Chemistry 10th Edition International Edition by Kenneth W - Test Bank.

Chapter 1—The Foundations of Chemistry MULTIPLE CHOICE 1. Which of the following statements is incorrect? a. A body in motion possesses kinetic energy because of its motion. b. An object possesses potential energy because of its position or composition. c. Nuclear energy is an important kind of potential energy. d. Chemical reactions and physical changes that release energy to their surroundings are endothermic. e. The Law of Conservation of Matter and Energy states that the combined amount of matter and energy in the universe is fixed. ANS: D OBJ: Define the Laws of Conservation of matter and energy. | Define the terms endothermic and exothermic. | Classify energy as potential or kinetic. TOP: Matter and Energy 2. A braking automobile converts kinetic energy into heat in the brake pads. This is an example of the: a. law of conservation of energy b. law of constant composition c. law of conservation of matter d. law of multiple proportions e. law of gravity ANS: A OBJ: Apply the law of conservation of energy. TOP: Matter and Energy 3. When magnesium is burned in air the mass of the product is heavier than the original mass of the magnesium. However, the product formed still has the same exact mass of magnesium with the remainder of the mass being oxygen. This is an example of: a. law of conservation of energy b. law of definite proportions c. law of conservation of matter d. law of multiple proportions e. law of gravity ANS: C OBJ: Apply the law of conservation of energy. TOP: Matter and Energy 4. Which of the following represents matter that could be described as macroscale? a. a bromine atom b. molecules of water c. bacteria observed under a microscope d. a paperclip e. none of these ANS: D OBJ: Classify a description of matter as atomic-, micro-, or macro-scale. TOP: Chemistry – A Molecular View of Matter Whitten 10e Test Bank 1 5. Dalton's Atomic Theory included all of the ideas listed below except: a. Atoms cannot be created or destroyed. b. An element is composed of very small particles called protons, neutrons and electrons. c. All atoms of a given element have identical properties. d. All atoms of a given element have properties that differ from those of other elements. e. Compounds are formed when atoms of different elements combine with one another in small whole-number ratios. ANS: B OBJ: Identify the tenets of Dalton's atomic theory. TOP: Chemistry – A Molecular View of Matter 6. Atoms consist of three fundamental particles. What are these particles and their charges? a. proton (+1), neutron (neutral) and electron (1) b. proton (1), neutron (+1) and electron (neutral) c. proton (+1), neutron (1) and electron (neutral) d. proton (neutral), neutron (+1) and electron (1) e. proton (1), neutron (neutral) and electron (+1) ANS: A OBJ: Identify the three subatomic particles that make up an atom. TOP: Chemistry – A Molecular View of Matter 7. One of the following does not describe gases. Which one is it? a. Expands infinitely. b. Rigid shape. c. Easily compressed. d. Relatively low densities. e. Particles far apart. ANS: B OBJ: Classify a gas. TOP: States of Matter 8. One of the following does not describe solids. Which one is it? a. Particles in definite positions. b. Definite shape. c. Easily compressed. d. Relatively high densities. e. Particles compact. ANS: C OBJ: Classify a solid. TOP: States of Matter 9. Which response lists characteristics of liquids? I. II. III. IV. V . Volume does not vary much upon heating. Shape is constant. Easily compressed. Fills the container completely. Flows. Whitten 10e Test Bank 2 a. I, III, IV, and V b. II, III, and V c. I d. I, II, IV, and IV e. IandV ANS: OBJ: TOP: 10. All of a. It b. It c. It d. It E Classify a liquid. States of Matter the following are properties of antimony. Which one is not a physical property? is a solid at room temperature. has both yellow and gray forms (allotropes) in the solid state. burns in an atmosphere of chlorine. is one of the few substances that expands upon freezing. e. The gray form melts at 631C. ANS: C OBJ: Classify a property as physical or chemical. TOP: Chemical and Physical Properties 11. The following properties describe zinc. Which one(s) is (are) chemical properties? I. It is bluish-white metal. II. It corrodes upon prolonged contact with moist air. 3 III. Its density is 7.14 g/cm . IV. It melts at 419C. V. It conducts electricity. a. IVandV b. IV c. V d. II, IV, and V e. II ANS: OBJ: TOP: 12. All of a. It b. It c. It d. It E Classify a property as physical or chemical. Chemical and Physical Properties the following are properties of oxygen. Which one is a physical property? supports combustion. condenses to a liquid at 219C and atmospheric pressure. causes iron to rust. reacts with calcium to produce calcium oxide, CaO. e. All of these are physical properties. ANS: B OBJ: Classify a property as physical or chemical. TOP: Chemical and Physical Properties Whitten 10e Test Bank 3 13. The following statements describe some physical and chemical properties of sucrose (table sugar). Which response includes all that describe chemical properties, and none that describe physical properties? I. It is a colorless solid. II. It chars or blackens when heated gently. III. Its density is 1.6 g/mL. IV. It ignites and burns with a yellow flame when heated strongly. V. It is usually in the form of small crystals although it can occur as a powder. a. I, III, and IV b. II and IV c. II, IV, and V d. IandV e. another combination is the answer ANS: B OBJ: Classify a property as physical or chemical. TOP: Chemical and Physical Properties 14. Which of the following is not an intensive property of matter? a. color b. density c. melting point d. weight e. boiling point ANS: D OBJ: Classify a property as intensive or extensive. TOP: Chemical and Physical Properties 15. Which of the following is an extensive property of matter? a. weight b. melting point c. specific gravity d. color e. density ANS: A OBJ: Classify a property as intensive or extensive. TOP: Chemical and Physical Properties 16. Identify which of the following properties of methane would be observed only with a change in composition. a. The melting point is 182.5C. 4 3 b. The density is 6.67  10 g/cm . c. Carbon dioxide forms when it burns. d. The boiling point is 161.5C. e. It dissolves slightly in water. ANS: C OBJ: Classify a property as chemical or physical. TOP: Chemical and Physical Properties Whitten 10e Test Bank 4 17. Which response includes all of the following that involve chemical changes, and none that involve physical changes? I. converting milk to cheese II. converting water to steam III. composting leaves IV. burning of gasoline V. melting wax a. IIandV b. I, III, and IV c. I, II, and III d. IVandV e. III, IV , and V ANS: B OBJ: Classify a property as chemical or physical. TOP: Chemical and Physical Changes 18. Which answer includes all of the following that are physical changes and no chemical changes? I. the electrolysis of molten sodium chloride to produce metallic sodium and gaseous chlorine II. the solidification of mercury by cooling III. the reaction of hydrochloric acid with calcium carbonate IV. the mixing of water with ethyl alcohol V. cutting an iron bar into small pieces a. I and III b. II, IV, and V c. IandIV d. II, III, and V e. IV ANS: B OBJ: Classify a property as chemical or physical. TOP: Chemical and Physical Changes 19. Which of these physical changes would require the liberation of energy? a. condensation of steam to form liquid water b. melting of ice c. boiling of water d. all of