...This page intentionally left blank SEVENTH EDITION Fundamentals of Heat and Mass Transfer THEODORE L. BERGMAN Department of Mechanical Engineering University of Connecticut ADRIENNE S. LAVINE Mechanical and Aerospace Engineering Department University of California, Los Angeles FRANK P. INCROPERA College of Engineering University of Notre Dame DAVID P. DEWITT School of Mechanical Engineering Purdue University JOHN WILEY & SONS VICE PRESIDENT & PUBLISHER EXECUTIVE EDITOR EDITORIAL ASSISTANT MARKETING MANAGER PRODUCTION MANAGER PRODUCTION EDITOR DESIGNER EXECUTIVE MEDIA EDITOR PRODUCTION MANAGEMENT SERVICES Don Fowley Linda Ratts Renata Marchione Christopher Ruel Dorothy Sinclair Sandra Dumas Wendy Lai Thomas Kulesa MPS Ltd. This book was typeset in 10.5/12 Times Roman by MPS Limited, a Macmillan Company and printed and bound by R. R. Donnelley (Jefferson City). The cover was printed by R. R. Donnelley (Jefferson City). Founded in 1807, John Wiley & Sons, Inc. has been a valued source of knowledge and understanding for more than 200 years, helping people around the world meet their needs and fulfill their aspirations. Our company is built on a foundation of principles that include responsibility to the communities we serve and where we live and work. In 2008, we launched a Corporate Citizenship Initiative, a global effort to address the environmental, social, economic, and ethical challenges we face in our business. Among the issues we are addressing...
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...Efficient use and installation of Thermal Mass to utilize solar thermal energy Submitted to: Dr. M.S. Soni Submitted by: Prateek Jain(2011B1A4696P) Chintan Singhvi(2011B2A4811P) Contents ABSTRACT...................................................................................................................................................... 3 KEY WORDS ................................................................................................................................................... 3 BASIC OPERATING PRINCIPLE ....................................................................................................................... 3 INTRODUCTION ............................................................................................................................................. 4 THEORY ......................................................................................................................................................... 6 METHODOLOGY .......................................................................................................................................... 10 Data Collected: ............................................................................................................................................ 11 Analysis of material thermal properties and performance: ................................................................... 11 Measurements of the hostel rooms: ...........................
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...The Changes of Heat in Calorimetry Summary The purpose of this experiment is to learn how heat flows into and through an unknown substance while using a calorimeter to measure the temperature. In this set of experiments we will focus our attention upon one particular area of thermodynamics, calorimetry, a technique used to measure heat flow into and out of matter. This is really simple procedure. The unknown metal is placed into a container called a calorimeter that separates it from everything else. As changes occur, we can follow the movement of heat from one portion of the matter to another by the temperature changes. The container we use as a calorimeter should insulate the metal, it should prevent matter from entering or exiting once our measurement has begun, and it should allow for easy measurement of temperature changes. A reasonable calorimeter can be constructed from a pair Styrofoam cups with lid on top to limit heat transfers into and out of the cups. Introduction The amount of heat, Q, required to raise the temperature of a solid body at constant pressure depends on the change in temperature, ∆T, of the body, its mass, m, and a characteristic of the material forming the body called its specific heat, C. This relationship is expressed by the equation Q = mC∆T and the dimensions of C are thus heat per unit mass per unit temperature change. The values of C do depend on temperature with those of the unknown metal. Specific heat can be considered to be the amount...
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...HEAT 4.1 UNDERSTANDING THERMAL EQUILIBRIUM 1. Define: The measure of the degree of hotness of an object. (a) Temperature Measured in SI unit Kelvin, K A hot object is at a higher temperature than a cold object. Form of energy, measured in Joules, J (b) Heat Heat is transferred from hotter object (higher temperature) to colder object (lower temperature) When an object is heated, it will absorb heat energy and the temperature will increase. When an object is cooled, it will release heat energy and the temperature will decrease. (c) Thermal Two objects are in thermal contact when heat energy contact can be transferred between them. (d)Heat transfer When two objects with different degrees of hotness come into thermal contact, heat energy is transferred between the two objects. (e) Mechanism of Thermal Equilibrium Energy is transferred at a faster rate from the hotter object to the colder object. Energy is also transferred from the colder object to the hotter one, but at a slower rate. There is a net flow of energy from the hotter object to the colder object. (f) Thermal When two objects are in thermal equilibrium, there is Equilibrium no net flow of heat between them. Two objects in thermal equilibrium have the same temperature 60 The hotter object cools down while the colder object warms up . After some time, energy is transferred at the same rate between the two objects. There is no net heat transfer between the objects. The two objects are said to be in thermal equilibrium...
