# Exam 4 Practice Problems false false

Size: px
Start display at page:

## Transcription

1 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 and solids. c. Gases completely fill any container they occupy and are easily compressed. d. Vapor refers to a gas formed by evaporation of a liquid or sublimation of a solid. e. Solid water (ice), unlike most substances, is denser than its liquid form (water). 2. Which statement is false? a. The density of a gas is constant as long as its temperature remains constant. b. Gas expands without limit. c. Gases diffuse into each other and mix almost immediately when put into the same container. d. The molecular mass of a gaseous compound is an invariable quantity. e. Pressure must be exerted on a sample of a gas in order to confine it. 3. If the volume of a sample of Ne is tripled while the temperature is held constant, what happens to the pressure of the gas? a. It triples b. It stays the same. c. It doubles. d. It decreases by 1/3. e. It decreases by 1/2. 4. A sample of a gas occupies milliliters at 20.0 C and 600. torr. What volume will it occupy at the same temperature and 800. torr? a ml b ml c ml d ml e ml 5. Ammonia, NH 3, is used to as fertilizer and as a refrigerant. What is the new pressure if 25.0 g of ammonia with a volume of 750 ml at 1.50 atm is expanded to 7.50 L at constant temperature? a. 15 atm b. 114 mm Hg c psi d atm e. 15 mm Hg 6. A sample of oxygen occupies 47.2 liters under a pressure of torr at 25 C. By what percent does the volume of this sample change if the pressure were decreased to 730. torr at 25 C? a. 37.8% b. 41.1% c. 43.4% d. 46.1% e. 69.9% 7. If the volume of a sample of Cl 2 gas is tripled while pressure is held constant, what happens to the absolute temperature? a. It remains constant. b. It decreases by 1/3. c. It triples. d. It increases nine-fold. e. It decreases by 1/6.

2 8. Radon is a radioactive gas found below ground. If a sample of radon occupies 29 ml at 25 C, what volume will it occupy at 500 K? Assume constant pressure. a ml b. 29 ml c. 49 ml d. 17 ml e. 500 ml 9. A sample of nitrogen occupies 5.50 liters under a pressure of 900. torr at 25.0 C. At what temperature will it occupy 10.0 liters at the same pressure? a. 32 C b C c. 154 C d. 269 C e. 370 C 10. A sample of helium occupies 5.00 L at STP. What volume will the sample occupy at 0.0 C and 890. torr? a L b L c L d L e L 11. Which of the following statements about the combined gas law is incorrect? a. At constant temperature the volume occupied by a definite mass of a gas varies inversely with the applied pressure. b. Doubling the volume and pressure of a sample of gas quadruples the absolute temperature. c. At constant pressure the volume occupied by a definite mass of a gas varies inversely with the absolute temperature. d. Halving the volume of a sample of gas while doubling the pressure leaves the absolute temperature unchanged. e. Doubling the volume and pressure of a sample of gas doubles the absolute temperature. 12. A 1 L sample of gas at 25 C and 1 atm pressure is subjected to an increase in pressure and a decrease in temperature. The density of the gas. a. decreases b. increases c. remains the same d. becomes zero e. either increases or decreases, depending on the sizes of the pressure and temperature changes 13. What is the volume occupied by 10.0 grams of NH 3 at STP, if it behaves ideally? a L b L c L d L e L 14. What is the molecular weight of a gas if gram of the gas occupies 48.7 ml at STP? a g/mol b g/mol c g/mol d g/mol e g/mol 2

3 3 15. Given the mass of one mole of gaseous NO is 30.0 grams/mole, calculate the density of NO in grams/liter at STP. a g/l b g/l c g/l d g/l e g/l 16. Calculate the density of O 2, in g/l, at STP. a g/l b g/l c g/l d g/l e g/l 17. What is the volume that 57.0 grams of F 2 would occupy at 227 C and 1.50 atm? a L b L c L d L e. 106 L 18. How many oxygen atoms are contained in a sample of O 2 that occupies ml at 50.0 C and 1.00 atm pressure? a b c d e g sample of a gas occupies a volume of 275 ml at 10. C and 365 torr. What is the molecular weight of the gas? a g/mol b g/mol c g/mol d g/mol e g/mol 20. What is the pressure exerted by a mixture of 14.0 grams of N 2, 71.0 grams of Cl 2, and 16.0 grams of He in a 50.0-liter container at 0 C? a atm b atm c atm d atm e atm 21. A mixture of gas contains g Ar and 1.95 g Xe and has a total pressure of 2.33 atm. What are the partial pressures of each gas? P Ar (atm) P Xe (atm) a b c d e A 10.0-liter vessel contains gas A at a pressure of 300. torr. A 3.0-liter vessel contains gas B at a pressure of 400. torr. Gas A is forced into the second vessel. Calculate the resulting pressure in torr. Assume temperature remains constant.