these e. none of these ANS: A OBJ: Identify physical changes as endothermic or exothermic. TOP: Chemical and Physical Changes 20. Which of the following changes in water represents a chemical change? a. Melting of ice. b. Boiling water. c. Sublimation of solid ice directly to gaseous water. d. Electrolyzing water to produce hydrogen and oxygen. e. Heating water from 25C to 60C. Whitten 10e Test Bank 5 ANS: D OBJ: Classify changes as chemical or physical. TOP: Chemical and Physical Changes 21. Which answer lists all the substances below that are compounds and not any elements or mixtures? I ethanol II. neon III. bromine IV. water V. crude oil a. I, II, and III b. I,IV,andV c. IVandV d. II, III, and V e. IandIV ANS: E OBJ: Classify a substance as an element, compound, or mixture. TOP: Mixtures, Substances, Compounds, and Elements 22. Which of the following is not a mixture? a. air b. steel c. soda d. gasoline e. nitrogen ANS: E OBJ: Distinguish between examples of pure substances and mixtures. TOP: Mixtures, Substances, Compounds, and Elements 23. Crude oil can be separated into gasoline, diesel, heating oil, etc. by differences in boiling points. The form of matter which would best describe crude oil is: a. homogeneous mixture b. heterogeneous mixture c. compound d. mineral e. element ANS: A OBJ: Classify matter. TOP: Mixtures, Substances, Compounds, and Elements 24. Which statement is false? a. A compound is a substance that can be decomposed by chemical means into simpler substances. b. All samples of a particular pure substance have the same composition and properties. c. An example of a homogeneous mixture is one prepared by mixing two liquids, ethyl alcohol (grain alcohol) and water. d. An example of a heterogeneous mixture is one prepared by dissolving the solid, sodium chloride (table salt), in the liquid, water. e. Different mixtures of the same two substances can have different compositions. Whitten 10e Test Bank 6 ANS: D OBJ: Define elements, compounds, or mixtures. | Classify matter. TOP: Mixtures, Substances, Compounds, and Elements 25. Which of the following is a compound? a. cola b. air c. mercury d. gasoline e. calcium fluoride ANS: E OBJ: Identify elements, compounds, and mixtures. TOP: Mixtures, Substances, Compounds, and Elements 26. Which mixture is incorrectly labeled? a. homogeneous / sugar dissolved in water b. homogeneous / sand stirred into water c. heterogeneous / orange juice with pulp d. heterogeneous / chocolate chip cookie e. heterogeneous / concrete sidewalk ANS: B OBJ: Classify a mixture as homogeneous or heterogeneous. TOP: Mixtures, Substances, Compounds, and Elements 27. A sample of matter that can be decomposed into three different elements a. must be a solution. b. must be a compound. c. must be a heterogeneous mixture. d. must be a homogeneous mixture. e. could be any of these answers. ANS: E OBJ: Classify matter. TOP: Mixtures, Substances, Compounds, and Elements 28. A form of matter is isolated and tested. No physical procedures can produce simpler forms of matter but heating the sample produces mercury and oxygen. The sample of matter must be: a. element b. compound c. solution d. mixture e. molecule ANS: B OBJ: Classify matter. TOP: Mixtures, Substances, Compounds, and Elements 29. What is the symbol for the element potassium? a. K b. P c. Pt d. W e. Po ANS: A OBJ: Identify the symbol representing an element. TOP: Mixtures, Substances, Compounds, and Elements 30. The element whose symbol is Ca is Whitten 10e Test Bank 7 a. carbon. b. cadmium. c. calcium. d. californium. e. none of these. ANS: C OBJ: Identify an element name given the symbol. TOP: Mixtures, Substances, Compounds, and Elements 31. What is the symbol for the element magnesium? a. Mg b. Fe c. Mn d. Mo e. Hg ANS: A OBJ: Identify the symbol representing an element. TOP: Mixtures, Substances, Compounds, and Elements 32. Which element / symbol pair is incorrect? a. Fe / iron b. Ca / calcium c. Ag / gold d. Pb / lead e. O / oxygen ANS: C OBJ: Identify the incorrect symbol/element name combination. TOP: Mixtures, Substances, Compounds, and Elements 33. Identify which of the following statements about elements and their abundance is false? a. Each element has its own unique symbol. b. Oxygen and silicon are very common. c. More than 99% of the Earth's mass is made up of only 10 of the naturally occurring elements. d. Most elements occur in nature as free elements, not in compounds. e. Gold is very uncommon. ANS: D OBJ: Know the qualitative abundance of the elements, the form of their occurrence in nature, and the terminology of the periodic table. TOP: Mixtures, Substances, Compounds, and Elements Whitten 10e Test Bank 8 34. What is the symbol for the element strontium? a. Si b. S c. Sr d. Se e. Sm ANS: C OBJ: Identify the symbol representing an element. TOP: Mixtures, Substances, Compounds, and Elements 35. The element whose symbol is Br is a. boron. b. barium. c. bromine. d. berkelium. e. beryllium. ANS: C OBJ: Identify the element name given the symbol. TOP: Mixtures, Substances, Compounds, and Elements 36. The element whose symbol is Sn is a. silver. b. sulfur. c. tin. d. samarium. e. strontium. ANS: C OBJ: Identify the element name given the symbol. TOP: Mixtures, Substances, Compounds, and Elements 37. Which symbol / name combination is incorrect? a. Mn / manganese b. Zn / zinc c. Sn / tin d. Sr / strontium e. Pd / lead ANS: E OBJ: Identify the incorrect symbol/element name combination. TOP: Mixtures, Substances, Compounds, and Elements 38. Which name / symbol combination is incorrect? a. aluminum / Al b. cadmium / Ca c. cobalt / Co d. magnesium / Mg e. chromium / Cr ANS: B OBJ: Identify the incorrect symbol/element name combination. TOP: Mixtures, Substances, Compounds, and Elements Whitten 10e Test Bank 9 39. Water is always 11.1% hydrogen and 88.9 % oxygen by mass. This is a statement of the a. Law of Conservation of Matter. b. Law of Definite Proportions. c. Law of Multiple Proportions. d. Law of Conservation of Matter and Energy. e. none of these. ANS: B OBJ: Identify the Law represented by percent mass of a pure compound. TOP: Mixtures, Substances, Compounds, and Elements 40. Below is a list of physical properties and the fundamental unit used in the SI system to measure each. Which unit is not the correct fundamental unit for the property? physical property / unit a. length / meter b. time / second c. mass / gram d. temperature / kelvin e. electric current / ampere ANS: C OBJ: Identify the incorrect physical property/ fundamental SI unit combination. TOP: Measurements in Chemistry 41. Which of the following is not an SI system unit of measurement? a. seconds b. joules c. kelvins d. meters e. pounds ANS: E OBJ: Recognize SI and non-SI units of measurement. TOP: Measurements in Chemistry 42. Below is a list of common prefixes used in the SI and metric systems. Included with each is an abbreviation and meaning. Which set contains an error? a. mega- M 106 b. deci- d 101 c. centi- c 102 d. micro- m 106 e. kilo- k 103 ANS: D OBJ: Recognize common measurement prefixes, and their abbreviation and meaning. TOP: Measurements in Chemistry 43. Below is a list of common prefixes used in the SI and metric systems. Included with each is an abbreviation and meaning. Which set contains an error? a. mega- M 106 b. deci- d 101 c. nano- n 109 d. milli- m 103 e. kilo- k 103 ANS: A OBJ: Recognize common measurement prefixes, and their abbreviation and meaning. TOP: Measurements in Chemistry Whitten 10e Test Bank 10 44. Which of the following is equivalent to 10 cm? a. 1m b. 0.1 dm c. 100 mm d. 1000 m e. 1mm ANS: C OBJ: Express a