ChE 344 Winter 2011 Final Exam + Solution. Open Book, Notes, and Web

Size: px
Start display at page:

Download "ChE 344 Winter 2011 Final Exam + Solution. Open Book, Notes, and Web"

Transcription

1 ChE 344 Winter 011 Final Exam + Solution Monday, April 5, 011 Open Book, Notes, and Web Name Honor Code (Please sign in the space provided below) I have neither given nor received unauthorized aid on this examination, nor have I concealed any violations of the Honor Code. (Signature) The Basics 1) / 5 pts ) / 5 pts 3) / 5 pts 4) / 5 pts 5) / 5 pts 6) / 5 pts 7) / 5 pts Applications 8) / 5 pts 9) /10 pts 10) /10 pts 11) /10 pts Professional 1) /10 pts 13) /0 pts Total /100 pts

2 (5 pts) 1) Mole Balances, Chapter 1 The reaction A + B C takes place in an unsteady CSTR. The feed is only A and B in equimolar proportions. Which of the following set of equations gives the correct mole balances on A, B and C. Species A and B are disappearing and Species C is being formed. Circle the correct answer where all the mole balances are correct (a) F B0 F A V r A dv = dn A F B0 F B V r A dv = dn B Wrong sign for r A, should be + V r A dv (b) F C + F A0 F A + V V r A dv = dn C r A dv = dn A F A0 F B + V r A dv = dn B All are correct. (c) F C V V F A0 F A + 0 r A dv = dn C r A dv = dn A F A0 F B + V r A dv = dn B Wrong sign for F C, should be F C (d) F C + F B0 F A V V r C dv = dn C r A dv = dn A F B0 F B V r A dv = dn B Wrong sign for r A, should be + V r A dv F C + V r C dv = dn C Solution Answer is (b). 1

3 (5 pts) ) Circle the correct answer, true (T), False (F) or (CT) Can t tell from the information given. T F CT (a) Multiple steady states can exist for an irreversible endothermic first order reactions. T F CT (b) A steady-state CSTR operates at 150 C. The reactor effluent is at the same temperature as the reactor contents. Is the reactor operating isothermally? T F CT (c) Multiple steady states can only exist for adiabatic reactions. T F CT (d) Reactor staging is only used for irreversible reactions. T F CT (e) The detrimental effect of pressure drop in gas phase reactions is more pronounced for adiabatic- exothermic reactions than for adiabatic endothermic reactions. Solution (a) False. R T G (b) Insufficient information to answer definitively. Need to know the feed temperature. T 0 = 300 K T = 300 K T = 300 K (c) False. See Equation 1-8 (d) False. See Figure 11-4 (e) True. dy dw = α y Exothermic T y Endothermic T y ( 1+ εx) T T 0

4 (5 pts) 3) Circle the correct answer. Consider the following Levenspiel plot (1 pt) (a) The equilibrium conversion is (1) X e < 0.6 () X e = 0.8 (3) X e > 0.8 (4) Can t tell from the information given (1 pt) (b) The flow rate to an 8 dm 3 CSTR corresponding to Figure E4-1 where 80% conversion is achieved is (1) F A0 = 0.8 mol/s () F A0 = 10 mol/s (3) F A0 = 1 mol/s (4) Can t tell from the information given (1 pt) (c) If the conversion achieved in a single 8 dm 3 CSTR is 80%, what would the conversion be if the flow is equally divided into to two CSTRs in parallel with first reactor having a volume of 4 dm 3 each (same total volume). " 0 " 0 " 0 " 0 vs. 8 dm 3 X=0.8 4 dm 3 4 dm 3 X=_?_ X=_?_ The total reactor volume is constant at 8 dm 3. The conversion for the two reactors in parallel is (1) X > 0.8 () X < 0.8 (3) X = 0.8 (4) Can t tell from the information given ( pts) (d) If the conversion achieved in a single 8 dm 3 CSTR is 80%, what would the conversion be if two CSTRs are connected in series with first reactor having a volume of approximately 3.0 dm 3 and the second reactor having a volume of 0.6 dm 3. 3

5 υ 0 vs. 8 dm dm 3 X= dm 3 X=_?_ The conversion for the two reactors in series is (1) X > 0.8 () X < 0.8 (3) X = 0.8 (4) Can t tell from the information given Solution (a) Ans. (3) X e > 0.8 (b) Ans. (d) Can t tell from information given (c) Ans. (3) X = 0.8. See p161. (d) Ans. () X < 0.8. Try X = dm 3 = 5 dm 3 x 0.6 = 3 dm 3 checks Try ΔV = 0.1 between X = 0.6 and 0.7 V = 0.1 x 6 dm 3 = 0.6 dm 3 checks F A0 r A (dm 3 ) 3dm X 4

6 (5 pts) 4) Consider the following reaction for parts (a), (b) and (c) A + B C Write the rate law in terms of the specific reaction rate and species concentration when (a) The reaction is irreversible and second order in A, and independent of the concentration of C, and overall first order. r A = (b) The reaction is elementary and reversible r A = (c) Now consider the case when the reaction is first order in A and first order in B at high concentrations of A and B and is first order in A and second order in B at low concentrations of B. The rate law is r A = (d) What is the rate law for the reaction CH 3 CHO CH 4 + CO? r CH 3 CHO = Solution A + B C (a) r A = k A C A C B (b) r A = k A C A C B C C (c) r A = k 1 C A C B 1+ k C B K C (d) r A = kc A 3 (see page 80) 5

7 (5 pts) 5) The following figure shows the energy distribution function at 300 K for the reaction A + B C f(e,t) (kcal) E (kcal) (a) What fraction of the collisions have energies between 3 and 5 kcal? (b) What fraction of collisions have energies greater than 5 kcal? Solution (a) Between 0 and 4 k cal f( E,T) = 0.5 E 4 Between 4 and 8 kcal f( E,T) = E f(e,t) (kcal) at E = 3 f( E,T) = 3.5 = at E = 5 f( E,T) = 3.5 = (b) ( ) E (kcal) Area =1 ( 0.5) + ( 1) = 0.44 = 44% f(e,t) (kcal) Area = = 0.8 = 8% ( ) 3 1 = E (kcal) 6

8 (5 pts) 6) Consider the following elementary gas phase reaction A + B C Write r A solely as a function of conversion (i.e., evaluating all symbols) when the reaction is an elementary, reversible, gas phase, isothermal reaction with no pressure drop with an equal molar feed with C A0 =.0, k A = and K C = 0.5 all in proper units. r A = Solution Elementary r A = k C A C B C C K C A is the limiting reactant A + B C y A0 = 1 (Equimolar) ε = y A0 δ = = 1 C A = C A0 1 X C A0 Θ B X X C A0, C B =, C C = 1+ εx 1+ εx r A = k ( ) ( ) 3 C A0 ( ) ( 1 X ) Θ B X ( 1+ εx) 3 C A0 X K C 1+ εx ( ) 1+ εx ( ) 1 r A = k C A0( 1 X) C A X X C 1 1 A0 X X K C 1 1 X r A = C 3 A0 1 X 1 1 X ( ) C A0 X K C 1 1 X 7

