Ch 18. Kinetic Theory of Gases
|
|
|
- Arnold Daniel
- 5 years ago
- Views:
Transcription
1 Physics 5D: Heat, Thermo, Kinetics Ch 18. Kinetic Theory of Gases Prof. Joel Primack 318 ISB Text Copyright Text 2009 Pearson Text Education, Text Inc. Neuschwanstein Bavaria
2 Physics 5D: Heat, Thermo, Kinetics Homework 2 and the slides from this Lecture 2 are posted at The solutions to Homework 1 will be posted after this lecture. Prof. Joel Primack 318 ISB joel@physics.ucsc.edu Text Copyright Text 2009 Pearson Text Education, Text Inc. Neuschwanstein Castle, Bavaria
3 Real Gases and Changes of Phase A PT diagram is called a phase diagram; it shows all three phases of matter. The solidliquid transition is melting or freezing; the liquid-vapor one is boiling or condensing; and the solid-vapor one is sublimation. Water Phase Diagram The Triple point is the only point where all three phases can coexist in equilibrium.
4 Real Gases and Changes of Phase The Triple point is the only point where all three phases can coexist in equilibrium. Water Phase Diagram
5 Assumptions of kinetic theory: large number of molecules, moving in random directions with a variety of speeds molecules are far apart, on average molecules obey laws of classical mechanics and interact only when colliding collisions are perfectly elastic 18-1 The Ideal Gas Law and the Molecular Interpretation of Temperature
6 A superball is thrown straight at a wall and bounces straight back. The magnitude of the momentum transferred to the wall is A. equal to the original momentum of the superball. B. twice the original momentum of the superball. C. zero. D. none of the above.
7 A superball is thrown straight at a wall and bounces straight back. The magnitude of the momentum transferred to the wall is A. equal to the original momentum of the superball. B. twice the original momentum of the superball. C. zero. D. none of the above. The superball s change in momentum is 2p, so the wall s must be -2p by momentum conservation: 2p - 2p = 0.
8 18-1 The Ideal Gas Law and the Molecular Interpretation of Temperature Pressure P = Force/Area = NkT/V. The force exerted on the wall by the collisions of one molecule is Then the force due to all N molecules colliding with that wall is Daniel Bernoulli ( )
9 18-1 The Ideal Gas Law and the Molecular Interpretation of Temperature The averages of the squares of the speeds in all three directions are equal: vx 2 = vy 2 = vz 2 = v 2 /3, where v 2 = vx 2 + vy 2 + vz 2. Therefore implies that So the pressure P F/A is Rewriting,.
10 18-1 The Ideal Gas Law and the Molecular Interpretation of Temperature We just showed that but the Ideal Gas Law says PV = NkT, so The average translational kinetic energy K of the molecules in an ideal gas is directly proportional to the temperature of the gas.
11 Suppose the speed of every molecule in a gas were tripled. What would happen to the Kelvin temperature of the gas? A. It would triple. B. It would go up by 3 1/2. C. It would go up by a factor of 9.
12 Suppose the speed of every molecule in a gas were tripled. What would happen to the Kelvin temperature of the gas? A. It would triple. B. It would go up by 3 1/2. C. It would go up by a factor of 9.
13 18-1 The Ideal Gas Law and the Molecular Interpretation of Temperature We can now calculate the root mean square speed of molecules in a gas as a function of temperature: since
14 The air in this room is a mixture of mostly nitrogen and oxygen molecules. Which of the following statements is true? A. The average speeds of the nitrogen and oxygen molecules are equal. B. The average magnitudes of momentum of the nitrogen and oxygen molecules are equal. C. The average kinetic energies of the nitrogen and oxygen molecules are equal.
15 The air in this room is a mixture of mostly nitrogen and oxygen molecules. Which of the following statements is true? A. The average speeds of the nitrogen and oxygen molecules are equal. B. The average magnitudes of momentum of the nitrogen and oxygen molecules are equal. C. The average kinetic energies of the nitrogen and oxygen molecules are equal.
16 Example 18-2: Speeds of air molecules. What is the rms speed of air molecules (O 2 and N 2 ) at room temperature (20 C)? A. Oxygen: 480 m/s. Nitrogen: 510 m/s B. Nitrogen: 480 m/s. Oxygen: 510 m/s C. Oxygen: 500 m/s. Nitrogen: 500 m/s.
17 Example 18-2: Speeds of air molecules. What is the rms speed of air molecules (O 2 and N 2 ) at room temperature (20 C)? A. Oxygen: 480 m/s. Nitrogen: 510 m/s B. Nitrogen: 480 m/s. Oxygen: 510 m/s C. Oxygen: 500 m/s. Nitrogen: 500 m/s.
18 Conceptual Example 18-3: Less gas in the tank. A tank of helium is used to fill some balloons. As each balloon is filled, the number of helium atoms remaining in the tank decreases. How does this affect the rms speed of molecules remaining in the tank? A. Increases. B. Decreases. C. Stays the same.
19 Conceptual Example 18-3: Less gas in the tank. A tank of helium is used to fill some balloons. As each balloon is filled, the number of helium atoms remaining in the tank decreases. How does this affect the rms speed of molecules remaining in the tank? A. Increases. B. Decreases. C. Stays the same. (assuming the temperature of the tank stays the same)
20 18-2 Distribution of Molecular Speeds The molecules in a gas will not all have the same speed; their distribution of speeds is called the Maxwell distribution: vp = most probable speed = mode - v = average speed - vrms = (v 2 ) 1/2 = root-mean-square speed
21 18-2 Distribution of Molecular Speeds The Maxwell distribution depends only on the absolute (Kelvin) temperature. This figure shows distributions for two different temperatures; at the higher temperature, the whole curve is shifted to the right.
22 18-3 Real Gases and Changes of Phase The isotherm curves here represent the behavior of the gas at different temperatures. The cooler it gets, the further the gas is from ideal. Ideal Gas Higher T In curve D, the gas becomes liquid; it begins condensing at (b) and is entirely liquid at (a). The point (c) is called the critical point. Below the critical temperature TC, the gas can liquefy if the pressure is sufficient; above it, no amount of pressure will suffice.
23 18-3 Real Gases and Changes of Phase A PT diagram is called a phase diagram; it shows all three phases of matter. The PV diagram below shows the liquid and vapor phases at different temperatures. H2O Phase Diagram Ideal Gas Higher T
24 18-3 Real Gases and Changes of Phase Below the critical temperature, the gas can liquefy if the pressure is sufficient; above it, no amount of pressure will suffice.
25 18-3 Real Gases and Changes of Phase A PT diagram is called a phase diagram; it shows all three phases of matter. The solidliquid transition is melting or freezing; the liquid-vapor one is boiling or condensing; and the solid-vapor one is sublimation. H2O Phase Diagram CO2 Phase Diagram
26 The triple point is the only point where all three phases can coexist in equilibrium. Below the critical temperature TC, the gas can liquefy if the pressure is sufficient; above it, no amount of pressure will suffice. H2O Phase Diagram CO2 Phase Diagram
27 18-4 Vapor Pressure and Humidity An open container of water can evaporate, rather than boil, away. The fastest molecules are escaping from the water s surface, so evaporation is a cooling process as well. The inverse process is called condensation. When the evaporation and condensation processes are in equilibrium, the vapor just above the liquid is said to be saturated, and its pressure is the saturated vapor pressure.
28 18-4 Vapor Pressure and Humidity The saturated vapor pressure increases with temperature. Boiling point on summit of Mt. Everest Boiling point in airplane Boiling point at sea level
29 18-4 Vapor Pressure and Humidity A liquid boils when its saturated vapor pressure equals the external pressure.
30 18-4 Vapor Pressure and Humidity Partial pressure is the pressure each component of a mixture of gases would exert if it were the only gas present. The partial pressure of water in the air can be as low as zero, and as high as the saturated vapor pressure at that temperature. Relative humidity is a measure of the saturation of the air.
31 18-4 Vapor Pressure and Humidity When the humidity is high, it feels muggy; it is hard for any more water to evaporate. The dew point is the temperature at which the air would be saturated with water. Neuschwanstein Castle Bavaria, Germany If the temperature goes below the dew point, dew, fog, or even rain may occur.
32 18-5 Van der Waals Equation of State To get a more realistic model of a gas, we include the finite size of the molecules and the range of the intermolecular force beyond the size of the molecule.
33 18-5 Van der Waals Equation of State We assume that some fraction b of the volume per mole is unavailable due to the finite size of the molecules. We also expect that the pressure will be reduced by a factor proportional to the square of the density, due to interactions between the molecules. This gives the Van der Waals equation of state; the constants a and b are found experimentally for each gas:
34 18-5 Van der Waals Equation of State The PV diagram for a Van der Waals gas fits most experimental data quite well. Johannes Diderik van der Waals ( , Nobel Prize 1910)
Lecture PowerPoints. Chapter 13 Physics: Principles with Applications, 7 th edition Giancoli
Lecture PowerPoints Chapter 13 Physics: Principles with Applications, 7 th edition Giancoli This work is protected by United States copyright laws and is provided solely for the use of instructors in teaching
Atomic Mass and Atomic Mass Number. Moles and Molar Mass. Moles and Molar Mass
Atomic Mass and Atomic Mass Number The mass of an atom is determined primarily by its most massive constituents: protons and neutrons in its nucleus. The sum of the number of protons and neutrons is called
Lecture 24. Ideal Gas Law and Kinetic Theory
Lecture 4 Ideal Gas Law and Kinetic Theory Today s Topics: Ideal Gas Law Kinetic Theory of Gases Phase equilibria and phase diagrams Ideal Gas Law An ideal gas is an idealized model for real gases that
Lecture 24. Ideal Gas Law and Kinetic Theory
Lecture 4 Ideal Gas Law and Kinetic Theory Today s Topics: Ideal Gas Law Kinetic Theory of Gases Phase equilibria and phase diagrams Ideal Gas Law An ideal gas is an idealized model for real gases that
17-6 The Gas Laws and Absolute Temperature
17-6 The Gas Laws and Absolute Temperature The relationship between the volume, pressure, temperature, and mass of a gas is called an equation of state. We will deal here with gases that are not too dense.
Chemistry Joke. Once you ve seen 6.02 x You ve seen a mole!
States of Matter Chemistry Joke Once you ve seen 6.02 x 10 23 atoms You ve seen a mole! Kinetic Theory Kinetic Theory explains the states of matter based on the concept that the particles in all forms
Lecture Outline Chapter 17. Physics, 4 th Edition James S. Walker. Copyright 2010 Pearson Education, Inc.
Lecture Outline Chapter 17 Physics, 4 th Edition James S. Walker Chapter 17 Phases and Phase Changes Ideal Gases Kinetic Theory Units of Chapter 17 Solids and Elastic Deformation Phase Equilibrium and
Physics 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.
Matter & Energy. Objectives: properties and structures of the different states of matter.
Matter & Energy Objectives: 1. Use the kinetic theory to describe the properties and structures of the different states of matter. 2. Describe energy transfers involved in changes of state. 3. Describe
Chemistry A: States of Matter Packet Name: Hour: Page!1. Chemistry A States of Matter Packet
Chemistry A: States of Matter Packet Name: Hour: Page!1 Chemistry A States of Matter Packet Chemistry A: States of Matter Packet Name: Hour: Page!2 Worksheet #1: States of Matter In this packet we will
KINETIC THEORY OF GASES
LECTURE 8 KINETIC THEORY OF GASES Text Sections 0.4, 0.5, 0.6, 0.7 Sample Problems 0.4 Suggested Questions Suggested Problems Summary None 45P, 55P Molecular model for pressure Root mean square (RMS) speed
Name Date Class STATES OF MATTER. SECTION 13.1 THE NATURE OF GASES (pages )
Name Date Class 13 STATES OF MATTER SECTION 13.1 THE NATURE OF GASES (pages 385 389) This section introduces the kinetic theory and describes how it applies to gases. It defines gas pressure and explains
Chemistry B11 Chapter 6 Gases, Liquids, and Solids
Chapter 6 Gases, Liquids, and Solids States of matter: the physical state of matter depends on a balance between the kinetic energy of particles, which tends to keep them apart, and the attractive forces
Gases, Liquids and Solids
Chapter 5 Gases, Liquids and Solids The States of Matter Gases Pressure Forces between one molecule and another are called intermolecular forces. Intermolecular forces hold molecules together and kinetic
CHAPTER 13. States of Matter. Kinetic = motion. Polar vs. Nonpolar. Gases. Hon Chem 13.notebook
CHAPTER 13 States of Matter States that the tiny particles in all forms of matter are in constant motion. Kinetic = motion A gas is composed of particles, usually molecules or atoms, with negligible volume
Name 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
States of Matter. Solids Liquids Gases
States of Matter Solids Liquids Gases 1 Solid vs. Liquid vs. Gas Depends on only two things: What? Attractions Kinetic between particles vs Energy of particles 2 Intermolecular Forces (Molecular Attractions)
Name Date Class STATES OF MATTER. SECTION 13.1 THE NATURE OF GASES (pages )
Name Date Class 13 STATES OF MATTER SECTION 13.1 THE NATURE OF GASES (pages 385 389) This section introduces the kinetic theory and describes how it applies to gases. It defines gas pressure and explains
1 Energy is supplied to a fixed mass of gas in a container and the absolute temperature of the gas doubles.
1 Energy is supplied to a fixed mass of gas in a container and the absolute temperature of the gas doubles. The mean square speed of the gas molecules A remains constant. B increases by a factor of 2.
States of Matter. Solids Liquids Gases
States of Matter Solids Liquids Gases 1 Solid vs. Liquid vs. Gas Depends on only two things: What? Attractions Kinetic between particles vs Energy of particles 2 Intermolecular Forces (Molecular Attractions)
Thermal 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,
Gases and IMFs Unit Exam Review Guide
Gases and IMFs Unit Exam Review Guide The following review guide does not necessarily contain all topics that will appear on the test. Make sure to review all notes and concepts from this unit. This review
Name Date Class STATES OF MATTER. Match the correct state of matter with each description of water by writing a letter on each line.
10 STATES OF MATTER SECTION 10.1 THE NATURE OF GASES (pages 267 272) This section describes how the kinetic theory applies to gases. It defines gas pressure and explains how temperature is related to the
Name. Objective 1: Describe, at the molecular level, the difference between a gas, liquid, and solid phase.
Unit 6 Notepack States of Matter Name Unit 4 Objectives 1. Describe, at the molecular level, the difference between a gas, liquid, and solid phase. (CH 10) 2. Describe states of matter using the kinetic
Properties of Gases. 5 important gas properties:
Gases Chapter 12 Properties of Gases 5 important gas properties: 1) Gases have an indefinite shape 2) Gases have low densities 3) Gases can compress 4) Gases can expand 5) Gases mix completely with other
Chapter 10 States of Matter
Chapter 10 States of Matter 1 Section 10.1 The Nature of Gases Objectives: Describe the assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define
The OTHER TWO states of matter
` The OTHER TWO states of matter LIQUIDS A decrease in the average kinetic energy of gas particles causes the temperature to decrease. As it cools, the particles tend to move more slowly if they slow down
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 11 The Gaseous State by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 11 1 Properties of Gases
Chapter 13 - States of Matter. Section 13.1 The nature of Gases
Chapter 13 - States of Matter Section 13.1 The nature of Gases Kinetic energy and gases Kinetic energy: the energy an object has because of its motion Kinetic theory: all matter is made if particles in
Matter changes phase when energy is added or removed
Section 12.4 Phase Changes Explain how the addition and removal of energy can cause a phase change. Interpret a phase diagram. Matter changes phase when energy is added or removed Energy Changes Accompanying
STATES OF MATTER. The Four States of Ma/er. Four States. Solid Liquid Gas Plasma
STATES OF MATTER The Four States of Ma/er Solid Liquid Gas Plasma Four States STATES OF MATTER Ø What makes a substance a par:cular state of ma
OUTLINE. States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry
UNIT 6 GASES OUTLINE States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry STATES OF MATTER Remember that all matter exists in three physical states: Solid Liquid
Unit 8 Kinetic Theory of Gases. Chapter 13-14
Unit 8 Kinetic Theory of Gases Chapter 13-14 This tutorial is designed to help students understand scientific measurements. Objectives for this unit appear on the next slide. Each objective is linked to
Gases, Liquids, Solids, and Intermolecular Forces
Chapter 6 Gases, Liquids, Solids, and Intermolecular Forces Solids: The particles of a solid have fixed positions and exhibit motions of vibration. Liquids: The particles of a liquid are free to move within
Unit 08 Review: The KMT and Gas Laws
Unit 08 Review: The KMT and Gas Laws It may be helpful to view the animation showing heating curve and changes of state: http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/031_changesstate.mov
Temperature Thermal Expansion Ideal Gas Law Kinetic Theory Heat Heat Transfer Phase Changes Specific Heat Calorimetry Heat Engines
Temperature Thermal Expansion Ideal Gas Law Kinetic Theory Heat Heat Transfer Phase Changes Specific Heat Calorimetry Heat Engines Zeroeth Law Two systems individually in thermal equilibrium with a third
Pure Substance Properties and Equation of State
Pure Substance Properties and Equation of State Pure Substance Content Pure Substance A substance that has a fixed chemical composition throughout is called a pure substance. Water, nitrogen, helium, and
Name Date Class STATES OF MATTER
13 STATES OF MATTER Chapter Test A A. Matching Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line. Column A Column B 1. amorphous
Chapter 3 PROPERTIES OF PURE SUBSTANCES
Thermodynamics: An Engineering Approach Seventh Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2011 Chapter 3 PROPERTIES OF PURE SUBSTANCES Copyright The McGraw-Hill Companies, Inc. Permission
Temperature 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.
A).5 atm B) 1 atm C) 1.5 atm D) 2 atm E) it is impossible to tell
1. ne atmosphere is equivalent to A) 1.00 g ml 1 B) 22,400 ml ) 273 K D) 760. mmhg E) 298 K 2. A cylinder contains 2.50 L of air at a pressure of 5.00 atmospheres. At what volume, will the air exert a
Module 5: Rise and Fall of the Clockwork Universe. You should be able to demonstrate and show your understanding of:
OCR B Physics H557 Module 5: Rise and Fall of the Clockwork Universe You should be able to demonstrate and show your understanding of: 5.2: Matter Particle model: A gas consists of many very small, rapidly
Chemistry A: States of Matter Packet Name: Hour: Page 1. Chemistry A States of Matter Packet
Chemistry A: States of Matter Packet Name: Hour: Page 1 Chemistry A States of Matter Packet Chemistry A: States of Matter Packet Name: Hour: Page 2 Worksheet #1: States of Matter In this packet we will
Chapter 11. Liquids and Intermolecular Forces
Chapter 11 Liquids and Intermolecular Forces States of Matter The three states of matter are 1) Solid Definite shape Definite volume 2) Liquid Indefinite shape Definite volume 3) Gas Indefinite shape Indefinite
Thermodynamics. Atoms are in constant motion, which increases with temperature.
Thermodynamics SOME DEFINITIONS: THERMO related to heat DYNAMICS the study of motion SYSTEM an object or set of objects ENVIRONMENT the rest of the universe MICROSCOPIC at an atomic or molecular level
Liquids. properties & structure
Liquids properties & structure Energetics of Vaporization when the high energy molecules are lost from the liquid, it lowers the average kinetic energy if energy is not drawn back into the liquid, its
First Law of Thermodynamics
First Law of Thermodynamics Remember: ΔE univ = 0 Total energy of the universe is constant. Energy can be transferred: ΔE = q + w q = heat w = work (F*D) = ΔPV 1 st Law, review For constant volume process:
CHEM 116 Phase Changes and Phase Diagrams
CHEM 116 Phase Changes and Phase Diagrams Lecture 4 Prof. Sevian Please turn in extra credit assignments at the very beginning of class. Today s agenda Finish chapter 10 Partial pressures Vapor pressure
Chapter 3 PROPERTIES OF PURE SUBSTANCES
Thermodynamics: An Engineering Approach Seventh Edition in SI Units Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2011 Chapter 3 PROPERTIES OF PURE SUBSTANCES Copyright The McGraw-Hill Companies, Inc.
