John C. Kotz, Paul M. Treichel, John R. Townsend
ISBN #9780495387039
7th Edition
2,044 Questions
Homework Questions
Chemistry and Chemical Reactivity is a comprehensive textbook that introduces the fundamental concepts of chemistry, from matter classification and atomic structure to the intricacies of chemical bonding and reactivity. The book systematically builds on foundational principles—such as stoichiometry, thermodynamics, and kinetics—illustrating how analytical techniques and theoretical models are applied in both laboratory and industrial contexts. It explores a wide range of topics, including periodic trends, intermolecular forces, nuclear reactions, and electron transfer processes, providing clear links between core theories and real-world applications. By integrating detailed quantitative analyses with modern scientific methods, this text serves as an essential guide for developing a robust understanding of chemical principles and their practical implications.
Chapter 1
Basic Concepts of Chemistry
Chapter 2
Atoms, Molecules, and Ions
Chapter 3
Chemical Reactions
Chapter 4
Stoichiometry: Quantitative Information About Chemical Reactions
Chapter 5
Principles of Chemical Reactivity: Energy and Chemical Reactions
Chapter 6
The Structure of Atoms
Chapter 7
The Structure of Atoms and Periodic Trends
Chapter 8
Bonding and Molecular Structure
Chapter 9
Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals
Chapter 10
Carbon: More Than Just Another Element
Chapter 11
Gases and Their Properties
Chapter 12
Intermolecular Forces and Liquids
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Chapter 13
The Chemistry of Solids
Chapter 14
Solutions and Their Behavior
Chapter 15
Chemical Kinetics: The Rates of Chemical Reactions
Chapter 16
Principles of Reactivity: Chemical Equilibria
Chapter 17
The Chemistry of Acids and Bases
Chapter 18
Principles of Reactivity: Other Aspects of Aqueous Equilibria
Chapter 19
Principles of Reactivity: Entropy and Free Energy
Chapter 20
Principles of Reactivity: Electron Transfer Reactions
Chapter 21
The Chemistry of the Main Group Elements
Chapter 22
The Chemistry of the Transition Elements
Chapter 23
Nuclear Chemistry
Problem 1
Boron phosphide, BP, is a semiconductor and a hard, abrasion-resistant material. It is made by reacting boron tribromide and phosphorus tribromide in a hydrogen atmosphere at high temperature $\left(>750^{\circ} \mathrm{C}\right)$ (a) Write a balanced chemical equation for the synthesis of BP. (Hint: Hydrogen is a reducing agent.) (b) Boron phosphide crystallizes in a zinc blende structure, formed from boron atoms in a face-centered cubic lattice and phosphorus atoms in tetrahedral holes. How many tetrahedral holes are filled with $\mathrm{P}$ atoms in each unit cell? (c) The length of a unit cell of BP is 478 pm. What is the density of the solid in $\mathrm{g} / \mathrm{cm}^{3}$. (d) Calculate the closest distance between a $\mathrm{B}$ and a $\mathrm{P}$ atom in the unit cell. (Assume the B atoms do not touch along the cell edge. The $\mathrm{B}$ atoms in the faces touch the $\mathrm{B}$ atoms at the corners of the unit cell. See page $594 .)$
David Collins Numerade Educator
Problem 2
How much energy is evolved when 1.0 L of water at $0^{\circ} \mathrm{C}$ solidifies to ice? (The heat of fusion of water is $333 \mathrm{J} / \mathrm{g} .)$
Himanshu Garg Numerade Educator
Problem 3
A collapsed balloon is filled with He to a volume of $12.5 \mathrm{L}$ at a pressure of 1.00 atm. Oxygen, $\mathrm{O}_{2},$ is then added so that the final volume of the balloon is $26 \mathrm{L}$ with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is $21.5^{\circ} \mathrm{C}$ (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of $\mathrm{O}_{2}$ in the balloon? (d) What is the mole fraction of each gas?
Vishal Sharma Numerade Educator
Problem 4
Which of the following compounds would be expected to form intermolecular hydrogen bonds in the liquid state? (a) $\mathrm{CH}_{3} \mathrm{OCH}_{3}$ (dimethyl ether) (b) $\mathrm{CH}_{4}$ (c) HF (d) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$ (acetic acid) (e) $\mathrm{Br}_{2}$ (f) $\mathrm{CH}_{3} \mathrm{OH}$ (methanol)
Prashant Bana Numerade Educator
Problem 5
Capsaicin, the compound that gives the hot taste to chili peppers, has the formula $\mathrm{C}_{18} \mathrm{H}_{27} \mathrm{NO}_{3}$ (a) Calculate its molar mass. (b) If you eat 55 mg of capsaicin, what amount (moles) have you consumed? (c) Calculate the mass percent of each element in the compound. (d) What mass of carbon (in milligrams) is there in $55 \mathrm{mg}$ of capsaicin?
Noah Boudrie Numerade Educator
Problem 6
A halothane-oxygen mixture $\left(\mathrm{C}_{2} \mathrm{HBrClF}_{3}+\mathrm{O}_{2}\right)$ can be used as an anesthetic. A tank containing such a mixture has the following partial pressures: $P$ (halothane) $=170 \mathrm{mm}$ Hg and $P\left(\mathrm{O}_{2}\right)=570 \mathrm{mm}$ Hg. (a) What is the ratio of the number of moles of halothane to the number of moles of $\mathrm{O}_{2} ?$ (b) If the tank contains 160 g of $\mathrm{O}_{2}$, what mass of $\mathrm{C}_{2} \mathrm{HBrClF}_{3}$ is present?
Jennifer Hudspeth Numerade Educator
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