9 dm 3 k =, C A0 = mol mol s dm 3, Θ B =1, K C = 0.5 dm3 mol r A = 8( 1 X) 1 1 X X 1 1 X 8

10 (5 pts) 7) The elementary gas phase isomerization exothermic reaction A B cat is carried out isothermally at 400K in a PBR where the pressure drop occurs with α = kg 1. The flow is laminar. Currently 50% conversion is achieved. The equilibrium constant at this temperature is 3.0. (a) For a fixed mass flow rate m, if the reactor diameter is increased by a factor of 4, the conversion X is (1) X > 0.5 () X < 0.5 (3) X = 0.5 (4) insufficient information to tell. (b) For a fixed mass flow rate m, the equilibrium conversion X e is (1) X e = 0.5 () X e = (3) X e = 0.75 (4) insufficient information to tell. (c) For a fixed mass flow rate m, if the reactor diameter is increased by a factor of, the equilibrium conversion X e will (1) increase () decrease (3) remain the same (4) insufficient information to tell (d) For a fixed mass flow rate m, if the particle size is increased the equilibrium conversion X e will (1) increase () decrease (3) remain the same (4) insufficient information to tell (e) Consider the case where an adiabatic endothermic reaction becomes frozen in a PFR [cf. p.541]. The actual conversion, X, can be greater than the equilibrium conversion, X e, near the point where the reaction becomes frozen. (1) True () False (3) Depends on feed condition Solution (a) Ans. (1) X > 0.5 α ~ 1 D Increase D, decrease α, increase X. (b) Ans. (3) X e = 0.75 X e = K C 1+ K C = =

11 (c) Ans. (3) remain the same K C = C A = C A0( 1 X e )y C Ae C A0 X e y X e is not a function of pressure drop parameter α. = 1 X e X e (d) Ans. (3) or (4) Exothermic D P then K then X e X e is not a function of particle size or any other geometry. But will a change in pressure drop affect the achievable conversion, and therefore temperature? X e is a function of temperature. So probably accept unchanged OR Can t tell (e) Ans. () X e can never be less than X, (i.e., X can never be greater than X e). 10

12 (5 pts) 8) Suppose inerts are added to the system in Example 13-. The dashed line represents the relationship after the inerts were added. Which figure represents how the relationship between the line the reactor failed after start up, ts, and the down time, t d, would change? The solid line represents the case without inerts? Solution Answer: B Explanation: dt = Qg Qr N i C Pi = Qg Qr N A C PA + N B C PB + N C C PC + N I C PI We see the rate of temperature increase,, decreases as the amount of inert, N I, increases. Therefore, the temperature will not rise as rapidly during the adiabatic period (down time, td) and we can have longer down times without having an explosion. 11

13 (10 pts) 9) P10-5A Study Problem. The rate law for the hydrogenation (H) of ethylene (E) to form ethane (A) H + C H 4 C cat H 6 over a cobalt-molybdenum catalyst [Collection Czech. Chem. Commun., 51, 760 (1988)] is r E ʹ = kp EP H 1+ K E P E Suggest a mechanism and rate-limiting step consistent with the rate law and then derive the rate law. Solution H = H E = Ethylene A = Ethane H + C H 4 H + E A C cat H 6 Because neither H or C H 6 are not in the denominator of the rate law they are either not adsorbed or weakly adsorbed. Assume H in the gas phase reacts with C H 6 adsorbed on the surface and ethane goes directly into the gas phase. Then check to see if this mechanism agrees with the rate law Eley Rideal E + S E S r AD = k AD P E C V C E S E S + H A + S r S = k S C E S P H E S A + S Assume surface reaction C E S = K E P E C V r S = k S [ C E S P H ] C T = C V + C E S P r A ʹ = k S K E C E P H T 1+ K E P E K E 1

14 (10 pts) 10) P7-10 B Study Problem. In order to study the photochemical decay of aqueous bromine in bright sunlight, a small quantity of liquid bromine was dissolved in water contained in a glass battery jar and placed in direct sunlight. The following data were obtained at 5 C: Time (min) Ppm Br, C A (a) Determine whether the reaction rate is zero, first, or second order in bromine, and calculate the reaction rate constant in units of your choice. (Hint: Preliminary calculations suggest the reaction may be first order.) (b) Assuming identical exposure conditions, calculate the required hourly rate of injection of bromine (grams per hour) into a very large sunlit body of water, 5,000 gal (94,600 dm ) in volume, in order to maintain a sterilizing level of bromine of 1.0 ppm. Note: ppm = parts of bromine per million parts of brominated water by weight. In dilute aqueous solutions, 1 ppm = 1 milligram per liter.) (From California Professional Engineers Exam.) 3 13

15 Solution P7-10 (a) Photochemical decay of bromine in bright sunlight: t (min) CA (ppm) Mole balance: constant V dc A = ra = kcαa dc A α = 1, therefore = kc A dc A C = kc A, ln A0 = kt CA After plotting and differentiating by equal area Time (min) Ppm Br, CA dca/ ln( dca/) ln CA ln CA0/CA First order ln C A0 CA t

16 Slope of Plot of ln (C A0/C A) versus t.0 Slope = 58 min k = min 1 P7-10 (b) dn A dn A = Vr A = F A0 0 + r A V Steady state dn A F A0 = r A V at CA = 1 ppm r A = ppm min = 0 F A0 94,600 dm 3 = mg l min ( ) mg 1g dm 3 min 1,000mg 60m =195 g h h 15

17 This problem is continued from Problem (6) on MidTerm Exam II (Complete parts (e) and (f)) (10 pts) 11) The temperature and conversion in a virtually infinitely long PFR are shown below as a function of the reactor volume. The reactor is surrounded by a jacket for heat transfer. The value of Ua is 100 cal/(sec m 3 K) with T a being constant. The gasphase, reversible reaction is A B + C and pure A is fed to the reactor at a concentration C A0 = 1.0 mol/m 3 and a molar flow rate of 10 mol/s. The absolute value of the heat of reaction is 5,000 cal/mol of A at 500K, and the heat capacities of A, B, and C are each 10 cal/mol/k. T(K) V(m 3 ) (a) Using what is the equilibrium constant at 500 K? K e (500) = 0.11 (From MidTerm Exam II solution) (b) What is the rate of disappearance of A, r A, at 10 m 3? r A = mol/m 3 s (From MidTerm Exam II solution) (6 pt) (c) What is the equilibrium constant at 400 K? K e (400) = (8 pt) (d) What is the specific reaction rate at V = 10 m 3? k = (6 pt) (e) What is the total amount of heat added/removed to the entire reactor per mol of A feed? Include proper sign in your numerical answer if possible. Q F A0 = X 16

