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 Akimoto, Hajime, author.
 Hoboken, NJ : Wiley, 2020.
 Description
 Book — 1 online resource
 Summary

 Historical background of atmospheric secondary aerosol research
 Fundamentals of multiphase chemical reactions
 Gasphase reactions related to secondary organic aerosols
 Aqueousphase reactions related to secondary organic aerosols
 Heterogeneous oxidation reactions at organic aerosol surfaces
 Reactions at the airwater and airsolid particle interface
 Atmospheric new particle formation and cloud condensation nuclei
 Field observation of secondary organic aerosols (SOA).
(source: Nielsen Book Data)
2. Atmospheric reaction chemistry [2016]
 Taiki hanno kagaku. English
 Akimoto, Hajime, author.
 Tokyo : Springer, 2016.
 Description
 Book — 1 online resource (xvi, 433 pages) : illustrations Digital: text file; PDF.
 Summary

 Introduction to Atmospheric Chemistry
 Dawn of Modern Chemistry and Chemistry of Atmosphere
 Chemistry of Atmosphere to Atmospheric Chemistry
 Textbooks of Atmospheric Chemistry
 Fundamentals of Chemical Reactions
 Photochemistry and Photolytic Reactions
 Bimolecular Reactions
 Termolecular and Unimolecular Reactions
 Multiphase Heterogeneous Reactions
 Solar Radiation and Actinic Flux
 Solar Spectrum Outside of the Atmosphere
 Attenuation of Solar Radiation by N2, O2 and O3 in the Atmosphere
 Solar Zenith Angle and Air Mass
 Scattering by Atmospheric Molecule and Particles, and Surface Albedo
 Actinic Flux and Photolysis Rates
 Absorption Spectrum of Atmospheric Molecules, and Photolysis Reactions
 Solar Spectrum in the Troposphere and the Stratosphere
 Photolysis in the Troposphere
 Photolysis in the Stratosphere
 Photolysis of Inorganic Halogen Compounds
 Homogeneous Elementary Reactions in the Atmosphere and Rate Constants
 Reactions of O(3P) and O(1D) Atoms
 Reactions of OH Radicals
 Reactions of HO2 and CH3O2 Radicals
 Reactions of O3
 Reactions of NO3 Radicals
 Reactions of Cl Atoms and ClO Radicals
 Heterogeneous Reactions in the Atmosphere and Uptake Coefficients
 Uptake to Water Droplet
 Uptake to Sea Salt and Alkali Halides, and Surface Reactions
 Uptake to Soil and Mineral Dusts, and Surface Reactions
 Uptake to Soot, and Surface Reactions
 Surface Reactions on Polar Stratospheric Clouds (PSC)
 Tropospheric Reaction Chemistry
 HOx Chain Reactions and Oxidation of Methane in the Natural Atmosphere
 Oxidation Reactions of VOC in the Polluted Atmosphere
 Production and Loss of O3 by HOx Chain Reactions
 Measurements of OH and HO2 Radicals in the Atmosphere, and Validation of Models
 Tropospheric Halogen Chemistry
 Tropospheric Sulfur Chemistry
 "Discovery" of OH Radical Chain Mechanism
 Smog Chamber
 Stratospheric Reaction Chemistry
 Pure Oxygen Atmosphere and Ozone Layer
 Ozone Loss Cycles by Trace Gases
 Gas Phase Chain Reactions and Ozone Destruction by CFC
 Multiphase Reactions on PSC and Ozone Hole
 Stratospheric Sulfur Chemistry.
3. Highperformance systems biology and associated combinatorial scientific computing problems [2008]
 Alber, David.
 [Golden, Colo.] : National Renewable Energy Laboratory, [2008]
 Description
 Book — 25 unnumbered slides : digital, PDF file.
 Alexander D. Ryabov, author.
 Newcastle upon Tyne : Cambridge Scholars Publishing, 2021
 Description
 Book — 1 online resource
 Altkorn, Robert Ira.
 1984.
 Description
 Book — vii, 181 leaves, bound : ill. ; 28 cm.
 Online
SAL3 (offcampus storage), Special Collections
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3781 1984 A  Available 
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6. Reaction kinetics and unit operations [1959]
 American Institute of Chemical Engineers.
 New York : American Institute of Chemical Engineers, 1959.
 Description
 Book — 227 p. : ill ; 28 cm.
 Online
SAL3 (offcampus storage)
SAL3 (offcampus storage)  Status 

See linked record to request items bound together  
660.5 .C514S NO.25  Available 
 Ancheyta Juárez, Jorge, author.
 Hoboken, NJ : John Wiley & Sons, Inc., 2017.
 Description
 Book — 1 online resource.
 Summary

