Steven S. Zumdahl, Susan A. Zumdahl
ISBN #9781305079243
2nd Edition
2,858 Questions
Homework Questions
Chemistry An Atoms First Approach is a comprehensive text that begins with the evolution of atomic theory and builds a solid foundation in chemical principles through the exploration of atomic structure, periodic trends, and chemical bonding. The book methodically integrates core concepts like reaction stoichiometry, kinetics, thermodynamics, and equilibrium with practical applications ranging from industrial chemistry to environmental and biological systems. By interweaving historical experiments with modern theories, it offers a unique glimpse into the microscopic world, empowering students to understand and predict the behavior of matter at the atomic level.
Chapter 1
Chemical Foundations
Chapter 2
Atomic Structure and Periodicity
Chapter 3
Bonding: General Concepts
Chapter 4
Molecular Structure and Orbitals
Chapter 5
Stoichiometry
Chapter 6
Types of Chemical Reactions and Solution Stoichiometry
Chapter 7
Chemical Energy
Chapter 8
Gases
Chapter 9
Liquids and Solids
Chapter 10
Properties of Solutions
Chapter 11
Chemical Kinetics
Chapter 12
Chemical Equilibrium
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Chapter 13
Chapter 14
Acid-Base Equilibria
Chapter 15
Solubility and Complex lon Equilibria
Chapter 16
Spontaneity, Entropy, and Free Energy
Chapter 17
Electrochemistry
Chapter 18
The Nucleus: A Chemist's View
Chapter 19
The Representative Elements
Chapter 20
Transition Metals and Coordination Chemistry
Chapter 21
Organic and Biological Molecules
Problem 1
The following are actual student responses to the question: Why is it necessary to balance chemical equations? a. The chemicals will not react until you have added the correct mole ratios. b. The correct products will not be formed unless the right amount of reactants have been added. c. A certain number of products cannot be formed without a certain number of reactants. d. The balanced equation tells you how much reactant you need and allows you to predict how much product you'll make. e. A mole-to-mole ratio must be established for the reaction to occur as written. Justify the best choice, and for choices you did not pick, explain what is wrong with them.
Joanna Josey Numerade Educator
Problem 2
You are making cookies and are missing a key ingredienteggs. You have most of the other ingredients needed to make the cookies, except you have only 1.33 cups of butter and no eggs. You note that the recipe calls for two cups of butter and three eggs (plus the other ingredients) to make six dozen cookies. You call a friend and have him bring you some eggs. a. What number of eggs do you need? b. If you use all the butter (and get enough eggs), what number of cookies will you make? Unfortunately, your friend hangs up before you tell him how many eggs you need. When he arrives, he has a surprise for you- -to save time, he has broken them all in a bowl for you. You ask him how many he brought, and he replies, "I can't remember." You weigh the eggs and find that they weigh $62.1 \mathrm{g}$. Assuming that an average egg weighs $34.21 \mathrm{g}$ a. What quantity of butter is needed to react with all the eggs? b. What number of cookies can you make? c. Which will you have left over, eggs or butter? d. What quantity is left over?
Problem 3
Assume you have a highly magnified view of a solution of HCI that allows you to "see" the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear and hydrogen gas would be released. Represent this change using symbols for the elements, and write out the balanced equation.
Iva Lazarova Numerade Educator
Problem 4
A fire is started in a fireplace by striking a match and lighting crumpled paper under some logs. Explain all the energy transfers in this scenario using the terms exothermic, endothermic, system, surroundings, potential energy, and kinetic energy in the discussion.
Jeffrey Aglow Numerade Educator
Problem 5
Figure $8-2$ shows a picture of a barometer. Which of the following statements is the best explanation of how this barometer works? a. Air pressure outside the tube causes the mercury to move in the tube until the air pressure inside and outside the tube is equal. b. Air pressure inside the tube causes the mercury to move in the tube until the air pressure inside and outside the tube is equal. c. Air pressure outside the tube counterbalances the weight of the mercury in the tube. d. Capillary action of the mercury causes the mercury to go up the tube. e. The vacuum that is formed at the top of the tube holds up the mercury. Justify your choice, and for the choices you did not pick, explain what is wrong with them. Pictures help!
Cathy Geisel Numerade Educator
Problem 6
Consider a sealed container half-filled with water. Which statement best describes what occurs in the container? a. Water evaporates until the air is saturated with water vapor; at this point, no more water evaporates. b. Water evaporates until the air is overly saturated (supersaturated) with water, and most of this water recondenses; this cycle continues until a certain amount of water vapor is present, and then the cycle ceases. c. Water does not evaporate because the container is sealed. d. Water evaporates, and then water evaporates and recondenses simultaneously and continuously. e. Water evaporates until it is eventually all in vapor form. Explain each choice. Justify your choice, and for choices you did not pick, explain what is wrong with them.
Kevin Zaborsky Numerade Educator
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