1 Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Gases
3 A Gas Has neither a definite volume nor shape. Uniformly fills any container. Mixes completely with any other gas Exerts pressure on its surroundings.
4 Earth-like Atmosphere Composition of Earth s Atmosphere Compound %(Volume) Mole Fraction a Nitrogen Oxygen Argon Carbon dioxide Methane 2 x x 10-6 Hydrogen 5 x x 10-7 a. mole fraction = mol component/total mol in mixture.
5 Pressure Pressure is the amount of force applied to an area. P = F A Atmospheric pressure is the weight of air per unit of area.
6 Elevation and Atmospheric Pressure
7 Pressure is equal to force/unit area SI units = Newton/meter 2 = 1 Pascal (Pa) 1 standard atmosphere = 101,325 Pa (100,000 Pa = 1 bar) 1 standard atmosphere = 1 atm = 760 mm Hg = 760 torr = hpa = psi Meteorologists often report pressure in millibar; 1 mbar =0.001bar =0.1 kpa = 1hPa
8 The barometric pressure reported for Butte by the weather service was P b = 1018 hpa. What is this pressure in Torr, Atm, and Bar?
9 Units of Pressure mm Hg or torr These units are literally the difference in the heights measured in mm (h) of two connected columns of mercury. Atmosphere 1 atm = 760 torr = kpa = 14.7 lb/in 2
10 Manometer This device is used to measure the difference in pressure between atmospheric pressure and that of a gas in a vessel.
11 Variables Affecting Gases Pressure (P) Volume (V) Temperature (T) Number of Moles (n)
12 Boyle s Law The volume of a fixed quantity of gas at constant temperature is inversely proportional to the pressure.
13 Boyle Law pressure is inversely proportional to volume (at constant T and moles, n).
14 As P and V are inversely proportional A plot of V versus P results in a curve. Since PV = k V = k (1/P) This means a plot of V versus 1/P will be a straight line.
15 Boyle s Law P 1/V (T and n fixed) P V = Constant P 1 V 1 = P 2 V 2
16 Problem. The volume of 1.00 mol of ammonia gas at 1.00 atm of pressure is gradually decreased from 78.0 ml to 39.0 ml. What is the final pressure of ammonia if there is no change in temperature? ans. = 2.00 atm
17 Charles s Law The volume of a gas is directly proportional to Kelvin temperature, and extrapolates to zero at zero Kelvin. V T (P & n are constant) V 1 = V 2 T 1 T 2
18 Problem. A 5.6 L sample of gas is cooled from 78 C to a temperature at which its volume is 4.3 L. What is this new temperature? Assume no change in pressure of the gas. ans. = K
19 The temperature in the troposphere is also proportional to pressure.
20 Avogadro s Law For a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas (at low pressures). V n V 1 = V 2 n 1 n 2
21 Avogadro s Law The volume of a gas at constant temperature and pressure is directly proportional to the number of moles of the gas. Mathematically, this means V = kn
22 Ideal-Gas Equation So far we ve seen that V 1/P (Boyle s law) V T (Charles s law) V n (Avogadro s law) Combining these, we get nt V P
23 Combined Gas Law Combining the gas laws the relationship P T(n/V) can be obtained. If n (number of moles) is held constant, then PV/T = constant. P 1 V 1 T 1 = P 2 V 2 T 2
24 Ideal Gas Law PV = nrt R = universal gas constant = L atm K -1 mol -1 P = pressure in atm V = volume in liters n = moles T = temperature in Kelvin
25 Ideal-Gas Equation The constant of proportionality is known as R, the gas constant.
26 Ideal-Gas Equation The relationship V nt P then becomes nt V = R P or the classic PV = nrt
27 Problem Calculate the pressure in atmospheres and pascals of a 1.2 mol sample of methane gas in a 3.3 L container at 25 C.
28 Problem If the pressure of ozone, O 3, in the stratosphere is 3.0E-3 atm and the temperature is 250K, how many ozone molecules are in one liter.
29 STP Standard Temperature and Pressure (for gases) P = 1 atmosphere T = 0 C The molar volume of an ideal gas is liters at STP (put 1 mole, 1 atm, R, and 273 K in the ideal gas law and calculate V) Note STP is different for other phases, e.g. solutions or the phases associated with enthalpies of formation.