Conceptual Chemistry
Conceptual Chemistry Objective 1 Describe, at the molecular level, the difference between a gas, liquid, and solid phase. Solids Definite shape Definite volume Particles are vibrating and packed close
STATES OF MATTER STATES OF MATTER. The Four States of Matter 3/5/2015. Solid. Liquid Commonly found on Gas Earth Plasma
Unit 10: States of Matter Lesson 10.1: States and Their Changes (Review) STATES OF MATTER The Four States of Matter Solid } Liquid Commonly found on Gas Earth Plasma STATES OF MATTER Based upon particle
STATES OF MATTER STATES OF MATTER. The Four States of Matter 3/5/2015
The Four States of Matter Unit 10: States of Matter Lesson 10.1: States and Their Changes (Review) Solid } Liquid Commonly found on Gas Earth Plasma Based upon particle arrangement Based upon energy of
Chapter 3 PROPERTIES OF PURE SUBSTANCES SUMMARY
Chapter 3 PROPERTIES OF PURE SUBSTANCES SUMMARY PURE SUBSTANCE Pure substance: A substance that has a fixed chemical composition throughout. Compressed liquid (sub-cooled liquid): A substance that it is
Ch10.4 Attractive Forces
Ch10.4 Attractive Forces Intermolecular Forces are the forces holding molecules to each other. Solids have strong forces Gases (vapor) have weak forces Intermolecular forces determine the phase of matter.
Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. a. The gas
Kinetic Molecular Theory, Weak Interactions, States of Matter (Why do liquids & solids exist?)
Kinetic Molecular Theory, Weak Interactions, States of Matter (Why do liquids & solids exist?) Themes for the day: 1. What is the Kinetic Molecular Theory? 2. ow do #1 & weak interactions help us with
Warning!! Chapter 5 Gases. Chapter Objectives. Chapter Objectives. Chapter Objectives. Air Pollution
Warning!! Larry Brown Tom Holme www.cengage.com/chemistry/brown Chapter 5 Gases These slides contains visual aids for learning BUT they are NOT the actual lecture notes! Failure to attend to lectures most
Phase Diagrams. Department of Mechanical Engineering Indian Institute of Technology Kanpur Kanpur India
Phase Diagrams 1 Increasing the temperature isobarically T-v diagram of constant-pressure phase-change processes of a pure substance at various pressures numerical values are for water. 2 Temperature -
0. Matter can exist in different states A. The state depends on the (and ). Of interest to living things.
Kinetic Molecular Theory, Weak Interactions, States of Matter (Why do liquids & solids exist?) http://chemwiki.ucdavis.edu/wikitexts/sacramento_ity_ollege/s%3a_hem_309/hapters ead chapters 5.6 (Intermolecular
There are three phases of matter: Solid, liquid and gas
FLUIDS: Gases and Liquids Chapter 4 of text There are three phases of matter: Solid, liquid and gas Solids: Have form, constituents ( atoms and molecules) are in fixed positions (though they can vibrate
CHAPTER III: Kinetic Theory of Gases [5%]
![CHAPTER III: Kinetic Theory of Gases [5%]](/thumbs/83/88327276.jpg "CHAPTER III: Kinetic Theory of Gases [5%]")
CHAPTER III: Kinetic Theory of Gases [5%] Introduction The kinetic theory of gases (also known as kinetic-molecular theory) is a law that explains the behavior of a hypothetical ideal gas. According to
The Kinetic Theory of Gases
PHYS102 Previous Exam Problems CHAPTER 19 The Kinetic Theory of Gases Ideal gas RMS speed Internal energy Isothermal process Isobaric process Isochoric process Adiabatic process General process 1. Figure
Temperature, Thermal Expansion and the Gas Laws
Temperature, Thermal Expansion and the Gas Laws z x Physics 053 Lecture Notes Temperature,Thermal Expansion and the Gas Laws Temperature and Thermometers Thermal Equilibrium Thermal Expansion The Ideal
CHEMISTRY. Chapter 11 Intermolecular Forces Liquids and Solids
CHEMISTRY The Central Science 8 th Edition Chapter 11 Liquids and Solids Kozet YAPSAKLI States of Matter difference between states of matter is the distance between particles. In the solid and liquid states
States of Matter Chapter 10 Assignment & Problem Set
States of Matter Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. States of Matter 2 Study Guide: Things You Must Know Vocabulary (know the definition
Chapter 1. The Properties of Gases Fall Semester Physical Chemistry 1 (CHM2201)
Chapter 1. The Properties of Gases 2011 Fall Semester Physical Chemistry 1 (CHM2201) Contents The Perfect Gas 1.1 The states of gases 1.2 The gas laws Real Gases 1.3 Molecular interactions 1.4 The van
Physics 231 Topic 12: Temperature, Thermal Expansion, and Ideal Gases Alex Brown Nov
Physics 231 Topic 12: Temperature, Thermal Expansion, and Ideal Gases Alex Brown Nov 18-23 2015 MSU Physics 231 Fall 2015 1 homework 3 rd midterm final Thursday 8-10 pm makeup Friday final 9-11 am MSU
Solids (cont.) Describe the movement of particles in a solid and the forces between them.
