CHEMICAL ENGINEERING '«r f I»' CD'RQM Elements of Chemical INCLlfflEO Reaction Engineering 5 H. Scott Fogler H. Scott Fogler Third Edition Applied. Elements of Chemical Reaction Engineering Fogler Fourth Edition The reaction of triphenyl methyl chloride (trityl) (A) and methanol (B). A. + B. Ж. C. + D. Time. Elements of Chemical. Reaction. Engineering. Third Edition. H. SCOTT FOGLER. Ame and Catherine Vennema Professor of Chemical Engineering.

Elements Chemical Reaction Engineering Fogler Pdf

Language:English, French, Dutch
Genre:Personal Growth
Published (Last):05.04.2016
ePub File Size:21.54 MB
PDF File Size:9.76 MB
Distribution:Free* [*Registration Required]
Uploaded by: MONIKA

Elements of Chemical. Reaction. Engineering. Fifth Edition. H. SCOTT FOGLER. Ame and Catherine Vennema Professor of Chemical Engineering and the. Fogler - Elements of Chemical Reaction Engineering 3a hypmarevlimist.gq - Ebook download as PDF File .pdf) or read book online. chemical engineering. Elements of Chemical Reaction Engineering 4th Ed Fogler Solution Manual - Ebook download as PDF File .pdf) or read book online.

See Pl Many students like this straight forward problem becausethey see how CRE principles can be applied to an everyday example. It is often assigned as an in classproblem and part g is usually omitted. Problems Pl-ll and PI show a bit of things to come in terms of reactor sizing. Can be rotated from year to year with PI-3 and PI Asks for details of operation of an industrial reactor.

Encouragesand requires the student to go outside the text for information related to CRE.


May be a bit early in the text to assign this problem. Encouragesand requires using other sources to obtain information. Can I get help with questions outside of textbook solution manuals? You bet!

Just post a question you need help with, and one of our experts will provide a custom solution. You can also find solutions immediately by searching the millions of fully answered study questions in our archive. How do I view solution manuals on my smartphone? You can download our homework help app on iOS or Android to access solutions manuals on your mobile device. Asking a study question in a snap - just take a pic.

This time is the average time the molecules spend in the reactor. A range of typical processing times in terms of the space time residence time for industrial reactors is shown in Table In other words. Gulf Publishing Company. Chemical Engineering. Table gives typical sizes for batch and CSTR reactors along with the comparable size of a familiar object and the costs associated with those sizes.

Chemical Reactor Data. These space times are the times for each of the reactors to take the volume of fluid equivalent to one reactor volume and put it into the reactor. Strange but true. The two space velocities commonly used in industry are the liquid-hourly and gas-hourly space veloci- ties. For the space time.

From Example The gas volumetric flow rate. This example gives an important industrial concept. The entering volumetric flow rate. Ch 5 In this chapter. After completing this chapter. S FA0 For reactors in series with no side streams. Ch 5 as a function of conversion. The conversion X is the moles of A reacted per mole of A fed. Show that by expressing —rA as a function of conversion X. In principle.

This relationship will be developed in a two-step process. We can then use the methods developed in this chapter. In Step 1. By combining the information in Coming attractions in Chapters 3 and 4 Chapters 3 and 4.

Define the parameter conversion and rewrite the mole balances in terms of conversion b. Combining Steps 1 and 2 in Chapters 3 and 4. S - Moles A fed to the first reactor.. Ch 11 and PFRs. In terms of the conversion.

Numerical Integration See Appendix A.

X Conversion. Space time. If the rate of disappearance of A is given as a function of conversion. Chapter 2 Summary 63 2. Summary Notes for Chapter 2 2. Solved Problems A. Interactive Computer Games Reactor Staging 4. Your professor has the key to decode your performance number.

To play this game you must have Windows or a later version. Problems PA a Revisit Examples through Q Go to the Web site www. Use Figure B on page 41 to calculate the conversion for each of the reactors in the fol- lowing arrangements.

How would your answers change if the flow rate. What conversion can you achieve? How would your answers change if the two CSTRs one 0. What conversion could you achieve if you could convince your boss. Being a company about to go bankrupt.

If it were doubled? What conversion can be achieved in a 4. X dX f Revisit Example Calculate the overall conversion. This breaking bad.. Is this arrangement a good arrangement or is there a better one? PB The exothermic reaction of stillbene A to form the economically important trospophene B and methane C.

Below is the Levenspiel plot for this reaction. Part e is a C level problem. Approximately what is the corresponding highest conversion with your arrangement of reactors?

