Introductory Lecture Notes (Lecture 01).pptx

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1. Industrial Stoichiometry-I Ch.E. – 101

2. Chemical engineering is a branch of engineering that deals with the application of principles from chemistry, physics, and mathematics to design, analyze, and optimize processes involving chemical transformations. The primary goal of chemical engineering is to convert raw materials into useful products through various chemical and physical processes. These products can range from everyday items like pharmaceuticals, plastics, and fuels to more specialized materials used in aerospace, electronics, and other industries. Chemical engineers play a crucial role in the development and improvement of manufacturing processes, ensuring that they are efficient, safe, and environmentally sustainable. They are involved in all stages of a process, from conceptualization and design to operation, control, and optimization. Introduction to Chemical Engineering 2 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

3. Name Of Course/Module Industrial Stoichiometry-I Course Code Ch.E-101 Name of Academic Staff Engr. Tayyab Ali Rationale for the inclusion of course in the program To familiarize students with k nowledge of determining the right stoichiometric ratios of reactants, thus maximizing product yield and minimizing waste generation Semester 1 st Credit Value (3) Knowledge Area Engineering Foundation 3 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

4. To introduce students with the deep understanding of technical and economic problems used in chemical industries to design, analyze, and optimize chemical processes effectively. Industrial stoichiometry helps chemical engineers make efficient use of resources. By calculating the precise amounts of raw materials required, they can reduce waste, energy consumption, and overall production costs. Objectives Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 4

5. Measurable Student Learning Outcomes CLOs DESCRIPTION PLOs DOMAIN DOMAIN LEVEL CLO 1 Describe fundamental quantities and terminologies associated with dimensional analysis and stoichiometric PLO 1 Cognitive 2. Understand CLO 2 Apply ideal gas laws and principles of psychrometry to solve related problems PLO 2 Cognitive 3. Apply CLO 3 Perform material and energy balance calculations for chemical systems PLO 2 Cognitive 3. Apply Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 5

6. Basic Principles and Calculations in Chemical Engineering, 8th Edition By David M. Himmelblau, and J. B. Riggs BOOK MAIN TEXT Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 6

7. ALL BOOKS Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 7

8. COURSE ASSESSMENT CRITERIA Description Percentage Observations Attendance 5% Strict Compliance, also includes class performance Assignments 5% Achievement of CLOs 1st Quiz 10% Before Mid Term 2nd Quiz 10% After Mid Term Mid Paper 30% - Final Paper 40% Mid term course will also be included Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 8

9. Stoichiometry is a fundamental concept in chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. In chemical engineering, industrial stoichiometry is of paramount importance as it forms the basis for process design and optimization. By understanding the stoichiometry of a reaction, engineers can determine the exact amounts of reactants needed to produce a desired quantity of product, as well as predict the amount of byproducts or waste generated. Importance of Industrial Stoichiometry in Chemical Process Industries 9 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

10. Course Outline Dimension and units (Conversion of units, Dimensional consistency and analysis), Stoichiometric and composition relations: Mole fraction, mass fraction, volume fraction, molarity, molality, normality, formality, parts per million, parts per billion, Stoichiometric calculations based on ideal gas laws (Ideal gas mixtures and partial pressure, Pure component volume), Specific gravity and different gravity scales, Composition of a gas on dry and wet basis, Material balance involving gases (reactive and non-reactive), Humidity and saturation (Vapor pressure, saturation, humidity, absolute humidity, relative humidity, Dew point, bubble point, wet bulb and dry bulb temperature. Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 10

11. Course Outline (continued……) Material balance involving saturation), Steady state mass and energy balance: (a) Processes Classification (open, closed, batch, semi-batch, continuous, transient, steady state), Unit operations (general definition, introduction of concept), Flow diagrams, General material balance equation, System boundaries, Degrees of freedom analysis; (b) Material balances for non-reacting systems; (c) Material balances for reacting; (d) systems (stoichiometry, conversion, excess/limiting reactant, yield, selectivity, extent of reaction); (e) Species material balance on steady state systems involving single unit and single reaction; (f) Elemental material balance on steady state systems involving single unit and single reaction & (g) General Energy balance equation, Energy balances for non-reacting systems, Energy balances for closed systems, Energy balances for open systems. Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 11

12. Introductory Concepts Chapter 2 12 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

13. Contents Systems of Units Conversion of Units Dimensional Consistency Significant Figures Validation of Results The Mole and Molecular Weight Choosing a Basis Density and Specific Gravity Concentration Temperature Pressure and Hydrostatic Head Flow Rate 13 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

14. Units & Dimensions SI System Engineering System Unit Conversions

15. Unit Systems SI System The SI system is an international standard of measurement developed and maintained by the International Bureau of Weights and Measures (BIPM) based in France. It was established in 1960 and has been widely adopted by most countries worldwide, including the United States. American Engineering System The American Engineering System, as the name suggests, is primarily used in the United States. It evolved from customary units that were inherited from British colonial times and has been retained in various industries in the US. 15 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

16. 16 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) Physical Quantity Name of Unit Symbol for Unit Definition Length meter m Mass gram, tonne, ton g, t Time second s Temperature Kelvin, degree Celsius K, º C Amount of Substance mole mol Force (F) newton N (kg)(m)(s -2 ) → (J)(m -1 ) Energy (E) joule J (kg)(m 2 )(s -2 ) Power (P) watt W (J)(s -1 ) Density ( ρ ) kilogram per cubic meter (kg)(m 3 ) Velocity (v) meter per second (m)(s -1 ) Acceleration (a, g) meter per second squared (m)(s -2 ) Pressure (p) pascal (N)(m -2 ), Pa Heat Capacity (Cp) joule per (kilogram x kelvin) (J)(kg -1 )(K -1 ) Table for SI units