18 Solution T(K) V(m 3 ) X (a) K e (500) = _? at V = 10 m 3 Q g = Q r A 1 B+ 1 C δ = 0 ε = 0 C A = C A0 ( 1 X) C B = C C = C A0 X at 500 K X = X e = 0.4 K e = C BC C C A K e = 0.11 = ( ) = ( 0.4) 4( 1 0.4) = ( 0.36) = 0.11 C A0 X e C A0 4 1 X e (b) r A = _? dx dw = r A F A0 Q g Q r!#" # $!#" # $ dt dv = ( r A) ( ΔH Rx ) Ua( T T a ) F i C Pi At minimum dt dv = 0 Q g = Q r At large V no further change in temperature so assume T = T a = 500 K and that T at minimum is 400 K. At minimum 17

19 Q r = Ua (T T a) = 100 ( ) = 10,000 cal/s m 3 Q g = ( r A )( ΔH Rx ) ( r A )( ΔH Rx ) = ( r A )( 5,000) = Q r = 0,000 cal m 3 s r A = 10,000 cal s m 3 5,000 cal mol (c) K e (400) = _? K e ( 400) = K C 500 K e 400 = mol m 3 s ( )exp ΔH Rx 1 1 R T 1 T ( ) = 0.11exp 5,000 = 0.11exp ( )( 500) 5, K e = 0.11exp( 1.5) = ( 0.11) ( 0.8) = (d) k = _? r A = k C A0 C BC C K e A B + C C A = C A0 ( 1 X) C B = C C = C A0 X at V = 10 m 3 T = 400, X = 0., K e =

20 r A = k C A0 1 X = kc A0 1 X = k ( ) C A0 ( ) X X 4K C 4K e ( ) ( 0.) ( 4) ( 0.031) = k r A = mol mol m 3 = 0.3 s m 3 k = k[ ] (e) k = m3 = mol s Q =? F A0 Q F A0 Θ i C Pi T T 0 Per Mole A Q F A0 = C PA T T 0 A B + C! ( ) ΔH Rx [ + ΔC P ( T T a )]F A0 X = 0 Eqn. (11-8) [ ( )X] [ ] + ΔH Rx + ΔC P T T R ΔC P = C P C + C P B C P A = = 0 = 0 Q F A0 = ( ) + +5,000 [ ] 0.4 [ ] = 1,000 +,000 =1,000 cal mol 19

21 (10 pts) 1) Let s revisit homework Problem P1-3 where the reaction B C A + B is carried out in a packed bed reactor. Match the following temperature and conversion profiles for the 4 different heat exchange cases adiabatic, constant T, co-current exchange and counter current exchange. a Figure 1 Figure Figure 3 Figure 4 0

22 Figure A Figure B Figure C Figure D (a) Figure 1 matches Figure (b) Figure matches Figure (c) Figure 3 matches Figure (d) Figure 4 matches Figure Solution (a) Figure 1 matches Figure _C_ (b) Figure matches Figure _A_ (c) Figure 3 matches Figure _D_ (d) Figure 4 matches Figure _B_ 1

23 In Class Problem 14 Solution (a) Adiabatic

24 Constant T In Class Problem 14 Solution (b) Constant T Heat Exchange a 3 a

25 In Class Problem 14 Solution (c) Variable T Co-Current Heat Exchange a 4

26 In Class Problem 14 Solution (d) Variable T Counter Current Heat Exchange a Matches 5

27 (0 pts) 13) The following reactions are taking place in a,000 dm 3 liquid phase batch reactor under a pressure of 400 psig k 1A A + B C ΔH Rx1B = 5,000 cal mol r 1A = k 1A C A C B k A 3C + A D ΔH RxC = +10,000 cal mol r A = k A C A C C B+ 3C k 3C E ΔH Rx3B = 50,000 cal mol r 3C = k 3C C B C C The initial temperture is 450 K and the initial concentrations of A, B and C are 1.0, 0.5 and 0. mol/dm 3 respectively. The coolant flow rate was at it s maximum value so that T a1 = T a = T a = 400 K so that the product the exchange area and overall heat transfer coefficient, UA, is UA = 100 cal/s K. (a) What is Q r at t = 0? (b) What is Q g at t = 0? (c) If Q r > Q g at time t = 0, and there is no failure of the heat exchange system, is there any possibility that reactor will run away? Explain (d) What is the initial rate of increase in temperature, (dt/) at t = 0? dt = (e) Suppose that the ambient temperature T a is lowered from 400 K to 350 K, what is the initial rate of reactor temperature change? dt = (f) A suggestion was made to add 50 mole of inerts at a temperature of 450 K. Will the addition of the inerts make runaway more likely or less likely? How? Show quantitatively. Additional information As a first approximation, assume all heats of reaction are constant ( ΔC P 0) Specific reaction rates at 450 K are ( ) s k 1A = dm 3 mol k A = 1 ( dm 3 mol) s k 3C = ( dm 3 mol) s 6

28 C PA =10cal mol K C PB =10cal mol K C PD = 80cal mol K C PE = 50cal mol K Solution Part (a) Part (b) C PC = 50cal mol K Q r = UA( T T a ) =100 cal cal [ ]K = 5,000 5 K s Q g = V[ r 1B ΔH Rx1B + r C ΔH RxC + r 3B ΔH Rx3B ] Initially T = 350 K Reaction 1: Reaction : r 1A 1 = r 1B = r 1C 1 r A = r C 3 = r D 1 r 1B = r 1A r C = 3 r A Part (c) Reaction 3: r 3B 1 = r 3C 3 = r 3E 1 Q g = V[ k 1A C A C B ] ΔH Rx1B r 3B = 1 3 r 3C [ ] + V 3 k AC A C C ΔH RxC [ ] + V 1 3 k 3CC B C C = (,000) [( ) ( 10 3 ) ( 1 ) ( 0.5 ) 5,000]!### "#### $ +, ( 1) ( 0.) [ 10,000] +!####"#### $ 5,000 ( ) 0.5 +, ( )( 0.) 3 [ 50,000 ] = 5,000!##### "###### $ Q g = 5,000cal s dt = dt = +,000 Q r Q g N A0 C PA + N B0 C PB + N C0 C PC = Q g Q r N A C PA + N B C PB + N C C PC,000 5,000 5,000 N A0 C PA + N B0 C PB + N C0 C PC = 0 ΔH Rx3C [ ] If Q r > Q g then the temperature can only decrease causing the specific reaction rates k i to decrease, hence runaway is unlikely. 7