 Preface
 Chapter 1. Fundamentals of chemical reaction kinetics 1.1. Concepts of stoichiometry 1.1.1. Stoichiometric number and coefficient 1.1.2. Molecularity 1.1.3. Reaction extent 1.1.4. Molar conversion 1.1.5. Types of feed composition in a chemical reaction 1.1.6. Limiting reactant 1.1.7. Molar balance in a chemical reaction 1.1.8. Relationship between conversion and physical properties of the reacting system 1.2. Reacting systems 1.2.1. Mole fraction, weight fraction and molar concentration 1.2.2. Partial pressure 1.2.3. Isothermal systems at constant density 1.2.4. Isothermal systems at variable density 1.2.5. General case of reacting systems 1.2.6. Kinetic point of view of the chemical equilibrium 1.3. Concepts of chemical kinetics 1.3.1. Rate of homogeneous reactions 1.3.2. Power law 1.3.3. Elemental and nonelemental reactions 1.3.4. Comments on the concepts of molecularity and reaction order 1.3.5. Dependency of k with temperature 1.4. Description of ideal reactors 1.4.1. Batch reactor 1.4.2. Continuous reactors
 Chapter 2. Irreversible reactions of one component 2.1. Integral method 2.1.1. Reactions of zero order 2.1.2. Reactions of first order 2.1.3. Reaction of second order 2.1.4. Reactions of nth order 2.2. Differential method 2.2.1. Numerical differentiation 2.2.2. Graphical differentiation 2.3. Method of total pressure 2.3.1. Reactions of zero order 2.3.2. Reactions of first order 2.3.3. Reactions of second order 2.3.4. Reactions of nth order 2.3.5. Differential method with data of total pressure 2.4. Method of the halflife time 2.4.1. Reactions of zero order 2.4.2. Reactions of first order 2.4.3. Reaction of second order 2.4.4. Reaction of nth order 2.4.5. Direct method to calculate k and n with data of t1/2 2.4.6. Extension of the method of halflife time (t1/2) to any fractional life time (t1/m) 2.4.7. Calculation of activation energy with data of halflife time 2.4.8. Some observations of the method of halflife time
 Chapter 3. Irreversible reactions with two or three components 3.1. Irreversible reactions with two components 3.1.1. Integral method 3.1.2. Differential method 3.1.3. Method of initial reaction rates 3.2. Irreversible reactions between three components
 Chapter 4. Reversible reactions 4.1. Reversible reactions of first order 4.2. Reversible reactions of second order 4.3. Reversible reactions with combined orders
 Chapter 5. Complex reactions 5.1. Yield and selectivity 5.2. Simultaneous or parallel irreversible reactions 5.2.1. Simultaneous reactions with the same order 5.2.2. Simultaneous reactions with combined orders 5.3. Consecutive or in series irreversible reactions 5.3.1. Consecutive reactions with the same order 5.3.2. Consecutive reactions with combined orders
 Chapter 6. Special topics in kinetic modeling 6.1. Data reconciliation 6.1.1. Data reconciliation method 6.1.2. Results and discussion 6.1.3. Conclusions 6.2. Methodology for sensitivity analysis of parameters 6.2.1. Description of the method 6.2.2. Results and discussion 6.2.3. Conclusions 6.3. Methods for determining rate coefficients in enzymatic catalyzed reactions 6.3.1. The model of MichaelisMenten 6.3.2. Methods to determine the rate coefficients of the MichaelisMenten equation 6.3.3. Application of the methods 6.3.4. Discussion of results 6.3.5. Conclusions 6.4. A simple method for estimating gasoline, gas and coke yields in FCC processes 6.4.1. Introduction 6.4.2. Methodology 6.4.3. Results and discussion 6.4.4 Conclusions 6.5. Estimation of activation energies during hydrodesulfurization of middle distillates 6.5.1. Introduction 6.5.2. Experimental 6.5.3. Results and discussion 6.5.4. Conclusions Problems References Nomenclature.
 (source: Nielsen Book Data)
 About the Author xi Preface xiii 1 Fundamentals of Chemical Reaction Kinetics 1 1.1 Concepts of Stoichiometry 1 1.1.1 Stoichiometric Number and Coefficient 1 1.1.2 Molecularity 2 1.1.3 Reaction Extent 3 1.1.4 Molar Conversion 4 1.1.5 Types of Feed Composition in a Chemical Reaction 5 1.1.6 Limiting Reactant 6 1.1.7 Molar Balance in a Chemical Reaction 7 1.1.8 Relationship between Conversion and Physical Properties of the Reacting System 8 1.2 Reacting Systems 11 1.2.1 Mole Fraction, Weight Fraction and Molar Concentration 11 1.2.2 Partial Pressure 13 1.2.3 Isothermal Systems at Constant Density 13 1.2.3.1 Relationship between Partial Pressure (pA) and Conversion (xA) 16 1.2.3.2 Relationship between Partial Pressure (pA) and Total Pressure (P) 16 1.2.3.3 Relationship between Molar Concentration (CA) and Total Pressure (P) 16 1.2.4 Isothermal Systems at Variable Density 18 1.2.5 General Case of Reacting Systems 22 1.2.6 Kinetic Point of View of the Chemical Equilibrium 22 1.3 Concepts of Chemical Kinetics 24 1.3.1 Rate of Homogeneous Reactions 24 1.3.2 Power Law 26 1.3.2.1 Relationship between kp and kc 27 1.3.2.2 Units of kc and kp 27 1.3.3 Elemental and Nonelemental Reactions 29 1.3.4 Comments on the Concepts of Molecularity and Reaction Order 30 1.3.5 Dependency of k with Temperature 30 1.3.5.1 Arrhenius Equation 30 1.3.5.2 Frequency Factor and Activation Energy 32 1.3.5.3 Evaluation of the Parameters of the Arrhenius Equation 32 1.3.5.4 Modified Arrhenius Equation 42 1.4 Description of Ideal Reactors 43 1.4.1 Batch Reactors 43 1.4.1.1 Modes of Operation 44 1.4.1.2 Data Collection 46 1.4.1.3 Mass Balance 48 1.4.2 Continuous Reactors 49 1.4.2.1 SpaceTime and SpaceVelocity 50 1.4.2.2 Plug Flow Reactor 50 1.4.2.3 Continuous Stirred Tank Reactor 52 2 Irreversible Reactions of One Component 55 2.1 Integral