17. 17 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) Physical Quantity Name of Unit Symbol Length foot or inch ft or in Mass pound (mass) lb m Time second, hour s, hr Temperature degree Rankine or degree Fahrenheit º R or º F Amount of Substance pound mole lb mol Force (F) pound (force) Lb f Energy (E) British thermal unit, foot pound (force) Btu, (ft)(lb f ) Power (P) horsepower hp Density ( ρ ) pound (mass) per cubic foot Velocity (v) feet per second Acceleration (a, g) feet per second squared Pressure (p) pound (force) per square inch Heat Capacity (Cp) Btu per pound (mass) per degree Fahrenheit Physical Quantity Name of Unit Symbol Length foot or inch ft or in Mass pound (mass) lb m Time second, hour s, hr Temperature degree Rankine or degree Fahrenheit º R or º F Amount of Substance pound mole lb mol Force (F) pound (force) Lb f Energy (E) British thermal unit, foot pound (force) Btu, (ft)( lb f ) Power (P) horsepower hp Density ( ρ ) pound (mass) per cubic foot Velocity (v) feet per second Acceleration (a, g) feet per second squared Pressure (p) pound (force) per square inch Heat Capacity (Cp) Btu per pound (mass) per degree Fahrenheit Table for American Engineering (AE) System units

18. SI Prefixes Factor Prefix Symbol Factor Prefix Symbol 10 9 giga G 10 -1 deci d 10 6 mega M 10 -2 centi c 10 3 kilo k 10 -3 milli m 10 2 hecto h 10 -6 micro μ 10 1 deka da 10 -9 nano n Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) 18

19. Length Mass Force Pressure Volume 1 mile = 1.61 km 1 g = 15.432 grain 1 N = 10 5 dynes 1 atm = 1.01325 bar 1 bbl = 42 gal 1 mile = 1.852 km (nautical) 1 lb = 7000 gr. 1kg f = 9.806 N 1 bar = 10 5 Pa 1 bbl = 35 UK gal 1 m = 3.28 ft. 1 lb = 16 oz. 1 lb f = 4.45 N 1 atm = 14.7 psi 1 gal = 3.785 L 1 m = 39.37 in. 1 slug = 32.174 lb 1 lb f = 32.174 poundal 1 atm = 33.91 ft. H 2 O 1 L = 1 dm 3 1 ft. = 12 in. 1 metric ton or 1 tonne = 1000 kg 1 tonne f = 1000 kg f 1 atm = 760 torr or mm Hg 1 L = 1000 cm 3 1 ft. = 30.48 cm 1 ton (short or US) = 2000 lb 1 ton f = 2000 lb f 1 atm = 29.921 in. Hg 1 m 3 = 1000 L 1 in. = 2.54 cm 1 ton (long or UK) = 2240 lb 1 UK ton f = 2240 lb f 1 atm = 1.033 kg f /cm 2 1 m 3 = 35.31 ft 3 1 micron = 10 -6 m 1 kg = 2.2045 lb 1 atm = 101.325 kPa 1 yard = 3 ft. 1 lb = 454 g 1 atm = 101325 Pa

20. Heat, Energy or Work Equivalents (ft)(lb f ) kWh (hp)(hr) BTU calorie* joule (ft)(lb f ) 1 3.766 x 10 -6 5.05 x 10 -7 1.285 x 10 -3 0.3241 1.356 kWh 2.655 x 10 6 1 1.341 3.413 x 10 3 8.606 x 10 5 3.6 x10 6 (hp)(hr) 1.98 x10 6 0.7455 1 2.545 x10 3 6.416 x10 5 2.684 x10 6 BTU 778.16 2.93 x10 -4 3.93 x10 -4 1 252 1055 calorie* 3.086 1.162 x10 -6 1.558 x10 -6 3.97 x10 -3 1 4.184 joule 0.7376 2.773 x10 -7 3.725 x10 -7 9.484 x10 -4 0.239 1 20 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

21. Gravitational Constant (g c ) Concept In the AE system the conversion of terms involving pound mass and pound force deserve special attention. Let us start the discussion with Newton’s law, which states that force (F) is proportional to the product of mass (m) and acceleration (a), that is, where C is a constant whose numerical values and units depend on the units selected for F, m, and a.   In SI System the unit of force is defined to be the newton (N), which corresponds to 1 kg accelerated at 1 m/s 2 . Therefore, the conversion factor C = 1 N/(kg)(m/s 2 ) results so that the force is expressed in newtons (N): 21 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) F = 1 N 1 kg 1 m = 1N s 2 F = 1 N 1 kg 1 m = 1N s 2

22. Gravitational Constant (g c ) In the American Engineering system an analogous conversion factor is required. In the AE system, one pound force (1 lb f ) corresponds to the action of the Earth’s gravitational field on one pound mass (1 lb m ): A numerical value of 1/32.174 has been chosen to maintain the numerical correspondence between lb f and lb m on the surface of the Earth. The acceleration caused by gravity, you may recall, varies by a few tenths of 1% from place to place on the surface of the Earth but, of course, is quite different on the surface of the moon. The inverse of this conversion factor is given the special symbol   22 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

23. Problem: Which of the following best represents the force needed to lift a heavy suitcase? 25 N 25 kN 250 N 250 kN 23 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

24. Problem: If a plane travels at twice the speed of sound (assume that the speed of sound is 1100 ft/s), how fast is it going in miles per hour? 24 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

