Name: Chemical Engineering: First-Year Calculations (CIR 113)
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Created byKaamil-Inaam Naicker

Last updated 1/2025

English

What you'll learn

Make use of the Ladder Method for basic and complex conversions
Convert between Metric, Imperial and CGS unit systems
Perform dimensional analysis for equations
Convert between mass, molar and volumetric flowrates
Interpret density and bulk density
Interpret specific gravity and specific volume
Understand ideal liquid mixing
Understand mole ratios and empirical formulae
Calculate mass and mole fractions, and mass and mole percentages
Know when to use mass fractions and mole fractions in calculations
Calculate density for a liquid mixture
Calculate density for a pure gas, and a gas mixture
Calculate average molar mass of a gas mixture
Calculate linear velocity in a pipeline
Understand NTP (Normal Temperature and Pressure) and STP (Standard Temperature and Pressure)
Convert gas volume between NTP and STP
Know under which conditions the Ideal Gas Law is valid
Use the Ideal Gas Law to calculate gas properties
Understand the difference between Molarity and Molality
Calculate the Molarity and Molality of a susbstance
Understand Normality and apply it in calculations
Stoichiometrically react acids and bases
Understand ratios and apply them to chemical compositions

Course content

7 sections • 65 lectures • 9h 5m total length

Thank you from Kaamil-Inaam!0:11

Unit Conversions - All Questions0:05
This PDF contains all the questions you need to complete for Tutorial 1. The questions focus on:
1. converting between different unit sets
2. doing dimensional analysis to break down complex units into base units (ie: mass, distance and time)
a: Converting flowrates10:03
Convert a flowrate of 30 m3 per day to cm3/s
b: Converting flowrates10:16
Convert a flow rate of 2 cubic miles per year to L/s
c: Converting density5:02
Convert a density of 62.3 lbm/ft3 to kg/m3
d: Converting density6:52
Convert a density of 1.3 oz/ft3 to kg/m3
e: Converting energy (lbf, poundal, J)14:22
Convert a kinetic energy of 50 ft.lbf to J
f: Converting kinetic energy (lbf, poundal, J)18:39
Convert a kinetic energy of 400 kJ to ft.lbf
h: Converting viscosity (using base units)11:59
Convert a viscosity of 20 cP to lbm/ft.h
i: Converting viscosity (using base units)7:34
Convert a viscosity of 1.5 cP to SI units
j: Converting power12:14
Convert 40 ft.lbf/h to W
k: Converting flowrates7:11
Convert 2.02 million bbl/day to ft3/s
l: Converting density6:08
Convert a density of 1 kg/L to lbm/Imp gall and lbm/ft3
m: Converting power (using hp and BTU)4:36
Convert 182 hp to BTU/h
n: Dimensional analysis3:24
Convert 800 kg/m3 to poundal
Unit Conversion Test

ADVANCED Unit Conversions - All Questions0:05
This PDF contains all the questions you need to complete for Tutorial 2. The questions focus on:

Solving physical science problems (eg: volume, energy, speed, distance) while making use of different unit sets. You will need to perform dimensional analysis and unit conversions to answer these questions.
a: Volume calculation11:26
30 000 bbl of oil is spilled in the sea. According to a newspaper article, this led to an oil slick 2 miles long, half a mile wide and 25 mm thick.
Is the newspaper report correct?
b: Kinetic energy calculation9:44
What is the kinetic energy in ft·poundals and in ft·lbf of an 8 lb mass which has a velocity of 60 miles per hour?
Show how the units are obtained.
c: Potential energy calculation11:15
A certain mass has a potential energy of 700 ft·lbf relative to a surface which is 4 m below the mass.
What is the mass in kg?
d: Reynolds number calculation14:30
Water flows in a 4-inch pipe at a velocity of 0.6 m/s. ρ = 1 g/cm3 and µ = 1 cP.
Convert the given data to SI units and calculate the Reynolds number. Convert the given data to British units and calculate the Reynolds number.
e: Speed, distance, time calculation18:12
A light-year is the distance that light travels in one year. The velocity of light is 3.0 x 108 m/s.
The distance between planet γ and earth is 8.4 light years. The inhabitants of planet γ recently paid us a visit. How long did it take them to travel the distance if their spaceship maintained an average speed of 3.8 x 108 J·s/lbm·ft? Give the answer in hours.

