William L. Masterton, Cecile N. Hurley
ISBN #9781305079373
8th Edition
1,898 Questions
Homework Questions
Chemistry Principles and Reactions is a comprehensive textbook that guides readers through the fundamental concepts of chemistry, starting with matter, measurements, and atomic theory and progressing to advanced topics such as thermodynamics, kinetics, and complex equilibria. The book is structured as a logical journey, building on precise measurements and elemental understanding to embed the critical principles behind chemical reactions, from stoichiometry and gas laws to acid–base behavior and organic synthesis. Throughout the text, clear explanations of concepts like molecular geometry, electron configurations, and reaction spontaneity are woven together with practical applications in electrochemistry, nuclear reactions, and materials chemistry. This cohesive framework not only reinforces the theoretical foundations of chemistry but also equips students with the quantitative tools and practical insights essential for mastering the subject.
Chapter 1
Matter and Measurements
Chapter 2
Atoms, Molecules, and lons
Chapter 3
Mass Relations in Chemistry; Stoichiometry
Chapter 4
Reactions in Aqueous Solution
Chapter 5
Gases
Chapter 6
Electronic Structure and the Periodic Table
Chapter 7
Covalent Bonding
Chapter 8
Thermochemistry
Chapter 9
Liquids and Solids
Chapter 10
Solutions
Chapter 11
Rate of Reaction
Chapter 12
Gaseous Chemical Equilibrium
View More
Chapter 13
Acids and Bases
Chapter 14
Equilibria in Acid-Base Solutions
Chapter 15
Complex lon and Precipitation Equilibria
Chapter 16
Spontaneity of Reaction
Chapter 17
Electrochemistry
Chapter 18
Nuclear Reactions
Chapter 19
Complex lons
Chapter 20
Chemistry of the Metals
Chapter 21
Chemistry of the Nonmetals
Chapter 22
Organic Chemistry
Chapter 23
Organic Polymers, Natural and Synthetic
Problem 1
Titanium is a metal used in jet engines. Its specific heat is $0.523 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}$. If $5.88 \mathrm{~g}$ of titanium absorb $4.78 \mathrm{~J}$, what is the change in temperature?
Pronoy Sinha Numerade Educator
Problem 2
Two basic laws of chemistry are the law of conservation of mass and the law of constant composition. Which of these laws (if any) do the following statements illustrate? (a) Lavoisier found that when mercury(II) oxide, $\mathrm{HgO}$, decomposes, the total mass of mercury $(\mathrm{Hg})$ and oxygen formed equals the mass of mercury(II) oxide decomposed. (b) Analysis of the calcium carbonate found in the marble mined in Carrara, Italy, and in the stalactites of the Carlsbad Caverns in New Mexico gives the same value for the percentage of calcium in calcium carbonate. (c) Hydrogen occurs as a mixture of two isotopes, one of which is twice as heavy as the other.
Dr. Satish Ingale Numerade Educator
Problem 3
Gold has a specific heat of $0.129 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}$. When a $5.00-\mathrm{g}$ piece of gold absorbs $1.33 \mathrm{~J}$ of heat, what is the change in temperature?
Problem 4
One chocolate chip used in making chocolate chip cookies has a mass of $0.324 \mathrm{~g}$. (a) How many chocolate chips are there in one mole of chocolate chips? (b) If a cookie needs 15 chocolate chips, how many cookies can one make with a billionth $\left(1 \times 10^{-9}\right)$ of a mole of chocolate chips? (A billionth of a mole is scientifically known as a nanomole.)
Margarita Fong Numerade Educator
Problem 5
Classify each of the following as element, compound, or mixture. (a) air (b) iron (c) soy sauce (d) table salt
Narayan Hari Numerade Educator
Problem 6
Benzene, a known carcinogen, was once widely used as a solvent. A sample of benzene vapor in a flask of constant volume exerts a pressure of $325 \mathrm{~mm} \mathrm{Hg}$ at $80^{\circ} \mathrm{C}$. The flask is slowly cooled. (a) Assuming no condensation, use the ideal gas law to calculate the pressure of the vapor at $50^{\circ} \mathrm{C} ;$ at $60^{\circ} \mathrm{C}$. (b) Compare your answers in (a) to the equilibrium vapor pressures of benzene: $269 \mathrm{~mm} \mathrm{Hg}$ at $50^{\circ} \mathrm{C}$, $389 \mathrm{~mm} \mathrm{Hg}$ at $60^{\circ} \mathrm{C}$ (c) On the basis of your answers to (a) and (b), predict the pressure exerted by the benzene at $50^{\circ} \mathrm{C}$; at $60^{\circ} \mathrm{C}$.
Eileen Sullivan Numerade Educator
WHAT OUR STUDENTS SAY
“I finally understand my textbook questions. Before Numerade, I’d skip hard problems. Now I get instant help with videos that explain everything simply.”
Edwin V. Penn State Freshman