For each the following questions,choose one correct answer from the drop-down multiple choice menu box.The following data were obtained atconstant temperature for the reactionbelow:2A(g) + 3/2B(g)C(g)Rate = k[A]m[B]"%3DInitialInitialExperimentInitial rate[A][B](mol/L.s)(mol/L) (mol/L)10.25x10-45x10-25x10-222.25x10-4 15x10-25x10-20.50x10-45x10-210x10-2а)The reaction order with respect toA isb) !The reaction order with respect toBis

Given- Rate of reaction is given by, Rate = k[A]m[B]n data from experiments 1,2 and 3- 0.25 x 10-4 =…

Answered: For each the following questions,…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Q1
4- For the irreversible gas phase reaction A— 2B The following correlation was determined from laboratory data. The initial concentration of A is 0.2 gmol/litre. 1p+8 md.s For X 0.5; =3+10(X - 0.5) ~Ti mol The volumetric flow rate is 5 m¥s. a. Over what range of conversions are the plug-flow reactor and CSTR volumes identical? b. What conversion will be achieved in a CSTR that has a volume of 90 L? c. What plug-flow reactor volume is necessary to achieve 70% conversion? d. What CSTR reactor volume is required if effluent from the plug-flow reactor in part (c) is fed to a CSTR to raise the conversion to 90%? e. If the reaction is carried out in a constant-pressure batch reactor in which pure A is fed to the reactor, what length of time is necessary to achieve 40 % conversion?
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An isothermal reaction is run in both a 15 L PFR and a 15 L CSTR. The conversion in each reactor is measured to be 54%. It is suggested that this result means that the reaction is zeroth order in the reactants - that is, the reaction rate is not a function of conversion. Could this hypothesis explain the result? Suppose that you are to do an experiment to test this hypothesis, and that you have the ability to change the total volumetric flow rate of the feed stream prior to re-establishment of steady state. Explain how you would run this experiment and analyze the results to prove or disprove the hypothesis.
Hi, I need help with this, it was an activity done in class but I couldn't solve anything. From the following multiple reactions: (Reactions attached in the jpg file) If the initial concentration of A is 10 mol/L define the reaction rates of each species considering a batch reactor. For both reactions 1 and 2 obtain the dynamics of the concentrations of each species and discuss their behavior. a) Consider k1=k1=0.1 1 1/min and a time of 20 minutes. Explain the behavior of the concentrations for both reactions. b) Consider k1=0.2 and k2=0.3 1/min and a time of 20 minutes. Explain the behavior of the concentrations for both reactions. Justify your answer c) Consider k1=0.4 and k2=0.1 1/min and a time of 20 minutes. Explain the behavior of the concentrations for both reactions. Justify your answer. d) What happens if the concentration of A or the time of the process changes. Justify your answer.
Binary Distillation: The colum operates with a 1000 kgmoles/hr of a feed in which component A is the more volatile species. The feed q-value (thermal nature) is graphed as well and a specific reflux ratio designed and the appropriate operating line graphed. Solve d)
The irreversible reaction A - B was carried out in a batch reactor and the following concentration- time data were obtained as follows: to tz t3 ty Time (min) CA(mol/dm) 4 If the rate equation is expressed as : analysis to determine the kinetic constants k and 'n. 10 15 20 0.008 - rA=kC"A . Apply the differential method of 2.25 1 0.25
ot pt 1 pt 1 pt 1 pt 1 pt 1 pt 1 pt Z 40 what is the value of the rate constant? The decomposition of N₂O5 in CCl4 is a first-order reaction. If 1.47 mg of N₂O5 is present initially and 1.45 mg is present after 2.92 minutes at 55 °C, min-1 1 pt D Rate constant = Submit Answer W S Jull 3 X Alt E Try Another Version Q Search 14 с P % F 5 V FO 3 item attempts remaining G [References] SUS ZenBook as H N J S M Alt fuent Ctrl Home
A B Make a plot of equilibrium conversion as a function of temperature. i. ii. iii. Combine the rate law and stoichiometric table to write -гд as a function of k, CA, X and Xe. Determine the adiabatic equilibrium temperature and conversion when pure A is fed to the reactor at a temperature of 300 K. What is the CSTR volume to achieve 85% of the adiabatic equilibrium conversion for v₂ = dm³ ? 5 min Additional information: H°(298K)=-40 000 cal/mol H°(298K) = −60 000 cal/mol cal CpA = 50- mol. K CPB 50- cal mol. K 1 Kc 100 000 at 298 K, k = 10-3 exp - min with E = 10 000 cal/mol 298
PLEASE SOLVE WITH NUMERICAL INTEGRAL METHOD.
4
A junior engineer gave you a batch reactor data. y = 5.2143x + 1.4 R? = 1 InCb/Ca 18 17.0429 16 14 12 11.8286 10 "6.6143 • InCb/Ca 2 0.5 1 1.5 2.5 3.5 time You saw this and you immediately returned it and said "Repeat it! Idon't believe you." Why would you do this? (In cb)/CA 64

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