29 Part (d) Part (e) N A0 C PA = C A0 VC PA = ( 1) (,000) ( 10) = 0,000 N B0 C PB = C B0 VC PB = ( 0.5) (,000) ( 10) =10,000 N C0 C PC = C C0 VC PC = ( 0.) (,000) ( 50) = 0,000 dt = Q g Q r 50,000 Drop T a by 50 Q r = UA( T T a ) =100( ) =10,000 dt Part (f) = 5,000 10,000 50,000 = 0.1 [ ] UA( T T a ) dt = Q g Q r = r 1B VΔH Rx1B + r C VΔH RxC + r 3A VΔH Rx3A N i C Pi N A C PA + N B C PB + N C C PC + N D C PD + N E C PE + N Inerts C PInerts Inerts (N Inerts) will not change Q g or Q r, they will only show the rate of temperature increase or decrease. 8

30 Blank sheet

31 Blank sheet

ChE 344 Winter 2011 Final Exam. Open Book, Notes, and Web

ChE 344 Winter 2011 Final Exam. Open Book, Notes, and Web ChE 344 Winter 2011 Final Exam Monday, April 25, 2011 Open Book, Notes, and Web Name Honor Code (Please sign in the space provided below) I have neither given nor received unauthorized aid on this examination,

More information

ChE 344 Winter 2013 Final Exam + Solution. Open Course Textbook Only Closed everything else (i.e., Notes, In-Class Problems and Home Problems

ChE 344 Winter 2013 Final Exam + Solution. Open Course Textbook Only Closed everything else (i.e., Notes, In-Class Problems and Home Problems ChE 344 Winter 03 Final Exam + Solution Thursday, May, 03 Open Course Textbook Only Closed everything else (i.e., Notes, In-Class Problems and Home Problems Name Honor Code (Please sign in the space provided

More information

ChE 344 Winter 2013 Mid Term Exam II Tuesday, April 9, 2013

ChE 344 Winter 2013 Mid Term Exam II Tuesday, April 9, 2013 ChE 344 Winter 2013 Mid Term Exam II Tuesday, April 9, 2013 Open Course Textbook Only Closed everything else (i.e., Notes, In-Class Problems and Home Problems Name Honor Code (Please sign in the space

More information

Name. Honor Code: I have neither given nor received unauthorized aid on this examination, nor have I concealed any violations of the Honor Code.

Name. Honor Code: I have neither given nor received unauthorized aid on this examination, nor have I concealed any violations of the Honor Code. ChE 344 Fall 014 Mid Term Exam II Wednesday, November 19, 014 Open Book Closed Notes (but one 3x5 note card), Closed Computer, Web, Home Problems and In-class Problems Name Honor Code: I have neither given

More information

ChE 344 Chemical Reaction Engineering Winter 1999 Final Exam. Open Book, Notes, CD ROM, Disk, and Web

ChE 344 Chemical Reaction Engineering Winter 1999 Final Exam. Open Book, Notes, CD ROM, Disk, and Web ChE 344 Chemical Reaction Engineering Winter 1999 Final Exam Open Book, Notes, CD ROM, Disk, and Web Name Honor Code 1) /25 pts 2) /15 pts 3) /10 pts 4) / 3 pts 5) / 6 pts 6) / 8 pts 7) / 8 pts 8) / 5

More information

ChE 344 Winter 2011 Mid Term Exam I + Solution. Closed Book, Web, and Notes

ChE 344 Winter 2011 Mid Term Exam I + Solution. Closed Book, Web, and Notes ChE 344 Winter 011 Mid Term Exam I + Thursday, February 17, 011 Closed Book, Web, and Notes Name Honor Code (sign at the end of exam) 1) / 5 pts ) / 5 pts 3) / 5 pts 4) / 15 pts 5) / 5 pts 6) / 5 pts 7)

More information

ChE 344 Winter 2013 Mid Term Exam I Tuesday, February 26, Closed Book, Web, and Notes. Honor Code

ChE 344 Winter 2013 Mid Term Exam I Tuesday, February 26, Closed Book, Web, and Notes. Honor Code ChE 344 Winter 2013 Mid Term Exam I Tuesday, February 26, 2013 Closed Book, Web, and Notes Name Honor Code (Sign at the end of exam period) 1) / 5 pts 2) / 5 pts 3) / 5 pts 4) / 5 pts 5) / 5 pts 6) / 5

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 21 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. Web Lecture 21 Class Lecture

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 19 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. oday s lecture Gas Phase

More information

Chemical Reaction Engineering. Dr. Yahia Alhamed

Chemical Reaction Engineering. Dr. Yahia Alhamed Chemical Reaction Engineering Dr. Yahia Alhamed 1 Kinetics and Reaction Rate What is reaction rate? It is the rate at which a species looses its chemical identity per unit volume. The rate of a reaction

More information

CBE 142: Chemical Kinetics & Reaction Engineering

CBE 142: Chemical Kinetics & Reaction Engineering CBE 142: Chemical Kinetics & Reaction Engineering Midterm #2 November 6 th 2014 This exam is worth 100 points and 20% of your course grade. Please read through the questions carefully before giving your

More information

PHEN 612 SPRING 2008 WEEK 1 LAURENT SIMON

PHEN 612 SPRING 2008 WEEK 1 LAURENT SIMON PHEN 612 SPRING 2008 WEEK 1 LAURENT SIMON Chapter 1 * 1.1 Rate of reactions r A A+B->C Species A, B, and C We are interested in the rate of disappearance of A The rate of reaction, ra, is the number of

More information

Midterm II. ChE 142 April 11, (Closed Book and notes, two 8.5 x11 sheet of notes is allowed) Printed Name

Midterm II. ChE 142 April 11, (Closed Book and notes, two 8.5 x11 sheet of notes is allowed) Printed Name ChE 142 pril 11, 25 Midterm II (Closed Book and notes, two 8.5 x11 sheet of notes is allowed) Printed Name KEY By signing this sheet, you agree to adhere to the U.C. Berkeley Honor Code Signed Name_ KEY

More information

4 th Edition Chapter 9

4 th Edition Chapter 9 Insert Page 547A 4 th Edition Chapter 9 In summary, if any one of the following three things had not occurred the explosion would not have happened. 1. Tripled production 2. Heat exchanger failure for

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 22 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. Web Lecture 22 Class Lecture

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 24 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. Web Lecture 24 Class Lecture

More information

CHE 404 Chemical Reaction Engineering. Chapter 8 Steady-State Nonisothermal Reactor Design

CHE 404 Chemical Reaction Engineering. Chapter 8 Steady-State Nonisothermal Reactor Design Textbook: Elements of Chemical Reaction Engineering, 4 th Edition 1 CHE 404 Chemical Reaction Engineering Chapter 8 Steady-State Nonisothermal Reactor Design Contents 2 PART 1. Steady-State Energy Balance

More information

Problems Points (Max.) Points Received

Problems Points (Max.) Points Received Chemical Engineering 142 Chemical Kinetics and Reaction Engineering Midterm 1 Tuesday, October 8, 2013 8:10 am-9:30 am The exam is 100 points total. Please read through the questions very carefully before