25. Problem: Nanosize materials have become the subject of intensive investigation in the last decade because of their potential use in semiconductors, drugs, protein detectors, and electron transport. Nanotechnology is the generic term that refers to the synthesis and application of such small particles. An example of a semiconductor is ZnS with a particle diameter of 1.8 nm. Convert this value to (a) decimeters (dm) and (b) inches (in.). 25 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

26. Problem: In biological systems, enzymes are used to accelerate the rates of certain biological reactions. Glucoamylase is an enzyme that aids in the conversion of starch to glucose (a sugar that cells use for energy). Experiments show that 1 μg mol of glucoamylase in a 4% starch solution results in a production rate of glucose of 0.6 μg mol/(mL)(min). Determine the production rate of glucose for this system in units of lb mol/(ft 3 )(day). 26 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

27. Problem: What is the potential energy in (ft)(lb f ) of a 100 lb drum hanging 10 ft above the surface of the Earth with reference to the surface of the Earth? 27 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

28. Problem: Electronic communication via radio travels at approximately the speed of light (186,000 mi/s). The edge of the solar system is roughly at Pluto, which is 3.6 × 10 9 mi from the Earth at its closest approach. How long in hours does it take for a radio signal from Earth to reach Pluto? 28 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

29. Problem: Convert the following: to all SI units   29 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

30. 30 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) A technical publication describes a new model 20 hp Stirling (air cycle) engine that drives a 68 kW generator. Is this possible? Your boss announced that the speed of the company Boeing 737 is to be cut from 525 mi/hr to 475 mi/hr to “conserve fuel,” thus cutting consumption from 2200 gal/hr to 2000 gal/hr. How many gallons are saved in a 1000 mi trip? In the American Engineering system of units, the viscosity can have the units of (lb f )(h)/ft 2 , while in a handbook the units are (g)/[(cm)(s)]. Convert a viscosity of 20.0 (g)/[(m)(s)] to the given American Engineering units. Consider water pumped at a rate of 75 gal/min through a pipe which undergoes a 100 ft elevation increase by a 2 hp pump. The rate energy input from the pump that goes into heating the water is approximately equal to the rate of energy input from the pump minus the rate of potential energy generated by pumping the water up the elevation change ( m′gh , where m′ is the mass flow rate of water and h is the elevation change). Estimate the rate of energy input for heating the water for this case in British thermal units per hour.

31. 31 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) Water is flowing through a 2 in. diameter pipe with a velocity of 3 ft/s. What is the kinetic energy of the water in (ft)(lb f )/lb m ? What is the flow rate in gallons per minute? A tractor pulls a load with a force equal to 800 lb (4.0 kN ) with a velocity of 300 ft/min (1.5 m/s). What is the power required using the given American Engineering system data? The SI data? What is the kinetic energy of a vehicle with a mass of 2300 kg moving at the rate of 10.0 ft/s in British thermal units? A pallet of boxes weighing 10 tons is dropped from a lift truck from a height of 10 ft. The maximum velocity the pallet attains before hitting the ground is 6 ft/s. How much kinetic energy does the pallet have in (ft)(lb f ) at this velocity?

32. Solve the following problem: Calculate the protein elongation (formation) rate per mRNA per minute based on the following data: One protein molecule is produced from x amino acid molecules. The protein (polypeptide) chain elongation rate per active ribosome uses about 1200 amino acids/min. One active ribosome is equivalent to 264 ribonucleotides. 3x ribonucleotides equal each mRNA. Messenger RNA (mRNA) is a copy of the information carried by a gene in DNA and is involved in protein synthesis. 32 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

33. Dimensional Consistency Representing different equations to check their dimensional consistency

34. 34 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) Van der Waal’s equation Reynold’s Number Euler’s number Prandtl Number Schmidt number Grashof Number Van der Waal’s equation Reynold’s Number Euler’s number Prandtl Number Schmidt number Grashof Number Dimensionless numbers

35. Problem: Your handbook shows that microchip etching roughly follows the relation where d is the depth of the etch in microns [micrometers (μm)] and t is the time of the etch in seconds. What are the units associated with the numbers 16.2 and 0.021? Convert this relation so that d becomes expressed in inches and t can be used in minutes.   35 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

36. Problem: The following equation is proposed to calculate the pressure drop (Δp) across a length of pipe (L) due to flow through the pipe. Determine the dimensional consistency of this equation: where ν is the average velocity of the fluid flowing through the pipe, D is the diameter of the pipe, and f is a dimensionless coefficient called the friction factor, which is a function of the Reynolds number.   36 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

37. 37 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) The density of a certain liquid is given an equation of the following form: where ρ = density (g/cm 3 ) T = temperature (°C) P = pressure (atm) For this equation to be dimensionally consistent, what are the units of A, B, and C? Explain in detail whether the following equation for flow over a rectangular weir is dimensionally consistent. (This is the modified Francis formula.) where q = volumetric flow rate (ft 3 /s) L = crest height (ft) h o = weir head (ft) g = acceleration of gravity (32.2 ft/s 2 )  

38. 38 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) In an article on measuring flows from pipes, the author calculated q = 80.8 m 3 /s using the formula where q = volumetric flow rate (m 3 /s) C = dimensionless coefficient (0.6) A 1 = cross-sectional area 1 (m 2 ) A 2 = cross-sectional area 2 (m 2 ) V = specific volume (10 –3 m 3 /kg) P = pressure p 1 – p 2 = 50 kPa g = acceleration of gravity (9.80 m/s) Was the calculation correct? (Answer yes or no and explain briefly the reasoning underlying your answer.)  

