PHYSICS 220. Lecture 24. Textbook Sections Lecture 25 Purdue University, Physics 220 1
|
|
- Bennett Spencer
- 5 years ago
- Views:
Transcription
1 PHYSICS 220 Lecture 24 Heat Textbook Sections Lecture 25 Purdue University, Physics 220 1
2 Exam 2 Average: 96.7 out of 150 Std Dev: 30.5 Lecture 25 Purdue University, Physics 220 2
3 Overview Last Lecture Thermal Expansion ΔL = α L 0 ΔT (linear expansion) ΔV = β L 0 ΔT (volume expansion) Kinetic Theory of Monatomic Ideal Gas <K tr >=3/2k B T Today Heat Specific Heat Phase Transitions Lecture 25 Purdue University, Physics 220 3
4 Quiz 1) A pendulum is made from an aluminum rod with a mass attached to its free end. If the pendulum is cooled does the pendulum's period A) increase B) decrease C) stay the same 2) A steel tape measure is marked in such a way that it gives accurate length measurements at a normal room temperature of about 20 C. If this tape measure is used outdoors on a cold day when the temperature is 0 C, are its measurements A) too long B) too short C) accurate Lecture 25 Purdue University, Physics 220 4
5 Internal Energy Energy of all molecules including Random motion of individual id molecules l <K tr > = 3/2 k T for ideal gas Vibrational energy of molecules and atoms Chemical energy in bonds and interactions DOES NOT INCLUDE Macroscopic motion of object Potential energy due to interactions with other objects Lecture 25 Purdue University, Physics 220 5
6 Heat Definition: Flow of energy between two objects due to difference in temperature Note: similar to WORK Object does not have heat (it has energy) Units: calorie Amount of heat needed to raise 1g of water 1ºC 1 Calorie = 1 kcal = 1000 cal = 4186 Joules Heat flows from a system at higher temperature to one at lower temperature Lecture 25 Purdue University, Physics 220 6
7 Heat The energy that flows between the systems is called heat or heat energy Heat is energy that passes from one system to another by virtue of a temperature difference The terms heat and heat energy are often used interchangeably In physics, they always refer to the transfer of energy between systems According to the principle of conservation of energy, the amount of heat energy that leaves system 1 must equal the amount of heat energy that enters system 2 The transfer can take place in different ways The direction of the transfer depends only on the temperature difference Lecture 25 Purdue University, Physics 220 7
8 Units of Heat The SI unit of heat is the same as for energy, the Joule (J) A unit called the calorie is widely used for heat 1 cal = J The Calorie, with an uppercase C, is used to measure the energy content of food 1 Calorie = 1000 calories So 1 food Calorie is a kcal Lecture 25 Purdue University, Physics 220 8
9 Heat and Mechanical Energy James Joule measured the mechanical equivalent of heat energy The apparatus he used is similar to the one shown As the mass fell, its potential energy rotated the paddle, raising the temperature of the liquid Joule could then relate the mechanical energy to the heat energy Lecture 25 Purdue University, Physics 220 9
10 Heat Capacity and Specific Heat Heat capacity is the ratio between the heat energy added to a system and the resulting change in temperature Q heat capacity = ΔTT Specific heat takes into account the size (mass) of the system specific heat = c = Q mδt Lecture 25 Purdue University, Physics
11 Specific Heat Heat adds energy to object/system IF system does NO work then: Heat increases internal energy: Q = ΔU Heat increases temperature: t Q = C ΔTT Q = c m ΔT Heat required to increase temperature depends on amount of material (m) and type of material (c) Q = cmδt : Cause = inertia x effect (just like F=ma) cause = Q effect = ΔT inertia = cm (mass x specific heat capacity) c specific heat ΔT = Q/cm (just like a = F/m) Lecture 25 Purdue University, Physics
12 Exercise After a grueling work out, you drink a liter of cold water (0 C). How many Calories does it take for your body to raise the water up to body temperature peaueof 36C C? A) 36 B) 360 C) 3,600 D) 36,000 1 liter = 1,000 grams of H g x 1 calorie/(gram degree) x (36 degree) = 36,000 calories 36,000 calories = 36 Calories! Lecture 25 Purdue University, Physics
13 Question Suppose you have equal masses of aluminum and copper at the same initial temperature. You add 1000 J of heat to each of them. Which one ends up at the higher final temperature A) aluminum B) copper C) the same Substance c in J/(kg-C) aluminum 900 copper 387 iron 452 lead 128 human body 3500 water 4186 ice 2000 ΔT =Q/cm Lecture 25 Purdue University, Physics
14 ILQ Two insulated buckets contain the same amount of water at room temperature. Two blocks of metal of the same mass, both at the same temperature, are warmer than the water in the buckets. One block is made of aluminum (c=0.9) and one is made of copper. You put the aluminum block into one bucket of water, and the copper (c=0.385) block into the other. After waiting a while you measure the temperature of the water in both buckets. Which is warmer? A) The water in the bucket containing the aluminum block B) The water in the bucket containing the copper block C) The water in both buckets will be at the same temperature Since aluminum has a higher specific heat than copper, you are adding more heat to the water when you dump the aluminum in the bucket (Q=mcΔT). Lecture 25 Purdue University, Physics
15 Specific Heat for Ideal Gas Monatomic Gas (single atom) Translational kinetic energy only At constant Volume work = 0 Q = ΔU = 3/2 nrδt C V = 3/2 R = 12.5 J/(K mole) Diatomic Gas (two atoms) Can also rotate C V = 5/2 R = 20.8 J/(K mole) Lecture 25 Purdue University, Physics
16 Latent Heat As you add heat to water, the temperature increases for a while, then it remains constant, t despite the additional heat! 100 o C Substance L f (J/kg) L v (J/kg) water 33.5 x x 10 5 f=fusion T v=vaporization water water changes temp to steam rises (boils) Latent Heat Q added to water steam temp rises Latent Heat L [J/kg] is heat which must be added (or removed) for material to change phase (liquid-gas). Q = m L Lecture 25 Purdue University, Physics
17 Phases of Matter There are three states t of matter: Solid Liquid Gas Lecture 25 Purdue University, Physics
18 Solids The atoms in many solids are arranged in an orderly and repeating pattern called a crystalline lattice Each atom is held in place by the forces exerted by neighboring atoms These forces are a result of chemical bonds within the solid The atoms actually vibrate about their positions as simple harmonic oscillators An amorphous solid has atoms arranged without the repeating structure found in a crystal Lecture 25 Purdue University, Physics
19 Liquids The atoms in a liquid are not held in fixed locations by the forces of neighboring atoms The atoms are able to move about The atoms adjacent to a particular atom are not likely to be adjacent a short time later This motion helps liquids to flow Although the bonds between neighboring atoms do not persist, there is still potential energy associated with the forces between the molecules Lecture 25 Purdue University, Physics
20 Gases In some ways, a gas is similar to a liquid The molecules are able to move over long distances The density of a gas is generally much lower than that of a liquid The spacing between the molecules of a gas is larger The magnitude of the intermolecular force, and therefore potential energy, is much smaller Most of the mechanical energy in a gas is found in the kinetic energies of its molecules Lecture 25 Purdue University, Physics
21 Internal Energy The mechanical energy of the molecules in a system is called the internal energy of the system Denoted by U The internal energy of a system is the sum of all potential energies associated with all the intermolecular bond plus the kinetic energies of all the molecules The value of U increases as we go from solid to liquid to gas In general, the internal energy of all systems increases as the temperature is increased Lecture 25 Purdue University, Physics
22 Phase Transitions A phase transition occurs whenever a material is changed from one phase, such as the solid phase, to another phase, such as the liquid phase. Phase transitions occur at constant temperature. The latent heat of vaporization L V is the heat per unit mass that must flow to change the phase from liquid to gas or from gas to liquid. Fusion occurs when a liquid id turns into a solid. Evaporation occurs when a liquid turns into a gas. Sublimation occurs when a solid changes directly to a gas without going into a liquid form. Lecture 25 Purdue University, Physics
23 Phase Changes The transformation of a solid to a liquid, a liquid to a gas, etc. is called a phase change Phase changes can be produced by changing the temperature or by changing g the pressure of the system A phase diagram shows the phases found at different temperatures and pressures Lecture 25 Purdue University, Physics
24 Phase Changes, cont. Phase diagrams show the phase changes a system can experience The line that separates liquid and gas ends at the critical ii point The triple point is where solid, liquid, and gas phase regions all meet For water, this is K This was actually used in the definition of the Kelvin scale Table 14.3 lists the melting and evaporation temperatures of some common substances Lecture 25 Purdue University, Physics
25 Phase Diagram H 2 O Lecture 25 Purdue University, Physics
26 Phase Diagram CO 2 Lecture 25 Purdue University, Physics
27 Ice ILQ Which can absorb more energy from your soda, a cooler filled with water at 0 C, or a cooler filled with ice at 0 C. A) Water B) About Same C) Ice Latent Heat L [J/kg] is heat which must be added (or removed) for material to change phase (liquid- gas). 0 o C Substance L f (J/kg) L v (J/kg) water 33.5 x x 10 5 T ice temp rises ice changes to water (melts) Latent Heat water temp rises Q added to water Lecture 25 Purdue University, Physics
28 Exercise During a tough work out, your body sweats (and evaporates) 1 liter of water to keep cool (37 C). How much cold water would you need to drink (at 2 C) to achieve the same thermal cooling? (recall C 22 V = 4.2 J/g for water, L v =2.2x10 3 J/g) A) 0.15 liters B) 1.0 liters C) 15 liters D) 150 liters Q evaporative = L m = 2.2x10 3 kj/kg x 1kg Q c = c m Δt = 4.2kJ/kgK x 35K x m m = x10 3 / 147 = 15kg or 15 liters! Lecture 25 Purdue University, Physics
29 Boiling Point Going from Lafayette to Denver the temperature at which water boils: A) Increases B) Decreases C) Same Lecture 25 Purdue University, Physics
30 Boiling ILQ What happens to the boiling point when beaker is placed in ice-water? A) Increases B) Decreases C) Same Lecture 25 Purdue University, Physics
31 Cooling ILQ What happens to the pressure in the beaker when placed in ice-water? A) Increases B) Decreases C) Same PV = nrt Lecture 25 Purdue University, Physics
32 ILQ What will happen to the water in the container when I pour ice water over the container A) cool down B) Boil C) Both D) Neither Lecture 25 Purdue University, Physics
33 Exercise How much ice (at 0 C) do you need to add to 0.5 liters of a water at 25 C, to cool it down to 10 C? (L = 80 cal/g, c = 1 cal/g C) Q water = mc Δ T = (0.5 kg)(1 cal / gc)(15 C) = (7,500 calories) Q = ml + mc Δ T ice Qice m = L + c Δ T 7,500cal = = 80 cal / g + (1 cal / gc )(10) 83.3 grams Lecture 25 Purdue University, Physics
34 Exercise Ice cube trays are filled with 0.5 kg of water at 20 C and placed into the freezer. e How much energy e must be removed from the water to turn it into ice cubes at -5 C? (L = 80 cal/g, c water = 1 cal/g C, c ice = 0.5 cal/g C) Water going from 20 C to 0 C: Q = mc ΔT 1 water 1 = ( 20) = 10000( cal) Water turning into ice at 0 C: Q2 = ml = = 40000( cal ) Ice going from 0 C to -5 C: Q3 = mciceδt2 = ( 5) = 1250( cal) Q= Q1+ Q2 + Q3 = 51250( cal ) Lecture 25 Purdue University, Physics
35 Summary of Concepts Heat is FLOW of energy Flow of energy may increase temperaturet Specific Heat ΔT = Q / (c m) Monatomic IDEAL Gas C V = 3/2 R Diatomic IDEAL Gas C V = 5/2 R V Latent Heat Heat associated with change in phase Lecture 25 Purdue University, Physics
Physics 101: Lecture 25 Heat
Final Physics 101: Lecture 25 Heat Today s lecture will cover Textbook Chapter 14.1-14.5 Physics 101: Lecture 25, Pg 1 Internal Energy Energy of all molecules including Random motion of individual molecules»
More informationChapter 14 Temperature and Heat
Nicholas J. Giordano www.cengage.com/physics/giordano Chapter 14 Temperature and Heat Thermodynamics Starting a different area of physics called thermodynamics Thermodynamics focuses on energy rather than
More informationPHYSICS 149: Lecture 26
PHYSICS 149: Lecture 26 Chapter 14: Heat 14.1 Internal Energy 14.2 Heat 14.3 Heat Capacity and Specific Heat 14.5 Phase Transitions 14.6 Thermal Conduction 14.7 Thermal Convection 14.8 Thermal Radiation
More informationTemperature and Its Measurement
Temperature and Its Measurement When the physical properties are no longer changing, the objects are said to be in thermal equilibrium. Two or more objects in thermal equilibrium have the same temperature.
More informationPhysics 101: Lecture 26 Kinetic Theory and Heat
Physics 101: Lecture 6 Kinetic Theory and Heat What concepts did you find most difficult, or what would you like to be sure we discuss in lecture? list of eam topics Eam 3: net W-F, covers Lectures 16
More informationThermochemistry. The study of energy changes that occur during chemical reactions and changes in state.
Energy Thermochemistry The study of energy changes that occur during chemical reactions and changes in state. The Nature of Energy Energy - the ability to do work or produce heat Energy is stored in the
More informationA). Yes. B). No. Q15 Is it possible for a solid metal ball to float in mercury?
Q15 Is it possible for a solid metal ball to float in mercury? A). Yes. B). No. The upward force is the weight of liquid displaced and the downward force is the weight of the ball. If the density of the
More informationLecture 25 Thermodynamics, Heat and Temp (cont.)
Lecture 25 Thermodynamics, Heat and Temp (cont.) Heat and temperature Gases & Kinetic theory http://candidchatter.files.wordpress.com/2009/02/hell.jpg Specific Heat Specific Heat: heat capacity per unit
More informationChapter 10 Temperature and Heat
Chapter 10 Temperature and Heat Thermodynamics deals with 1. Temperature. 2. The transfer and transformation of energy. 3. The relationship between macroscopic properties and microscopic dynamics. Temperature
More informationWhat are the states of Matter?
What are the states of Matter? Solid Lowest energy/heat Molecules barely moving Definite, uniform shape Example: ice States of Matter Liquid Medium energy/heat Molecules slowly moving Shape of container
More informationKinetic Theory continued
Chapter 12 Kinetic Theory continued 12.4 Kinetic Theory of Gases The particles are in constant, random motion, colliding with each other and with the walls of the container. Each collision changes the
More informationKinetic Theory continued
Chapter 12 Kinetic Theory continued 12.4 Kinetic Theory of Gases The particles are in constant, random motion, colliding with each other and with the walls of the container. Each collision changes the
More informationHomework - Lecture 11.
Homework - Lecture 11. Name: Topic: Heat Capacity and Specific Heat Type: Numerical 1. Two liquids, A and B, are mixed together, and the resulting temperature is 22 C. If liquid A has mass m and was initially
More information0 o K is called absolute zero. Water Freezes: 273 o K Water Boils: 373 o K
Part I Notes Temperature and Heat The terms at the right all mean the same thing. The heat energy of a substance is the sum of the kinetic and potential energies of all of the atoms and molecules in the
More informationPage 1 SPH3U. Heat. What is Heat? Thermal Physics. Waterloo Collegiate Institute. Some Definitions. Still More Heat
SPH3U Thermal Physics electrons and holes in semiconductors An Introductory ourse in Thermodynamics converting energy into work magnetism thin films and surface chemistry thermal radiation (global warming)
More informationChapter 12. Temperature and Heat. continued
Chapter 12 Temperature and Heat continued 12.3 The Ideal Gas Law THE IDEAL GAS LAW The absolute pressure of an ideal gas is directly proportional to the Kelvin temperature and the number of moles (n) of
More informationChapter 14 Temperature and Heat
Chapter 14 Temperature and Heat To understand temperature and temperature scales. To describe thermal expansion and its applications. To explore and solve problems involving heat, phase changes and calorimetry.
More informationThermal Energy. Practice Quiz Solutions
Thermal Energy Practice Quiz Solutions What is thermal energy? What is thermal energy? Thermal energy is the energy that comes from heat. This heat is generated by the movement of tiny particles within
More informationChapter 2 Heat, Temperature and the First Law of Thermodynamics
Chapter 2 Heat, Temperature and the First Law of Thermodynamics 2.1. Temperature and the Zeroth Law of Thermodynamics 2.2. Thermal Expansion 2.3. Heat and the Absorption of Heat by Solids and Liquids 2.4.
More informationPhysics 111. Lecture 34 (Walker 17.2,17.4-5) Kinetic Theory of Gases Phases of Matter Latent Heat
Physics 111 Lecture 34 (Walker 17.2,17.4-5) Kinetic Theory of Gases Phases of Matter Latent Heat Dec. 7, 2009 Kinetic Theory Pressure is the result of collisions between gas molecules and walls of container.
More informationCHEM What is Energy? Terminology: E = KE + PE. Thermodynamics. Thermodynamics
Thermodynamics 2 Thermodynamics The study of energy changes accompanying physical and chemical processes. From the laws of thermodynamics, one can: 1. Predict the results of chemical reactions 2. Ascertain
More informationChapters 17 &19 Temperature, Thermal Expansion and The Ideal Gas Law
Chapters 17 &19 Temperature, Thermal Expansion and The Ideal Gas Law Units of Chapter 17 & 19 Temperature and the Zeroth Law of Thermodynamics Temperature Scales Thermal Expansion Heat and Mechanical Work
More information2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container?
1. Which gas law states that the volume of a fixed mass of a gas is directly proportional to its Kelvin temperature if the pressure is kept constant? A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac
More informationThermal Properties Of Matter
Thermal Properties Of Matter 3.2.2 Explain why different substances have different specific heat capacities. Heat two same size objects of different materials for the same amount of time they will not
More informationPhysics 1501 Lecture 35
Physics 1501: Lecture 35 Todays Agenda Announcements Homework #11 (Dec. 2) and #12 (Dec. 9): 2 lowest dropped Honors students: see me after the class! Todays topics Chap.16: Temperature and Heat» Latent
More informationZeroth Law of Thermodynamics
Thermal Equilibrium When you two systems are placed in contact with each other there is no net energy transfer between them. Consequently, these two systems would be at the same temperature. Zeroth Law
More informationThermal Equilibrium. Zeroth Law of Thermodynamics 2/4/2019. Temperature
Thermal Equilibrium When you two systems are placed in contact with each other there is no net energy transfer between them. Consequently, these two systems would be at the same temperature. Zeroth Law
More informationChapter 11. Energy in Thermal Processes
Chapter 11 Energy in Thermal Processes Energy Transfer When two objects of different temperatures are placed in thermal contact, the temperature of the warmer decreases and the temperature of the cooler
More informationSPH3U1 Lesson 03 Energy
THERMAL ENERGY AND LATENT HEAT LEARNING GOALS Students will learn: Heat changes the amount of thermal energy in an object Temperature is a measure of the average thermal energy in an object Heat capacity
More informationFor more info visit
Heat:- Heat is the agent which produces in us the sensation of warmth and makes bodies hot. It is form of energy. The part of thermal energy which flows from one body to the other due to temperature difference
More information3.3 Phase Changes 88 A NATURAL APPROACH TO CHEMISTRY. Section 3.3 Phase Changes
Section 3.3 Phase Changes 3.3 Phase Changes Solid, liquid and gas During a phase change, a substance rearranges the order of its particles (atoms or molecules). Examples of phase change include melting
More informationPROGRAM OF PHYSICS. Lecturer: Dr. DO Xuan Hoi Room A
PROGRAM OF PHYSICS Lecturer: Dr. DO Xuan Hoi Room A1. 503 E-mail : dxhoi@hcmiu.edu.vn PHYSICS 2 (FLUID MECHANICS AND THERMAL PHYSICS) 02 credits (30 periods) Chapter 1 Fluid Mechanics Chapter 2 Heat, Temperature
More informationChapter Notes: Temperature, Energy and Thermal Properties of Materials Mr. Kiledjian
Chapter 10-11 Notes: Temperature, Energy and Thermal Properties of Materials Mr. Kiledjian 1) Temperature 2) Expansion of Matter 3) Ideal Gas Law 4) Kinetic Theory of Gases 5) Energy, Heat transfer and
More informationThermodynamics Test Wednesday 12/20
Thermodynamics Test Wednesday 12/20 HEAT AND TEMPERATURE 1 Temperature Temperature: A measure of how hot (or cold) something is Specifically, a measure of the average kinetic energy of the particles in
More informationLecture 23. Specific Heat and Phase Changes
Lecture 23 Specific Heat and Phase Changes Today s Topics: Heat and Temperature Change Specific heat Heat and Phase Change Latent heat Heat and Temperature Change Heat is energy that flows from a higher-temperature
More informationCHAPTER 17 Thermochemistry
CHAPTER 17 Thermochemistry Thermochemistry The study of the heat changes that occur during chemical reactions and physical changes of state. Chemical Change: new substances created during chemical reaction
More informationPhysical Science Chapter 5 Cont2. Temperature & Heat
Physical Science Chapter 5 Cont2 Temperature & Heat What are we going to study? Temperature Heat Specific Heat and Latent Heat Heat Transfer Phases of Matter The Kinetic Theory of Gases Thermodynamics
More informationTemperature and Heat. Two systems of temperature. Temperature conversions. PHY heat - J. Hedberg
Temperature and Heat 1. Two systems of temperature 1. Temperature conversions 2. Real science (one scale to rule them all) 3. Temperature scales 2. Effects of temperature on materials 1. Linear Thermal
More informationChapter 11. Energy in Thermal Processes
Chapter 11 Energy in Thermal Processes Energy Transfer When two objects of different temperatures are placed in thermal contact, the temperature of the warmer decreases and the temperature of the cooler
More informationPhase Change Diagram. Rank Solids, liquids and gases from weakest attractive forces to strongest:
Unit 11 Kinetic molecular theory packet Page 1 of 13 Chemistry Unit 11 Kinetic Theory Unit Quiz: Test Objectives Be able to define pressure and memorize the basic pressure units. Be able to convert to/from:
More informationq = m. C p. T q = heat (Joules) m = mass (g) C p = specific heat (J/g.o C) T = change in temp. ( o C) UNIT 11 - SOLIDS, LIQUIDS, & PHASE CHANGES
HEAT ENERGY NOTES UNIT 11 - SOLIDS, LIQUIDS, & PHASE CHANGES SECTION (A): same temp or change? SECTION (B): same temp or change? temp is called the energy difference at same temp = SECTION (C): same temp
More informationSPECIFIC HEAT CAPACITY AND HEAT OF FUSION
SPECIFIC HEAT CAPACITY AND HEAT OF FUSION Apparatus on each table: Thermometer, metal cube, complete calorimeter, outer calorimeter can (aluminum only), balance, 4 styrofoam cups, graduated container,
More informationDuncan. Q = m. C p. T. Q = heat (Joules) m = mass (g) C p = specific heat capacity (J/g.o C) T = change in temp. ( o C)
HEAT ENERGY NOTES SECTION (A): phase(s) of matter = SECTION (B): phase(s) of matter = energy difference at same temp = temp is called the SECTION (C): phase(s) of matter = SECTION (D): phase(s) of matter
More informationThermal Energy. solid. liquid. gas
Heat (Chapter 10) What is heat? What is the relationship between quantity of heat and temperature? What happens to a body (solid, liquid, gas) when thermal energy is added or removed? Thermal Energy Solid:
More informationI. The Nature of Energy A. Energy
I. The Nature of Energy A. Energy is the ability to do work or produce heat. It exists in 2 forms: 1. Potential energy is energy due to the composition or position of an object. 2. Kinetic energy is energy
More informationExercises Temperature (pages ) 1. Define temperature. 2. Explain how a common liquid thermometer works.
Exercises 21.1 Temperature (pages 407 408) 1. Define temperature. 2. Explain how a common liquid thermometer works. Match each number with the corresponding description. Temperature Description 3. 273
More informationChapter 11. Important to distinguish between them. They are not interchangeable. They mean very different things when used in physics Internal Energy
Chapter 11 Energy in Thermal Processes Energy Transfer When two objects of different temperatures are placed in thermal contact, the temperature of the warmer decreases and the temperature of the cooler
More informationThermal Effects. IGCSE Physics
Thermal Effects IGCSE Physics Starter What is the difference between heat and temperature? What unit is thermal energy measured in? And what does it depend on? In which direction does heat flow? Heat (Thermal
More informationStart Part 2. Tro's "Introductory Chemistry", Chapter 3
Start Part 2 1 Separation of Mixtures Separate mixtures based on different physical properties of the components. Physical change. Different Physical Property Boiling point State of matter (solid/liquid/gas)
More informationCIE Physics IGCSE. Topic 2: Thermal Physics
CIE Physics IGCSE Topic 2: Thermal Physics Summary Notes Simple kinetic molecular model of matter Molecular model Solids Molecules close together in regular pattern Strong intermolecular forces of attraction
More informationChapter 9. Preview. Objectives Defining Temperature. Thermal Equilibrium. Thermal Expansion Measuring Temperature. Section 1 Temperature and
Section 1 Temperature and Thermal Equilibrium Preview Objectives Defining Temperature Thermal Equilibrium Thermal Expansion Measuring Temperature Section 1 Temperature and Thermal Equilibrium Objectives
More informationChapter 18 Heat and the First Law of Thermodynamics
Chapter 18 Heat and the First Law of Thermodynamics Heat is the transfer of energy due to the difference in temperature. The internal energy is the total energy of the object in its centerofmass reference
More informationThermal energy. Thermal energy is the internal energy of a substance. I.e. Thermal energy is the kinetic energy of atoms and molecules.
Thermal energy Thermal energy is the internal energy of a substance. I.e. Thermal energy is the kinetic energy of atoms and molecules. Heat is the transfer of thermal energy between substances. Until the
More informationChemical Thermodynamics
Chemical Thermodynamics 1 Thermodynamics Thermodynamics is a Greek term which means, heat power. Thermodynamics is the study of energy and its transformations. 2 Thermodynamics Thermochemistry how we observe,
More informationName... Class... Date... Specific heat capacity and specific latent heat
Specific heat capacity and specific latent heat Specification references: P3.2.2 Temperature changes in a system and specific heat capacity P3.2.3 Changes of heat and specific latent heat Aims This is
More informationHonors Physics. Notes Nov 16, 20 Heat. Persans 1
Honors Physics Notes Nov 16, 20 Heat Persans 1 Properties of solids Persans 2 Persans 3 Vibrations of atoms in crystalline solids Assuming only nearest neighbor interactions (+Hooke's law) F = C( u! u
More informationTemperature Energy and Heat
CHAPTER 3 Temperature Energy and Heat 3.1 Temperature What is temperature? Why is temperature important in chemistry? How is energy related to temperature? 2 3.1 Temperature Milk fat particles are being
More informationThermal Physics. Temperature (Definition #1): a measure of the average random kinetic energy of all the particles of a system Units: o C, K
Thermal Physics Internal Energy: total potential energy and random kinetic energy of the molecules of a substance Symbol: U Units: J Internal Kinetic Energy: arises from random translational, vibrational,
More informationPhase Changes and Latent Heat
Review Questions Why can a person remove a piece of dry aluminum foil from a hot oven with bare fingers without getting burned, yet will be burned doing so if the foil is wet. Equal quantities of alcohol
More informationPer 5 Activity Solutions: Thermal Energy, the Microscopic Picture
er 5 Activity Solutions: Thermal Energy, the Microscopic icture 5. How Is Temperature Related to Molecular Motion? ) Temperature Your instructor will discuss molecular motion and temperature. a) Watch
More informationTemperature and Thermometers. Temperature is a measure of how hot or cold something is. Most materials expand when heated.
Heat Energy Temperature and Thermometers Temperature is a measure of how hot or cold something is. Most materials expand when heated. Thermometers are instruments designed to measure temperature. In order
More informationPhysics 231. Topic 13: Heat. Alex Brown Dec 1, MSU Physics 231 Fall
Physics 231 Topic 13: Heat Alex Brown Dec 1, 2015 MSU Physics 231 Fall 2015 1 8 th 10 pm correction for 3 rd exam 9 th 10 pm attitude survey (1% for participation) 10 th 10 pm concept test timed (50 min))
More informationCHAPTER 17: THERMOCHEMISTRY. Mrs. Brayfield
CHAPTER 17: THERMOCHEMISTRY Mrs. Brayfield REVIEW What is the law of conservation of energy? It states that energy cannot be created or destroyed So the energy of any process is the same THERMOCHEMISTRY
More informationHigh temperature He is hot
Lecture 9 What is Temperature and Heat? High temperature He is hot Some important definitions * Two objects are in Thermal contact with each other if energy can be exchanged between them. Thermal equilibrium
More informationEnergy in Thermal Processes. Heat and Internal Energy
Energy in Thermal Processes Heat and Internal Energy Internal energy U: associated with the microscopic components of a system: kinetic and potential energies. The larger the number of internal degrees
More informationChemistry Heat Review. Heat: Temperature: Enthalpy: Calorimetry: Activation energy:
Chemistry Heat Review Name Date Vocabulary Heat: Temperature: Enthalpy: Calorimetry: Activation energy: Formulas Heat of phase change Heat for temperature increase Heat of reaction Endothermic/Exothermic
More information, is placed in thermal contact with object B, with mass m, specific heat c B. and initially at temperature T B
4C_PLC http://www.cabrillo.edu/~jmccullough/physics4c/files/4c_plc/4c_plc.htm Page 1 of 8 /6/201 1. The heat capacity at constant volume and the heat capacity at constant pressure have different values
More informationCHEMISTRY 109 #25 - REVIEW
CHEMISTRY 109 Help Sheet #25 - REVIEW Chapter 4 (Part I); Sections 4.1-4.6; Ch. 9, Section 9.4a-9.4c (pg 387) ** Review the appropriate topics for your lecture section ** Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc
More informationthe energy of motion!
What are the molecules of matter doing all the time?! Heat and Temperature! Notes! All matter is composed of continually jiggling atoms or molecules! The jiggling is! If something is vibrating, what kind
More informationChapter 5. Thermochemistry
Chapter 5 Thermochemistry Energy Thermodynamics Study of the relationship between heat, work, and other forms of energy Thermochemistry A branch of thermodynamics Focuses on the study of heat given off
More informationENERGY. Unit 12: IPC
ENERGY Unit 12: IPC WHAT IS ENERGY? Energy- is the ability to do work. Energy is the ability to cause a change. Energy can change an object s: motion shape temperature color THERMAL internal motion of
More informationHeat gained by soda = Heat lost by watermelon Qsoda = Qwatermelon
PHYS1114 SAMPLE EXAM 5 SOLUTIONS Spring 2013 Professor Kenny L. Tapp 1. Dermatologists often remove small precancerous skin lesions by freezing them quickly with liquid nitrogen, which has a temperature
More informationEDULABZ INTERNATIONAL. Heat ASSIGNMENT
Heat ASSIGNMENT 1. Fill in the blank spaces by choosing the correct words from the list given below : List : substance, thermal capacity, mass, latent, heat, cold, constant, water, J C 1, fusion, hot.
More informationChapter 12. Temperature and Heat
Chapter 12 Temperature and Heat 12.1 Common Temperature Scales Temperatures are reported in degrees Celsius or degrees Fahrenheit. Kelvin Scale 100 o C or 212 o F T K = T + 273.15 Temperature changes,
More information3. When the external pressure is kpa torr, water will boil at what temperature? a C b C c. 100 C d. 18 C
Chemistry EOC Review 5: Physical Behavior of Matter 1. Which gas is monatomic at STP? a. chlorine b. fluorine c. neon d. nitrogen 2. What Kelvin temperature is equal to 25 C? a. 248 K b. 298 K c. 100 K
More informationChapter 12 Solutions. Q Reason: We ll use Equation Q = McΔT and solve for M. We are given. In each case we want to solve for.
Chapter 12 Solutions Q12.12. Reason: Assume the gas is an ideal gas, and use the ideal gas law pv = nrt. Since the number of moles doesn t change and R is a constant, then Equation 12.14 gives In each
More informationAnswer: The relation between kelvin scale and Celsius scale is TK =TC => TC=TK
Question The triple points of neon and carbon dioxide are 24.57 K and 216.55 K respectively. Express these temperatures on the Celsius and Fahrenheit scales. Answer: The relation between kelvin scale and
More informationHence. The second law describes the direction of energy transfer in spontaneous processes
* Heat and Work The first law of thermodynamics states that: Although energy has many forms, the total quantity of energy is constant. When energy disappears in one form, it appears simultaneously in other
More informationAP PHYSICS 2 WHS-CH-14 Heat Show all your work, equations used, and box in your answers! 1 108kg
AP PHYSICS 2 WHS-CH-4 Heat Show all your work, equations used, and box in your answers! James Prescott Joule (88 889) James Prescott Joule studied the nature of heat, and discovered its relationship to
More informationHeat CHAPTER BIOMEDICAL APPLICATIONS
College Physics, Fourth Edition 51 Heat CHAPTER 14 The weather forecast predicts a late spring hard freeze one night; the temperature is to fall several degrees below 0 C and the apple crop is in danger
More informationLecture 5. > Specific Heat. > Calorimetry. (Source: Cutnell, Giancoli, Tippens) Villacorta--DLSUM-SCIENVP-L Term01
Lecture 5 > Specific Heat > Calorimetry (Source: Cutnell, Giancoli, Tippens) 1 Heat > An increase in a body's temperature is related to the increase in the kinetic energy of the molecules composing the
More information* Defining Temperature * Temperature is proportional to the kinetic energy of atoms and molecules. * Temperature * Internal energy
* Defining Temperature * We associate temperature with how hot or cold an object feels. * Our sense of touch serves as a qualitative indicator of temperature. * Energy must be either added or removed from
More informationEntropy & the Second Law of Thermodynamics
PHYS102 Previous Exam Problems CHAPTER 20 Entropy & the Second Law of Thermodynamics Entropy gases Entropy solids & liquids Heat engines Refrigerators Second law of thermodynamics 1. The efficiency of
More informationPhysics 1301, Exam 4 Review
c V Andersen, 2006 1 Physics 1301, Exam 4 Review The following is a list of things you should definitely know for the exam, however, the list is not exhaustive. You are responsible for all the material
More informationIGCSE Double Award Extended Coordinated Science
IGCSE Double Award Extended Coordinated Science Physics 5 - Thermal Properties of Matter Thermal Expansion You need to know thermal expansions for solids, liquids, and gases, and their applications. Thermal
More informationChapter 5 Energy and States of Matter. Changes of State. Melting and Freezing. Calculations Using Heat of Fusion
Chapter 5 Energy and States of Matter Changes of State 5.6 Melting and Freezing 5.7 Boiling and Condensation 1 2 Melting and Freezing A substance is melting while it changes from a solid to a liquid. A
More information6. (6) Show all the steps of how to convert 50.0 F into its equivalent on the Kelvin scale.
General Physics I Quiz 8 - Ch. 13 - Temperature & Kinetic Theory July 30, 2009 Name: Make your work clear to the grader. Show formulas used. Give correct units and significant figures. Partial credit is
More informationQuestion 11.1: The triple points of neon and carbon dioxide are 24.57 K and 216.55 K respectively. Express these temperatures on the Celsius and Fahrenheit scales. Kelvin and Celsius scales are related
More informationCHAPTER 17 WORK, HEAT, & FIRST LAW OF THERMODYNAMICS
CHAPTER 17 WORK, HEAT, and the FIRST LAW OF THERMODYNAMICS In this chapter, we will examine various thermal properties of matter, as well as several mechanisms by which energy can be transferred to and
More informationCh. 11 States of matter
Ch. 11 States of matter States of Matter Solid Definite volume Definite shape Liquid Definite volume Indefinite shape (conforms to container) Gas Indefinite volume (fills any container) Indefinite shape
More informationKinetic Theory of Matter
1 Temperature and Thermal Energy Kinetic Theory of Matter The motion of the particles in matter is described by kinetic theory of matter. Matter is composed of particles that are atoms, molecules, or ions
More informationRecap. There are 3 different temperature scales: Celsius, Kelvin, and Fahrenheit
Recap Temperature, T, is related to the average kinetic energy of each atom/molecule the given material consists of: The ideal gas law relates pressure to density and temperature: There are 3 different
More informationWe call the characteristic of a system that determines how much its temperature will change heat capacity.
3/3 Measuring Heat If all we do is add heat to a system its temperature will rise. How much the temperature rises depends on the system. We call the characteristic of a system that determines how much
More informationThermodynamics Heat Capacity Phase Changes
Thermodynamics Heat Capacity Phase Changes Lana Sheridan De Anza College April 24, 2018 Last time finish applying the ideal gas equation thermal energy introduced heat capacity Overview heat capacity phase
More informationUnit 6. Unit Vocabulary: Distinguish between the three phases of matter by identifying their different
*STUDENT* Unit Objectives: Absolute Zero Avogadro s Law Normal Boiling Point Compound Cooling Curve Deposition Energy Element Evaporation Heat Heat of Fusion Heat of Vaporization Unit 6 Unit Vocabulary:
More informationChapter 14: Liquids and Solids
I. Phases of matter and phase changes a. Recall the three main phases of matter: Chapter 14: Liquids and Solids Energy is involved during the transition from one phase of matter to another. You should
More informationLiquids & Solids: Section 12.3
Liquids & Solids: Section 12.3 MAIN IDEA: The particles in and have a range of motion and are not easily. Why is it more difficult to pour syrup that is stored in the refrigerator than in the cabinet?
More informationName Date Class THE NATURE OF GASES
13.1 THE NATURE OF GASES Section Review Objectives Describe the assumptions of the kinetic theory as it applies to gases Interpret gas pressure in terms of kinetic theory Define the relationship between
More informationTypes of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy
Unit 7: Energy Outline Types of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy Energy Energy is the ability to do work or produce heat. The energy
More informationTells us the average translational kinetic energy of the particles
Temperature and Heat What is temperature? Kinetic Energy What is heat? Thermal Expansion Specific Heat Latent Heat and phase changes Unit 03, Slide 1 Temperature Tells us the average translational kinetic
More information