Gases: Their Properties & Behavior. Chapter 09 Slide 1


 Marsha Cooper
 7 months ago
 Views:
Transcription
1 9 Gases: Their Properties & Behavior Chapter 09 Slide 1
2 Gas Pressure 01 Chapter 09 Slide 2
3 Gas Pressure 02 Units of pressure: atmosphere (atm) Pa (N/m 2, 101,325 Pa = 1 atm) Torr (760 Torr = 1 atm) bar ( bar = 1 atm) mm Hg (760 mm Hg = 1 atm) lb/in 2 ( lb/in 2 = 1 atm) in Hg ( in Hg = 1 atm) Chapter 09 Slide 3
4 Boyle s Law 01 Pressure Volume Law (Boyle s Law): Chapter 09 Slide 4
5 Boyle s Law 01 Pressure Volume Law (Boyle s Law): Chapter 09 Slide 5
6 Boyle s Law 02 Pressure Volume Law (Boyle s Law): Volume 1 Pressure The volume of a fixed amount of gas maintained at constant temperature is inversely proportional to the gas pressure. V 1 P 1 = k 1 Chapter 09 Slide 6
7 A sample of chlorine gas occupies a volume of 946 ml at a pressure of 726 mmhg. What is the pressure of the gas (in mmhg) if the volume is reduced at constant temperature to 154 ml? P 1 x V 1 = P 2 x V 2 P 1 = 726 mmhg V 1 = 946 ml P 2 =? V 2 = 154 ml P 2 = P 1 x V 1 V mmhg x 946 ml = = 4460 mmhg 154 ml 5.3 Chapter 09 Slide 7
8 As T increases V increases Chapter 09 Slide 8
9 Charles Law 01 Temperature Volume Law (Charles Law): T(K)=Temperature in Kelvin T (K) = t (0C) Chapter 09 Slide 9
10 Charles Law 01 Temperature Volume Law (Charles Law): V T The volume of a fixed amount of gas at constant pressure is directly proportional to the Kelvin temperature of the gas. V 1 T 1 =k 1 Chapter 09 Slide 10
11 Variation of gas volume with temperature at constant pressure. P 1 <P 2 <P 3 <P 4 V α T V = constant x T V 1 /T 1 = V 2 /T 2 Temperature must be in Kelvin T (K) = t ( 0 C) Chapter 09 Slide 11
12 A sample of carbon monoxide gas occupies 3.20 L at C. At what temperature will the gas occupy a volume of 1.54 L if the pressure remains constant? V 1 /T 1 = V 2 /T 2 V 1 = 3.20 L T 1 = K V 2 = 1.54 L T 2 =? T 2 = V 2 x T 1 V L x K = = 192 K 3.20 L Chapter 09 Slide 12
13 Avogadro s Law 01 The Volume Amount Law (Avogadro s Law): Chapter 09 Slide 13
14 Avogadro s Law 01 The Volume Amount Law (Avogadro s Law): V n At constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of the gas present. V 1 = k n 1 1 Chapter 09 Slide 14
15 Ammonia burns in oxygen to form nitric oxide (NO) and water vapor. How many volumes of NO are obtained from one volume of ammonia at the same temperature and pressure? 4NH 3 + 5O 2 4NO + 6H 2 O 1 mole NH 3 1 mole NO At constant T and P 1 volume NH 3 1 volume NO Chapter 09 Slide 15
16 Ideal Gas Equation Boyle s law: V α 1 (at constant n and T) P Charles law: V α T (at constant n and P) Avogadro s law: V α n (at constant P and T) V α nt P nt V = constant x = R nt P P R is the gas constant PV = nrt Chapter 09 Slide 16
17 The conditions 0 0 C and 1 atm are called standard temperature and pressure (STP). Experiments show that at STP, 1 mole of an ideal gas occupies L. PV = nrt R = PV nt = (1 atm)(22.414l) (1 mol)( K) R = L atm / (mol K) Chapter 09 Slide 17
18 The Ideal Gas Law 01 Ideal gases obey an equation incorporating the laws of Charles, Boyle, and Avogadro. P V = n R T R =The gas constant R = L atm K 1 mol 1 Chapter 09 Slide 18
19 What is the volume (in liters) occupied by 49.8 g of HCl at STP? T = 0 0 C = K PV = nrt V = nrt P P = 1 atm n = 49.8 g x 1 mol HCl g HCl = 1.37 mol V = L atm 1.37 mol x x K mol K 1 atm V = 30.6 L 5.4 Chapter 09 Slide 19