39. 39 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) Leaking oil tanks have become such an environmental problem that the federal government has implemented a number of rules to reduce the problem. A flow rate from a leak from a small hole in a tank can be predicted from the following relation: where Q is the leakage rate (gal/min) S is the cross-sectional area of the hole causing the leak (in. 2 ) Δp is the pressure drop between the inside of the tank opposite the leak and the atmospheric pressure (psi) ρ is the fluid density (lb/ft 3 ) To test the tank, the vapor space is pressurized with N 2 to a pressure of 23 psig. If the tank is filled with 73 in. of gasoline (sp. gr. = 0.703) and the hole is ¼ in. in diameter, what is the value of Q (in cubic feet per hour)?  

40. 40 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

41. 41 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) A relation for a dimensionless variable called the compressibility (z), which is used to describe the pressure-volume-temperature behavior for real gases, is where ρ is the density in g mol/cm 3 . What are the units of B, C, and D? Convert the coefficients in the equation for z so that the density can be introduced into the equation in the units of lb m /ft 3 thus: ρ* is in lb m /ft 3 . Give the units for B*, C*, and D*, and give the equations that relate B* to B, C* to C, and D* to D. A letter to the editor says: “An error in units was made in the article ‘Designing Airlift Loop Fermenters.’ Equation is not correct.” Is the author of the letter correct? (f is dimensionless.)  

42. 42 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) The velocity in a pipe in turbulent flow is expressed by the following equation: where τ is the shear stress in N/m 2 at the pipe wall ρ is the density of the fluid in kg/m 3 u is the velocity in m/s k is a coefficient You are asked to modify the equation so that the shear stress can be introduced in the units of τ which are lb f /ft 2 , and the density ρ′ for which the units are lb /ft 3 so that the velocity u comes out in the units of ft/s. Show all calculations, and give the final equation in terms of u, τ, and ρ′ so a reader will know that American Engineering units are involved in the equation.  

43. 43 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) In 1916 Nusselt derived a theoretical relation for predicting the coefficient of heat transfer between a pure saturated vapor and a colder surface: where h is the mean heat transfer coefficient, Btu/[(hr)(ft 2 )(°F)] k is the thermal conductivity, Btu/[(hr)(ft)(°F)] ρ is the density in lb/ft 3 g is the acceleration of gravity, 4.17×10 8 ft/(hr) 2 λ is the enthalpy change of evaporation in Btu/lb L is the length of tube in ft m is the viscosity in lb m /[(hr)(ft)] Δ T is a temperature difference in °F What are the units of the constant 0.943?  

44. 44 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) The Antoine equation, which is an empirical equation, is used to model the effect of temperature on the vapor pressure of a pure component. The Antoine equation is given by where p* is the vapor pressure, T is the absolute temperature, and A, B, and C are empirical constants specific to the pure component and the units used for the vapor pressure and temperature. Determine under what conditions this equation will be dimensionally consistent.  

45. Mole & Molecular Weight Mole & Mass Molecular Weight Mole Fraction Mass Fraction Avg. Mol. Weight

46. Definition Mole (n) A mole is a certain amount of material corresponding to a specified number of molecules, atoms, electrons, or other specified types of particles. In the SI system a mole (which we will call a gram mole to avoid confusing units) is composed of 6.022 × 10 23 (Avogadro’s number) molecules. Mass (m) Mass refers to the amount of matter present in a substance and is typically measured in grams (g) or kilograms (kg). Mass is a scalar quantity and does not depend on the location of the substance; it remains the same regardless of the gravitational force acting on it. 46 Molecular Weight Molecular weight, also known as molar mass, is the mass of one mole of a substance and is expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms present in a molecule.   Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

47. Fractions Mass Fraction The mass fraction of a component in a mixture is the ratio of the mass of that component to the total mass of the mixture. It is expressed as a percentage or a decimal fraction. Mass fraction helps determine how much of a specific substance is present in a mixture by weight. Mole Fraction The mole fraction of a component in a mixture is the ratio of the number of moles of that component to the total number of moles in the mixture. It is also expressed as a decimal fraction. Mole fraction helps determine the proportion of a specific substance in a mixture based on the number of moles. 47 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

48. Problem: If a bucket holds 2.00 lb of NaOH: How many pound moles of NaOH does it contain? How many gram moles of NaOH does it contain? 48 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

49. Problem: How many pounds of NaOH are in 7.50 g mol of NaOH? 49 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

50. Problem: Calculate the average molecular weight of air, assuming that air is 21% O 2 and 79% N 2 . 50 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

51. Problem: An industrial-strength drain cleaner contains 5.00 kg of water and 5.00 kg of NaOH. What are the mass (weight) fraction and mole fraction of each component in the drain cleaner? 51 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

52. 52 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) Convert 39.8 kg of NaCl per 100 kg of water to kilogram moles of NaCl per kilogram mole of water. How many pound moles of NaNO 3 are there in 100 lb? Commercial sulfuric acid is 98% H 2 SO 4 and 2% H 2 O. What is the mole ratio of H 2 SO 4 to H 2 O? A solid compound contains 50% sulfur and 50% oxygen. Is the empirical formula of the compound (a) SO, (b) SO 2 , (c) SO 3 , or (d) SO 4 ? A gas mixture contains 40 lb of O 2 , 25 lb of SO 2 , and 30 lb of SO 3 . What is the composition of the mixture? Saccharin, an artificial sweetener that is 3000 times sweeter than sucrose, is composed of 45.90% carbon, 2.73% hydrogen, 26.23% oxygen, 7.65% nitrogen, and 17.49% sulfur. Is the molecular formula of saccharin (a) C 14 H 10 O 6 N 2 S 2 , (b) C 5 H 7 O 3 NS, (c) C 8 H 9 O 2 NS, or (d) C 7 H 5 O 3 NS?

