Chapter 5: Phenomena. Chapter 5: Gases. Molar Mass. Volume (L) Amount (mol) Pressure (atm) Temperature ( C) Odor
|
|
- Brianna Lester
- 5 years ago
- Views:
Transcription
1 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 gases. Use these patterns to fill in the information for the mystery gas. Gas Color Amount (mol) Volume (L) Molar Mass g mol Pressure (atm) Odor Temperature ( C) Cl 2 Yellow Bleach Like 25 C Cl 2 Yellow Bleach Like 25 C CH 4 Colorless Odorless 25 C CH 4 Colorless Odorless 25 C NH 3 Colorless Feline Urine 25 C NH 3 Colorless Feline Urine 25 C NO 2 Brown Pungent 25 C NO 2 Brown Pungent 25 C Xe Colorless Odorless 25 C Xe Colorless Odorless 919 C Mystery C Mystery C
2 Big Idea: The pressure, volume, number of moles, and temperature are needed to classify a gas. Knowing 3 of these quantities allows us to calculate the forth, using the ideal gas law. Generally these properties are independent of gas type. The ideal gas laws can be explained using a model of a gas in which the molecules are in ceaseless random motion and widely spread out. Chapter 5 Gases Properties of Gases Pressure Ideal Gas Law Other Equations of States Gas Stoichiometry Dalton s Law of Partial Pressures The Kinetic Model of Gases Effusion and Diffusion 2
3 Properties of Gases Eleven elements are gases under standard conditions. In addition, many compounds with low molar masses (HCl, CH 4, C 3 H 8 ) are also gases under standard conditions. Note: All elements that are gases at room temperature temperatures are diatomic with the exception of the 6 noble gases, which are monatomic. 3
4 Properties of Gases Bulk Matter: Forms of matter consisting of large numbers of molecules. The properties of a gas sample emerge from the collective behavior of vast numbers of its individual particles. Properties of Gases Compressible. Fill up the space that is available (this implies that the molecules are moving quickly in a chaotic motion). 4
5 Pressure 5 A barometer is used to measure the pressure of the atmosphere. The pressure of the atmosphere is balanced by the pressure exerted by the column of mercury. The height of the column is proportional to the atmospheric pressure. Therefore, by measuring the height of the column, we can monitor the pressure of the atmosphere. P=dhg
6 Pressure 6 (a) An open-tube manometer. The pressure inside the apparatus to which the narrow horizontal tube is connected pushes against the external pressure. In this instance, the pressure inside the system is lower than the atmospheric pressure by an amount proportional to the difference in heights of the liquid in the two arms. (b) The pressure in the adjoining apparatus is proportional to the difference in heights of the liquid in the two arms. The space inside the closed end is a vacuum.
7 Pressure Common Units of Pressure Units Pa* mm Hg Torr psi in Hg Conversion to atm Pa = 1 atm 760 mm Hg = 1 atm 760 torr = 1 atm 14.7 psi = 1 atm in Hg = 1 atm *The SI derived unit of pressure is Pa. 7
8 Ideal Gas Law Temperature and Moles Constant Boyle s Law: For a fixed amount of gas under constant temperature, the volume is inversely proportional to pressure. Mathematically Volume α 1 Pressure PV = constant P I V I = P F V F Note: A change that occurs at constant temperature is referred to as an isothermal change. 8
9 Ideal Gas Law Pressure and Moles Constant Charles s Law: For a fixed amount of gas under constant pressure, the volume varies linearly with the temperature. Mathematically Volume α Temperature V = constant T V I T I = V F T F Note: A change that occurs at constant pressure is referred to as an isobaric change. 9
10 Ideal Gas Law Temperature Conversions Units Kelvin (K)* Conversion to Kelvin T K Celsius ( C) T K = T C Fahrenheit ( F) T K = 5 9 T F *SI unit Note: Temperature conversions involve both multiplication/division and addition/subtraction, therefore, be very careful when using a unit other than Kelvin. 10