20 PV = nrt nr V P 1 T 1 Argon is an inert gas used in lightbulbs to retard the vaporization of the filament. A certain lightbulb containing argon at 1.20 atm and 18 0 C is heated to 85 0 C at constant volume. What is the final pressure of argon in the lightbulb (in atm)? = P T = P 2 T 2 n, V and R are constant = constant P 1 = 1.20 atm T 1 = 291 K P 2 = P 1 x T 2 T 1 = 1.20 atm x 358 K 291 K P 2 =? T 2 = 358 K = 1.48 atm Chapter 09 Slide 20
21 USING GAS DENSITY The density of air at 15 o C and 1.00 atm is 1.23 g/l.. What is the molar mass of air? 1. Calc. moles of air. V = 1.00 L, m=1.23 g, P = 1.00 atm, T = ( )= 288 K n = PV/RT = mol, m=1.23 g 2. Calc. molar mass mass/mol = 1.23 g/ mol = 29.1 g/mol Chapter 09 Slide 21
22 Dalton s Law of Partial Pressures 01 Flash Animation  Click to Continue Chapter 09 Slide 22
23 Dalton s Law of Partial Pressures V and T are constant P 1 P 2 P total = P 1 + P 2 Chapter 09 Slide 23
24 Consider a case in which two gases, A and B, are in a container of volume V. P A = n A RT V P B = n B RT V n A is the number of moles of A n B is the number of moles of B Chapter 09 Slide 24
25 P A = n A RT V P B = n B RT V P T = n A RT V n B RT V RT V + = (n A + n B ) P A / P T = n A n A + n B X A = n A n A + n B P A / P T = X A P A = X A P T P B = X B P T X B = n B n A + n B P i = X i P T P T = P A + P B Chapter 09 Slide 25
26 A sample of natural gas contains 8.24 moles of CH 4, moles of C 2 H 6, and moles of C 3 H 8. If the total pressure of the gases is 1.37 atm, what is the partial pressure of propane (C 3 H 8 )? P i = X i P T X propane = P T = 1.37 atm = P propane = x 1.37 atm = atm Chapter 09 Slide 26
27 Gas Stoichiometry 01 In gas stoichiometry, for a constant temperature and pressure, volume is proportional to moles. Assuming no change in temperature and pressure, calculate the volume of O 2 (in liters) required for the complete combustion of 14.9 L of butane (C 4 H 10 ): 2 C 4 H 10 (g) + 13 O 2 (g) 8 CO 2 (g) + 10 H 2 O(l) Chapter 09 Slide 27
28 Gas Stoichiometry What is the volume of CO 2 produced at 37 0 C and 1.00 atm when 5.60 g of glucose are used up in the reaction: C 6 H 12 O 6 (s) + 6O 2 (g) 6CO 2 (g) + 6H 2 O (l) g C 6 H 12 O 6 mol C 6 H 12 O 6 mol CO 2 V CO 2 1 mol C 5.60 g C 6 H 12 O 6 H 12 O 6 6 x 180 g C 6 H 12 O 6 6 mol CO x 2 = mol CO 1 mol C 6 H 12 O 2 6 V = nrt P L atm mol x x K mol K = = 4.76 L 1.00 atm Chapter 09 Slide 28
29 Chapter 09 Slide 29
30 Kinetic Molecular Theory 01 This theory presents physical properties of gases in terms of the motion of individual molecules. Average Kinetic Energy Kelvin Temperature Gas molecules are points separated by a great distance Particle volume is negligible compared to gas volume Gas molecules are in rapid random motion Gas collisions are perfectly elastic Gas molecules experience no attraction or repulsion Chapter 09 Slide 30
31 KineticMolecular 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. Chapter 09 Slide 31
32 Kinetic Molecular Theory 03 Average Kinetic Energy (KE) is given by: KE = 1 2 mu2 u 2 = u2 N Chapter 09 Slide 32
33 Kinetic Molecular Theory 03 Average Kinetic Energy (KE) is given by: KE = 1 2 mu2 u 2 = u2 N Chapter 09 Slide 33
34 Kinetic Molecular Theory 05 Maxwell speed distribution curves. Chapter 09 Slide 34
35 Kinetic Molecular Theory 04 The Root Mean Square Speed: is a measure of the average molecular speed. u 2 = 3RT M Taking square root of both sides gives the equation Calculate the root mean square speeds of helium atoms and nitrogen molecules in m/s at 25 C. R=8.314 J/K.mol 1J = 1Kg.m 2 /s 2 3RT u rms = M H m/s Chapter 09 Slide 35