53. 53 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) A solid compound was found to contain 42.11% C, 51.46% O, and 6.43% H. Its molecular weight was about 341. What is the formula for the compound? A sample has a specific volume of 5.2 m 3 /kg and a molar volume of 1160 m 3 /kg mol. Determine the molecular weight of the material. You have 100 kg of gas of the following composition: CH 4 30%, H 2 10%, N 2 60% What is the average molecular weight of this gas? You analyze the gas in 100 kg of gas in a tank at atmospheric pressure and find the following: CO 2 19.3%, O 2 6.5%, H 2 O 2.1%, N 2 72.1% What is the average molecular weight of the gas?

54. Choosing a Basis How to choose basis for any given question?

55. Choosing a Basis Definition: A basis is a reference chosen by you for the calculations you plan to make in a particular problem, and a proper choice of basis often can make a problem much easier to solve than a poor choice. The basis may be a period of time such as hours, or a given mass of material, or some other convenient quantity. How to choose it? To select a sound basis (which in many problems is predetermined for you but in some problems is not so clear), ask yourself the following three questions: What do I have to start with? What answer is called for? What is the most convenient basis to use? 55 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

56. For liquids and solids in which a mass (weight) analysis applies, a convenient basis is often 1 or 100 lb or kg; similarly, because gas compositions are usually provided in terms of moles, 1 or 100 moles is often a good choice for a gas. 56 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

57. Problem: Considering a gas containing O 2 (20%), N 2 (78%), and SO 2 (2%), find the composition of the gas on an SO 2 -free basis, meaning gas without the SO 2 in it. 57 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

58. 58 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) A gas mixture consists of three components: argon, B, and C. The following analysis of this mixture is given: 40.0 mol % argon, 18.75 mass % B, 20.0 mol % C. The molecular weight of argon is 40 and the molecular weight of C is 50. Find (1) the molecular weight of B and (2) the average molecular weight of the mixture. Two engineers are calculating the average molecular weight of a gas mixture containing oxygen and other gases. One of them uses the correct molecular weight of 32 for oxygen and determines the average molecular weight as 39.2. The other uses an incorrect value of 16 and determines the average molecular weight as 32.8. This is the only error in the calculations. What is the percentage of oxygen in the mixture expressed as mole percent? Chlorine usage at a water treatment plant averages 134.2 lb/day. The average flow rate of water leaving the plant is 10.7 million gal/day. What is the average chlorine concentration in the treatment water leaving the plant (assuming no reaction of the chlorine), expressed in milligrams per liter?

59. Density & Specific Gravity Density Specific gravity Different scales of gravity

60. Density Density and specific gravity are both terms used in physics and materials science to describe the properties of substances, particularly their mass and volume. While they are related, they have distinct meanings. Density is usually expressed in units like grams per cubic centimeter (g/cm³) or kilograms per cubic meter (kg/m³) for solid materials and grams per milliliter (g/mL) or kilograms per liter (kg/L) for liquids. Density is a measure of mass per unit volume of a substance. It quantifies how much mass is contained in a given volume of a material. The formula for calculating density is:   60 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

61. Relationship between temperature and density In general The relationship between temperature and density is different for solids, liquids, and gases. Solids and liquids typically experience a decrease in density with increasing temperature, whereas gases exhibit an increase in density with increasing temperature. However, some substances, like water, have unique density-temperature behaviors that deviate from these general trends. 61 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

62. Quantities related to Density Specific Volume,   Specific volume is the reciprocal of density and is used to describe the volume occupied by a unit mass of a substance. It is defined as:   Molar Density Molar density, also known as molar volume, is the amount of volume occupied by one mole of a substance. It is the reciprocal of molar density. Molar density is given by the equation:   62 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

63. Problem: If penicillin has a specific gravity of 1.41, what is the density in: g/cm 3 lb m /ft 3 kg/m 3 63 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

64. Problem: In the production of a drug having a molecular weight of 192, the exit stream from the reactor containing water and the drug flows at the rate of 10.5 L/min. The drug concentration is 41.2% (in water), and the specific gravity of the solution is 1.024. Calculate the concentration of the drug (in kilograms per liter) in the exit stream, and the flow rate of the drug in kilogram moles per minute. 64 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

65. 65 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) If you add 50 g of sugar to 500 mL of water, how do you calculate the density of the sugar solution? A solution in water contains 1.704 kg of HNO 3 /kg H 2 O, and the solution has a specific gravity of 1.382 at 20°C. How many kilograms of HNO 3 per cubic meter of solution at 20°C are there?

66. Density Scales Hydrometer A hydrometer is an instrument used for measuring the relative density of liquids based on the concept of buoyancy. They are typically calibrated and graduated with one or more scales such as specific gravity. Scales API gravity, universally used worldwide by the petroleum industry. Baumé scale, formerly used in industrial chemistry and pharmacology Brix scale, primarily used in fruit juice, wine making and the sugar industry Twaddell scale, formerly used in the bleaching and dyeing industries 66 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

67. API Gravity Scale Introduction The American Petroleum Institute gravity, or API gravity, is a measure of how heavy or light a petroleum liquid is compared to water: if its API gravity is greater than 10, it is lighter and floats on water; if less than 10, it is heavier and sinks. Formula The formula to calculate API gravity from Specific Gravity (SG) is: 67 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

68. Baumé scale Introduction Baumé scale is a pair of hydrometer scales developed by French pharmacist Antoine Baumé in 1768 to measure density of various liquids. The unit of the Baumé scale has been notated variously as degrees Baumé, B°,  Bé °. One scale measures the density of liquids heavier than water and the other, liquids lighter than water. Formula The formula for conversions between specific gravity and degrees Baumé is: (For density greater than water) (For density lesser than water) 68 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