Method 56 2.1.1 Reactions of Zero Order 58 2.1.2 Reactions of the First Order 59 2.1.3 Reaction of the Second Order 61 2.1.4 Reactions of the nth Order 64 2.2 Differential Method 69 2.2.1 Numerical Differentiation 71 2.2.1.1 Method of Approaching the Derivatives ( dCA/dt) to ( CA/ t) or (dxA/dt) to ( xA/ t) 71 2.2.1.2 Method of Finite Differences 72 2.2.1.3 Method of a Polynomial of the nth Order 74 2.2.2 Graphical Differentiation 74 2.2.2.1 Method of Area Compensation 74 2.2.2.2 Method of Approaching the Derivative ( dCA/dt) to ( CA/ t) 76 2.2.2.3 Method of Finite Differences 77 2.2.2.4 Method of a Polynomial of the nth Order 78 2.2.2.5 Method of Area Compensation 80 2.2.2.6 Summary of Results 82 2.3 Method of Total Pressure 83 2.3.1 Reactions of Zero Order 84 2.3.2 Reactions of the First Order 85 2.3.3 Reactions of the Second Order 85 2.3.4 Reactions of the nth Order 86 2.3.5 Differential Method with Data of Total Pressure 88 2.4 Method of the HalfLife Time 91 2.4.1 Reactions of Zero Order 92 2.4.2 Reactions of the First Order 92 2.4.3 Reaction of the Second Order 93 2.4.4 Reaction of the nth Order 93 2.4.5 Direct Method to Calculate k and n with Data of t1/2 95 2.4.6 Extension of the Method of HalfLife Time (t1/2) to Any Fractional Life Time (t1/m) 97 2.4.7 Calculation of Activation Energy with Data of HalfLife Time 97 2.4.8 Some Observations of the Method of HalfLife Time 99 2.4.8.1 Calculation of n with Two Data of t1/2Measured with Different CAo 99 2.4.8.2 Generalization of the Method of HalfLife Time for Any Reaction Order 101 3 Irreversible Reactions with Two or Three Components 103 3.1 Irreversible Reactions with Two Components 103 3.1.1 Integral Method 103 3.1.1.1 Method of Stoichiometric Feed Composition 104 3.1.1.2 Method of Nonstoichiometric Feed Composition 109 3.1.1.3 Method of a Reactant in Excess 117 3.1.2 Differential Method 120 3.1.2.1 Stoichiometric Feed Composition 120 3.1.2.2 Feed Composition with a Reactant in Excess 120 3.1.2.3 Nonstoichiometric Feed Compositions 121 3.1.3 Method of Initial Reaction Rates 123 3.2 Irreversible Reactions between Three Components 127 3.2.1 Case
 1: Stoichiometric Feed Composition 127 3.2.2 Case
 2: Nonstoichiometric Feed Composition 129 3.2.3 Case
 3: Feed Composition with One Reactant in Excess 130 3.2.4 Case
 4: Feed Composition with Two Reactants in Excess 131 4 Reversible Reactions 135 4.1 Reversible Reactions of First Order 135 4.2 Reversible Reactions of Second Order 139 4.3 Reversible Reactions with Combined Orders 146 5 Complex Reactions 153 5.1 Yield and Selectivity 153 5.2 Simultaneous or Parallel Irreversible Reactions 155 5.2.1 Simultaneous Reactions with the Same Order 155 5.2.1.1 Case
 1: Reactions with Only One Reactant 155 5.2.1.2 Case
 2: Reactions with Two Reactants 161 5.2.2 Simultaneous Reactions with Combined Orders 163 5.2.2.1 Integral Method 165 5.2.2.2 Differential Method 166 5.3 Consecutive or InSeries Irreversible Reactions 167 5.3.1 Consecutive Reactions with the Same Order 167 5.3.1.1 Calculation of CR max and t 171 5.3.1.2 Calculation of CR max and t for k1= k2 172 5.3.2 Consecutive Reactions with Combined Orders 174 6 Special Topics in Kinetic Modelling 179 6.1 Data Reconciliation 180 6.1.1 Data Reconciliation Method 181 6.1.2 Results and Discussion 182 6.1.2.1 Source of Data 182 6.1.2.2 Global Mass Balances 185 6.1.2.3 Outlier Determination 187 6.1.2.4 Data Reconciliation 187 6.1.2.5 Analysis of Results 189 6.1.3 Conclusions 195 6.2 Methodology for Sensitivity Analysis of Parameters 196 6.2.1 Description of the Method 198 6.2.1.1 Initialization of Parameters 199 6.2.1.2 Nonlinear Parameter Estimation 201 6.2.1.3 Sensitivity Analysis 201 6.2.1.4 Residual Analysis 202 6.2.2 Results and Discussion 202 6.2.2.1 Experimental Data and the Reaction Rate Model from the Literature 202 6.2.2.2 Initialization of Parameters 204 6.2.2.3 Results of Nonlinear Estimation 206 6.2.2.4 Sensitivity Analysis 207 6.2.2.5 Analysis of Residuals 210 6.2.3 Conclusions 210 6.3 Methods for Determining Rate Coefficients in Enzymatic Catalysed Reactions 211 6.3.1 The MichaelisMenten Model 213 6.3.1.1 Origin 213 6.3.1.2 Development of the Model 213 6.3.1.3 Importance of Vmax and Km 214 6.3.2 Methods to Determine the Rate Coefficients of the MichaelisMenten Equation 214 6.3.2.1 Linear Regression 214 6.3.2.2 Graphic Method 215 6.3.2.3 Integral Method 215 6.3.2.4 Nonlinear Regression 216 6.3.3 Application of the Methods 217 6.3.3.1 Experimental Data 217 6.3.3.2 Calculation of Kinetic Parameters 220 6.3.4 Discussion of Results 222 6.3.5 Conclusions 225 6.4 A Simple Method for Estimating Gasoline, Gas and Coke Yields in FCC Processes 226 6.4.1 Introduction 226 6.4.2 Methodology 227 6.4.2.1 Choosing the Kinetic Models 227 6.4.2.2 Reaction Kinetics 228 6.4.2.3 Estimation of Kinetic Parameters 229 6.4.2.4 Evaluation of Products Yields 230 6.4.2.5 Advantages and Limitations of the Methodology 230 6.4.3 Results and Discussion 231 6.4.4 Conclusions 234 6.5 Estimation of Activation Energies during Hydrodesulphurization of Middle Distillates 234 6.5.1 Introduction 234 6.5.2 Experiments 235 6.5.3 Results and Discussion 236 6.5.3.1 Experimental Results 236 6.5.3.2 Estimation of Kinetic Parameters 237 6.5.3.3 Effect of Feed Properties on Kinetic Parameters 240 6.5.4 Conclusions 241 Problems 243 Nomenclature 273 References 277 Index 283.
 (source: Nielsen Book Data)
(source: Nielsen Book Data)
 Ancheyta Juárez, Jorge, author.
 Hoboken, NJ : John Wiley & Sons, Inc., 2017.
 Description
 Book — 1 online resource
 Summary

