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Q1: 1. Your Biotech Company is interested in manufacturing catalyst particles to be used (suspended) in a stirred tank reactor. The manufacturing process will generate porous, cylindrically shaped particles (i.e. with a characteristic height - h, and radius-R) - which will allow for diffusion only through the end caps (i.e. axial, NOT radial diffusion). A local pharmaceutical company requests that you immobilize an enzyme that they use in the production of an antibiotic onto the internal surface (i.e. within the pores) of the cylindrical catalyst particles. When these catalyst particles are created, it is determined that standard Michaelis. Mention kinetics are observed, where: V (mol/m² s) = Vm"[S] / Km + [S] With and Vm" = 1 mol/m² min, defined per unit of catalyst surface area Km = 10 mol/l. The catalyst particle having a density of 1.4 g/ml and 2.0 m² of internal surface area per gram of catalyst particle. The concentration of substrate in the antibiotic production process is 0.25 mol/l. The effective diffusivity of the substrate in the interior of the catalysts is 1 x 10-⁹ m²/s. There is no enzyme bound to the exterior of the particle. The radius of the particles is 8mm. The conditions in the stirred tank are such that the bulk substrate concentration is equal to the substrate concentration at the entrance to the pores (i.e. no external mass transfer resistance), and is constant over time (i.e. CSTR). a.) Develop a differential equation that represents the conservation of substrate inside the catalyst particle. List the boundary conditions. b.) Make this differential equation dimensionless, and identify the Thiele modulus (and the parameters, such as De, that make it up). c.) Solve the dimensionless differential equation, obtaining the concentration profile of substrate versus position inside the catalyst particle. Apply the boundary conditions to obtain the specific solution. d.) Determine the relationship between the effectiveness factor and the Thiele modulus for this cylindrical catalyst particle, and plot this relationship. e.) Recommend the maximum particle length to use for the antibiotic production process, that ensures that the reaction is not significantly (i.e. less than 5% reduction from the max possible reaction rate) reduced by diffusional limitations inside the particle.See Answer
Q2:Exercise 1. An aqueous stream F of 0.11 kg/s comprises pyridine and water in equal weights. This stream should be purified in a countercurrent extraction process (see Figure 1). The concentration of pyridine in the raffinate RN should be reduced to 5 wt% (or less). Pure benzene is to be used as solvent S. The ternary equilibrium diagram of water-pyridine-benzene is given in Figure 2. a) Calculate the minimum solvent stream, Smin b) The solvent stream Sis chosen to be 0.11 kg/s. Determine the value of flow E₁ c) d) Determine the number of equilibrium separation stages, N. Determine the size and composition of the extract leaving the second stage, E₂, 17 ke/s. (c) Nr. = 3, (d) XSee Answer
Q3:Question A1 (25 marks). Your laboratory is studying a bioreaction which requires Mn²+ as a cofactor. In the presence of an excess of the cofactor, normal Michaelis-Menten kinetics is followed; however, Mn²+ in excess causes issues with scale formation and side redox processes. Decrease of the level of the cofactor, however, slows down the process. You are testing the following rate law: max [S] r = [S] + KM 1+ Kc [Mn²+] 1 1 Kc 1 [Mn²+] [S] r max The process was studied experimentally in a chemostat and the rate data in Table 1 were collected: max [S], mM r, mM-min-¹, great excess of Mn²+ r, mM-min-¹, [Mn²+] = 3 mM + , or in linear form, Км 1 + Table 1 20 0.35 0.21 40 0.54 0.36 60 0.63 0.50 (1) Here, [S] is the concentration of the substrate and r is the rate of the reaction. 80 0.70 0.55 a) Plot the data in coordinates 1/r vs. 1/[S]. Does the effect of the cofactor on the slope and the intercept agree with eq. (1)? [7 marks] b) Use the data in excess of Mn²+ to determine the values of the Michaelis constant KM and the maximal rate max of the uninhibited reaction. c) Determine the dissociation constant Kc of the enzyme-cofactor complex. [6 marks] [6 marks] d) The enzymatic fermenter is currently operating at [S] = 65 mM and [Mn²+] = 12 mM. Your team aims at decreasing Mn²+ to 5 mM, to avoid scaling. How much will the reaction rate drop? Suggest ways to compensate for this drop. [6 marks] Do not forget the units of each quantity you calculate; mark the units on the axes of your plot.See Answer