69. Brix scale Degrees Brix (symbol °Bx) is the sugar content of an aqueous solution. One degree Brix is 1 gram of sucrose in 100 grams of solution and represents the strength of the solution as percentage by mass. If the solution contains dissolved solids other than pure sucrose, then the °Bx only approximates the dissolved solid content. For example, when one adds equal amounts of salt and sugar to equal amounts of water, the degrees of refraction (BRIX) of the salt solution rises faster than the sugar solution. The °Bx is traditionally used in the wine, sugar, carbonated beverage, fruit juice, fresh produce, maple syrup and honey industries. where S is the apparent specific gravity of the solution at 20 °C/20 °C. 69 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

70. Twaddell scale Introduction Twaddell scale is only used for liquids with specific gravity greater than that of water. The scale was used in the British dye and bleach manufacturing industries. While the Baumé scale was adopted throughout England, the Twaddell scale was used in England and Scotland. Formula Converting between Twaddell scale and specific gravity 70 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

71. Problem: A solution has a gravity of 80° Twaddell. Calculate its specific gravity and its gravity in degrees Baume’? 71 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

72. 72 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) An oil has a specific gravity at 60°/60°F of 0.790. Calculate its gravity in degrees API and degrees Baumé? 500 cubic meters of 30°API gas oil is blended with 2000 cubic meters of 15°API fuel oil. What is the density of the resultant mixture in kg/m 3 ? The density of water at 288.5 K = 0.999 g/ml. Assume no volume change on mixing. 100 liter each of gasoline (55°API), kerosene ( 40°API), gas oil (31°API), and isopentane (96°API) are mixed. The density of water at 288.5 K = 0.999 g/ mL. Determine the density of the mixture in kg/m 3 . What is the specific gravity in °API? Express the composition of the mixture in weight percent.

73. Concentration Problem Solving

74. Definition Concentration refers to the amount of solute present in a given amount of solvent or solution. It is a measure of the quantity of a substance dissolved or dispersed in a particular volume of the mixture. Concentration is an essential concept in chemistry, biochemistry, and various other fields, as it helps describe the properties and behavior of solutions. There are several ways to express the concentration of a solution, depending on the context and the specific application: Mass per unit volume such as lb m of solute/ft 3 of solution, g of solute/L, lb m of solute/ bbl , kg of solute/m 3 . Moles per unit volume such as lb mol of solute/ft 3 of solution, g mol of solute/L, g mol of solute/cm 3 . 74 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

75. Continued…… Mass (weight) fraction —the ratio of the mass of a component to the total mass of the mixture, a fraction (or a percent). Mole fraction —the ratio of the moles of a component to the total moles of the mixture, a fraction (or a percent). Parts per million (ppm) and parts per billion (ppb) —a method of expressing the concentration of extremely dilute solutions; ppm is equivalent to a mass (weight) ratio for solids and liquids. It is a mole ratio for gases. Parts per million by volume (ppm v ) and parts per billion by volume (ppb v ) —the ratio of the volume of the solute per volume of the mixture (usually used only for gases). 75 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

76. Other expressions for Concentration Molality Molality (usually denoted by the symbol "m") is a concentration unit used in chemistry to express the amount of solute in a solution relative to the mass of the solvent.   Molarity Molarity (often denoted by the symbol "M") is a common unit of concentration used in chemistry to express the amount of solute dissolved in a given volume of solution. It represents the number of moles of solute (n) per liter of solution (V). 76 Normality Normality (often denoted by the symbol "N") is another unit of concentration used in chemistry, especially in acid-base reactions and redox reactions. It represents the number of equivalent units of solute (acid, base, or oxidizing/reducing agent) per liter of solution. Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

77. Problem: In normal living cells, the nitrogen requirement for the cells is provided from protein metabolism (i.e., consumption of protein in the cells). When cells are grown commercially such as in the pharmaceutical industry, (NH 4 ) 2 SO 4 is usually used as the source of nitrogen. Determine the amount of (NH 4 ) 2 SO 4 consumed in a fermentation medium in which the final cell concentration is 35 g/L in a 500 L volume of fermentation medium. Assume that the cells contain 9 wt % N, and that (NH 4 ) 2 SO 4 is the only nitrogen source. 77 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

78. Problem: The current OSHA 8 hr limit for HCN in air is 10.0 ppm. A lethal dose of HCN in air is (from the Merck Index) 300 mg/kg of air at room temperature. How many milligrams of HCN per kilogram of air is 10.0 ppm? What fraction of the lethal dose is 10.0 ppm? 78 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

79. 79 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) How many milligrams per liter are equivalent to a 1.2% solution of a substance in water? The danger point in breathing sulfur dioxide for humans is 2620 μg /m 3 . How many ppm is this value? The specific gravity of a solution of KOH at 15°C is 1.0824 and contains 0.813 lb KOH per gal of solution. What are the mass fractions of KOH and H 2 O in the solution? You purchase a tank with a volume of 2.1 ft 3 . You pump the tank out and add first 20 lb of CO 2 gas and then 10 lb of N 2 gas. What is the analysis of the gas mixture in the tank? Twenty-seven pounds (27 lb ) of chlorine gas is used for treating 750,000 gal of water each day. The chlorine used up by the microorganisms in the water is measured to be 2.6 mg/L. What is the residual (excess) chlorine concentration in the treated water?