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...Title: Specific Heat of a Metal Purposes: Be able to measure specific heat. Be able to use a calorimeter correctly. Be able to find and measure the specific heat of a metal. Calculate the change in water temperature. Hypothesis: The specific heat of the metal sample (lead) will be very low. Safety: goggles, apron, hair restraints, Bunsen burner, heated water, harmful metals, breakable glass containers Materials: goggles and apron, beaker (250 mL or 400 mL) , hot plate/burner with ring stand, ring, and wire gauze, test tube(18 x 150 mm), plastic foam cup, thermometer, balance Procedure: 1. Put on goggles and apron. 2. Fill beaker half way with water. Put beaker on ring stand with wire gauze. Heat beaker with water to boiling point. 3. Fill test tube half way with metal 4. Put a weight boat on the balance. Pour metal from test tube into the weight boat. Record weight and pour metal back into test tube. 5. Put test tube of metal into the water. Leave inside the beaker of boiling water while completing step 6 and 7. 6. Use the foam cup as calorimeter. Measure mass and record. 7. Fill foam cup with room temperature water and record mass. 8. Put thermometer in test tube and record temperature. 9. Put thermometer inside the foam cup and record the temperature of the water. 10. Take test tube out of the boiling water and immediately pour inside the foam cup. 11. Stir the water and record highest temperature. 12. Pour water out,...
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...CHM130 Lab 4 Calorimetry Name: Data Table: (12 points) |ALUMINUM METAL | | |Pre-weighed Aluminum metal | | |sample mass (mmetal) |19.88 | |Temperature of boiling water and metal sample in | | |the pot (Ti(metal)) | | | | | | | | | | | |dsdfa(Ti | | |Temperature of cool water in | | |the calorimeter prior to adding hot metal sample | | |(Ti(water)) | | |Maximum Temperature of | ...
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...experiment was to measure the latent heat of ice. The value of the latent heat of ice was obtained by measuring the amount of boiling water needed to melt a given mass of ice. After repeating the procedure three times, the latent heat of ice was calculated for each test, and then averaged. The heat released by the boiling water is the product of specific heat, mass, and temperature change, while the heat required to melt the ice is the product of the mass of ice and the latent heat. (1) Einitial = Mwatercpwater (Tw) + Micecpice (Tice) (2) Efinal = Mwatercpwater (Tw) + Micecpice (Tice) + MiceLice, where M is defined as mass, cp is specific heat, and Lice is the latent heat of ice. Then, the First Law of Thermodynamics dictates that the change in Energy is equal to zero, and the final Energy is equal to the initial Energy. Thus, latent heat was calculated by substituting experimental values for mass and the literature values for specific heat. The averaged values of the latent heat of ice was computed to be 233.6 kJ/kg—a percent error of 30.1% from the literature value of 334 kJ/kg. These equations and relationships are based on several assumptions. The heat transfer from the boiling water is assumed to only melt the ice, and that no heat had been lost to the environment. It is also assumed that the temperature after melting the ice was 0 oC, and so the change in temperature is the full range between 0oC and 100oC. Lastly, there is no net work and mass flow. Also, the final volume of...
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...Energy Balance on RV1 Component Molecular mass (kg kmol-1) Component Molecular mass (kg kmol-1) Na+ 23 NaHCO3 84 Ca2+ 40 Na2CO3 106 Cl- 35.5 CO2 44 NaCl 58.5 H2O 18 CaCl2 111 CaCO3 100 Table 1: Relative molecular mass values for all components in system Data was taken from Tuesday 11:28-11:40. Flow rates and temperatures throughout this period were fairly constant and so the mean values were found using the density of water at the relevant temperature (it was assumed that all streams in the process have the density of water). Data for the density of water was taken from Perry (1999). An example calculation for the mean product flow rate is shown below: m ̇=ρV ̇ m ̇=(4.63*60*991.77)/1000=275.7 kg h^(-1) A mass balance was then carried out on the whole system. The product specification was taken as 1% w/w Na+. From this, the amount of feedstock added, the amount and composition of material leaving the reactor and the composition of the recycle stream were found: Figure 1: Block diagram of overall process Assuming the product was on specification (1% w/w Na+), the mass of sodium ions in the product can be obtained by simply finding 1% of the total mass flow of product (2.755 kg h-1). Converting to molar flow rate using the molecular weight of sodium ions, the amount of chloride ions was found using a stoichiometric balance. 2NaHCO3 Na2CO3 + H2O + CO2 (1) Na2CO3 + CaCl2 CaCO3 + 2NaCl (2) n ̇=m ̇/RMM=2.755/23=0.12 kmol h^(-1) One mole...
