testbankbyte.comtestbankbyte.com/wp-content/uploads/2016/09/ch011.docx · Web viewb.a statement describing a relationship between phenomena that is always the same under the same

Chapter 1Scientific Measurements

Multiple Choice Questions

1. A tentative explanation used to explain observed facts or laws is called

a. the scientific method.b. a scientific law.c. a theory.d. a hypothesis.e. an empirical fact.

Answer: dSection 1.1Difficulty Level: easy

2. A broad generalization based on the results of many experiments is called

a. the scientific method.b. a scientific law.c. a theory.d. a hypothesis.e. an empirical fact.

Answer: bSection 1.1 Difficulty Level: medium

3. Which of the following is false?

a. Experiments can be used to show that a theory is somewhat limited in scope.b. A hypothesis which has successfully withstood many tests eventually can become

a theory.c. In general, a theory can be proven to be absolutely true.

d. In general, a theory cannot be proven to be absolutely true.e. A theory is an explanation of general principles which has withstood repeated

testing.

Answer: cSection 1.1Difficulty Level: hard

1-1

4. A scientific law is

a. a tentative explanation for a set of observations that can be tested by further experimentation.

b. a statement describing a relationship between phenomena that is always the same under the same conditions.

c. a unifying principle that explains a body of facts and relations. d. a model used to visualize the invisible.e. a rule that sets the standard units of scientific values.

Answer: bSection 1.1Difficulty Level: hard

5. Which of the following gives the best description of what the scientific method is?

a. It is the process of carefully following the steps of a lab procedure.b. It is the guidelines that are followed during laboratory measurements.c. It is unifying principle that explains a body of facts and relations. d. It is the process of making observations and then designing ways to evaluate or

explain those observations.e. It is a guidebook for laboratory techniques that is followed by all chemists.

Answer: dSection 1.1Difficulty Level: medium

6. An example of an element is

a. glucose, C6H12O6. b. table salt, NaCl.

c. gold, Au. d. an oxide of iron, Fe2O3. e. limestone, CaCO3.

Answer: cSection 1.2Difficulty Level: easy

1-2

7. An example of an element is

a. ozone gas, O3.b. water, H2O.c. benzene, C6H6.

d. carbon dioxide gas, CO2.e. ammonium nitrate, NH4NO3.

Answer: aSection 1.2Difficulty Level: easy

8. An example of a chemical compound is

a. iron metal, Fe.b. brass, a solution of Cu and Zn.c. ozone gas, O3.d. sand.e. table salt, NaCl.

Answer: eSection 1.2 Difficulty Level: easy

9. An example of a chemical compound is

a. silver, Ag.b. helium gas, He.c. carbon dioxide gas, CO2.d. mercury metal, Hg.e. hydrogen gas, H2.

Answer: cSection 1.2 Difficulty Level: easy

1-3

10. The two types of pure substances are

a. compounds and elements.b. compounds and solutions.c. elements and mixtures.d. mixtures and solutions.e. solutions and elements.

Answer: aSection 1.2Difficulty Level: medium

11. Which is an example of a chemical change?

a. Steam from the boiling water condenses on the ceiling.b. The solid metal is heated until it melts.c. The gas is cooled until it finally becomes a liquid.d. A piece of paper burns in air with a smoky flame.e. The table salt in the warehouse container had very large chunks in it.

Answer: dSection 1.2 Difficulty Level: medium

12. Which is an example of a physical change?

a. The milk in the box left on the table becomes sour after a few days.b. The bit of scrap metal dissolves when placed in the container of acid.c. The gas is cooled until it finally becomes a liquid.d. A piece of paper burns in air with a smoky flame.e. Bubbles are seen on the egg shell after some vinegar is poured on it.

Answer: cSection 1.2 Difficulty Level: medium

1-4


a. Water, when heated, forms steam.b. Bleach turns hair yellow.c. Sugar, when heated, becomes brown.d. Milk turns sour over time.e. Apples, when exposed to air, turn brown over time.

Answer: aSection 1.2 Difficulty Level: medium


a. The milk in the carton became frozen after the carton was accidentally placed in the freezing compartment.

b. The bit of scrap metal was crushed by the heavy machine.c. The gas was cooled until it eventually became a liquid.d. The piece of paper was cut into many thin strips by the shredding machine.

e. Bubbles were seen on the egg shell after some vinegar was poured on it.

Answer: eSection 1.2 Difficulty Level: medium


a. Steam from the boiling water condenses on the cooler part of the ceiling.b. The crude metal ore was first heated then combined with pure oxygen gas to make

the oxide of the metal.c. The chef made scrambled eggs for their breakfast.d. A piece of paper burns in air with a smoky flame.e. The table salt in the warehouse was used to make some of the polymeric material.


