Gas 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.
|
|
- Christian Jones
- 6 years ago
- Views:
Transcription
1 Standard T & P (STP) T = 73 K (0 o C) P = 1 atm = kpa = 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 units of density? He balloons mass/volume What does this suggest about gas density? It will depend strongly on T, P, and the mass of the gas molecules. Hot-air balloon Contrast with liquids and solids, whose densities depend somewhat on T, but far less on P. 1
2 What is the density of O gas in g/l at 5 o C and atm? Calculate # moles in 1 L, use MM of O to get g, divide by V. P = atm V = 1 L n =? R = L atm/mol K T = 5 C + 73 = 98 K n = Gas Density Example PV = nrt atm1 L L atm 98 K mol K PV n = RT = mol O? g/l O = mol O 3.00 g O 1 1 mol O 1 L Note: A value for gas density is meaningful only if accompanied by the T and P at which it was measured. = 1.11 g/l O 5 C, atm Gas Density and Molar Mass We can develop an expression relating density and MM using PV = nrt. Substituting: m PV = RT M PV = nrt Density!! m PM = RT V m n = M PM = drt Therefore, the density of an ideal gas depends on T, P, V, and Molar Mass We can use the density of a gas to determine its molar mass.
3 PM = drt Example A.30-g sample of an unknown solid was vaporized in a 345-mL vessel. If the vapor has a pressure of 985 mmhg at 148 o C, what is the molecular weight of the solid? P = 985 mmhg M =? d =.30 g L T = 148 o C = 41 K = 1.96 atm = g/l R = L atm/mol K V = 345 ml mass of solid =.30 g Heat applied mass of gas =.30 g M = drt = P g/l L atm 41 K 1.96 atm mol K = g/mol Chemical Equations and Calculations Atoms (Molecules) Avogadro s Number Reactants 6.0 x 10 3 mol -1 Moles Molar Mass Mass g/mol Products Molarity moles / L PV = nrt Solutions Gases 3
4 Gas Stoichiometry Example What volume of N (g) is produced when 70.0 g NaN 3 is decomposed? P = 735 mmhg, T = 6 o C NaN 3 (s) Na(l) + 3 N (g) 70.0 g? L g/mol 735 mmhg 6 o C 8.0 g/mol 1. The Stoichiometry Part: mass NaN 3 mol NaN 3 mol N. The Gas Law Part: mol N, P, T V of N (g) Example: The Stoichiometry Part What volume of N (g) is produced when 70.0 g NaN 3 is decomposed? P = 735 mmhg, T = 6 o C NaN 3 (s) Na(l) + 3 N (g) 1 mol NaN? mol N 3 3 mol N = 70.0 g NaN g NaN 3 mol NaN 3 = mol N 4
5 What volume of N (g) is produced when 70.0 g NaN 3 is decomposed? (P = 735 mmhg, T = 6 o C) P = 735 mmhg 1 atm 760 mmhg V =? L n = mol N R = L.atm/mol.K T = 6 o C + 73 = 99 K V = Example: The Gas Law Part = atm PV = nrt V = nrt P mol N L atm 99 K V = L = 41.0 L Yay!!! atm mol K Dalton s Law of Partial Pressures P He = 00 torr P Ar = 500 torr P = 700 torr Recall that according to the ideal gas law, gas molecules are non-interacting point particles. Increasing the number of point particles increases the pressure by an amount that is proportional to the number of particles. For a mixture of ideal gases in a container: pressure = the sum of the individual gas pressures. 5
6 Dalton s Law of Partial Pressures Say we have a container with some amount of three different gases inside, at a certain T and P. n = n 1 + n + n3 Dalton s Law says that the pressure exerted by the three gases is the sum of the individual pressures. P = P 1 + P + P 3 P = P 1 + P + P 3 1 P = + + P V = n1rt + nrt + n3rt P V = n RT n RT n RT n3rt V V V P V = n + n + n RT 1 3 Partial Pressures Example Mixtures of He and O are used in scuba tanks to help prevent the bends. For a particular dive, 1 L of O at 5 o C and 1.0 atm was pumped along with 46 L of He at 5 o C and 1.0 atm into a 5.0-L tank. What is the partial pressure of each gas? What is the pressure? 1. Find the number of moles of each gas that were delivered to the tank.. Find the partial pressure of each gas in the tank. 3. Add them up! 6
7 Mixtures of He and O are used in scuba tanks to help prevent the bends. For a particular dive, 1 L of O at 5 o C and 1.0 atm was pumped along with 46 L of He at 5 o C and 1.0 atm into a 5.0-L tank. What is the partial pressure of each gas? What is the pressure? O Data: P = 1.0 atm V = 1 L n =? mol R = L atm/mol K T = 5 o C = 98 K He Data: P = 1.0 atm V = 46 L n =? mol R = L atm/mol K T = 5 o C = 98 K PV n = RT n = O n = He 1.0 atm1 L L atm 98 K mol K 1.0 atm46 L L atm 98 K mol K = 0.49 mol O = 1.9 mol He Using the moles of each gas, the temperature, and volume of the tank we can now calculate the partial pressure of each gas, then add them to get the pressure. P = O P = He 0.49 mol O L atm 98 K 5.0 L mol K 1.9 mol He L atm 98 K 5.0 L mol K P = =.4 atm = 9.3 atm P = 11.7 atm Partial pressures of O and He in the 5.0 L scuba tank nrt V 7
8 Mole Fraction and Partial Pressure In the last example, we determined the pressure by adding the partial pressures. We could have also added the moles of each gas, and determined a pressure. These two approaches suggest that a relationship exists between the moles of each gas and the pressure. Mole Fraction and Partial Pressure Mole Fraction (): ratio of the number of moles of a component in a mixture to the number of moles in the mixture. n1 n1 1 n n n n ni i n 1 3 V Pi RT V P RT Pi P P P i i Dalton s Law The fraction of moles of a certain gas in a mixture is equal to the ratio of its partial pressure to the pressure of the mixture. 8