Mass, Moles, Density - All Questions0:05
This PDF contains all the questions you need to complete for Tutorial 3. The questions focus on:

Specific gravity
Density calculations
Bulk density calculations
Ideal liquid mixing
Mass fractions (used for solids and liquids)
Mole fractions (used primarily for gases)
Q 3a: Using density data4:18
The density of solution A is 8.8 lb/Imp gallon.
What is the volume in litres of 10.28 lb of the solution?
Q 3b: Calculating specific gravity10:24
The density of benzene at 60 °F is 0.879 g/cm3. The density of water at 60°F is 62.4 lb/ft3.
Calculate SG60°F / 60°F for benzene
Q 3c: Calculating density and specific volume12:23
A liquid has a specific gravity of 0.90 at 25 °C. What is its:
(a) Density at 25 °C in kg/m3?
(b) Specific volume at 25 °C in ft3/lbm?
(c) If the liquid is placed in a 1.5-L bottle that has a mass of 232 g, how much will the full bottle weigh?
Q 3d: Calculating liquid transfer time14:25
Forty US gal/min of a hydrocarbon fuel having a specific gravity of 0.91 flows into a tank truck with a load limit of 40 000 lb of fuel.
How long will it take to fill the tank in the truck?
Q 3e: Ideal liquid mixing20:51
How many litres of liquid X (SG = 2.1) must be added to 100 litres of liquid Y (SG = 1.2) to give the final density of 100 lb/ft3? The liquids mix ideally.
Q 3f: Bulk density16:13
The bulk density of gravel is 1800 kg/m3. The SG of the stone is 2.6.
If a 50-litre container is full of gravel, how many litres of water can be poured into the container?
Q 3g: Calculating bulk density11:32
A 5-litre container is filled with metal spheres. The SG of the metal is 3.1. It is now possible to pour 1.5 litre of water into the container.
What is the bulk density of the metal spheres?
Q 3h (part a): Mole fractions; Choosing a basis11:39
Commercial sulphuric acid is 98% H2SO4 and 2% H2O.
What is the mole ratio of H2SO4 to H2O?
Q 3h (part b): Empirical formula; Choosing a basis7:02
A compound contains 50% sulfur and 50% oxygen by mass.
Is the empirical formula of the compound (1) SO, (2) SO2, (3) SO3, or (4) SO4?
Q 3h (part c): Mass fractions and powder mixing8:31
How many kgs of activated carbon must be mixed with 38 kg of sand so that the final mixture is 28% activated carbon?
Q 3h (part d): Mole fractions and gas mixtures10:09
A gas mixture contains 40 lb of O2, 25 lb of SO2, and 30 lb of SO3.
What is the composition of the mixture in mole fractions?

ADVANCED Mass, Moles and Density - All Questions0:05
This PDF contains all the questions you need to complete for Tutorial 5. The questions focus on concentrations of mixtures, specifically:

