iron oxide
- 17.1.1. Key words
- 17.1.2. Problem
- 17.1.3. Data
- 17.1.4. Solution
- 17.2. Stability of calcium carbonate
- 17.2.1. Key words
- 17.2.2. Problem
- 17.2.3. Data
- 17.2.4. Solution
- 17.3. Thermodynamics of a solid-solid reactions
- 17.3.1. Key words
- 17.3.2. Problem
- 17.3.3. Data
- 17.3.4. Solution
- 17.4. Hydrates of alumina
- 17.4.1. Key words
- 17.4.2. Problem
- 17.4.3. Data
- 17.4.4. Solution
- 17.5. Point defects in a metal sulfide
- 17.5.1. Key words
- 17.5.2. Problem
- 17.5.3. Data
- 17.5.4. Solution
- 17.6. Point defects of an alkaline bromide
- 17.6.1. Key words
- 17.6.2. Problem
- 17.6.3. Data
- 17.6.4. Solution
- 17.7. Diffusion of a metal into another metal
- 17.7.1. Key words
- 17.7.2. Problem
- 17.7.3. Data
- 17.7.4. Solution
- 17.8. Generation of atmospheres with very low pressures
- 17.8.1. Key words
- 17.8.2. Problem
- 17.8.3. Data
- 17.8.4. Solution
- Chapter 18. Mechanisms and Kinetic Laws
- 18.1 Coalescence of anatase grains
- 18.1.1. Key words
- 18.1.2. Problem
- 18.1.3. Data
- 18.1.4. Solution
- 18.2. Reaction of a cubic sample
- 18.2.1. Key words
- 18.2.2. Problem
- 18.2.3. Data
- 18.2.4. Solution
- 18.3. Anisotropic growth
- 18.3.1. Key words
- 18.3.2. Problem
- 18.3.3. Data
- 18.3.4. Solution
- 18.4. Gas-solid reaction with one-process model
- 18.4.1. Key words
- 18.4.2. Problem
- 18.4.3. Data
- 18.4.4. Solution
- 18.5. The direction of the development of a layer
- 18.5.1. Key words
- 18.5.2. Problem
- 18.5.3. Data
- 18.5.4. Solution
- 18.6. Mampel modeling by way of the point of inflection
- 18.6.1. Key words
- 18.6.2. Problem
- 18.6.3. Data
- 18.6.4. Solution
- 18.7. Nucleation in a reaction of dehydration
- 18.7.1. Key words
- 18.7.2. Problem
- 18.7.3. Data
- 18.7.4. Solution
- 18.8. Influence of particle size in nucleation-growth approach
- 18.8.1. Key words
- 18.8.2. Problem
- 18.8.3. Data
- 18.8.4. Solution
- 18.9. Decomposition with slow nucleation and slow anisotropic growth determined by diffusion
- 18.9.1. Key words
- 18.9.2. Problem
- 18.9.3. Data
- 18.9.4. Solution
- 19. Mechanisms and Reactivity
- 19.1. Competition oxidation - volatilization by TGA
- 19.1.1. Key words
- 19.1.2. Problem
- 19.1.3. Data
- 19.1.4. Solution
- 19.2. Controlled rate thermal analysis (CRTA)
- 19.2.1. Key words
- 19.2.2. Problem
- 19.2.3. Data
- 19.2.4. Solution
- 19.3. Sulfurization of a metal
- 19.3.1. Key words
- 19.3.2. Problem
- 19.3.3. Data
- 19.3.4. Solution
- 19.4. Oxidation of a metal and some of its alloys
- 19.4.1. Key words
- 19.4.2. Problem
- 19.4.3. Data
- 19.4.4. Solution
- 19.5. Reduction of octo-oxide of triuranium by dihydrogen
- 19.5.1. Key words
- 19.5.2. Problem
- 19.5.3. Data
- 19.5.4. Solution
- 19.6. Dehydration of kaolinite
- 19.6.1. Key words
- 19.6.2. Problem
- 19.6.3. Data
- 19.6.4. Solution
- 19.7. Decomposition of a carbonate of a metal
- 19.7.1. Key words
- 19.7.2. Problem
- 19.7.3. Data
- 19.7.4. Solution
- 19.8. Reaction between two solids
- 19.8.1. Key words
- 19.8.2. Problem
- 19.8.3. Data
- 19.8.4. Solution
- Appendix 1
- Appendix 2
- Appendix 3
- Appendix 4
- Appendix 5
- Appendix 6
- Appendix 7
- Appendix 8
- Appendix 9
- Appendix 10
- Appendix 11
- Bibliography
- Index
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Das Dateiformat PDF zeigt auf jeder Hardware eine Buchseite stets identisch an. Daher ist eine PDF auch für ein komplexes Layout geeignet, wie es bei Lehr- und Fachbüchern verwendet wird (Bilder, Tabellen, Spalten, Fußnoten). Bei kleinen Displays von E-Readern oder Smartphones sind PDF leider eher nervig, weil zu viel Scrollen notwendig ist.
Mit Adobe-DRM wird hier ein „harter” Kopierschutz verwendet. Wenn die notwendigen Voraussetzungen nicht vorliegen, können Sie das E-Book leider nicht öffnen. Daher müssen Sie bereits vor dem Download Ihre Lese-Hardware vorbereiten.
Bitte beachten Sie: Wir empfehlen Ihnen unbedingt nach Installation der Lese-Software diese mit Ihrer persönlichen Adobe-ID zu autorisieren!
Weitere Informationen finden Sie in unserer E-Book Hilfe.