Practice Makes Perfect in Chemistry: The Physical Behavior of Matter with Answers
By John Parnell
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About this ebook
One of the best ways to succeed in Chemistry is to practice taking real test questions. This volume contains 445 problems on Physical Behavior of Matter divided into five chapters: Energy, Properties of Gases, Energy, Forces, and Change, Mixtures, and Solutions. Answers are provided. Try the problems. With a little Practice, Practice, Practice, you’ll be Perfect, Perfect, Perfect. Good Luck!
John Parnell
About the author: Mr. Parnell holds teaching certification in physics, chemistry, biology, general science, mathematics, and business and distributed education. Over the course of forty years of teaching, he has taught students from the sixth grade through graduate school. In addition, Mr. Parnell has taught for the New York State Research Foundation preparing students for the SAT exam in mathematics.
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Practice Makes Perfect in Chemistry - John Parnell
Practice Makes Perfect in Chemistry:
Volume Five – Physical Behavior of Matter
445 Practice Problems with Answers
John E. Parnell, B.S., M.S.
Certified Math and Science Teacher
Published by Tutor Turtle Press at Smashwords.com.
© 2009 by John E. Parnell
Smashwords Edition, License Notes
This ebook is licensed for your personal enjoyment only. This ebook may not be re-sold or given away to other people. If you would like to share this book with another person, please purchase an additional copy for each person you share it with. If you’re reading this book and did not purchase it, or it was not purchased for your use only, then you should return to Smashwords.com and purchase your own copy. Thank you for respecting the hard work of this author.
Discover all the titles in the Practice Makes Perfect in Chemistry series by John E. Parnell at Smashwords.com:
Volume One: Atomic Concepts – 220 Review Questions with Answers
Atomic Structure
Isotopes
Atomic Theories
Volume Two: The Periodic Table – 191 Review Questions with Answers
1. Development of the Periodic Table
Valence Electrons
Properties of Groups
Properties of Periods
Volume Three: Compounds, Reactions and Moles – 254 Review Questions with Answers
Compounds
Empirical and Molecular Formulas
Gram Formula Mass, Moles and Percent Composition
Math and Chemical Equations
Types of Chemical Reactions
Volume Four: Chemical Bonding – 113 Review Questions with Answers
Bond Energy and Electronegativity
Bond Types
Bond and Molecular Polarity
Volume Five: The Physical Behavior of Matter – 445 Review Questions with Answers
Energy
Properties of Gases
Energy, Forces and Change
Mixtures
Solutions
Volume Six: Kinetics and Equilibrium – 167 Review Questions with Answers
Rates of Reactions
Enthalpy
Equilibrium
Entropy
Volume Seven: Organic Chemistry – 211 Review Questions with Answers
Hydrocarbons
General Properties and Isomers
Other Organic Compounds
Organic Reactions
Volume Eight: Oxidation-Reduction – 183 Review Questions with Answers
Redox Reactions and Oxidation Numbers
Electrochemical Cells
Volume Nine: Acids, Bases and Salts – 249 Review Questions with Answers
Electrolytes
Theories and Properties
Reactions
Miscellaneous
Volume Ten: Nuclear Chemistry – 183 Review Questions with Answers
1. Natural Radioactivity
2. Transmutation, Fission and Fusion
Beneficial Uses of Isotopes
Miscellaneous
FORWARD
One of the best ways to succeed in Chemistry is to practice taking real test questions. This volume contains 445 problems on Physical Behavior of Matter divided into five chapters: Energy, Properties of Gases, Energy, Forces, and Change, Mixtures, and Solutions. Following each chapter are the answers for each problem presented in the chapter. Try the problems. Check your answers. With a little Practice, Practice, Practice, you’ll be Perfect, Perfect, Perfect. Good Luck!
Table of Contents
Chapter 1: Energy
49 Practice Questions
Answers to questions on Energy
Chapter 2: Properties of Gases
101 Practice Questions
Answers to questions on Properties of Gases
Chapter 3: Energy, Forces and Change
159 Practice Questions
Answers to questions on Energy, Forces and Change
Chapter 4: Mixtures
37 Practice Questions
Answers to questions on Mixtures
Chapter 5: Solutions
99 Practice Questions
Answers to questions on Solutions
Appendix
Table A: Standard Temperature and Pressure
Table B: Physical Constants for Water
Table C: Selected Prefixes
Table D: Selected Units
Table E: Selected Polyatomic Ions
Table F: Solubility Guidelines for Aqueous Solutions
Table G: Solubility Curves
Table H: Vapor Pressure of Four Liquids
Table I: Heats of Reaction at 101.3 kPa and 198 K
Table J: Activity Series
Table K: Common Acids
Table L: Common Bases
Table M: Common Acid-Base Indicators
Table N: Selected Radioisotopes
Table O: Symbols Used in Nuclear Chemistry
Table P: Organic Prefixes
Table Q: Homologous Series of Hydrocarbons
Table R: Organic Functional Groups
Table S: Properties of Selected Elements
Table T: Important Formulas and Equations
The Periodic Table
Chapter 1: Energy
1. In which beaker would the particles have the highest average kinetic energy?
2. At one atmosphere of pressure, the fixed temperature points on a Celsius thermometer are located on the basis of
the ice/water equilibrium temperature only
the water/steam equilibrium temperature only
both the ice/water and water/steam equilibrium temperatures
neither the ice/water nor the water/steam equilibrium temperature
3. The average kinetic energy of the molecules of an ideal gas is directly proportional to the
number of moles present
volume occupied by individual gas molecules
temperature measured on the Kelvin scale
pressure at standard temperature
4. What type of change do the reactants undergo in the reaction
2H2(g) + O2(g) → 2H2O(g)?
atomic
phase
chemical
nuclear
5. Two pure water samples held in separate containers at one atmosphere pressure must have molecules possessing the same average kinetic energy if the samples have the same
volume
temperature
mass
density
6. Which equilibrium at one atmosphere pressure is correctly associated with Kelvin temperature at which it occurs?
ice-water equilibrium at 0 K
ice-water equilibrium at 32 K
steam-water equilibrium at 212 K
steam-water equilibrium at 373 K
7. When a sample of a gas is heated at constant pressure, the average kinetic energy of its molecules
decreases and the volume of the gas increases
decreases and the volume of the gas decreases
increases and the volume of the gas increases
increases and the volume of the gas decreases
8. The temperature of a sample of a substance changes from 10°C to 20°C. By how many Kelvins does the temperature change?
10
20
283
293
9. What is the number of Kelvins between the freezing point and the boiling point of water at a pressure of 760 torr?
100
212
273
373
10. The boiling point of water at standard pressure is
0.000 K
100. K
273 K
373 K
11. Which temperature represents absolute zero?
0 K