80. 80 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) A radioactive tracer-labeled microorganism (MMM) decomposes to NN as follows: If the CO 2 (g) yields 2×10 7 dpm (disintegrations per minute) in a detection device, how many μCi (microcuries) is this? How many cpm (counts per minute) will be noted if the counting device is 80% efficient in counting disintegrations? Data: 1 curie = 3×10 10 dps (disintegrations per second). The National Institute for Occupational Safety and Health (NIOSH) sets standards for CCl 4 in air at 12.6 mg/m 3 of air (a time-weighted average over 40 hr). The CCl 4 found in a sample is 4800 ppb. Does the sample exceed the NIOSH standard? A gas contains 350 ppm of H 2 S in CO 2 . If the gas is liquefied, what is the weight fraction of H 2 S?  

81. 81 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) Several alternative compounds have been added to gasoline, including methanol, ethanol, and methyl tert-butyl ether (MTBE), to increase the oxygen content of gasoline in order to reduce the formation of CO on combustion. Unfortunately, MTBE has been found in groundwater at concentrations sufficient to cause concern. Persistence of a compound in water can be evaluated from its half-life, , that is, the time for one-half of the compound to leave the system of interest. The half-life depends on the conditions in the system, of course, but for environmental evaluation can be approximated by where is the concentration of hydroxyl radical in the system that for this problem of the contamination of water is equal to 1.5×10 6 molecules/cm 3 . The values of k determined from experiment are Calculate the half-life of each of the three compounds, and order them according to their persistence.   Methanol Ethanol MTBE Methanol Ethanol MTBE

82. 82 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) The following table shows the annual inputs of phosphorus to Lake Erie A Short Tons/Yr Source Lake Huron Lake drainage Municipal waste Industrial waste 2240 6740 19,090 2030 Total of sources Outflow 30,100 4500 Retained 25,600 Convert the retained phosphorus to concentration in micrograms per liter, assuming that Lake Erie contains 1.2×10 14 gal of water and that the average phosphorus retention time is 2.60 yr. What percentage of the input comes from municipal water? What percentage of the input comes from detergents, assuming they represent 70% of the municipal waste? If 10 ppb of phosphorus triggers nuisance algal blooms, as has been reported in some documents, would removing 30% of the phosphorus in the municipal waste and all the phosphorus in the industrial waste be effective in reducing the eutrophication (i.e., the unwanted algal blooms) in Lake Erie? Would removing all of the phosphate in detergents help?

83. Temperature Relative scale Absolute scale Unit change

84. Definition Temperature is a measure of the average kinetic energy of the particles in a substance or system. It is a fundamental physical quantity that characterizes the hotness or coldness of an object or the environment. Temperature is an essential concept in physics, thermodynamics, and everyday life, influencing a wide range of natural processes and human activities. The SI unit for temperature is the kelvin (K), but Celsius (°C), Fahrenheit (°F) and Rankine (°R) are also commonly used in different regions of the world. 84 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

85. Temperature Scales Relative Scale ( °C & °F ) A relative temperature scale does not have a true zero point, and temperatures are measured and expressed relative to a specific reference point. In other words, relative temperature values indicate the difference in temperature between two points or states, but they do not convey information about the absolute temperature value. Absolute Scale ( K & °R ) An absolute temperature scale has a true zero point, representing the complete absence of heat or the lowest possible temperature. Absolute temperature values are measured in terms of the actual kinetic energy of the particles in a substance. 85 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

86. Temperature Conversions ( Unit Degree change) 86 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

87. Problem: The heat capacity of sulfuric acid in a handbook has the units and is given by the relation where T is expressed in degrees Celsius. Modify the formula so that the resulting expression yields the heat capacity with the associated units of with T in degrees Rankine.   87 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

88. Pressure Gauge pressure Absolute pressure Atmospheric pressure Differential Pressure

89. Definition Pressure is a fundamental physical quantity used to describe the force exerted per unit area on a surface. It is an essential concept in physics, engineering, and various scientific and industrial applications. Pressure is caused by the collisions of particles (atoms or molecules) with the walls of a container or a surface, resulting in a force per unit area. The SI unit for pressure is the pascal (Pa), which is defined as one newton per square meter (N/m²). However, other units such as atmospheres (atm), millimeters of mercury (mm Hg), and pounds per square inch (psi) are also commonly used depending on the context. 89 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

90. Various forms of Pressure Atmospheric Pressure ( p o ) Atmospheric pressure is the pressure exerted by the Earth's atmosphere on the surface of the Earth. At sea level, the average atmospheric pressure is approximately 101.3 kPa (kilopascals) or 1 atm (atmosphere). Gauge Pressure ( p g ) Gauge pressure is the pressure measured relative to the atmospheric pressure. It is the difference between the total pressure and atmospheric pressure. When a pressure gauge indicates zero, it means the pressure is equal to atmospheric pressure. 90 Absolute Pressure ( p abs ) Absolute pressure is the total pressure measured relative to absolute vacuum (zero pressure). It includes both the atmospheric pressure and the gauge pressure.   Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

91. Problem: The pressure gauge on a tank of CO 2 used to fill soda-water bottles reads 51.0 psi. At the same time the barometer reads 28.0 in. Hg. What is the absolute pressure in the tank in psia? 91 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

92. Problem: Small animals such as mice can live at reduced air pressures down to 20 kPa absolute (although not comfortably). In a test, a mercury manometer attached to a tank as shown in Figure reads 64.5 cm Hg and the barometer reads 100 kPa. Will the mice survive? 92 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

93. Differential Pressure Definition Differential pressure refers to the difference in pressure between two points in a fluid or gas system. It is the contrast between the pressure at one location and the pressure at another location within the same system. This concept is used in various engineering applications to measure, monitor, and control processes. Differential pressure is commonly measured using devices called pressure gauges, pressure transmitters, or manometers. These devices compare the pressure at two different points and display or transmit the difference as a reading. 93 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)  

