Principles of
Chemical Engineering
Department of Chemical Engineering
CHEG 1001
Semester 2
chapter 1
Dr Mohamed G Hassan Sayed
Dr Giuseppe Pileio
Dr Nuno bimbo
Mr Colin M Flowers
Your CHEG1001 lecturers
Mr Colin M Flowers
C.M.Flowers@soton.ac.uk
Dr Mohamed Hassan
mghs1v19@soton.ac.uk
Department of Chemical Engineering
Dr Nuno bimbo
n.bimbo@soton.ac.uk
Dr Giuseppe Pileio
G.Pileio@soton.ac.uk
What is Chemical Engineering?
“is
the
application
of
science,
mathematics and economics to the
process of converting raw materials or
chemicals into more sustainable forms.
The terms economics & sustainability are
very important here” (IChemE)
Department of Chemical Engineering
More than just process engineering – to
apply specials technical knowledge to
address implant the SDGs on time and
over come the challenges of the future
•Work with unit
operations
• purposes of chemical synthesis and/or separation (chemical reaction, mass-,
heat- and momentum- transfer operations)
• conservation of mass, energy and momentum
Apply physical
laws
• thermodynamics, reaction kinetics and transport phenomena
Apply principles
• design & operate processes
Solve problems
1.
Core of chemical engineering deals with conversion of raw materials to useful products; finding the optimal synthesis routes and
operating the processes for their designed applications, and through the use of science, mathematics, economics, ….
2.
The core, needs to be enhanced by suitable levels of science and engineering to find sustainable and innovative solutions.
3.
The inclusive goals are to assist societal needs through teaching the engineers to apply their education-training for industrialized
development captivating advantage of the opportunities and addressing the challenges of the future
Grand challenges-opportunities
Sustainable solutions (water, energy, resources)
Processing Routes
(reaction; separation; mixing;
heating-cooling; etc.)
Innovative solutions (process, product)
Application (industrial development)
Society
Products
(needs)
Raw Materials
(resources)
Engineering
Science
Education
Department of Chemical Engineering
Operation/Design
(production)
Breadth Of Sustainability
• This way of looking at the (sustainable
development goals (SDGs) links back to the three
pillars idea and that sustainability is made up of
environmental/biosphere, social/society, and
economic/economy factors.
Department of Chemical Engineering
• This also shows that the economy only exists
within society, and likewise, society within a
functioning biosphere – in the same way as we
need all three pillars we also need a healthy
biosphere and a healthy society to enable a
healthy economy to exist
• Partnership is shown as the ‘golden thread’
throughout all three – much like Responsible
Futures! Partnership is at the core of success in
achieving sustainability aims.
Chemical engineering/process engineering
Pollution emissions
Minerals
Gasoline,
diesel
Fossil fuel
Fertilizers
plants
Chemical
reaction
Food,
leather
Department of Chemical Engineering
Animals
Unit operation
Hydrogen
water
Nitrogen
air
Resources
Processes
Products
Sustainable chemical/process engineering
Sustainable use of
natural resources
Department of Chemical Engineering
Sustainable
chemicals
Sustainable
development and
environment
Sustainable processes with
minimized pollution emission
Sustainable energy and
food systems
PROCESS INDUSTRY
REDUCE
Within the existing installed base of industrial processes
Department of Chemical Engineering
• Reduce feedstock: enhance the availability and quality of existing
resources
• Reduce emissions
• Reduce energy and water: integrated use, new materials
• Reduce, prevent waste
PROCESS INDUSTRY
RE-USE
Within the existing installed base of industrial processes
Department of Chemical Engineering
• Re-use
energy
within
and
between
energy harvesting, storage and re-use
different
sectors:
• Re-use water within the sector and within the area
• Re-use waste streams as feed, including recovery, recycling and
re-use of post-consumer waste; waste system approach – new business
models
PROCESS INDUSTRY
REPLACE
Within the existing installed base of industrial processes
Department of Chemical Engineering
• Replace current feedstock by integrating novel and renewable feedstock
(such as bio-based) to reduce dependency while reducing the CO2 footprint
of processes or increase the efficiency of primary feed stock.
• Replace current inefficient processes
PROCESS INDUSTRY
RE-INVENT
Rejuvenate & invest in industrial processes
• (Re-)invent feedstock
Department of Chemical Engineering
• (Re-)invent more efficient equipment
• (Re-)invent devices for better monitoring, control & optimisation
• (Re-)invent energy & resource mngt. concepts, incl. industrial symbiosis
• (Re-)invent materials & products with a significantly increased impact on resource
& energy efficiency down the value chain: transport, housing
