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CHEE 321: Chemical Reaction Engineering CHEE 321: Chemical Reaction Engineering Module 4: Finding Rate Laws (Chapter 5, Fogler)

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Presentation on theme: "CHEE 321: Chemical Reaction Engineering CHEE 321: Chemical Reaction Engineering Module 4: Finding Rate Laws (Chapter 5, Fogler)"— Presentation transcript:

1 CHEE 321: Chemical Reaction Engineering CHEE 321: Chemical Reaction Engineering Module 4: Finding Rate Laws (Chapter 5, Fogler)

2 Topics to be covered in this module Rate law from batch reactor –Differential Method Methods for calculating dC A /dt Method Excess Method of initial rates –Integral Method Rate law from differential reactor Brief description of other reactor types employed for kinetics study

3 Common Reactor Types for Obtaining Rate Laws Batch Reactor –used primarily for homogeneous reactions Differential Reactor –used primarily for heterogeneous (solid-fluid catalytic) reactions

4 Rate Law from Batch Reactor

5 Typical Experimental Data Available from Batch Reactor Experiments Time (min) t 0 t 1 t 2 t 3 t 4 t 5 Concentration (mol/L)C A0 C A1 C A2 C A3 C A4 C A5 Time (min) t 0 t 1 t 2 t 3 t 4 t 5 Pressure (kPa)P T0 P T1 P T2 P T3 P T4 P T5 OR

6 Rate Law from Batch Reactor There are two general methods for obtaining rate law from batch reactor: Differential Method –Batch reactor data in differential form, i.e. dC A /dt or dP A /dt, is analyzed. Integral Method –Batch reactor data in integral form, i.e. C(t), is analyzed

7 Differential Method of Determining Rate Law from Batch Reactor

8 Differential Method for Obtaining Rate Law from Batch Reactor 1. General Mole Balance 3. Stoichiometry 2. Rate Law 4. Combine V=V o For constant volume or constant density system

9 Rate Law from Batch Reactor - Differential Method Reaction order (  ) can be found from slope of log-log plot of - dC A /dt and C A Taking the logarithm of combined equation dC A dt p CACA p

10 Typical Experimental Data Available from Batch Reactor Experiments Time (min) t 0 t 1 t 2 t 3 t 4 t 5 Concentration (mol/L)C A0 C A1 C A2 C A3 C A4 C A5 Time (min) t 0 t 1 t 2 t 3 t 4 t 5 Pressure (kPa)P T0 P T1 P T2 P T3 P T4 P T5 OR

11 Methods for Calculating dC A /dt

12 Methods for Calculating dC A /dt from [C A vs t] data 1. Graphical Method (Appendix A.2 of Fogler) Step 1: Calculate  C A and  t Step 3: Read - dC A /dt at “t” for which corresponding C A has been measured Step 2: Plot -  C A /  t vs t

13 Methods of Calculating dC A /dt from [C A vs t] data 2. Polynomial Fit Method Step 1: Fit C A vs t data using a polynomial of “n” th order C A = a o +a 1 t +a 2 t 2 +… a n t n Step 2: Calculate dC A /dt dC A /dt = a a 2 t+… (n-1) a n t n-1

14 Methods of Calculating dC A /dt from [C A vs t] data 3. Numerical Method (See Appendix A of Fogler) Can be used when independent variable (in our case “t”) is equally spaced, i.e. t 1 -t 0 = t 2 -t 1 =t 3 -t 2 =t n -t n-1 =  t First Point Last Point Interior Points

15 Integral Method of Determining Rate Law from Batch Reactor

16 Integral Method for Obtaining Rate Law from Batch Reactor 1. General Mole Balance 3. Stoichiometry 2. Rate Law 4. Combine V=VoFor constant density system

17 Integral Method for Obtaining Rate Law from Batch Reactor In the integral method, the reaction order is hypothesized (or guessed) and the preceding equation is then integrated. The hypothesis is verified against experimental data. One disadvantage of the method is that if the reaction order is not known a priori, several trial and errors may have to be done before an acceptable solution is achieved.

18 Reaction Order and Rate Constant Zero-order First-order Second-order

19 Method of Excess and Method of Initial Rates

20 Method of Excess - Rate Law for Reactions Involving Two Reactants Method of Excess: Experiment is carried out under conditions such that one species is in excess. e.g. If B is in excess We follow the same method for determining k' and  as we have discussed previously Reaction: A + B  Products The rate law can be written as follows:

21 Method of Initial Rates For reversible reactions, both forward and backward reaction may become significant. In such case, the methods discussed earlier may not be suitable Slope =  Initially or at time t=0, C A =C A0 and the rate is given by(-r A0 ) = kC A0  Method of Initial Rates may provide the solution Methodology Conduct a number of experiments at various initial concentrations (C A0 ) is carried out Next, plot (-r A0 ) vs C A0 The slope =  Knowing the slope, one can calculate the rate constant ‘k’

22 Rate Law from Differential Reactor

23 Channeling must be avoided Volumetric flow rate, inlet and outlet concentrations must be monitored Heat release per unit volume is low, as such the reactor behaves isothermally. The reactor is assumed to be gradientless, i.e., concentration is assumed to be uniform in the catalyst bed. Differential Reactor F A0 F Ae Catalyst Bed Inert Filling Catalyst weight =W

24 Method for Obtaining Rate Law from Differential Reactor 1. General Mole Balance - in terms of concentration - in terms of conversion (X) and molar flow rate of product (F B ) - in terms of molar flow rates Reaction: a A  b B

25 Method for Obtaining Rate Law from Differential Reactor - For constant volumetric flow rates Concentration of product 2. Rate Law Where,

26 Method for Obtaining Rate Law from Differential Reactor 3. Stoichiometery 4. Combine Known from experiment Kinetic parameters, k and , can be obtained by fitting the experimental data

27 Other Types of Reactors used in Determining Rate Laws

28 Integral Fixed Bed Reactor Ease of construction less prone to rate data being affected by channeling/bypassing of some areas of catalyst bed

29 Stirred Batch Reactor Catalyst dispersed as slurry Good fluid-solid contact Sampling can be problematic

30 Stirred Contained Solids Reactor Also called “spinning basket reactor” Good fluid-solid contact


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