36 Graham s Law 02 Effusion is when gas molecules escape, through a tiny hole into a vacuum. Chapter 09 Slide 36
37 Graham s Law 03 Graham s Law: Rate of effusion is proportional to its rms speed, u rms. Rate α u rms = 3RT M For two gases at same temperature and pressure: Rate 1 Rate 2 = M 2 M 1 = M 2 M 1 Chapter 09 Slide 37
38 A Problem to Consider How much faster would H 2 gas effuse through an opening than methane, CH 4? Rate of Rate of H CH 2 = 4 M m M m (CH (H 2 4 ) ) Rate of H Rate of CH 16.0 g/mol 2.0 g/mol 2 = = So hydrogen effuses 2.8 times faster than CH 4 Chapter 09 Slide 38
39 Behavior of Real Gases 01 Deviations result from assumptions about ideal gases. 1. Molecules in gaseous state do not exert any force, either attractive or repulsive, on one another. 2. Volume of the molecules is negligibly small compared with that of the container. Chapter 09 Slide 39
40 Behavior of Real Gases 02 At higher pressures, particles are much closer together and attractive forces become more important than at lower pressures. As a result, the pressure of real gases will be smaller than the ideal value Chapter 09 Slide 40
41 Behavior of Real Gases 03 The volume taken up by gas particles is actually less important at lower pressures than at higher pressure. As a result, the volume at high pressure will be greater than the ideal value. Chapter 09 Slide 41
42 Behavior of Real Gases 04 Test of ideal gas behavior. Chapter 09 Slide 42
43 Behavior of Real Gases 05 Test of ideal gas behavior. Chapter 09 Slide 43
44 Behavior of Real Gases 05 Corrections for nonideality require van der Waals equation. P + a n V 2 2 ( V n b) = nrt Intermolecular Attractions Excluded Volume Chapter 09 Slide 44
45 A Problem to Consider If sulfur dioxide were an ideal gas, the pressure at 0 o C exerted by mol occupying L would be atm. Use the van der Waals equation to estimate the real pressure. Use the following values for SO 2 a = L 2. atm/mol 2 b = L/mol Chapter 09 Slide 45
46 A Problem to Consider First, let s rearrange the van der Waals equation to solve for pressure. 2 P = nrt V  nb  n V R= L. atm/mol. K T = K a = L 2. atm/mol 2 V = L b = L/mol a 2 Chapter 09 Slide 46
47 A Problem to Consider P = nrt V  nb  2 n a 2 V P 2 (1.000 mol) =  2 L atm (1.000 mol)( mol K)(273.2K) L  (1.000 mol)( L/mol) P = atm (6.865 (22.41 L) L atm 2 mol 2 ) The real pressure exerted by 1.00 mol of SO 2 at STP is slightly less than the ideal pressure. Chapter 09 Slide 47
48 Thermochemical Equations The physical states of all reactants and products must be specified in thermochemical equations. H 2 O (s) H 2 O (l) ΔH = 6.01 kj H 2 O (l) H 2 O (g) ΔH = 44.0 kj How much heat is evolved when 266 g of white phosphorus (P 4 ) burn in air? P 4 (s) + 5O 2 (g) P 4 O 10 (s) ΔH = kj 1 mol P g P 4 x g P 4 x 3013 kj 1 mol P 4 = 6470 kj Chapter 09 Slide 48
Apparatus for Studying the Relationship Between Pressure and Volume of a Gas
Apparatus for Studying the Relationship Between Pressure and Volume of a Gas As P (h) increases V decreases 1 Boyle s Law P α 1/V P x V = constant P 1 x V 1 = P 2 x V 2 Constant temperature Constant amount
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 informationA Gas Uniformly fills any container. Easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings.
Chapter 5 Gases Chapter 5 A Gas Uniformly fills any container. Easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings. Copyright Cengage Learning. All rights reserved
More informationChapter 10 Gases. Dr. Ayman Nafady. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E.