• (Re-)invent technologies for valorisation of waste streams
CHEG 1001
Department of Chemical Engineering
Module overview
This module covers the chemical aspects of thermodynamics, equilibria, and kinetics, with a focus
on their relationship to mass and energy balances and application of the concepts of physical
chemistry in chemical engineering.
Learning
Outcomes
•Use phase diagrams thermodynamic data tables to describe and analyse the properties of single
and multi-component chemical systems.
•Determine the order of a chemical reaction and write expressions for the rate law, explaining the
effects of temperature on the rate constants and outcome of the reaction.
•Calculate the equilibrium constant for a chemical process and describe the effects of changes in
conditions (temperature, pressure, and composition) on the value of the equilibrium constant.
•Describe and calculate the thermodynamic variables (enthalpy, entropy, internal energy, Gibbs
energy, and Helmholtz energy) that describe chemical reactions and transformations.
•Perform mass and energy balance calculations representative of chemical processes.
Four
practical 1. Process enthalpies;
exercises
2. Energy balances/heat transfer;
3. Temperature dependence of vapour pressure of a liquid;
4. Determination of reaction order.
Assessment
Laboratory Exercises
Final Exam
50%
50%
Course content – Dr Hassan Week 18-21 and 25
Department of Chemical Engineering
1.
2.
3.
4.
5.
6.
Engineering problem analysis.
What some chemical engineers do for a living.
Introduction to engineering calculations.
Processes and process variables.
Fundamentals of material balances
Material balances in Single-Phase Systems & Multiphase Systems
Course content – Dr Giuseppe Pileio Week 22-25
Department of Chemical Engineering
1.
2.
3.
4.
5.
6.
1st law of Thermodynamics (internal energy, work, heat)
Enthalpy and heat capacities
Entropy and 2nd law of Thermodynamics
Gibbs Energy
Phase diagrams
Phase transitions
Course content – Dr Nuno Bimbo, weeks 30 - 33
Department of Chemical Engineering
1.
2.
3.
4.
5.
Energy and enthalpy
Energy balances
Energy balances on closed and open systems
Balances on reactive and non-reactive processes
Balances on transient processes
Course content – Practical's (Colin Flowers)
The practical element for this course is based on the undertaking of a series of
4 x 4 hour practical's:
Department of Chemical Engineering
1. Measurement of process (i.e. Reaction, Sublimation, Fusion, Solution)
enthalpies – Utilizing calorimetric equipment.
2. Energy balances/heat transfer – Utilizing heat exchangers.
3. Temperature dependence of the vapour pressure of a liquid.
4. Determination of reaction order – Utilizing colorimetric monitoring of
reaction rate.
Assessment will be via post-lab reports.
Refer to your online timetable for details of the scheduling of your practical
sessions.
Reference Books for CHEG 1001
Mohamed the course is from “Elementary principles of chemical
processes” Chapter 1-5 Richard Felder
Department of Chemical Engineering
Peppe Elements of Physical Chemistry, P. Atkins, J. de Paula, Oxford
University Press
Nuno Main textbook is also “Elementary Principles of Chemical
Processes” from Felder, Rousseau and Bullard, Chapters 7 – 10
Introduction to
Engineering Calculations
Department of Chemical Engineering
Ch2
Material and Energy Balances
Objectives
• Convert a quantity expressed in one set of units into
Department of Chemical Engineering
its equivalent in any other dimensionally consistent
units.
• Identify common SI, CGS, and American Engineering
units.
• Understand and apply the concept of significant
figures.
Units and Dimensions
• A measured or counted quantity has a numerical value and a unit. In
most engineering calculations, it is essential to include both when
expressing this quantity (e.g., 2 seconds, 0.5 grams, 3 students).
Department of Chemical Engineering
• A dimension is a property that can be measured.
• time, length, mass, temperature
• or calculated by multiplying or dividing dimensions
• velocity (length/time), density (mass/length3)
Units and Dimensions
• The numerical values of two quantities may be added or subtracted
ONLY if the units are the same:
3 apples + 2 apples = 5 apples
3 apples + 2 oranges = ?
Department of Chemical Engineering
• Numerical values and their corresponding units may always be
combined by multiplication or division.
3.0 grams / 1.5 cm3 = 2.0 g/cm3
4.0 hours × 55 miles/hour = 220 miles (2.2×102 miles)
1.0 kg × 9.8 m/s2 = 9.8 kg m/s2 = 9.8 N
(5.0 kg/s) / (0.20 kg/m3) = 25 m3/s
Conversion of Units
Department of Chemical Engineering
• A measured quantity can be expressed in terms of any units having
the appropriate dimension.
• The equivalence between two expressions of the same quantity may
be defined in terms of a ratio, known as a conversion factor.
• examples of conversion factors with equivalent numerators and
denominators
3600