 About the Author xi Preface xiii 1 Fundamentals of Chemical Reaction Kinetics 1 1.1 Concepts of Stoichiometry 1 1.1.1 Stoichiometric Number and Coefficient 1 1.1.2 Molecularity 2 1.1.3 Reaction Extent 3 1.1.4 Molar Conversion 4 1.1.5 Types of Feed Composition in a Chemical Reaction 5 1.1.6 Limiting Reactant 6 1.1.7 Molar Balance in a Chemical Reaction 7 1.1.8 Relationship between Conversion and Physical Properties of the Reacting System 8 1.2 Reacting Systems 11 1.2.1 Mole Fraction, Weight Fraction and Molar Concentration 11 1.2.2 Partial Pressure 13 1.2.3 Isothermal Systems at Constant Density 13 1.2.3.1 Relationship between Partial Pressure (pA) and Conversion (xA) 16 1.2.3.2 Relationship between Partial Pressure (pA) and Total Pressure (P) 16 1.2.3.3 Relationship between Molar Concentration (CA) and Total Pressure (P) 16 1.2.4 Isothermal Systems at Variable Density 18 1.2.5 General Case of Reacting Systems 22 1.2.6 Kinetic Point of View of the Chemical Equilibrium 22 1.3 Concepts of Chemical Kinetics 24 1.3.1 Rate of Homogeneous Reactions 24 1.3.2 Power Law 26 1.3.2.1 Relationship between kp and kc 27 1.3.2.2 Units of kc and kp 27 1.3.3 Elemental and Nonelemental Reactions 29 1.3.4 Comments on the Concepts of Molecularity and Reaction Order 30 1.3.5 Dependency of k with Temperature 30 1.3.5.1 Arrhenius Equation 30 1.3.5.2 Frequency Factor and Activation Energy 32 1.3.5.3 Evaluation of the Parameters of the Arrhenius Equation 32 1.3.5.4 Modified Arrhenius Equation 42 1.4 Description of Ideal Reactors 43 1.4.1 Batch Reactors 43 1.4.1.1 Modes of Operation 44 1.4.1.2 Data Collection 46 1.4.1.3 Mass Balance 48 1.4.2 Continuous Reactors 49 1.4.2.1 SpaceTime and SpaceVelocity 50 1.4.2.2 Plug Flow Reactor 50 1.4.2.3 Continuous Stirred Tank Reactor 52 2 Irreversible Reactions of One Component 55 2.1 Integral Method 56 2.1.1 Reactions of Zero Order 58 2.1.2 Reactions of the First Order 59 2.1.3 Reaction of the Second Order 61 2.1.4 Reactions of the nth Order 64 2.2 Differential Method 69 2.2.1 Numerical Differentiation 71 2.2.1.1 Method of Approaching the Derivatives ( dCA/dt) to ( CA/ t) or (dxA/dt) to ( xA/ t) 71 2.2.1.2 Method of Finite Differences 72 2.2.1.3 Method of a Polynomial of the nth Order 74 2.2.2 Graphical Differentiation 74 2.2.2.1 Method of Area Compensation 74 2.2.2.2 Method of Approaching the Derivative ( dCA/dt) to ( CA/ t) 76 2.2.2.3 Method of Finite Differences 77 2.2.2.4 Method of a Polynomial of the nth Order 78 2.2.2.5 Method of Area Compensation 80 2.2.2.6 Summary of Results 82 2.3 Method of Total Pressure 83 2.3.1 Reactions of Zero Order 84 2.3.2 Reactions of the First Order 85 2.3.3 Reactions of the Second Order 85 2.3.4 Reactions of the nth Order 86 2.3.5 Differential Method with Data of Total Pressure 88 2.4 Method of the HalfLife Time 91 2.4.1 Reactions of Zero Order 92 2.4.2 Reactions of the First Order 92 2.4.3 Reaction of the Second Order 93 2.4.4 Reaction of the nth Order 93 2.4.5 Direct Method to Calculate k and n with Data of t1/2 95 2.4.6 Extension of the Method of HalfLife Time (t1/2) to Any Fractional Life Time (t1/m) 97 2.4.7 Calculation of Activation Energy with Data of HalfLife Time 97 2.4.8 Some Observations of the Method of HalfLife Time 99 2.4.8.1 Calculation of n with Two Data of t1/2Measured with Different CAo 99 2.4.8.2 Generalization of the Method of HalfLife Time for Any Reaction Order 101 3 Irreversible Reactions with Two or Three Components 103 3.1 Irreversible Reactions with Two Components 103 3.1.1 Integral Method 103 3.1.1.1 Method of Stoichiometric Feed Composition 104 3.1.1.2 Method of Nonstoichiometric Feed Composition 109 3.1.1.3 Method of a Reactant in Excess 117 3.1.2 Differential Method 120 3.1.2.1 Stoichiometric Feed Composition 120 3.1.2.2 Feed Composition with a Reactant in Excess 120 3.1.2.3 Nonstoichiometric Feed Compositions 121 3.1.3 Method of Initial Reaction Rates 123 3.2 Irreversible Reactions between Three Components 127 3.2.1 Case