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Gases Dr. Ayman Nafady 2009, PrenticeHall, 10.1. Characteristics of Gases Unlike liquids
More informationChapter 5 Gases and the KineticMolecular Theory
Chapter 5 Gases and the KineticMolecular 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 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 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. Question. Question. Answer. Answer. Question (continued) The Gaseous State
Chapter 5 CRS s The Gaseous State Equal volumes of propane, C 3 H 8, and carbon monoxide at the same temperature and pressure have the same a. density. b.. c. number of atoms. 1) a only 2) b only 3) c
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 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 informationThe KineticMolecular Theory of Gases
The KineticMolecular Theory of Gases kineticmolecular theory of gases Originated with Ludwig Boltzman and James Clerk Maxwell in the 19th century Explains gas behavior on the basis of the motion of individual
More informationGases and Kinetic 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 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 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 openend manometer to calculate the pressure of the gas. Use conversion factors to
More informationThe KineticMolecular Theory of Gases
The KineticMolecular Theory of Gases kineticmolecular 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 8 Gases. 8.1 Kinetic Theory of Gases. 8.2 Barometer. Properties of Gases. 8.1 Gases and Kinetic Theory 8.2 Gas Pressure 8.
Chapter 8 Gases 8.1 Gases and Kinetic Theory 8.2 Gas Pressure 8.8 Ideal Gas Law * You do not need to know Boyle s (8.3), Charles (8.4), GayLussac s (8.5), Avogadro s (8.7) or the Combined gas (8.6) laws.
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 informationCHAPTER 12 GASES AND KINETICMOLECULAR THEORY
. Pressure CHAPER GASES AND KINEICMOLECULAR HEORY. Boyle s Law: he P Relationship 3. Charles Law: he  Relationship 4. Standard &P 5. he Combined Gas Law Equation 6. Avogadro s Law and the Standard Molar
More informationUnit Outline. I. Introduction II. Gas Pressure III. Gas Laws IV. Gas Law Problems V. KineticMolecular Theory of Gases VI.
Unit 10: Gases Unit Outline I. Introduction II. Gas Pressure III. Gas Laws IV. Gas Law Problems V. KineticMolecular Theory of Gases VI. Real Gases I. Opening thoughts Have you ever: Seen a hot air balloon?
More informationChapter 5. Gases and the KineticMolecular Theory
Chapter 5. Gases and the KineticMolecular Theory 1 5.1 An Overview of the Physical States of Matter The reason we study gases in Chemistry: The observable properties of gases give us a window into what
More information1. What is the value of the quantity PV for one mole of an ideal gas at 25.0 C and one atm?
Real Gases Thought Question: How does the volume of one mole of methane gas (CH4) at 300 Torr and 298 K compare to the volume of one mole of an ideal gas at 300 Torr and 298 K? a) the volume of methane
More 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 informationmcdonald (pam78654) HW 4B: Gases and Kinetics laude (89560) 1
mcdonald (pam78654) HW 4B: Gases and Kinetics laude (89560) 1 This printout should have 20 questions. Multiplechoice questions may continue on the next column or page find all choices before answering.
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 informationCHAPTER 13 Gases The Gas Laws
CHAPTER 13 Gases 13.1 The Gas Laws The gas laws apply to ideal gases, which are described by the kinetic theory in the following five statements. Gas particles do not attract or repel each other. Gas particles
More 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 informationGases and the Kinetic Molecular Theory. ก ก ก ก McGraw Hill. Gases and the Kinetic Molecular Theory
ก ก Gases and the Kinetic Molecular Theory ก ก ก ก McGraw Hill 1 Gases and the Kinetic Molecular Theory 5.1 An Overview of the Physical States of Matter 5. Gas Pressure and Its Measurement 5.3 The Gas
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) 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 MultipleChoice 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 informationUseful Information to be provided on the exam: 1 atm = 760 mm Hg = 760 torr = lb/in 2 = 101,325 Pa = kpa. q = m C T. w = P V.
Chem 101A Study Questions, Chapters 5 & 6 Name: Review Tues 10/25/16 Due 10/27/16 (Exam 3 date) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach
More informationChapter 11. = 14.1 psi. = 28.7 in. Hg. 1 bar 1 atm 101, 325 Pascal 1000 mbar bar 1 atm 1 bar 1 atm 760 torr 1000 mbar 1.