 1 h


s  24 h  365 day 
 

 
1
day
1
yr
 

 


 1 m   1 km 
 2
  3 
10 cm  10 m 


10 3 m 


 1 km 


Systems of Units
• Base units
• mass, length, time, temperature, electrical current, light intensity
• Multiple units
• defined as multiples or fractions of base units (minutes and hours are
multiples of the unit second)
Department of Chemical Engineering
• Derived units
• compound units obtained by multiplying and/or dividing base or multiple
units
• defined as equivalents of compound units
e.g., 1 erg ≡ 1 g·cm/s2
Units and Dimensions
Department of Chemical Engineering
Units and Dimensions
Department of Chemical Engineering
Units and Dimensions
Department of Chemical Engineering
Systems of Units
• SI (Système Internationale d’Unités)
• internationally accepted system of units
• meter (length), kilogram (mass), second (time), Kelvin (temperature), ampere
(electric current), candela (luminous intensity)
• CGS
Department of Chemical Engineering
• identical to SI, with g and cm replacing kg and m as base units for mass and
length, respectively.
• American engineering system
• foot (length), pound-mass (mass), second (time)
• conversions not based on multiples of ten
Conversion Factors
• Sources of unit conversion factors
• Perry’s Chemical Engineers’ Handbook
• Mathcad
• Onlineconversion.com
Department of Chemical Engineering
• Process of converting units
• unit conversion factors may be found in tables or from electronic resources.
• the process of converting units may be performed manually or electronically.
• It is expected that you will be capable of either.
Examples unit conversions
2 to km/yr2
• convert acceleration
unit
of
cm/s
2
2 
2 2  2 2 



cm 3600 s
365 day
24 h



1


 2  2 2  2
 2 2
 s  1 h 1 day2 
 1 yr

Department of Chemical Engineering

• convert

1 km 
9 km


9.95
10
 3 
10 2 cm 
10 m 
yr 2

1m





3
density
units
of
lb
/gal
to
kg/m
 lb  264 gal  0.454
m kg 
m
2 kg
1
 

1.20

10



 gal   1 m3   1 lb m 
m3



Force and Weight
• Newton’s 2nd law of motion defines force (F) to be proportional to the
2),
 mg
product of mass (m) and acceleration (a, Flength/time
Department of Chemical Engineering
• SI:
• CGS:
• AES:
kg⋅m/s2 ≡ 1 newton (N)
g⋅cm/s2 ≡ 1 dyne (dyne)
32.174 lbm⋅ft/s2 ≡ 1 pound-force (lbf)

• gc is used to denote conversion factor from natural to derived force
units
1 kg  m s2 32.174 lb m  ft s2
gc 

1N

1 lb f
Force and Weight
• The weight (W) of an object of mass (m) is the force exerted on the
object by gravitational attraction,
W  mg
Department of Chemical Engineering
• where the gravitational acceleration (g) varies with the mass of the
attracting body (which
will
be
the
Earth
in
most
cases
in
this
course).

