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 3

Today’s lectureBlock 1

Mole Balances (Review)Size CSTRs and PFRs given –rA= f(X)Conversion for Reactors in Series

Block 2Rate LawsReaction OrdersArrhenius EquationActivation EnergyEffect of Temperature

2

Reactor Mole Balance Summary

Reactor

Differential Algebraic Integral

The GMBE applied to the four major reactor types (and the general reaction AB)

V FA 0 FA

rA

CSTR

Review Lecture 1

Vrdt

dNA

A 0

A

A

N

N A

A

VrdNtBatch

NA

t

dFA

dVrA

A

A

F

F A

A

drdFV

0

PFRFA

V

dFA

dW r A

A

A

F

F A

A

rdFW

0

PBRFA

W3

fedA moles reactedA moles X

D ad C

ac B

ab A

ncalculatio of basis asA reactant limiting ChooseD d C c B b A a

Review Lecture 2

4

Reactor Mole Balances in terms of conversionReactor Differential Algebraic Integral

A

0A

rXFV

CSTR

A0A rdVdXF

X

0 A0A r

dXFVPFR

VrdtdXN A0A

VrdXNt

X

0 A0A

BatchX

t

A0A rdWdXF

X

0 A0A r

dXFWPBRX

W5

Levenspiel Plots

6

Reactors in Series

7

reactorfirst tofedA of molesipoint toup reactedA of molesX i

Only valid if there are no side streams

Reactors in Series

8

BAA CkCr

βαβα

OrderRection OverallBin order Ain order

Lecture 3 Rate Laws - Power Law Model

9

C3BA2 A reactor follows an elementary rate law if the reaction orders just happens to agree with the stoichiometric coefficients for the reaction as written.e.g. If the above reaction follows an elementary rate law

2nd order in A, 1st order in B, overall third order

B2AAA CCkr

If 2AA kCr

›Second Order in A›Zero Order in B›Overall Second Order

2A+B3C

€

−rA = kACA2CB

€

−rB = kBCA2CB

€

rC = kCCA2CB

10

iA Cgr Step 1: Rate Law

XhCi Step 2: Stoichiometry

XfrA Step 3: Combine to get

XfrA How to find

11

dDcCbBaA

dr

cr

br

ar DCBA

DadC

acB

abA

Relative Rates of Reaction

12

3r

1r

2r CBA

Relative Rates of ReactionC3BA2

sdmmol10r 3A

sdmmol5

2rr 3A

B

sdmmol15r

23r 3AC

13

Reversible Reaction

Elementary

e

3C2

BAA

AA

3C2

BAA

3CA

2BAAA

KCCCk

kkCCCk

CkCCkr

14

C3BA2

Reversible ReactionA+2B

3C

kA

k-A

Reaction is: First Order in ASecond Order in BOverall third Order

sdm

molesr 3A 3A dmmolesC

smoledm

dmmoledmmolesdmmole

CCrk 2

6

233

3

2BA

A

15

16

Arrhenius Equation

k Ae E RT

k is the specific reaction rate (constant) and is given by the Arrhenius Equation.where:

T k AT 0 k 0

A 1013k

T17

Arrhenius Equationwhere:E = Activation energy (cal/mol)R = Gas constant (cal/mol*K)T = Temperature (K)A = Frequency factor (same units as rate constant k)(units of A, and k, depend on overall reaction order)

18

Reaction CoordinateThe activation energy can be thought of as a barrier to the reaction. One way to view the barrier to a reaction is through the reaction coordinates. These coordinates denote the energy of the system as a function of progress along the reaction path. For the reaction:

A BC A ::: B ::: C AB C

The reaction coordinate is

19

Why is there an Activation Energy?We see that for the reaction to occur, the reactants must overcome an energy barrier or activation energy EA. The energy to overcome their barrier comes from the transfer to the kinetic energy from molecular collisions and internal energy (e.g. Vibrational Energy).1.The molecules need energy to disort or

stretch their bonds in order to break them and thus form new bonds

2.As the reacting molecules come close together they must overcome both stearic and electron repulsion forces in order to react.20

Distribution of Velocities

dUUeTk

mdUTUf TkmU

B

B 2223

2

24,

We will use the Maxwell-Boltzmann Distribution of Molecular Velocities. For a species af mass m, the Maxwell distribution of velocities (relative velocities) is

21

Distribution of VelocitiesA plot of the distribution function, f(U,T), is shown as a function of U:

Maxwell-Boltzmann Distribution of velocities.

T2>T1T2

T1

U22

One such distribution of energies is in the following figure:

f(E,T)dE=fraction of molecules with energies between E+dE

23

End of Lecture 3

24

BC AB

kJ/Molecule

rBC

kJ/Molecule

r0

Potentials (Morse or Lennard-Jones)

VABVBC

rAB

r0

Supplementary Material

25

For a fixed AC distance as B moves away from C the distance of separation of B from C, rBC increases as N moves closer to A. As rBC increases rAB decreases and the AB energy first decreases then increases as the AB molecules become close. Likewise as B moves away from A and towards C similar energy relationships are found. E.g., as B moves towards C from A, the energy first decreases due to attraction then increases due to repulsion of the AB molecules as they come closer together. We now superimpose the potentials for AB and BC to form the following figure:

One can also view the reaction coordinate as variation of the BC distance for a fixed AC distance: l

BCA l

CAB BCAB rr

l

CBA

26

Energy

r

BC

ABS2S1

E*

Reference

E1PE2P

Ea

∆HRx=E2P-E1P

27