 1: Stoichiometric Feed Composition 127 3.2.2 Case
 2: Nonstoichiometric Feed Composition 129 3.2.3 Case
 3: Feed Composition with One Reactant in Excess 130 3.2.4 Case
 4: Feed Composition with Two Reactants in Excess 131 4 Reversible Reactions 135 4.1 Reversible Reactions of First Order 135 4.2 Reversible Reactions of Second Order 139 4.3 Reversible Reactions with Combined Orders 146 5 Complex Reactions 153 5.1 Yield and Selectivity 153 5.2 Simultaneous or Parallel Irreversible Reactions 155 5.2.1 Simultaneous Reactions with the Same Order 155 5.2.1.1 Case
 1: Reactions with Only One Reactant 155 5.2.1.2 Case
 2: Reactions with Two Reactants 161 5.2.2 Simultaneous Reactions with Combined Orders 163 5.2.2.1 Integral Method 165 5.2.2.2 Differential Method 166 5.3 Consecutive or InSeries Irreversible Reactions 167 5.3.1 Consecutive Reactions with the Same Order 167 5.3.1.1 Calculation of CR max and t 171 5.3.1.2 Calculation of CR max and t for k1= k2 172 5.3.2 Consecutive Reactions with Combined Orders 174 6 Special Topics in Kinetic Modelling 179 6.1 Data Reconciliation 180 6.1.1 Data Reconciliation Method 181 6.1.2 Results and Discussion 182 6.1.2.1 Source of Data 182 6.1.2.2 Global Mass Balances 185 6.1.2.3 Outlier Determination 187 6.1.2.4 Data Reconciliation 187 6.1.2.5 Analysis of Results 189 6.1.3 Conclusions 195 6.2 Methodology for Sensitivity Analysis of Parameters 196 6.2.1 Description of the Method 198 6.2.1.1 Initialization of Parameters 199 6.2.1.2 Nonlinear Parameter Estimation 201 6.2.1.3 Sensitivity Analysis 201 6.2.1.4 Residual Analysis 202 6.2.2 Results and Discussion 202 6.2.2.1 Experimental Data and the Reaction Rate Model from the Literature 202 6.2.2.2 Initialization of Parameters 204 6.2.2.3 Results of Nonlinear Estimation 206 6.2.2.4 Sensitivity Analysis 207 6.2.2.5 Analysis of Residuals 210 6.2.3 Conclusions 210 6.3 Methods for Determining Rate Coefficients in Enzymatic Catalysed Reactions 211 6.3.1 The MichaelisMenten Model 213 6.3.1.1 Origin 213 6.3.1.2 Development of the Model 213 6.3.1.3 Importance of Vmax and Km 214 6.3.2 Methods to Determine the Rate Coefficients of the MichaelisMenten Equation 214 6.3.2.1 Linear Regression 214 6.3.2.2 Graphic Method 215 6.3.2.3 Integral Method 215 6.3.2.4 Nonlinear Regression 216 6.3.3 Application of the Methods 217 6.3.3.1 Experimental Data 217 6.3.3.2 Calculation of Kinetic Parameters 220 6.3.4 Discussion of Results 222 6.3.5 Conclusions 225 6.4 A Simple Method for Estimating Gasoline, Gas and Coke Yields in FCC Processes 226 6.4.1 Introduction 226 6.4.2 Methodology 227 6.4.2.1 Choosing the Kinetic Models 227 6.4.2.2 Reaction Kinetics 228 6.4.2.3 Estimation of Kinetic Parameters 229 6.4.2.4 Evaluation of Products Yields 230 6.4.2.5 Advantages and Limitations of the Methodology 230 6.4.3 Results and Discussion 231 6.4.4 Conclusions 234 6.5 Estimation of Activation Energies during Hydrodesulphurization of Middle Distillates 234 6.5.1 Introduction 234 6.5.2 Experiments 235 6.5.3 Results and Discussion 236 6.5.3.1 Experimental Results 236 6.5.3.2 Estimation of Kinetic Parameters 237 6.5.3.3 Effect of Feed Properties on Kinetic Parameters 240 6.5.4 Conclusions 241 Problems 243 Nomenclature 273 References 277 Index 283.
 (source: Nielsen Book Data)
 Preface