4 a torr b torr c torr d torr e torr 23. A 75 ml sample of CO 2 is collected over water at 25 C when the atmospheric pressure is 1.05 atm. How many moles of CO 2 are present? The vapor pressure of water at 25 C is 24.3 torr. a b c d e Consider the following gas phase reaction. 4 4HCl(g) + O 2 (g) 2Cl 2 (g) + 2H 2 O(g) What volume of chlorine at STP can be prepared from the reaction of 600. ml of gaseous HCl, measured at STP, with excess O 2, assuming that all the HCl reacts? a ml b. 267 ml c ml d. 425 ml e ml 25. Calculate the weight of KClO 3 that would be required to produce liters of oxygen measured at 127 C and 760. torr. 2KClO 3 (s) 2KCl(s) + 3O 2 (g) a g b g c g d g e g 26. A 10.0 g sample of CaCO 3 is placed in a 10 L container and heated to 500 K. What is the pressure in the container, assuming all the CaCO 3 reacts. CaCO 3 (s) CaO (s) + CO 2 (g) a. 4.1 atm b atm c. 11 atm d. 42 atm e atm

5 27. Silver oxide decomposes completely at temperatures in excess of 300 C to produce metallic silver and oxygen gas. A 1.60-gram sample of impure Ag 2 O gives 72.1 ml of O 2 measured at STP. What is the percentage of Ag 2 O in the original sample? 5 2Ag 2 O(s) 4Ag(s) + O 2 (g) a. 79.6% b. 62.0% c. 86.4% d. 93.3% e. 73.3% 28. If 36.0 g of C 3 H 8 and 112 g of O 2 are placed in a closed container and the mixture is ignited, what is the maximum mass of CO 2 that could be produced? The other product of the reaction is water. a g b g c g d g e. 108 g 29. The average kinetic energy of ideal gas molecules is directly proportional to the. a. volume of the sample b. pressure of the sample c. mass of the molecule d. density of the sample e. absolute temperature of the sample 30. All of the following statements, except one, are important postulates of the kinetic-molecular theory of gases. Which one? a. Gases consist of large numbers of particles in rapid random motion. b. The volume of the molecules of a gas is very small compared to the total volume in which the gas is contained. c. The average kinetic energy of the molecules is inversely proportional to the absolute temperature. d. The time during which a collision between two molecules occurs is negligibly short compared to the time between collisions. e. There are no attractive or repulsive forces between the individual molecules. 31. What is the order of increasing rate of effusion for the following gases? Ar, CO 2, He, N 2 a. N 2 <Ar<CO 2 <He b. Ar<CO 2 <He<N 2 c. Ar<He<CO 2 <N 2 d. CO 2 <N 2 <Ar<He e. CO 2 <Ar<N 2 <He 32. The most significant intermolecular forces of attraction between individual nonpolar atoms or molecules in the gas phase are attractions. a. dispersion b. strong electrostatic c. covalent d. ionic e. strong dipole

6 6 33. The van der Waals constant, a, in the relationship (P + )(V - nb) = nrt is a factor that corrects for a. deviations in the gas constant, R. b. the attractive forces between gas molecules. c. the tendency of the gas molecules to ionize. d. the average velocities of the gas molecules. e. the volume occupied by the gas molecules. 34. The van der Waals constant, b, in the relationship (P + )(V - nb) = nrt is a factor that corrects for a. deviations in the gas constant, R. b. the attractive forces between gas molecules. c. the tendency of the gas molecules to ionize. d. the average velocities of the gas molecules. e. the volume occupied by the gas molecules. 35. Which of the following interactions are the strongest? a. hydrogen bonding force b. ion-ion interactions c. permanent dipole force d. dispersion force e. London force 36. The boiling points of the halogens increase in the order F 2 < Cl 2 < Br 2 < I 2 due to the resulting increasing interactions. a. ion-dipole b. hydrogen-bonding c. ion-ion d. dispersion forces e. permanent dipole-dipole 37. For which of the following would permanent dipole-dipole interactions play an important role in determining physical properties in the liquid state? a. BF 3 b. ClF c. BeCl 2 d. F 2 e. CCl For which of the following would hydrogen bonding not be an important factor in determining physical properties in the liquid state? a. HI b. H 2 O c. HF d. NH 3 e. H 2 O Which response correctly identifies all the interactions that might affect the properties of BrI? a. dispersion force, ion-ion interaction b. hydrogen bonding force, dispersion force c. permanent dipole force d. permanent dipole force, dispersion force e. dispersion force