measurement in different units. TOP: Measurements in Chemistry 45. One of the following is a reasonable approximation of the diameter of a quarter (U.S. coin). Which one? a. 24Mm b. 0.24 m c. 24mm d. 24cm e. 0.0024 km ANS: C OBJ: Approximate a measurement and express it in a variety of common units. TOP: Units of Measurement 46. The mass of an average adult male would be closest to? a. 82kg b. 100 lbs c. 28kg d. 280 lbs e. 8200 g ANS: A OBJ: Approximate a measurement and express it in a variety of common units. TOP: Units of Measurement 47. A bug travels at a speed of 1 cm/s. The notation cm/s could also be written as: a. cms b. cm1  s1 c. cm1s d. cms1 e. none of these. ANS: D OBJ: Know the different ways to express units found in the denominator of a measurement. TOP: Units of Measurement 48. Which of the following numbers has 4 significant figures? a. 0.04309 b. 0.0430 c. 0.0431 d. 0.43980 e. 0.043090 ANS: A OBJ: Identify the measurement with the stated number of significant figures. TOP: Use of Numbers 49. The sum 2.834 + 5.71520 + 2.12 + 178.1 + 250.2619 expressed to the proper number of significant figures is: a. 439 b. 439.0 Whitten 10e Test Bank 11 c. 439.03 d. 439.031 e. 439.0311 ANS: B OBJ: Express a measurement derived from a calculation with the correct precision by applying the significant figure rules for calculations. TOP: Use of Numbers 50. Perform the indicated mathematical operations and express the answer in scientific notation rounded off to the proper number of significant figures: (8.001102)(2.88103 2.4103) = a. 9.6  102 b. 9.60  108 c. 9.601  108 d. 9.6  108 e. 9.6  102 ANS: D OBJ: Express a value in scientific notation. | Express a measurement derived from a calculation with the correct precision by applying the significant figure rules for calculations. TOP: Use of Numbers 51. The answer to the following calculation, rounded to the proper number of significant digits, is: 23.413 g(2.15 cm1.1 cm3.73 cm) a. 2.654 g/cm3 b. 2.65 g/cm3 c. 2.7 g/cm3 d. 3.0 g/cm3 e. 2.66 g/cm3 ANS: C OBJ: Express a measurement derived from a calculation with the correct precision by applying the significant figure rules for calculations. TOP: Use of Numbers 52. How many millimeters are there in 25 feet? a. 7.6102 mm b. 2.6103 mm c. 1.0102 mm d. 7.6103 mm e. 1.2103 mm Whitten 10e Test Bank 12 ANS: D OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 53. What is the height in centimeters of a person who is 5 feet 10 inches tall? a. 1.8104 cm b. 3.6  102 cm c. 27cm d. 1.5102 cm e. 1.8102 cm ANS: E OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 54. If 5.76  1013 neon atoms (spherical) were laid in a line, each touching the next, the line would measure 2.54 miles. What is the diameter of a neon atom in Å? a. 0.92 Å b. 0.71 Å c. 1.86 Å d. 1.44 Å e. 1.74 Å ANS: B OBJ: Calculate a value using the data provided. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 55. Convert 25.2 kilometers to inches. a. 99.2 in b. 6.40  106 in c. 9.92  105 in d. 9.92  101 in e. 6.40  103 in ANS: C OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 56. Convert 175 milliliters to gallons. a. 0.0462 gal b. 0.0414 gal c. 0.740 gal d. 0.164 gal e. 0.660 gal ANS: A OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) Whitten 10e Test Bank 13 57. Express 39.34 square yards in square centimeters. a. 0.6417 cm2 b. 17280 cm2 c. 1.835  106 cm2 d. 3.289  105 cm2 e. 7.632  106 cm2 ANS: D OBJ: Express an area in different units. TOP: The Unit Factor Method (Dimensional Analysis) 58. What is the area in square millimeters of a rectangle that is 8.632 cm long and 26.41 mm wide? a. 2280 mm2 b. 3.060 mm2 c. 22.80 mm2 d. 0.3060 mm2 e. 30.60 mm2 ANS: A OBJ: Determine the area of an object. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 59. What is the area (in mm2) of a rectangular surface that is 0.640 inch wide and 1.14 inches long? a. 471 mm2 b. 328 mm2 c. 84.2 mm2 d. 242 mm2 e. 680 mm2 ANS: A OBJ: Determine the area of an object. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 60. What is 16.7 cubic feet expressed in cubic centimeters? a. 1.55  104 cm3 b. 510 cm3 c. 0.159 cm3 d. 1.76  103 cm3 e. 4.73  105 cm3 ANS: E OBJ: Determine the volume of an object. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 61. Express 21.5 cubic centimeters in quarts. a. 2.03  102 qt b. 2.26  104 qt c. 9.24  102 qt d. 2.27  102 qt e. 2.02  104 qt ANS: D OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) Whitten 10e Test Bank 14 3 62. Assuming a magnesium atom is spherical, calculate its volume in nm . The diameter of a magnesium atom is 3.20 Å . The volume of a sphere is V = (4/3) r3. 1 Å = 1  1010 m and 1 nm = 1  109 m (Both of these relationships are exact).  = 3.14. a. 5.57  103 nm3 b. 2.34  1022 nm3 c. 5.57  1024 nm3 d. 1.71  102 nm3 e. 5.57  103 nm3 ANS: D OBJ: Determine the volume of an object. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 3 63. Assuming that a lithium atom is spherical, calculate its volume in cm . The volume of a sphere is given by V = (4/3) r3. The radius of a lithium atom is 1.52 Å. 1 Å = 108 cm and  = 3.14. a. 4.78  108 cm3 b. 1.47  1023 cm3 c. 6.14  1022 cm3 d. 3.06  1017 cm3 e. 4.68  1024 cm3 ANS: B OBJ: Determine the volume of an object. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 64. How many kilograms of lead are there in 749 pounds of lead? a. 95.1 kg b. 340 kg c. 760 kg d. 28.0 kg e. 1650 kg ANS: B OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 65. What is the mass, in grams, of a 16.0 lb bowling ball? a. 7300 g b. 0.0352 g c. 7260 g d. 6520 g e. 8000 g ANS: C OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 66. It requires 2.26  103 J to boil 1 g H2O. How many kJ are required to boil 1.00 lb H2O? a. 1030 kJ b. 4.98 kJ c. 4980 kJ d. 201 kJ e. 2260 kJ Whitten 10e Test Bank 15 ANS: A OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 67. If an airplane's speed is 550 mi/h, what is its speed in m/s? a. 40 m/s b. 328 m/s c. 246 m/s d. 528 m/s e. 885 m/s ANS: C OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 68. The mileage rating of a new high efficiency automobile is 52.0 miles per gallon. This could also be expressed as ____ kilometers per liter. a. 28.2 b. 31.6 c. 22.0 d. 72.6 e. 83.6 ANS: C OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 69. The 1970 standard established by the U.S. government for carbon monoxide emission for automobiles limited exhaust to 23.0 grams of CO per vehicle-mile. Assume that in a given metropolitan area there are 82,700 automobiles, driven an average of 13.5 miles per 24-hour period. How many tons/day of CO could legally be discharged into the area's atmosphere? a. 270 tons/day b. 0.155 tons/day c. 28.3 tons/day d. 0.0535 tons/day e. 39.0 tons/day ANS: C OBJ: Calculate a value using the data provided. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 70. At 25C, one milliliter of mercury has a mass of 13.6 grams. How many liters of mercury are required to have a mass of 500 kg of mercury? a. 500L b. 25.2 L c. 42.1 L d. 13.6 L e. 36.8 L ANS: E OBJ: Calculate a value using the data provided. | Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) Whitten 10e Test Bank 16 71. Caffeine, a stimulant in coffee and some cola drinks, is 49.47% carbon, 5.19% H, 28.8% N, 16.48% O. What is the mass of carbon contained in 37.1 g of caffeine? a. 18.4 g b. 36.8 g c. 6.11 g d. 1840 g e. 24.3 g ANS: A OBJ: Determine the mass of a component in a substance using percent mass. TOP: Percentage 72. Dark dental 22 carat gold is an alloy consisting of 92% Au, 4.9% Ag, and 3.1% Cu. If a patient leaves the dentist's office with 3.25 g of dark dental gold in her mouth, what mass of each element does she have in her mouth? (Note: round off may result in total mass not quite equaling 3.25 g.) a. 2.8gAu 0.25gAg 0.15gCu b. 2.9gAu 0.10gAg 0.16gCu c. 2.3gAu 0.75gAg 0.20gCu d. 3.0gAu 0.16gAg 0.10gCu e. 2.9gAu 0.25gAg 0.10gCu ANS: D OBJ: Determine the mass of a component in a substance using percent mass. TOP: Percentage 73. A 125 g sample of calcium carbonate contains 50.1 g calcium, 15.0 g carbon, and 59.9 g oxygen. Which of the following statements about calcium carbonate is incorrect? a. Calcium carbonate is 40.1 % calcium by mass. b. Calcium carbonate is 47.9 % oxygen by mass. c. Calcium carbonate is 15.0 % carbon by mass. d. Calcium carbonate has a smaller % by mass of carbon than of calcium. e. Calcium carbonate follows the Law of Definite Proportions. ANS: C OBJ: Determine the percent by mass of a component from its composition. | Identify the Law represented by percent mass of a pure compound. TOP: Percentage 74. A cube of metal is 1.42 centimeters on an edge. Its mass is 16.3 grams. What is its density? a. 4.68 g/cm3 b. 4.30 g/cm3 c. 5.69 g/cm3 d. 6.14 g/cm3 e. 4.86 g/cm3 ANS: C OBJ: Calculate density from mass and volume. TOP: Density and Specific Gravity Whitten 10e Test Bank 17 75. A metal cube having a mass of 112 grams is dropped into a graduated cylinder containing 30.00 mL of water. This causes the water level to rise to 39.50 mL. What is the density of the cube? a. 2.86 g/mL b. 11.8 g/mL c. 10.8 g/mL d. 3.74 g/mL e. 10.6 g/mL ANS: B OBJ: Calculate total volume from liquid displacement data. | Calculate density from mass and volume. TOP: Density and Specific Gravity 76. What is the specific gravity of nickel if 2.35 cm3 of nickel has the same mass as 20.9 mL of water at room temperature? a. 0.112 b. 2.14 c. 8.89 d. 19.7 e. 49.2 ANS: C OBJ: Calculate the specific gravity of a substance. TOP: Density and Specific Gravity 33 77. The density of mercury is 13.6 g/cm . What is the mass of 6.50 cm of mercury? a. 0.478 g b. 88.4 g c. 18.9 g d. 2.38 g e. 1.10102 g ANS: B OBJ: Convert volume to mass using density. TOP: Density and Specific Gravity 78. A gold ring has a mass of 15.37 g. If this ring is pure gold (density = 16.1g/mL), what would the volume of the ring be? a. 15.37 mL b. 1.04 mL c. 0.955 mL d. 16.1 mL e. 8.05 mL ANS: C OBJ: Convert mass to volume using density. TOP: Density and Specific Gravity 3 79. The density of octane is 0.702 g/cm . What is the mass of 65.0 mL of octane? a. 110g b. 92.6 g c. 22.5 g d. 45.6 g e. 1.08  102 g Whitten 10e Test Bank 18 ANS: D OBJ: Convert volume to mass using density. | Express a measurement in different units. TOP: Density and Specific Gravity 80. The specific gravity of ethyl chloride, an external painkiller, is 1.37 at 10C. What is the mass of 47.4 mL of the liquid? a. 64.9 g b. 0.346 g c. 34.6 g d. 52.5 g e. 56.6 g ANS: A OBJ: Convert volume to mass using specific gravity. TOP: Density and Specific Gravity 81. What is the volume of a 2.50-gram block of metal whose density is 6.72 grams per cubic centimeter? a. 16.8 cm3 b. 2.69 cm3 c. 0.0595 cm3 d. 0.372 cm3 e. 1.60 cm3 ANS: D OBJ: Convert mass to volume using density. TOP: Density and Specific Gravity 82. What volume is occupied by 14.3 g of mercury? Density = 13.6 g/mL. a. 37.2 mL b. 0.236 mL c. 193 mL d. 1.05 mL e. 4.82 mL ANS: D OBJ: Convert mass to volume using density. TOP: Density and Specific Gravity 83. What is the volume of a 58.5 gram sample of a liquid with a specific gravity of 1.24? a. 47.2 mL b. 63.2 mL c. 72.8 mL d. 20.2 mL e. 35.2 mL ANS: A OBJ: Convert mass to volume using specific gravity. TOP: Density and Specific Gravity Whitten 10e Test Bank 19 84. A saltwater aquarium should have a specific gravity of approximately 1.07. What is the density of seawater? a. 1.07 g/mL b. 10.7 g/mL c. 1.00 g/mL d. 0.935 g/mL e. 0.00107 g/mL ANS: A OBJ: Determine the density of a solution from its specific gravity. TOP: Density and Specific Gravity 85. Bromine, a brick red liquid, has a specific gravity of 3.12. What is the mass of 25.6 mL of bromine? a. 8.21 g b. 39.9 g c. 82.1 g d. 79.9 g e. 7.99 g ANS: D OBJ: Convert volume to mass using specific gravity. TOP: Density and Specific Gravity 86. Which of the following statements about density is incorrect? a. The densities of gases are usually expressed in units of g/L. b. The intensive property density can be calculated from the two extensive properties: mass and volume. c. The densities of liquids are usually expressed in units of g/mL (or g/cm3). d. If oil and water are placed in a container, they form two layers with oil as the top layer because it has the greater density. e. Densities of gases change greatly with changes in temperature and pressure. ANS: D OBJ: Understand the effect of temperature on density. | Know the units of density. | Understand the effect of pressure on density. | Understand how density effects layering of immiscible substance. TOP: Density and Specific Gravity 87. The freezing point of argon is 189C. What is its freezing point on the absolute temperature scale? a. 84K b. 136K c. 461K d. 112K e. 72K ANS: A OBJ: Convert degrees Celsius to kelvins. TOP: Heat and Temperature 88. Liquid propane boils at 231K. What is its boiling point in C? a. 42C b. 315C c. 42C d. 504C e. 231C Whitten 10e Test Bank 20 ANS: C OBJ: Convert kelvins to degrees Celsius. TOP: Heat and Temperature 89. Methane, CH4, boils at 162C. What is the boiling point of methane in F? a. 58F b. 108F c. 260F d. 323F e. 464F ANS: C OBJ: Convert degrees Celsius to degrees Fahrenheit. TOP: Heat and Temperature 90. Tungsten melts at 3422C which is why it is used as the filament in incandescent lights. What is its melting temperature in F? a. 1933F b. 1901F c. 619F d. 6150F e. 6192F ANS: E OBJ: Convert degrees Celsius to degrees Fahrenheit. TOP: Heat and Temperature 91. If normal body temperature is 98.6F, what is normal body temperature in C? a. 45.0C b. 37.0C c. 20.0C d. 52.6C e. 25.6C ANS: B OBJ: Convert degrees Fahrenheit to degrees Celsius. TOP: Heat and Temperature 92. The freezing point of the noble gas, argon, is 308F. What is this temperature in kelvins? a. 120K b. 462K c. 249 K d. 84K e. 462K ANS: D OBJ: Convert degrees Fahrenheit to degrees Celsius. | Convert degrees Celsius to kelvins. TOP: Heat and Temperature Whitten 10e Test Bank 21 93. Heptane melts at 182 K, and it boils at 371K. Which statement below is incorrect? a. Heptane will be a liquid at room temperature. b. The melting point of heptane is 132F. c. The melting point of heptane is lower than the melting point of water. d. Heptane would be a solid in a 200 K room. e. Heptane would be a solid at 100 K. ANS: D OBJ: Understand melting point. | Understand boiling point. | Convert kelvins to degrees Celsius. | Convert degrees Celsius to degrees Fahrenheit. TOP: Heat and Temperature 94. Gallium, a metal, has a freezing point near room temperature so it can be melted by holding it in your hands. If gallium's melting point is 302.8 K, what is that temperature in C? a. 0.0C b. 575.8C c. 302.8C d. 39.8C e. 29.8C ANS: E OBJ: Convert kelvins to degrees Celsius. TOP: Heat and Temperature 95. What is the boiling point of liquid nitrogen, 77 K, on the Fahrenheit scale? a. 321F b. 171F c. 168F d. 14.0F e. 144F ANS: A OBJ: Convert kelvins to degrees Celsius. | Convert degrees Celsius to degrees Fahrenheit. TOP: Heat and Temperature 96. Which of the following are sets of equivalent temperatures? I. 77F II. 86F III. 194F IV. 68F a. IandII b. II and III c. I and III d. II and IV e. III and IV 25C 278 K 30C 303 K 90C 363 K 22C 251 K ANS: B OBJ: Convert between three temperature units:degrees Fahrenheit, degrees Celsius, and kelvins. TOP: Heat and Temperature Whitten 10e Test Bank 22 97. How many kilojoules are equivalent to 565 calories? a. 130 kJ b. 930 kJ c. 0.135 kJ d. 2.36 kJ e. 2360 kJ ANS: D OBJ: Convert calories to kJ. TOP: Heat Transfer and the Measurement of Heat 98. How much heat is released as the temperature of 25.2 grams of iron is decreased from 72.1C to 9.8C? The specific heat of iron is 0.444 J/gC. a. 113J b. 566.1 J c. 1.11 kJ d. 0.697 kJ e. 957J ANS: D OBJ: Calculate the change in temperature of a substance. | Calculate the heat released based on the temperature change of a substance. TOP: Heat Transfer and the Measurement of Heat 99. The specific heat of aluminum is 0.900 J/gC. How many joules of heat are absorbed by 15.0 g of Al if it is heated from 20.0C to 60.0C? a. 540J b. 270J c. 812J d. 2.40 J e. 1.17104 J ANS: A OBJ: Calculate the change in temperature of a substance. | Calculate the heat released or gained based on the temperature change of a substance. TOP: Heat Transfer and the Measurement of Heat 100. An endothermic reaction a. evolves heat. b. is also called exothermic. c. would have its heat transferred measured in Joules. d. is not possible. e. would be described by all of these. ANS: C OBJ: Know the units of energy. | Define the terms endothermic and exothermic. TOP: Heat Transfer and the Measurement of Heat 101. An exothermic reaction a. absorbs heat. b. is also called kinetic. c. is not possible. d. would have its heat transferred measured in Joules. e. would be described by all of these. Whitten 10e Test Bank 23 ANS: D OBJ: Know the units of energy. | Define the terms endothermic and exothermic. TOP: Heat Transfer and the Measurement of Heat 102. If 10.0 g of copper cools from 35.0C to 28.8C and loses 23.6 joules of heat, what is the specific heat of copper? a. 0.076 J/gC b. 3.8  102 J/gC c. 0.38 J/gC d. 0.62 J/gC e. 76 J/gC ANS: C OBJ: Calculate the change in temperature of a substance. | Calculate the specific heat of a substance based on the change in heat content and the temperature change of the substance. TOP: Heat Transfer and the Measurement of Heat 103. What is the specific heat of a 5.75 g piece of metal if the addition of 175 joules of heat causes a 22.3C temperature increase? a. 1.36 J/gC b. 4.18 J/gC c. 1.11 J/gC d. 0.73 J/gC e. 1.54 J/gC ANS: A OBJ: Calculate the specific heat of a substance based on the change in heat content and the temperature change of the substance. TOP: Heat Transfer and the Measurement of Heat 104. A 10.0 kg piece of metal at 50.0C is placed in 1000. g of water at 10.0C in an insulated container. The metal and water come to the same temperature at 30.6C. What is the specific heat of metal? The specific heat of water is 4.18 J/gC. a. 0.0686 J/gC b. 0.444 J/gC c. 0.721 J/gC d. 0.124 J/gC e. 0.0216 J/gC ANS: B DIF: Harder Question OBJ: Calculate the specific heat of a substance based on the temperature equilibration of two substances. | Express a measurement in different units. | Calculate the change in temperature of a substance. TOP: Heat Transfer and the Measurement of Heat Whitten 10e Test Bank 24 105. The same amount of heat is added to a 25-g sample of each of the following metals. If each of the metals was initially at 20.0C, which metal will reach the highest temperature? Metal a. beryllium b. calcium c. copper d. gold e. nickel Specific Heat 1.82 J/gC 0.653 J/gC 0.385 J/gC 0.129 J/gC 0.444 J/gC ANS: D OBJ: Identify the substance with the greatest change in temperature. | Understand the relationship between the specific heat of a substance and the change in temperature of a substance. TOP: Heat Transfer and the Measurement of Heat 106. If 100. grams of liquid water at 100.0C and 200. grams of water at 20.0C are mixed in an insulated container, what will be the final temperature of the water? The specific heat of water is 4.18 J/gC. a. 41.9C b. 44.2C c. 46.7C d. 48.3C e. 45.1C ANS: C DIF: Harder Question OBJ: Calculate the equilibrium temperature of a mixture. TOP: Heat Transfer and the Measurement of Heat 107. How many grams of water at 25C must be mixed in an insulated container with 250. grams of water at 93C if the final temperature of the combined water is to be 75C? a. 45g b. 376g c. 120g d. 90g e. 140g ANS: D OBJ: Calculate the mass of one substance required to cool another substance to a specified temperature. TOP: Heat Transfer and the Measurement of Heat 108. If a 10.0 g ball of iron at 160.0C is dropped into 50.0 g of water at 20.0C in an insulated container, what will be the final temperature of the water? The specific heat of iron is 0.444 J/gC and that of water is 4.18 J/gC. a. 23C b. 38C c. 48C d. 82C e. 110C ANS: A DIF: Harder Question OBJ: Calculate the equilibrium temperature of a mixture. TOP: Heat Transfer and the Measurement of Heat Whitten 10e Test Bank 25 109. One of the following does not describe gases. Which one is it? a. fills any container completely b. slight expansion on heating c. easily compressed d. relatively low densities e. particles far apart ANS: B OBJ: Classify a gas or solid. TOP: States of Matter 110. Which of the following is not an intensive property of matter? a. malleability b. boiling point c. thermal conductivity d. weight e. color ANS: D OBJ: Classify a property as intensive or extensive. TOP: Chemical and Physical Properties 111. Which of these physical changes would require the addition of energy? a. boiling a liquid b. condensing a gas c. freezing a liquid d. all of these e. none of these ANS: A OBJ: Identify the endothermic or exothermic physical change. TOP: Chemical and Physical Changes 112. Which of following represents a physical change? a. the decomposition of cinnabar (HgS) to mercury metal upon heating b. the electrolysis of water to produce hydrogen and oxygen c. the tarnishing of the surface of copper in the presence of oxygen d. the dissolution of sugar in water e. the rusting of iron ANS: D OBJ: Classify changes as chemical or physical. TOP: Chemical and Physical Changes 113. Which of the following is not a mixture? a. sea shells b. cow manure c. ice cream d. gasoline e. diamond ANS: E OBJ: Distinguish between examples of pure substances and mixtures. TOP: Mixtures, Substances, Compounds, and Elements Whitten 10e Test Bank 26 114. Which of the following is a compound? a. soda b. air c. copper ore d. skim milk e. table salt ANS: E OBJ: Distinguish between examples of pure substances and mixtures. TOP: Mixtures, Substances, Compounds, and Elements 115. What is the symbol for the element tin? a. Sn b. Ti c. S d. Zn e. K ANS: A OBJ: Identify the symbol representing an element. TOP: Mixtures, Substances, Compounds, and Elements 116. The element whose symbol is K is a. potassium. b. krypton. c. cobalt. d. calcium. e. none of these. ANS: A OBJ: Identify the symbol representing an element. TOP: Mixtures, Substances, Compounds, and Elements 117. Below is a list of physical properties and the fundamental unit used in the SI system to measure each. Which unit is not the correct fundamental unit for the property? physical property / unit a. amount of substance / mole b. luminous intensity / candela c. time / meter d. temperature / kelvin e. electric current / ampere ANS: C OBJ: Identify the incorrect physical property/ fundamental SI unit combination. TOP: Measurements in Chemistry 118. What is the height in centimeters of a person who is 4 ft 10 in tall? (2.54 cm = 1 in; 1 ft = 12 in) a. 1.5104cm b. 2.9102 cm c. 22cm d. 1.2102 cm e. 1.5102 cm DIF: Hard Whitten 10e Test Bank 27 ANS: E OBJ: Express a measurement in different units. TOP: The Unit Factor Method (Dimensional Analysis) 119. Which of the following would you classify as nano-scale? a. An amoeba (one-celled animal) b. Coffee grounds c. A water molecule d. A cell membrane e. Gold ore ANS: C OBJ: Approximate the size-scale of matter. TOP: Chemistry – A Molecular View of Matter 120. Which of the following substances is an element? a. F2 b. C2H5OH c. Sodium chloride d. Water e. Brass ANS: A OBJ: Identify the element. TOP: Mixtures, Substances, Compounds, and Elements 121. Which of the following represents a mixture of two elements? a. b. c. Whitten 10e Test Bank 28 d. e. ANS: D OBJ: Identify the mixture of two elements. TOP: Mixtures, Substances, Compounds, and Elements 122. What kind of change is depicted below? a. Chemical change c. Both chemical and physical change b. Physical change d. No change ANS: A OBJ: Classify changes as chemical or physical. TOP: Chemical and Physical Changes 123. What kind of change is depicted below? a. chemical change b. physical change c. both chemical and physical d. no change Whitten 10e Test Bank 29 ANS: C OBJ: Classify changes as chemical or physical. TOP: Chemical and Physical Changes 124. How many significant figures are there in the number 0.097 a.1 b. 2 c. 3 d. 4 ANS: B OBJ: Identify the number of significant figures in a measurement. TOP: Use of Numbers 125. How many significant figures are there in the number 75100 a.1 b. 2 c. 3 d. 4 ANS: C OBJ: Identify the number of significant figures in a measurement. TOP: Use of Numbers 126. How many significant figures are there in the number 1.0720 a.1 b. 2 c. 3 d. 4 ANS: E OBJ: Identify the number of significant figures in a measurement. TOP: Use of Numbers 127. How many significant figures are there in the number 0.0306960? a.4 b. 5 c. 6 d. 7 ANS: C OBJ: Identify the number of significant figures in a measurement. TOP: Use of Numbers 128. What is the best answer to report for (515 x 0.0025) + 24.57? a. 25.858 b. 25.86 c. 25.8575 d. 26 e. 5 e. 5 e. 5 e. 8 e. 25.9 ANS: E OBJ: Report the answer in a mixed operation to the correct number of significant figures. TOP: Use of Numbers 129. When 87.7 is added to 73.841, the result should be reported with _____ significant figures. And when 87.7 is divided by 73.841 the result should be reported with ______ significant figures. a. 3, 3 b. 3, 5 c. 4, 3 d. 4, 4 e. 3, 4 ANS: C OBJ: Determine the number of significant figures for the given operations. TOP: Use of Numbers 130. When 45.24 is subtracted from 40.1, the result should have _____ sig figs. When 45.24 is multiplied by 40.1, the result should have _____ sig figs. a. 2 , 5 b. 3 , 3 c. 2 , 3 d. 4 , 4 ANS: C OBJ: Determine the number of significant figures for the given operations. TOP: Use of Numbers e. 3 , 2 Whitten 10e Test Bank 30 131. When 51.8 and 67.5 are multiplied, the product has ____ significant figures, and when 51.8 and 67.5 are added, the sum has ____ significant figures. a. 5 , 3 b. 3 , 4 c. 3 , 5 d. 4 , 3 e. 3 , 3 ANS: B OBJ: Determine the number of significant figures for the given operations. TOP: Use of Numbers 132. Which is higher: 144oF or 63.6oC? { oF = 9/5(oC) + 32 } a. 144oF c. The temperatures are equivalent b. 63.6oC ANS: B OBJ: Compare two temperatures in different units. TOP: Heat and Temperature 133. As part of the calibration of a new laboratory balance, a 0.200-g mass is weighed with the following results: Trial Mass 1 0.216-g 2 0.196-g 3 0.187-g Choose the statement that best describes the calibration data. a. The balance is both accurate and precise. b. The balance is accurate but imprecise. c. The balance is precise but inaccurate. d. The balance is both inaccurate and imprecise. ANS: B OBJ: Interpret the accuracy and precision of a set of data. TOP: Accuracy and Precision 134. The liquid 1,2-ethanedithiol is insoluble in water. If a 75.5 g sample of 1,2-ethanedithiol has a volume of 61.2 mL, what is its density, and would it float or sink if poured into a beaker containing water? a. 1.20g/mL and it would sink in water c. 0.811 g/mL and it would sink in water b. 1.20 g/mL and it would float on water d. 0.811 g/mL and it would float on water ANS: A OBJ: Calculate the density and determine if the substance floats or sinks. TOP: Density 135. An empty Erlenmeyer flask weighs 241.3g. When filled with water (density = 0.997g/mL), the flask and its contents weigh 489.1g. What volume of water does the flask hold? a. 246.3 mL b. 247.1 mL c. 247.8 mL d. 248.5 mL e. ANS: D OBJ: Calculate a volume given density and mass. TOP: Density 240.6 mL Whitten 10e Test Bank 31 SHORT ANSWER Instructions: Use the pictures below to answer the following questions: A) B) C) D) E) 1. Which of the figures above depicts a heterogeneous mixture? ANS: B OBJ: Identify the heterogeneous mixture. TOP: Mixtures, Substances, Compounds, and Elements 2. Which of the figures above depicts a liquid compound? ANS: E OBJ: Identify the liquid compound. TOP: States of Matter | Mixtures, Substances, Compounds, and Elements 3. Which of the figures above depicts a gaseous compound? ANS: D OBJ: Identify the gaseous compound. TOP: States of Matter | Mixtures, Substances, Compounds, and Elements 4. Which of the figures above depicts a homogeneous mixture? ANS: C OBJ: Identify the homogeneous mixture. TOP: Mixtures, Substances, Compounds, and Elements Whitten 10e Test Bank 32 Instructions: Use the figures below to answer the following questions: A) B) C) D) E) 5. Which of the figures above represents a gaseous compound? ANS: B OBJ: Identify the gaseous compound. TOP: States of Matter | Mixtures, Substances, Compounds, and Elements 6. Which of the figures above represents a liquid element? ANS: D OBJ: Identify the liquid element. TOP: States of Matter | Mixtures, Substances, Compounds, and Elements 7. Which of the figures above represents a homogeneous mixture? ANS: E OBJ: Identify the homogeneous mixture. TOP: Mixtures, Substances, Compounds, and Elements 8. Which of the figures above represents a gaseous element? ANS: A OBJ: Identify the gaseous element. TOP: States of Matter | Mixtures, Substances, Compounds, and Elements 9. Which of the figures above represents a liquid compound? ANS: C OBJ: Identify the liquid compound. TOP: States of Matter | Mixtures, Substances, Compounds, and Elements Whitten 10e Test Bank 33 CONCEPTUAL 1. What are some experiments that might be performed to determine the identity of an unknown metal from the moon? OBJ: Propose an experiment to determine the density of a substance. TOP: Density 2. Why is having a universal system of units for the entire planet a good idea? Why does the United States still use other units? OBJ: Explain the value of a universal system of units. TOP: Units of Measurement | Measurements in Chemistry 3. If there are only about 88 naturally occurring type of atoms, why is there such a tremendous variety of matter in the universe? OBJ: Explain why matter is not limited to the 88 naturally occurring elements. TOP: Mixtures, Substances, Compounds, and Elements 4. A 50-lb rock is removed from the bottom of a pool and placed in a canoe on the surface of the pool. Does the water level in the pool increase or decrease? OBJ: Explain the effect of density with respect to liquid displacement. TOP: Density 5. What are some pure elements that we encounter every day? What are some pure compounds? OBJ: Classify a common substance as an element or a compound. TOP: Mixtures, Substances, Compounds, and Elements 6. If Einstein's equation E = mc2 is correct what happens when energy is released from a nuclear reaction? OBJ: Propose the fate of matter in a nuclear reaction. TOP: Nuclear reactions. | Matter and Energy Whitten 10e Test Bank 34 Chapter 2—Chemical Formulas and Composition Stoichiometry MULTIPLE CHOICE 1. There are two different common crystalline forms of carbondiamond and graphite. A less common form called fullerene, C60, also exists. Different forms of the same element in the same physical state are called: a. isotopes. b. isomers. c. alloforms. d. allotropes. e. structural formulas. ANS: D OBJ: Define allotrope. TOP: Chemical Formulas 2. How many atoms are in a sulfuric acid molecule? a. 1 b. 7 c. 5 d. 6 e. 8 ANS: B OBJ: Know the chemical formulae of common acids. TOP: Chemical Formulas 3. If a sample of butane, C4H10, contains a total of 8.0  103 atoms of carbon, how many molecules of butane are in the sample? a. 6.0  103 b. 3.0  103 c. 8.0  103 d. 1.1  104 e. 2.0  103 ANS: E OBJ: Understand the relationship between molecular formula and the number of atoms of a specific type contained in a single compound. | Convert the number of atoms in a substance to the number of molecules in a substance. TOP: Chemical Formulas 4. Name the molecular compound, HNO3. a. ammonia b. nitric acid c. nitrous acid d. nitric oxide e. methane ANS: B OBJ: Know the names and chemical formulae of common acids. TOP: Chemical Formulas Whitten 10e Test Bank 1 5. Name the molecular compound, SO3. a. sulfur oxide b. sulfurous acid c. sulfur trioxide d. sulfuric acid e. none of these ANS: C OBJ: Translate the chemical formula of a binary molecule into a name. TOP: Chemical Formulas 6. Which formula / name pair does not match? a. HNO3 / nitric acid, used to produce explosives b. CH3OH / methyl alcohol, wood alcohol c. CH3CH2OH / ethyl alcohol, alcohol in wine d. CHCl3 / acetic acid, found in vinegar e. CH3CH2OCH2CH3 / diethyl ether, an anesthetic ANS: D OBJ: Know the names and chemical formulae of common acids. | Recognize the names and chemical formulae of common organic compounds. TOP: Chemical Formulas 7. Name the molecular compound, CH3COCH3. a. acetone b. ethanol c. diethyl ether d. propane e. ethyl alcohol ANS: A OBJ: Know the names and chemical formulae of common organic compounds. TOP: Chemical Formulas 8. What is the molecular formula for ethanol? a. CH3COOH b. CH3COCH3 c. CH3CH2OCH2CH3 d. CH3CH2CO2H e. CH3CH2OH ANS: E OBJ: Know the names and chemical formulae of common organic compounds. TOP: Chemical Formulas 9. Butane, a highly combustible hydrocarbon found in disposable lighters, has the chemical formula: a. CO2 b. C4H8 c. C4H10 d. C3H8 e. CH3OCH3 Whitten 10e Test Bank 2 ANS: C OBJ: Know the names and chemical formulae of common organic compounds. | Translate the chemical formula of a binary molecule into a name. TOP: Chemical Formulas 10. What is the molecular formula for hydrogen chloride? a. HCl b. HClO c. HClO2 d. HClO3 e. HClO4 ANS: A OBJ: Know the names and chemical formulae of common acids. TOP: Chemical Formulas 11. A compound contains only calcium and fluorine. A sample of the compound is determined to contain 2.00 g of calcium and 1.90 g of fluorine. According to the Law of Definite Proportions, how much calcium should another sample of this compound contain if it contains 2.85 g of fluorine? a. 2.71 g b. 4.00 g c. 3.00 g d. 4.50 g e. 6.00 g ANS: C OBJ: Apply the Law of Definite Proportions. TOP: Chemical Formulas 12. A compound contains only magnesium and oxygen. A sample of the compound is determined to contain 3.50 g of magnesium and 2.30 g of oxygen. According to the Law of Definite Proportions, how much magnesium should another sample of this compound contain if it contains 6.91 g of oxygen? a. 1.16 g b. 10.5 g c. 4.54 g d. 55.5 g e. 0.858 g ANS: B OBJ: Apply the Law of Definite Proportions. TOP: Chemical Formulas 13. Which of the following is not the name of a cation? a. sodium b. iron (III) c. magnesium d. sulfide e. ammonium ANS: D OBJ: Understand how to name monatomic anions and cations. | Know the names and charges of polyatomic ions. TOP: Ions and Ionic Compounds Whitten 10e Test Bank 3 14. Which of the following statements is incorrect? a. Potassium chloride forms molecules that consist of one K+ ion and one Cl ion. b. Ions that possess a positive charge are called cations. c. Polyatomic ions are groups of atoms that have an electric charge. d. It is acceptable to use formula unit to refer to either an ionic compound or a molecular compound. e. Ions that possess a negative charge are called anions. ANS: A OBJ: Distinguish between properties that define a substance as ionic or molecular. TOP: Ions and Ionic Compounds  ANS: D OBJ: Classify a species as a monatomic ion, polyatomic ion, or molecule. TOP: Ions and Ionic Compounds 16. What is the correct formula for the carbonate ion? a. CH3COO b. Cl c. CO22 d. CO32 e. (COO)2 ANS: D OBJ: Know the names, chemical formulae, and charges of common polyatomic ions. TOP: Ions and Ionic Compounds 17. Each response below lists an ion by name and by chemical symbol or formula. Also each ion is classified as monatomic or polyatomic and as a cation or anion. Which response contains an error? a. hydroxide / OH / monatomic / anion b. carbonate / CO32 / polyatomic / anion c. ammonium / NH4+ / polyatomic / cation d. magnesium / Mg2+ / monatomic / cation e. sulfite / SO32 / polyatomic / anion ANS: A OBJ: Know the names, chemical formulae, and charges of monatomic ions and common polyatomic ions. TOP: Ions and Ionic Compounds 18. Each response below lists an ion by name and by chemical symbol or formula. Also each ion is classified as monatomic or polyatomic and as a cation or anion. Which response contains an error? a. phosphate / PO43 / polyatomic / anion b. sulfite / SO32 / polyatomic / anion c. nitrite / NO3 / polyatomic / anion d. iron(II) / Fe2+ / monatomic / cation e. bromide / Br / monatomic / anion ANS: C OBJ: Know the names, chemical formulae, and charges of monatomic ions and common polyatomic ions. TOP: Ions and Ionic Compounds 15. What is the correct classification for OCl? a. polyatomic molecule b. monatomic cation c. polyatomic cation d. polyatomic anion e. monatomic anion Whitten 10e Test Bank 4 19. What is the formula for ammonium fluoride? a. AlF b. Al2F3 c. NH3F d. NH4F2 e. NH4F ANS: E OBJ: Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 20. What is the formula for manganese(III) oxide? a. MgO b. MnO c. MnO4 d. Mg2O3 e. Mn2O3 ANS: E OBJ: Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 21. What is the formula for aluminum oxide? a. Al2O3 b. Ag2O3 c. AlO3 d. AlO e. AlO2 ANS: A OBJ: Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 22. What is the name of Fe(OH)3? a. iron hydroxide b. iron trihydroxide c. iron (III) hydroxide d. iron (II) hydroxide e. none of these ANS: C OBJ: Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 23. What is the formula for copper(II) sulfate? a. CuSO4 b. Cu2SO3 c. CuSO2 d. Cu2SO4 e. Cu(SO4)2 ANS: A OBJ: Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 24. Choose the name / formula pair that does not correctly match. a. aluminum phosphate / AlPO4 b. calcium acetate / CaCH3COO c. ammonium sulfide / (NH4)2S d. magnesium hydroxide / Mg(OH)2 Whitten 10e Test Bank 5 e. zinc carbonate / ZnCO3 ANS: B OBJ: Translate the chemical formula of an ionic compound into a name. | Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 25. From the following ionic compounds, choose the name / formula pair that is not correctly matched. a. sodium sulfide / Na2S b. ammonium nitrate / NH4NO3 c. zinc hydroxide / Zn(OH)2 d. sodium sulfate / Na2SO3 e. calcium oxide / CaO ANS: D OBJ: Translate the chemical formula of an ionic compound into a name. | Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 26. From the following compounds choose the name / formula pair that is incorrectly matched. a. sodium sulfite / Na2SO3 b. ammonium fluoride / NH4F c. copper(II) carbonate / CuCO3 d. ferric chloride / FeCl3 e. cuprous sulfide / Co2S ANS: E OBJ: Translate the chemical formula of an ionic compound into a name. | Translate the name of an ionic compound into a chemical formula. TOP: Names and Formulas of Some Ionic Compounds 27. Which element has a mass that is 7.30 times that of carbon-12? a. Mg b. Sr c. Ca d. Br e. Rb ANS: B OBJ: Apply the modern definition of relative atomic mass. TOP: Atomic Weights Whitten 10e Test Bank 6 28. Which element has a mass approximately 4 times that of an H atom? a. Be b. He c. Li d. Ti e. K ANS: B OBJ: Apply the concept of relative atomic mass. TOP: Atomic Weights 29. The molecular formula for a compound is CX4. If 2.819 g of this compound contains 0.102 g of carbon, what is the atomic weight of X? a. 320 b. 160 c. 35.5 d. 79.9 e. 39.9 ANS: D DIF: Harder Question OBJ: Calculate the atomic weight of an unknown element based on the chemical formula and mass of each component in a sample. TOP: Atomic Weights 30. How many atoms of hydrogen are in 1.00 mole of water? a. 6.02  1023 b. 1.20  1024 c. 1.81  1024 d. 2.41  1024 e. 3.01  1023 ANS: B OBJ: Translate the name of a binary molecule into a chemical formula. | Use Avogadro's number and the molecular formula to convert moles of a substance to number of atoms. TOP: The Mole 31. Calculate the number of moles of oxygen atoms in 35.2 grams of oxygen. a. 2.20 moles b. 4.42 moles c. 0.54 moles d. 2.57 moles e. 1.13 moles ANS: A OBJ: Translate the name of a diatomic element into a chemical formula. | Use the formula weight or molecular weight of a substance to convert grams of a substance to moles. TOP: The Mole 32. How many grams are contained in 0.644 mol oxygen? a. 10.3 g b. 20.6 g c. 0.0201 g d. 0.0403 g e. 0.644 g ANS: B OBJ: Translate the name of a diatomic element into a chemical formula. | Use the formula weight or molecular weight of a substance to convert moles of a substance to grams. Whitten 10e Test Bank 7 TOP: The Mole 33. Calculate the mass of one bromine atom. a. 2.654  1022 g b. 6.022  1023 g c. 1.661  1024 g d. 4.812  1025 g e. 1.327  1022 g ANS: E OBJ: Use Avogadro's number and atomic weight to convert the number of atoms to grams. TOP: The Mole 34. Determine the number of sulfur atoms in 27.1 g of molecular sulfur (S8). a. 0.845 b. 5.27  1023 c. 5.09  1023 d. 2.07  1023 e. 0.106 ANS: C OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use Avogadro's number, molecular formula, and molecular weight to convert grams to number of atoms. TOP: The Mole 35. Calculate the formula weight of NaHSO4. a. 193 amu b. 104 amu c. 120 amu d. 215 amu e. 185 amu ANS: C OBJ: Determine the formula weight of a substance using atomic weights and the chemical formula. TOP: Formula Weights, Molecular Weights, and Moles 36. Determine the formula weight of Ca3(PO4)2. a. 230 amu b. 279 amu c. 215 amu d. 310 amu e. 135 amu ANS: D OBJ: Determine the formula weight of a substance using atomic weights and the chemical formula. TOP: Formula Weights, Molecular Weights, and Moles Whitten 10e Test Bank 8 37. What is the mass of 2.2  109 CO2 molecules? a. 9.7  1010 g b. 1.0  1012 g c. 1.2106 g d. 4.4  1014 g e. 1.6  1013 g ANS: E OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use Avogadro's number and molecular weight to convert molecules to grams. TOP: Formula Weights, Molecular Weights, and Moles 38. What is the mass of 0.432 moles of C8H9O4? a. 86.9 g b. 391g c. 169g d. 113.8 g e. 73.0 g ANS: E OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use the formula weight or molecular weight of a substance to convert moles to grams. TOP: Formula Weights, Molecular Weights, and Moles 39. How many grams of CaCl2 equal 4.26 moles of CaCl2? a. 26.1 g b. 170g c. 302g d. 473g e. 322g ANS: D OBJ: Determine the formula weight of a substance using atomic weights and the chemical formula. | Use the formula weight or molecular weight of a substance to convert moles to grams. TOP: Formula Weights, Molecular Weights, and Moles 40. How many moles of POCl3 are there in 10.0 grams of POCl3? a. 6.51  102 mol b. 3.68  101 mol c. 4.09  102 mol d. 1.21  101 mol e. 1.17  103 mol ANS: A OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use the formula weight or molecular weight of a substance to convert grams to moles. TOP: Formula Weights, Molecular Weights, and Moles 41. How many moles of CCl4 are present in 118. g of carbon tetrachloride? a. 0.839 b. 1.19 c. 0.538 d. 1.30 e. 0.767 ANS: E OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use the formula weight or molecular weight of a substance to convert grams to moles. TOP: Formula Weights, Molecular Weights, and Moles Whitten 10e Test Bank 9 42. How many molecules are contained in 5.00 grams of NH3? a. 5.42  1022 b. 3.00  1024 c. 3.40  1022 d. 1.77  1023 e. 9.45  1022 ANS: D OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use Avogadro's number and molecular weight or formula weight to convert grams to molecules. TOP: Formula Weights, Molecular Weights, and Moles 43. A 12.0-gram sample of Cr2(SO4)3 contains how many sulfur atoms? a. 1.84  1022 b. 1.53  1021 c. 4.82  1021 d. 6.67  1022 e. 5.52  1022 ANS: E OBJ: Determine the formula weight of a substance using atomic weights and the chemical formula. | Use Avogadro's number, molecular formula, and formula weight to convert grams to atoms. TOP: Formula Weights, Molecular Weights, and Moles 44. How many atoms of carbon are present in 34.5 g of caffeine, C8H10N4O2? a. 8.57  1023 b. 2.68  1025 c. 1.08  1024 d. 2.09  1023 e. 4.83  1023 ANS: A OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use Avogadro's number, molecular formula, and molecular weight to convert grams to atoms. TOP: Formula Weights, Molecular Weights, and Moles 45. What is the mass in grams of 5.00  1012 water molecules? a. 1.50  1010 g b. 1.67  1035 g c. 2.17  1012 g d. 6.69109 g e. 4.61  1013 g ANS: A OBJ: Translate the name of a binary molecule into a formula. | Determine the molecular weight of a substance using atomic weights and the chemical formula. | Use Avogadro's number and molecular weight to convert molecules to grams. TOP: Formula Weights, Molecular Weights, and Moles Whitten 10e Test Bank 10 46. Which of the following is not a correct description of 16.0 grams of methane, CH4? a. It is one mole of methane. b. It is the amount of methane that contains 12.0 g of carbon. c. It is 16.0  6.02  1023 molecules of methane. d. It is the amount of methane that contains 4.0 grams of hydrogen. e. It is the amount of methane that contains 4  6.02  1023 hydrogen atoms. ANS: C OBJ: Determine the molecular weight of a substance using atomic weights and the chemical formula.| Convert grams of a substance to moles, grams of a component, molecules, or atoms. TOP: Formula Weights, Molecular Weights, and Moles 23 47. A sample of ethane, C2H6, contains a total of 16N atoms, where N = 6.02  10 the sample? a. 2.0g b. 30g c. 60g d. 16 mol e. 4mol . How much C2H6 is in ANS: C OBJ: Determine the molecular weight of a substance using atomic weights and the formula of the substance.| Use Avogadro's number, molecular formula, and molecular weight to convert total atoms in a sample to grams or moles. TOP: Formula Weights, Molecular Weights, and Moles 48. Suppose you have a 100-gram sample of each of the following compounds. Which sample contains the smallest number of moles of compound? a. NH3 b. MgCl2 c. H3PO4 d. CrCl3 e. NaCl ANS: D OBJ: Understand and apply the relationship between mass, molar mass, and moles of a sample. TOP: Formula Weights, Molecular