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chemistry principles and practice

Questions and Answers of Chemistry Principles And Practice

A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 °C.(a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the ideal gas law,
Why do free-floating liquids in an orbiting spacecraft adopt a spherical shape?
What is the volume change when 1 mol of graphite (d = 2.26 g/cm3) is converted to diamond (d = 3.51 g/cm3)?
The metallic bonding found in the element gold is such that 1.00 ounce of Au can be flattened into a sheet that is 3.00 × 102 ft2. If there are 28.35 g/ounce and 30.48 cm/ft, how thin is this sheet?
Predict the types of intermolecular forces important for the following substances.(a) He(b) CH3OCH3(c) C2ClF5 Correlate the enthalpies of vaporization listed below with each of these substances. 1.
Indicate which type of bonding is expected for the following crystalline substances.(a) N2O(b) GeO2(c) CaCl2Correlate the properties below with each of these substances.1. Melting point = -90.8
The edge of the face-centered cubic unit cell of copper is 362 pm long. Assume that the copper atoms are spheres that are in contact along the diagonal of the face of the cube. Find the radius of a
X rays with a wavelength of 1.790 × 10-10 m are diffracted at an angle of 14.7 degrees by a crystal of KI.(a) What is the spacing between layers in the crystal that gives rise to this angle of
Avogadro’s number can be calculated quite accurately from the density of a solid and crystallographic data. Europium (molar mass = 151.94 g/mol) has a body centered cubic array of atoms in which
The coordination number of uniformly sized spheres in a cubic closest-packing (FCC) array is 12. Give the coordination number of each atom in(a) A simple cubic lattice.(b) A body-centered cubic
Which of the following pairs are allotropes?(a) Oxygen gas (O2) and ozone gas (O3)(b) Liquid oxygen (O2) and oxygen gas (O2)(c) Amorphous silicon dioxide and quartz (crystalline silicon dioxide)
What is the wavelength of x rays in which the first-order diffraction occurs at 16.5 degrees from layers of atoms spaced 315 pm apart?
What is the wavelength of x rays in which the first-order diffraction occurs at 13.4 degrees from layers of atoms spaced 232 pm apart?
At what angle does first-order diffraction from layers of atoms 325 pm apart occur, using x rays with a wavelength of 179 pm?
At what angle does first-order diffraction from layers of atoms 293 pm apart occur, using x rays with a wavelength of 154 pm?
Which of the following materials should produce well defined x-ray diffraction patterns?(a) Polyethylene(b) Liquid ethanol(c) CaO(d) A diamond
Which of the following materials should produce well defined x-ray diffraction patterns?(a) KBr(b) Liquid H2O(c) Glass(d) A sugar crystal
Chromium has a cubic crystal structure in which the edge of the unit cell is 288 pm long. If the density of chromium is 7.20 g/cm3, how many chromium atoms are in a unit cell? In which of the cubic
Palladium has a cubic crystal structure in which the edge of the unit cell is 389 pm long. If the density of palladium is 12.02 g/cm3, how many palladium atoms are in a unit cell? In which of the
Cesium iodide crystallizes as a simple cubic array of iodide ions with a cesium ion in the center of the cell. The edge of this unit cell is 445 pm long. Calculate the density of CsI.
Lithium hydride (LiH) has the sodium chloride structure, and the length of the edge of the unit cell is 4.086 × 10-8 cm. Calculate the density of this solid.
Polonium crystallizes in a simple cubic unit cell with an edge length of 336 pm.(a) What is the mass of the unit cell?(b) What is the volume of the unit cell?(c) What is the theoretical density of
Nickel crystallizes in a face-centered cubic array of atoms in which the length of the unit cell’s edge is 351 pm. Calculate the density of this metal.
Calcium fluoride (fluorite) has a unit cell with Ca2+ ions in a face-centered cubic arrangement. How many fluoride ions are present in each unit cell? (Remember that the ratio of fluoride ions to
In the rutile structure of TiO2, the unit cell has a titanium ion in the center of the unit cell and a titanium ion at each of the eight corners. How many oxide ions are present in each unit cell?
Solid xenon forms crystals with a face-centered cubic unit cell that has an edge of 620 pm. Calculate the atomic radius of xenon.
Iron crystallizes in a body-centered cubic array of atoms and has a density of 7.875 g/cm3.(a) What is the length of the edge of the unit cell?(b) Assuming that the atoms are spheres in contact along
Silver crystallizes in a cubic close-packing (FCC) array of atoms. How many silver atoms are present in each unit cell?
How many atoms of tungsten are present in each unit cell of that metal, if it crystallizes in a body-centered cubic array of atoms?
Calcium oxide consists of a face-centered cubic array of O2- ions, with Ca2+ ions at the center of the unit cell and along the centers of all 12 edges. Calculate the number of each ion in the unit
Ammonium chloride consists of a simple cubic array of Cl- ions, with an NH+4 ion at the center of the unit cell. Calculate the number of ammonium ions and chloride ions in each unit cell.
Silicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?
Two of the Group 4A oxides, CO2 and SiO2, have very different melting points. What is the difference in their crystal forces that accounts for the very large difference in their melting points?
Arrange the following substances in order of increasing strength of the crystal forces: He, NH3, NO2, NaBr, BaO.
Identify the kinds of forces that are most important in holding the particles together in a crystalline solid sample of each of the following substances.(a) Kr(b) HF(c) K2O(d) CO2(e) Zn(f) NH3
Identify the kinds of forces that are most important in holding the particles together in a crystalline solid sample of each of the following substances.(a) H2O(b) C6H6(c) CaCl2(d) SiO2(e) Fe
Arrange the liquids ethanol (C2H5OH), glycerol [HOCH2CH(OH)CH2OH], and ethylene glycol (CH2OH)2 in decreasing order of expected viscosities.
Arrange the liquids hexane (C6H14), ethanol (C2H5OH), and ethylene glycol [(CH2OH)2] in order of increasing expected surface tensions.
Select the liquid in each part that has the greater expected enthalpy of vaporization.(a) C3H8 or CH4(b) I2 or ICl(c) S2Cl2 or S2F2(d) H2Se or H2O(e) CH2Cl2 or CH3Cl(f) NOF or NOCl
Identify the types of all the intermolecular forces that cause each of the following gases to condense to a liquid when cooled.(a) N2O(b) CH4(c) NH3(d) SO2
In each part, select the substance that has the greater boiling point, based on the relative strengths of the intermolecular attractions.(a) C2H4 or CH4(b) Cl2 or ClF(c) S2F2 or S2Cl2(d) NH3 or
Identify the kinds of intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding) that are important in each of the following substances.(a) Propane (C3H8)(b) Ethylene glycol
Describe how the equilibrium system responds to the change described in each of the following parts.(a) The pressure on a solid in equilibrium with its vapor is increased abruptly at constant
Answer the following questions by using the phase diagram in Exercise 11.44.(a) Sketch the heating curve that is expected when heat is added to the sample at constant pressure, starting at point
Use the accompanying phase diagram to do the following:(a) Label each region of the diagram with the phase that is present.(b) Identify the phase or phases present at each of the points G, H, J, and
Use the accompanying phase diagram to do the following:(a) Label each region of the diagram with the phase that is present.(b) Identify the phase or phases present at each of the points A, B, C, D,
The normal melting point of iodine is 113.5 °C, and its normal boiling point is 184.3 °C. The triple point occurs at 92.3 torr and 113.4 °C, and the critical point is 512 °C at 112 atm. Sketch
There are two allotropic forms of the element tin, called gray tin and white tin. The density of gray tin is 5.75 g/cm3, and that of white tin is 7.28 g/cm3. Determine which allotropic form of tin is
Using the same x-ray source, a different crystal diffracts x rays at an angle of 12.3 degrees. Using n = 1, calculate the distance between the layers of atoms that produce this diffraction.
Draw the delocalized orbital for benzene. Clearly indicate the atomic orbitals that form the molecular orbital.
In Exercise 10.25 , the shapes of the following molecules were determined. State whether each molecule is polar or nonpolar.(a) CF4(b) CS2(c) AsF5(d) F2COExercise 10.25Use the VSEPR model to
Show the orbital diagram for each of the answers in Exercise 7.71.Exercise 7.71For all elements with Z ≤ 10, write the electron configuration for(a) Those that have two unpaired electrons.(b) The
A solution of 1.00 g of a protein in 20.0 mL water has an osmotic pressure of 35.2 torr at 298 K. Calculate the molar mass of the protein.
The molar mass of a polymer was determined by measuring the osmotic pressure, 7.6 torr, of a solution containing 5.0 g of the polymer dissolved in 1.0 L benzene. What is the molar mass of the
Arrange the following aqueous solutions in order of increasing boiling points: 0.02 m LiBr, 0.03 m sucrose, 0.03 m MgSO4, 0.03 m CaCl2, and 0.025 m (NH4)2Cr2O7.
Arrange the following solutions in order of decreasing osmotic pressure: 0.10 M urea, 0.06 M NaCl, 0.05 M Ba(NO3)2, 0.06 M sucrose, and 0.04 M KMnO4.
A sample of seawater freezes at -2.01 °C. What is the total molality of solute particles? If we assume that all of the solute is NaCl, how many grams of that compound are present in 1 kg of water?
An aqueous solution of sodium bromide freezes at -1.61 °C. What is the total molality of solute particles? How many grams of sodium bromide are present in 1 kg of water? (Assume an ideal value for
A solution of 6.3 g calcium chloride in 1.20 kg water is prepared. Assuming an ideal value for the van’t Hoff i, calculate the boiling point of this solution.
A 3.4-g sample of CaCl2 is dissolved in water to give 500 mL of solution at 298 K. What is the osmotic pressure of this solution? (Assume an ideal value for the van’t Hoff factor.)
The saline solution used for intravenous injections contains 8.5 g NaCl in 1.00 kg water. Assuming an ideal value for the van’t Hoff i, calculate the freezing point of this solution.
An 8.5-g sample of NaCl is dissolved in water to give 1.00 L of solution at 298 K. What is the osmotic pressure of this solution? (Assume an ideal value for the van’t Hoff factor.)
A 0.010-molar solution of sodium chloride is separated from pure water by a semipermeable membrane at 298 K. In which direction does net transport of water occur across the membrane when the applied
A 0.010-molar solution of calcium chloride is separated from pure water by a semipermeable membrane at 298 K. In which direction does net transport of water occur across the membrane when the applied
A 0.029 M solution of potassium sulfate has an osmotic pressure of 1.79 atm at 25 °C.(a) Calculate the van’t Hoff factor, i, for this solution.(b) Would the van’t Hoff factor be larger,
The freezing point of a 0.031-m solution of copper(II) sulfate in water is -0.075 °C.(a) Calculate the van’t Hoff factor, i, for this solution.(b) Would the van’t Hoff factor be larger, smaller,
A mixture contains 15.0 g hexane (C6H14) and 20.0 g heptane (C7H16). At 40 °C, the vapor pressure of hexane is 278 torr and that of heptane is 92.3 torr. Assume that this is an ideal solution.(a)
A mixture contains 25.0 g cyclohexane (C6H12) and 44.0 g 2-methylpentane (C6H14). At 35 °C, the vapor pressure of cyclohexane is 150 torr and that of 2-methylpentane is 313 torr. Assume that this is
At a pressure of 760 torr, acetic acid (CH3COOH; boiling point = 118.1 °C) and 1,1-dibromoethane (C2H4Br2; boiling point = 109.5 °C) form an azeotropic mixture, boiling at 103.7 °C, that is 25% by
Typical dinner wines are 9.00% alcohol by volume, which corresponds to 7.23% alcohol by mass. The density of the solution is 0.9877 g/mL. Express the alcohol concentration as(a) Molality.(b) Mole
At a pressure of 760 torr, formic acid (HCO2H; boiling point = 100.7 °C) and water (H2O; boiling point = 100.0 °C) form an azeotropic mixture, boiling at 107.1 °C, that is 77.5% by mass formic
Give quantitative directions for preparing a 0.0520-m aqueous solution of sodium carbonate. Assuming an ideal van’t Hoff factor, what is the expected freezing point of this solution?
Predict the relative solubility of each compound in the two solvents, based on the intermolecular attractions.(a) Is potassium iodide more soluble in water or in methylene chloride (CH2Cl2)?(b) Is
The enthalpy of solution of potassium perchlorate (KClO4) is 51.0 kJ/mol. Compare the solubilities of this compound at 25 °C and at 92 °C.