Solids A solid is matter that has a definite shape and a definite volume. The attractive forces between the particles in a solid are strong and pull them close together. Solids (cont.) Describe the movement
Chapter 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
Understanding KMT using Gas Properties and States of Matter
Understanding KMT using Gas Properties and States of Matter Learning Goals: Students will be able to describe matter in terms of particle motion. The description should include Diagrams to support the
Phy 231 Sp 02 Homework #10 Page 1 of 4
Phy 231 Sp 02 Homework #10 Page 1 of 4 10-1A) What temperature gives the same reading in both the C and F scales? (a) 0 (b) 100 (c) -40 (d) 20 (e) None of these. 10-2A) A comfortable room temperature is
Ch Kinetic Theory. 1.All matter is made of atoms and molecules that act like tiny particles.
Ch. 15.1 Kinetic Theory 1.All matter is made of atoms and molecules that act like tiny particles. Kinetic Theory 2.These tiny particles are always in motion. The higher the temperature, the faster the
The Kinetic-Molecular Theory of Gases
The Kinetic-Molecular Theory of Gases kinetic-molecular theory of gases Originated with Ludwig Boltzman and James Clerk Maxwell in the 19th century Explains gas behavior on the basis of the motion of individual
Chapter 5 The Gaseous State
Chapter 5 The Gaseous State Contents and Concepts Gas Laws We will investigate the quantitative relationships that describe the behavior of gases. 1. Gas Pressure and Its Measurement 2. Empirical Gas Laws
Chapter 10. Thermal Physics
Chapter 10 Thermal Physics Thermal Physics Thermal physics is the study of Temperature Heat How these affect matter Thermal Physics, cont Descriptions require definitions of temperature, heat and internal
PROPERTIES OF PURE SUBSTANCES. Chapter 3. Mehmet Kanoglu. Thermodynamics: An Engineering Approach, 6 th Edition. Yunus A. Cengel, Michael A.
Thermodynamics: An Engineering Approach, 6 th Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2008 Chapter 3 PROPERTIES OF PURE SUBSTANCES Mehmet Kanoglu Copyright The McGraw-Hill Companies, Inc.
Hood River Valley High
Chemistry Hood River Valley High Name: Period: Unit 7 States of Matter and the Behavior of Gases Unit Goals- As you work through this unit, you should be able to: 1. Describe, at the molecular level, the
17-1 Ideal Gases. Gases are the easiest state of matter to describe - All ideal gases exhibit similar behavior.
17-1 Ideal Gases Gases are the easiest state of matter to describe - All ideal gases exhibit similar behavior. An ideal gas is one that is thin enough, that the interactions between molecules can be ignored.
Name: Class: Date: Figure 3-1
Name: Class: Date: Chapter 3 test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A gas has a. a definite volume but no definite shape. b. a definite shape
Unit 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:
Chemistry States of Matter Lesson 9 Lesson Plan David V. Fansler
Chemistry States of Matter Lesson 9 Lesson Plan David V. Fansler States of Matter The Nature of Gases Objectives: Describe the motion of gas particles according to the kinetic theory; Interpret gas pressure
Chapter 14 9/21/15. Solids, Liquids & Gasses. Essential Questions! Kinetic Theory! Gas State! Gas State!
Chapter 14 Solids, Liquids & Gasses Essential Questions What is the kinetic theory of matter? How do particles move in the different states of matter? How do particles behave at the boiling and melting
First Law of Thermodynamics Second Law of Thermodynamics Mechanical Equivalent of Heat Zeroth Law of Thermodynamics Thermal Expansion of Solids
Slide 1 / 66 1 What is the name of the following statement: "When two systems are in thermal equilibrium with a third system, then they are in thermal equilibrium with each other"? A B C D E First Law
1 Points to Remember Subject: Chemistry Class: XI Chapter: States of matter Top concepts 1. Intermolecular forces are the forces of attraction and repulsion between interacting particles (atoms and molecules).
FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY MIDTERM 1. Examiners: Prof. B. Siwick Prof. I. Butler Dr. A.
FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY MIDTERM 1 Examiners: Prof. B. Siwick Prof. I. Butler Dr. A. Fenster Name: INSTRUCTIONS 1. Enter your student number and name on the
Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces Pearson Education, Inc.
Lecture Presentation Chapter 11 Liquids and States of Matter The fundamental difference between states of matter is the strength of the intermolecular forces of attraction. Stronger forces bring molecules
q = 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
A) 2.0 atm B) 2.2 atm C) 2.4 atm D) 2.9 atm E) 3.3 atm
Name: Date: 1. On a cold day ( 3 C), the gauge pressure on a tire reads 2.0 atm. If the tire is heated to 27 C, what will be the absolute pressure of the air inside the tire? A) 2.0 atm B) 2.2 atm C) 2.4
10/15/2015. Why study gases? An understanding of real world phenomena. An understanding of how science works.
0/5/05 Kinetic Theory and the Behavior of Ideal & Real Gases Why study gases? An understanding of real world phenomena. An understanding of how science works. 0/5/05 A Gas fills any container. completely
Chapter 3 PROPERTIES OF PURE SUBSTANCES
Chapter 3 PROPERTIES OF PURE SUBSTANCES PURE SUBSTANCE Pure substance: A substance that has a fixed chemical composition throughout. Air is a mixture of several gases, but it is considered to be a pure
CHEMISTRY Matter and Change. Chapter 12: States of Matter
CHEMISTRY Matter and Change Chapter 12: States of Matter CHAPTER 12 States of Matter Section 12.1 Section 12.2 Section 12.3 Section 12.4 Gases Forces of Attraction Liquids and Solids Phase Changes Click
Chapter 15: Thermal Properties of Matter
Chapter 15 Lecture Chapter 15: Thermal Properties of Matter Goals for Chapter 15 To understand and learn to use the mole and Avogadro's number. To see applications for equations of state. To study the
14.3 Ideal Gases > Chapter 14 The Behavior of Gases Ideal Gases Properties of Gases The Gas Laws Gases: Mixtures and Movements
Chapter 14 The Behavior of Gases 14.1 Properties of Gases 14.2 The Gas Laws 14.3 Ideal Gases 14.4 Gases: Mixtures and Movements 1 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
van der Waals & Wilson
van der Waals & Wilson N.G. Schultheiss translated and adapted by K. Schadenberg 1 Introduction There are various ways to detect and measure particles. This module will discuss two of them, the bubble
Chapter Elements That Exist as Gases at 25 C, 1 atm. 5.2 Pressure basic physics. Gas Properties
5.1 Elements That Exist as Gases at 25 C, 1 atm Chapter 5 The Gaseous State YOU READ AND BE RESPONSIBLE FOR THIS SECTION! Gaseous compounds include CH 4, NO, NO 2, H 2 S, NH 3, HCl, etc. Gas Properties
Chapter 10 Notes: Gases
Chapter 10 Notes: Gases Watch Bozeman Videos & other videos on my website for additional help: Big Idea 2: Gases 10.1 Characteristics of Gases Read p. 398-401. Answer the Study Guide questions 1. Earth
Ch. 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
Gases. Chapter 5. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Gases Chapter 5 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Elements that exist as gases at 25 0 C and 1 atmosphere 2 3 Physical Characteristics of Gases
CHAPTER 1. MEASURES OF ATMOSPHERIC COMPOSITION
1 CHAPTER 1. MEASURES OF ATMOSPHERIC COMPOSITION The objective of atmospheric chemistry is to understand the factors that control the concentrations of chemical species in the atmosphere. In this book
CHAPTER 3 TEST REVIEW
IB PHYSICS Name: Period: Date: # Marks: 52 Raw Score: IB Curve: DEVIL PHYSICS BADDEST CLASS ON CAMPUS CHAPTER 3 TEST REVIEW 1. Water at a temperature of 0 C is kept in a thermally insulated container.