Chemical Thermodynamics : Georg Duesberg
|
|
- Hector Stanley
- 6 years ago
- Views:
Transcription
1 The Properties of Gases Kinetic gas theory Maxwell Boltzman distribution, Collisions Real (non-ideal) gases fugacity, Joule Thomson effect Mixtures of gases Entropy, Chemical Potential Liquid Solutions - Electrolyte activity, Henry s and Raoult s Law Thermodynamics of Mixtures - Colligative Properties
2 Readings Atkins - PC Mortimer PC Pitzer and Brewer Thermodynamics Kittel Kroemer - Thermal Physics 20web/ /teaching.html Or also via my chemistry staff page - link to ASIN page
3 Chapter 1 The Properties of Gases
4 pressure = p = F / A Pressure force area Ar molecules/atoms of gas are constantly in motion
5 Kinetic theory and Gas Laws the pressure of a gas increases when it is compressed at constant temperature? Boyles Law When a gas is compressed at constant temperature, the molecules have less volume to move and hit the wall of the container more frequently. As a result, pressure will increases.
6 Kinetic theory and Gas Laws Boyle s Law pressure volume relationship (temperature is constant) Boyle ( ) p 1/V
7 The volume of a gas increases when heated at constant pressure - Charles Law When a gas is heated, the gas molecules move faster and hit the wall of the container violently. The volume of gas must increase to keep the pressure constant. So that the gas molecules hit the wall less frequently. Kinetic theory and Gas Laws
8 Gay-Lussac s Law (also Charles law) temperature volume relationship (pressure is constant) Gay-Lussac ( ) V T
9 Kinetic theory and Gas Laws ISOTHERMS p 1/V p = const/v => p V = const p 1 V 1 = const p 2 V 2 = const The pressure-volume dependence of a fixed amount of perfect gas at different temperatures. Each curve is a hyperbola (pv = constant) and is called an isotherm. p 1 V 1 = p 2 V 2
10 Kinetic theory and Gas Laws The pressure of a fixed volume of gas increases with temperature. As temperature rises, the molecules move faster The molecules will hit the walls of the container frequently and violently Hence, the pressure increases
11 Isobare V T V = const T V/T = const V 1 / T 1 = const V 2 / T 2 = const The variation of the volume of a fixed amount of gas with the temperature constant. Note that in each case they extrapolate to zero volume at C. V 1 / T 1 = V 2 / T 2
12 Surface of states Isobare and Isotherm Chapter 1 : Slide 12
13 Avogadro s Law 2 H 2 (g) + O 2 (g) 2 H 2 O(l) R = J / mol / K Avogadro ( ) n V n 1 / V 1 = n 2 / V 2 k=1.38x10-23 J/K N A = Avogadro number N k = A R
14 Avogadro principle: Volume of real gases At a given T and p, equal volumes of gases contain the same number of molecules, V m = V/n. Table below presents the molar volumes of selected gases at standard conditions (SATP 25 C and 100kPa) Gas V m /(dm 3 mol 1 ) Perfect gas * Ammonia 24.8 Argon 24.4 Carbon dioxide 24.6 Nitrogen 24.8 Oxygen 24.8 Hydrogen 24.8 Helium 24.8 At STP V m = m 3 /kmol at 0 C and kpa dm 3 mol -1. At IUPAC = m 3 /kmol at 0 C and 100 kpa m3/kmol p V n T 1 1 useful : = 1 1 p n 2 2 V T 2 2
15 IDEAL GAS EQUATION (1) Boyle Law p 1/V (2) Gay-Lussac s Law V T (3) Avogadro s Law n V V 1/p V T V n V T n / p N = nn A p V = const n T p V = k nn A T k=1.38x10-23 J/K p V = R n T R = J / mol / K N k = R A N A = Avogadro number
16 Application: Barometric formula: p as a function of height Consider a column of gas with unit cross sectional area. Variation of pressure with altitude
17 Barometric formula: p as a function of height Boundary condition: ground level pressure is p 0 so that p = p 0 exp(-mgh/rt) An exponential decrease of p with height. Equal Δh's always give the same proportional change in p. Note the assumptions: 1) Ideal gas behavior 2) Constant g 3) Isothermal atmosphere Mgh is the gravitational potential energy. We will often see properties varying in proportion to exp(-e/rt) = exp(-ε/k B T) where E is a form of molar energy (ε is a molecular energy) because these are examples of "Boltzmann distributions". Chapter 1 : Slide 17
18 Barometric Formula As elevation increases, the height of the atmosphere decreases and its pressure decreases. F P = = Write in differential form. dp mg F S = = ρ Vg = ρghs S ρhsg = ρgh = ρ gdh Therefore, density = ρ = mass volume Rewrite PV = nrt as = ρ kg 3 m PM W RT Check units. m x 2 s x m = = kg 2 m moles V n = V m 2 s N = 2 m ( M ) P RT W