11 Ideal Gas Law A balloon containing 1.0 L of air at 25 C is put in liquid nitrogen which is at a temperature of -196 C. What is the final volume of the balloon? 11
12 Ideal Gas Law Implications of Charles s Law 12
13 Ideal Gas Law Pressure and Temperature Constant Avogadro s Law: At constant pressure and temperature, the volume of a gas varies linearly with the number of moles. Mathematically Volume α Number of Moles V = constant n V I n I = V F n F 13
14 Ideal Gas Law Ideal Gas Law PV=nRT Boyle s, Charles's, and Avogadro s Law are just special cases of ideal gas law Boyle s Law Charles s Law Avogadro s Law PV = C B V = C c T V = nc A C B = nrt C C = nr P C A = TR P 14
15 Ideal Gas Law How do they get R? Three pistons all with different gases. (P = 1 atm, T = K, n = 1 mol) He N 2 O 2 R= Ideal Gas Constant L atm (P(atm),V(L), n(mol) and T(K)) mol K V He =V N2 =V O2 =24.5L J mol K (P(Pa),V(m3 ), n(mol) and T(K)) 15
16 Ideal Gas Law Student Question What is the volume (in L) occupied by 35.2 g of nitrogen gas at 35 C and atm? Helpful Information: M N = g mol a) 26.8 L b) 18.7 L c) 21.8 L d) 32.6 L e) None of the above 16
17 Ideal Gas Law 17
18 Other Equations of State Equation of State: A mathematical expression relating the pressure, volume, temperature, and amount of substance present in a sample. Note: The ideal gas law is an example of an equation of state. Limiting Law: A law that is accurately obeyed only at the limit of a property, which is when a property (the pressure of a gas, for example) is made very small. Note: The ideal gas law is a limiting law. 18
19 Other Equations of State A common procedure in chemistry to improve the ideal gas law is to suppose that the terms on the right-hand side of an equation (such as nrt in PV=nRT of the ideal gas law) are just the leading (and predominant) term of a more complicated expression. Virial Equation: PV = nrt 1 + B V m + C V m 2 + B,C, are called the second virial coefficient, third virial coefficient and so on. The virial coefficients are found by fitting experimental data and are temperature dependent. 19
20 Other Equations of State Gas a atm L2 mol 2 b L mol He Ne Ar Kr Xe H N O Cl CO CH Parameter a corrects for attractions (intermolecular forces) between particles; particles with strong intermolecular forces (large molecules with many electrons)have larger a values. Parameter b corrects for the size of the particle; it can be thought of as representing the volume of an individual molecule. 20
21 Dalton s Law of Partial Pressure Dalton wondered if he had a certain amount of oxygen in a container that has a pressure of 0.60 atm and he had another container of the same size of nitrogen that had a pressure of 0.40 atm, if he combined the two gases in a third container of the same size, what the pressure would be. He found that the pressure would be 1.00 atm. 21
22 Dalton s Law of Partial Pressure Partial Pressure (P x ): The pressure that a gas (X) in a mixture would exert if it alone occupied the container. Law of Partial Pressures: The total pressure of gases is the sum of the partial pressures of its components. P tot = P A + P B + Mole Fraction (χ): The amount of particles (molecules, atoms, or ions) of a substance in a mixture expressed as a fraction of the total amount of particles in the mixture. χ A = n A n tot = n A n A + n B + 22
23 The Kinetic Model of Gases Assumptions Made for the Kinetic Model of Gases 1) The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be negligible (zero). 2) The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas. 3) The particles are assumed to exert no forces on each other; they are assumed to neither attract nor repel each other. 4) The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas. 23
24 The Kinetic Model of Gases Purpose: Want to show that ideal gas law and kinetic model of gases are consistent with each other PV n T Calculate the Pressure in a Rectangular Prism (Kinetic Model) 1) P = F A F= Force, A=Area 2) F = p t (Newton's second law) p=momentum (p = mu u=velocity) z y x A x = Area of a side on x A y = Area of a side on y A z = Area of a side on z 24
