Unit 8 Kinetic Theory of Gases. Chapter 13-14
|
|
- Elfrieda Wright
- 5 years ago
- Views:
Transcription
1 Unit 8 Kinetic Theory of Gases Chapter 13-14
2 This tutorial is designed to help students understand scientific measurements. Objectives for this unit appear on the next slide. Each objective is linked to its description. Select the number at the front of the slide to go directly to its description. Throughout the tutorial, key words will be defined. Select the word to see its definition.
3 Objectives 4 Define kinetic theory of gases including collisions 5 Define pressure, including atmospheric pressure, vapor pressure, pressure differentials, and how a barometer works 6 Describe boiling points, including normal boiling points, using vapor pressure graphs, explaining the difference between boiling and evaporation, and how intermolecular forces and molecular weight determine evaporation rates 7 Define and use data based on the triple point phase diagram 8 Define and know the variables of the Gas Laws, including Boyle s Law, Charles Law, Gay-Lussac s Law, and the combined gas law 9 State Avogadro s Principle 10 Use the ideal gas law to solve problems and know the variables of the ideal gas law 11 State and use Dalton s Law of Partial Pressures 12 State and use Graham s Law of effusion and define diffusion
4 4 The Kinetic Theory Particles at the molecular level have been described previously. It has been stated that these particles are in a constant state of motion and are attracted to each other through intermolecular forces. The kinetic theory as described on the next slide is specific to gases.
5 Kinetic Theory of Gases There are five parts to the kinetic theory of gases. 1. Gases will fill the entire volume allowed. This means that is 10 oxygen molecules are released in a classroom, they will arrange themselves equally throughout that space. If the same 10 were released in a gymnasium, they will do the same.
6 Kinetic Theory of Gases 2. Gases can be compressed. The volume a gas holds can be increased or decreased. 3. The motion of gases is random. Gas molecules will travel in straight lines until they run into an object. 4. Gas molecules have elastic collision. When gas molecules collide, there is no loss in kinetic energy.
7 Kinetic Theory of Gases 5. The kinetic energy of a gas molecule is measured by temperature. As the temperature increases, gas molecules move faster, and as the temperature decreases, gas molecules move slower.
8 Kinetic Theory of Gases A quick recap: 1. Gases fill the entire volume allowed. 2. Gases can be compressed. 3. The motion of a gas is random. 4. Gases have elastic collisions. 5. The kinetic energy of gases is measured with temperature. The link below is for a simulator that demonstrates some of these ideas.
9 5 Pressure Pressure is a measure of force per unit surface area. For instance, assume you are standing. You are exerting a force on the floor. The surface area is the size of both of your feet. If you stand on only one foot, the force would be the same but the surface area is halved so the pressure doubles. When referring to gases, pressure is the measure of the force exerted when two gas particles collide.
10 Air Pressure and Vapor Pressure The molecules that make of the air around you are constantly colliding with each other and the objects in the room (including you). These collisions make up air pressure. Vapor pressure is the pressure exerted by the air on a liquid.
11 Measuring pressure Atmospheric pressure is determined using an instrument known as a barometer. The barometer is filled with mercury because of its density. As atmospheric pressure pushes down on the mercury, it forces the mercury up the column. Atmospheric pressure is measured by the distance the mercury is displaced. Atmospheric Pressure Mercury 760 mm
12 Pressure The barometer was invented by a scientist by the name of Torricelli. Pressure is often given with units of mm Hg but the torr is used as well. To make the numbers easier to work with, atmospheric pressure was set equal to 1 atm (atmosphere)
13 Units of Pressure There are several units for pressure and all are used. Therefore the following values are equal to atmospheric pressure: 1 atm = kpa (kilopascals) 101,325 Pa (Pascals) 760 mm Hg 760 torr
14 6 Temperature vs. Heat The last part of the kinetic theory mentioned temperature. Temperature is often confused with heat but the two are quite different. Temperature is a measure of the average kinetic energy of molecules. Heat is the measure of the total kinetic energy of molecules.
15 Temperature vs. Heat All molecules are in a state of motion. The motion is measured by kinetic energy. However, not all molecules are moving at the same speed and thus do not have the same kinetic energy. The average is taken to determine the speed of the majority of the molecules. The total is determined for a purpose that will be discussed in Unit 9.