30 Densities of Gases If we divide both sides of the ideal-gas equation by V and by RT, we get n V = P RT
31 Densities of Gases We know that moles molecular mass = mass n = m So multiplying both sides by the molecular mass ( ) gives m V = P RT
32 Problem Calculate the density of sulfur hexafluoride gas at 707 torr and 21 C.
33 Molecular Mass We can manipulate the density equation to enable us to find the molecular mass of a gas: d = P RT Becomes = drt P
34 Problem To identify a diatomic gas (X 2 ), a researcher carried out the following experiment: She weighed an empty 1.00L- bulb, then filled it with the gas at 1.10 atm and 23.0 C and weighed it again. The difference in mass was 1.72 g. Identify the gas.
36 Problem Chloroform is a common lab reagent. If the pressure of chloroform in a flask at 25C is 195 mmhg and the density is 1.25 g/l. What is the molar mass of chloroform?
37 Dalton s Law of Partial Pressures For a mixture of gases in a container P Total = P 1 + P 2 + P
38 Consider a mixture of oxygen and nitrogen gases
39 Mole Fraction & Partial Pressure Mole Fraction: the ratio of the number of moles of a given component in a mixture to the total number of moles in a mixture. 1 = n 1 = n 1 n TOTAL n 1 + n 2 + n 3 + Mole Fraction in terms of pressure (n = PV/RT) 1 = P 1 (V/RT) P 1 (V/RT) + P 2 (V/RT) + P 3 (V/RT) +
40 Continued 1 = P 1 = P 1 P 1 + P 2 + P 3 + P TOTAL 1 = n 1 = P 1 n TOTAL P TOTAL
41 Mole Fraction Example At 25 0 C, a 1.0 L flask contains moles of nitrogen, mg of oxygen and 4 x molecules of ammonia. A. What is the partial pressure of each gas? B. What is the total pressure in the flask? C. What is the mole fraction of each?
44 Problem A sample of KClO 3 is heated and decomposes to produce O 2 gas. The gas is collected by water displacement at 25 C. The total volume of the collected gas is 370 ml at a pressure of 754 torr. How many moles of oxygen are formed? Hint: The gas collected is a mixture so use Dalton s Law to calculate the pressure of oxygen then the ideal gas law to find the number of moles oxygen. P T = P O 2 + P H 2O
45 Collecting a Gas Over Water
46 P H2O (25 C) = 23.8 torr
47 Problem A sample of 4.10 ml of diethylether (d = g/mL) is introduced into a 5.10 L vessel that already contains a mixture of N 2 and O 2, whose partial pressures are atm and atm, respectively. The temperature is held at 35.0 C, and the diethylether totally evaporates. a. Calculate the partial pressure of the diethylether. b. Calculate the total pressure in the container.
48 a. Calculate the partial pressure of the diethylether.
49 b. Calculate the total pressure in the container.
50 Kinetic Molecular Theory 1. The volume of the gas molecules is negligible compared with the container s volume. 2. Gas molecules move randomly and constantly. 3. The motion of these molecules is associated with their average kinetic energy that is proportional to the absolute temperature of the gas.
51 Kinetic Molecular Theory 4 Gas molecules continuously and elastically collide with one another and container walls. 5 Each molecule acts independently of all the other molecules in the sample. There are no forces of attraction (or repulsion) between molecules.
52 The temperature of an ideal monatomic gas is a measure related to the average kinetic energy of its atoms as they move. In this animation, the size of helium atoms relative to their spacing is shown to scale under 1950 atmospheres of pressure. These room-temperature atoms have a certain, average speed (slowed down here two trillion fold).
53 Main Tenets of Kinetic- Molecular Theory Energy can be transferred between molecules during collisions, but the average kinetic energy of the molecules does not change with time, as long as the temperature of the gas remains constant.
54 The path of individual particles is a Random Walk The Mean Free Path is the average distance traveled between collisions.
55 Kinetic Molecular Theory K.E. = 1/2mu 2 rms U rms - the root-meansquared speed of the molecules At Constant Temp U rms = 3RT M
56 u rms 3RT M root mean square velocity Calculate the root mean square velocity of O 2 at 60 C (333 K). [3 (8.314 kg m 2 s -2 mol -1 K -1 ) (333 K)/(0.032 kg mol -1 )] 1/2 = 509 m s -1
57 Problem. Calculate the velocity (in mi/hr) for water molecules at room temperature.
58 Diffusion and Effusion Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing. Effusion: describes the escape of gas through a tiny hole into a space of lower pressure.
59 The difference in the rates of effusion for helium and nitrogen, for example, explains why a helium balloon deflates faster. Effusion
61 At a given temperature the u rms velocity of a gas particle is dependent on temperature and mass of the particle. (from Kinetic Molecular Theory) The u rms equation can be used to derive Graham s Law of effusion (or diffusion). rate of rate of effusion effusion gas gas 1 2 M( gas 2) M( gas1)
62 Problem List the following gases, which are at the same temperature, in the order of increasing rates of diffusion. O 2, He, & NO
63 What will be the relative rate of effusion of hydrogen gas as compared to oxygen? r H 2 M O r O 2 M H
64 A sample of helium diffuses 4.58 times faster than an unknown gas. What is the likely identity of the unknown gas? (use Graham s Law) r r He unk M M unk He M He M unk M unk 83.9 [krypton(83.8)]
65 Real Gases For real gasses correct ideal gas behavior assumption when at high pressure (smaller volume) and low temperature (attractive forces become important).
66 Deviations from Ideal Behavior For 1 mole of an ideal gas under standard conditions we can define a compressibility factor, Z = 1 deviations of Z from 1 reflect non-ideal behavior.
67 In general, deviations from ideal behavior become more significant the closer a gas is to a phase change, the lower the temperature or the larger the pressure.
68 The value of Z generally increases with pressure and decreases with temperature.
69 The value of Z generally increases with pressure and decreases with temperature. Briefly At high pressures molecules are colliding more often, and at low temperatures they are moving less rapidly. This allows attractive forces between molecules to have a notable effect, making the volume of the real gas (V real ) less than the volume of an ideal gas (V ideal ) which causes Z to drop below one When pressures are lower or temperatures higher, the molecules are more free to move. In this case repulsive forces dominate, making Z > 1. The closer the gas is to its critical point or its boiling point, the more Z deviates from the ideal case.
70 Real Gases van der Waals Equation [ P + a ( n / V) ] x ( V - nb ) = nrt obs 2 corrected pressure corrected volume P ideal V ideal
71 Table 8.4 Van der Waal Constants for Selected Gases Substance a (L 2 atm/mol 2 ) b (L 2 /mol) He H CH CO SO P n 2 a V 2 V n b n R T
72 The van der Waals Equation (P + n 2 a V 2 ) (V nb) = nrt
73 At high pressures, real gases do not behave ideally. Use the van der Waals equation and data in the text to calculate the pressure exerted by mol H 2 at 25 C in a 1.00 L container. P P P nrt V nb L atm 17.55mol 298K mol K 1.00L 17.55mol L mol 729atm 2 n a 2 V 2 2 L atm 17.55mol mol L Repeat the calculation assuming that the gas behaves like an ideal gas. (check yourself, ans. 429 atm)
74 (a) Calculate the pressure exerted by 1.00 mol of CO 2 in a 1.00 L vessel at 300 K, assuming that the gas behaves ideally. (b) Repeat the calculation by using the van der Waals equation.
75 (b) Repeat the calculation by using the van der Waals equation.co2; a: 3.59 b: n 2 a P V n b n V 2 R T
#28 notes Unit 4: Gases Ch. Gases I. Pressure and Manometers Gas particles move in straight line paths. As they collide, they create a force, pressure. Pressure = Force / Area Standard Atmospheric Pressure
Chapter 5 The Gaseous State I) Pressure Pressure is the force exerted per unit area. A) Devices used to measure pressure 1) barometer used to measure the atmospheric pressure at seal level and 0 o C, P
Characteristics of Gases Practice Problems A. Section 10.2 Pressure Pressure Conversions: 1 ATM = 101.3 kpa = 760 mm Hg (torr) SAMPLE EXERCISE 10.1 Converting Units of Pressure (a) Convert 0.357 atm to
Kinetic Molecular Theory Particle volume - The volume of an individual gas particle is small compaired to that of its container. Therefore, gas particles are considered to have mass, but no volume. There
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 The things we will cover in this chapter: How differ from solids and liquids Pressure,
Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.