25 The Kinetic Model of Gases Goal: Calculate Change in Momentum 3) Calculate of Δp of 1 molecule hitting 1 of the walls. p before hits wall p x = mu x p after hits wall p x = m u x Change in p p x = m u x mu x = 2mu x 4) Calculate p for multiple molecules (traveling at the same speed) p xtot = N col p x = N col 2mu x N col = number of molecules that collide with wall 25
26 The Kinetic Model of Gases Goal: Calculate Change in Momentum 5) How many molecules collide with wall in time period Δt? Kinetic Model: particles in random motion, therefore, roughly evenly distributed N pos = V pos V tot N tot N pos = number of molecules that could hit wall V pos = the volume that those particles are in V tot = total volume of rectangular prism N tot = total number of molecules Note: V tot is the same volume used in the ideal gas law but we need to find expressions for the rest of the variables. 26
27 The Kinetic Model of Gases Goal: Calculate Change in Momentum 6) What is the volume in which particles have the potential of hitting the wall (V pos ) x max = u x t x max = max distance away from wall and still collide with side V pos = A x x max = A x u x t 27 7) Plug expression into N pos N pos = V pos N V tot = A xu x t N tot V tot tot Problem: Half of the molecules in that area are moving toward the wall and half are moving away. N col = N pos 2 = A xu x a t N tot 2V tot
28 The Kinetic Model of Gases Goal: Calculate Change in Momentum 8) Plug N col into Δp tot p xtot = N col 2mu x = A xu x t N 2V tot 2mu x = A xmu 2 x t tot V tot N tot Goal: Calculate Force 9) Calculate force on 1 side of rectangle prism F x = p t = A x mu x 2 t V tot t N tot = A xmu x 2 V tot N tot Note: When we originally calculated the change in momentum it was with respect to the molecules. When we calculate the force, we need the change in momentum with respect to the wall, therefore, the sign must be flipped. 28
29 The Kinetic Model of Gases Goal: Calculate Pressure 10) Calculate pressure on 1 side of the rectangular prism P x = F x A x = A x mu x 2 N V tot tot A x = mu 2 x N V tot tot 11) Remove requirement that all molecules are traveling at the same speed. 2 P x(rms) = mu x(rms) V tot N tot Note: A line over a variable represents the average value. 29
30 The Kinetic Model of Gases Goal: Calculate Pressure 12) Calculate P tot Note: The pressure inside the container is constant. P tot = P x(rms) = mu 2 x(rms) V tot N tot 12) Change to overall velocity instead of velocity in x u2 2 rms = u x(rms) 2 u x(rms) 2 = u y(rms) 2 2 u rms = 3u x(rms) 2 + u y(rms) 2 = u z(rms) 2 + u z(rms) P tot = mu x 2 N V tot = m1 3 tot u2 rms V tot N tot 30
31 The Kinetic Model of Gases Goal: Calculate Pressure 14) Change to number of moles n tot N A = N tot N A = Avogadro s Constant P tot = mu 2 rms N 3V tot = mu 2 rms n tot 3V tot N A = n totmu rms tot 3V tot 2 N A 31
32 The Kinetic Model of Gases Goal: Calculate Pressure 15) Kinetic Model: The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas. KE ave = 1 2 mu2 T P tot = n 2 totmu rms N A 3V tot n tott V tot Note: The variables boxed in green are proportional to the kinetic energy and the variables boxed in red are constants. Ideal Gas Law P tot n tott V tot Kinetic Theory P tot n tott V tot 32
33 The Kinetic Model of Gases Maxwell Distribution ( N = Nf u u) ΔN = Number of molecules with a speeds in the narrow range between u and u+ ΔU f u = 4π M 2πRT Τ 3 2 u 2 e Τ Mu 2 2RT f(u) = Maxwell distribution of speeds James Clerk Maxwell Wrote the equations that unified electricity, magnetism, and optics. 33
34 The Kinetic Model of Gases The heavier the atom, the slower the average speed and the closer the speeds are to the average speed. As the temperature increases, the average speed increases and the spread of speeds widens. 34