16 Temperature The average kinetic energy is reported in three different scales. Fahrenheit Celsius Kelvin ( F) ( C) (K) Each scale is used by certain individuals about the world. The scientific community prefers Celsius or Kelvin.
17 Temperature The Celsius scale was designed to have the boiling point of water be 100 C while the freezing point of water would be 0 C. The Kelvin scale was designed using the same increments as Celsius but instead placed zero at absolute zero.
18 Temperature It is important to be able to convert from one scale to another so the following equations were determined: F = C C=( F 32) x 5 9 K = C
19 Boiling Points Boiling is the process of taking a liquid to the gaseous state. This process occurs by adding heat to the liquid. However, there are additional factors that can affect the boiling point. These include intermolecular forces and vapor pressure.
20 Intermolecular Forces When heat is added to a liquid, the particles in that liquid gain kinetic energy. Gaining kinetic energy means that they are moving faster. It is the intermolecular forces that hold the molecules close together. With enough kinetic energy, a molecule can overcome the intermolecular forces and break free. The stronger the intermolecular force, the more kinetic energy will be required to break free.
21 Boiling versus Evaporation It also depends on where the heat is added as to how easy it will be to overcome the intermolecular force. Both boiling and evaporation are ways to bring a liquid to a gas but each can occur at different temperatures.
22 Evaporation When considering evaporation, the heat comes from a source above the liquid. This means the particles on the top of the liquid gain kinetic energy (shown in red) Once they gain enough energy, they can break free of the intermolecular forces. Heat Notice, it is only the top that increases kinetic energy while the rest of the molecules remain the same. This is why the temperature of the liquid does not have to greatly increase during evaporation.
23 Boiling In comparison to evaporation, boiling adds heat to the bottom of the liquid. Since the bottom particles have to work their way to the top, it is more difficult to overcome the intermolecular forces. In order to overcome the intermolecular forces, all particles will need to gain kinetic energy. Because all particles must gain energy, the temperature increases. This is also why boiling proceeds faster than evaporation.
24 Vapor Pressure The other factor effecting the boiling point is vapor pressure. Vapor pressure is the pressure from the atmosphere above a liquid. The gas particles above a liquid can prevent molecules that have enough energy to break free from the intermolecular forces from becoming a gas. The image on the next slide illustrates this idea.
25 Vapor Pressure Gas Particles The particle escapes but transfers its energy to a gas particle. The particle falls back to the liquid.
26 Vapor Pressure If there were less particles above the liquid, it would be easier to boil. The boiling point at one atmosphere is considered to be the normal boiling point. A vapor pressure diagram can help determine the boiling point.
27 Pressure (atm) Vapor Pressure Diagrams Vapor pressure diagrams show the relationship between vapor pressure and the boiling point. The red line below represents the normal boiling point. Notice, it is easier to boiling if there is a smaller vapor pressure. This liquid would boil at 62 C if the pressure of 0.18 atm. The normal boiling point is 101 C at 1 atm. Vapor Pressure Diagram Temperature (C)
28 Standard Temperature and Pressure (STP) For the purposes of scientific consistency, a select temperature and pressure were selected. This way, all experiments could be repeated at the same atmospheric conditions. STP is 1 atm of pressure and 0 C.
29 7 Triple Point Diagrams The vapor pressure diagram shows a portion of a larger diagram known as the triple point diagram. This diagram represents the three types of matter and their relationships to pressure and temperature. The following slide shows a possible triple point diagram. There are six phase changes that occur as you cross each line form one phase to the next. The triple point is denoted with a blue dot.
30 Pressure (atm) Triple Point Diagram 1.20 Critical Point 1.00 Solid Liquid 0.80 Melting 0.60 Freezing Vaporization 0.40 Condensation Sublimation Deposition Gas Triple Pt Temperature (C)
31 Triple Point Diagrams The triple point indicates a point where all three phases are present at the same time. It only occurs at one temperature and pressure for each substance. The critical point is also marked. The critical point indicates where the kinetic theory does not accurately describe the properties of this chemical.
32 8 Gas Laws Temperature, pressure, and volume have a distinct affect on gases. It was determined that these three variables have distinct relationships. These relationships are known as the gas laws.
33 Pressure (atm) Boyle s Law Boyle s Law describes the relationship between pressure and volume. The relationship is inverse which means as one increases, the Boyle's Law other decreases. 1 The equation for Boyle s Law is: 0.5 P 1 V 1 =P 2 V Volume (L)
34 Volume (L) Charles Law Charles Law describes the relationship between temperature and volume. The relationship is direct which means as one increases, the Charles' Law 14 other increases. 12 The equation for 10 8 Charles Law is: 6 V 1 T 1 =V 2 T Temperature (K)
35 Pressure (atm) Gay-Lussac s Law Gay-Lussac s Law describes the relationship between pressure and temperature. The relationship is direct which means as one increases, the Gay-Lussac's Law 1.4 other increases The equation for 0.8 Gay-Lussac s Law is: 0.6 P 1 T 1 =P 2 T Temperature (K)
36 Gas Laws The three gas laws described require certain units to be used. Volume = liters Temperature = Kelvin Pressure = kpa or atm The three can also be combined.
37 Combined Gas Law As that all three variables can be difficult to hold constant, the three gas laws can be combined to create the combined gas law. P 1 V 1 T 1 = P 2V 2 T 2
38 Gas Law Recap Gas Law Boyle s Charles Gay- Lussac s Combined Equation P 1 V 1 =P 2 V 2 V 1 T 1 = V 2 T 2 P 1 T 1 = P 2 T 2 P 1 V 1 T 1 = P 2V 2 T 2 Relationship Inverse Direct Direct Constant Temperature Pressure Volume Nothing
39 9 Avogadro s Principle Up to this point, we have examined gases under the assumption that we always held the same number of moles in the container. This is not always the case. Just as a relationship was determined between pressure, volume, and temperature, a relationship was determined between the number of moles and volume.
40 Avogadro s Principle According to Avogradro s Principle, if the number of moles increase, the volume also must increase assuming constant temperature and pressure. V 1 n 1 = V 2 n 2 n = moles
41 Avogadro s Principle Using this principle, it was determined that at STP (standard temperature and pressure), one mole of a gas would always take up the same volume. At 0 C and 1 atm, 1 mole will take up 22.4 liters.
42 10 Ideal Gas Law With the inclusion of the mole into the relationships of gases, it could be added to the combined gas law as well. PV T = k V n = k K represents a constant PV nt = k
43 Ideal Gas Law Upon further analysis, it was determined that the constant could be calculated and was the same for each container. Assume STP conditions: 1 Mole 22.4 Liters K 1 atm PV nt = k 1 atm x 22.4 L 1 mole x K = k k = atm x L mole x K
44 Ideal Gas Law The constant was changed to R and requires specific units to be used. There are two commonly used values for atm x L kpa x L R: or mole x K mole x K Required Units: Volume: Liters Amount: moles Temperature: Kelvin Pressure: atm or kpa
45 Ideal Gas Law The equation for the Ideal Gas Law is: PV=nRT The value of R is chosen based on the units on the pressure.
46 11 Dalton s Law of Partial Pressures When gases were discussed in Unit 10, it was mentioned that pressure was measured with the collisions gas particles underwent. The total pressure is a sum of all of those collisions. Therefore, Dalton s Law states that the pressure of each gas can be added to determine the total pressure.
47 Dalton s Law of Partial Pressures Though Dalton s Law seems fairly basic, it is extremely useful when collecting a gas. When most experiments are performed, the gases produced are allowed to escape. However, if it is the gas that needs to be analyzed, the gas most be collected. The collection of this gas is typically done over water.
48 Collecting a Gas over Water Collecting a gas over water requires a sealed container with a tube into a tank of water. In the tank of water, an inverted tube is filled with water. As the reaction progresses, the gas produced follows the tube into the water chamber and up the inverted tube.
49 Dalton s Law Dalton s Law comes into play because a small amount of water with change to a gas in the container. Therefore, the gas collected and water vapor combine to give the pressure. That pressure is equal to the atmospheric pressure outside of the tube. Therefore, the following equation applies: P atmosphere = P gas + P water
50 12 Effusion and Diffusion Graham s Law of Effusion states that at the same temperature, a heavier molecule will move slower than a lighter molecule. Recall that temperature is the average kinetic energy of a molecule. Kinetic energy is calculated by taking the mass times the velocity squared (KE=mv 2 ) The relationship between speed and mass is inverse. Diffusion is the dispersion of molecules from areas of high concentration to areas of low concentration.
51 This concludes the tutorial on measurements. To try some practice problems, click here. To return to the objective page, click here. To exit the tutorial, hit escape.
52 Definitions-Select the word to return to the tutorial Absolute zero the temperature at which molecules no longer move. Intermolecular Forces forces that hold molecules together. These include hydrogen bonding, dipole forces, and London 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
More informationOUTLINE. 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
More informationCentimeters of mercury
CHAPTER 11 PROPERTIES OF GASES Gases have an indefinite shape: a gas takes the shape of its container and fills it uniformly. If the shape of the container changes, so does the shape of the gas. Gases
More informationProperties 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
More informationChemistry 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
More informationINTRODUCTORY 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
More informationCHEMISTRY 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
More informationCh10.4 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.
More informationChemistry 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
More informationGases. Measuring Temperature Fahrenheit ( o F): Exceptions to the Ideal Gas Law. Kinetic Molecular Theory
Ideal gas: a gas in which all collisions between atoms or molecules are perfectly elastic (no energy lost) there are no intermolecular attractive forces Think of an ideal gas as a collection of perfectly
More informationGas Laws. Gas Properties. Gas Properties. Gas Properties Gases and the Kinetic Molecular Theory Pressure Gas Laws
Gas Laws Gas Properties Gases and the Kinetic Molecular Theory Pressure Gas Laws Gas Properties 1) Gases have mass - the density of the gas is very low in comparison to solids and liquids, which make it
More informationHood 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
More informationChapter 11. Preview. Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures
Preview Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures Section 1 Gases and Pressure Lesson Starter Make a list of gases you already know about. Separate your list into elements,
More informationUnit Outline. I. Introduction II. Gas Pressure III. Gas Laws IV. Gas Law Problems V. Kinetic-Molecular Theory of Gases VI.
Unit 10: Gases Unit Outline I. Introduction II. Gas Pressure III. Gas Laws IV. Gas Law Problems V. Kinetic-Molecular Theory of Gases VI. Real Gases I. Opening thoughts Have you ever: Seen a hot air balloon?
More informationChapter 6 The States of Matter. Examples of Physical Properties of Three States of Matter
Chapter 6 The States of Matter Examples of Physical Properties of Three States of Matter 1 Three States of Matter Solids: Fixed shape, fixed volume, particles are held rigidly in place. Liquids: Variable
More informationComparison of Solids, Liquids, and Gases
CHAPTER 8 GASES Comparison of Solids, Liquids, and Gases The density of gases is much less than that of solids or liquids. Densities (g/ml) Solid Liquid Gas H O 0.97 0.998 0.000588 CCl 4.70.59 0.00503
More informationName 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
More informationLecture Presentation. Chapter 10. Gases. James F. Kirby Quinnipiac University Hamden, CT Pearson Education, Inc.
Lecture Presentation Chapter 10 James F. Kirby Quinnipiac University Hamden, CT Characteristics of Physical properties of gases are all similar. Composed mainly of nonmetallic elements with simple formulas
More informationdensity (in g/l) = molar mass in grams / molar volume in liters (i.e., 22.4 L)
Unit 9: The Gas Laws 9.5 1. Write the formula for the density of any gas at STP. Name: KEY Text Questions from Corwin density (in g/l) = molar mass in grams / molar volume in liters (i.e., 22.4 L) Ch.
More informationChapter 10. Gases. The Gas Laws
Page 1 of 12 10.1 Characteristics of Gases. Chapter 10. Gases. All substances have three phases; solid, liquid and gas. Substances that are liquids or solids under ordinary conditions may also exist as
More informationComparison of Solid, Liquid, and Gas
Gas Laws Comparison of Solid, Liquid, and Gas State Shape and Volume Compressibility Ability to Flow Gas Conforms to shape and volume of container Particles can move past one another High Lots of free
More informationGases. Pressure is formally defined as the force exerted on a surface per unit area:
Gases Pressure is formally defined as the force exerted on a surface per unit area: Force is measure in Newtons Area is measured in m 2 and it refers to the Area the particle/object is touching (From the
More informationSCH 3UI Unit 08 Outline: Kinetic Molecular Theory and the Gas Laws. The States of Matter Characteristics of. Solids, Liquids and Gases
SCH 3UI Unit 08 Outline: Kinetic Molecular Theory and the Gas Laws Lesson Topics Covered Handouts to Print 1 Note: The States of Matter solids, liquids and gases state and the polarity of molecules the
More informationCHEMISTRY Matter and Change. Chapter 13: Gases
CHEMISTRY Matter and Change Chapter 13: Gases CHAPTER 13 Table Of Contents Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry Click a hyperlink to view the corresponding
More informationChapter 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
More informationSTATES 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
More informationSTATES 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
More informationThe fundamental difference between. particles.
Gases, Liquids and Solids David A. Katz Department of Chemistry Pima Community College States of Matter The fundamental difference between states t of matter is the distance between particles. States of
More informationAP Chemistry Ch 5 Gases
AP Chemistry Ch 5 Gases Barometer - invented by Evangelista Torricelli in 1643; uses the height of a column of mercury to measure gas pressure (especially atmospheric) Manometer- a device for measuring
More informationChapter 6: The States of Matter
Spencer L. Seager Michael R. Slabaugh www.cengage.com/chemistry/seager Chapter 6: The States of Matter PHYSICAL PROPERTIES OF MATTER All three states of matter have certain properties that help distinguish
More informationChapter 13. Kinetic Theory (Kinetikos- Moving ) Based on the idea that particles of matter are always in motion
Chapter 3 Kinetic Theory (Kinetikos- Moving ) Based on the idea that particles of matter are always in motion The motion has consequences Behavior of Gases Physical Properties of Gases Ideal Gas an imaginary
More informationGases. Section 13.1 The Gas Laws Section 13.2 The Ideal Gas Law Section 13.3 Gas Stoichiometry
Gases Section 13.1 The Gas Laws Section 13.2 The Ideal Gas Law Section 13.3 Gas Stoichiometry Click a hyperlink or folder tab to view the corresponding slides. Exit Section 13.1 The Gas Laws State the
More informationName: Regents Chemistry: Notes: Unit 8 Gases.
Name: Regents Chemistry: Notes: Unit 8 Gases 1 Name: KEY IDEAS The concept of an ideal gas is a model to explain the behavior of gases. A real gas is most like an ideal gas when the real gas is at low
More informationCh 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
More informationThe Gas Laws. Learning about the special behavior of gases
The Gas Laws Learning about the special behavior of gases The States of Matter What are the 3 states of matter that chemists work with? Solids, liquids, and gases We will explain the behavior of gases
More informationLecture Presentation. Chapter 10. Gases. James F. Kirby Quinnipiac University Hamden, CT Pearson Education
Lecture Presentation Chapter 10 2015 Pearson Education James F. Kirby Quinnipiac University Hamden, CT Characteristics of Physical properties of gases are all similar. Composed mainly of nonmetallic elements
More informationUnit 3 - Part 2: Gas Laws. Objective - learn the main gas laws that all molecules follow.
Unit 3 - Part 2: Gas Laws Objective - learn the main gas laws that all molecules follow. Pressure - Pressure = Force / Area Created by collisions of the gas molecules with each other and with surfaces.
More informationChemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10. Gases.
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Characteristics of Unlike liquids and solids, they Expand to fill their containers.
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 informationGases. Characteristics of Gases. Unlike liquids and solids, gases
Gases Characteristics of Gases Unlike liquids and solids, gases expand to fill their containers; are highly compressible; have extremely low densities. 1 Pressure Pressure is the amount of force applied
More informationCHEM. Ch. 12 Notes ~ STATES OF MATTER
CHEM. Ch. 12 Notes ~ STATES OF MATTER NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 12.1 topics States of Matter: SOLID, LIQUID, GAS, PLASMA I. Kinetic Theory
More information13.1 The Nature of Gases (refer to pg )
13.1 The Nature of Gases (refer to pg. 420-424) Essential Understanding any other state of matter. Temperature and pressure affect gases much more than they affect Lesson Summary Kinetic Theory and a Model
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 informationKinetic Molecular Theory and Gas Law Honors Packet. Name: Period: Date: Requirements for honors credit: Read all notes in packet
Kinetic Molecular Theory and Gas Law Honors Packet Name: Period: Date: Requirements for honors credit: Read all notes in packet Watch the 10 Brighstorm videos shown on the right and take Cornell notes
More informationLecture Presentation. Chapter 10. Gases. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 10 John D. Bookstaver St. Charles Community College Cottleville, MO Characteristics of Unlike liquids and solids, gases Expand to fill their containers. Are highly compressible.
More informationName 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
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin
Lecture INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Gases by Christopher G. Hamaker Illinois State University Properties of Gases There are five important
More informationChapter 5. The Properties of Gases. Gases and Their Properties. Why Study Gases? Gas Pressure. some very common elements exist in a gaseous state
Chapter 5 Gases and Their Properties Why Study Gases? some very common elements exist in a gaseous state our gaseous atmosphere provides one means of transferring energy and material throughout the globe
More informationName 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
More informationChapter 10. Chapter 10 Gases
Chapter 10 Gases Earth is surrounded by a layer of gaseous molecules - the atmosphere - extending out to about 50 km. 10.1 Characteristics of Gases Gases low density; compressible volume and shape of container
More informationStates of Matter. The Solid State. Particles are tightly packed, very close together (strong cohesive forces) Low kinetic energy (energy of motion)
States of Matter The Solid State Particles are tightly packed, very close together (strong cohesive forces) Low kinetic energy (energy of motion) Fixed shape and volume Crystalline or amorphous structure
More informationEngr. Yvonne Ligaya F. Musico Chemical Engineering Department
GASEOUS STATE Engr. Yvonne Ligaya F. Musico Chemical Engineering Department TOPICS Objective Properties of Gases Kinetic Molecular Theory of Gases Gas Laws OBJECTIVES Determine how volume, pressure and
More information10/15/2015. 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
More informationBoyle s law states the relationship between the pressure and the volume of a sample of gas.
The Ideal Gas Law Boyle s law states the relationship between the pressure and the volume of a sample of gas. Charles s law states the relationship between the volume and the absolute temperature of a
More informationWhy study gases? A Gas 10/17/2017. An understanding of real world phenomena. An understanding of how science works.
Kinetic Theory and the Behavior of Ideal & Real Gases Why study gases? n understanding of real world phenomena. n understanding of how science works. Gas Uniformly fills any container. Mixes completely
More informationThis should serve a s a study guide as you go on to do the problems in Sapling and take the quizzes and exams.
CHM 111 Chapter 9 Worksheet and Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding
More informationChapter 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
More informationAlthough different gasses may differ widely in their chemical properties, they share many physical properties
IV. Gases (text Chapter 9) A. Overview of Chapter 9 B. Properties of gases 1. Ideal gas law 2. Dalton s law of partial pressures, etc. C. Kinetic Theory 1. Particulate model of gases. 2. Temperature and
More informationChapter 10. Gases. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 John Bookstaver St. Charles Community College Cottleville, MO Characteristics of Unlike
More informationTOPIC 2. Topic 2. States of Matter (I) - Gases. 1
Chemistry TOPIC 2 States of Matter (I) - Gases Topic 2. States of Matter (I) - Gases. 1 Contents 1. Introduction 2. Pressure measurement 3. The Ideal Gas equation 4. Efusion and Diffusion 5. Kinetic Molecular
More informationChemistry Day 5. Friday, August 31 st Tuesday, September 4 th, 2018
Chemistry Day 5 Friday, August 31 st Tuesday, September 4 th, 2018 Do-Now Title: BrainPOP: States of Matter 1. Write down today s FLT 2. List two examples of gases 3. List two examples of things that are
More informationPhase Change DIagram
States of Matter Phase Change DIagram Phase Change Temperature remains during a phase change. Water phase changes Phase Diagram What is a phase diagram? (phase diagram for water) Normal melting point:
More informationClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
Chapter 11 THE NATURE OF GASES States of Matter Describe the motion of gas particles according to the kinetic theory Interpret gas pressure in terms of kinetic theory Key Terms: 1. kinetic energy 2. gas
More informationUNIT 7: The Gas Laws. Mrs. Howland Chemistry 10 Rev. April 2016
UNIT 7: The Gas Laws ì Mrs. Howland Chemistry 10 Rev. April 2016 ì Learners will be able to ì ì ì ì ì ì ì ì ì ì ì ì ì ì ì Unit 7: Gas Laws Describe atmospheric pressure and explain how a barometer works
More informationChapter 3. States of Matter
Chapter 3 States of Matter 1. Solid 2. Liquid 3. Gas States of Matter Two More (discuss later) Plasma Bose-Einstein condensate States of Matter Solid (definite shape and volume) Particles are tightly packed
More information10/16/2018. Why study gases? An understanding of real world phenomena. An understanding of how science works.
