CHEMISTRY WKST: Gases Review p. 1
|
|
- Loreen Perry
- 5 years ago
- Views:
Transcription
1 CHEMISTRY WKST: Gases Review p. 1 1) a) b) c) V directly proportional to Kelvin temperature V inversely proportional to pressure V directly proportional to moles 2) Air pressure is caused by the collisions of gas particles against a surface. 3) barometer, manometer 4) Gas particles are so small, compared to the distances between them, the volume of individual particles is assumed to be negligible (zero volume). Gas particles are in constant random motion, colliding with the walls of the container to cause air pressure. The collisions are perfectly elastic. Gas particles are assumed not to attract or to repel each other. The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature of the gas. 5) Gases approach ideal behavior at low pressure and high temperature. 6) The mole ratio of N2:H2 is equal to the volume ratio of the gases. In this case both are 1 N2: 3 H2 7) 22.4 L 8) Average kinetic energy is directly proportional to the Kelvin temperature of the gas sample. 9) a) increases b) increases c) increases d) same e) same 10) a) same b) increases c) increases d) increases e) increases 11) The particles of Xe in the 100 C sample will have more kinetic energy and, therefore, be moving faster than the particles of Xe in the 25 C sample. 12) The He in both samples will be moving at the same speed. Since both samples have the same temperature, both samples will have the same average kinetic energy. Therefore, the particles in both samples will have the same velocity. 13) H g/mol CH g/mol N2O g/mol O g/mol NH g/mol The lighter the gas the faster it moves. N2O3 < O2 < NH3 < CH4 < H2 (slowest) (fastest)
2 CHEMISTRY WKST: Gases Review p. 2 14) An ideal gas is one in which its volume is: directly proportional to its Kelvin temperature directly proportional to its moles inversely proportional to its pressure 15) PHe = 0.75 atm ( ) = 76 kpa 1 atm P O2 = 225 torr ( ) = 30.0 kpa 760 torr P N2 = 12.0 psi ( ) = 82.7 kpa 14.7 psi Ptotal = 76 kpa kpa kpa = 189 kpa 16) Pvap of water at 25 C = torr P1V1 T1 = P2V2 T2 V1 = ml P1 = torr torr = torr T1 = 25 C = 298 K V2 =? P2 = 760 torr T2 = K P1V1T2 = P2V2T1 V2 = P1V1T2 V2= P2T1 (726.2 torr)(250.0 ml)( K) (760 torr)(298 K) V2 = 219 ml 17) V1 = L T1 =? V2 = L T2 = 0 C = 273 K V1 = V2 T1 T2 V1T2 = V2T1 T1 = V1T2 V2 T1 = (2.250 L)(273 K) (4.115 L) = 149 K T1 = 149 K = 124 C 18) Since T goes up 4, V goes up 4. Since P goes up 8, V goes down 8. Therefore, V ends up going down 2.
3 CHEMISTRY WKST: Gases Review p. 3 19) C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g) 5 mol O2 a) 2.25 L C3H8 ( ) = L O2 = 11.2 L O2 1 mol C3H8 1 mol C3H8 4 mol H2O g H2O b) L C3H8 ( ) ( ) ( ) = 1.61 g H2O 22.4 L C3H8 1 mol C3H8 1 mol H2O c) Need molar V at 725 torr and 15 C 725 torr ( 1 atm ) = atm 760 torr PV = nrt V = nrt P L atm (1 mol)( = mol K )(288 K) atm = 24.8 L 1 mol O2 mol CO L CO g O2 ( ) (3 ) ( ) = 34.9 L CO g O2 5 mol O2 1 mol CO2 20) P1 = atm T1 = C = K T2 =? P2 = atm T 1 = P 2 T 2 T 2 = P 2 T 1 T 2 = P 2T 1 T 2 = (1.500 atm)( K) atm = K T2 = K = C = C 21) V1 = ml P1 = kpa V2 =? P2 = kpa P1V1 = P2V2 V2 = P1V1 V2= P2 (92.55 kpa)(22.50 ml) ( kpa) V2 = ml
4 CHEMISTRY WKST: Gases Review p. 4 22) n1 = mol = mmhg ( ) = kpa 760 mmhg P2 = kpa n2 =? Both P s need to be the same unit doesn t matter which. If you made both mmhg, the kpa would become mmhg. Final answer is the same regardless. n 1 = P 2 n 2 n 2 = P 2 n 1 n 2 = P 2n 1 n 2 = (120.3 kpa)(0.750 mol) kpa n2 = mol 23) n1 = mol V1 = ml V2 =? n2 = mol V1 = V2 n1 n2 V1n2 = V2n1 V2 = V1n2 n1 V2= (62.00 ml)(0.500 mol) ( mol) V2 = ml 24) g = 32.0 g NH3 V = 17.4 L T = 41 C = 314 K P =? PV = grt (MM) P = grt V(MM) L atm (32.0 g)( )(314 K) mol K = (17.4 L)(17.04 g ) mol = 2.78 atm 25) g =? SO3 V = ml = L P = 745 torr ( 1 atm ) = atm 760 torr T = 15 C = 258 K PV = grt (MM) g = PV(MM) RT = g (0.980 atm)( L)(80.07 mol ) ( L atm = )(258 K) mol K g 26) rate O2 rate Cl2 MM Cl2 = MM O2 rate O2 rate Cl g/mol Cl2 = g/mol O2 = O2 is times faster than Cl2
5 CHEMISTRY WKST: Gases Review p. 5 27) rate NH3 rate unk = MM unk MM NH3 rate unk rate NH3 MM NH3 = MM unk ml/min ml/min = g/mol NH ml/min ml/min = g/mol NH = g/mol NH g/mol NH = = g = g mol = g/mol = g mol = g mol 28) a) When heated, the gas particles inside the can gain KE and will move faster. This increases the number of collisions against the surface of the can, causing an increase in pressure. Eventually the pressure will become too much for the can to hold, causing the can to eplode. b) When you inhale the air in the straw you are creating a vacuum inside the straw and your mouth. The higher atmospheric pressure pushing on the surface of the liquid in the container will force the liquid up the straw. c) The higher you go into the atmosphere the lower the pressure becomes (so does temperature but not as fast as pressure). Therefore, as the balloon rises and the pressure lowers, the balloon s volume increases. d) As the football cools the gas particles inside the ball loses KE and slows down. This causes fewer collisions against the side of the ball. Thus, the pressure decreases and ball gets soft. e) As more air goes into the tire, the number of collisions against the tire s surface increases. Therefore, the pressure inside the tire increases. f) When the air inside the can is removed there will be less collisions against the can s surface, causing the pressure to decrease. The higher outside pressure will then force the walls of the container to collapse. g) When the container is first closed, gravity pulls out a small amount of water through the hole causing the volume of air inside the container to epand and lower its pressure. Then the higher pressure outside the container will keep the water inside the container since the air inside has less pressure. When the lid is opened, the pressures equalize and water will pour out the hole. h) When the hot soup is put in the freezer the gas particles inside the container lose KE and slow down. This lowers the number of collisions of particles against the surface of the container and thereby lowers the pressure inside the container. When going to open the container you then must overcome the higher atmospheric pressure on the outside of the container. i) A popcorn kernel has a small amount of water inside. As the kernel is heated, the water gets superheated well above its boiling point. This causes etreme pressure inside the kernel as the water molecules begin to move faster with the increased KE. Eventually the pressure gets to the point where the kernel s hull can t contain it any longer and the kernel pops.
6 CHEMISTRY WKST: Gases Review p. 6 j) As the air inside the balloon is heated the gas particles gain KE and move faster. This causes the particles to spread out and increase the volume of the balloon. This in turn decreases the density of the air inside the balloon. The more dense air outside is pulled down by gravity causing the less dense air inside the balloon to rise. 29) Gas particles do have a volume and that space is NOT available to other gas particles as assumed. Gas particles do have attraction forces between them when they get close to each other, causing the particles to slow down a little. This would cause the pressure to be slightly less than epected. 30) The vapor pressure of water increases as temperature increases.
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
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 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. 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 informationthe drink won t rise very high in the straw vacuum straw 1 atm drink
vacuum the drink won t rise very high in the straw straw 1 atm drink vacuum the drink won t rise very high in the straw straw 1 atm drink vacuum the drink won t rise very high in the straw straw 0.007
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 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 informationGases. Chapter 5. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Gases Chapter 5 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Elements that exist as gases at 250C and 1 atmosphere 2 3 Physical Characteristics of Gases
More informationThe Gas Laws-Part I The Gaseous State
The Gas Laws-Part I The Gaseous State The States of Matter The Distinction of Gases from Liquids and Solids 1. Gas volume changes greatly with pressure. 2. Gas volume changes greatly with temperature.
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 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 informationExercises. Pressure. CHAPTER 5 GASES Assigned Problems
For Review 7. a. At constant temperature, the average kinetic energy of the He gas sample will equal the average kinetic energy of the Cl 2 gas sample. In order for the average kinetic energies to be the
More informationGas Density. Standard T & P (STP) 10/29/2011. At STP, 1 mol of any ideal gas occupies 22.4 L. T = 273 K (0 o C) P = 1 atm = kpa = 1.