 Chapter 1. Fundamentals of chemical reaction kinetics 1.1. Concepts of stoichiometry 1.1.1. Stoichiometric number and coefficient 1.1.2. Molecularity 1.1.3. Reaction extent 1.1.4. Molar conversion 1.1.5. Types of feed composition in a chemical reaction 1.1.6. Limiting reactant 1.1.7. Molar balance in a chemical reaction 1.1.8. Relationship between conversion and physical properties of the reacting system 1.2. Reacting systems 1.2.1. Mole fraction, weight fraction and molar concentration 1.2.2. Partial pressure 1.2.3. Isothermal systems at constant density 1.2.4. Isothermal systems at variable density 1.2.5. General case of reacting systems 1.2.6. Kinetic point of view of the chemical equilibrium 1.3. Concepts of chemical kinetics 1.3.1. Rate of homogeneous reactions 1.3.2. Power law 1.3.3. Elemental and nonelemental reactions 1.3.4. Comments on the concepts of molecularity and reaction order 1.3.5. Dependency of k with temperature 1.4. Description of ideal reactors 1.4.1. Batch reactor 1.4.2. Continuous reactors
 Chapter 2. Irreversible reactions of one component 2.1. Integral method 2.1.1. Reactions of zero order 2.1.2. Reactions of first order 2.1.3. Reaction of second order 2.1.4. Reactions of nth order 2.2. Differential method 2.2.1. Numerical differentiation 2.2.2. Graphical differentiation 2.3. Method of total pressure 2.3.1. Reactions of zero order 2.3.2. Reactions of first order 2.3.3. Reactions of second order 2.3.4. Reactions of nth order 2.3.5. Differential method with data of total pressure 2.4. Method of the halflife time 2.4.1. Reactions of zero order 2.4.2. Reactions of first order 2.4.3. Reaction of second order 2.4.4. Reaction of nth order 2.4.5. Direct method to calculate k and n with data of t1/2 2.4.6. Extension of the method of halflife time (t1/2) to any fractional life time (t1/m) 2.4.7. Calculation of activation energy with data of halflife time 2.4.8. Some observations of the method of halflife time
 Chapter 3. Irreversible reactions with two or three components 3.1. Irreversible reactions with two components 3.1.1. Integral method 3.1.2. Differential method 3.1.3. Method of initial reaction rates 3.2. Irreversible reactions between three components
 Chapter 4. Reversible reactions 4.1. Reversible reactions of first order 4.2. Reversible reactions of second order 4.3. Reversible reactions with combined orders
 Chapter 5. Complex reactions 5.1. Yield and selectivity 5.2. Simultaneous or parallel irreversible reactions 5.2.1. Simultaneous reactions with the same order 5.2.2. Simultaneous reactions with combined orders 5.3. Consecutive or in series irreversible reactions 5.3.1. Consecutive reactions with the same order 5.3.2. Consecutive reactions with combined orders
 Chapter 6. Special topics in kinetic modeling 6.1. Data reconciliation 6.1.1. Data reconciliation method 6.1.2. Results and discussion 6.1.3. Conclusions 6.2. Methodology for sensitivity analysis of parameters 6.2.1. Description of the method 6.2.2. Results and discussion 6.2.3. Conclusions 6.3. Methods for determining rate coefficients in enzymatic catalyzed reactions 6.3.1. The model of MichaelisMenten 6.3.2. Methods to determine the rate coefficients of the MichaelisMenten equation 6.3.3. Application of the methods 6.3.4. Discussion of results 6.3.5. Conclusions 6.4. A simple method for estimating gasoline, gas and coke yields in FCC processes 6.4.1. Introduction 6.4.2. Methodology 6.4.3. Results and discussion 6.4.4 Conclusions 6.5. Estimation of activation energies during hydrodesulfurization of middle distillates 6.5.1. Introduction 6.5.2. Experimental 6.5.3. Results and discussion 6.5.4. Conclusions Problems References Nomenclature.
 (source: Nielsen Book Data)
(source: Nielsen Book Data)
 Online
9. The effect of sodium carbonate additive on the reaction of S0 ?/0 ?mixtures with carbonate rocks [1979]
 Argonne National Laboratory. Chemical Engineering Division.
 Argonne, Ill. : Dept. of Energy, [Office of Energy Research], Argonne National Laboratory ; Springfield, Va. : for sale by the National Technical Information Service, 1979
 Description
 Book — v, 31 p. : ill. ; 28 cm.
 Online
Green Library
Green Library  Status 