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...SPH 3U1 Practical Examination Specific Heat Capacity of TCI Tap Water Date: 14th July 2014 Title: Specific Heat Capacity of water Purpose: To find the specific heat capacity of TCI tap water Hypothesis: I hypothesize that the specific heat capacity of water will be 4200 J/kg°C because water is known to have a high heat capacity Apparatus: * Top Pan Balance * Kettle * Alcohol Thermometer * Pencil * Paper * Water Procedure: 1. Record the mass of the empty kettle 2. Fill kettle with water 3. Record the mass of kettle with water 4. Calculate mass of water 5. Turn on kettle and place thermometer in kettle 6. Record the temperature on the thermometer every 30 seconds until the temperature reaches 100°C Readings: PKettle = 1200W mKettle = .946kg mKettle and Water = 2.402kg mwater = 1.456kg Theory: EH=mc∆T The relationship between heat energy, the mass of the substance, the specific heat capacity of the substance and temperature can be expressed in the equation above. The heat energy in joules required to heat a given substance to a certain temperature is equal to the mass of the substance heated multiplied by the value of the specific heat capacity of the substance multiplied by the difference between the initial temperature and the temperature of the substance after heating In this lab, the energy used to heat the water is calculated from the power of the kettle. The mass of the water is recorded after weighing...
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...Introduction The molar heat of combustion of a substance is the heat liberated when 1 mole of the substance undergoes complete combustion with oxygen at standard atmosphere pressure with products being CO₂ and H₂O and also releases heat in this process. The heat of combustion is commonly measured experimentally, where the combustions are always exothermic reactions. During combustion hydrocarbon bonds are broken and new ones are created for example; when ethanol combusts with the 3O₂ molecules it breaks the C-H bonds and the other hydrocarbon bonds that are in the ethanol molecule also break resulting in the release of energy and on once these bonds are broken and new molecules are formed and these new molecules are the products of the ethanol...
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...Design of heat exchangers required for a 50-100kW superheated Rankine cycle MECH 421 Huzeyfe SHAHIN Gokce SAGIR Usman Arshad SHAH 28th December 2015 Table of Contents 1. ABSTRACT .............................................................................................................................................. 3 2. INTRODUCTION ..................................................................................................................................... 3 3. LITERATURE REVIEW ............................................................................................................................. 3 4. SIMPLE DESIGN ..................................................................................................................................... 3 4.1 Evaporator at 800 kPa (Counter Flow) ................................................................................................ 4 4.1.1 Preheater ..................................................................................................................................... 4 4.1.2 Boiler ............................................................................................................................................ 4 4.1.3 Superheater ................................................................................................................................. 5 4.2 Evaporator at 800 kPa (Shell & Tube) ............................................
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...initial temperature of the hot water less complicated calculations find mass of cold water, and mass of mixed water are done by subtracting the total mass of (mixed or cold )waters and cup combined by the mass of the cup alone. Equation 1 Mass of Water and cup – Mass of cup = Mass of water Ex. From calculating mass of mixed water trial 1 139.786 g of mixed water and cup -15.436 g of cup = 124.35 g of mixed water 90.334 g of cold water and cup -15.436 g of cup = 74.898 g of cold water Another less complicated calculation was done to find the mass of hot water Equation 2 Mass of Mixed water-mass of cold Water = mass of Hot Water Ex. From trial 1 124.35 g of mixed water - 74.898 g of cold water=49.452 g of hot water Next in order to calculate the initial temperature of the hot water without being able to measure it with a thermometer the Calorimetry equation 3 must be used. Equation 3 q=m×C ×∆T * q is the heat change of the system (joules, J) * m is the mass(grams, g) * ∆T is the Temperature change, Tfinal-TinitialC * C is the specific heat for that substance(Jg ° C) After calculating the Heat change of the system using equation one we can use equation two ; The law of conservation of energy which states that while energy can be converted or transferred, it is not created or destroyed. Equation 4 qsystem + qsurroundings=0 Or qsystem = -qsurroundings Therefore if the heat change of the surroundings are known then the system and all of its...