Mass fractions
Mole fractions
Molarity
Molality
Normality
Q 4a: Mole fractions9:01
Calculate the empirical formula of an organic compound with the following mass analysis: carbon, 26.9 %; hydrogen, 2.2 %; and oxygen as the only other element present.
Q 4b (part i): Mass fractions4:20
Given a water solution that contains 1.704 kg of HNO3/kg·H2O and has a specific gravity of 1.382 at 20 °C, express the composition in the following ways:
(i) Mass percent HNO3
Q 4b (part ii): Density of mixture6:52
Given a water solution that contains 1.704 kg of HNO3/kg·H2O and has a specific gravity of 1.382 at 20 °C, express the composition in the following ways:
(i) Mass percent HNO3
(ii) Pound HNO3, per cubic foot of solution at 20 °C
Q 4b (part iii): Molarity11:29
Given a water solution that contains 1.704 kg of HNO3/kg·H2O and has a specific gravity of 1.382 at 20 °C, express the composition in the following ways:
(i) Mass percent HNO3
(ii) Pound HNO3, per cubic foot of solution at 20 °C
(iii) Molarity
Q 4c: Mass and Mole fractions of a mixture14:11
4 kg Na2SO4, 9 kg Na2CO3 and 5 kg NaCl are dissolved in water. Enough water is added to bring the final mass to 120 kg.
What are the mass fraction and mole fraction of each compound in the solution?
Q 4d (part a): Mole fractions7:28
Q 4d (part b): Mass fractions1:31
A nitric acid solution in water contains 56% HNO3 on a mass basis. The density of the solution is 1.345 g/cm3. Calculate the concentration of the solution expressed as:
(b) kg HNO3/kg H2O
Q 4d (part d): Density2:01
A nitric acid solution in water contains 56% HNO3 on a mass basis. The density of the solution is 1.345 g/cm3. Calculate the concentration of the solution expressed as:
(d) kg HNO3/m3 solution
Q 4d (part c): Molarity5:20
A nitric acid solution in water contains 56% HNO3 on a mass basis. The density of the solution is 1.345 g/cm3. Calculate the concentration of the solution expressed as:
(c) g HNO3/litre solution
Q 4d (part e): Molarity4:08
Learn molarity in chemical engineering first-year calculations by converting grams of nitric acid to moles using molar mass, to express concentration as moles per liter of solution.
Q 4d (part f): Normality5:08
A nitric acid solution in water contains 56% HNO3 on a mass basis. The density of the solution is 1.345 g/cm3. Calculate the concentration of the solution expressed as:
(f) Normality
Q 4e: Molar mass of an ideal gas mixture8:18
120 kg CH4, 40 kg H2 and 30 kg N2 are stored in a cylinder.
What is the average mole mass of the gas mixture?
Q 4f: Mass fractions of a liquid mixture15:36
A solution in water contains a mixture of salts (Na2CO3 and Na2SO4) and analyses as follows: Water = 70%; Salts = 30%.
The salts are present in the mole ratio Na2SO4/Na2CO3 = 1.6.
Calculate the % Na2SO4 and % Na2CO3 in the solution.
Q 4g (part a): Density of a liquid mixture16:04
10 kg of a 12% MgCl2 solution (SG = 1.1) is mixed with 20 kg of a 26% MgCl2 solution (SG = 1.3). The mixing is ideal. No temperature change takes place. The molecular mass of MgCl2 is 95.2.
Calculate the final mixture:
*a) The density in lbm/ft3
b) The mass fraction MgCl2
c) kg MgCl2 per kg water
d) Molarity
e) Molality
Q 4g (part b): Mass fraction of a liquid mixture4:44
10 kg of a 12% MgCl2 solution (SG = 1.1) is mixed with 20 kg of a 26% MgCl2 solution (SG = 1.3). The mixing is ideal. No temperature change takes place. The molecular mass of MgCl2 is 95.2.
Calculate the final mixture:
a) The density in lbm/ft3
*b) The mass fraction MgCl2
c) kg MgCl2 per kg water
d) Molarity
e) Molality
Tutorial 4g (part c): Mass ratio of a liquid mixture3:02
10 kg of a 12% MgCl2 solution (SG = 1.1) is mixed with 20 kg of a 26% MgCl2 solution (SG = 1.3). The mixing is ideal. No temperature change takes place. The molecular mass of MgCl2 is 95.2.
Calculate the final mixture:
a) The density in lbm/ft3
b) The mass fraction MgCl2
*c) kg MgCl2 per kg water
d) Molarity
e) Molality
Tutorial 4g (part d): Molarity of a liquid mixture4:25
10 kg of a 12% MgCl2 solution (SG = 1.1) is mixed with 20 kg of a 26% MgCl2 solution (SG = 1.3). The mixing is ideal. No temperature change takes place. The molecular mass of MgCl2 is 95.2.
Calculate the final mixture:
a) The density in lbm/ft3
b) The mass fraction MgCl2
c) kg MgCl2 per kg water
*d) Molarity
e) Molality
Tutorial 4g (part e): Molality of a liquid mixture5:16
10 kg of a 12% MgCl2 solution (SG = 1.1) is mixed with 20 kg of a 26% MgCl2 solution (SG = 1.3). The mixing is ideal. No temperature change takes place. The molecular mass of MgCl2 is 95.2.
Calculate the final mixture:
a) The density in lbm/ft3
b) The mass fraction MgCl2
c) kg MgCl2 per kg water
d) Molarity
*e) Molality
Tutorial 4h (part a,b,c): Normality16:25
To neutralise 60 kg of a 75% solution of H2SO4 in water requires how many litres of:
*a) 13.8 N NaOH solution?
*b) 2.4 N Ca(OH)2 solution?
*c) 2.4 N Al(OH)3 solution?
d) 6.2 M Ba(OH)2 solution?
Tutorial 4h (part d): Normality cont'd2:53
To neutralise 60 kg of a 75% solution of H2SO4 in water requires how many litres of:
a) 13.8 N NaOH solution?
b) 2.4 N Ca(OH)2 solution?
c) 2.4 N Al(OH)3 solution?
*d) 6.2 M Ba(OH)2 solution?