Q4:Question A2 (25 marks). The liquid phase reaction 2A → B is catalysed and follows the rate law rm = KAMCA². Here, Am is the specific area of the catalyst, and I'm is in mol-s-¹-(kg-cat)-¹. The process takes place in a packed bed reactor. a) Show that the design equation of the reactor is X= 2kAm Co 1+2kAm CAD/V Ao v where X is specified conversion, mc is the mass of catalyst in the reactor, v is feed flow rate. [9 marks] b) The catalyst slowly loses activity, due to sintering, abrasion and wash-off of the material. The sintering leads to linear drop of the specific area with time: Am = Amo(1-t/ts), where Amo is the initial specific area and ts is the characteristic time of the sintering process. The abrasion leads to a decrease of the mass of the catalyst, and is also linear with time: mc = moc(1-t/ta). By specification, the catalyst in the reactor has to be changed once its activity drops to 75% of its initial value. Find how often that is (i.e. design the schedule of catalyst refilling - the period to.75 between two changes). [8 marks] c) Since the reaction is 2nd order (i.e. the rate depends strongly on the concentration), an easy way to compensate for the loss of catalytic activity is by increasing the feed concentration of A with time. In order to stabilize the operation of the separation stages that follow the reactor, it is required that the conversion X is kept constant despite the loss of catalytic activity, by compensating the drop in mc and Am via a scheduled increase in the concentration CAO. Find what the schedule Cao(t) should be in order for X to remain constant. If CAO(t=0) = 0.5 M, what will CAO(t = to.75) be right before the change of catalyst? [8 marks]See Answer
Q5:Question B1 (50 marks). Dissolved Methylene Blue (MB) is adsorbed on a CaO photocatalyst under sun light. The results of a series of laboratory experiments using different amounts of the photocatalyst (indicated in grams in the graph) for a MB concentration of 10 mg/L are reported in figure 1. Removal (%) 100 80 60 40 20 200 400 600 == qt Time (min) Q1) comment the above results in view of potentially proposing a scale-up of the process. Make your own choice of catalyst concentration and briefly explain your decision. (you may choose any of the quantities represented in the plot providing your reasons are clearly explained). [20 Marks] 800 Q2) for your chosen concentration of the catalyst, make an estimate of the order of adsorption kinetics using the Lagergren model between the linearised equations below: k₁t 1st order: In(qe qt) = ln(qe) - 2.303 1 2nd order: k₂qć + - 0.05 g CaO/ 20 ml MB 0.2 g CaO/ 20 ml MB -0.4 g CaO/ 20 ml MB -0.6 g CaO/ 20 ml MB 1000 1200 1400 1600 qe Where qe and q are the amounts (mgMB Bat¹) of MB adsorbed on the catalyst at equilibrium and at time t (minutes), respectively, and k₁ and k₂ are the 1st and 2nd order kinetic constants, respectively. Take values from the above plotted results. Assume a 95% adsorption at equilibrium for all cases. [30 Marks]See Answer
Q6: To complete this solution, solve all the parts in sequence. For making plots use MatLab, Polymath or Excel as per your convince. • • Avoid submitting solutions from Al Write each and every explanation in detail Presentable skills helps to improve ratings and feedback ● Try to submit the solution in one pdf (Handwritten) • Separate software file needs to be uploaded Q1 The catalyst for the following reaction is in the form of 0.35 cm diameter spherical pellets. C+B+P The feed stock is pure C and the reactor operates at a pressure of 2 atm. The molecular weight of species C is 120.19 g/mol. The pellets have a specific surface area of 480 m²/g and a void volume of 0.42 cm³/g. The apparent first-order rate constant for this reaction is 1.49 cm³ /(s. 9 cat) at 412 C. What is the effectiveness factor of the catalyst?See Answer
Q7: To complete this solution, solve all the parts in sequence. For making plots use MatLab, Polymath or Excel as per your convince. • • Avoid submitting solutions from Al Write each and every explanation in detail Presentable skills helps to improve ratings and feedback ● Try to submit the solution in one pdf (Handwritten) • Separate software file needs to be uploaded Q2 Vanadium Pentaoxide can be used as a catalyst for the following reaction SO₂+02 → SO3 It was determined that the rate expression for this reaction is as follows: T= kps02 P12² 02 (1 + K₁Ps02)² where: and . k = 0.184 lb mol h-atm³/2 lbcat K₁ = 0.996 atm -1 lb-mol each, how many pounds of catalysts If SO2 and O2 are fed into the reactor at 100 h are need to reach 20% conversion if the reactor operates isothermally at 649 F and under constant pressure of 1 atm? See Answer