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... Physical and Chemical Changes 1.8 Temperature 2.2 Classification of Matter 1.9 What is Thermometer? 2.3 Mixtures & Pure Substances 1.10 Heat and Thermodynamics 2.4 Matter and its Phases 1.11 Energy Mass Relationship 2.5 Properties of Matter 1.12 Personal Reaction 2.6 ENERGY 2.7 Heat Energy 2. Matter and Energy 3.8 Physical and Chemical Changes 1.8 Temperature 3.9 Classification of Matter 1.9 What is Thermometer? 3.10 Mixtures & Pure Substances 1.10 Heat and Thermodynamics 3.11 Matter and its Phases 1.11 Energy Mass Relationship 3.12 Properties of Matter 1.12 Personal Reaction 3.13 ENERGY 3.14 Heat Energy Matter and Energy Matter and Energy 1. Matter & Energy Anything that we can see, touch or sense is made up of matter. The computer screen, the keyboard in front of you, the air that you breathe, the water that you drink are all examples of matter. Matter is anything that occupies space and has mass. Energy is not the same as matter, although the two are closely related and associated. Energy has the ability to move matter. Matter is converted into energy in nuclear reactors and nuclear bombs. Matter...
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...Reference: Mr. Smith’s Instructions B. Problem: To calculate the specific heat of Lead. C. Hypothesis: If the heat absorbed by water when lead is added is known then the specific heat of lead can be calculated. D. Theory: i. In this experiment it is assumed that the density of liquid water is 1.00 g/mL ii. The equation qlost = -qgained can be applied when the change in temperature of the water is calculated. The energy gained by the water is equal to the energy lost by the lead. iii. The equation q =m ×Cp ×∆T can be simplified to solve for lead’s specific heat (Cp) once the heat of lead (q) is solved for using the equation shown in (ii). E. Variables: i. Independent: type of metal (Pb) ii. Dependent: final temperature of water iii. Control: temperature and pressure of the lab environment, the volume of water II. Experimental Design A. Equipment: i. Hot plate ii. 200 mL tap water iii. Balance iv. Styrofoam calorimeter v. 250 mL beaker vi. Test tube vii. Lab Quest viii. Lab Quest temperature probe ix. Test tube clamp B. Chemicals: metal shot (Lead - Pb) C. Apparatus: D. Method: i. Heat 150 mL water in the 250 mL beaker on the hot plate at its highest setting ii. Add the metal (Pb) shots into the test tube and place the test tube into the heating water iii. When the water boils, turn down the heat setting so that the water is barely boiling iv. Place 9 mL of water into...
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...Heat of Fusion of Water 4-1: Heat of Fusion of Water The molar heat of fusion for a substance, ∆Hfus, is the heat required to transform one mole of the substance from the solid phase into the liquid phase. In this assignment, you will use a simple coffee cup calorimeter and a thermometer to measure the molar heat of fusion for water. 1. Start Virtual ChemLab, select Colligative Properties, and then select Heat of Fusion of Water from the list of assignments. The lab will open in the Calorimetry laboratory with a beaker of ice on the balance and a coffee cup calorimeter on the lab bench. 2. Click on the Lab Book to open it. Record the mass of the ice on the balance in the data table. If the mass is too small to read, click on the Balance area to zoom in. Note that the balance has already been tared for the mass of the empty beaker. 3. 100 mL of water is already in the coffee cup. Use the density of water at 25 C (0.998 g/mL) to determine the mass of water from the volume. Record the mass in the data table. Make certain the stirrer is On (you should be able to see the shaft rotating). In the thermometer window, click Save to begin recording data to the lab book. Allow 20-30 seconds to obtain a baseline temperature of the water. 4. Drag the beaker from the balance area until it snaps into place above the coffee cup and then pour the ice into the calorimeter. Click the thermometer and graph windows...
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