9 Mixtures of He and O are used in scuba tanks to help prevent the bends. For a particular dive, 1 L of O at 5 o C and 1.0 atm was pumped along with 46 L of He at 5 o C and 1.0 atm into a 5.0-L tank. What is the partial pressure of each gas? What is the pressure? n O = 0.49 mol n He = 1.9 mol 0.49 mol O O =.39 mol gas n =.39 mol P = 11.7 atm = 0.05 He 1.9 mol He =.39 mol gas = P = atm O P = atm He =.39 atm = 9.8 atm.4 atm 9.3 atm Previous results. Partial pressures of O and He in the 5.0 L scuba tank Saturation
10 Production of O (g) by thermal decomposition of KCIO 3 O is mixed with water vapor in the collection vessel. Collection of Hydrogen Gas Over Water Vapor pressure - I HCl (aq) + Zn (s) ZnCl (aq) + H (g) Calculate the mass of hydrogen gas collected over water if 156 ml of gas is collected at 0 o C and 769 mm Hg. P Total = P H + P H O P H = P Total - P H O FROM TABLE P H = 769 mm Hg mm Hg = 75 mm Hg T = 0 o C + 73 = 93 K P H = (75 mm Hg )(1 atm/ 760 mm Hg) = atm V = L 10
11 Collection of Hydrogen Gas Over Water Vapor Pressure - II P H V = n H RT n H = P H V / RT n H = (0.989 atm) (0.156 L) (0.081 L atm/mol K) (93 K) n H = mol Mass H = mol x (.016 g H / mol H ) = g H Kinetic Molecular Theory (KMT) The gas laws of Boyle, Charles, and Avogadro are empirical, meaning they are based on observation of a macroscopic property. These laws offer a general description of behavior based on many experiments. The empirical gas laws can tell you what happens to an ideal gas under certain conditions, but not why it happens. KMT is a theoretical, molecular-level model of ideal gases, which can be used to predict the macroscopic behavior of a gaseous system. KMT Simulation: 11
12 Postulates of KMT Gas particles are so small that their volume is negligible. Gas particles are in constant, random motion. This motion is associated with an average kinetic energy that is directly proportional to the Kelvin temperature of the gas. Gas molecules constantly collide with each other and with the container walls. The collisions of the particles with the container walls are the cause of the pressure exerted by the gas. Collisions are elastic. The particles are assumed to exert no forces on each other; they neither attract or repel their neighbors. KMT: Central Points The main ideas you should take from KMT are that we can describe temperature and pressure from a molecular perspective. Pressure: arises from molecules banging into the container walls. Temperature: Is directly related to the kinetic energy of the gas molecules. The more KE they have, the greater their temperature. 1
13 KMT Let s consider the average KE per molecule and see how it determines molecular speed. Total KE in 1 mol of gas: 3 RT From KMT. Note: T is measured in Kelvin Average KE per molecule: 1 mu Where u is an average of molecular velocity, and m is the mass of one molecule mu RT N A We are apportioning the KE in the mole of gas among all the molecules in an average fashion. KMT (cont.) mu RT N A We are apportioning the KE in the mole of gas among all the molecules in an average fashion. 3RT u Note that mn A = M. mn A u rms 3RT M u rms is the speed of a molecule that has the average KE. u rms gives us a formal connection between average gas speed, T, and M. 13
14 Distribution of Molecular Speeds Maxwell-Boltzmann curve (a statistical distribution) This plot represents the fraction of gas molecules in a sample that are traveling at a given velocity. u m most probable speed u av average speed u rms the speed of a molecule with the average molecular kinetic energy (m/s) 3RT u rms M Increased T increased average KE increased u rms. Increased M decreased u rms Increased T increased average KE increased u rms Maximum of curve shifts to higher u, and distribution spreads out. Distribution of speeds will be shorter and fatter at higher temperatures. Increased M decreased u rms Heavier molecules have lower average speed than lighter molecules at a given temperature. Distribution of speeds for heavier gases will be taller and skinnier than for lighter molecules. 3RT u rms M NOTE: There are always some molecules with low velocity in a Boltzmann distribution!! 14
Standard 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 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 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 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 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 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 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 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. 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 informationApparatus for Studying the Relationship Between Pressure and Volume of a Gas
The Gas Laws Apparatus for Studying the Relationship Between Pressure and Volume of a Gas As P (h) increases V decreases Boyle s Law P x V = constant P 1 x V 1 = P 2 x V 2 Constant temperature Constant
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 informationThe Kinetic-Molecular Theory of Gases
The Kinetic-Molecular Theory of Gases kinetic-molecular theory of gases Originated with Ludwig Boltzman and James Clerk Maxwell in the 19th century Explains gas behavior on the basis of the motion of individual
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 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 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 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 informationGases and Kinetic Theory
Gases and Kinetic Theory Chemistry 35 Fall 2000 Gases One of the four states of matter Simplest to understand both physically and chemically Gas Properties Low density Fluid Can be defined by their: 1.
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 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 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 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 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 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 informationDerived copy of The Kinetic-Molecular Theory *
OpenStax-CNX module: m62491 1 Derived copy of The Kinetic-Molecular Theory * Sylvia K. Quick Based on The Kinetic-Molecular Theory by OpenStax This work is produced by OpenStax-CNX and licensed under the
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 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 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 informationCHAPTER 14: The Behavior of Gases
Name: CHAPTER 14: The Behavior of Gases Period: RELATIONSHIPS BETWEEN PRESSURE, VOLUME & TEMPERATURE OF A GAS Boyle s Law-Pressure and Volume Volume (ml) Pressure ( ) 60 50 40 30 20 10 Practice problem:
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 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 informationExam 1. Remember to refer to the Periodic Table handout that is separate from this exam copy.
001 version last name first name signature McCord CH301 unique: 49885 TTh 9:30 am - 11 am Exam 1 Sep 17, 2018 Monday 7:30-9:00 PM A - Mi in BUR 106 Mo - Z in JES A121A Remember to refer to the Periodic
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 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 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 informationvapors: gases of substances that are normally liquids or solids 1 atm = 760 mm Hg = 760 torr = kpa = bar
Gases A Chemistry Lecture Outline Name: Basics on Gases composition of the atmosphere: properties of gases: vapors: gases of substances that are normally liquids or solids Equation for pressure: 1 atm
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 informationChapter 6: Gases. Philip Dutton University of Windsor, Canada N9B 3P4. Prentice-Hall 2002
General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 6: Gases Philip Dutton University of Windsor, Canada N9B 3P4 Prentice-Hall 2002 Prentice-Hall 2002 General
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 informationIdeal Gas & Gas Stoichiometry
Ideal Gas & Gas Stoichiometry Avogadro s Law V a number of moles (n) V = constant x n Constant temperature Constant pressure V 1 /n 1 = V 2 /n 2 Ammonia burns in oxygen to form nitric oxide (NO) and water
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 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 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 informationWarning!! Chapter 5 Gases. Chapter Objectives. Chapter Objectives. Chapter Objectives. Air Pollution
Warning!! Larry Brown Tom Holme www.cengage.com/chemistry/brown Chapter 5 Gases These slides contains visual aids for learning BUT they are NOT the actual lecture notes! Failure to attend to lectures most
More informationChapter 11. Molecular Composition of Gases
Chapter 11 Molecular Composition of Gases PART 1 Volume-Mass Relationships of Gases Avogadro s Law Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. Recall
More informationChapter 5 Gases - 4 Gas Stoichiometry. Dr. Sapna Gupta
Chapter 5 Gases - 4 Gas Stoichiometry Dr. Sapna Gupta Stoichiometry in Gases Amounts of gaseous reactants and products can be calculated by utilizing The ideal gas law to relate moles to T, P and V. Moles
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 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 informationSubstances that are Gases under Normal Conditions
Chapter 5: Gases 5.1 Early Experiments 5.2 The gas laws of Boyle, Charles, and Avogadro 5.3 The Ideal Gas Law 5.4 Gas Stiochiometry 5.5 Dalton s Law of Partial Pressures 5.6 The Kinetic molecular Theory
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 informationAP Chemistry Unit 5 - Gases
Common Gases at Room Temperature AP Chemistry Unit 5 - Gases Know these! HCN toxic slight odor of almonds HS toxic odor of rotten eggs CO toxic odorless CO odorless CH4 methane odorless, flammable CH4
More informationUnit 13 Gas Laws. Gases
Unit 13 Gas Laws Gases The Gas Laws Kinetic Theory Revisited 1. Particles are far apart and have negligible volume. 2. Move in rapid, random, straight-line motion. 3. Collide elastically. 4. No attractive
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 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 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 information9.5 The Kinetic-Molecular Theory
502 Chapter 9 Gases Figure 9.30 In a diffuser, gaseous UF 6 is pumped through a porous barrier, which partially separates 235 UF 6 from 238 UF 6 The UF 6 must pass through many large diffuser units to
More informationPreparation of the standard solution. Exp 5: Copyright Houghton Mifflin Company.All
Preparation of the standard solution Exp 5: Copyright Houghton Mifflin Company.All 1 1 Mass of KHP: 5.2 5.5 g Volume of volumetric flask: 250.0 cm Molarity of standard (KHP) solution: M = n/v Copyright
More informationGases: Units of pressure: the pascal(pa)(1 Pa = 1 N/m2 = 1 kg m-1
Gases: Units of pressure: the pascal(pa)(1 Pa = 1 N/m 2 = 1 kg m -1 s -2 ) psi(pounds per square inch) atmosphere(atm) millimeters of mercury(mm Hg) torr(1 torr = 1 mm Hg) kilopascal(kpa) Mercury Barometer:
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 informationGeneral Properties of Gases
Page III-9-1 / Chapter Nine Lecture Notes Gases and Their Properties Chapter 9 Importance of Gases Chemistry 222 Professor Michael Russell Airbags fill with N 2 gas in an accident. Gas is generated by
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 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 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 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 informationThe Kinetic-Molecular Theory of Gases
The Kinetic-Molecular Theory of Gases kinetic-molecular theory of gases Originated with Ludwig Boltzman and James Clerk Maxwell in the 19th century Explains gas behavior on the basis of the motion of individual
More informationGASES (Chapter 5) Temperature and Pressure, that is, 273 K and 1.00 atm or 760 Torr ) will occupy
I. Ideal gases. A. Ideal gas law review. GASES (Chapter 5) 1. PV = nrt Ideal gases obey this equation under all conditions. It is a combination ofa. Boyle's Law: P 1/V at constant n and T b. Charles's
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 informationCHEMISTRY II B. Chapter 10 & Chapter 12. Gases
CHEMISTRY II B Chapter 10 & Chapter 12 Gases Think to yourself! How do gas particles move/behavior?! What is the Kinetic Molecular Theory?! Gases are mostly empty space! Particles have no attractive or
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 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 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 informationAP Chapter 5: Gases Name
AP Chapter 5: Gases Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 5: Gases 2 Warm-Ups (Show your work for credit) Date 1. Date 2.
More informationTest Bank for Chemistry 9th Edition by Zumdahl
Test Bank for Chemistry 9th Edition by Zumdahl 1. Gases generally have A) low density B) high density C) closely packed particles D) no increase in volume when temperature is increased E) no decrease in
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 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 informationI. Gas Laws A. Four properties of gases 1. Volume - V
Gas Laws Learning Objectives TLW know the variables that influence the behavior of gases (TEKS 9) TLW be able to describe interrelationships between temperature, number of moles, pressure, and volume of
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 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 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 informationProperties of Gases. Gases have four main characteristics compared with solids and liquids:
1 Properties of Gases Gases have four main characteristics compared with solids and liquids: Gases take the volume and shape of their containers. Mix completely (homogeneously) with any other gas. Compressible:
More informationChapter 10 Gases. Dr. Ayman Nafady. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E.
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Gases Dr. Ayman Nafady 2009, Prentice-Hall, 10.1. Characteristics of Gases Unlike liquids
More informationKINETIC MOLECULAR DESCRIPTION OF THE STATES OF MATTER
KINETIC MOLECULAR DESCRIPTION OF THE STATES OF MATTER CHAPTER 9 The Gaseous State CHAPTER 10 Solids, Liquids, and Phase Transitions CHAPTER 11 Solutions 392 Gas Liquid Solid 9 THE GASEOUS STATE 9.1 The
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 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 informationCHAPTER 13 Gases The Gas Laws
CHAPTER 13 Gases 13.1 The Gas Laws The gas laws apply to ideal gases, which are described by the kinetic theory in the following five statements. Gas particles do not attract or repel each other. Gas particles
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 information