Q8: To complete this solution, solve all the parts in sequence. For making plots use MatLab, Polymath or Excel as per your convince. • • • Avoid submitting solutions from AI Write each and every explanation in detail Presentable skills helps to improve ratings and feedback Try to submit the solution in one pdf (Handwritten) Separate software file needs to be uploaded 1. Methyl ethyl ketone (MEK) is an important industrial solvent that can be produced from the dehydrogenation of butan-2-ol (Bu) over a zinc oxide catalyst. Bu → MEK + H₂ The following data giving the reaction rate for MEK were obtained in a differential reactor at 490 °C. PBu (atm) 2 0.1 0.5 1 2 1 PMEK (atm) 5 0 2 1 0 0 PH2 (atm) 0 0 1 1 0 10 Γ' ΜΕΚ 0.044 0.040 0.069 0.060 0.042 0.059 (mol/h-g-cat) a) Suggest a rate law consistent with the experimental data b) Suggest a reaction mechanism and rate-limiting step consistent with the rate law. Hint: Some species might be weakly adsorbed. c) Plot conversion and reaction rate as a function of catalyst weight for an entering molar flow rate of pure butan-2-ol of 10 mol/min at an entering pressure P0 = 10 atm. Please plot up to a 95% conversion of butan-2-ol. How much catalyst is required for this conversion?See Answer
Q9: To complete this solution, solve all the parts in sequence. For making plots use MatLab, Polymath or Excel as per your convince. • • Avoid submitting solutions from Al Write each and every explanation in detail Presentable skills helps to improve ratings and feedback • Try to submit the solution in one pdf (Handwritten) • Separate software file needs to be uploaded 1. (10 pt) Consider the following biochemical reactions that occur in an aqueous solution: S+E ES ES 2 P+E k₁ k-1 where E is a free enzyme that catalyses substrate S to produce product P. (1) a. (2 pt) Write the material balances for species S. E, ES, and P in a well-stirred batch fermenter. b. (2 pt) Denoting the time-dependent species concentrations as cs, CE, CES and cp, show that the total enzyme concentration is conserved: CE(t)+CES(t)=CE(0) + CES (0) = Eo c. (4 pt) Assume that k₁ »k-1,k2 such that Eo remains small. Show that with this assumption, the overall reaction SP has an effective rate constant r defined by Rp=r= μες 1+ Kcs' Rs = -r μ where and K depend on k₁, k-1, k2 and Eo. For full credit, you must find the expressions for u, K in terms of ki, k-1, k2, Eo. d. (2 pt) Solve numerically the full (part a) and reduced (part c) models to find CE(t), CES(t), cs(t), cp(t) for the following parameters (units: mole, liter, hour): CE (0) = 1, CES(0) = 0, cs(0) = 50, cp(0) = 0 k₁ =5, k11, k₂ = 10 Submit plots comparing concentrations vs. time for the full and reduced models.See Answer
Q10:Problem 1. The following table was obtained from the data taken in a slurry reactor for the hydrogenation of methyl linoleate to form methyl oleate. L+H₂ S = solubility of H2 in the liquid mixture, mol/dm³ m = catalyst charge, g/dm³ -r₁₁ = rate of reaction of methyl linoleate, mol/dm³/min Catalyst Size S/-r' (min) 1/m (dm³/g) A 4.2 0.01 A 7.5 0.02 B 1.5 0.01 B 2.5 0.03 B 3.0 0.04 a. Which catalyst size has the smaller effectiveness factor? b. If catalyst size A is to be used in the reactor at a concentration of 50 g/dm³, would a significant increase in the reaction be obtained if a more efficient gas sparger were used? c. If catalyst size B is to be used, what is the minimum catalyst charge that should be used to ensure that the combined diffusional resistances for the pellet are less than 50% of the total resistance?See Answer
Q11:Problem 2 The catalytic hydrogenation of methyl linoleate to methyl oleate was carried out in a laboratory-scale slurry reactor in which hydrogen gas was bubbled up through the liquid containing spherical catalyst pellets. The pellet density is 2 g/cm³. The following experiments were carried out at 25°C: Run Partial Pressure of H₂ (atm) Solubility of H₂ H₂ Rate of Reaction Catalyst (g mol/dm³) (g mol/dm³. Charge Catalyst Particle Size (g/dm³) (m) 1 3 0.007 min) 0.014 3.0 12 2 18 0.042 0.014 0.5 50 3 3 0.007 0.007 1.5 50 a. It has been suggested that the overall reaction rate can be enhanced by increasing the agitation, decreasing the particle size, and installing a more efficient sparger. With which, if any, of these recommendations do you agree? Are there other ways that the overall rate of reaction might be increased? Support your decisions with calculations. b. Is it possible to determine the effectiveness factor from the data above? If so, what is it? c. For economical reasons concerning the entrainment of the small solid catalyst particles in the liquid, it is proposed to use particles an order of magnitude larger. The following data were obtained from these particles at 25°C: Run 4 The Thiele modulus is 9.0 for the 750-μm particle size in run 4. Determine (if possible) the external mass transfer coefficient, kc, and the percent (of the overall) of the external mass transfer resistance to the catalyst pellet. Partial Pressure Solubility of H₂ H₂ Rate of Reaction (g mol/dm³. Catalyst Charge (g/dm³) Catalyst Particle Size 0.007 min) 0.00233 (μm) 2.0 750 of H₂ (atm) (g mol/dm³) 3See Answer
