Chapter 1. The Properties of Gases Fall Semester Physical Chemistry 1 (CHM2201)
|
|
- Esther Chambers
- 6 years ago
- Views:
Transcription
1 Chapter 1. The Properties of Gases 2011 Fall Semester Physical Chemistry 1 (CHM2201)
2 Contents The Perfect Gas 1.1 The states of gases 1.2 The gas laws Real Gases 1.3 Molecular interactions 1.4 The van der Waals equation
3 States of Matter Gases fill container, random rapid motion, never coming to rest or clumping together. Motion is mainly translational Liquids fixed volume, flow and assume shape of container, only slightly compressible, stronger forces hold molecules together. Motion is mainly translational Solids fixed volume, definite shape, generally less compressible than liquids, forces hold particles in a fixed shape. Motion is mainly vibrational
4 1.1 The states of gases Key points 1. Pressure provides a criterion of mechanical equilibrium for systems free to change their volume 2. Pressure is measured with a barometer 3. The Zeroth Law of thermodynamics
5 1.1 The states of gases Physical State 1. Two samples of a substance that have the same physical properties are in the same state 2. Physical Properties : V, n, p, and T 3. It is sufficient to specify only three of these variables 4. p = f(t,v,n) : an equation of state (e.g.) p = nrt/v for a perfect gas
6 1.1 The states of gases (a) Pressure Defined as force, F, divided by the area, A p = F/A Mechanical equilibrium
7 1.1 The states of gases (b) The measurement of pressure barometer Hydrostatic pressure : P = ρgh ü ρ : the mass density of liquid ü g : gravitational acceleration ü h : height
8 1.1 The states of gases (c) Temperature Indicates the direction of the flow of energy through a thermally conducting rigid wall Types of boundary between two objects at different temperatures ü Diathermic : a change of state is observed ü Adiabatic : no change occur Thermal equilibrium : No change of state occurs when two objects are in contact through a diathermic boundary
9 1.1 The states of gases (c) Temperature Thermal equilibrium
10 1.1 The states of gases The Zeroth Law of thermodynamics If A is in thermal equilibrium with B, and B is in thermal equilibrium with C, then C is also in thermal equilibrium with A Justifies the concept of temperature and the use of a thermometer Celcius scale : C Thermodynamic temperature scale : K (kelvins) T/K = θ/ C
11 The perfect gas : 1.2 The gas laws Key points 1. The perfect gas law summerizes Boyle s and Charles s laws and Avogadro s principle 2. The kinetic theory of gases provides a model for the gas laws 3. A mixture of perfect gases behaves like a single perfect gas
12 1.2 The gas laws (a) The perfect gas law Boyle s law : pv = constant at constant n, T Charles s law : V = constant T at constant n, P P = constant T at constant n, V Avogadro s principle : V = constant n at constant p, T isotherm isobars isochores
13 1.2 The gas laws (a) The perfect gas law pv = nrt : perfect gas law R : gas constant Perfect (ideal) gas vs. Real gas
14 1.2 The gas laws (a) The perfect gas law pv = nrt : perfect gas law R : gas constant Perfect (ideal) gas vs. Real gas The perfect gas law is important because it is used to derive a wide range of relations that are used throughout thermodynamics
15 1.2 The gas laws (b) The kinetic model of gases 1. The gas consists of molecules of mass m in ceaseless random motion 2. The size of the molecules is negligible, in the sense that their diameters are much smaller than the average distance travelled between collisions 3. The molecules interact only through brief, infrequent, and elastic collisions
16 1.2 The gas laws (b) The kinetic model of gases pv = 1 3 nmc2 M : the molar mass of the molecules c : the root mean-square speed of the molecules c = v 2 1/2! = 3RT $ # & " M % pv = nrt 1/2
17 1.2 The gas laws (c) Mixtures of gases Dalton s law : The pressure exerted by a mixture of gases is the sum of the pressures that each one would exert if it occupied the container alone. p J = x J p : partial pressure x J = n J N : mole fraction p A + p B + = (x A + x B + )p = p
18 The real gas : 1.3 Molecular Interactions Key points 1. The extent of deviations from perfect behavior is summarized by the compression factor 2. The virial equation is an empirical extension of the perfect gas equation 3. The isotherms of a real gas introduce the concept of vapor pressure and critical behavior 4. A gas can be liquefied by pressure alone only if T T C.
