Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
ISBN #9780132931281
11th Edition
3,230 Questions
Homework Questions
General Chemistry: Principles and Modern Applications is a comprehensive textbook that lays a solid foundation in essential chemical concepts while seamlessly integrating modern applications and problem-solving techniques. The book systematically introduces topics ranging from the measurement and properties of matter through atomic theory, chemical bonding, and periodic trends, all the way to complex subjects like thermodynamics, kinetics, and electrochemistry. It builds a logical progression from basic principles to advanced discussions on reaction mechanisms, organic syntheses, and nuclear as well as coordination chemistry, offering both theoretical insights and practical computational tools. Unique in its breadth and clarity, the text serves as an invaluable resource for students aiming to master the fundamental and applied aspects of chemistry.
Chapter 1
Matter: Its Properties and Measurement
Chapter 2
Atoms and the Atomic Theory
Chapter 3
Chemical Compounds
Chapter 4
Chemical Reactions
Chapter 5
Introduction to Reactions in Aqueous Solutions
Chapter 6
Gases
Chapter 7
Thermochemistry
Chapter 8
Electrons in Atoms
Chapter 9
The Periodic Table and Some Atomic Properties
Chapter 10
Chemical Bonding I: Basic Concepts
Chapter 11
Chemical Bonding II: Valence Bond and Molecular Orbital Theories
Chapter 12
Intermolecular Forces: Liquids and Solids
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Chapter 13
Spontaneous Change: Entropy and Gibbs Energy
Chapter 14
Solutions and Their Physical Properties
Chapter 15
Principles of Chemical Equilibrium
Chapter 16
Acids and Bases
Chapter 17
Additional Aspects of Acid–Base Equilibria
Chapter 18
Solubility and Complex-Ion Equilibria
Chapter 19
Electrochemistry
Chapter 20
Chemical Kinetics
Chapter 21
Chemistry of the Main-Group Elements I: Groups 1, 2, 13, and 14
Chapter 22
Chemistry of the Main-Group Elements II: Groups 18, 17, 16, 15, and Hydrogen
Chapter 23
The Transition Elements
Chapter 24
Complex Ions and Coordination Compounds
Chapter 25
Nuclear Chemistry
Chapter 26
Structures of Organic Compounds
Chapter 27
Reactions of Organic Compounds
Problem 1
Calculate the final temperature that results when (a) a 12.6 g sample of water at $22.9^{\circ} \mathrm{C}$ absorbs $875 \mathrm{J}$ of heat; (b) a 1.59 kg sample of platinum at $78.2^{\circ} \mathrm{C}$ gives off $1.05 \mathrm{kcal}$ of heat $\left(c_{p}=0.032 \mathrm{cal} \mathrm{g}^{-1} \mathrm{C}^{-1}\right)$
Elham Kordzadeh Numerade Educator
Problem 2
What are the principal reasons that one theory might be adopted over a conflicting one?
David Collins Numerade Educator
Problem 3
Which of the following is moderately soluble both in water and in benzene, $\mathrm{C}_{6} \mathrm{H}_{6}(\mathrm{l}),$ and why? (a) 1 -butanol, $\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{2} \mathrm{CH}_{2} \mathrm{OH} ;$ (b) naphthalene, $\mathrm{C}_{10} \mathrm{H}_{8} ;$ (c) hexane, $\mathrm{C}_{6} \mathrm{H}_{14} ;$ (d) $\mathrm{NaCl}(\mathrm{s})$.
Will Li Numerade Educator
Problem 4
Calculate the quantity of heat, in kilojoules, (a) required to raise the temperature of 9.25 Lof water from 22.0 to $29.4^{\circ} \mathrm{C} ;$ (b) associated with a $33.5^{\circ} \mathrm{C}$ decrease in temperature in a $5.85 \mathrm{kg}$ aluminum bar (specific heat capacity of aluminum $=0.903 \mathrm{Jg}^{-1} \mathrm{C}^{-1}$ ).
Bhumika Jayee Numerade Educator
Problem 5
Convert each pressure to an equivalent pressure in atmospheres. (a) $736 \mathrm{mmHg} ;$ (b) 0.776 bar; (c) 892 Torr; (d) 225 kPa.
Chareen Guzman Numerade Educator
Problem 6
When an iron object rusts, its mass increases. When a match burns, its mass decreases. Do these observations violate the law of conservation of mass? Explain.
Kristen Justice Numerade Educator
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