2
9.8066 m/s .
Scientific Notation
• Scientific notation is a convenient means to express very large and
very small numbers as a product of ten raised to a power.
• 123,000,000 = 12.3×107 = 1.23×108 = 0.123×109
• 0.000028 = 0.28×10-4 = 2.8×10-5 = 28×10-6
Department of Chemical Engineering
• Standard scientific notation form is written such that there is one digit
to the left of the decimal.
• Engineering scientific notation form is written such that the exponent
is a factor of 3.
Significant Figures
• The significant figures (sig figs) of a number are the digits from the
first nonzero digit on the left to either
• last digit (zero or non) on the right if there is a decimal, or
• last nonzero digit of a number if there is no decimal.
Department of Chemical Engineering
•
•
•
•
•
•
2300 or 2.3×103 has 2 sig figs
2300. or 2.300×103 has 4 sig figs
2300.0 or 2.3000×103 has 5 sig figs
23,040 or 2.304×104 has 4 sig figs
0.035 or 3.5×10-2 has 2 sig figs
0.03500 or 3.500×10-2 has 4 sig figs
• note the convenience of using scientific notation for expressing significant
figures
Process Variables
Department of Chemical Engineering
PENG 373
Ch3
Material and Energy Balances
Mass and Volume
• The density of a substance is the mass per unit volume of that
substance. The specific volume of a substance is the volume occupied
by a unit mass of that substance, the inverse of the density.
Department of Chemical Engineering
• Densities of pure solids and liquids are essentially insensitive to
pressure, and vary relatively slightly with temperature.
Mass and Volume
• Density of a pure substance can be used as a conversion factor to
relate the mass and volume of a quantity of that substance.
• e.g., 20 cm3 of carbon tetrachloride
1.595g
20 cm 
 31.9 g
3
1 cm
3
Department of Chemical Engineering
• or 6.20 lbm of carbon tetrachloride
454 g 1 cm3
6.20 lbm 

 31.9 cm3
1 lbm 1.595g
Mass and Volume
• The specific gravity (SG) of a substance is the ratio of the density (ρ)
of the substance to the density of a reference substance at a specific
condition (ρref).
• The most common reference for solids and liquids is water at 4.0°C,
which has the following density:
Department of Chemical Engineering
• 1.000 g/cm3 = 1000 kg/m3 = 62.43 lbm/ft3
• The density of a liquid or solid in g/cm3 is numerically equal to the SG
of that substance.
• The notation SG = 0.6(20°/4°) signifies that the specific gravity of a
substance a 20°C with reference to water at 4°C is 0.6.
Mass and Volume
• A thermometer uses mercury, the volume of which changes with
temperature.
• Read the book to understand the correlation alternatively you should
have done this FEEG units
Department of Chemical Engineering
Flow Rate
𝑁 mol fluid/s
Department of Chemical Engineering
Flow Rate
Department of Chemical Engineering
• The flow rate of a process stream can be expressed as a mass flow
rate (mass/time) or as a volumetric flow rate (volume/time).
• Density can be used as a conversion factor between. mass and
m m
volumetric flow rate.
  .
V V
• The mass flow rate of n-hexane (ρ=0.659 g/cm3) in a pipe is 6.59 g/s.
What is the volumetric flow rate of n-hexane?
g
.
6.59
. m
s
cm 3

