Solutions for Chemistry by OpenStax (2015-05-04)
Problem 1E:
In terms of their bulk properties, how do liquids and solids differ? How are they similar?Problem 2E:
In terms of the kinetic molecular theory, in what ways are liquids similar to solids? In what ways...Problem 3E:
In terms of the kinetic molecular theory, in what ways are liquids similar to gases? In what ways...Problem 4E:
Explain why liquids assume the shape of any container into which they are poured, whereas solids are...Problem 5E:
What is the evidence that all neutral atoms and molecules exert attractive forces on each other?Problem 6E:
Open the PhET States of Matter Simulation (http://openstaxcollege.org/l/16phetvisual) to answer the...Problem 7E:
Define the following and give an example of each: (a) dispersion force (b) dipole-dipole attraction...Problem 8E:
The types of intermolecular forces in a substance are identical whether it is a solid, a liquid, or...Problem 10E:
Neon and HF have approximately the same molecular masses. (a) Explain why the boiling points of Neon...Problem 11E:
Arrange each of the following sets of compounds in order of increasing boiling point temperature:...Problem 12E:
The molecular mass of butanol, C4H9OH, is 74.14; that of ethylene glycol, CH2(OH)CH2OH, is 62.08,...Problem 13E:
On the basis of intermolecular attractions, explain the differences in the boiling points of n...Problem 14E:
On the basis of dipole moments and/or hydrogen bonding, explain in a qualitative way the differences...Problem 15E:
The melting point of H2O(s) is O C. Would you expect the melting point of H2S(s) to be 85 C, O C, or...Problem 16E:
Silane SiH4, phosphine (PH3), and hydrogen sulfide (H2S) melt at 185 C, 133 C, and 85 C,...Problem 17E:
Explain why a hydrogen bond between two water molecules is weaker than a hydrogen bond between two...Problem 18E:
Under certain conditions, molecules of acetic acid, CH3COOH, form dimers, pairs of acetic acid...Problem 19E:
Proteins are chains of amino acids that can form in a variety of arrangements, one of which is a...Problem 20E:
The density of liquid NH3 is 0.64 g/mL; the density of gaseous NH3 at STP is 0.0007 g/mL. Explain...Problem 21E:
Identify the intermolecular forces present in the following solids: (a) CH3CH2OH (b) CH3CH2CH3 (c)...Problem 22E:
The test tubes shown here contain equal amounts of the specified motor oils. Identical metal spheres...Problem 23E:
Although steel is denser than water, a steel needle or paper clip placed carefully lengthwise on the...Problem 24E:
The surface tension and viscosity values for diethyl ether, acetone, ethanol, and ethylene glycol...Problem 25E:
You may have heard someone use the figure of speech slower than molasses in winter to describe a...Problem 26E:
It is often recommended that you let your car engine run idle to warm up before driving, especially...Problem 27E:
The surface tension and viscosity of water at several different temperatures are given in this...Problem 28E:
At 25 C, how high will water rise in a glass capillary tube with an inner diameter of 0.63 mm? Refer...Problem 29E:
Water rises in a glass capillary tube to a height of 17 cm. What is the diameter of the capillary...Problem 30E:
Heat is added to boiling water. Explain why the temperature of the boiling water does not change....Problem 31E:
Heat is added to ice at 0 C. Explain why the temperature of the ice does not change. What does...Problem 32E:
What feature characterizes the dynamic equilibrium between a liquid and its vapor in a closed...Problem 33E:
Identify two common observations indicating some liquids have sufficient vapor pressures to...Problem 34E:
Identify two common observations indicating some solids, such as dry ice and mothballs, have vapor...Problem 35E:
What is the relationship between the intermolecular forces in a liquid and its vapor pressure?Problem 36E:
What is the relationship between the intermolecular forces in a solid and its melting temperature?Problem 38E:
Carbon tetrachloride, CCl4, was once used as a dry cleaning solvent, but is no longer used because...Problem 41E:
Use the information in Figure 10.24 to estimate the boiling point of water in Denver when the...Problem 42E:
A syringe at a temperature of 20 C is filled with liquid ether in such a way that there is no space...Problem 43E:
Explain the following observations: (a) It takes longer to cook an egg in Ft. Davis, Texas...Problem 44E:
The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.Problem 45E:
Explain why the molar enthalpies of vaporization of the following substances increase in the order...Problem 46E:
Explain why the enthalpies of vaporization of the following substances increase in the order...Problem 47E:
The enthalpy of vaporization of CO2(l) is 9.8 kJ/mol. Would you expect the enthalpy of vaporization...Problem 48E:
The hydrogen fluoride molecule, HF, is more polar than a water molecule, H2O (for example, has a...Problem 49E:
Ethyl chloride (boiling point, 13 C) is used as a local anesthetic. When the liquid is sprayed on...Problem 50E:
Which contains the compounds listed correctly in order of increasing boiling points? (a) N2CS2H2OKCl...Problem 51E:
How much heat is required to convert 422 g of liquid H2O at 23.5 C into steam at 150 C?Problem 52E:
Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water...Problem 53E:
Titanium tetrachloride, TiCl4, has a melting point of 23.2 C and has a Hfusion=9.37 kJ/mol. (a) How...Problem 54E:
From the phase diagram for water (Figure 10.31), determine the state of water at: (a) 35 °C and 85...Problem 55E:
What phase changes will take place when water is subjected to varying pressure at a constant...Problem 56E:
Pressure cookers allow food to cook faster because the higher pressure inside the pressure cooker...Problem 57E:
From the phase diagram for carbon dioxide in Figure 10.34, determine the state of CO2 at: (a) 20 °C...Problem 58E:
Determine the phase changes that carbon dioxide undergoes as the pressure changes if (lie...Problem 59E:
Consider a cylinder containing a mixture of liquid carbon dioxide in equilibrium with gaseous carbon...Problem 60E:
Dry ice, CO2(s) , does not melt at atmospheric pressure. It sublimes at a temperature of 78 °C. What...Problem 61E:
If a severe storm results in the loss of electricity, it may be necessary to use a clothesline to...Problem 62E:
Is it possible to liquefy nitrogen at room temperature (about 25 C)? Is it possible to liquefy...Problem 63E:
Elemental carbon has one gas phase, one liquid phase, and two different solid phases, as shown in...Problem 65E:
At very low temperatures oxygen, O2, freezes and forms a crystalline solid. Which best describes...Problem 66E:
As it cools, olive oil slowly solidifies and forms a solid over a range of temperatures. Which best...Problem 67E:
Explain why ice, which is a crystalline solid, has a melting temperature of 0C, whereas butter,...Problem 68E:
Identify the type of crystalline solid (metallic, network covalent, ionic, or molecular) formed by...Problem 69E:
Identify the type of crystalline solid (metallic, network covalent, ionic, or molecular) formed by...Problem 70E:
Classify each substance in the table as either a metallic, ionic, molecular, or covalent network...Problem 71E:
Classify each substance in the table as either a metallic, ionic, molecular, or covalent network...Problem 72E:
Identify the following substances as ionic, metallic, covalent network, or molecular solids:...Problem 73E:
Substance A is shiny, conducts electricity well, and melts at 975 C. Substance A is likely a(n): (a)...Problem 74E:
Substance B is hard, does not conduct electricity, and melts at 1200 C. Substance B is likely a(n):...Problem 75E:
Describe the crystal structure of iron, which crystallizes with two equivalent metal atoms in a...Problem 76E:
Describe the crystal structure of Pt, which crystallizes with four equivalent metal atoms in a cubic...Problem 77E:
What is the coordination number of a chromium atom in the body-centered cubic structure of chromium?Problem 78E:
What is the coordination number of an aluminum atom in the facecentered cubic structure of aluminum?Problem 79E:
Cobalt metal crystallizes in a hexagonal closest packed structure. What is the coordination number...Problem 80E:
Nickel metal crystallizes in a cubic closest packed structure. What is the coordination number of a...Problem 81E:
Tungsten crystallizes in a body-centered cubic unit cell with an edge length of 3.165 . (a) What is...Problem 82E:
Platinum (atomic radius =1.38) crystallizes in a cubic closely packed structure. Calculate the edge...Problem 83E:
Barium crystallizes in a body-centered cubic unit cell with an edge length of 3.025 (a) What is the...Problem 84E:
Aluminum (atomic radius = 1.43 ) crystallizes in a cubic closely packed structure. Calculate the...Problem 85E:
The density of aluminum is 2.7 g/cm3; that of silicon is 2.3 g/cm3. Explain why Si has the lower...Problem 86E:
The free space in a metal may be found by subtracting the volume of the atoms in a unit cell from...Problem 87E:
Cadmium sulfide, sometimes used as a yellow pigment by artists, crystallizes with cadmium, occupying...Problem 88E:
A compound of cadmium, tin, and phosphorus is used in the fabrication of some semiconductors. It...Problem 89E:
What is the formula of the magnetic oxide of cobalt, used in recording tapes, that crystallizes with...Problem 90E:
A compound containing zinc, aluminum, and sulfur crystallizes with a closest-packed array of sulfide...Problem 91E:
A compound of thallium and iodine crystallizes in a simple cubic array of iodide ions with thallium...Problem 92E:
Which of the following elements reacts with sulfur to form a solid in which the sulfur atoms form a...Problem 93E:
What is the percent by mass of titanium in rutile, a mineral that contains titanium and oxygen, if...Problem 94E:
Explain why the chemically similar alkali metal chlorides NaCl and CsCl have different structures,...Problem 95E:
As minerals were formed from the molten magma, different ions occupied the same cites in the...Problem 96E:
Rubidium iodide crystallizes with a cubic unit cell that contains iodide ions at the corners and a...Problem 97E:
One of the various manganese oxides crystallizes with a cubic unit cell that contains manganese ions...Problem 98E:
NaH crystallizes with the same ciystal structure as NaCl. The edge length of the cubic unit cell of...Problem 99E:
Thallium(I) iodide crystallizes with the same structure a CsCl. The edge length of the Unit cell of...Problem 100E:
A cubic unit cell contains manganese ions at the corners and fluoride ions at the center of each...Problem 101E:
What is the spacing between crystal planes that diffract X-rays with a wavelength of 1.541 nm at an...Problem 102E:
A diffracrometer using X-rays with a wavelength of 0.2287 nm produced first-order diffraction peak...Problem 103E:
A metal with spacing between planes equal to 0.4164 nm diffracts X-rays with a wavelength of 0.2879...Browse All Chapters of This Textbook
Chapter 1 - Essential IdeasChapter 2 - Atoms, Molecules, And IonsChapter 3 - Composition Of Substances And SolutionsChapter 4 - Stoichiometry Of Chemical ReactionsChapter 5 - ThermochemistryChapter 6 - Electronic Structure And Periodic Properties Of ElementsChapter 7 - Chemical Bonding And Molecular GeometryChapter 8 - Advanced Theories Of Covalent BondingChapter 9 - GasesChapter 10 - Liquids And Solids
Chapter 11 - Solutions And ColloidsChapter 12 - KineticsChapter 13 - Fundamental Equilibrium ConceptsChapter 14 - Acid-base EquilibriaChapter 15 - Equilibria Of Other Reaction ClassesChapter 16 - ThermodynamicsChapter 17 - ElectrochemistryChapter 18 - Representative Metals, Metalloids, And NonmetalsChapter 19 - Transition Metals And Coordination ChemistryChapter 20 - Organic ChemistryChapter 21 - Nuclear Chemistry
Book Details
Chemistry is designed for the two-semester general chemistry course. For many students, this course provides the foundation to a career in chemistry, while for others, this may be their only college-level science course. As such, this textbook provides an important opportunity for students to learn the core concepts of chemistry and understand how those concepts apply to their lives and the world around them. The text has been developed to meet the scope and sequence of most general chemistry courses. At the same time, the book includes a number of innovative features designed to enhance student learning. A strength of Chemistry is that instructors can customize the book, adapting it to the approach that works best in their classroom. This is a full-color textbook.
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Chemistry (OER)
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ISBN: 9781947172623
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