Tutorial 6 All Questions0:05
Tutorial 6a: Gas mixtures (density, molar mass, mole fractions)22:12
Calculate gas mixture properties from mole fractions using the ideal gas law. Determine molar mass by weighted averaging, density, volumetric flow rate, and linear velocity in a 100 mm pipe.
Tutorial 6b: Normal Temperature and Pressure18:02
The linear velocity of CO2 in a 200 mm pipe is 240 m/s at 1.2 atm and 200° C.
What is the flowrate in nm3/s?
Tutorial 6c: Density of an ideal gas4:38
What is the density of air (mol mass = 29) at STP?
Tutorial 6d: Specific gravity of a gas2:12
What is the SG of air at STP?
Tutorial 6e: Standard Temperature and Pressure5:10
What is the density of CH4 at STP?
Tutorial 6f: Specific gravity of an ideal gas3:40
What is the SG of CH4 at STP relative to air at STP?
Tutorial 6g: Density of an ideal gas6:21
The SG of CH4 is 0.552 (air at STP = 1.00).
What is the density of the CH4?
Tutorial 6h: Specific volume of an ideal gas12:20
The SG of benzene vapour is 3.2 (H2 at 20° C, 200 kPa = 1.00)
What is the specific volume of the benzene vapour in m3/kmol? (Mol mass of Benzene = 78).
Tutorial 6i: Temperature of an ideal gas11:35
Nitrogen at 150 kPaa has an SG of 0.4 (air at STP = 1.00).
What is the temperature of the nitrogen?

Requirements

This course requires a good understanding of High School (Grade 12) Mathematics, Physical Science and Chemistry.
No chemical engineering experience is required.

Description

Hi, I'm Kaamil the Chemical Engineer.

I currently work as a Process Engineer in a multinational petrochemicals company. It is one of the largest companies by market cap on the Johannesburg Stock Exchange.

Many of the concepts you will read about in your textbooks, I have seen with my own two eyes. So, I would like to share these experiences with you. I hope that my stories will make your first year of Engineering a bit less abstract.

Chemical Engineers are lauded worldwide for their problem-solving abilities, and that is exactly what I want you to learn from this course. Once you have these skills, you can apply them to Investing, Engineering, Business and more.

We will cover a range of examples, all of which require an innovative approach and a sharp mind.
Sections covered include:
unit conversions, dimensional analysis, mass and mole fractions, densities and bulk densities, specific volume and specific gravity, the ideal gas law, molar mass of a gas mixture, flowrates in pipelines, mixing operations, and more.

You can use the examples to teach yourself, and then use the test questions to evaluate your problem-solving skills.

This should set you on your way to becoming a great Engineer!

Who this course is for:

First year Chemical Engineering Undergraduate Students
CIR 113 students at the University of Pretoria

What you'll learn

Explore related topics

Course content

Course Introduction1 lecture • 1min

Unit Conversions and Dimensional Consistency14 lectures • 1hr 58min

ADVANCED Unit Conversions and Dimensional Consistency6 lectures • 1hr 5min

Mass, Moles and Density12 lectures • 2hr 8min

ADVANCED Mass, Moles and Density21 lectures • 2hr 28min

Process variables (Pressure)1 lecture • 1min

Tutorial 6: Ideal gases (mixtures, STP, NTP)10 lectures • 1hr 26min

Requirements

Description

Who this course is for: