CHE 425. Engineering Economics and Design Principles. Prof. Adnan Alamer Chemical Engineering Dept., KFUPM.

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

Level 2: Input output structure

Chemical Reaction Engineering. Multiple Reactions. Dr.-Eng. Zayed Al-Hamamre

Second Law of Thermodynamics

Fundamentals of Combustion

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

Summary for TEP 4215 E&P/PI

Reactors. Reaction Classifications

Exercise 1. Material balance HDA plant

SKF4153 PLANT DESIGN PROCESS SYNTHESIS & CREATION. Prof. Dr. Zainuddin Abdul Manan Ir. Dr. Sharifah Rafidah Wan Alwi

Chemical Equilibrium

CBE 142: Chemical Kinetics & Reaction Engineering

Separations and Reactors Design Project. Production of Allyl Chloride

Process Design Decisions and Project Economics Prof. Dr. V. S. Moholkar Department of Chemical Engineering Indian Institute of Technology, Guwahati

Exercise 1. Material balance HDA plant

Stoichiometric Reactor Module

Process Design Decisions and Project Economics Prof. Dr. V. S. Moholkar Department of Chemical Engineering Indian Institute of Technology, Guwahati

Web Solved Problems Web Example SP-8.1 Hydrodealkylation of Mesitylene in a PFR CH 3 H 2. m-xylene can also undergo hydrodealkylation to form toluene:

Process Classification

Equilibrium and Reversible Rxns. CHAPTER 14 Chemical Equilibrium. What happens? Stoichiometry

Reactions and Reactors

Reaction rate. reaction rate describes change in concentration of reactants and products with time -> r = dc j

A First Course on Kinetics and Reaction Engineering Example 1.2

Chemistry 1A, Spring 2008 Midterm Exam III, Version A April 14, 2008 (90 min, closed book)

Chemical Equilibrium. Chapter

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

Chapter 17.3 Entropy and Spontaneity Objectives Define entropy and examine its statistical nature Predict the sign of entropy changes for phase

Process design decisions and project economics Dr. V. S. Moholkar Department of chemical engineering Indian Institute of Technology, Guwahati

Unit 12. Thermochemistry

Chemical Equilibrium Examples

What is a spontaneous reaction? One, that given the necessary activation energy, proceeds without continuous outside assistance

Heating value, adiabatic flame temperature, air factor

Chemistry 163B. Thermochemistry. Chapter 4 Engel & Reid

Exothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (l) + energy

Lecture (9) Reactor Sizing. Figure (1). Information needed to predict what a reactor can do.

Chapter 19 Chemical Thermodynamics Entropy and free energy

Thermodynamic Connection

3 A (aq) + 2 D (aq) + 5 C (s) <==> 3 B (aq) + 4 E (aq) + 2 G (ppt)

CHM 112 Chapter 16 Thermodynamics Study Guide

Ch 6. Energy and Chemical Change. Brady & Senese, 5th Ed.

Distillation Course MSO2015

Characteristics of Chemical Equilibrium. Equilibrium is Dynamic. The Equilibrium Constant. Equilibrium and Catalysts. Chapter 14: Chemical Equilibrium

(g) + 3 H 2. (g) 2 NH 3. 1) Only gases and dissolved species appear in an equilibrium expression. 4 NH 3. O(g) K c = (s) + 2N 2.

Chapter Eighteen. Thermodynamics

Chemistry 1A, Fall 2009 Midterm Exam #3 November 10, 2009 (90 min, closed book)

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

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

Separation Trains. Sieder et. al. Chapter 9 and 13. Terry A Ring Chemical Engineering University of Utah

Chapter 6: Thermochemistry

Chapter Outline. The Dynamics of Chemical Equilibrium

2017 AP Chemistry Sample Student Responses and Scoring Commentary Inside: Free Response Question 2 Scoring Guideline Student Samples

Review Unit #11. Review Unit # H 2 O (g) + CO (g) H 2(g) + CO 2(g) H>1

There are five problems on the exam. Do all of the problems. Show your work

(i.e., equilibrium is established) leads to: K = k 1

Solutions to: Thermodynamics HomeworkProblem Set S.E. Van Bramer 1/11/97

Name. Chem 116 Sample Examination #2

UNIT 15: THERMODYNAMICS

Thermodynamics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

ASSIGNMENT SHEET #11 APQ ANSWERS

1. Entropy questions: PICK TWO (6 each)

Thermochemistry. Chapter Energy Storage and Reference. 4.2 Chemical Rxns. 4.3 Hess s law Overview

Chapter Objectives. Chapter 9 Energy and Chemistry. Chapter Objectives. Energy Use and the World Economy. Energy Use and the World Economy

e) KC = [H + ] [HCOO - ] Kp = no expression [HCOOH]

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

1.8. ΔG = ΔH - TΔS ΔG = ΔG + RT ln Q ΔG = - RT ln K eq. ΔX rxn = Σn ΔX prod - Σn ΔX react. ΔE = q + w ΔH = ΔE + P ΔV ΔH = q p = m Cs ΔT

2012 AP CHEMISTRY FREE-RESPONSE QUESTIONS

Chemical Kinetics and Reaction Engineering

Thermochemistry. Chapter Energy Storage and Reference. 4.2 Chemical Rxns. 4.3 Hess s law Overview

Thermodynamics and Equilibrium. Chemical thermodynamics is concerned with energy relationships in chemical reactions.

3 A (aq) + 2 D (aq) 4 C (g) + B (s) + 2 E (l)

Chemical Equilibrium Basics

Chapter 6 Energy and Chemical Change. Brady and Senese 5th Edition

1.8. ΔG = ΔH - TΔS ΔG = ΔG + RT ln Q ΔG = - RT ln K eq. ΔX rxn = Σn ΔX prod - Σn ΔX react. ΔE = q + w ΔH = ΔE + P ΔV ΔH = q p = m Cs ΔT

The Laws of Thermodynamics

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

Kc is calculated for homogeneous reactions using the concentrations of the reactants and products at equilibrium:

How can we use the Arrhenius equation?

Lecture 2. Review of Basic Concepts

Chemical Process Industries Ch.E-203

CHAPTER THERMODYNAMICS

Chemistry 103 Spring Announcements 1. Ch. 16 OWL homework is active. 2. Next midterm exam on May 17 or 19.

CHEMISTRY. Chapter 15 Chemical Equilibrium

Chemical Equilibria 2

Chemical Reaction Engineering. Lecture 2

INTRODUCTION TO CHEMICAL PROCESS SIMULATORS

CHEM 1423 Chapter 17 Homework Questions TEXTBOOK HOMEWORK

Chapter 11 Spontaneous Change and Equilibrium

The Reaction module. Table of Contents

Chapter 5. Thermochemistry

Equilibrium. Reversible Reactions. Chemical Equilibrium

_ + Units of Energy. Energy in Thermochemistry. Thermochemistry. Energy flow between system and surroundings. 100º C heat 50º C

aa + bb ---> cc + dd

OHIO ASSESSMENTS FOR EDUCATORS (OAE) FIELD 009: CHEMISTRY

Fundamentals of Material Balances

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

First Law of Thermodynamics. Example of Spontaneous Rxns. Reversible and Irreversible 8/2/2016

CEE 370 Environmental Engineering Principles. Equilibrium Chemistry

TODAY 0. Why H = q (if p ext =p=constant and no useful work) 1. Constant Pressure Heat Capacity (what we usually use)

Downloaded from

Chemical Kinetics. What Influences Kinetics?

Transcription:

CHE 425 Engineering Economics and Design Principles 1

CHAPTER 4 Understanding Process Conditions 2

The ability to make an economic analysis of a chemical process based on a PFD is not proof that the process will actually work. 3

PURPOSE OF CHAPTER 4 Analyze reasons for selecting specific conditions: Temperatures Pressures Compositions Analyze process conditions that require special consideration 4

CONDITIONS OF SPECIAL CONCERN It is easier to adjust T and/or P of a stream than to change composition. The following conditions do not cause severe difficulties Temperatures between 40-260 C Pressures between 1-10 bar Conditions outside the above favored temperature and pressure ranges are identified as conditions of special concern 5

PRESSURE Above 10 bar Thicker walled expensive equipment Safety issue 1-10 bar Favorable condition Large equipment Below 1 bar Special construction material Increase in cost 6

PRESSURE (cont.) A decision to operate outside the pressure range of 1-101 10 bar must be justified 7

TEMPERATURE (cont.) 8

TEMPERATURE (cont.) 9

TEMPERATURE (cont.) A decision to operate above 400 C must be justified 10

TEMPERATURE (cont.) Below 40 C 40-260 C Above 260 C Require refrigeration Okay Require special heaters 11

TEMPERATURE (cont.) T < 40º C Refrigeration Use as much Cooling Water as Possible CW RW Operating Costs(Table 3.4) Cooling Water Refrigerated Water $0.16/ GJ $20.60/ GJ 12

Do we ever operate outside these limits? Tables 4.1 4.3 Reactors and Separators Table 4.4 Other Equipment DME Process pretty much inside limits 13

REASONS FOR OPERATING AT CONDITIONS OF SPECIAL CONCERN Favorable equilibrium conversion Increase in reaction rates k reaction = k e 0 E act RT Maintain a gas phase Improve selectivity 14

Table 4.1 15

Table 4.1 (cont.) 16

Table 4.2 17

Table 4.2 (cont.) 18

Table 4.3 19

Table 4.3 (cont.) 20

Table 4.4 21

Table 4.4 (cont.) 22

Table 4.4 (cont.) 23

Example 4.2 24

Example 4.2 (cont.) 25

Example 4.2 (cont.) 26

Example 4.2 (cont.) 27

Process Conditions Matrix (PCM) 28

Process Conditions Matrix (PCM) (cont.) 29

Evaluation of Reactor R-101 Three conditions of concern High Temperature High Pressure Non-stoichiometric Feed Conditions 30

Additional Information about toluene HDA reaction 31

Reactor Analysis 32

33

34

Thermodynamic Consideration High temperature concern Fig 4.1 implies the rxn is exothermic For exothermic rxn,, as T, Xeq Decrease in Xeq is undesirable Use of high T cannot be justified from thermodynamic point of view 35

Thermodynamic Consideration (cont.) High pressure concern Rxn stoichiometry shows that there are equal number of reactant and product moles in the HDA rxn. Thus, no effect of pressure on Xeq No reason to use high P from thermodynamic point of view 36

Example 4.3 37

Example 4.3 (cont.) 38

Example 4.4 39

Conclusions T < 40ºC Refrigeration T > 250ºC Fired Heater or Furnace T > 400ºC M.O.C. Issues P < 1 atm Vacuum and Large Equipment P > 10 atm Cost 40

SUMMARY Wall Thickness Increases 10 atm 1 atm Requires Refrigeration Requires Fired Heater Requires Special M.O.C. 40º C 250º C 400º C Vacuum Chemical Large Engineering Equipment Dept., KFUPM. 41