Q12:Problem 3 The hydrogenation of 2-butyne-1,4-diol to butenediol is to be carried out in a slurry reactor using a palladium-based catalyst. The reaction is first-order in hydrogen and in diol. The initial concentration of diol is 2.5 kmol/m³. Pure hydrogen is bubbled through the reactor at a pressure of 35 atm at 35°C. The equilibrium hydrogen solubility at these conditions is 0.01 kmol/m³, and the specific reaction rate is 0.048 m²/kg.kmol.s. The catalyst charge is 0.1 kg/m³ with a particle size of 0.01 cm and pellet density of 1500 kg/m³. a. Calculate the percent of the overall resistance contributed by each of the transport steps. b. Plot conversion as a function of time up to 95%. c. How could the reaction time be reduced? Additional Information: diffusivity = 10 m³/s for H₂ in organics k.a, = 0.3s¹¹ k = 0.005 cm/s for H, in organics k = 0.009 cm/s for 2-butyne-1,4-diol in butenediol pellet density = 1.6 g/cm³ pellet porosity = 0.45See Answer
Q13:Problem 3 Vanadium Pentaoxide can be used as a catalyst for the following reaction - S02+02SO3 It was determined that the rate expression for this reaction is as follows: r = kps02P1/2 (1 + K₁Ps02)² where: k = 0.184 lb mol h. atm³/2. lbcat and K₁ =0.996 atm If SO2 and O2 are fed into the reactor at 100 lb-mol each, how many pounds of catalysts h are need to reach 20% conversion if the reactor operates isothermally at 649 F and under constant pressure of 1 atm?See Answer
Q14:Need a lab report Write paragraphs in Abstract, introduction, Safety . And follow the experiment MEMO and the experiment procedure to know what data you should calculate.See Answer
Q15:Problem 4. Activation energy Razavi, Blagodatskaya, and Kuzyakox (2015) found the maximum rate of xylanase in soil samples at different temperatures. They used a sample size of 0.5 g of soil and an enzyme concentration of 1 umol, the results are in the following table: a) Calculate the values of KCAT and the energy of activation of the reaction.See Answer
Q16: 2. In this problem,biomass.we will analyze real data for a process to produce renewable chemicals from The reaction can be written R(a q)+H_{2}(g) \rightarrow P(a q) where R is the organic reactant and P is the product. This is an irreversible reaction. Reactions were carried out in a constant-volume stainless-steel, high-pressure batch reactor. The reactor was charged with 35-40 mL of the reactant solution (at a given concentration in water) and sealed. After removing air in the reactor with inert gas, pure H₂ gas was added to the reactor at room temperature (20 °C), filling the reactor gas head space (head space volume = 250 mL). Once the reactor was heated to reaction temperature, the concentration of the reactant R was monitored by taking samples from the reactor over time and analyzing their concentration by HPLC. R and P are dilute solutions in water, so you can ignore any changes in solution volume with time. The experimental data for this problem is in the attached Excel sheet. A platinum catalyst was used in all experiments, and the mass of catalyst used for each experiment is provided in the Excel file. In this problem, you will need to report reaction rates normalized per catalyst mass, in units of mol/hr/g catalyst. a) Compute the rate with units of mol/L/hr (from the concentration data), then use the provided liquid volume and catalyst mass to convert this to a rate per mass of catalyst (mol/hr/gcatalyst). Consider the following set of reaction conditions: Initial R concentration, CRO = 1500 mmol/L with a liquid volume of 40 mL Initial H₂ pressure, 1000 psig (charged at room temperature, 20 °C) with a headspace volume of 250 mL b) Which is the limiting reactant, R or H₂? Calculate the maximum conversion of the excess reactant. You can assume that the H₂ solubility in the liquid phase is negligible (i.e. the full amount of H₂ is in the gas phase). You should find that the excess reagent be treated as"differential" because its concentration does not change much during the experiment. The student running the experiments first wants to assess the reaction order with respect to H₂, so they keep temperature and CRO fixed and vary the H₂ pressure (Excel, experiments 1-3). Calculate the H₂reaction order using the differential method: c) Calculate the initial reaction rates ro (mol/hr/gecatalyst) for each p10 from the concentration vs time date d) Construct a log-log kinetic plot to calculate the H₂ reaction order. What is the H₂ reaction order? e) The student's supervisor suggests that they could speed up the rate of the reaction 3x by runningthe reaction at 3x higher H₂ pressures. Do you agree? Why or why not? Next, the student wants to assess the reaction order with respect to R, the liquid-phase reactant. They measured the concentration of R over time starting from an initial concentration of CRO= 752 mM (Excel,experiment 4). They hypothesize that this reaction is either 0, 1st, or 2nd order with respect to R. Gadsf) Fit their concentration vs time data to three integral kinetic models to determine which model best fits the data. Linearize all three models and show plots where the y-axis is a linearized function of concentration, the x-axis is time. g) Identify which of these three models best fits the experimental data and report the resulting rate constant with correct units (note that the rate should have unis of mol/hr/gcatalyst). You can ignore any terms associated with PH₂ in the rate equation because the pressure of H₂ is kept constant.. Next, the student, wants to assess the apparent activation energy, Eapp, so they keep the H₂ pressure and reactant concentration Cro fixed and vary the temperature (Excel, experiments 5-7). Note that the apparent activation energy is defined as dln(r)/d(). -h) Use the differential method to calculate the initial rate (mol/hr/gcatalyst) at each temperature i) Create an Arrhenius plot and use it to determine EappSee Answer
Q17: Consider the reaction of furfural (1) and butanol (2) reacting to form furfuryl alcohol (3) andbutyraldehyde (4). This reaction is important in the context of biomass upgrading, to form fuels andchemicals from platform molecules and is usually run in the liquid phase using an Mg6Al2O9 catalyst. Calculate the delta g° and the K of the reaction at 298 and at 433 K. Use data from NIST for enthalpies and entropies at 298 K. Remember, deltag° = deltah°-T deltasº. You may assume that the enthalpy change of the reaction is constant.i. ii.Calculate the deltag° and the K of the reaction at 298 and at 433 K using data from the Yaws handbook. Calculate the extent of the reaction at 433 K, if initially there are 2 mol of furfural and 1 mol of butanol in the system, assuming the system is an ideal solution of x1 = 0.2 and x2 = 0.1 in.toluene.See Answer
Q18: You will need the following data:R = 8.314 kPa L molK1I from the information above in KelvinV from the information above in LP in kPaNote: the units all have to be in the same form when used in calculations!!!100% H2O2 density is 1.45 g/mL5 mL of a solution containing an unknown concentration of hydrogen peroxide wasdecomposed at 25 °C releasing 48 mL of gas. The temperature of the container used to measure the volume of gas produced was 20 °C.To find BOTH the concentration of hydrogen peroxide in the solution AND the percentage of hydrogen peroxide in solution work through the following steps.1.Rearrange the ideal gas law to solve for n.2. Convert the temperature of the water in the collection vessel from °C to Kelvin (K). Therefore: T =3.Convert the current barometric pressure in the room from hPa to kPa. The Macquarie university weather station data can be used to find the pressure http://aws.mq.edu.au.Use the current pressure which is given in hectopascals. Use 1018 hPa if unavailable.10 hPa = 1 kPa So divide hPa by 10 to convert to kPa.Convert the volume of oxygen from mL to Liters and solve for the number of moles ofO2. Be sure the units cancel so that you end up with only the moles of O2. See Answer
Q19: 12. Plot the data above (volume vs time in sec) on graph paper and draw the line-of-best-fit through the first 3 or 4 of the data points.(Graph paper given. Label axes correctly)13. From the slope (rise over run) of this line of best fit what is the initial rate of reaction in mL O2 produced per sec.14. Convert this to mol/sec using the ideal gas law.15. Convert this to rate of reaction of hydrogen peroxide reacted per sec. (Hint: This will be twice the rate of oxygen production based on the stoichiometry as two H2O2 decompose to make one O2.) 16. Convert this to concentration of hydrogen peroxide reacted per second in the reaction(Assume the reaction volume is 10 mL and the units are mol L's').See Answer

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