35 The Kinetic Model of Gases Most Probable Velocity (u mp ) df u du u mp = = 0 solve for u 2RT M Average Velocity (u ave ) u ave = തu = 0 uf u du u ave = 8RT πm Root Mean Square Velocity (u rms ) u rms = 0 u 2 f u du u rms = 3RT M 35
36 The Kinetic Model of Gases Student Question Consider three 1.0-L flasks at STP. Flask A contains He gas, flask B contains O 2 gas, and flask C contains H 2 gas. In which flask do the gas particles have the lowest average kinetic energy? a) Flask A b) Flask B c) Flask C d) All are the same. 36
37 Effusion and Diffusion Diffusion: The spreading of one substance through another substance. Effusion: The escape of a substance (particularly a gas) through a small hole. Graham s Law of Effusion: At constant temperature, the rate of effusion of a gas is inversely proportional to the square root of its molar mass. Note: This law was determined experimentally. 37
38 Effusion and Diffusion Determining the relationship between rates of effusion of different substances. Rate effusiona = C 1 M A Rate effusionb = C 1 M B Divide the two quantities by each other. Rate effusiona Rate effusionb = C 1 M A Rate effusiona C 1 = Rate effusionb M B M B M A Note: rate = particles time 38
39 Effusion and Diffusion Student Question A sample of an unknown gas effuses in 8.2 minutes. An equal volume of krypton in the same apparatus at the same temperature and pressure effuses in 4.0 minutes. What is the likely identity of the gas? Helpful Information: M Kr = g mol, M Ar = g, mol M UF6 = g, M mol Ne = g, and M mol Br 2 = g mol a) UF 6 b) Br 2 c) Ar d) Ne e) None of the Above 39
40 Effusion and Diffusion NH 3 (g) +HCl(g) NH 4 Cl(s) Notice that the ammonium chloride initially forms closer to the end with HCl. 40
41 Take Away From Chapter 5 Big Idea: The pressure, volume, number of moles, and temperature are needed to classify a gas. Knowing 3 of these quantities allows us to calculate the forth by using the ideal gas law. Generally these properties are independent of gas type. The ideal gas law can be explained using a model of a gas in which the molecules are in ceaseless random motion and widely spread out. Properties of Gases Pressure (22) Know how to convert between different pressure units. Know the conditions of STP (1 atm and 0 C) and SATP (1 atm and 25 C). 41 Numbers correspond to end of chapter questions.
42 Take Away From Chapter 5 Ideal Gas Law Know how to use : Boyle s Law P 1 V 1 = P 2 V 2 Charles's Law V I T I = V F T F (41) Avogadro s Law V I n I = V F n F (42) 42 Ideal gas Law PV = nrt (11,33,34,36,37,40,43,55,56) Know the condition in which the ideal gas law is a good approximation. (93) Other Equations of State Know the advantages and disadvantages of the Virial equation. Know how to use the Van der Waal equation and what the Van der Waal constants correct for. (91,92) Gas Stoichiometry (8) Be able to use the gas laws to perform stoichiometry problems. (60,62,65,66,73,119) Numbers correspond to end of chapter questions.
43 Take Away From Chapter 5 Dalton s Law of Partial Pressure Be able to calculate the partial pressures of gases. (29,46,49,127) P A = χ A P tot P tot = P A + P B + The Kinetic Model of Gases Know what assumptions are made for kinetic model of gases. Know the relationship between kinetic energy, temperature, and velocity.(79,80) KE ave = 3 RT (81) 2 Know how the shape of the Maxwell distribution of speeds changes with mass and temperature. (94) Know the difference and how to calculate u rms, u mp, and u ave. (82,83,86,99) u rms = 2RT u M mp = 2RT u M ave = 8RT πm 43 Numbers correspond to end of chapter questions.
44 Take Away From Chapter 5 Effusion and Diffusion Know the difference between effusion and diffusion Be able to use the effusion equation: (89,90) Rate A Rate B = M B M A time for B to effuse time for A to effuse = M B M A The time equation only works if the number of particles that effused are the same Be able to use the diffusion equation: d A d B = M B M A 44 Numbers correspond to end of chapter questions.
Chapter 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 informationChapter 10 Notes: Gases
Chapter 10 Notes: Gases Watch Bozeman Videos & other videos on my website for additional help: Big Idea 2: Gases 10.1 Characteristics of Gases Read p. 398-401. Answer the Study Guide questions 1. Earth
More informationGases. 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 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 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 information10/15/2015. 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 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 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 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 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 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 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 11 Gases 1 Copyright McGraw-Hill 2009
Chapter 11 Gases Copyright McGraw-Hill 2009 1 11.1 Properties of Gases The properties of a gas are almost independent of its identity. (Gas molecules behave as if no other molecules are present.) Compressible
More informationChapter 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 informationAlthough different gasses may differ widely in their chemical properties, they share many physical properties
IV. Gases (text Chapter 9) A. Overview of Chapter 9 B. Properties of gases 1. Ideal gas law 2. Dalton s law of partial pressures, etc. C. Kinetic Theory 1. Particulate model of gases. 2. Temperature and
More informationChapter 10. Gases. 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 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 informationAP Chemistry Ch 5 Gases
AP Chemistry Ch 5 Gases Barometer - invented by Evangelista Torricelli in 1643; uses the height of a column of mercury to measure gas pressure (especially atmospheric) Manometer- a device for measuring
More informationChapter 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 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 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 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 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 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 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 informationGases. Characteristics of Gases. Unlike liquids and solids, gases
Gases Characteristics of Gases Unlike liquids and solids, gases expand to fill their containers; are highly compressible; have extremely low densities. 1 Pressure Pressure is the amount of force applied
More informationChapter 5 The Gaseous State
Chapter 5 The Gaseous State Contents and Concepts Gas Laws We will investigate the quantitative relationships that describe the behavior of gases. 1. Gas Pressure and Its Measurement 2. Empirical Gas Laws
More 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 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 informationSlide 1 / A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m 2 A 55 B 0.55 C 5.5 D 1.8 E 18
Slide 1 / 76 1 A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m 2 A 55 B 0.55 C 5.5 D 1.8 E 18 Slide 2 / 76 2 A pressure of 1.00 atm is the same as a pressure of of mm Hg. A 193 B
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 informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 5 GASES INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 5 GASES 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 5 GASES Properties of Gases Pressure History and Application of the Gas Laws Partial Pressure Stoichiometry of
More informationAP Chemistry 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 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 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 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 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 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 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 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 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 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 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 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 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 informationProperties of Gases. assume the volume and shape of their containers. most compressible of the states of matter
Gases Properties of Gases assume the volume and shape of their containers most compressible of the states of matter mix evenly and completely with other gases much lower density than other forms of matter
More 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 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 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 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. 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 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 information7/16/2012. Characteristics of Gases. Chapter Five: Pressure is equal to force/unit area. Manometer. Gas Law Variables. Pressure-Volume Relationship
7/6/0 Chapter Five: GASES Characteristics of Gases Uniformly fills any container. Mixes completely with any other gas. Exerts pressure on its surroundings. When subjected to pressure, its volume decreases.
More informationSubstances that Exist as Gases
Gases Properties of Gases assume the volume and shape of their containers most compressible of the states of matter mix evenly and completely with other gases much lower density than other forms of matter
More 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 informationD g << D R < D s. Chapter 10 Gases & Kinetic Molecular Theory. I) Gases, Liquids, Solids Gases Liquids Solids. Particles far apart
Chapter 10 Gases & Kinetic Molecular Theory I) Gases, Liquids, Solids Gases Liquids Solids Particles far apart Particles touching Particles closely packed very compressible slightly comp. Incomp. D g
More informationChapter 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 informationGases. Chapter 5. Elements that exist as gases at 25 0 C and 1 atmosphere
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 1 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 informationForces between atoms/molecules
Professor K gases Forces between atoms/molecules BONDS are the INTRAMOLECULAR FORCES holding the atoms in molecules together... What holds the molecules of a solid or liquid together?... INTERMOLECULAR
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 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 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 informationUnit 8 Kinetic Theory of Gases. Chapter 13-14
Unit 8 Kinetic Theory of Gases Chapter 13-14 This tutorial is designed to help students understand scientific measurements. Objectives for this unit appear on the next slide. Each objective is linked to
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 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 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 informationMixture of gases. Mix 5 moles of CO 2 V = 40L 2 moles of N 2 T = 0 C 1 mole of Cl 2 What is P? Mary J. Bojan Chem 110
Mixture of gases Mix 5 moles of CO 2 V = 40L 2 moles of N 2 T = 0 C 1 mole of Cl 2 What is P? 1 Partial Pressure Partial pressure: the pressure a gas would have if it was the only gas in the container.
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 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 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 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 informationChapter 5. Gases and the Kinetic-Molecular Theory
Chapter 5 Gases and the Kinetic-Molecular Theory Macroscopic vs. Microscopic Representation Kinetic Molecular Theory of Gases 1. Gas molecules are in constant motion in random directions. Collisions among
More informationGases 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 informationGas Density. Standard T & P (STP) 10/29/2011. At STP, 1 mol of any ideal gas occupies 22.4 L. T = 273 K (0 o C) P = 1 atm = kpa = 1.
Standard T & P (STP) T = 73 K (0 o C) P = 1 atm = 101.35 kpa = 1.0135 bar At STP, 1 mol of any ideal gas occupies.4 L.4 L Gas Density We can use PV = nrt to determine the density of gases. What are the
More informationThe Gaseous State. 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 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 informationProperties of Gases. Occupy the entire volume of their container Compressible Flow readily and mix easily Have low densities, low molecular weight
Chapter 5 Gases Properties of Gases Occupy the entire volume of their container Compressible Flow readily and mix easily Have low densities, low molecular weight Atmospheric Pressure Atmospheric pressure
More 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 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 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 informationChemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten; Catherine J.
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten; Catherine J. Murphy Chapter 10 Gases Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry
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 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 informationStates of Matter Lesson 3.6 CHEMISTRY 2 HONORS. Jeff Venables Northwestern High School
States of Matter Lesson 3.6 CHEMISTRY HONORS Molecular Effusion and Diffusion As kinetic energy increases, the velocity of the gas molecules increases. Average kinetic energy of a gas is related to its
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 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 information= mol NO 2 1 mol Cu Now we use the ideal gas law: atm V = mol L atm/mol K 304 K
CHEM 101A ARMSTRONG SOLUTIONS TO TOPIC C PROBLEMS 1) This problem is a straightforward application of the combined gas law. In this case, the temperature remains the same, so we can eliminate it from the
More informationChapter 11. Preview. Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures
Preview Lesson Starter Objectives Pressure and Force Dalton s Law of Partial Pressures Section 1 Gases and Pressure Lesson Starter Make a list of gases you already know about. Separate your list into elements,
More 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 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 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 informationChapter 10. Gases. Lecture Outline Characteristics of Gases 1, 10.2 Pressure. Atmospheric Pressure and the Barometer 3, 4, 5, 6,
1 Chapter 10. Lecture Outline 10.1 Characteristics of 1, 2 All substances have three phases: solid, liquid and gas. Substances that are liquids or solids under ordinary conditions may also exist as gases.
More 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 informationChapter 10. Gases. Characteristics of Gases. Units of Pressure. Pressure. Manometer. Units of Pressure 27/07/2014 P = F A
7/07/014 Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Characteristics of Chapter 10 Unlike liquids and solids, gases expand to fill their containers;
More information1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of. 2) A gas at a pressure of 325 torr exerts a force of N on an area of
10.1 Multiple-Choice and Bimodal Questions 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of A) 55 B) 0.55 C) 5.5 D) 1.8 E) 18 5.5 m. Answer: A Diff: Page Ref: Sec. 10. ) A gas at a pressure
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 informationOUTLINE. States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry
UNIT 6 GASES OUTLINE States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry STATES OF MATTER Remember that all matter exists in three physical states: Solid Liquid
More 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 informationThe Kinetic Molecular Theory of Gases
The Kinetic Molecular Theory of Gases Background: It is straightforward to observe that there is an inverse relationship between pressure and volume for a gas at constant temperature. Curious scientists
More information