7 40. Which response includes all of the following compounds that exhibit hydrogen bonding and no other compounds? 7 CH 4, AsH 3, CH 3 NH 2, H 2 Te, HF a. AsH 3, H 2 Te b. CH 3 NH 2, HF c. CH 4, AsH 3, H 2 Te d. AsH 3, CH 3 NH 2 e. HF, H 2 Te 41. Which of the following boils at the highest temperature? a. C 2 H 6 b. C 3 H 8 c. C 4 H 10 d. C 5 H 12 e. C 6 H Which one of the following boils at the lowest temperature? a. H 2 O b. H 2 S c. H 2 Se d. H 2 Te e. H 2 Po

8 Exam 4 Practice Problems Answer Section 8 MULTIPLE CHOICE 1. ANS: E PTS: 1 TOP: Comparison of Solids Liquids and Gases 2. ANS: A PTS: 1 TOP: Composition of the Atmosphere and Some Common Properties of 3. ANS: D PTS: 1 TOP: Boyle's Law 4. ANS: B PTS: 1 TOP: Boyle's Law 5. ANS: B PTS: 1 TOP: Boyle's Law 6. ANS: E PTS: 1 TOP: Boyle's Law 7. ANS: C PTS: 1 TOP: Charles's Law; the Absolute Temperature Scale 8. ANS: C PTS: 1 TOP: Charles's Law; the Absolute Temperature Scale 9. ANS: D PTS: 1 TOP: Charles's Law; the Absolute Temperature Scale 10. ANS: D PTS: 1 TOP: Standard Temperature and Pressure 11. ANS: E PTS: 1 TOP: The Combined Gas Law Equation 12. ANS: B PTS: 1 TOP: Avogadro's Law and the Standard Molar Volume 13. ANS: B PTS: 1 TOP: Avogadro's Law and the Standard Molar Volume 14. ANS: E PTS: 1 TOP: Avogadro's Law and the Standard Molar Volume 15. ANS: D PTS: 1 TOP: Avogadro's Law and the Standard Molar Volume 16. ANS: B PTS: 1 TOP: Avogadro's Law and the Standard Molar Volume 17. ANS: C PTS: 1 TOP: The Ideal Gas Equation 18. ANS: E PTS: 1 TOP: The Ideal Gas Equation 19. ANS: C PTS: 1 TOP: Determinations of Molecular Weights and Molecular Formulas of Gaseous Substances 20. ANS: A PTS: 1 TOP: Dalton's Law of Partial Pressures 21. ANS: B PTS: 1 TOP: Dalton's Law of Partial Pressures 22. ANS: B PTS: 1 TOP: Dalton's Law of Partial Pressures 23. ANS: C PTS: 1 TOP: Dalton's Law of Partial Pressures 24. ANS: C PTS: 1 TOP: Mass-Volume Relationships in Reactions Involving Gases 25. ANS: E PTS: 1 TOP: Mass-Volume Relationships in Reactions Involving Gases 26. ANS: E PTS: 1 TOP: Mass-Volume Relationships in Reactions Involving Gases 27. ANS: D PTS: 1 TOP: Mass-Volume Relationships in Reactions Involving Gases 28. ANS: D PTS: 1 TOP: Mass-Volume Relationships in Reactions Involving Gases 29. ANS: E PTS: 1 TOP: The Kinetic-Molecular Theory 30. ANS: C PTS: 1 TOP: The Kinetic-Molecular Theory 31. ANS: E PTS: 1 TOP: Diffusion and Effusion of Gases 32. ANS: A PTS: 1 TOP: Real Gases: Deviations from Ideality 33. ANS: B PTS: 1 TOP: Real Gases: Deviations from Ideality 34. ANS: E PTS: 1 TOP: Real Gases: Deviations from Ideality 35. ANS: B PTS: 1 TOP: Intermolecular Attractions and Phase Changes 36. ANS: D PTS: 1 TOP: Intermolecular Attractions and Phase Changes 37. ANS: B PTS: 1 TOP: Intermolecular Attractions and Phase Changes 38. ANS: A PTS: 1 TOP: Intermolecular Attractions and Phase Changes 39. ANS: D PTS: 1 TOP: Intermolecular Attractions and Phase Changes 40. ANS: B PTS: 1 TOP: Intermolecular Attractions and Phase Changes 41. ANS: E PTS: 1 TOP: Intermolecular Attractions and Phase Changes 42. ANS: B PTS: 1 TOP: Intermolecular Attractions and Phase Changes

