9) The liquid-phase reaction A → B was carried out in a batch reactor initially charged with 3mol/L species A. The graph below contains linearized data from the reaction. Determine thereaction order and specific reaction rate constant and write out the full rate law. Note: youmust have correct units (mol, L, min) for full credit.8In(CAO/CA)4260020y= 0.1112x-0.0129R² = 0.9992406080t (min)

Reaction OrderSince the plot of ln(CA0/CA) vs t is a straight line, the reaction is first-order.…

Answered: 9) The liquid-phase reaction A → B was…

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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You are carrying out a reaction in the laboratory. You need to convert 1.00 mole of reactant X into products. This reaction shows first-order kinetics, and the reaction mixture has a constant volume of 1.00 L. At 1:00pm, you start the reaction at 25\deg C with 1.00 mole of reactant X. At 2:00pm, you find that 0.70 moles of reactant X remain. You immediately increase the temperature of the reaction mixture to 35\deg C. At 3:00pm, you discover that 0.25 moles of reactant X are still present. You want to be able to finish the reaction by 4:00pm, but you cannot stop the reaction until only 0.01 moles of reactant X remain. You must increase the temperature again. What is the minimum temperature required to complete the reaction by 4:00pm? (Remember, the reaction is complete when only 0.01 moles of X remain.)
A reaction of the type is carried out: A ---> B From the following data, determine the reaction order: Time (s) [A] (mol/L) 0 2.33 319 1.91 867 1.36 1198 1.11 1877 0.72
avoid typing the answers and kindly answer the question
gas phase reactionA -> B + Ccarried out isothermally in a constant volume batch reactor of 100 L. An amount of 100 moles of pure A is initially placed in the reactor. The reactor is well mixed and the ideal gas equation holds. If the reaction is first order,-rA = kCA with k = 1 1/sCalculate the time required to consume 80% (moles) of A.
For the following reaction set, define or propose two types of reactor systems to maximize product D selectivity, sketch the reactor system and describe clearly the input reactant concentrations and separation requirements if necessary. The unit of reaction rate is in units (mol/dm^3.sec) and concentration in units (mol/dm^3). (question on picture)
The decomposition of formic acid vapor according to the following reaction at 550oC follows a first-order kinetics, and at the above temperature, the reaction has a half-life of 240 s. HCO2H (g) ® CO2(g) + H2(g); Rate = k[HCO2H] If the initial concentration of HCO2H was 0.160 M, what is its concentration after four half-lives? (A) 0.010 M (B) 0.020 M (C) 0.040 M (D) 0.0050 M
Please correct answer and don't use hand rating
2. The reaction A → B is to be carried out in a flow reactor. Data for the reaction is given below. You have two CSTRs and two PFRS, each with a volume of 2 L. ΧΑ FAO-TA (L) 0.0 1.112 0.1 1.363 0.2 0.4 1.663 2.563 0.6 4.425 Calculate the conversion for each reactor in the following arrangements: a. Two CSTRS in series 0.7 0.8 6.325 10.0 b. Two PFRs in series c. Two CSTRs in parallel with the feed, FA0, divided equally between the two reactors. d. Two PFRs in parallel with the feed divided equally between the two reactors. e. A CSTR followed by a PFR f. A PFR followed by a CSTR g. A PFR followed by two CSTRS
The equilibrium constant, K. for the following reaction is 9.52×102 at 350 K. CH4 (g) + CCl, (g) =2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.299 moles of CH4 and 0.299 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] [ CC4 ] [ CH,Cl, ] = | M M M

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