ractice Exercises. psi = 70 mm Hg in. Hg = 70 mm Hg 4.7 psi 760 mm Hg 9.9 in. Hg 760 mm Hg = 4. psi = 8.7 in. Hg. ascals = 888 mbar torr = 888 mbar bar 0, 5 ascal 000 mbar.0 bar bar 000 mbar.0 bar = 666
More informationBELL WORK, 6Mar2017
BELL WORK, 6Mar2017 Write a balanced equation for the reaction below: Zinc and bromide react to for Zinc (II) Bromide In series of trials a student recorded the following data when reacting Zinc and
More informationChapter 13 The Ideal Gas Law and Its Applications
Free Guide for Cracolice Peters Introductory Chemistry: An Active Learning Approach Second Edition www.brookscole.com/chemistry Chapter 13 The Ideal Gas Law and Its Applications Chapter 13 Assignment A:
More informationBoyle's Law. Solution: P 1 (0.6L)=(4atm)(2.4L) P 1 = 16atm
Page1 Boyle's Law Boyle's Law, a principle that describes the relationship between the pressure and volume of a gas. According to this law, the pressure exerted by a gas held at a constant temperature
More informationFTF Day 9. April 9, 2012 HW: Assessment Questions 13.1 (Wed) Folder Check Quiz on Wednesday Topic: Gas laws Question: What are gasses like?
Gas Laws Ch 13 FTF Day 9 April 9, 2012 HW: Assessment Questions 13.1 (Wed) Folder Check Quiz on Wednesday Topic: Gas laws Question: What are gasses like? Describe motion of particles, compressibility,
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 informationMolecular Composition of Gases
CHAPTER 11 Molecular Composition of Gases The study of gases led to the formulation of the laws and principles that are the foundations of modern chemistry. VolumeMass Relationships of Gases SECTION 111
More informationSAMPLE EXERCISE 10.1 Converting Units of Pressure. SAMPLE EXERCISE 10.1 continued
SAMPLE EXERCISE 10.1 Converting Units of Pressure (a) Convert 0.357 atm to torr. (b) Convert 6.6 10 2 torr to atm. (c) Convert 147.2 kpa to torr. Analyze: In each case we are given the pressure in one
More informationMind Catalyst Stick It!
Mind Catalyst Stick It! O With a partner, use the following scenarios as a guide to come up with the relationships of the gas properties. For each scenario, write the two properties and their relationship
More informationName Date Class STUDY GUIDE FOR CONTENT MASTERY. Use each of the terms below to complete the passage. Each term may be used more than once.
Gases Section 14.1 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
More informationCHEM 116 The Ideal Gas Model: Its Usefulness and Conditions Where it Breaks Down
Uass oston, Chem 116 CHE 116 The Ideal Gas odel: Its Usefulness and Conditions Where it reaks Down Lecture 3 Prof. Sevian Last Thursday Today Today s agenda Some uses of the ideal gas equation Typical
More informationMacroscopic vs. Microscopic Representation
Agenda Day 80 Gases Intro  11. 1 & 11.7 & 12.2 Lesson: PPT Handouts: 1.PPT Handout, 2. ISU  Kinetic Molecular Theory and Real vs. Ideal Gases Sections ( W1) Macroscopic vs. Microscopic Representation
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 informationPut your name on this exam paper!!!
DEPARTMENT OF CHEMISTRY Midterm Examination Chemistry 1110 (Modern Chemistry I) Name: Student ID Number: Instructions: 1. Put your name on this exam paper!!! Questions are to be answered directly on these
More information9/18/2013. Scientists represent atoms by using different colored circles, called a model.
PreLab Notes Lab Title: Behavior of Gases: Molar Mass of a Vapor Purpose: To determine the molar mass of a gas from a knowledge of its mass, temperature, pressure, and volume. Each element is unique.
More informationKINETIC MOLECULAR THEORY
KINETIC MOLECULAR THEORY IMPORTANT CHARACTERISTICS OF GASES 1) Gases are highly compressible An external force compresses the gas sample and decreases its volume, removing the external force allows the
More information101 chem GENERAL CHEMISTRY1
101 chem GENERAL CHEMISTRY1 First Mid Term (15 marks) Second Mid Term (15 marks) Lab (30 marks) Mid term (30 marks) Final (100 marks) Course# and Name: Chem101, General chemistryi Semester credit hours:
More informationChapter 12 Stoichiometry
12.2 Chemical Calculations > Chapter 12 Stoichiometry 12.1 The Arithmetic of Equations 12.22 Chemical Calculations 12.3 Limiting Reagent and Percent Yield 1 Copyright Pearson Education, Inc., or its affiliates.
More informationIdeal Gas Problems. 3. What is the pressure (in atmospheres) of a mol sample of helium gas at 20.0ºC if its volume is L? Latm.