19 1.3 Molecular interactions Repulsive forces and attractive forces assist expansion and compression, respectively 1. At low pressure, the intermolecular forces play no significant role 2. At moderate pressures, the attractive forces dominate 3. At high pressures, the repulsive forces dominate
20 1.3 Molecular interactions (a) Compression factor Z = V m V = pv m o m RT : Compression factor 1. At low pressure, Z 1 2. At moderate pressures, Z < 1 3. At high pressures, Z > 1
21 1.3 Molecular interactions (b) Virial coefficients The virial equation of state pv m = RT(1+ B' p + C' p 2 + )! = RT 1+ B + C 2 V m V + $ # & " m % = RTZ dz dp = B'+ 2pC'+ B as p 0 The virial coefficients depend on T dz/dp 0 as p 0 at Boyle temperature
22 1.3 Molecular interactions (c) Condensation vapor pressure A liquid appears The pressure is constant Two phases exist Deviate from the perfect gas law Relatively ideal Experimental Isotherms of carbon dioxide
23 1.3 Molecular interactions (c) Critical constants At T C, a surface separating two phases does not appear Critical Point : the volumes at each end of the horizontal part of the isotherm merge to a critical point T C : critical temperature p C : critical pressure V C : critical molar volume At T > T C, the supercritical fluid Experimental Isotherms of carbon dioxide
24 1.4 The van der Waals equation Key points 1. The van der Waals equation is a model equation of state with two parameters 2. The van der Waals equation captures the general features including the critical behavior 3. The properties of real gases are coordinated by expressing their equations of state in terms of reduced variables
25 1.4 The van der Waals equation (a) Formulation of the equation p = nrt V nb a n2 V 2 = RT V m b a 2 V m a : the strength of attractive interactions b : the volume taken by molecules
26 1.4 The van der Waals equation (b) The features p = nrt V nb a n2 V 2 = RT V m b a 2 V m Perfect gas isotherms are obtained at high T and large molar volumes Liquid and gases coexist when cohesive and dispersing effects are in balance The critical constants are related to a and b The unrealistic Van der Waals loops need be treated by the Maxwell construction
27 1.4 The van der Waals equation (b) The features p = nrt V nb a n2 V 2 = RT V m b a 2 V m The critical constants are related to a and b dp RT = dv m (V m b) + 2a 2 V = 0 3 m d 2 p dv m 2 = 2RT (V m b) 6a 3 V = 0 4 m V C = 3b, p C = a 27b 2, T C = 8a 27Rb Z C = p C V C RT C = 3 8
28 1.4 The van der Waals equation (b) The principle of corresponding states p = nrt V nb a n2 V = 2 Reduced variables V r = V m V C, p r = p p C, T r = T T C p r = 8T r 3V r V r RT V m b a 2 V m Real gases at the same reduced volume and reduced temperature exert the same reduced pressure
Real Gases. Sections (Atkins 6th Ed.), (Atkins 7-9th Eds.)
Real Gases Sections 1.4-1.6 (Atkins 6th Ed.), 1.3-1.5 (Atkins 7-9th Eds.) Molecular Interactions Compression factor Virial coefficients Condensation Critical Constants Van der Waals Equation Corresponding
More informationGaseous States of Matter
Gaseous States of Matter Semester-1 : ICY-101: CHEMISTRY-I, Unit III Dr. Tapta Kanchan Roy Assistant Professor Department of Chemistry & Chemical Sciences Central University of Jammu 1 The simplest state
More informationGeneral Physical Chemistry I
General Physical Chemistry I Lecture 5 Aleksey Kocherzhenko February 10, 2015" Last time " Diffusion, effusion, and molecular collisions" Diffusion" Effusion" Graham s law: " " " 1 2 r / M " (@ fixed T
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 informationSchool of Chemical & Biological Engineering, Konkuk University
School of Chemical & Biological Engineering, Konkuk University Chemistry is the science concerned with the composition, structure, and properties of matter, as well as the changes it undergoes during chemical
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 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 informationConcepts of Thermodynamics
Thermodynamics Industrial Revolution 1700-1800 Science of Thermodynamics Concepts of Thermodynamics Heavy Duty Work Horses Heat Engine Chapter 1 Relationship of Heat and Temperature to Energy and Work
More informationChapter 1 - The Properties of Gases. 2. Knowledge of these defines the state of any pure gas.
