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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 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
Q4: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
Q5: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
Q6: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
Q7: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
Q8: 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
Q9: 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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