Ideal Gas Problems. What are the values of STP (standard temperature and pressure)? Temperature: 7 K. Pressure: atm.. Calculate the volume of mol of an ideal gas under STP. (Memorize this relation!) p
More information5. None are true correct. 6. I only. 7. III only
Version 001 Practice Exam 3  F15 mccord (78704) 1 This printout should have 25 questions. Multiplechoice questions may continue on the next column or page find all choices before answering. Remember
More informationKinetic theory. Collective behaviour of large systems Statistical basis for the ideal gas equation Deviations from ideality
Kinetic theory Collective behaviour of large systems Statistical basis for the ideal gas equation Deviations from ideality Learning objectives Describe physical basis for the kinetic theory of gases Describe
More informationHomework 02  Ideal Gases
HW02  Ideal Gases This is a preview of the draft version of the quiz Started: Aug 8 at 4:48pm Quiz Instructions Homework 02  Ideal Gases Question 1 A gas is enclosed in a 10.0 L tank at 1200 mmhg pressure.
More informationExample Exercise 10.1 Interpreting Chemical Equation Calculations
Example Exercise 10.1 Interpreting Chemical Equation Calculations Given the chemical equation for the combustion of methane, CH 4, balance the equation and interpret the coefficients in terms of (a) moles
More information1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %
1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A. 9.372 % C. 28.12 % B. 21.38 % D. 42.73 % 2. How many grams of phosphorus are in 35.70 g of P 2 O 5? A. 6.359 g C. 15.58 g B. 23.37 g D. 31.16
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 informationChemistry Final Exam: Practice Problems
Chemistry Final Exam: Practice Problems 1. Key Vocabulary/Terms: atomic number element compound kinetic theory acid base salt vaporization condensation evaporation boiling sublimation energy level valence
More informationCHEM 150 Exam 2. Name Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
CHEM 150 Exam 2 Name Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. _A D 1. Formic acid, HCOOH, is what causes the sting of bee stings. What
More informationaskiitians Class: 11 Subject: Chemistry Topic: Kinetic theory of gases No. of Questions: The unit of universal gas constant in S.I.
Class: 11 Subject: Chemistry Topic: Kinetic theory of gases No. of Questions: 33 1. The unit of universal gas constant in S.I.unit is A. calorie per degree Celsius B. joule per mole C. joule/k mole C 2.
More 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 information3Fe +2 (aq) + 2PO 4. NaHCO 3 + H 2 O. Chem 121 Quiz 3 Practice Fall 2017
Chem 121 Quiz 3 Practice Fall 2017 The following quiz contains 22 questions (and bonuses!) valued at 1 point/question Name KEY G = H T S PV = nrt P 1 V 1 = P 2 V 2 P 1 /T 1 = P 2 /T 2 V 1 /T 1 = V 2 /T
More informationvan der Waals Isotherms near T c
van der Waals Isotherms near T c v d W loops are not physical. Why? Patch up with Maxwell construction van der Waals Isotherms, T/T c van der Waals Isotherms near T c Look at one of the van der Waals isotherms
More informationChapter Practice Test Grosser
Class: Date: Chapter 1011 Practice Test Grosser Multiple Choice Identify the choice that best completes the statement or answers the question. 1. According to the kineticmolecular theory, particles of
More informationChem 1411 Practice Exam 2
Chem 1411 Practice Exam 2 Instructions 1. Write your name on your exam. 2. You may use only the scratch paper and periodic table provided with the exam. You may also use a calculator, provided it cannot
More information3. What property and two conditions determine the phase of a sample of matter is? Property = Equilbirum Conditions = Temperature and Pressure
9.A Calorimetry: Basics Instructions: Provide a response for each question that is well thought out, satisfies the prompt, is clearly explained, and LEGIBLE. 1. In a closed system what basic fact must
More informationCHEM 1411 Zumdahl & Zumdahl PRACTICE EXAM II (Chapters 4, 5, 6)
CHEM 1411 Zumdahl & Zumdahl PRACTICE EXAM II (Chapters 4, 5, 6) Multiple Choices: Select one best answer. 1. Which of the following is a weak electrolyte? (a) barium hydroxide solution (b) ammonia solution
More informationVersion 001 HW02gas laws vandenbout (52130) 1
Version 001 HW02gas laws vandenbout (52130) 1 This printout should have 24 questions. Multiplechoice questions may continue on the next column or page find all choices before answering. Mlib 76 2075
More informationUnit 3  Part 2: Gas Laws. Objective  learn the main gas laws that all molecules follow.
Unit 3  Part 2: Gas Laws Objective  learn the main gas laws that all molecules follow. Pressure  Pressure = Force / Area Created by collisions of the gas molecules with each other and with surfaces.