Chapter 4 The Properties of Gases Significant Figure Convention At least one extra significant figure is displayed in all intermediate calculations. The final answer is expressed with the correct number
Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force
The Gas Laws Describe HOW gases behave. Can be predicted by the theory. The Kinetic Theory Amount of change can be calculated with mathematical equations. The effect of adding gas. When we blow up a balloon
CHEM110 Week 9 Notes (Gas Laws) Page 1 of 7 Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). Gases Are mostly empty space Occupy containers uniformly and completely Expand infinitely Diffuse
Chapter 10 - Gases Gas - a substance that is characterized by widely separated molecules in rapid motion. Mixtures of gases are uniform. Gases will expand to fill containers (compare with solids and liquids
CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids
Common Student Misconceptions Students need to be told to always use Kelvin temperatures in gas problems. Students should always use units (and unit factor analysis) in gas-law problems to keep track of
Sample Exercise 10.1 Converting Pressure Units (a) Convert 0.357 atm to torr. (b) Convert 6.6 10 2 torr to atmospheres. (c) Convert 147.2 kpa to torr. Solution Analyze In each case we are given the pressure
Gases States of Matter States of Matter Kinetic E (motion) Potential E(interaction) Distance Between (size) Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large
Assignment 6 Solutions Chapter 6, #6.4, 6.12, 6.32, 6.36, 6.43, 6.60, 6.70, 6.80, 6.88, 6.90, 6.100, 6.104, 6.108. 6.4. Collect and Organize When the temperature of the balloon Figure P6.3 increases, does
Boyle s Law Charles Law Guy-Lassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is
Gas Law Problems Abbreviations Conversions atm - atmosphere K = C + 273 mmhg - millimeters of mercury 1 cm 3 (cubic centimeter) = 1 ml (milliliter) torr - another name for mmhg 1 dm 3 (cubic decimeter)
Class: Date: Chapter 5 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is the pressure of the sample of gas trapped in the open-tube mercury manometer
Gas Density Lift GOODYEAR Goodyear blimp filled with He gas BADYEAR Weight Badyear blimp filled with Cl 2 gas At STP( 1.00 atm, 273 K) 1.00 mole gas = 22.4 L Gas density: d = mass/volume = molar mass/molar
Name Unit 11 Review: Gas Laws and Intermolecular Forces Date Block 1. If temperature is constant, the relationship between pressure and volume is a. direct b. inverse 2. If pressure is constant, the relationship
PROPERTIES OF GASES or GAS LAWS 1 General Properties of Gases There is a lot of empty space in a gas. Gases can be expanded infinitely. Gases fill containers uniformly and completely. Gases diffuse and
Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids
CHEMISTRY Matter and Change 13 Table Of Contents Chapter 13: Gases Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry State the relationships among pressure, temperature,
Gases and Kinetic-Molecular heory: Chapter Chapter Outline Comparison of Solids, Liquids, and Gases Composition of the Atmosphere and Some Common Properties of Gases Pressure Boyle s Law: he Volume-Pressure
Type: Double Date: Objective: Kinetic Energy of an Ideal Gas I Kinetic Energy of an Ideal Gas II Homework: Read 14.3, Do Concept Q. # (15), Do Problems # (8, 9, 31, 37) AP Physics Mr. Mirro Kinetic Energy
EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,
T-41 Tutorial 6 GASES Before working with gases some definitions are needed: PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg TEMPERATURE: Kelvin, K, which is o C + 273 STP: Standard Temperature and Pressure:
CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,
Gas Laws MULTIPLE CHOICE 1. What are standard temperature and pressure conditions for gases? a. 0 C and 0 torr b. 0 K and 760 torr c. -273 C and 1 atm d. 0 C and 760 torr e. 0 C and 1 torr 2. If the volume
Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55
Lecture 9 State of gas described by (n,p,v,t) n # moles P pressure V volume T (absolute) temperature (K) Sample Problem A balloon filled with helium has a volume of 1.60 L at 1.00 atm and 25oC. What will
Classical Mechanics & Properties of Gases Properties of gases The gas phase differs from the other phases in that there are only weak interactions between particles Relatively simple models can be used
Chapter 6 Gases Kinetic Theory of Gases 6.1 Properties of Gases 6.2 Gas Pressure A gas consists of small particles that move rapidly in straight lines. have essentially no attractive (or repulsive) forces.