Find it US Federal Documents  
E 1.28:ANL/CEN/FE7911  Unknown 
10. Chemical reactions of metal powders with organic and inorganic liquids during ball milling [1975]
 Arias, Alan.
 Washington, D.C. : National Aeronautics and Space Administration ; [Springfield, Va. : For sale by the National Technical Information Service], 1975.
 Description
 Book — 26 p. : ill. ; 27 cm.
SAL3 (offcampus storage)
SAL3 (offcampus storage)  Status 

See linked record to request items bound together  
NASA TN D8015  Available 
 Ashmore, Philip George.
 London, Butterworths, 1963.
 Description
 Book — xi, 374 p. illus., diagrs. 26 cm.
 Online
SAL3 (offcampus storage)
SAL3 (offcampus storage)  Status 

Stacks  Request (opens in new tab) 
QD501 .A82  Available 
 AsiaPacific Chemical Reaction Engineering Symposium (4th : 2005 : Kyŏngjusi, Korea)
 1st ed.  Amsterdam : Elsevier, 2006.
 Description
 Book — xxvii, 896 p. : ill.
 AsiaPacific Chemical Reaction Engineering Symposium (4th : 2005 : Kyŏngjusi, Korea)
 Amsterdam ; Elsevier, 2006. Oxford :
 Description
 Book — xxvii, 896 p. : ill. ; 25 cm.
 Summary