V 
 10.0 s
g
 0.659
cm 3
Flow Rate Measurement
• A flowmeter is a device mounted in a process line that provides a
continuous reading of the flow rate in that line.
• Two common flowmeters are the rotameter and the orifice meter.
Department of Chemical Engineering
Chemical Composition
Department of Chemical Engineering
• atomic weight – weight of an atom of an element on a scale by which
12C has a mass of exactly 12.
• molecular weight –sum of the atomic weights of the atoms that
constitute a molecule of the compound.
MW is a conversion factor between mass and moles for a particular
compound.
• gram-mole – the amount of that species whose mass in grams is
numerically equal to its molecular weight.
Conversion: Mass/Moles
Department of Chemical Engineering
• Consider 8-methyl-N-vanillyl-trans-6-nonenamide, also known as
capsaicin,
the active component of
chili peppers, having a
molecular formula of C18H27NO3
• Calculate the molecular weight of capsaisin.
C
18  12.0107
+
H
27  1.00794

O
3  15.9994

N
1  14.0067
= 216.193 + 27.2144 + 47.9982 + 14.0067 = 305.412

g
C18H27 NO3
gmol
Conversion: Mass/Moles
Department of Chemical Engineering
• Consider 8-methyl-N-vanillyl-trans-6-nonenamide, also known as
capsaicin,
the active component of
chili peppers, having a
molecular formula of C18H27NO3
• Calculate the number of moles of capsaicin in 100 g of the
substance…
100 g C18H27 NO3 

gmol C18H27 NO3
 0.327426 gmol C18H27 NO3
305.412 g C18H27 NO3
Conversion: Mass/Moles
Department of Chemical Engineering
• Consider 8-methyl-N-vanillyl-trans-6-nonenamide, also known as
capsaicin,
the active component of
chili peppers, having a
molecular formula of C18H27NO3
• Calculate the number of lbmoles of capsaicin in 100 g of the
substance…
100 g C18H27 NO3 

gmol C18H27 NO3
lbmol

 7.218  10 4 lbmol C18H27 NO3
305.412 g
453 .6 gmol
Conversion: Mass/Moles
Department of Chemical Engineering
• Consider 8-methyl-N-vanillyl-trans-6-nonenamide, also known as
capsaicin,
the active component of
chili peppers, having a
molecular formula of C18H27NO3
• Calculate the number of moles each element in 100 g of the
substance…
gmol C18H27 NO3
18 gmol C
100 g C18H27 NO3 
100 g C18H27 NO3 

305.412 g

1gmol C18H27 NO3
 5.89367 gmol C
gmol C18H27 NO3
27 gmol H

 8.84051 gmol H
305.412 g
1gmol C18H27 NO3
Conversion: Mass/Moles
Department of Chemical Engineering
• Consider 8-methyl-N-vanillyl-trans-6-nonenamide, also known as
capsaicin,
the active component of
chili peppers, having a
molecular formula of C18H27NO3
• Calculate the number of grams of C in 100 g of the substance…
100 g C18H27 NO3 

gmol C18H27 NO3
18 gmol C
12.0107 g C


 70.7871 g C
305.412 g
1 gmol C18H27 NO3
1 gmol C
Conversion: Mass/Moles
Department of Chemical Engineering
• Consider 8-methyl-N-vanillyl-trans-6-nonenamide, also known as
capsaicin,
the active component of
chili peppers, having a
molecular formula of C18H27NO3
• Calculate the number of molecules of capsaicin in 100 g of the
substance…
gmol C18H27 NO3 6.02 10 23 molecules C18H27 NO3
100 g C18H27 NO3 

305.412 g
1 gmol C18H27 NO3
 1.97 10 23 molecules C18H27 NO3

Mass and Mole Fractions
Department of Chemical Engineering
• mass fraction, xA
mass of A
xA 
total mass
• mole fraction, yA
moles of A
yA 
total moles