Standard T & P (STP) T = 73 K (0 o C) P = 1 atm = 101.35 kpa = 1.0135 bar At STP, 1 mol of any ideal gas occupies.4 L.4 L Gas Density We can use PV = nrt to determine the density of gases. What are the
More informationThe Gaseous State of Matter
The Gaseous State of Matter Chapter 12 Hein and Arena Version 1.1 Dr. Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Company The Kinetic- Molecular Theory 2 The Kinetic-Molecular
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 informationChapter 10 Gases Characteristics of Gases Elements that exist as gases: Noble gases, O 2, N 2,H 2, F 2 and Cl 2. (For compounds see table 10.
Chapter 10 Gases 10.1 Characteristics of Gases Elements that exist as gases: Noble gases, O 2, N 2,H 2, F 2 and Cl 2. (For compounds see table 10.1) Unlike liquids and solids, gases expand to fill their
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 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 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 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 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 informationAP CHEM WKST KEY: SOLIDS, LIQUIDS & GASES REVIEW
AP CHEM WKST KEY: SOLIDS, LIQUIDS & GASES REVIEW 1) a) NaCl ionic b) C6H12O6 HB c) PH3 LF d) H2O2 HB e) CH3CH2OH HB f) HI DD g) Kr LF h) diamond covalent 2) a) H2O Want the strongest IMF for highest BP.
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 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 informationPressure. Pressure Units. Molecular Speed and Energy. Molecular Speed and Energy
Pressure is defined as force per unit area. Pressure Pressure is measured with a device called a barometer. A mercury barometer uses the weight of a column of Hg to determine the pressure of gas pushing
More informationB 2, C 2, N 2. O 2, F 2, Ne 2. Energy order of the p 2p and s 2p orbitals changes across the period.
Chapter 11 Gases Energy order of the p p and s p orbitals changes across the period. Due to lower nuclear charge of B, C & N there is no s-p orbitals interaction Due to high nuclear charge of O, F& Ne
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 informationSTP : standard temperature and pressure 0 o C = 273 K kpa
GAS LAWS Pressure can be measured in different units. For our calculations, we need Pressure to be expressed in kpa. 1 atm = 760. mmhg = 101.3 kpa R is the Universal Gas Constant. Take note of the units:
More informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 5 GASES INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 5 GASES 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 5 GASES Properties of Gases Pressure History and Application of the Gas Laws Partial Pressure Stoichiometry 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 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 informationExample Problems: 1.) What is the partial pressure of: Total moles = 13.2 moles 5.0 mol A 7.0 mol B 1.2 mol C Total Pressure = 3.
5.6 Dalton s Law of Partial Pressures Dalton s Law of Partial Pressure; The total pressure of a gas is the sum of all its parts. P total = P 1 + P + P 3 + P n Pressures are directly related to moles: n
More informationChapter 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
More informationStandard T & P (STP) At STP, 1 mol of any ideal gas occupies 22.4 L. The standard temperature and pressure for gases is:
Standard T & P (STP) The standard temperature and pressure for gases is: At STP, 1 mol of any ideal gas occupies 22.4 L T = 273 K (0 o C) P = 1 atm = 101.325 kpa = 1.01325 bar 22.4 L Using STP in problems
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 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, 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 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 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 informationChapter 5. Gases and the Kinetic-Molecular Theory
Chapter 5 Gases and the Kinetic-Molecular Theory Macroscopic vs. Microscopic Representation Kinetic Molecular Theory of Gases 1. Gas molecules are in constant motion in random directions. Collisions among
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 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 informationProperties of Gases. Occupy the entire volume of their container Compressible Flow readily and mix easily Have low densities, low molecular weight
Chapter 5 Gases Properties of Gases Occupy the entire volume of their container Compressible Flow readily and mix easily Have low densities, low molecular weight Atmospheric Pressure Atmospheric pressure
More information4. 1 mole = 22.4 L at STP mole/volume interconversions at STP