The Gas, Liquid, and Solid Phase When are interparticle forces important? Ron Robertson Kinetic Theory A. Principles Matter is composed of particles in constant, random, motion Particles collide elastically
Honors Chemistry Name Chapter 11: Gas Law Worksheet Answer Key Date / / Period Complete the following calculation by list the given information, rewriting the formula to solve for the unknown, and plugging
Version 001 HW03-Non Ideal, Gas Mixtures & KMT vandenbout (52130) 1 This print-out should have 20 questions. Multiple-choice questions may continue on the next column or page find all choices before answering.
1.4.6-1.4.8 Gas Laws Heat and Temperature Often the concepts of heat and temperature are thought to be the same, but they are not. Perhaps the reason the two are incorrectly thought to be the same is because
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
Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular
Gas Laws and Kinetic Molecular Theory The Gas Laws are based on experiments, and they describe how a gas behaves under certain conditions. However, Gas Laws do not attempt to explain the behavior of gases.
CHM1045 Practice Test 3 v.1 - Answers Name Fall 013 & 011 (Ch. 5, 6, 7, & part 11) Revised April 10, 014 Given: Speed of light in a vacuum = 3.00 x 10 8 m/s Planck s constant = 6.66 x 10 34 J s E (-.18x10
SESSION 7: KINETIC THEORY OF GASES Key Concepts In this session we will focus on summarising what you need to know about: Kinetic molecular theory Pressure, volume and temperature relationships Properties
EXERCISE 139, Page 303 CHAPTER 5 IDEAL GAS LAWS 1. The pressure of a mass of gas is increased from 150 kpa to 750 kpa at constant temperature. Determine the final volume of the gas, if its initial volume
Signed in as Daniel Semenick, Instructor Help Sign Out AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward Instructor Resources
Stoichiometry 1gram molecular mass 6.022 x 10 23 molecules Avagadro No of particles 6.022 x 10 23 particles MOLE 1 gram atomic mass 6.022 x 10 23 atoms Molar volume 22.4dm 3 at STP Equivalent mass of an
Chemistry 13: States of Matter Name: Period: Date: Chemistry Content Standard: Gases and Their Properties The kinetic molecular theory describes the motion of atoms and molecules and explains the properties
CHEM 1411, chapter 5 exercises 1. A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21 C is allowed to rise to the stratosphere where the temperature is 5 C and the pressure is 1.0 millibar.
1 CHEM 1411 Chapter 12 Homework Answers 1. A gas sample contained in a cylinder equipped with a moveable piston occupied 300. ml at a pressure of 2.00 atm. What would be the final pressure if the volume
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
Gas Laws Some chemical reactions take place in the gas phase and others produce products that are gases. We need a way to measure the quantity of compounds in a given volume of gas and relate that to moles.
Course Mathematical Tools and Unit Conversion Used in Thermodynamic Problem Solving 1 Basic Algebra Computations 1st degree equations - =0 Collect numerical values on one side and unknown to the otherside
Gases Petrucci, Harwood and Herring: Chapter 6 CHEM 1000A 3.0 Gases 1 We will be looking at Macroscopic and Microscopic properties: Macroscopic Properties of bulk gases Observable Pressure, volume, mass,
Chapter 12 Gases and Their Behavior Page 1 CHAPTER 12 GASES AND THEIR BEHAVIOR 12-1. Which of the following represents the largest gas pressure? (a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa 12-2. Nitrogen
Chapter 19: THE KINETIC THEORY OF GASES 1. Evidence that a gas consists mostly of empty space is the fact that: A. the density of a gas becomes much greater when it is liquefied B. gases exert pressure
Chapter 1 Gas Thermometer and Absolute Zero Name: Lab Partner: Section: 1.1 Purpose Construct a temperature scale and determine absolute zero temperature (the temperature at which molecular motion ceases).