### CHEM 120 Online Chapter 7

CHEM 120 Online Chapter 7 Date: 1. Which of the following statements is not a part of kinetic molecular theory? A) Matter is composed of particles that are in constant motion. B) Particle velocity increases

### CHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry

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,

### Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

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. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.

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.

### Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline

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

### ESSAY. Write your answer in the space provided or on a separate sheet of paper.

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

### MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

General Chemistry PHS 1015 Practice Exam 4 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements about pressure

### The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10

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

### Boyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P

Boyles Law At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 or k 1 Boyles Law Example ressure olume Initial 2.00 atm 100 cm 3

### CHAPTER 12. Gases and the Kinetic-Molecular Theory

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

### 7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter

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

### Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

### CHEMISTRY GAS LAW S WORKSHEET

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

### 7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

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,

### = 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm

Chapter 13 Gases 1. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. Gases have volumes that depend on their conditions, and can be compressed or expanded by

### States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. 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. ideal gas

### Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134)

Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134) 1. Helium atoms do not combine to form He 2 molecules, What is the strongest attractive

### Chemistry 110 Lecture Unit 5 Chapter 11-GASES

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

### 87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X

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

### Intermolecular Forces

Intermolecular Forces: Introduction Intermolecular Forces Forces between separate molecules and dissolved ions (not bonds) Van der Waals Forces 15% as strong as covalent or ionic bonds Chapter 11 Intermolecular

### Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008

Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid

### Chapter 10. Can You... 1. draw the Lewis structure for a given covalently bonded molecule?

Chapter 10 Can You... 1. draw the Lewis structure for a given covalently bonded molecule? e.g. SF 6 and CH 3 Cl 2. identify and count the number of non-bonding and bonding domains within a given covalently

### Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT).

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

### Chemistry 13: States of Matter

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

### Gases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random)

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

### 5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C

1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )

### Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1

Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0

### Bonding Practice Problems

NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which

### CHEMISTRY 113 EXAM 4(A)

Summer 2003 1. The molecular geometry of PF 4 + ion is: A. bent B. trigonal planar C. tetrahedral D. octahedral CHEMISTRY 113 EXAM 4(A) 2. The Cl-C-Cl bond angle in CCl 2 O molecule (C is the central atom)

### The Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015

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

### Page 2. Base your answers to questions 7 through 9 on this phase diagram

1. The normal boiling point of water is often depressed at high altitudes. Which of the following explains this phenomenon? t high altitudes, the lower atmospheric pressure equals the equilibrium water

### Chapter 13 - LIQUIDS AND SOLIDS

Chapter 13 - LIQUIDS AND SOLIDS Problems to try at end of chapter: Answers in Appendix I: 1,3,5,7b,9b,15,17,23,25,29,31,33,45,49,51,53,61 13.1 Properties of Liquids 1. Liquids take the shape of their container,

### KINETIC MOLECULAR THEORY OF MATTER

KINETIC MOLECULAR THEORY OF MATTER The kinetic-molecular theory is based on the idea that particles of matter are always in motion. The theory can be used to explain the properties of solids, liquids,

### MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

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

### CHAPTER 10: INTERMOLECULAR FORCES: THE UNIQUENESS OF WATER Problems: 10.2, 10.6,10.15-10.33, 10.35-10.40, 10.56-10.60, 10.101-10.

CHAPTER 10: INTERMOLECULAR FORCES: THE UNIQUENESS OF WATER Problems: 10.2, 10.6,10.15-10.33, 10.35-10.40, 10.56-10.60, 10.101-10.102 10.1 INTERACTIONS BETWEEN IONS Ion-ion Interactions and Lattice Energy

### Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

### 10.7 Kinetic Molecular Theory. 10.7 Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory

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

### 10.7 Kinetic Molecular Theory. 10.7 Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic Molecular Theory

Week lectures--tentative 0.7 Kinetic-Molecular Theory 40 Application to the Gas Laws 0.8 Molecular Effusion and Diffusion 43 Graham's Law of Effusion Diffusion and Mean Free Path 0.9 Real Gases: Deviations

### 2. The percent yield is the maximum amount of product that can be produced from the given amount of limiting reactant.