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 4 hemical Reaction Engineering (RE) is the field that studies the rates and mechanisms of chemical reactions and the design of the reactors in which they take place. hapter 4 Lecture 4 Block 1

More information

Chemical Kinetics and Reaction Engineering

Chemical Kinetics and Reaction Engineering Chemical Kinetics and Reaction Engineering MIDTERM EXAMINATION II Friday, April 9, 2010 The exam is 100 points total and 20% of the course grade. Please read through the questions carefully before giving

More information

CHE 404 Chemical Reaction Engineering. Chapter 8 Steady-State Nonisothermal Reactor Design

CHE 404 Chemical Reaction Engineering. Chapter 8 Steady-State Nonisothermal Reactor Design Textbook: Elements of Chemical Reaction Engineering, 4 th Edition 1 CHE 404 Chemical Reaction Engineering Chapter 8 Steady-State Nonisothermal Reactor Design Contents 2 PART 1. Steady-State Energy Balance

More information

PFR with inter stage cooling: Example 8.6, with some modifications

PFR with inter stage cooling: Example 8.6, with some modifications PFR with inter stage cooling: Example 8.6, with some modifications Consider the following liquid phase elementary reaction: A B. It is an exothermic reaction with H = -2 kcal/mol. The feed is pure A, at

More information

Review: Nonideal Flow in a CSTR

Review: Nonideal Flow in a CSTR L3- Review: Nonideal Flow in a CSTR Ideal CSTR: uniform reactant concentration throughout the vessel Real stirred tank Relatively high reactant concentration at the feed entrance Relatively low concentration

More information

Chemical Reaction Engineering. Lecture 2

Chemical Reaction Engineering. Lecture 2 hemical Reaction Engineering Lecture 2 General algorithm of hemical Reaction Engineering Mole balance Rate laws Stoichiometry Energy balance ombine and Solve lassification of reactions Phases involved:

More information

Chapter 1. Lecture 1

Chapter 1. Lecture 1 Chapter 1 Lecture 1 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. 1 Lecture 1 Introduction

More information

Lecture 8. Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors

Lecture 8. Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors Lecture 8 Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors Mole alance in terms of Concentration and Molar Flow Rates Working in terms of number of moles

More information

Chemical Reaction Engineering Lecture 5

Chemical Reaction Engineering Lecture 5 Chemical Reaction Engineering g Lecture 5 The Scope The im of the Course: To learn how to describe a system where a (bio)chemical reaction takes place (further called reactor) Reactors Pharmacokinetics

More information

Dr. Trent L. Silbaugh, Instructor Chemical Reaction Engineering Final Exam Study Guide

Dr. Trent L. Silbaugh, Instructor Chemical Reaction Engineering Final Exam Study Guide Chapter 1 Mole balances: Know the definitions of the rate of reaction, rate of disappearance and rate of appearance Know what a rate law is Be able to write a general mole balance and know what each term

More information

To increase the concentration of product formed in a PFR, what should we do?

To increase the concentration of product formed in a PFR, what should we do? To produce more moles of product per time in a flow reactor system, what can we do? a) Use less catalyst b) Make the reactor bigger c) Make the flow rate through the reactor smaller To increase the concentration

More information

CE 329, Fall 2015 Second Mid-Term Exam

CE 329, Fall 2015 Second Mid-Term Exam CE 39, Fall 15 Second Mid-erm Exam You may only use pencils, pens and erasers while taking this exam. You may NO use a calculator. You may not leave the room for any reason if you do, you must first turn

More information

CHEMICAL REACTION ENGINEERING

CHEMICAL REACTION ENGINEERING CHEMICL RECTION ENGINEERING Unit 5 nalysis of reactor DT Collection and analysis of rate data Batch reactor for homogenous and heterogeneous reactions measurement during the unsteady-state operation Differential

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 2 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. 1 Lecture 2 Review of Lecture

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Chemical Reaction Engineering Dr. Yahia Alhamed Chemical and Materials Engineering Department College of Engineering King Abdulaziz University General Mole Balance Batch Reactor Mole Balance Constantly

More information

Lecture 4. Mole balance: calculation of membrane reactors and unsteady state in tank reactors. Analysis of rate data

Lecture 4. Mole balance: calculation of membrane reactors and unsteady state in tank reactors. Analysis of rate data Lecture 4 Mole balance: calculation of membrane reactors and unsteady state in tank reactors. nalysis of rate data Mole alance in terms of Concentration and Molar Flow Rates Working in terms of number

More information

5. Collection and Analysis of. Rate Data

5. Collection and Analysis of. Rate Data 5. Collection and nalysis of o Objectives Rate Data - Determine the reaction order and specific reaction rate from experimental data obtained from either batch or flow reactors - Describe how to analyze

More information

H 0 r = -18,000 K cal/k mole Assume specific heats of all solutions are equal to that of water. [10]

H 0 r = -18,000 K cal/k mole Assume specific heats of all solutions are equal to that of water. [10] Code No: RR320802 Set No. 1 III B.Tech II Semester Supplementary Examinations, November/December 2005 CHEMICAL REACTION ENGINEERING-I (Chemical Engineering) Time: 3 hours Max Marks: 80 Answer any FIVE

More information

A First Course on Kinetics and Reaction Engineering. Class 20 on Unit 19

A First Course on Kinetics and Reaction Engineering. Class 20 on Unit 19 A First Course on Kinetics and Reaction Engineering Class 20 on Unit 19 Part I - Chemical Reactions Part II - Chemical Reaction Kinetics Where We re Going Part III - Chemical Reaction Engineering A. Ideal

More information

Thermodynamics revisited

Thermodynamics revisited Thermodynamics revisited How can I do an energy balance for a reactor system? 1 st law of thermodynamics (differential form): de de = = dq dq--dw dw Energy: de = du + de kin + de pot + de other du = Work:

More information

BCIT Fall Chem Exam #2

BCIT Fall Chem Exam #2 BCIT Fall 2017 Chem 3310 Exam #2 Name: Attempt all questions in this exam. Read each question carefully and give a complete answer in the space provided. Part marks given for wrong answers with partially

More information

CHEMICAL REACTORS - PROBLEMS OF REACTOR ASSOCIATION 47-60

CHEMICAL REACTORS - PROBLEMS OF REACTOR ASSOCIATION 47-60 2011-2012 Course CHEMICL RECTORS - PROBLEMS OF RECTOR SSOCITION 47-60 47.- (exam jan 09) The elementary chemical reaction in liquid phase + B C is carried out in two equal sized CSTR connected in series.

More information

Lecture 8. Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors

Lecture 8. Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors Lecture 8 Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors Mole alance in terms of oncentration and Molar low Rates Working in terms of number of moles

More information

Chem 6 sample exam 1 (100 points total)

Chem 6 sample exam 1 (100 points total) Chem 6 sample exam 1 (100 points total) @ This is a closed book exam to which the Honor Principle applies. @ The last page contains several equations which may be useful; you can detach it for easy reference.

More information

HW Help. How do you want to run the separation? Safety Issues? Ease of Processing

HW Help. How do you want to run the separation? Safety Issues? Ease of Processing HW Help Perform Gross Profitability Analysis on NaOH + CH4 --> Na+CO+H NaOH+C-->Na+CO+1/H NaOH+1/ H-->Na+HO NaOH + CO Na+CO+1/H How do you want to run the reaction? NaOH - Solid, Liquid or Gas T for ΔGrxn

More information

The underlying prerequisite to the application of thermodynamic principles to natural systems is that the system under consideration should be at equilibrium. http://eps.mcgill.ca/~courses/c220/ Reversible

More information

Exam 1 Chemical Reaction Engineering 26 February 2001 Closed Book and Notes

Exam 1 Chemical Reaction Engineering 26 February 2001 Closed Book and Notes Exam 1 Chemical Reaction Engineering 26 February 21 Closed Book and Notes (2%) 1. Derive the unsteady-state mole balance for a chemical species A for a packed bed reactor using the following steps: a)

More information

Investigation of adiabatic batch reactor

Investigation of adiabatic batch reactor Investigation of adiabatic batch reactor Introduction The theory of chemical reactors is summarized in instructions to Investigation of chemical reactors. If a reactor operates adiabatically then no heat

More information

1. Introductory Material

1. Introductory Material CHEE 321: Chemical Reaction Engineering 1. Introductory Material 1b. The General Mole Balance Equation (GMBE) and Ideal Reactors (Fogler Chapter 1) Recap: Module 1a System with Rxn: use mole balances Input

More information

Chemical Reaction Engineering

Chemical Reaction Engineering CHPTE 7 Chemical eaction Engineering (Gate 00). The conversion for a second order, irreversible reaction (constant volume) () k B, in batch mode is given by k C t o ( kcot) (C) k C t o + (D) kcot (B) k

More information

10.37 Exam 2 25 April, points. = 10 nm. The association rate constant

10.37 Exam 2 25 April, points. = 10 nm. The association rate constant Problem 1: 35 points 10.37 Exam 2 25 April, 2007 100 points A protein and ligand bind reversibly with = 10 nm. The association rate constant k on = 2x10 4 M 1 s -1. The two species are mixed at an initial

More information

CHEMISTRY 102 FALL 2010 EXAM 2 FORM C SECTION 502 DR. KEENEY-KENNICUTT PART 1

CHEMISTRY 102 FALL 2010 EXAM 2 FORM C SECTION 502 DR. KEENEY-KENNICUTT PART 1 NAME CHEMISTRY 102 FALL 2010 EXAM 2 FORM C SECTION 502 DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated. (2) Sign the Aggie

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 8 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. oday s lecture Block 1: Mole

More information

Chemical reactors. H has thermal contribution, pressure contribution (often negligible) and reaction contribution ( source - like)

Chemical reactors. H has thermal contribution, pressure contribution (often negligible) and reaction contribution ( source - like) Chemical reactors - chemical transformation of reactants into products Classification: a) according to the type of equipment o batch stirred tanks small-scale production, mostly liquids o continuous stirred

More information

10A. EVALUATION OF REACTION RATE FORMS IN STIRRED TANK. Most of the problems associated with evaluation and determination of proper rate forms from

10A. EVALUATION OF REACTION RATE FORMS IN STIRRED TANK. Most of the problems associated with evaluation and determination of proper rate forms from UPDATED 04/0/05 0A. EVALUATIO OF REACTIO RATE FORMS I STIRRED TAK REACTORS Most of the problems associated with evaluation and determination of proper rate forms from batch data are related to the difficulties

More information

TABLE OF CONTENT. Chapter 4 Multiple Reaction Systems 61 Parallel Reactions 61 Quantitative Treatment of Product Distribution 63 Series Reactions 65

TABLE OF CONTENT. Chapter 4 Multiple Reaction Systems 61 Parallel Reactions 61 Quantitative Treatment of Product Distribution 63 Series Reactions 65 TABLE OF CONTENT Chapter 1 Introduction 1 Chemical Reaction 2 Classification of Chemical Reaction 2 Chemical Equation 4 Rate of Chemical Reaction 5 Kinetic Models For Non Elementary Reaction 6 Molecularity

More information

CHEMICAL ENGINEERING KINETICS/REACTOR DESIGN. Tony Feric, Kathir Nalluswami, Manesha Ramanathan, Sejal Vispute, Varun Wadhwa

CHEMICAL ENGINEERING KINETICS/REACTOR DESIGN. Tony Feric, Kathir Nalluswami, Manesha Ramanathan, Sejal Vispute, Varun Wadhwa CHEMICAL ENGINEERING KINETICS/REACTOR DESIGN Tony Feric, Kathir Nalluswami, Manesha Ramanathan, Sejal Vispute, Varun Wadhwa Presentation Overview Kinetics Reactor Design Non- Isothermal Design BASICS OF

More information

C A0 0.8 mol/dm 3. C T0 1.0 mol/dm 3. r A. v 0 C A0 vc A + r A V V dc A. 4. Stoichiometry (gas phase, P P 0, T T 0 ). From Equation (3-41) we have

C A0 0.8 mol/dm 3. C T0 1.0 mol/dm 3. r A. v 0 C A0 vc A + r A V V dc A. 4. Stoichiometry (gas phase, P P 0, T T 0 ). From Equation (3-41) we have Chapter 10 Catalsis and Cataltic Reactors W10-1 Web Example W10 Catalst Deca in a Fluidized Bed Modeled as a CSTR The gas-phase cracking reaction Gas oil (g) Products (g) B C is carried out in a fluidized

More information

Development of Dynamic Models. Chapter 2. Illustrative Example: A Blending Process

Development of Dynamic Models. Chapter 2. Illustrative Example: A Blending Process Development of Dynamic Models Illustrative Example: A Blending Process An unsteady-state mass balance for the blending system: rate of accumulation rate of rate of = of mass in the tank mass in mass out

More information

FLOW REACTORS FOR HOMOGENOUS REACTION: PERFORMANCE EQUATIONS AND APPLICATIONS

FLOW REACTORS FOR HOMOGENOUS REACTION: PERFORMANCE EQUATIONS AND APPLICATIONS FLOW REACTORS FOR HOMOGENOUS REACTION: PERFORMANCE EQUATIONS AND APPLICATIONS At the end of this week s lecture, students should be able to: Develop and apply the performance equation for plug flow reactors.

More information

CE 329, Fall 2015 Assignment 16, Practice Exam

CE 329, Fall 2015 Assignment 16, Practice Exam CE 39, Fall 15 Assignment 16, Practice Exam You may only use pencils, pens and erasers while taking this exam. You may NO use a calculator. You may not leave the room for any reason if you do, you must

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 6 hemical Reaction Engineering (RE) is the field that studies the rates and mechanisms of chemical reactions and the design of the reactors in which they take place. Lecture 6 Tuesday 1/9/13 Block

More information

Basic Concepts in Reactor Design

Basic Concepts in Reactor Design Basic Concepts in Reactor Design Lecture # 01 KBK (ChE) Ch. 8 1 / 32 Introduction Objectives Learning Objectives 1 Different types of reactors 2 Fundamental concepts used in reactor design 3 Design equations

More information

Thermodynamic Processes and Thermochemistry

Thermodynamic Processes and Thermochemistry General Chemistry Thermodynamic Processes and Thermochemistry 박준원교수 ( 포항공과대학교화학과 ) 이번시간에는! Systems, states, and processes The first law of thermodynamics: internal energy, work, and heat Heat capacity,

More information

Chemical Equilibrium. Professor Bice Martincigh. Equilibrium

Chemical Equilibrium. Professor Bice Martincigh. Equilibrium Chemical Equilibrium by Professor Bice Martincigh Equilibrium involves reversible reactions Some reactions appear to go only in one direction are said to go to completion. indicated by All reactions are

More information

Review for Final Exam. 1ChE Reactive Process Engineering

Review for Final Exam. 1ChE Reactive Process Engineering Review for Final Exam 1ChE 400 - Reactive Process Engineering 2ChE 400 - Reactive Process Engineering Stoichiometry Coefficients Numbers Multiple reactions Reaction rate definitions Rate laws, reaction

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture # Chemical Reaction Engineering Youn-Woo Lee School of Chemical and Biological Engineering Seoul National University 155-741, 599 Gwanangro, Gwanak-gu, Seoul, Korea ywlee@snu.ac.kr http://sfpl.snu.ac.kr

More information

Steady-State Molecular Diffusion

Steady-State Molecular Diffusion Steady-State Molecular Diffusion This part is an application to the general differential equation of mass transfer. The objective is to solve the differential equation of mass transfer under steady state

More information

Mathematical Modeling Of Chemical Reactors

Mathematical Modeling Of Chemical Reactors 37 Mathematical Modeling Of Chemical Reactors Keywords: Reactors, lug flow, CSTR, Conversion, Selectivity Chemical reactor calculations are based on the elementary conservation laws of matter and energy.

More information

(1) This reaction mechanism includes several undesired side reactions that produce toluene and benzene:

(1) This reaction mechanism includes several undesired side reactions that produce toluene and benzene: HYSYS Multiple Reactions - Styrene Prepared by Robert P. Hesketh Spring 005 Styrene Reactor System You have been studying how to use HYSYS using the example of a Styrene reactor system. In this session

More information

Physical Chemistry I CHEM 4641 Final Exam 13 questions, 30 points

Physical Chemistry I CHEM 4641 Final Exam 13 questions, 30 points Physical Chemistry I CHEM 4641 Final Exam 13 questions, 30 points Name: KEY Gas constant: R = 8.314 J mol -1 K -1 = 0.008314 kj mol -1 K -1. Boltzmann constant k = 1.381 10-23 J/K = 0.6950 cm -1 /K h =

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lecture 13 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. Today s lecture Complex

More information

CHEMISTRY 202 Hour Exam III. Dr. D. DeCoste T.A. 21 (16 pts.) 22 (21 pts.) 23 (23 pts.) Total (120 pts)

CHEMISTRY 202 Hour Exam III. Dr. D. DeCoste T.A. 21 (16 pts.) 22 (21 pts.) 23 (23 pts.) Total (120 pts) CHEMISTRY 202 Hour Exam III December 1, 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 23 questions on 12 numbered pages. Check now to make sure you have a complete exam. You have two hours

More information

Last Name or Student ID

Last Name or Student ID 10/06/08, Chem433 Exam # 1 Last Name or Student ID 1. (3 pts) 2. (3 pts) 3. (3 pts) 4. (2 pts) 5. (2 pts) 6. (2 pts) 7. (2 pts) 8. (2 pts) 9. (6 pts) 10. (5 pts) 11. (6 pts) 12. (12 pts) 13. (22 pts) 14.

More information

General Chemistry revisited

General Chemistry revisited General Chemistry revisited A(g) + B(g) C(g) + D(g) We said that G = H TS where, eg, H = f H(C) + f H(D) - f H(A) - f H(B) G < 0 implied spontaneous to right G > 0 implied spontaneous to left In a very

More information

Chemical Reaction Engineering. Lecture 7

Chemical Reaction Engineering. Lecture 7 hemical Reaction Engineering Lecture 7 Home problem: nitroaniline synthesis the disappearance rate of orthonitrochlorobenzene [ ] d ONB ra k ONB NH dt Stoichiometric table: [ ][ ] 3 hange Remaining* oncentration**

More information

AP Chem Chapter 14 Study Questions

AP Chem Chapter 14 Study Questions Class: Date: AP Chem Chapter 14 Study Questions 1. A burning splint will burn more vigorously in pure oxygen than in air because a. oxygen is a reactant in combustion and concentration of oxygen is higher

More information

Name ID# Section # CH 1020 EXAM 2 Spring Form A

Name ID# Section # CH 1020 EXAM 2 Spring Form A Name ID# Section # CH EXAM Spring 7 - Form A Fill in your name, ID#, and section on this test booklet. Fill in and bubble in your name, ID# (bubble for C ), and section on the scantron form. For question

More information

1/r plots: a brief reminder

1/r plots: a brief reminder L10-1 1/r plots: a brief reminder 1/r X target X L10-2 1/r plots: a brief reminder 1/r X target X L10-3 1/r plots: a brief reminder 1/r X target X Special Case: utocatalytic Reactions Let s assume a reaction

More information

Chem Hughbanks Final Exam, May 11, 2011

Chem Hughbanks Final Exam, May 11, 2011 Chem 107 - Hughbanks Final Exam, May 11, 2011 Name (Print) UIN # Section 503 Exam 3, Version # A On the last page of this exam, you ve been given a periodic table and some physical constants. You ll probably

More information

Chemical Reaction Engineering - Part 14 - intro to CSTRs Richard K. Herz,

Chemical Reaction Engineering - Part 14 - intro to CSTRs Richard K. Herz, Chemical Reaction Engineering - Part 4 - intro to CSTRs Richard K. Herz, rherz@ucsd.edu, www.reactorlab.net Continuous Stirred Tank Reactors - CSTRs Here are a couple screenshots from the ReactorLab, Division

More information

Module 1: Mole Balances, Conversion & Reactor Sizing (Chapters 1 and 2, Fogler)

Module 1: Mole Balances, Conversion & Reactor Sizing (Chapters 1 and 2, Fogler) CHE 309: Chemical Reaction Engineering Lecture-2 Module 1: Mole Balances, Conversion & Reactor Sizing (Chapters 1 and 2, Fogler) Module 1: Mole Balances, Conversion & Reactor Sizing Topics to be covered

More information

IDEAL REACTORS FOR HOMOGENOUS REACTION AND THEIR PERFORMANCE EQUATIONS

IDEAL REACTORS FOR HOMOGENOUS REACTION AND THEIR PERFORMANCE EQUATIONS IDEAL REACTORS FOR HOMOGENOUS REACTION AND THEIR PERFORMANCE EQUATIONS At the end of this week s lecture, students should be able to: Differentiate between the three ideal reactors Develop and apply the

More information

Chemical Reaction Engineering - Part 12 - multiple reactions Richard K. Herz,

Chemical Reaction Engineering - Part 12 - multiple reactions Richard K. Herz, Chemical Reaction Engineering - Part 12 - multiple reactions Richard K. Herz, rherz@ucsd.edu, www.reactorlab.net Multiple reactions are usually present So far we have considered reactors in which only

More information

WINTER-15 EXAMINATION Model Answer

WINTER-15 EXAMINATION Model Answer Subject code :(735) Page of 9 Important Instructions to examiners: ) The answers should be examined by key words and not as word-to-word as given in the model answer scheme. ) The model answer and the

More information

Chemical Reaction Engineering

Chemical Reaction Engineering Lectue 3 hemical Reaction Engineeing (RE) is the field that studies the ates and mechanisms of chemical eactions and the design of the eactos in which they take place. Web Lectue 3 lass Lectue 9-Thusday

More information

Pre GATE Pre-GATE 2018

Pre GATE Pre-GATE 2018 Pre GATE-018 Chemical Engineering CH 1 Pre-GATE 018 Duration : 180 minutes Total Marks : 100 CODE: GATE18-1B Classroom Postal Course Test Series (Add : 61C, Kalusarai Near HauzKhas Metro, Delhi 9990657855)

More information

CHEMISTRY 107 Section 501 Final Exam Version A December 12, 2016 Dr. Larry Brown

CHEMISTRY 107 Section 501 Final Exam Version A December 12, 2016 Dr. Larry Brown NAME: (print) UIN #: CHEMISTRY 107 Section 501 Final Exam Version A December 12, 2016 Dr. Larry Brown This is a 2-hour exam, and contains 11 problems. There should be 14 numbered pages, including this

More information

CHAPTER 3 : MATHEMATICAL MODELLING PRINCIPLES

CHAPTER 3 : MATHEMATICAL MODELLING PRINCIPLES CHAPTER 3 : MATHEMATICAL MODELLING PRINCIPLES When I complete this chapter, I want to be able to do the following. Formulate dynamic models based on fundamental balances Solve simple first-order linear

More information

The Equilibrium Law. Calculating Equilibrium Constants. then (at constant temperature) [C] c. [D] d = a constant, ( K c )

The Equilibrium Law. Calculating Equilibrium Constants. then (at constant temperature) [C] c. [D] d = a constant, ( K c ) Chemical Equilibrium 1 The Equilibrium Law States If the concentrations of all the substances present at equilibrium are raised to the power of the number of moles they appear in the equation, the product

More information

P a g e What is the algebraic sign for enthalpy of solution? A. positive B. negative C. not enough information is given

P a g e What is the algebraic sign for enthalpy of solution? A. positive B. negative C. not enough information is given P a g e 1 Chem 123 Practice Questions for EXAM II Spring 2014 Exam II on Wed 3/12/14 This HAS BEEN updated after Monday s lecture (3/10/14) JUST studying these questions is not sufficient preparation.

More information

13 th Aug Chemical Reaction Engineering CH3010. Home work problems

13 th Aug Chemical Reaction Engineering CH3010. Home work problems 13 th ug 18. Chemical Reaction Engineering CH31. Home work problems 1. Batch reactor, variable volume. Consider a gas phase reaction B, conducted isothermally and at constant pressure in a batch reactor.

More information

CST Review Part 2. Liquid. Gas. 2. How many protons and electrons do the following atoms have?

CST Review Part 2. Liquid. Gas. 2. How many protons and electrons do the following atoms have? CST Review Part 2 1. In the phase diagram, correctly label the x-axis and the triple point write the names of all six phases transitions in the arrows provided. Liquid Pressure (ATM) Solid Gas 2. How many

More information

CHEMICAL EQUILIBRIUM. I. Multiple Choice 15 marks. 1. Reactions that can proceed in both the forward and reverse directions are said to be:

CHEMICAL EQUILIBRIUM. I. Multiple Choice 15 marks. 1. Reactions that can proceed in both the forward and reverse directions are said to be: Name: Unit Test CHEMICAL EQUILIBRIUM Date: _ 50 marks total I. Multiple Choice 15 marks 1. Reactions that can proceed in both the forward and reverse directions are said to be: A. complete B. reversible

More information

A First Course on Kinetics and Reaction Engineering Unit 19. Analysis of Batch Reactors

A First Course on Kinetics and Reaction Engineering Unit 19. Analysis of Batch Reactors Unit 19. Analysis of Batch Reactors Overview As noted in Unit 18, batch reactor processing often follows an operational protocol that involves sequential steps much like a cooking recipe. In general, each

More information

Review Sheet 6 Math and Chemistry

Review Sheet 6 Math and Chemistry Review Sheet 6 Math and Chemistry The following are some points of interest in Math and Chemistry. Use this sheet when answering these questions. Molecular Mass- to find the molecular mass, you must add

More information

Chem Hughbanks Final Exam, May 11, 2011

Chem Hughbanks Final Exam, May 11, 2011 Chem 107 - Hughbanks Final Exam, May 11, 2011 Name (Print) UIN # Section 503 Exam 3, Version # A On the last page of this exam, you ve been given a periodic table and some physical constants. You ll probably

More information

BAE 820 Physical Principles of Environmental Systems

BAE 820 Physical Principles of Environmental Systems BAE 820 Physical Principles of Environmental Systems Acquisition of reaction rate data Dr. Zifei Liu Uncertainties in real world reaction rate data Most interesting reaction systems involves multiple reactions,

More information

Thermodynamics 1. Hot Milk in a thermos flask is an example for 1) Isolated system ) Open system 3) Closed system 4) Adiabatic system. In open system, system and surroundings exchange 1) Energy only )

More information

CHEM Chapter 14. Chemical Kinetics (Homework) Ky40

CHEM Chapter 14. Chemical Kinetics (Homework) Ky40 CHEM 1412. Chapter 14. Chemical Kinetics (Homework) Ky40 1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO 2 (aq) + 2OH (aq) ClO

More information

Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set.

Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set. Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set. The symbols used here are as discussed in the class. Use scratch paper as needed. Do not give more than one answer for any question.

More information

The reactions we have dealt with so far in chemistry are considered irreversible.

The reactions we have dealt with so far in chemistry are considered irreversible. 1. Equilibrium Students: model static and dynamic equilibrium and analyse the differences between open and closed systems investigate the relationship between collision theory and reaction rate in order

More information