Chapter 1 - The Properties of Gases I. The perfect gas. A. The states of gases. (definition) 1. The state variables: volume=v amount of substance, moles = n pressure = p temperature = T. Knowledge of these
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 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 information5.60 Thermodynamics & Kinetics Spring 2008
MIT OpenCourseWare http://ocw.mit.edu 5.60 Thermodynamics & Kinetics Spring 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. 5.60 Spring 2008 Lecture
More information1 Points to Remember Subject: Chemistry Class: XI Chapter: States of matter Top concepts 1. Intermolecular forces are the forces of attraction and repulsion between interacting particles (atoms and molecules).
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 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 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 informationfiziks Institute for NET/JRF, GATE, IIT-JAM, JEST, TIFR and GRE in PHYSICAL SCIENCES
Content-Thermodynamics & Statistical Mechanics 1. Kinetic theory of gases..(1-13) 1.1 Basic assumption of kinetic theory 1.1.1 Pressure exerted by a gas 1.2 Gas Law for Ideal gases: 1.2.1 Boyle s Law 1.2.2
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 informationCHAPTER 12 GASES AND KINETIC-MOLECULAR THEORY
. Pressure CHAPER GASES AND KINEIC-MOLECULAR HEORY. Boyle s Law: he -P Relationship 3. Charles Law: he - Relationship 4. Standard &P 5. he Combined Gas Law Equation 6. Avogadro s Law and the Standard Molar
More informationProperties of Gases. The perfect gas. States of gases Gas laws Kinetic model of gases (Ch th ed, th ed.) Real gases
Properties of Gases Chapter 1 of Physical Chemistry - 6th Edition P.W. Atkins. Chapter 1 and a little bit of Chapter 24 of 7th Edition. Chapter 1 and a little bit of Chapter 21 of 8th edition. The perfect
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 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. T boil, K. 11 gaseous elements. Rare gases. He, Ne, Ar, Kr, Xe, Rn Diatomic gaseous elements H 2, N 2, O 2, F 2, Cl 2
Gases Gas T boil, K Rare gases 11 gaseous elements He, Ne, Ar, Kr, Xe, Rn 165 Rn 211 N 2 O 2 77 F 2 90 85 Diatomic gaseous elements Cl 2 238 H 2, N 2, O 2, F 2, Cl 2 H 2 He Ne Ar Kr Xe 20 4.4 27 87 120
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 informationis more suitable for a quantitative description of the deviation from ideal gas behaviour.
Real and ideal gases (1) Gases which obey gas laws or ideal gas equation ( PV nrt ) at all temperatures and pressures are called ideal or perfect gases. Almost all gases deviate from the ideal behaviour
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 informationChemistry 11. Unit 11 Ideal Gas Law (Special Topic)
Chemistry 11 Unit 11 Ideal Gas Law (Special Topic) 2 1. States of substances It has been studied in Unit 3 that there exist 3 states of matter in nature: gas, liquid and solid. (Technically there is the
More informationSummary of Gas Laws V T. Boyle s Law (T and n constant) Charles Law (p and n constant) Combined Gas Law (n constant) 1 =
Summary of Gas Laws Boyle s Law (T and n constant) p 1 V 1 = p 2 V 2 Charles Law (p and n constant) V 1 = T 1 V T 2 2 Combined Gas Law (n constant) pv 1 T 1 1 = pv 2 T 2 2 1 Ideal Gas Equation pv = nrt
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 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 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 informationvan der Waals Isotherms near T c
van der Waals Isotherms near T c v d W loops are not physical. Why? Patch up with Maxwell construction van der Waals Isotherms, T/T c van der Waals Isotherms near T c Look at one of the van der Waals isotherms
More informationSatish Chandra. Unit I, REAL GASES. Lecture Notes Dated: Dec 08-14, Vander-Waals Gas
Vander-Waals Gas Lecture Notes Dated: Dec 08-14, 01 Many equations have been proposed which describe the pvt relations of real gases more accurately than does the equation of state of an ideal gas. Some
More informationChapter 7. Gases, liquids, and solids. Water coexisting in three states H 2 O (g) in air H 2 O (l) ocean H 2 O (s) iceberg
Chapter 7 Gases, liquids, and solids Water coexisting in three states H 2 O (g) in air H 2 O (l) ocean H 2 O (s) iceberg What s crack a lackin? Kinetic-molecular theory of gases Physical states and the
More informationProperties of Gases. Molecular interactions van der Waals equation Principle of corresponding states
Properties of Gases Chapter 1 of Atkins and de Paula The Perfect Gas States of gases Gas laws Real Gases Molecular interactions van der Waals equation Principle of corresponding states Kinetic Model of
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 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 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 informationSome Fundamental Definitions:
Lecture 2. The GAS LAWS Some Fundamental Definitions: SYSTEM: the part of the universe being the subject of study 1 Some Fundamental Definitions: State of the System: condition of a system at any given
More informationFUNDAMENTALS OF THERMODYNAMICS AND HEAT TRANSFER
FUNDAMENTALS OF THERMODYNAMICS AND HEAT TRANSFER Lecture 2: Evaluating properties Pierwsza strona STATES OF THE MATTER Phase is a quantity is of matter that is homogeneous throughout in both chemical composition
More informationPV = nrt where R = universal gas constant
Ideal Gas Law Dd Deduced dfrom Combination of Gas Relationships: V 1/P, Boyle's Law V, Charles's Law V n, Avogadro'sLaw Therefore, V nt/p or PV nt PV = nrt where R = universal gas constant The empirical
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 informationaskiitians Class: 11 Subject: Chemistry Topic: Kinetic theory of gases No. of Questions: The unit of universal gas constant in S.I.