More informationOH (ammonium hydroxide) are in 3.47 moles of NH 4. OH? 1 grams. 2 Na(s) + Cl 2. (g) 2 NaCl(s) (32.00 g/mol) according to the reaction C 3
Question #: 1 Posting ID: 423347 Course: CHE 105 2015 SU Instructor: Sarah Edwards How many grams of NH 4 OH (ammonium hydroxide) are in 3.47 moles of NH 4 OH? 1 grams Question #: 2 When 2.61 grams of
More information10. 2 P R O B L E M S L I Q U I D S A N D G A S E S
South Pasadena AP Chemistry Name 10 States of Matter Period Date 10. 2 P R B L E M S L I Q U I D S A N D G A S E S 1. Use the following table to answer these questions. Vapor Pressures of Various Liquids
More informationStoichiometry: Chemical Calculations. Chemistry is concerned with the properties and the interchange of matter by reaction structure and change.
Stoichiometry: Chemical Calculations Chemistry is concerned with the properties and the interchange of matter by reaction structure and change. In order to do this, we need to be able to talk about numbers
More information10.2 MoleMass and Mole Volume Relationships. Chapter 10 Chemical Quantities. Volume Relationships The Mole: A Measurement of Matter
Chapter 10 Chemical Quantities 101 The Mole: A Measurement of Matter 102 MoleMass and Mole 103 Percent Composition and Chemical Formulas 1 http://wwwbrightstormcom/science/chem istry/chemicalreactions/molarmass/
More informationChem 1411 Practice Exam 2
Chem 1411 Practice Exam 2 Instructions 1. Write your name on your exam. 2. You may use only the scratch paper and periodic table provided with the exam. You may also use a calculator, provided it cannot
More informationGeneral Chemistry Study Guide
General Chemistry 1311 Study Guide Name : Louise K number: Date: Oct 02006 Instructor: Jingbo Louise Liu kfjll00@tamuk.edu 1 Chapter 04 & 05 (10 questions required and 5 questions for extra credit) Credited
More informationUnit 3: STATES OF MATTER
Unit 3: STATES OF MATTER Chapter 5: Gases 5.: Pressure Pressure:  the amount of force per unit of area [ N/m Pascal (Pa)], measured in kilopascal (kpa), mm g, torr, atmospheric pressure (atm).  in a
More informationChapter 8. The Mole Concept
Chapter 8 The Mole Concept Chapter 9 2 Avogadro s Number Avogadro s number (symbol N) is the number of atoms in 12.01 grams of carbon. Its numerical value is 6.02 10 23. Therefore, a 12.01 g sample of
More informationStoichiometry. Consider the reaction in which the reactants are nitrogen gas and hydrogen gas. They produce the product ammonia gas.
1 1. Interpreting Chemical Equations Stoichiometry Calculations using balanced equations are called stoichiometric calculations. The starting point for any problem involving quantities of chemicals in
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 informationCHEMISTRY 102B Hour Exam II. Dr. D. DeCoste T.A.
CHEMISTRY 10B Hour Exam II March 19, 015 Dr. D. DeCoste Name Signature T.A. This exam contains questions on 9 numbered pages. Check now to make sure you have a complete exam. You have one hour and thirty
More informationQ.4 Which of the following of will have the same number of
year n0te chemitry new t Chapter 3rd GASES MCQ Q.1 The order of the rate of diffuion of gae NH3, SO2, Cl2 and CO2 i: (a) NH3 > SO2 > Cl2 > CO2 (b) NH3 > CO2 > SO2 > Cl2 Cl2> SO2 > CO2 > NH3 None of thee
More informationCHEMISTRY Practice Exam #3  SPRING 2013
CHEMISTRY 1710  Practice Exam #3  SPRING 2013 Section 1  This section of the exam is multiple choice. Choose the BEST answer from the choices which are given and write the letter for your choice in
More informationGases and IMFs Unit Exam Review Guide
Gases and IMFs Unit Exam Review Guide The following review guide does not necessarily contain all topics that will appear on the test. Make sure to review all notes and concepts from this unit. This review
More informationCHEM 101 WINTER MAKEUP EXAM
CHEM 101 WINTER 0809 MAKEUP EXAM On the answer sheet (Scantron) write you name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on
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 informationPUT A SQUARE BOX AROUND ALL ANSWERS
UNIVERSITY OF TORONTO FACULTY OF APPLIED SCIENCE AND ENGINEERING CHE 112F PHYSICAL CHEMISTRY MIDTERM EXAM, OCTOBER 16 2014 6:10 pm to 8:00 pm EXAMINER P.V. Yaneff 1. Answer all questions. The marks add
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
AP Chemistry: Practice Test, Ch. 5.  Gases Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) According to kineticmolecular theory, in which
More informationCHEMISTRY MOLES PACKET PAGE 1. Chemistry Moles Packet
CHEMISTRY MOLES PACKET PAGE 1 Chemistry Moles Packet CHEMISTRY MOLES PACKET PAGE 2 INTRODUCTION TO MOLES We are about to start on a unit of chemical calculations called stoichiometry. Stoichiometry is
More informationREVIEW QUESTIONS Chapter Determine the pressure of the gas (in mmhg) in the diagram below, given atmospheric pressure= atm.
Chemistry 101 ANSWER KEY REVIEW QUESTIONS Chapter 5 1. Determine the pressure of the gas (in mmhg) in the diagram below, given atmospheric pressure= 0.975 atm. atm = 0.975 atm h = 5 cmhg gas atm 760 mmhg
More informationTHE GASEOUS STATE OF MATTER
THE GASEOUS STATE OF MATTER The gaseous state of matter is a form of matter in which the particles are in a high state of energy, which causes them to vibrate rapidly, experiencing a strong repulsion among
More informationmolality: m = = 1.70 m
C h e m i s t r y 1 2 U n i t 3 R e v i e w P a g e 1 Chem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet 1. What is miscible? Immiscible? Miscible: two or more substances blend together for form a solution
More informationChemical Equations 10/30/13. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions
Chemical Equations A chemical equation just like a mathematical equation is a way to express, in symbolic form, the reactions occurring in a chemical system. n Balancing chemical equations n Reaction stoichiometry
More informationPhases of Matter Vocabulary
Word Avogadro s Hypothesis Boiling Condensing Deposition Equilibrium Evaporating Freezing Gas Heat of Fusion Heat of Vaporization Ideal Gas Liquid Melting Pressure Solid Specific Heat Sublimation Vapor
More informationName: Class: Date: SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. a. The gas
More informationName May 2, 2012 Physical Behavior of Matter and Bonding Review
Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool
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 informationWhere are we going? Chem Lecture resources. Gases. Charles Law. Boyle s Law. A/Prof Sébastien Perrier. Login: chem1101 Password: carbon12
Chem 1101 Where are we going? examinable A/Prof Sébastien Perrier Room: 351 Phone: 93513366 Email: s.perrier@chem.usyd.edu.au Prof Scott Kable Room: 311 Phone: 93512756 Email: s.kable@chem.usyd.edu.au
More informationUpon completion of this lab, the student will be able to:
1 Learning Outcomes EXPERIMENT 30A5: MOLAR VOLUME OF A GAS Upon completion of this lab, the student will be able to: 1) Demonstrate a single replacement reaction. 2) Calculate the molar volume of a gas
More informationCHEMISTRY 101 EXAM 3 FORM 3M
CHEMISTRY 101 EXAM 3 SECTIONS 572580 Dr. Joy Heising Directions: FORM 3M November 20, 2001 1. This examination consists of two parts: 17 multiple choice questions (6 points each) in Part 1 and 4 free
More informationGASES. PV = nrt N 2 CH 4 CO 2 O 2 HCN N 2 O NO 2. Pressure & Boyle s Law Temperature & Charles s Law Avogadro s Law IDEAL GAS LAW
GASES Pressure & Byle s Law Temperature & Charles s Law Avgadr s Law IDEAL GAS LAW PV = nrt N 2 CH 4 CO 2 O 2 HCN N 2 O NO 2 Earth s atmsphere: 78% N 2 21% O 2 sme Ar, CO 2 Sme Cmmn Gasses Frmula Name
More informationDraw the Lewis structures of all 7 diatomic elements
Warm up Draw the Lewis structures of all 7 diatomic elements States of Matter  Part 1  Gasses Definitions kineticmolecular theory particles of matter are always in motion ideal gas hypothetical gas
More informationเคม เช งฟ ส กส I. Physical Chemistry I Chongrak_kinetics. Physical Chemistry
เคม เช งฟ ส กส I Physical Chemistry I 014034 สาขาว ชาเคม คณะศ ลปศาสตร และว ทยาศาสตร ม.ก. กพส. Sc.4309 : faaspmp@ku.ac.th Physical Chemistry The study of underlying physical principles that governs the
More information