UNIT 6 stoichiometry practice test True/False Indicate whether the statement is true or false. moles F 1. The mole ratio is a comparison of how many grams of one substance are required to participate in

### CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING

CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING Essential Standard: STUDENTS WILL UNDERSTAND THAT THE PROPERTIES OF MATTER AND THEIR INTERACTIONS ARE A CONSEQUENCE OF THE STRUCTURE OF MATTER,

### AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1

Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol -1. Example

### In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.

Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.

### Chapter 4 Practice Quiz

Chapter 4 Practice Quiz 1. Label each box with the appropriate state of matter. A) I: Gas II: Liquid III: Solid B) I: Liquid II: Solid III: Gas C) I: Solid II: Liquid III: Gas D) I: Gas II: Solid III:

### F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.

Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.

### Name: Class: Date: 2) Which one of the following exhibits dipole-dipole attraction between molecules? A) XeF 4 B) AsH 3 C) CO 2 D) BCl 3 E) Cl 2

Name: Class: Date: IM Bonding 1) In liquids, the attractive intermolecular forces are. A) very weak compared with kinetic energies of the molecules B) strong enough to hold molecules relatively close together

### Why? Intermolecular Forces. Intermolecular Forces. Chapter 12 IM Forces and Liquids. Covalent Bonding Forces for Comparison of Magnitude

1 Why? Chapter 1 Intermolecular Forces and Liquids Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water?

### CHEMISTRY II FINAL EXAM REVIEW

Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas

### Kinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check.

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.

### Unit 11 Practice. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Name: Class: Date: Unit 11 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1) Crystalline solids. A) have their particles arranged randomly B) have

### Chem 1A Exam 2 Review Problems

Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?

### Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

### MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Given: 4 NO2(g) + O2(g) 2 N2O5(g) ΔH = -110.2 kj find ΔH for N2O5(g) 2 NO2(g) + 1/2 O2(g).

### Chemistry 151 Final Exam

Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must

### Test 5 Review questions. 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will

Name: Thursday, December 13, 2007 Test 5 Review questions 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will 1. decrease 2. increase 3. remain the same 2. The graph below

### 1.4.6-1.4.8 Gas Laws. Heat and Temperature

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

### Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)

BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in

### Part B 2. Allow a total of 15 credits for this part. The student must answer all questions in this part.

Part B 2 Allow a total of 15 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit for 3 Mg(s) N 2 (g) Mg 3 N 2 (s). Allow credit even if the coefficient 1 is

### CHEM 36 General Chemistry EXAM #1 February 13, 2002

CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show

### Gas Laws. vacuum. 760 mm. air pressure. mercury

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.

### Test Review # 9. Chemistry R: Form TR9.13A

Chemistry R: Form TR9.13A TEST 9 REVIEW Name Date Period Test Review # 9 Collision theory. In order for a reaction to occur, particles of the reactant must collide. Not all collisions cause reactions.

### Unit 3: States of Matter Practice Exam

Page 1 Unit 3: States of Matter Practice Exam Multiple Choice. Identify the choice that best completes the statement or answers the question. 1. Two gases with unequal masses are injected into opposite

### Study the following diagrams of the States of Matter. Label the names of the Changes of State between the different states.

Describe the strength of attractive forces between particles. Describe the amount of space between particles. Can the particles in this state be compressed? Do the particles in this state have a definite

### Problem Solving. Stoichiometry of Gases

Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.

### Multiple Choice questions (one answer correct)

Mole Concept Multiple Choice questions (one answer correct) (1) Avogadro s number represents the number of atoms in (a) 12g of C 12 (b) 320g of sulphur (c) 32g of oxygen (d) 12.7g of iodine (2) The number

### IB Chemistry. DP Chemistry Review

DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

### Molar Mass of Butane

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

### Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K

Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K Kinetic Molecular Theory of Gases 1. Large number of atoms/molecules in random motion 2.

### Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and

### POLAR COVALENT BONDS Ionic compounds form repeating. Covalent compounds form distinct. Consider adding to NaCl(s) vs. H 2 O(s):

POLAR COVALENT BONDS Ionic compounds form repeating. Covalent compounds form distinct. Consider adding to NaCl(s) vs. H 2 O(s): Sometimes when atoms of two different elements form a bond by sharing an

### 10. Calculate the mass percent nitrogen in (NH 4 ) 2 CO 3 (molar mass = 96.09 g/mol). a. 29.1 % c. 17.9 % e. 14.6 % b. 35.9 % d. 0.292 % f. 96.