Ch. 10 Gases and the Ideal Gas Law(s) Chem 210 Jasperse Ch. 10 Handouts 1 10.1 The Atmosphere 1. Earth surrounded by gas 2. Major components: Nitrogen 78% Oxygen 21% Miscellaneous: All
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 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 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 information1,2,8,9,11,13,14,17,19,20,22,24,26,28,30,33,38,40,43,45,46,51,53,55,57,62,63,80,82,88,94
CHAPTER 5GASES 1,,8,9,11,1,14,17,19,0,,4,6,8,0,,8,40,4,45,46,51,5,55,57,6,6,80,8,88,94 5.1 a) The volume of the liquid remains constant, but the volume of the gas increases to the volume of the larger
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 informationSOLID 1. Make sure your state of matter is set on solid. Write your observations below:
Chemistry Ms. Ye Name Date Block Properties of Matter: Particle Movement Part 1: Follow the instructions below to complete the activity. Click on the link to open the simulation for this activity: http://phet.colorado.edu/sims/states-of-matter/states-of-matterbasics_en.jnlp***note:
More informationGases: Their Properties & Behavior. Chapter 09 Slide 1
9 Gases: Their Properties & Behavior Chapter 09 Slide 1 Gas Pressure 01 Chapter 09 Slide 2 Gas Pressure 02 Units of pressure: atmosphere (atm) Pa (N/m 2, 101,325 Pa = 1 atm) Torr (760 Torr = 1 atm) bar
More informationGases, 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 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 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 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 informationD g << D R < D s. Chapter 10 Gases & Kinetic Molecular Theory. I) Gases, Liquids, Solids Gases Liquids Solids. Particles far apart
Chapter 10 Gases & Kinetic Molecular Theory I) Gases, Liquids, Solids Gases Liquids Solids Particles far apart Particles touching Particles closely packed very compressible slightly comp. Incomp. D g
More informationCHAPTER 5 GASES AND THE KINETIC- MOLECULAR THEORY
CHAPTER 5 GASES AND THE KINETIC- MOLECULAR THEORY FOLLOW UP PROBLEMS 5.1A Plan: Use the equation for gas pressure in an open-end manometer to calculate the pressure of the gas. Use conversion factors to
More informationGases. Which elements exist as gases at ordinary temperature and pressure? Gases: Have simple molecular formulas. Chapter 10 part 1: Ideal Gases
Chapter 10 part 1: Ideal Gases Read: BLB 10.1 5 HW: BLB 10.2,19a,b, 23, 26, 30, 39, 41, 45, 49 Sup 10:1 6 Know: What is pressure? Gases Which elements exist as gases at ordinary temperature and pressure?
More informationThe Gaseous State. Definition
The Gaseous State Lecture Material Basic Chemistry 1 2013/2014 Inneke Hantoro Definition A gas is a substance that is normally in the gaseous state at ordinary temperatures and pressures. A vapor is the
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 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 informationChapter 5: Gases. Definitions: Phases of Matter 10/27/2011
Chapter 5: Gases 5.1 Definitions 5.2 The First Laws 5.3 The Ideal Gas Law 5.4 Stoichiometry and Gases 5.5 Mixtures of Gases (Partial Pressures) 5.6 Kinetic Molecular Theory 5.7 Effusion and Diffusion 5.8-9
More informationGases. What are the four variables needed to describe a gas?
Gases What are the four variables needed to describe a gas? 1 Gases The simplest state of matter K.E. >> intermolecular forces Random motion Predictable behavior 2 Gases at STP Few Elements: H 2 N 2 O
More informationDumas Method. A method to determine the molar mass of a compound.
Dumas Method A method to determine the molar mass of a compound. The Dumas method uses the ideal gas law to determine the molar mass of a compound which is a liquid that has a boiling point between room
More informationGases CHAPTER. Section 10.1 Properties of Gases
CHAPTER Gases 10 Section 10.1 Properties of Gases 2. The following are observed properties of gases: (a) Gases have a variable volume. (b) Gases expand infinitely. (c) Gases compress uniformly. (d) Gases
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 informationChapter 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
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 informationProperties of Gases. assume the volume and shape of their containers. most compressible of the states of matter
Gases Properties of Gases assume the volume and shape of their containers most compressible of the states of matter mix evenly and completely with other gases much lower density than other forms of matter
More informationUseful Information to be provided on the exam: 1 atm = 760 mm Hg = 760 torr = lb/in 2 = 101,325 Pa = kpa. q = m C T. w = -P V.
Chem 101A Study Questions, Chapters 5 & 6 Name: Review Tues 10/25/16 Due 10/27/16 (Exam 3 date) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach
More informationChapter 5 Gases. A Gas- Uniformly fills any container Mixes completely with any other gas Can easily be compressed Exerts pressure on its surroundings
Chapter 5 Gases A Gas- Uniformly fills any container Mixes completely with any other gas Can easily be compressed Exerts pressure on its surroundings The properties of a gas depends upon four variables-
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 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 informationCh. 12 Notes - GASES NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 12 Notes - GASES NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. STANDARD ATMOSPHERIC PRESSURE: 1* atm 760* mm Hg 760* torr 101.3 kpa 14.7 psi * atm, mm Hg,
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 informationExam 4, Enthalpy and Gases
CHEM 1100 Dr. Stone November 8, 2017 Name_ G Exam 4, Enthalpy and Gases Equations and constants you may need: ΔE system = q + w PV = nrt R = 0.0821 (L*atm)/(mole*K) w = -PΔV K.E. = 1 2 m *µ 2 rms µ rms=
More informationCHEM 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
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 informationQuick Review 1. Properties of gases. 2. Methods of measuring pressure of gases. 3. Boyle s Law, Charles Law, Avogadro s Law. 4. Ideal gas law.
Quick Review 1. Properties of gases. 2. Methods of measuring pressure of gases. 3. Boyle s Law, Charles Law, Avogadro s Law. 4. Ideal gas law. 5. Dalton s law of partial pressures. Kinetic Molecular Theory
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 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 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 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 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 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 informationProperties of Gases. Properties of Gases. Pressure. Three phases of matter. Definite shape and volume. solid. Definite volume, shape of container
Properties of Gases Properties of Gases Three phases of matter solid Definite shape and volume liquid Definite volume, shape of container gas Shape and volume of container Properties of Gases A gas is
More informationAirbags fill with N 2 gas in an accident. Gas is generated by the decomposition of. 2 NaN 3 ---> > 2 Na + 3 N 2
1 2 Airbags fill with N 2 gas in an accident. Gas is generated by the decomposition of sodium azide,, NaN 3. 2 NaN 3 ---> > 2 Na + 3 N 2 3 4 There is a lot of free space in a gas. Gases can be expanded
More informationChapter 8 Gases. 8.1 Kinetic Theory of Gases. 8.2 Barometer. Properties of Gases. 8.1 Gases and Kinetic Theory 8.2 Gas Pressure 8.
Chapter 8 Gases 8.1 Gases and Kinetic Theory 8.2 Gas Pressure 8.8 Ideal Gas Law * You do not need to know Boyle s (8.3), Charles (8.4), Gay-Lussac s (8.5), Avogadro s (8.7) or the Combined gas (8.6) laws.
More informationGases and the Kinetic Molecular Theory
Gases and the Kinetic olecular Theory Importance in atmospheric phenomena, gas phase reactions, combustion engines, etc. 5.1 The hysical States of atter The condensed states liquid and solid The gaseous
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 informationKINETIC MOLECULAR THEORY
KINETIC MOLECULAR THEORY IMPORTANT CHARACTERISTICS OF GASES 1) Gases are highly compressible An external force compresses the gas sample and decreases its volume, removing the external force allows the
More informationUNIT 10.
UNIT 10 Pressure: F/A http://chemlab.truman.edu/chem130labs/calorimetryfiles/thermobackground.asp There are four variable needed to define the physical state of a gas. They are: o Temperature o Pressure
More informationLecture 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
More information1. What is the value of the quantity PV for one mole of an ideal gas at 25.0 C and one atm?
Real Gases Thought Question: How does the volume of one mole of methane gas (CH4) at 300 Torr and 298 K compare to the volume of one mole of an ideal gas at 300 Torr and 298 K? a) the volume of methane
More informationGases and Kinetic Molecular Theory
1 Gases and Kinetic Molecular Theory 1 CHAPTER GOALS 1. Comparison of Solids, Liquids, and Gases. Composition of the Atmosphere and Some Common Properties of Gases 3. Pressure 4. Boyle s Law: The Volume-Pressure
More information1. What does the test cover? All the material in the Unit 5 study guide and homework, plus review from earlier units (see practice test).
FAQs about HONORS CHEMISTRY EXAM 5: GASES 1. What does the test cover? All the material in the Unit 5 study guide and homework, plus review from earlier units (see practice test). 2. How long is the test?
More informationGases. Chapter 11. Preview. 27-Nov-11
Chapter 11 Gases Dr. A. Al-Saadi 1 Preview Properties and measurements of gases. Effects of temperature, pressure and volume. Boyle s law. Charles s law, and Avogadro s law. The ideal gas equation. Gas
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 information2012 AP CHEMISTRY FREE-RESPONSE QUESTIONS
01 AP CHEMISTRY FREE-RESPONSE QUESTIONS. A sample of a pure, gaseous hydrocarbon is introduced into a previously evacuated rigid 1.00 L vessel. The pressure of the gas is 0.00 atm at a temperature of 17C.
More information