Conversion: Mass/Molar composition
• A gas mixture of the mass composition:
• 16% O2, 4.0% CO, 17% CO2, 63% N2
• The molar composition of the gas can be found assuming a 100 g
Mi (g/mol)
ni = mi/Mi
yi = ni/ntotal
mi as…
= xi (mtotal)
i calculation
xi
basis for
Department of Chemical Engineering
O2
0.16
16 g O2
32 g/mol
0.500 mol
0.15
CO
0.040
4.0 g CO
28 g/mol
0.143 mol
0.044
CO2
0.17
17 g CO2
44 g/mol
0.386 mol
0.12
N2
0.63
63 g N2
28 g/mol
2.250 mol
0.69
Total
1.00
1.0x102 g
3.279 mol
1.00
Conversion: Molar/Mass composition
• A gas mixture of the molar composition:
• 16% O2, 4.0% CO, 17% CO2, 63% N2
• The molar composition of the gas can be found assuming a 100 mole
yi
nias…
= yi(Mtotal)
Mi (g/mol)
mi = ni(Mi)
xi = mi/mtotal
basis for icalculation
Department of Chemical Engineering
O2
0.16
16 mol O2
32
512 g
0.16
CO
0.04
4 mol CO
28
112 g
0.036
CO2
0.17
17 mol CO2
44
748 g
0.24
N2
0.63
63 mol N2
28
1764 g
0.56
Total
1.00
100 mol
3136 g
1.00
Pressure
P  Po  gh
• hydrostatic pressure
Department of Chemical Engineering
• Consider a fluid contained in a vertical column.
• The hydrostatic pressure is based

on the total force acting on the
bottom of the container, and may
be considered as the sum of the
atmospheric pressure (Po) acting on
the top of column of liquid and the
weight of the column.
• Height h of a column is proportional
to the pressure, thus pressures may be expressed as an equivalent length,
referred to as a head of liquid.
Absolute = Atmospheric + Gauge
Department of Chemical Engineering
• Absolute pressure (psia) includes the sum of the atmospheric
contribution as well as that due to the fluid acting on a particular
area.
• Gauge pressure (psig) is that contribution from the fluid, and does not
include atmospheric pressure.
• Consequently, a pressure of 0 psig indicates only atmospheric
pressure is acting on the gauge.
Pabsolute  Patmospheric  Pgauge
Temperature
Department of Chemical Engineering
• Temperature of a substance in a particular state (solid, liquid, gas) is a
measure of the average kinetic energy possessed by the substance
molecules.
• The energy cannot be directly measured, and therefore must be
inferred through indirect means of a physical property of the
substance
•
•
•
•
resistance thermometer (electrical resistance)
thermocouple (voltage at junction of 2 dissimilar metals)
pyrometer (spectra of emitted radiation)
thermometer (density change of a fluid)
Temperature scales
• Temperatures can be expressed directly in terms of the measured
physical properties (i.e., ohms/cm3).
• Defined temperature scales:
Department of Chemical Engineering
• Celsuis or Fahrenheit scales most common whjereby the scale is arbitrarily
assigned two values based on the freezing (0°C or 32°F) and boiling (100°C or
212°F) points of water at 1 atm pressure.
• Absolute zero (lowest theoretical temperature attainable in nature) is 273.15°C or -459.67°F.
• Kelvin and Rankine are scales equivalent to Celsius and Fahrenheit,
respectively, but have a value of 0 assigned to absolute zero.
Converting Temperature scales
• Derived from T(°B) = aT(°A) + b, where temperatures represent
arbitrarily assigned values of the scale.
  
TR TF  459 .67
TR 1.8TK
TF  1.8TC 32
T K  T C  273 .15
Department of Chemical Engineering
• Note the interval size of
temperature on the
Fahrenheit (or Rankine)
scale is 1.8 times the size
of an interval on the
Celsius (or Kelvin) scale.
Q1Liquid acetone is fed at 400 L/min into a heated chamber where it
evaporates into N2. Gas leaving heater is diluted by more N2 flowing at a
rate of 419 m3 (STP)/min. Gases are compressed to Pg= 6.3 atm at 325°C.
At effluent Partial pressure of acetone is 501 mm Hg. nitrogen entering
the evaporator stream is 27°C and 475 mm Hg gauge. If 1 Atm = 760 mm
Hg. And acetone density = 0.791 g/cm3 answer the following
• What is the molar composition of the compressor effluent (outlet)?
• What is the volumetric flow rate of the nitrogen entering the evaporator?
Department of Chemical Engineering