Gases Section 13.1 The Gas Laws In your textbook, read about the basic concepts of the three gas laws. Use each of the terms below to complete the passage. Each term may be used more than once. pressure
1.23 Gas Calculations Gas calculations at A-level are done in two different ways although both link the volumes of a gas to the amount in moles of the gas. The same amount in moles of any gas will have
Chemistry 360 Dr. Jean M. Standard roblem Set Solutions 1. The atmospheric surface pressure on Venus is 90 bar. The atmosphere near the surface is composed of 96% carbon dioxide and 4% other gases. Given
Kinetic Theory of Gases Important Points:. Assumptions: a) Every gas consists of extremely small particles called molecules. b) The molecules of a gas are identical, spherical, rigid and perfectly elastic
SECTION 1 Gases and Pressure Key Terms pressure millimeters of mercury partial pressure newton atmosphere of pressure Dalton s law of partial pressures barometer pascal In the chapter States of Matter,
The first scheduled quiz will be given next Tuesday during Lecture. It will last 5 minutes. Bring pencil, calculator, and your book. The coverage will be pp 364-44, i.e. Sections 0.0 through.4. 0.7 Theory
Major chemistry laws. Mole and Avogadro s number. Calculating concentrations. Major chemistry laws Avogadro's Law Equal volumes of gases under identical temperature and pressure conditions will contain
Test 1 General Chemistry CH116 Summer, 2012 University of Massachusetts, Boston Name ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Sodium hydride reacts with excess
CHEMISTRY 101 Hour Exam I September 25, 2006 Adams/Le Name KEY Signature Section Iron rusts from disuse; stagnant water loses its purity and in cold weather becomes frozen; even so does inaction sap the
Chapter 14 he Ideal Gas Law and Kinetic heory Chapter 14 HE IDEAL GAS LAW AND KINEIC HEORY REIEW Kinetic molecular theory involves the study of matter, particularly gases, as very small particles in constant
1 P a g e Physics Notes Class 11 CHAPTER 13 KINETIC THEORY Assumptions of Kinetic Theory of Gases 1. Every gas consists of extremely small particles known as molecules. The molecules of a given gas are
PHYS-2010: General Physics I Course Lecture Notes Section XIII Dr. Donald G. Luttermoser East Tennessee State University Edition 2.5 Abstract These class notes are designed for use of the instructor and
Chemistry 110 Lecture Unit 5 Chapter 11-GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all
Version 001 HW04-Ideal Gas Laws, Gas Mixtures and KMT sparks (52100) 1 This print-out should have 15 questions. Multiple-choice questions may continue on the next column or page find all choices before
Name: Wednesday, January 16, 2008 Test 6: Phases of Matter Review Questions 1. According to the kinetic theory of gases, which assumption is correct? 1. Gas particles strongly attract each other. 3. The
CHAPTER FIVE Questions 16. a. Heating the can will increase the pressure of the gas inside the can, P T, V and n constant. As the pressure increases, it may be enough to rupture the can. b. As you draw
Thermodynamics: The Kinetic Theory of Gases Resources: Serway The Kinetic Theory of Gases: 10.6 AP Physics B Videos Physics B Lesson 5: Mechanical Equivalent of Heat Physics B Lesson 6: Specific and Latent
HONORS CHEMISTRY - CHAPTER 13 STATES OF MATTER OBJECTIVES AND NOTES - V15 NAME: DATE: PAGE: THE BIG IDEA: KINETIC THEORY Essential Questions 1. What factors determine the physical state of a substance?
Chapter 12 Exploring Gas Laws Solutions for Practice Problems Student Textbook page 477 1. Problem At 19 C and 100 kpa, 0.021 mol of oxygen gas, O 2(g), occupy a volume of 0.50 L. What is the molar volume
Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures
7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter Kinetic Molecular Theory of Matter The Kinetic Molecular Theory of Matter is a concept that basically states that matter is composed
The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical
This is Gases, chapter 6 from the book Beginning Chemistry (index.html) (v. 1.0). This book is licensed under a Creative Commons by-nc-sa 3.0 (http://creativecommons.org/licenses/by-nc-sa/ 3.0/) license.
1a. Mole fraction How many moles of X per mole of air? 1b. Volume mixing ratio how many liters of X per liter of air? 2. Partial pressure what is the pressure exerted by X in the air? Remember that for