Chem 171-2-3: Final Exam Review Multiple Choice Problems 1. What is the molar mass of barium perchlorate, Ba(ClO 4 ) 2? a. 189.90 g/mol c. 272.24 g/mol e. 336.20 g/mol b. 240.24 g/mol d. 304.24 g/mol f.

### Questions on Chapter 8 Basic Concepts of Chemical Bonding

Questions on Chapter 8 Basic Concepts of Chemical Bonding Circle the Correct Answer: 1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be 2+ C) B2+ D) C2+ E) N 2-2) Of the ions below,

### Chapter 3 Mass Relationships in Chemical Reactions

Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative

### Chapter 1 The Atomic Nature of Matter

Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.

### H 2O gas: molecules are very far apart

Non-Covalent Molecular Forces 2/27/06 3/1/06 How does this reaction occur: H 2 O (liquid) H 2 O (gas)? Add energy H 2O gas: molecules are very far apart H 2O liquid: bonding between molecules Use heat

### Chemistry 1050 Chapter 13 LIQUIDS AND SOLIDS 1. Exercises: 25, 27, 33, 39, 41, 43, 51, 53, 57, 61, 63, 67, 69, 71(a), 73, 75, 79

Chemistry 1050 Chapter 13 LIQUIDS AND SOLIDS 1 Text: Petrucci, Harwood, Herring 8 th Edition Suggest text problems Review questions: 1, 5!11, 13!17, 19!23 Exercises: 25, 27, 33, 39, 41, 43, 51, 53, 57,

### Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)

Name Date Class 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches

### Mole Calculations Multiple Choice Review PSI Chemistry

Mole Calculations Multiple Choice Review PSI Chemistry Name The Mole and Avogadro's Number 1)What is the SI unit for measurement of number of particles in a substance? A) kilogram B) ampere C) candela

### Chapter 14 Solutions

Chapter 14 Solutions 1 14.1 General properties of solutions solution a system in which one or more substances are homogeneously mixed or dissolved in another substance two components in a solution: solute

### Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :

Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles

### EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES

Name Section EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to

### Intermolecular and Ionic Forces

Intermolecular and Ionic Forces Introduction: Molecules are attracted to each other in the liquid and solid states by intermolecular, or attractive, forces. These are the attractions that must be overcome

### INTERMOLECULAR FORCES

INTERMOLECULAR FORCES Intermolecular forces- forces of attraction and repulsion between molecules that hold molecules, ions, and atoms together. Intramolecular - forces of chemical bonds within a molecule

### KINETIC THEORY OF MATTER - molecules in matter are always in motion - speed of molecules is proportional to the temperature

1 KINETIC TERY F MATTER - molecules in matter are always in motion - speed of molecules is proportional to the temperature TE STATES F MATTER 1. Gas a) ideal gas - molecules move freely - molecules have

### Chapter 12 - Liquids and Solids

Chapter 12 - Liquids and Solids 12-1 Liquids I. Properties of Liquids and the Kinetic Molecular Theory A. Fluids 1. Substances that can flow and therefore take the shape of their container B. Relative

### Structure, Polarity & Physical Properties

tructure, Polarity & Physical Properties upplemental packet handouts 92-96 I. Lewis structure, stability, and bond energies A. ydrogen, oxygen, and nitrogen are present in the atmosphere as diatomic molecular

### Mole Notes.notebook. October 29, 2014

1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the

### Solution. Practice Exercise. Concept Exercise

Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of

### Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O

Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent

### Chapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT

Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass

### CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)

CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26

### Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.

TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present

### EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor

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,

### Element of same atomic number, but different atomic mass o Example: Hydrogen

Atomic mass: p + = protons; e - = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon-12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine-35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass

### Sample Exercise 8.1 Magnitudes of Lattice Energies

Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas

### Chemical Composition. Introductory Chemistry: A Foundation FOURTH EDITION. Atomic Masses. Atomic Masses. Atomic Masses. Chapter 8

Introductory Chemistry: A Foundation FOURTH EDITION by Steven S. Zumdahl University of Illinois Chemical Composition Chapter 8 1 2 Atomic Masses Balanced equation tells us the relative numbers of molecules

### Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358)

Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.

### Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)

10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches you how to calculate

### Calculating Atoms, Ions, or Molecules Using Moles

TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary