Lecture 11 - University of Michigan › ~essen › html › powerpoints › lecture... · Lecture...
Transcript of Lecture 11 - University of Michigan › ~essen › html › powerpoints › lecture... · Lecture...
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Chemical Reaction Engineering (CRE) is the field that studies the rates and mechanisms of
chemical reactions and the design of the reactors in which they take place.
Lecture 11
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Today’s lecture Determining the Rate Law from Experimental Data
Integral Method Differential (Graphical) Method Nonlinear Least Regression
Multiple Reactions The Four Types What’s New to Our Algorithm Reactions in Series
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Integral Method Consider the following reaction that occurs in a constant volume Batch Reactor: (We will withdraw samples and record the concentration of A as a function of time.)
A Products
Mole Balance:
Rate Law:
Stochiometry:
Combine: 3
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Finally we should also use the formula to plot reaction rate data in terms of conversion vs. time for 0, 1st and 2nd order reactions.
Derivation Equations used to Plot 0, 1st and 2nd order reactions.
These types of plots are usually used to determine the values k for runs at various temperatures and then used to determine the activation energy.
Zero order First Order Second Order
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Guess and check for α = 0, 1, 2 and check against experimental plot
t
CA
t
ln(CA0/CA)
t
1/CA
Finding the Rate law (Integral Method)
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Differential Method Taking the natural log of
The reaction order can be found from a ln-ln plot of:
Slope = α
ln
ln
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Methods for finding the slope of log-log and semi-log graph papers may be found at
http://www.physics.uoguelph.ca/tutorials/GLP/.
However, we are usually given concentration as a function of time from batch reactor experiments:
time (s) 0 t1 t2 t3
concentration (moles/dm3) CA0 CA1 CA2 CA3
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Three Ways to determine (-dCA/dt) from Concentration-Time Data Graphical differentiation Numerical differentiation formulas Differentiation of a polynomial fit to the data 1. Graphical
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The method accentuates measurement error! 9
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Example - Finding Rate Law t(min) 0 1 2 3
CA(mol/L) 1 0.7 0.5 0.35
0.3 0.2 0.15
.1
.2
.3
t 1 2 3
Areas equal for both sides of the histogram
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Example - Finding Rate Law Find the f(t) of using equal area differentiation
CA 1 0.7 0.5 0.35
-dCA/dt 0.35 0.25 0.175 0.12
Plot –dCA/dt as a function of CA ln
CA
Slope = α dCA/dt
ln 11
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Non-Linear Least-Square Analysis
That is we want to be a minimum.
We want to find the parameter values (α, k, E) for which the sum of the squares of the differences, the measured rate (rm), and the calculated rate (rc) is a minimum.
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Non-Linear Least-Square Analysis
For concentration-time data, we can integrate the mole balance equation for to obtain
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Non-Linear Least-Square Analysis
We find the values of alpha and k which minimize s2
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Cmeas 1 0.7 0.5 0.35
CCalc 1 0.5 0.33 0.25
(Cc-Cm) 0 -0.2 -0.17 -0.10
(Cc-Cm)2 0 0.04 0.029 0.01 0.07
for α= 2, k = 1 → S2 = 0.07
for α = 2, k = 2 → S2 = 0.27
etc. until S2 is a minimum 15
Regression Method Guess values forα and k and solve for measured data points then sum squared differences:
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Residuals
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End of Lecture 11
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