19 Continue Derivation of Barometric Formula Substitute the expression for density into the differential eqn. dp = PM RT W g dh Divide both sides of the above equation by P and integrate. dp P MW g = dh RT Integration of the left side and moving the constants outside the integral on the right side of the differential equation gives, MW g MW g ln P = dh = h + RT RT lnc
20 Continue Derivation of Barometric Formula Evaluating the integral between the limits of P 0 at zero height and P h at height h, gives The constant of integration C can be determined from the initial condition P(h = 0) = P 0, where P 0 is the average sea level atmospheric pressure. ln M gh P = W + h RT ln P 0 P h = 0 P e M W RT gh
21 Sample calculation Calculate the pressure on Mount Carrauntoohil (1,038 m) under normal conditions? h = 1082 m Temperature as 25 C T = 298 K P 0 = kpa = 1 bar (760 Torr) m (air) = 29 g/mol (N 2 = 28 amu, O 2 =32 amu) g = 9.81 ms -2 Standard gravity R = J / mol / K p = p 0 exp(-mgh/rt) = 89.5 kpa = 671 Torr 21
22 Height distribution in a gas IG-09 Energy (E = Mgy) being considered is significantly higher than a quanta of energy. E is nearly continuous. Easier to think of probability density functions: (, ;, ;, ) e mgy kt P x x+ dx x y+ dy x z+ dz dxdydz P is the probability of finding a molecule between x & x + dx, y & y + dy and z & z + dz NB: dx, dy and dz are large compared to a molecule but small compared to the size of the system 22
23 ( ) P y Probability density function e mgy kt dxdydz The directions parallel to the ground (x & z) do not contribute to the probability density function; only the height (y) above ground has an influence y dy x dx
24 Height distribution in a gas ( ) P y e mgy kt dxdydz For an ideal gas at constant temperature T, the probability density P(y) is related to the number density (# of molecules N per unit volume V ) n(y) : ( ) n y ( = 0) n y = e mgy kt
25 DALTON S LAW pure gases gas mixtures Dalton (1801) (atmospheres) the total pressure of a gas mixture, p, is the sum of the pressures of the individual gases (partial pressures) at a constant temperature and volume p = p A + p B + p C +.
26 p V = n R T p A = n A R T / V p B = n B R T / V p = p A + p B p = (n A + n B ) R T / V mole fraction x < 1 p A / p = n A /(n A + n B ) = x A p A = x A p n p = Σ p i i=1
27 Dalton s Law Suppose we have two gases in a container: n A moles of gas A and n B moles of gas B. We can define individual partial pressures p A = n A RT/V and p B = n B RT/V. Dalton s Law is that the measured total pressure p is the sum of the partial pressures of all the components: p = p A +p B + = (n A +n B + )RT/V. Mole fractions: define x J for species J as n J /n where n = (n A +n B + ). Then, x A + x B + = 1 and p J = p x J
28 Chapter 2 Kinetic gas theory
29 Kinetic Molecular Theory of Gases macroscopic (gas cylinder) microscopic Maxwell ( ) (atoms/molecules) Boltzmann ( )
30 Kinetic Molecular Theory of Gases Physical properties of gases can be described by motion of individual gas atoms/molecules Assumptions: 1)each macroscopic and microscopic particle in motion holds an kinetic energy according to Newton s law 2)They undergo elastic collisions 3)They are large in number and are randomly distributed 4)They can be treated as points of mass (diameter<< mean free path)
31 Kinetic Molecular Theory of Gases: Assumptions 1)According to Newton's law of action reaction, the force on the wall is equal in magnitude to this value, but oppositely directed. 2.) Elastic collision with wall: v after = -v before - v v Δvelocity Force = mass = Δtime m 2v Δt
32 Kinetic Molecular Theory of Gases: Assumptions 3. Avogardo Number Brownian motion 4. Gases are composed of atoms/molecules which are separated from each other by a distance l much more than their own diameter d d = m L = 10-3 m.. few m molecules are mass points with negligible volume
33 Collisions of the gas molecules with a wall L Small volume, v=la, adjacent to wall where L is less than the mean free path F reaction As a result of a collision with the wall the momentum of a molecule changes by
34 Kinetic Molecular Theory of Gases Pressure = Force total /Area P=F/A F total = F 1 collision x number of collisions in a particular time interval Only molecules within a distance ν x Δt with ν x > 0 can reach the wall on the right in an interval Δt. L = v x Δ t Assume that in a time Δt every molecule (atom) in the original volume, v=la, within the range of velocities will collide with the wall.
35 Collisions of the gas molecules with a wall This means that Δt is given by: The reaction force of a molecule on the wall is the negative of the average rate of change in the momentum of gas molecules in the volume v that collide with the wall in the time Δt. The total force on the wall is the sum of the average rate of momentum change for all molecules in the volume v=la that collide with the wall Here we have divided by 2 since only ½ of the molecules in our volume have a positive velocity toward the wall
36 Collisions of the gas molecules with a wall (cont.) We do the sum by noting that the total number of molecules in the volume v is (N/ V) v=la N/ V = density L Remembering Pascal s law dividing by A yields the pressure everywhere. P = F A
37 Kinetic theory: go from 1 to 3 dimensions L Velocity squared of a molecule: 2 2 x 2 y v = v + v + v 2 z The average of a sum is equal to the sum of averages All the directions of motion (x, y, z) are equally probable. Remember homogeneous and isotropic! Equipartition principle
38 Kinetic theory Combing these results yields From the ideal gas law And with c = <v> v 2 = c = 3kT 2 = 3kT 2m m Relation between the absolute temperature and average kinetic energy of a molecule.
39 Kinetic theory v rms of a molecule is thermal speed : The absolute temperature is a measure of the average kinetic energy of a molecule. Example: What is the thermal speed of hydrogen molecules at 800K?
Properties 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 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 informationChapter 17 Temperature & Kinetic Theory of Gases 1. Thermal Equilibrium and Temperature
Chapter 17 Temperature & Kinetic Theory of Gases 1. Thermal Equilibrium and Temperature Any physical property that changes with temperature is called a thermometric property and can be used to measure
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 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 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. 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 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 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 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 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 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 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 informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 11 The Gaseous State by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 11 1 Properties of Gases
More 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 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 informationPV = n R T = N k T. Measured from Vacuum = 0 Gauge Pressure = Vacuum - Atmospheric Atmospheric = 14.7 lbs/sq in = 10 5 N/m
PV = n R T = N k T P is the Absolute pressure Measured from Vacuum = 0 Gauge Pressure = Vacuum - Atmospheric Atmospheric = 14.7 lbs/sq in = 10 5 N/m V is the volume of the system in m 3 often the system
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 informationThe Gas Laws. Section 1.2 (7th and 8th editions) Individual Gases Boyle s Law Charles Law. Perfect (Ideal) Gas Equation
The Gas Laws Section 1.2 (7th and 8th editions) Individual Gases Boyle s Law Charles Law Perfect (Ideal) Gas Equation Mixtures of Gases Dalton s Law Mole Fractions Last updated: Sept. 14, 2009; minor edits
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 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 information(2) The volume of molecules is negligible in comparison to the volume of gas. (3) Molecules of a gas moves randomly in all direction.
9.1 Kinetic Theory of Gases : Assumption (1) The molecules of a gas are identical, spherical and perfectly elastic point masses. (2) The volume of molecules is negligible in comparison to the volume of
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 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 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 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 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 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 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 informationHomework: 13, 14, 18, 20, 24 (p )
Homework: 13, 14, 18, 0, 4 (p. 531-53) 13. A sample of an ideal gas is taken through the cyclic process abca shown in the figure below; at point a, T=00 K. (a) How many moles of gas are in the sample?
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 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 informationנושא 6 גזים. 1 Prof. Zvi C. Koren
נושא 6 גזים 1 Prof. Zvi C. Koren Torricelli Charles Avogadro Graham Dalton Boyle Gay-Lussac Kelvin Maxwell Boltzmann 2 Prof. Zvi C. Koren Gas Laws: A Practical Application - Air Bags Example: An automobile
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 informationPhysics 231 Topic 12: Temperature, Thermal Expansion, and Ideal Gases Alex Brown Nov
Physics 231 Topic 12: Temperature, Thermal Expansion, and Ideal Gases Alex Brown Nov 18-23 2015 MSU Physics 231 Fall 2015 1 homework 3 rd midterm final Thursday 8-10 pm makeup Friday final 9-11 am MSU
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 informationCHEMISTRY XL-14A GASES. August 6, 2011 Robert Iafe
CHEMISTRY XL-14A GASES August 6, 2011 Robert Iafe Chemistry in the News 2 Polymer nicotine trap is composed of a porphyrin derivative (black), in which amide pincers (green) are attached to the zinc (violet)
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 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 informationGases. Petrucci, Harwood and Herring: Chapter 6
Gases Petrucci, Harwood and Herring: Chapter 6 CHEM 1000 3.0 Gases 1 We will be looking at Macroscopic and Microscopic properties: Macroscopic Properties of bulk gases Observable Pressure, volume, mass,
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 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 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 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 informationTOPIC 2. Topic 2. States of Matter (I) - Gases. 1
Chemistry TOPIC 2 States of Matter (I) - Gases Topic 2. States of Matter (I) - Gases. 1 Contents 1. Introduction 2. Pressure measurement 3. The Ideal Gas equation 4. Efusion and Diffusion 5. Kinetic Molecular
More informationPhysics 2 week 7. Chapter 3 The Kinetic Theory of Gases
Physics week 7 Chapter 3 The Kinetic Theory of Gases 3.1. Ideal Gases 3.1.1. Experimental Laws and the Equation of State 3.1.. Molecular Model of an Ideal Gas 3.. Mean Free Path 3.3. The Boltzmann Distribution
More informationPhysics 4C Chapter 19: The Kinetic Theory of Gases
Physics 4C Chapter 19: The Kinetic Theory of Gases Whether you think you can or think you can t, you re usually right. Henry Ford The only thing in life that is achieved without effort is failure. Source
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 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 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 information--Lord Kelvin, May 3rd, 1883
When you can measure what you are speaking about and express it in numbers, you know something about it; but when you cannot measure it, when you cannot express it in numbers, you knowledge is of a meager
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 informationPHYSICS - CLUTCH CH 19: KINETIC THEORY OF IDEAL GASSES.
!! www.clutchprep.com CONCEPT: ATOMIC VIEW OF AN IDEAL GAS Remember! A gas is a type of fluid whose volume can change to fill a container - What makes a gas ideal? An IDEAL GAS is a gas whose particles
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 1. The Properties of Gases Fall Semester Physical Chemistry 1 (CHM2201)
Chapter 1. The Properties of Gases 2011 Fall Semester Physical Chemistry 1 (CHM2201) 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
More informationRate of Heating and Cooling
Rate of Heating and Cooling 35 T [ o C] Example: Heating and cooling of Water E 30 Cooling S 25 Heating exponential decay 20 0 100 200 300 400 t [sec] Newton s Law of Cooling T S > T E : System S cools
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 information14 The IDEAL GAS LAW. and KINETIC THEORY Molecular Mass, The Mole, and Avogadro s Number. Atomic Masses
14 The IDEAL GAS LAW and KINETIC THEORY 14.1 Molecular Mass, The Mole, and Avogadro s Number Atomic Masses The SI Unit of mass: An atomic mass unit is de ned as a unit of mass equal to 1/12 of the mass
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 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 informationATMOS Lecture 3
ATMOS 5130 Lecture 3 Physical Properties of Air Introduction to Kinetic Theory of Gases Boyle s Law Charles Law Avogadro's Law Definition of a Mole and Molecular Weight Ideal Gas Law Kinetic Theory of
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 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 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 informationChapter 10. Thermal Physics. Thermodynamic Quantities: Volume V and Mass Density ρ Pressure P Temperature T: Zeroth Law of Thermodynamics
Chapter 10 Thermal Physics Thermodynamic Quantities: Volume V and Mass Density ρ Pressure P Temperature T: Zeroth Law of Thermodynamics Temperature Scales Thermal Expansion of Solids and Liquids Ideal
More informationKINETIC THEORY OF GASES
KINETIC THEORY OF GASES VERY SHORT ANSWER TYPE QUESTIONS ( MARK). Write two condition when real gases obey the ideal gas equation ( nrt). n number of mole.. If the number of molecule in a container is
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 informationChapter 11. Preview. Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures
Preview Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures Section 1 Gases and Pressure Lesson Starter Make a list of gases you already know about. Separate your list into elements,
More informationε tran ε tran = nrt = 2 3 N ε tran = 2 3 nn A ε tran nn A nr ε tran = 2 N A i.e. T = R ε tran = 2
F1 (a) Since the ideal gas equation of state is PV = nrt, we can equate the right-hand sides of both these equations (i.e. with PV = 2 3 N ε tran )and write: nrt = 2 3 N ε tran = 2 3 nn A ε tran i.e. T
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 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 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 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 informationPhysics 231 Lecture 30. Main points of today s lecture: Ideal gas law:
Physics 231 Lecture 30 Main points of today s lecture: Ideal gas law: PV = nrt = Nk BT 2 N 1 2 N 3 3 V 2 3 V 2 2 P = m v = KE ; KE KE = kbt Phases of Matter Slide 12-16 Ideal Gas: properties Approximate
More informationChapter 5. The Properties of Gases. Gases and Their Properties. Why Study Gases? Gas Pressure. some very common elements exist in a gaseous state
Chapter 5 Gases and Their Properties Why Study Gases? some very common elements exist in a gaseous state our gaseous atmosphere provides one means of transferring energy and material throughout the globe
More informationWeb Resource: Ideal Gas Simulation. Kinetic Theory of Gases. Ideal Gas. Ideal Gas Assumptions
Web Resource: Ideal Gas Simulation Kinetic Theory of Gases Physics Enhancement Programme Dr. M.H. CHAN, HKBU Link: http://highered.mheducation.com/olcweb/cgi/pluginpop.cgi?it=swf::00%5::00%5::/sites/dl/free/003654666/7354/ideal_na.swf::ideal%0gas%0law%0simulation
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 informationKinetic theory of the ideal gas
Appendix H Kinetic theory of the ideal gas This Appendix contains sketchy notes, summarizing the main results of elementary kinetic theory. The students who are not familiar with these topics should refer
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 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 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 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 informationImportance of Gases Airbags fill with N gas in an accident. Gas is generated by the decomposition of sodium azide, NaN.
Gas Laws Importance of Gases Airbags fill with N 2 gas in an accident. Gas is generated by the decomposition of sodium azide, NaN 3. 2 NaN 3 (s) 2 Na (s) + 3 N 2 (g) 2 Importance of Gases C 6 H 12 O 6
More 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 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 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 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 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 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 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 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 informationSpeed Distribution at CONSTANT Temperature is given by the Maxwell Boltzmann Speed Distribution
Temperature ~ Average KE of each particle Particles have different speeds Gas Particles are in constant RANDOM motion Average KE of each particle is: 3/2 kt Pressure is due to momentum transfer Speed Distribution
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 informationModule 5: Rise and Fall of the Clockwork Universe. You should be able to demonstrate and show your understanding of:
OCR B Physics H557 Module 5: Rise and Fall of the Clockwork Universe You should be able to demonstrate and show your understanding of: 5.2: Matter Particle model: A gas consists of many very small, rapidly
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 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 informationKINETIC THEORY OF GASES
LECTURE 8 KINETIC THEORY OF GASES Text Sections 0.4, 0.5, 0.6, 0.7 Sample Problems 0.4 Suggested Questions Suggested Problems Summary None 45P, 55P Molecular model for pressure Root mean square (RMS) speed
More information10 TEMPERATURE, THERMAL EXPANSION, IDEAL GAS LAW, AND KINETIC THEORY OF GASES.
10 TEMPERATURE, THERMAL EXPANSION, IDEAL GAS LAW, AND KINETIC THEORY OF GASES. Key words: Atoms, Molecules, Atomic Theory of Matter, Molecular Mass, Solids, Liquids, and Gases, Thermodynamics, State Variables,
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 informationBoyle s law states the relationship between the pressure and the volume of a sample of gas.
The Ideal Gas Law Boyle s law states the relationship between the pressure and the volume of a sample of gas. Charles s law states the relationship between the volume and the absolute temperature of a
More information