At 10 °C, the solubility of CO2 gas in water is 0.240 g per 100 mL water at a pressure of 1.00 atm. A soft drink is saturated with carbon dioxide at 4.00 atm and sealed.(a) What mass of carbon
The vapor pressure of trichloroethane (C2H3Cl) is 100 torr at 20.0 °C. What is the vapor pressure of trichloroethane, at 20.0 °C, above a solution containing 2.00 g ferrocene [Fe(C5H5)2, which is
A 0.325-g sample of dark red crystalline compound dissolves in 12.2 g ethylene dibromide, giving a solution that freezes at 7.97 °C. Ethylene dibromide has a normal freezing point of 9.80 °C and a
A reverse osmosis unit is used to obtain drinkable water from a source that contains 500 ppm sodium chloride (0.500 g NaCl per liter). What is the minimum pressure that must be applied across the
Sketch graphs of total vapor pressure versus the mole fraction of two volatile substances that show(a) Positive deviation from Raoult’s law.(b) Pegative deviation from Raoult’s law.(c) A maximum
A 2.00% solution of H2SO4 in water freezes at -0.796 °C.(a) Calculate the van’t Hoff factor, i.(b) Which of the following best represents sulfuric acid in a dilute aqueous solution: H2SO4, H+ +
A 51.0-mL sample of a gas at 745 torr and 25 °C has a mass of 0.262 g. The entire gas sample dissolves in 12.0 g water, forming a solution that freezes at -0.61 °C.(a) Calculate the molar mass of
Hemoglobin contains 0.33% Fe by mass. A 0.200-g sample of hemoglobin is dissolved in water to give 10.0 mL of solution, which has an osmotic pressure of 5.5 torr at 25 °C. How many moles of Fe atoms
A benzene solution and a water solution of acetic acid (CH3CO2H; molar mass = 60.05 g/mol) are both 0.50 mass percent acid. The freezing-point depression of the benzene solution is 0.205 °C, and
A 10.00-mL sample of a 24.00% solution of ammonium bromide (NH4Br) requires 23.41 mL of 1.200 molar silver nitrate (AgNO3) to react with all of the bromide ion present.(a) Calculate the molarity of
A white crystalline compound is analyzed and found to have the following composition: 33.8% Na, 17.7% C, 47.0% O.(a) Calculate the empirical formula of this compound.(b) A solution is made by
The ethoxide ion, C2H5O-, is a strong base. It is similar to hydroxide, OH-, but with the hydrogen atom in hydroxide replaced by the C2H5 group. When mixed with water, the salt sodium ethoxide will
The normal melting point of dinitrogen tetroxide is -9.3 °C, and its normal boiling point is 21.0 °C. The triple point occurs at 140 torr and -10.9 °C, and the critical point is 158 °C at 100
What is the enthalpy change when 50.8 g butane condenses at its boiling point of -0.6 °C? The enthalpy of vaporization of C4H10 is 22.3 kJ/mol. Is this process exothermic or endothermic?
What is the enthalpy change when a 1.00-kg block of dry ice, CO2(s), sublimes at -78 °C? The enthalpy of sublimation of CO2(s) is 26.9 kJ/mol. Is this process exothermic or endothermic?
Calculate the amount of heat required to convert 70.0 g of ice at 0 °C to liquid water at 100 °C. The specific heat of liquid water is 4.184 J/mol · K.
How much energy is needed to melt 100.0 g H2O(s) at its melting point if its enthalpy of fusion is 6.01 kJ/mol? Is this process exothermic or endothermic?
Dichlorobenzene (mothballs) has an enthalpy of fusion of 17.2 kJ/mol and an enthalpy of sublimation of 68.3 kJ/mol. What is the enthalpy of vaporization for this compound?
The enthalpy of sublimation of iodine is 60.2 kJ/mol, and its enthalpy of vaporization is 45.5 kJ/mol. What is the enthalpy of fusion of iodine?
The critical temperature of nitrogen dioxide (NO2) is 158 °C, and that of dinitrogen monoxide (N2O) is 37 °C.(a) Which of these compounds has the stronger intermolecular attractions?(b) Based on
The critical temperature of butane, the fuel in cigarette lighters, is 152 °C, and that of benzene, a useful organic solvent, is 289 °C.(a) Which of these compounds has the stronger intermolecular
Diethyl ether, a substance once used by physicians as a general anesthetic, and n-butanol both have the molecular formula C4H10O. At 25 °C, the vapor pressure of diethyl ether is 530 torr, and that
Isopropanol (rubbing alcohol) and methyl ethyl ether both have the same molecular formula, C3H8O. At 0 °C, the vapor pressure of isopropanol is 8.4 torr, and that of methyl ethyl ether is 560
Explain how the vapor pressure of a liquid changes with each of the following changes.(a) The surface area of the liquid decreases from 50 to 10 cm2 when the liquid is poured into a container with a
Explain how the vapor pressure of a liquid changes with each of the following changes.(a) The surface area of the liquid is increased from 1 to 10 cm2 when the liquid is poured into a container with
Derive the relation between the radius of the atoms and the length of the unit-cell edge for the simple cubic, body-centered cubic, and face-centered cubic cells.

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