Scheme and sketch your reactor volumes. Chapter 2 Questions and Problems 67 What reactors do you choose. What will be the conversion with the new digestive arrangement? Can the hippo survive? Section I. Will the hippo survive? A Levenspiel plot for this reac- tion is shown in Figure PB. Use the dimensions of the door as a scale. Just go home and relax. Karrass Ltd. Effective Negotiating: Workbook and Discussion Guide.

Chapter 6. Additional information: Beverly Hills. Chemical Reaction Engineering. The Adventures of Poor Mrs. X Figure PB Levenspiel plot for an adiabatic exothermic heterogeneous reaction. Dover Publications. In Chapter 2. Not to fear.

Washington Overview. Rate Laws 3 Success is measured not so much by the position one has reached in life. This relationship between reaction rate and conversion will be obtained in two steps. A heterogeneous reaction involves more than one phase.

An irreversible reaction is one that proceeds in only one direction and continues in that direction until one of the reactants is Types of reactions exhausted. In discussing Rates of Chemical Reaction. The most common example of a unimolecular reaction is radioactive decay. Strictly speaking. The terms unimolecular. A reversible reaction. Rate Laws are the algebraic equations that apply to a given reaction. An irreversible reaction behaves as if no equilibrium condition exists. The molecularity of a reaction is the number of atoms.

For Reaction Section 3.

Prof. Fogler's Lecture Notes

A thorough discussion of net rates is given in Chapter 8 where we dis- cuss multiple reactions. D a a a we see that for every mole of A that is consumed. A is the sum of the rate of reactions of A all the reactions in which A is either a reactant or product in the system.

A sche- matic of the reaction of A and B molecules colliding and reacting is shown in Figure R3. The rate law The algebraic equation that relates —rA to the species concentrations is gives the relation- ship between reac.

Law of Mass Action. For many irreversible reactions. A in kA. The rate law for bimolecular collisions is derived in the collision theory section of the Professional Reference Shelf R3.

One of. Although the functional dependence on concentration may be postulated from theory. The rate of reaction increases with increas- ing concentration of reactants owing the corresponding increase in the number of molecular collisions. The limiting reactant is usually chosen as our basis for calculation. The overall order of the reaction. Kline and Fogler. Here the rate law is the product of concentrations of the individual reacting spe- cies.

The units of rate.

Consider a reaction involving only one reactant. The order of a reaction refers to the powers to which the con- centrations are raised in the kinetic rate law.

Chem Fundamentals The rate con- stant. This form of the rate law can be derived from Collision Theory.

MD They are a function of the reaction chemistry and not the type of reactor in which the reactions occur. Evaluate No. Table gives examples of rate laws for a number of reactions. National Bureau of Standards the lab. Additional sources are before going to Tables of Chemical Kinetics: Homogeneous Reactions. Circular Sept. It is important to remember that the rate laws are determined by experimental obser- vation! Chapter 7 describes how these and other rate laws can be developed from experimental data.

JPL Pub- lication Pasadena. Jet Propulsion Laboratories. By saying a reaction follows an elementary rate law as writ- ten gives us a quick way to look at the reaction stoichiometry and then write the mathematical form of the rate law. The rate constants.

The overall order of a reaction does not have to be an integer. As an example. Rate expressions of this type are very common for liquid and gaseous reactions promoted by solid catalysts see Chapter Sometimes reactions have complex rate expressions that cannot be sepa- rated into solely temperature-dependent and concentration-dependent portions. An example of first-order reaction not involving radioactive decay is the decomposition of eth- anol to form ethylene and hydrogen.

When a rate expression such as the one given above occurs. It is interesting to note that although the reaction orders often correspond to the stoichiometric coefficients. They also occur in homogeneous reaction systems with reactive intermediates see Chapter 9. In the decomposition of nitrous oxide.

Because the law of mass action in collision theory shows that two molecules must collide giving a second-order dependence on the rate. As will be shown in Chapter 9. An active intermediate is a high-energy molecule that reacts virtually as fast as it is formed. Longman Publishing Group. In the absence of photochemical effects or similar phenomena.. The activated molecule can become deacti- vated by collision with another molecule or the activated molecule can decom- pose to B and C.

Physical Chemistry Reading. Active intermediates e. The translational kinetic energy must be absorbed into the chemical bonds where high-amplitude oscillations will lead to bond ruptures. As a result. In heterogeneous catalysis it is the weight of cata- lyst that is important. To express the rate of reaction in terms of concentration rather than par- tial pressure. One must determine the reaction order from the literature or from experiments.

In summary on reaction orders. In this discussion. At equilib- rium. To illustrate how to write rate laws for reversible reactions. Even though a number of reactions follow elementary rate laws.

The net rate of formation of benzene is the sum of the rates of formation from the forward reaction [i. Equation ] and the reverse reaction [i. The rate of formation of diphenyl. From Appendix C.

Equation C Applying Equation and Appendix C to the diphenyl reaction and substituting the appropriate species concentration and exponents. KC decreases with increasing temperature.

For large values of the equilibrium constant. KC T1 ]. This assumption is valid in most laboratory and industrial reactions. T1 [i.

K Equation A further discussion of the equilibrium constant and its thermodynamic relationship is given in Appendix C. It also depends on whether or not a catalyst is present.

It is almost always strongly dependent on temperature. The quantity k is referred to as either the specific reaction rate or the rate constant. The rate of reaction increases with increasing concentration of reactants owing to the increased number of molec- ular collisions at the higher reactant concentrations.

We now discuss Concept 2. In liquid systems it can also be a function of other parameters. Concept 1. In Section 3. For endothermic reactions. BC and product molecules AB and C. One way to view the barrier to a reaction is through the use of potential energy surfaces and the reaction coordinates. For reactions of molecules with small barrier heights occurring at room temperatures. This kinetic energy can in turn be transferred through molecular collisions to internal energy to increase the stretching and bending of the bonds.

If we have a small barrier height. The molecules need energy to distort or stretch their bonds so that they break and now can form new bonds. These coordinates denote the minimum potential energy of the system as a function of the progress along the reaction path as we go from reactants to an intermediate to products. We will dis- cuss each of these concepts separately. Why is there an activation energy?

If the reactants are free radicals that essentially react immediately on collision. In addition to the concentrations of the reacting species.

A couple of the reasons are that in order to react Here EA. Potential Energy Surfaces and Energy Barriers. By increasing the temperature. This increase can be provided by the kinetic energy of the colliding molecules.

The activation energy is the minimum increase in potential energy of the reactants that must be provided to transform the reactants into products. The activation energy can be thought of as a barrier to energy transfer from kinetic energy to potential energy between reacting molecules that must be overcome. Figure a shows the 3—D plot of the potential energy surface.

The molecules need energy to overcome the steric and electron repul- sive forces as they come close together. Concept 2. B—C Distance angstroms 1 X 1. Transition state Energy RBC. A and BC are in their minimum potential energy in the valley and the steep rise up from the valley to the col from X would correspond to increases in the potential energy as A comes close to BC.

Figure b shows a contour plot of the pass and valleys and the reaction coordinate as we pass over the col from valley to valley.

RBC is just the equilibrium bond length. The lines in the figure are contours of constant energy. Richard I. Chemical Kinetics and Catalysis. Energy changes as we move within the potential energy surfaces. Chapter 3 Web Module. If the BC bond is stretched from its equilibrium position at X.

At point X in Figure b. If the BC bond is compressed at X from its equilibrium position. The activation energy. The energy barrier. We see that for the reaction to occur. In the transition state the molecular distances between A and B and between B and C are close. The potential energy is now greater because of the attractive forces trying to bring the B—C distance back to its equilibrium position.. As we proceed further along the arc length of the reaction coordinate depicted in Figure a.

Now that we have the general idea for a reaction coordinate. The reaction coordinate quantifies how far the reaction has progressed. RBC decreases at X. The energy barrier height. We next discuss the pathway over the barrier shown along the line Y—X. As we move along the A—B distance axis in Figure a.

A comes closer to BC and B begins to bond with A and to push BC apart such that the potential energy of the reac- tion pair continues to increase until we arrive at the top of the energy barrier. We want the minimum energy path across the barrier for converting the kinetic energy of the molecules into potential energy.

The sides of the valley at Y represent the cases where AB is either compressed or stretched causing the corresponding increases in potential energy at point Y and can be described in an analogous manner to BC at point X. At the end of the reaction. Now that we have established a barrier height.

Stay ahead with the world's most comprehensive technology and business learning platform.

Courtesy of Richard I. T with dU. As one continues along the reaction coordinate. To discuss this issue. Some will have high velocities and some will have low velocities as they move around and collide. Concept 3. The Maxwell-Boltzmann distribu- tion of relative velocities is given by the probability function.

Other molecular orbitals of the ethane also distort. T dE This fraction is shown by the shaded area in Figure and is approxi- mated by the average value of f E. T is most easily interpreted by recognizing that [f E. This function is plotted for two different temperatures in Figure The distribution function f E.

To summarize this discussion on the three concepts Concept 1 The rate increases with increasing reactant concentration. We can also determine the fraction of collision that have energies greater than a certain value. Concept 2 The rate is related to the potential barrier height and to the conversion of translational energy into potential energy. After taking the natural logarithm of Equation The larger the activation energy.

Recapping the last section. T is the energy distribution function for the kinetic energies of the reacting molecules. The fraction of the molecular collisions that have an energy EA or greater is shown by the shaded areas at the right in Figure Figure shows the fraction of collisions with energies greater than as a func- tion of EA at two different temperatures.

Semilog Plot High E 10 Calculation of the activation energy k 1. One such distribution is the Boltzmann distribution. It is interpreted most easily by recognizing the product [f E. The activation energy has been equated with a minimum energy that must be possessed by reacting molecules before the reaction will occur.

The data in Table E One way is to make a semilog plot of k vs. Another way is to use Excel or Polymath to regress the data. From the slope of the line given in Figure T1 and T2. A and E. We can either use the Arrhenius equation twice. Moore and R. Next we showed that if the rate of disappear- Where are we? Prentice Hall. One such correlation is the Polanyi-Semenov equation.

Thermochemical Kinetics. Kinetics and Mechanisms. Another correlation relates the activation energy to differences in bond strengths between products and reactants. Ch 5 In Chapter 4. One can use either the numerical techniques described in Chapter 2 or. In Chapter 4. Having completed this chapter. Examples of reactions that follow an elementary rate law: Reaction order is determined from experimental observation: Relative rates of reaction for the generic reaction: Molecular Reaction Engineering Molecular simulators e.

Collision Theory 2. Transition State 3. Web Modules A. Molecular Simulation 4. Summary Notes for Chapter 3 2.

Elements of Chemical Reaction Engineering, Fifth Edition

Gaussian are used to make predictions of the activation energy. Similarly from Appendix C. The reaction probability is found by counting up the number of reactive trajectories after Karplus. Transition-State Theory In this section. Figure PW3B-1 shows the energy of the molecules along the reaction coor- dinate.

Collision Theory In this section. Molecular Dynamics Simulations The reaction trajectories are calculated to determine the reaction cross section of the reacting mole- cules. Problems PA a Example Select a topic and explain it. Select one and critique it. What concepts are you not clear about? PB Use Equation to make a plot of f E.

T —1 —1 kcal 0. At K? PB a Use Figure b to sketch the trajectory over the saddle point when the BC and AB molecules vibrate with the minimum separation distance being 0. Recall the range of validity for T in Equation Describe what you find. What are kB and kC? PB Molecular collision energies—refer to Figure What are their differences? If so. Water collects at the bottom of the column and HCN collects at the top.

Copyright c The Hot-Blooded Insects Cambridge. Corrosion of high-nickel stainless steel plates was found to occur in a distillation column used at DuPont to separate HCN and water. Harvard University Press. Keith J. You may also do a pair-wise comparison. Reprinted by permission. Pick an insect. For ants: For honeybees: PB Troubleshooting. The amount of corrosion on each tray is shown in Figure PB as a function of plate loca- tion in the column.

Sulfuric acid is always added at the top of the col- umn to prevent polymerization of HCN. For an alternative to this problem. For fireflies: For crickets: American Chemical Society. The Hot-Blooded Insects Cam- bridge. Lefty was unaware she had coated her glass with an antidote before she filled both glasses with the poisoned brandy. Neglect any variations in con- centrations.

Ambercromby arrives. It is believed. Develop a relationship between the temperature and activation energy for which the rule of thumb holds. Clyde suggested that instead of brandy. She had the fatal end in mind for Clyde. The next day. PB Determine the rate law for the reaction described in each of the cases below involving species A.

View the YouTube video www.When only one reaction is occurring. NY Most graphics boards are automatically supported. Golden Bell Press. The Learning Resources give an overview of the material in each chapter and provide extra explanations, examples, and applications to reinforce the basic concepts of CRE; the Learning Resources are described in Appendix I.

Catalysis Ch. This is the second printing of the text and the CD. Write a paragraph describing two or more of the reactors. A comes closer to BC and B begins to bond with A and to push BC apart such that the potential energy of the reac- tion pair continues to increase until we arrive at the top of the energy barrier.