10/16/018 Kinetic Theory and the Behavior of Ideal & Real Gases Why study gases? An understanding of real world phenomena. An understanding of how science works. 1 10/16/018 A Gas Uniformly fills any container.
More informationGases Over View. Schweitzer
Gases Over View Schweitzer Collision theory Describing Ideal gases Particles are very far apart relative to their size. Particles are traveling very fast Particles are traveling in straight lines Collisions
More information7/16/2012. Characteristics of Gases. Chapter Five: Pressure is equal to force/unit area. Manometer. Gas Law Variables. Pressure-Volume Relationship
7/6/0 Chapter Five: GASES Characteristics of Gases Uniformly fills any container. Mixes completely with any other gas. Exerts pressure on its surroundings. When subjected to pressure, its volume decreases.
More informationCHAPTER 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
More informationch 12 acad.notebook January 12, 2016 Ch 12 States of Matter (solids, liquids, gases, plasma, Bose Einstein condensate)
Ch 12 States of Matter (solids, liquids, gases, plasma, Bose Einstein condensate) BIG IDEA The kinetic molecular theory explains the different properties of solids, liquids and gases. I CAN: 1) use the
More informationChapter Ten- Gases. STUDY GUIDE AP Chemistry
STUDY GUIDE AP Chemistry Chapter Ten- Gases Lecture Notes 10.1 Characteristics of Gases All substances have three phases: solid, liquid and gas. Substances that are liquids or solids under ordinary conditions
More informationName 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
More informationIMPORTANT CONCEPTS. 5.1 Pressure Units for pressure STP. 5.6 Kinetic Molecular Theory. 5.3 Ideal Gas Law. 5.4 Gas Stoichiometry Gas density Molar mass
TOPICS 1. Intermolecular Forces 2. Properties of Gases 3. Pressure 4. Gas Laws Boyle, Charles, Lussac 5. Ideal Gas Law 6. Gas Stoichiometry 7. Partial Pressure 8. Kinetic Molecular Theory 9. Effusion &
More informationIntroduction Matter has three possible states: - Solid - Liquid - Gas. Chem101 - Lecture 6
Chem101 - Lecture 6 States of Matter Introduction Matter has three possible states: - Solid - Liquid - Gas We will investigate the differences in the physical properties exhibited by each of these states
More informationGases, 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
More informationChapter 10. Gases. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 John Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall, Inc.
More informationChapter 5. The Gas Laws
Chapter 5 The Gas Laws 1 Pressure Force per unit area. Gas molecules fill container. Molecules move around and hit sides. Collisions are the force. Container has the area. Measured with a barometer. 2
More informationImportance of Gases Airbags fill with N gas in an accident. Gas is generated by the decomposition of sodium azide, NaN.
Gas Laws Importance of Gases Airbags fill with N 2 gas in an accident. Gas is generated by the decomposition of sodium azide, NaN 3. 2 NaN 3 (s) 2 Na (s) + 3 N 2 (g) 2 Importance of Gases C 6 H 12 O 6
More informationFig Note the three different types of systems based on the type of boundary between system and surroundings.
CHAPTER 1 LECTURE NOTES System, Surroundings, and States Fig. 1.4 Note the three different types of systems based on the type of boundary between system and surroundings. Intensive and Extensive Properties
More informationUnit 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
More informationGases, Liquids, and Solids. Chapter 5
Gases, Liquids, and Solids Chapter 5 Educational Goals 1. Define, compare, contrast the terms specific heat, heat of fusion, and heat of vaporization. Know the equations that involve these concepts and
More informationLBS 172 Exam 1 Review
Chapter 12- Gases LBS 172 Exam 1 Review I. What is a gas? a. Properties i. Non-definite volume, fills container, can flow, spread out, can be compressed b. Air is a gas composed of many gases i. Relatively
More informationChapter 5 Gases and the Kinetic-Molecular Theory
Chapter 5 Gases and the Kinetic-Molecular Theory Name (Formula) Methane (CH 4 ) Ammonia (NH 3 ) Chlorine (Cl 2 ) Oxygen (O 2 ) Ethylene (C 2 H 4 ) Origin and Use natural deposits; domestic fuel from N
More informationSection Using Gas Laws to Solve Problems
Gases and Gas Laws Section 13.2 Using Gas Laws to Solve Problems Kinetic Molecular Theory Particles of matter are ALWAYS in motion Volume of individual particles is zero. Consists of large number of particles
More informationChapter 10. Lesson Starter. Why did you not smell the odor of the vapor immediately? Explain this event in terms of the motion of molecules.
Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of Gases Deviations of Real Gases from Ideal Behavior Section 1 The Kinetic-Molecular
More informationChapter 11 Gases 1 Copyright McGraw-Hill 2009
Chapter 11 Gases Copyright McGraw-Hill 2009 1 11.1 Properties of Gases The properties of a gas are almost independent of its identity. (Gas molecules behave as if no other molecules are present.) Compressible
More informationChapter 10. Gases THREE STATES OF MATTER. Chapter 10 Problems 6/29/2012. Problems 16, 19, 26, 33, 39,49, 57, 61
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 John Bookstaver St. Charles Community College Cottleville, MO Chapter 10 Problems Problems
More informationIntroductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 13 Gases Properties of
More informationA Gas Uniformly fills any container. Easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings.
Chapter 5 Gases Chapter 5 A Gas Uniformly fills any container. Easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings. Copyright Cengage Learning. All rights reserved
More informationGases. A gas. Difference between gas and vapor: Why Study Gases?
Gases Chapter 5 Gases A gas Uniformly fills any container. Is easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings. Difference between gas and vapor: A gas is a substance
More information(b) The measurement of pressure
(b) The measurement of pressure The pressure of the atmosphere is measured with a barometer. The original version of a barometer was invented by Torricelli, a student of Galileo. The barometer was an inverted
More informationStates of Matter Unit
Learning Target Notes Section 1: Matter and Energy What makes up matter? Matter is made of atoms and molecules that are in constant motion. Kinetic Theory of Matter A. Particles that make up matter are
More informationChapter 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
More informationWhat we will learn about now
Chapter 4: Gases What we will learn about now We will learn how volume, pressure, temperature are related. You probably know much of this qualitatively, but we ll learn it quantitatively as well with the
More informationGases! n Properties! n Kinetic Molecular Theory! n Variables! n The Atmosphere! n Gas Laws!
Gases n Properties n Kinetic Molecular Theory n Variables n The Atmosphere n Gas Laws Properties of a Gas n No definite shape or volume n Gases expand to fill any container n Thus they take the shape of
More informationPart One: The Gas Laws. gases (low density, easy to compress)
CHAPTER FIVE: THE GASEOUS STATE Part One: The Gas Laws A. Introduction. 1. Comparison of three states of matter: fluids (flow freely) solids condensed states liquids (high density, hard to compress) gases
More informationGeneral Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University. Module 3: The Three States of Matter
General Chemistry I Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University Module 3: The Three States of Matter Gas state (Equation of state: ideal gas and real gas). Liquid state
More informationC L A S S I F I C AT I O N O F M AT T E R
UNIT 2: C L A S S I F I C AT I O N O F M AT T E R MATTER Reflect: What is matter? MATTER Matter: Anything that has mass and occupies space. You can describe matter in terms of quantity by mass NOT weight.
More informationGases. 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
More informationChapter 10. Gases. Lecture Outline Characteristics of Gases 1, 10.2 Pressure. Atmospheric Pressure and the Barometer 3, 4, 5, 6,
1 Chapter 10. Lecture Outline 10.1 Characteristics of 1, 2 All substances have three phases: solid, liquid and gas. Substances that are liquids or solids under ordinary conditions may also exist as gases.
More information