Class: 11 Subject: Chemistry Topic: Kinetic theory of gases No. of Questions: 33 1. The unit of universal gas constant in S.I.unit is A. calorie per degree Celsius B. joule per mole C. joule/k mole C 2.
More informationCh 6 Gases 6 GASES. Property of gases. pressure = force/area
6 GASES Gases are one of the three states of matter, and while this state is indispensable for chemistry's study of matter, this chapter mainly considers the relationships between volume, temperature and
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 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 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 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 informationLecture 2 PROPERTIES OF GASES
Lecture 2 PROPERTIES OF GASES Reference: Principles of General Chemistry, Silberberg Chapter 6 SOME FUNDAMENTAL DEFINITIONS: SYSTEM: the part of the universe being the subject of study 1 SOME FUNDAMENTAL
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 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 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 informationCHEMISTRY NOTES Chapter 12. The Behavior of Gases
Goals : To gain an understanding of : 1. The kinetic theory of matter. 2. Avogadro's hypothesis. 3. The behavior of gases and the gas laws. NOTES: CHEMISTRY NOTES Chapter 12 The Behavior of Gases The kinetic
More informationChapter 10. Thermal Physics
Chapter 10 Thermal Physics Thermal Physics Thermal physics is the study of Temperature Heat How these affect matter Thermal Physics, cont Descriptions require definitions of temperature, heat and internal
More informationChapter 15 Thermal Properties of Matter
Chapter 15 Thermal Properties of Matter To understand the mole and Avogadro's number. To understand equations of state. To study the kinetic theory of ideal gas. To understand heat capacity. To learn and
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 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 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 informationPhases of matter and phase diagrams
Phases of matter and phase diagrams Transition to Supercritical CO2 Water Ice Vapor Pressure and Boiling Point Liquids boil when the external pressure equals the vapor pressure. Temperature of boiling
More informationThermodynamics 1 Lecture Note 1
Thermodynamics 1 Lecture Note 1 March 02, 2015 Kwang Kim Yonsei University kbkim@yonsei.ac.kr 39 8 7 34 53 Y O N Se I 88.91 16.00 14.01 78.96 126.9 Scientific Thinking - System under investigation - Description
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 informationReal Gases 1. The value of compressibility factor for one mole of a gas under critical states is 1) 3/8 2) 2/3 3) 8/27 4) 27/8 2. an der Waal s equation for one mole of CO2 gas at low pressure will be
More informationCh. 19: The Kinetic Theory of Gases
Ch. 19: The Kinetic Theory of Gases In this chapter we consider the physics of gases. If the atoms or molecules that make up a gas collide with the walls of their container, they exert a pressure p on
More informationCHEM1100 Summary Notes Module 2
CHEM1100 Summary Notes Module 2 Lecture 14 Introduction to Kinetic Theory & Ideal Gases What are Boyle s and Charles Laws? Boyle s Law the pressure of a given mass of an ideal gas is inversely proportional
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 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 informationUNIT 5 : STATES OF MATTER Concept 1. INTERMOLECULAR FORCES
www.tiwariacademy.in UNIT 5 : STATES OF MATTER CONCEPT WISE HANDOUTS KEY CONCEPTS : 1. Intermolecular Forces 2. Gas Laws 3. Behaviour of gases Concept 1. INTERMOLECULAR FORCES Intermolecular forces- forces
More informationPhysics 160 Thermodynamics and Statistical Physics: Lecture 2. Dr. Rengachary Parthasarathy Jan 28, 2013
Physics 160 Thermodynamics and Statistical Physics: Lecture 2 Dr. Rengachary Parthasarathy Jan 28, 2013 Chapter 1: Energy in Thermal Physics Due Date Section 1.1 1.1 2/3 Section 1.2: 1.12, 1.14, 1.16,
More informationLecture PowerPoints. Chapter 13 Physics: Principles with Applications, 7 th edition Giancoli
Lecture PowerPoints Chapter 13 Physics: Principles with Applications, 7 th edition Giancoli This work is protected by United States copyright laws and is provided solely for the use of instructors in teaching
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 informationHeat, Work, Internal Energy, Enthalpy, and the First Law of Thermodynamics. Internal Energy and the First Law of Thermodynamics
CHAPTER 2 Heat, Work, Internal Energy, Enthalpy, and the First Law of Thermodynamics Internal Energy and the First Law of Thermodynamics Internal Energy (U) Translational energy of molecules Potential