94. 94 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) A U-tube manometer filled with mercury is connected between two points in a pipeline. If the manometer reading is 26 mm Hg, calculate the pressure difference in kilopascals between the points when (a) water is flowing through the pipeline, and (b) air at atmospheric pressure and 20°C with a density of 1.20 kg/m 3 is flowing in the pipeline. A problem with concrete wastewater treatment tanks set belowground was realized when the water table rose and an empty tank floated out of the ground. This buoyancy problem was overcome by installing a check valve in the wall of the tank so that if the water table rose high enough to float the tank, it would fill with water. If the density of concrete is 2080 kg/m 3 , determine the maximum height at which the valve should be installed to prevent a buoyant force from raising a rectangular tank with inside dimensions of 30 m by 27 m that is 5 m deep. The walls and floor have a uniform thickness of 200 mm. A centrifugal pump is to be used to pump water from a lake to a storage tank that is 148 ft above the surface of the lake. The pumping rate is to be 25.0 gal/min, and the water temperature is 60°F. The pump on hand can develop a pressure of 50.0 psig when it is pumping at a rate of 25.0 gal/min. (Neglect pipe friction, kinetic energy effects, and factors involving pump efficiency.) How high (in feet) can the pump raise the water at this flow rate and temperature? Is this pump suitable for the intended service?

95. 95 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) A manufacturer of large tanks calculates the mass of fluid in the tank by taking the pressure measurement at the bottom of the tank in psig , and then multiplying that value by the area of the tank in square inches. Can this procedure be correct? Suppose that a submarine inadvertently sinks to the bottom of the ocean at a depth of 1000 m. It is proposed to lower a diving bell to the submarine and attempt to enter the conning tower. What must the minimum air pressure be in the diving bell at the level of the submarine to prevent water from entering the bell when the opening valve at the bottom is cracked open slightly? Give your answer in absolute kilopascals. Assume that seawater has a constant density of 1.024 g/cm 3 . A pressure gauge on a welder’s tank gives a reading of 22.4 psig . The barometric pressure is 28.6 in. Hg. Calculate the absolute pressure in the tank in (a) lb /ft 2 , (b) in. Hg, (c) N/m 2 , and (d) ft water. John Long says he calculated from a formula that the pressure at the top of Pikes Peak is 9.75 psia. John Green says that it is 504 mm Hg because he looked it up in a table. Which John is right?

96. 96 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101) The floor of a cylindrical water tank was distorted into 7 in. bulges because of the settling of improperly stabilized soil under the tank floor. However, several consulting engineers restored the damaged tank to use by placing plastic skirts around the bottom of the tank wall and devising an air flotation system to move it to an adjacent location. The tank was 30.5 m in diameter and 13.1 m deep. The top, bottom, and sides of the tank were made of 9.35-mm-thick welded steel sheets. The density of the steel is 7.86 g/cm 3 . What was the gauge pressure in kilopascals of the water at the bottom of the tank when it was completely full of water? What would the air pressure have to be in kilopascals beneath the empty tank in order to just raise it up for movement? Oil (density = 0.91g/cm 3 ) flows in a pipe, and the flow rate is measured via a mercury (density = 13.546 g/cm 3 ) manometer. If the difference in height of the two legs of the manometer is 0.78 in., what is the corresponding pressure difference between points A and B in mm Hg? At which point, A or B, is the pressure higher? The temperature is 60°F.

97. Assignment A poundal is the force required to accelerate a mass of 1lb m at a rate of 1ft/s 2 , and a slug is the mass of an object that will accelerate at a rate of 1ft/s 2 when subjected to a force of 1lb f . Calculate the mass in slugs and the weight in poundals of a 175 lb m man ( i ) on earth and (ii) on the moon, where the acceleration of gravity is one-sixth of its value on earth. A force of 355 poundals is exerted on a 25.0 slug object. At what rate (m/s 2 ) does the object accelerate? Due Date: October 4, 2024 (03 marks) CLO 1 attainment [ Note: Marks will be deducted upon late submission] 97 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

98. Assignment 215 kg of mercury was found to occupy 0.560 ft 3 at 20°C. (1) What volume would the mercury occupy at 100°C? (2) Suppose the mercury is contained in a cylinder having a diameter of 0.25 in. What change in height would be observed as the mercury is heated from 20°C to 100°C? A 0.50-molar aqueous solution of sulfuric acid flows into a process unit at a rate of 1.25 m 3 /min. The specific gravity of the solution is 1.03. Calculate (1) the mass concentration of H 2 SO 4 in kg/m 3 , (2) the mass flow rate of H 2 SO 4 in kg/s, and (3) the mass fraction of H 2 SO 4 . Due Date: October 4, 2024 (03 marks) CLO 1 attainment [ Note: Marks will be deducted upon late submission] 98 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

99. Assignment A gas stream contains 18.0 mole% hexane and the remainder nitrogen. The stream flows to a con­denser, where its temperature is reduced and some of the hexane is liquefied. The hexane mole fraction in the gas stream leaving the condenser is 0.05. Liquid hexane condensate is recovered at a rate of 1.50 L/min. What is the flow rate of the gas stream leaving the condenser in mol/min? ( Hint: First calculate the molar flow rate of the condensate and note that the rates at which C 6 H 14 and N 2 enter the unit must equal the total rates at which they leave in the two exit streams.) What percentage of the hexane entering the condenser is recovered as a liquid? Due Date: October 4, 2024 (03 marks) CLO 1 attainment [ Note: Marks will be deducted upon late submission] 99 Introductory Lecture Notes Industrial Stoichiometry-I (Ch.E. – 101)

100. THANKS!!!