1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu AR STANDARDS for ch. 10-11 (see ch.11 for more)

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 10 States of Matter Section 1 The Kinetic-Molecular Theory of Matter

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives State the kinetic-molecular theory of matter, and describe how it explains certain properties of matter. List the five assumptions of the kinetic-molecular theory of gases. Define the terms ideal gas and real gas. Describe each of the following characteristic properties of gases: expansion, density, fluidity, compressibility, diffusion, and effusion. Describe the conditions under which a real gas deviates from “ideal” behavior. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

4. End Show © Copyright Pearson Prentice Hall 4 Slide of 29 The Nature of Gases The skunk releases its spray! Within seconds you smell that all-too-familiar foul odor. You will discover some general characteristics of gases that help explain how odors travel through the air, even on a windless day. 10.1

5. End Show Slide of 29 © Copyright Pearson Prentice Hall 5 > The Nature of Gases Kinetic Theory and a Model for Gases The word kinetic refers to motion. The energy an object has because of its motion is called kinetic energy. According to the kinetic theory, all matter consists of tiny particles that are in constant motion. 10.1

6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The kinetic-molecular theory is based on the idea that particles of matter are always in motion. The theory can be used to explain the properties of solids, liquids, and gases in terms of the energy of particles and the forces that act between them. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

7. End Show © Copyright Pearson Prentice Hall 7 The Nature of Gases > Slide of 29 Kinetic Theory and a Model for Gases What are the assumptions of the kinetic theory as it applies to gases? 10.1

8. End Show Slide of 29 © Copyright Pearson Prentice Hall 8 > The Nature of Gases Kinetic Theory and a Model for Gases According to kinetic theory: The particles in a gas are considered to be small, hard spheres with an insignificant volume. The motion of the particles in a gas is rapid, constant, and random. All collisions between particles in a gas are perfectly elastic. 10.1

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory of Gases An ideal gas is a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory. The kinetic-molecular theory of gases is based on the following five assumptions: Gases consist of large numbers of tiny particles that are far apart relative to their size. Most of the volume occupied by a gas is empty space which is the reason that gases have lower density than liquids and solids and are easily compressed. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory of Gases, continued Collisions between gas particles and between particles and container walls are elastic collisions. An elastic collision is one in which there is no net loss of total kinetic energy. Gas particles are in continuous, rapid, random motion. They therefore possess kinetic energy, which is energy of motion. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory of Gases, continued There are no forces of attraction between gas particles. 4.The temperature of a gas depends on the average kinetic energy of the particles of the gas. The kinetic energy of any moving object is given by the following equation: Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory of Gases, continued All gases at the same temperature have the same average kinetic energy. At the same temperature, lighter gas particles, have higher average speeds than do heavier gas particles. Hydrogen molecules will have a higher speed than oxygen molecules. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Click below to watch the Visual Concept. Visual Concept Kinetic Molecular Theory Chapter 10 http://my.hrw.com/sh/hc6_003036809x/stu dent/ch10/sec01/vc00/hc610_01_v00fs.ht m

14. End Show Slide of 29 © Copyright Pearson Prentice Hall 14 > The Nature of Gases Kinetic Theory and a Model for Gases Particles in a gas are in rapid, constant motion. 10.1 Properties of Gases

15. End Show Slide of 29 © Copyright Pearson Prentice Hall 15 > The Nature of Gases Kinetic Theory and a Model for Gases Gas particles travel in straight-line paths. 10.1 Properties of Gases

16. End Show Slide of 29 © Copyright Pearson Prentice Hall 16 > The Nature of Gases Kinetic Theory and a Model for Gases The gas fills the container. 10.1 Properties of Gases

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Click below to watch the Visual Concept. Visual Concept Additional Properties of Gases - watch visual Chapter 10 http://my.hrw.com/sh/hc6_003036809x /student/ch10/sec01/vc03/hc610_01_v 03fs.htm

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory and the Nature of Gases The kinetic-molecular theory applies only to ideal gases. Many gases behave nearly ideally if pressure is not very high and temperature is not very low. Expansion Gases do not have a definite shape or a definite volume. They completely fill any container in which they are enclosed. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory and the Nature of Gases, continued Expansion, continued Gas particles move rapidly in all directions (assumption 3) without significant attraction between them (assumption 4). Fluidity Because the attractive forces between gas particles are insignificant (assumption 4), gas particles glide easily past one another. Because liquids and gases flow, they are both referred to as fluids. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Fluid Chapter 10

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory and the Nature of Gases, continued Low Density The density of a gaseous substance at atmospheric pressure is about 1/1000 the density of the same substance in the liquid or solid state. The reason is that the particles are so much farther apart in the gaseous state (assumption 1). Compressibility During compression, the gas particles, which are initially very far apart (assumption 1), are crowded closer together. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory and the Nature of Gases, continued Diffusion and Effusion Gases spread out and mix with one another, even without being stirred. The random and continuous motion of the gas molecules (assumption 3) carries them throughout the available space. Such spontaneous mixing of the particles of two substances caused by their random motion is called diffusion. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Kinetic-Molecular Theory and the Nature of Gases, continued Diffusion and Effusion, continued Effusion is a process by which gas particles pass through a tiny opening. The rates of effusion of different gases are directly proportional to the velocities of their particles. Molecules of low mass effuse faster than molecules of high mass. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Click below to watch the Visual Concept. Visual Concept Comparing Diffusion and Effusion Chapter 10 http://my.hrw.com/sh/hc6_003036809x/st udent/ch10/sec01/vc05/hc610_01_v05fs. htm

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Deviations of Real Gases from Ideal Behavior Because particles of gases occupy space and exert attractive forces on each other, all real gases deviate to some degree from ideal gas behavior. A real gas is a gas that does not behave completely according to the assumptions of the kinetic-molecular theory. At very high pressures and low temperatures, a gas is most likely to behave like a non−ideal gas. The more polar the molecules of a gas are, the more the gas will deviate from ideal gas behavior. Section 1 The Kinetic-Molecular Theory of Matter Chapter 10

26. End Show © Copyright Pearson Prentice Hall 26 The Nature of Gases > Slide of 29 Gas Pressure How does kinetic theory explain gas pressure? 10.1

27. End Show Slide of 29 © Copyright Pearson Prentice Hall 27 > The Nature of Gases Gas Pressure Gas pressure results from the force exerted by a gas per unit surface area of an object. An empty space with no particles and no pressure is called a vacuum. Atmospheric pressure results from the collisions of atoms and molecules in air with objects. 10.1

28. End Show © Copyright Pearson Prentice Hall 28 Slide of 29 > The Nature of Gases Gas Pressure Gas pressure is the result of simultaneous collisions of billions of rapidly moving particles in a gas with an object. 10.1

29. End Show Slide of 29 © Copyright Pearson Prentice Hall 29 > The Nature of Gases Gas Pressure A barometer is a device that is used to measure atmospheric pressure. 10.1

30. End Show Slide of 29 © Copyright Pearson Prentice Hall 30 > The Nature of Gases Gas Pressure The SI unit of pressure is the pascal (Pa). One standard atmosphere (atm) is the pressure required to support 760 mm of mercury in a mercury barometer at 25°C. 10.1

31. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide of 29 End Show 13.1

32. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide of 29 End Show 13.1

33. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide of 29 End Show 13.1

34. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide of 29 End Show 13.1

35. © Copyright Pearson Prentice Hall Slide of 29 End Show Practice Problems for Sample Problem 13.1 Problem Solving 13.1 Solve Problem 1 with the help of an interactive guided tutorial.

36. End Show © Copyright Pearson Prentice Hall 36 The Nature of Gases > Slide of 29 Kinetic Energy and Temperature What is the relationship between the temperature in kelvins and the average kinetic energy of particles? 10.1

37. End Show Slide of 29 © Copyright Pearson Prentice Hall 37 > The Nature of Gases Kinetic Energy and Temperature Average Kinetic Energy The particles in any collection of atoms or molecules at a given temperature have a wide range of kinetic energies. Most of the particles have kinetic energies somewhere in the middle of this range. 10.1

38. End Show Slide of 29 © Copyright Pearson Prentice Hall 38 > The Nature of Gases Kinetic Energy and Temperature 10.1

39. End Show Slide of 29 © Copyright Pearson Prentice Hall 39 > The Nature of Gases Kinetic Energy and Temperature Absolute zero (0 K, or –273.15°C) is the temperature at which the motion of particles theoretically ceases. Particles would have no kinetic energy at absolute zero. Absolute zero has never been produced in the laboratory. 10.1

40. End Show Slide of 29 © Copyright Pearson Prentice Hall 40 > The Nature of Gases Kinetic Energy and Temperature Average Kinetic Energy and Kelvin Temperature The Kelvin temperature of a substance is directly proportional to the average kinetic energy of the particles of the substance. 10.1

41. End Show Slide of 29 © Copyright Pearson Prentice Hall 41 > The Nature of Gases Kinetic Energy and Temperature In this vacuum chamber, scientists cooled sodium vapor to nearly absolute zero. 10.1

42. End Show © Copyright Pearson Prentice Hall 42 The Nature of Gases > Slide of 29 Kinetic Energy and Temperature Animation 14 Observe particles in motion and discover the connection between temperature and kinetic energy.

43. End Show © Copyright Pearson Prentice Hall Slide of 29 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 10.1 Section Quiz. 10.1.

44. © Copyright Pearson Prentice Hall Slide of 29 End Show 10.1 Section Quiz. 1.According to the kinetic theory, the particles in a gas a.are attracted to each other. b.are in constant random motion. c.have the same kinetic energy. d.have a significant volume.

45. © Copyright Pearson Prentice Hall Slide of 29 End Show 10.1 Section Quiz. 2.The pressure a gas exerts on another object is caused by a.the physical size of the gas particles. b.collisions between gas particles and the object. c.collisions between gas particles. d.the chemical composition of the gas.

46. © Copyright Pearson Prentice Hall Slide of 29 End Show 10.1 Section Quiz. 3.The average kinetic energy of the particles in a substance is directly proportional to the a.Fahrenheit temperature. b.Kelvin temperature. c.molar mass of the substance. d.Celsius temperature.

47. © Copyright Pearson Prentice Hall Slide of 25 End Show Online Self-Check Quiz Complete the online Quiz and record answers. Ask if you have any questions about your answers. click here for online Quiz 10.1 (8 questions) You must be in the “Play mode” for the slideshow for hyperlink to work.

48. © Copyright Pearson Prentice Hall Slide of 28 End Show VIDEOS FOR ADDITIONAL INSTRUCTION Additional Videos for Chapter 10: States of Matter Section 10.1: Kinetic Theory of Matter Gases Ideal Gas Law Three States of Matter

49. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu End of Chapter 10.1 Show