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 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 informationChapter 10 Gases. Measurement of pressure: Barometer Manometer Units. Relationship of pressure and volume (Boyle s Law)
Chapter 10 Gases Conditions of ideal gases: Ideal gases have no attractive forces between the molecules. the atoms volume taken into account when looking at the volume a gas occupies. Low pressure and
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 informationUNIT 5 States of matter I. Questions carrying one mark
UNIT 5 States of matter I. Questions carrying one mark 5. What are van der Waals forces? 5.2 What type of van der Waals force exists between HCl molecules? 5.3 Between which type of molecules does dipole
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 informationGases. Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures.
Gases Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures Gases Properties of Gases All elements will form a gas at
More informationChapter 5 Gases. Chapter 5: Phenomena. Properties of Gases. Properties of Gases. Pressure. Pressure
Chapter 5: Phenomena Phenomena: To determine the properties of gases scientists recorded various observations/measurements about different gases. Analyze the table below looking for patterns between the
More informationKINETIC THEORY OF GASES
KINETIC THEORY OF GASES Boyle s Law: At constant temperature volume of given mass of gas is inversely proportional to its pressure. Charle s Law: At constant pressure volume of a given mass of gas is directly
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 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 informationCHAPTER III: Kinetic Theory of Gases [5%]
CHAPTER III: Kinetic Theory of Gases [5%] Introduction The kinetic theory of gases (also known as kinetic-molecular theory) is a law that explains the behavior of a hypothetical ideal gas. According to
More informationSPH 302 THERMODYNAMICS
THERMODYNAMICS Nyongesa F. W., PhD. e-mail: fnyongesa@uonbi.ac.ke 1 Objectives Explain the Laws of thermodynamics & their significance Apply laws of thermodynamics to solve problems relating to energy
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 informationDownloaded from
Chapter 13 (Kinetic Theory) Q1. A cubic vessel (with face horizontal + vertical) contains an ideal gas at NTP. The vessel is being carried by a rocket which is moving at a speed of500 ms in vertical direction.
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 informationS OF MATTER TER. Unit. I. Multiple Choice Questions (Type-I)
Unit 5 STATE TES TE S OF MATTER MA TER I. Multiple Choice Questions (Type-I) 1. A person living in Shimla observed that cooking food without using pressure cooker takes more time. The reason for this observation
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 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 13: Temperature, Kinetic Theory and Gas Laws
Chapter 1: Temperature, Kinetic Theory and Gas Laws Zeroth Law of Thermodynamics (law of equilibrium): If objects A and B are separately in thermal equilibrium with a third object C, then A and B are in
More informationKinetic theory. Collective behaviour of large systems Statistical basis for the ideal gas equation Deviations from ideality
Kinetic theory Collective behaviour of large systems Statistical basis for the ideal gas equation Deviations from ideality Learning objectives Describe physical basis for the kinetic theory of gases Describe
More informationChap. 5 GASES & KINETIC- MOLECULAR THEORY
Chap. 5 GASES & KINETIC- OLECULAR THEORY Use the ideal gas law to describe the behavi of gases. Understand how kinetic-molecular they provides the basis f understanding gas behavi Be able to describe effusion
More informationIdeal Gas Behavior. NC State University
Chemistry 331 Lecture 6 Ideal Gas Behavior NC State University Macroscopic variables P, T Pressure is a force per unit area (P= F/A) The force arises from the change in momentum as particles hit an object
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 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 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 informationImperfect Gases. NC State University
Chemistry 431 Lecture 3 Imperfect Gases NC State University The Compression Factor One way to represent the relationship between ideal and real gases is to plot the deviation from ideality as the gas is
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: 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 information