 Plenary Lectures Invited Lectures Biological and Biochemical Reaction Engineering Catalysis and Catalytic Reaction Engineering Chemical Reaction Engineering in Microelectronics Environmental Reaction Engineering Fluidized Bed and Multiphase Reactors Fuel Cells and Electrochemical Reaction Engineering MicroReaction Technology Modeling, Simulation and Control of Chemical Reactors Nano Materials Synthesis and Application Novel Reactors and Processes Polymer Reaction Engineering.
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(source: Nielsen Book Data)
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TP155.7 .A85 2005  Available 
 Atkin, Lawrence, 1908
 New York : New York University, 1946.
 Description
 Book — 18 p. : ill ; 23 cm.
 Online
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QP603 .S9 A85 1945  Available 
15. Atoms, electrons, and change [1990]
 Atkins, P. W. (Peter William), 1940
 New York : Scientific American Library, c1990.
 Description
 Book — 242 p.
 Summary

A century and a half ago the pioneering physicist and chemist Michael Faraday delivered a celebrated series of lectures that attempted to explain the inner workings of matter through the chemical history of a candle. "There is no better, there is no more open door by which you can enter into the study of natural philosophy", Faraday told his audience. Now the distinguished chemist P.W. Atkins follows in Faraday's footsteps, using his predecessor's deceptively simple theme to show how far we have come in understanding the remarkable chemical reactions that govern everything from how candles burn to how life functions. While Faraday could say little more than that a chemical reaction changes a substance's appearance and properties, chemists today understand reactions in terms of the rearrangement of atoms and electrons. Atkins  tracing the course of a carbon atom released by a flaming candle  explores the complex forces that operate at the atomic and sub atomic levels to drive these rearrangements.
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QD461 .A84 1990  Available 
16. Reactions : the private life of atoms [2011]
 Atkins, P. W. (Peter William), 1940
 Oxford : OUP Oxford, 2011.
 Description
 Book — 1 online resource (viii, 191 pages) : color illustrations
 Summary

 PREFACE
 A PRELIMINARY COMMENT: WATER
 THE BASIC TOOLS
 ASSEMBLING THE WORKSHOP
 BUILDING BY DESIGN
 A RETROSPECTIVE: BRINGING IT ALL TOGETHER
 GLOSSARY.
 (source: Nielsen Book Data)
(source: Nielsen Book Data)
17. Reactions : the private life of atoms [2011]
 Atkins, P. W. (Peter William), 1940
 Oxford ; New York : Oxford University Press, 2011.
 Description
 Book — viii, 191 p. : col. ill. ; 23 cm.
 Summary

 PREFACE
 A PRELIMINARY COMMENT: WATER
 THE BASIC TOOLS
 ASSEMBLING THE WORKSHOP
 BUILDING BY DESIGN
 A RETROSPECTIVE: BRINGING IT ALL TOGETHER
 GLOSSARY.
 (source: Nielsen Book Data)
(source: Nielsen Book Data)
 Online
Science Library (Li and Ma)
Science Library (Li and Ma)  Status 

Stacks  
QD501 .A86 2011  Unknown 
 Bai, J. M.
 Norfolk, Va. : Old Dominion University Research Foundation ; [Washington, DC : National Aeronautics and Space Administration ; Springfield, Va. : National Technical Information Service, distributor, 1987]
 Description
 Book — 1 v.
 Online
Green Library
Green Library  Status 

Find it US Federal Documents  
NAS 1.26:180978  Unknown 
19. Selected elementary reactions [1976]
 Bamford, C. H.
 Amsterdam, New York, Elsevier Pub. Co., 1976.
 Description
 Book — xv, 486 p. illus. 25 cm.
 Online

 www.sciencedirect.com ScienceDirect
 Google Books (Full view)
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QD501 .B242 V.18  Available 
 Bansal, Narottam P.
 [Cleveland, Ohio] : National Aeronautics and Space Administration, Glenn Research Center ; [Springfield, Va. : National Technical Information Service, distributor, 1999]
 Description
 Book — 1 v.
 Online
Green Library
Green Library  Status 

Find it Bing Wing lower level: Microform cabinets  
NAS 1.15:209057  Inlibrary use 