AR STANDARDS for ch. 10-11 (see ch.11 for more) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 States of Matter Table of Contents Section 1 The Kinetic-Molecular Theory of Matter Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter Objectives • State the kinetic-molecular theory of matter, and describe how it explains certain properties of matter. • List theoffive assumptions of terms the kinetic-molecular theory gases. Define the ideal gas and real gas. • Describe each of theexpansion, following density, characteristic properties of gases: compressibility, diffusion, and effusion. fluidity, • Describe the conditions under which a real gas deviates from “ideal” behavior. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 10.1 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. Slide of 29 4 © Copyright Pearson Prentice Hall End Show 10.1 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. Slide of 29 5 © Copyright Pearson Prentice Hall End Show Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter • 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 10.1 The Nature of Gases > Kinetic Theory and a Model for Gases Kinetic Theory and a Model for Gases What are the assumptions of the kinetic theory as it applies to gases? Slide of 29 7 © Copyright Pearson Prentice Hall End Show 10.1 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. Slide of 29 8 © Copyright Pearson Prentice Hall End Show Section 1 The Kinetic-Molecular Theory of Matter Chapter 10 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 volume occupied by lower a gasdensity is empty space which is the the reason that gases have than liquids and solids and are easily compressed. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter The Kinetic-Molecular Theory of Gases, continued • Collisions between gas particles and between particles and container walls are elastic collisions. • An is one in which there is no net losselastic of totalcollision kinetic energy. • Gas particles are in continuous, rapid, random motion. They therefore possess kinetic energy, which is energy of motion. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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: 1 KE m2 2 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Visual Concepts Kinetic Molecular Theory Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/stu Visual Concept dent/ch10/sec01/vc00/hc610_01_v00fs.ht m Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 10.1 The Nature of Gases > Kinetic Theory and a Model for Gases Properties of Gases Particles in a gas are in rapid, constant motion. Slide of 29 14 © Copyright Pearson Prentice Hall End Show 10.1 The Nature of Gases > Kinetic Theory and a Model for Gases Properties of Gases Gas particles travel in straight-line paths. Slide of 29 15 © Copyright Pearson Prentice Hall End Show 10.1 The Nature of Gases > Kinetic Theory and a Model for Gases Properties of Gases The gas fills the container. Slide of 29 16 © Copyright Pearson Prentice Hall End Show Chapter 10 Visual Concepts Additional Properties of Gases - watch visual Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x Visual Concept /student/ch10/sec01/vc03/hc610_01_v 03fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Visual Concepts Chapter 10 Fluid QuickTime™ and a Sorenson Video 3 decompressor are needed to see this picture. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Visual Concepts Comparing Diffusion and Effusion Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/st Visual Concept udent/ch10/sec01/vc05/hc610_01_v05fs. htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 10 Section 1 The Kinetic-Molecular Theory of Matter 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 gasto is the a gas that does not behave completely according assumptions of the kinetic-molecular theory. • At very hightopressures anda low temperatures, a gas is most likely behave like nonideal gas. • The polar molecules a gas the moremore the gas willthe deviate from of ideal gasare, behavior. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 10.1 The Nature of Gases > Gas Pressure Gas Pressure How does kinetic theory explain gas pressure? Slide of 29 26 © Copyright Pearson Prentice Hall End Show 10.1 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. Slide of 29 27 © Copyright Pearson Prentice Hall End Show 10.1 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. Slide of 29 28 © Copyright Pearson Prentice Hall End Show 10.1 The Nature of Gases > Gas Pressure A barometer is a device that is used to measure atmospheric pressure. Slide of 29 29 © Copyright Pearson Prentice Hall End Show 10.1 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. Slide of 29 30 © Copyright Pearson Prentice Hall End Show SAMPLE PROBLEM 13.1 Slide of 29 © Copyright Pearson Prentice Hall End Show SAMPLE PROBLEM 13.1 Slide of 29 © Copyright Pearson Prentice Hall End Show SAMPLE PROBLEM 13.1 Slide of 29 © Copyright Pearson Prentice Hall End Show SAMPLE PROBLEM 13.1 Slide of 29 © Copyright Pearson Prentice Hall End Show Practice Problems for Sample Problem 13.1 Problem Solving 13.1 Solve Problem 1 with the help of an interactive guided tutorial. Slide of 29 © Copyright Pearson Prentice Hall End Show 10.1 The Nature of Gases > Kinetic Energy and Temperature Kinetic Energy and Temperature What is the relationship between the temperature in kelvins and the average kinetic energy of particles? Slide of 29 36 © Copyright Pearson Prentice Hall End Show 10.1 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. Slide of 29 37 © Copyright Pearson Prentice Hall End Show 10.1 The Nature of Gases > Kinetic Energy and Temperature Slide of 29 38 © Copyright Pearson Prentice Hall End Show 10.1 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. Slide of 29 39 © Copyright Pearson Prentice Hall End Show 10.1 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 energy10.1 of the particles of the substance. Slide of 29 40 © Copyright Pearson Prentice Hall End Show 10.1 The Nature of Gases > Kinetic Energy and Temperature In this vacuum chamber, scientists cooled sodium vapor to nearly absolute zero. Slide of 29 41 © Copyright Pearson Prentice Hall End Show The Nature of Gases > Kinetic Energy and Temperature Animation 14 Observe particles in motion and discover the connection between temperature and kinetic energy. Slide of 29 42 © Copyright Pearson Prentice Hall End Show 10.1 Section Quiz. Assess students’ understanding of the concepts in Section 10.1. Continue to: -or- Launch: Section Quiz Slide of 29 © Copyright Pearson Prentice Hall 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. Slide of 29 © Copyright Pearson Prentice Hall 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. Slide of 29 © Copyright Pearson Prentice Hall 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. Slide of 29 © Copyright Pearson Prentice Hall 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. Slide of 25 © Copyright Pearson Prentice Hall 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 Slide of 28 © Copyright Pearson Prentice Hall End Show End of Chapter 10.1 Show Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.