1-5


a. Water freezing at 0°C.b. Burning gasoline.c. A potato turns brown after being cut open and left out.d. Heating magnesium metal causes it to turn into an off white solid.e. When exposed to certain metals hydrogen peroxide will bubble and fizz.


17. Which is an example of both a physical and a chemical change?

a. The milk in the carton became frozen after the carton was accidentally placed in the freezing compartment overnight.

b. The bit of scrap metal was removed to the junkyard after being crushed by the heavy machine.

c. The gas was collected in a flask and cooled until it eventually became a liquid.d. The old parchment became dry after being placed in the hot oven, but then was

charred since it was not removed in the specified time.e. Bubbles were seen on the egg shell when the vinegar was poured on it.

Answer: dSection 1.2 Difficulty Level: hard

18. Which is an example of both a physical and a chemical change?

a. The milk in the carton became frozen because the carton was accidentally placed in the freezing compartment overnight.

b. The bit of scrap metal was removed to the junkyard after being crushed by the heavy machine.

c. The gas was collected in a flask and cooled until it eventually became a liquid.d. The old parchment became dry when it was placed in the warm oven for ten

minutes. e. Bubbles were seen on the egg shell soon after a sample of the vinegar was

poured on it.

Answer: eSection 1.2 Difficulty Level: hard

1-6

19. An example of a chemical change is

a. the mixing of glucose with table salt.b. the dissolving of table salt in water.c. sodium combining with chlorine to form table salt. d. mixing rust with sand.e. mixing chalk with helium in a balloon.


20. Which of the examples below is a chemical change?

a. A bottle of wine completely evaporates in two weeks.b. Bleach changes the color of the stain on the white shirt. c. The ‘dry ice’ (solid CO2) changes to vapor.d. Bubbles form in the water when He gas is blown into the water.e. These are all examples of chemical change.

Answer: bSection 1.2Difficulty Level: easy


a. the separation of air into oxygen, nitrogen, and other componentsb. the separation of a compound into its elementsc. the separation of gases from liquidsd. the separation of a mixture into its componentse. the separation of solids from liquids


1-7

22. Which one of the following is a physical change?

a. When ignited with a match in open air, paper burns.b. In cold weather, water condenses on the inside surface of single pane windows.c. When treated with bleach, some dyed fabrics change color. d. When heated strongly, sugar turns dark brown.e. Grape juice left in an open unrefrigerated container turns sour.



a. The ‘dry ice’ (solid CO2) changes to vapor.b. A bottle of wine turns into vinegar in a few months.c. Bleach changes the color of the stain on the white shirt. d. Bubbles form on the egg shell when it is placed in the vinegar.e. A portion of the figurine dissolves after being placed in the container of acid.


24. Which one of the following examples does not involve a chemical change?

a. A fish that is left for some time in an unrefrigerated place decomposes.b. Apple juice which is left in an open bottle, ferments.c. A loaf of bread rises and its volume expands when it is baked in an oven.d. When a lake starts to freeze in winter, ice is formed on the surface.e. When sugar is fermented under certain conditions, alcohol is produced.


1-8

25. Which one of the following is a chemical change?

a. When blood is mixed with 3% hydrogen peroxide solution, it changes color.b. When water is boiled, it forms steam.c. When a solid stick of butter is heated, it becomes a liquid.d. When blue paint is mixed with yellow paint, a green colored paint is obtained.e. When a bar of gold metal is pounded with a hammer, it flattens out.


26. Which of the following is not a chemical change?

a. A nail rusts when exposed to air and moisture.b. Milk turns sour if left unrefrigerated.c. Yeast produces carbon dioxide to help bread rise.d. Copper is molded with heat to form pipes.e. Mixing baking soda and vinegar causes fizzing and bubbling.

Answer: eSection 1.2Difficulty Level: easy

27. Each of the following properties of a sample of a pure substance can be used for identification except its

a. density.b. freezing point temperature.c. mass.d. melting point temperature.e. solubility in water.


1-9

28. A physical property is one that

a. can be observed without changing the chemical identity of a substance.b. is based on one particular scientific law.c. describes a chemical reaction that a substance undergoes.d. cannot be seen with the naked eye.e. is considered hypothetical in origin.


29. Which is an example of a physical property?

a. corrosiveness of sulfuric acidb. toxicity of cyanidec. flammability of gasolined. neutralization of stomach acid with an antacide. lead become a liquid when heated to 601 °C


30. Which is an example of a physical property?

a. dynamite explodesb. meat rots if it is not refrigeratedc. honey tastes sweetd. ice floats on top of liquid watere. a silver platter tarnishes over time.

Answer: eSection 1.3Difficulty Level: medium

1-10

31. All of these statements describe properties of sodium. Which one describes a physical property of sodium?

a. Sodium’s surface turns black when first exposed to air.b. Sodium is a solid at 25°C and changes to a liquid when heated to 98°C.c. When exposed to water, sodium reacts violently and a gas is formed.d. When placed in contact with chlorine, sodium forms a compound that melts at

801°C.e. Sodium is never found as a pure metal in nature.

Answer: bSection 1.3Difficulty Level: medium

32. Water can also exist as a gas that is called a. ice.b. steam.c. the melt.d. molecules.e. atomic water.


33. Which of the following describes a chemical property?

a. A property based solely on the scientific method.b. A property which is based on a particular scientific law.c. A property which describes a change a substance undergoes. d. A property which cannot be seen. e. A property which is considered hypothetical.

Answer: cSection 1.3Difficulty Level: medium

1-11

34. All of these statements describe properties of tin. Which one describes a chemical property of tin?

a. Tin can be hammered into a thin sheet.b. The density of white tin is 7.365 g cm-3.c. Tin melts at 231.9°C.d. When a bar of tin is bent, it emits an audible “cry”.e. Tin dissolves slowly in cold, dilute hydrochloric acid, but it dissolves readily in

concentrated hydrochloric acid.


35. Which is an example of a chemical property?

a. combustibilityb. volatilityc. viscosityd. malleabilitye. ductility


36. Which is an example of an intensive property of matter?

a. colorb. volumec. massd. weighte. length


1-12

37. Which is an example of an intensive property of matter?

a. temperatureb. volumec. lengthd. weighte. melting point


38. Which is an example of an extensive property of matter?

a. colorb. densityc. massd. melting pointe. flash point


39. Which is an example of an extensive property of matter?

a. surface areab. boiling pointc. densityd. hardnesse. freezing point


1-13

40. The kilo isa. a unit of mass.b. a unit used in medical terminology.c. a decimal multiplier in the metric system.d. a unit of speed.e. a volume unit used by the DEA (drug enforcement agency).


41. The SI base units of temperature and mass, respectively, are

a. degree and gram.b. kelvin and kilogram.c. Celsius and milligram.d. degree and kilogram. e. kelvin and gram.


42. The SI base units of length and mass, respectively, are

a. centimeter and gram.b. inch and kilogram.c. meter and kilogram.d. meter and gram. e. inch and pound.


1-14

43. Which of the following is an SI base unit?

a. dyneb. newtonc. milliliterd. amperee. calorie


44. Which is a unit of surface area of a circular object?

a. pascalb. joulec. square meterd. cubic centimeter e. kilometer


45. The SI derived unit for area is

a. square centimeter.b. square yard.c. square kilometer.d. square meter.e. pascal.


1-15

46. The density of an object is the ratio of its mass to its volume. What is the derived SI unit for density?

a. kg m/s3 b. kg m/sc. kg/m3 d. m/s2 e. pounds per cubic inches


47. The momentum of an object is its mass times its velocity. What is the derived SI unit for momentum?

a. kg/m b. kg m/sc. g m/s d. m/s2 e. pounds per inches


48. The force experienced by an object is its mass times its acceleration. What is the derived SI unit for force?

a. kg m/s2 b. kg m/sc. g m/s d. m/s2 e. pounds per inches squared


1-16

49. The volume of a cylinder is r2h, where r is the radius and h is the height. What is the derived SI unit for the volume of a cylinder?

a. kg m/s3 b. literc. cm3 d. m3 e. cubic inches


50. The SI prefixes giga and micro, indicate respectively:

a. 109 and 10-6 b. 10-9 and 10-6

c. 106 and 10-3 d. 103 and 10-3 e. 10-9 and 10-3


51. The SI prefixes mega and nano indicate, respectively:

a. 109 and 10-6 b. 10-6 and 109

c. 106 and 10-9 d. 106 and 109 e. 10-6 and 10-9


1-17

52. The SI prefixes kilo and centi indicate, respectively:

a. 103 and 10-2 b. 106 and 10-1

c. 10-3 and 10-2 d. 10-6 and 102 e. 102 and 10-3


53. Which is the longest measurement?

a. 10 mm b. 10 dmc. 10 cm d. 10 m e. They are all the same measurement.


54. Which is the shortest measurement?

a. 10 mm b. 1 kmc. 10 cm d. 10 m e. They are all the same measurement.


1-18

55. Which is the shortest measurement?

a. 10 mm b. 1 kmc. 10 cm d. 10 in e. They are all the same measurement.


56. Which is the longest measurement?

a. 10 mm b. 10 dmc. 10 cm d. 10 in e. They are all the same measurement.

Answer: dSection 1.4Difficulty Level: hard

57. What is the number needed to complete the following: 1 dm = __ m?

a. 10 b. 20c. 1 d. 0.1 e. 0.01


1-19

58. What is the number needed to complete the following: 1 m = __ pm?

a. 10-6 b. 2.010-9

c. 10-12

d. 0.1 e. 1012


59. What is the number needed to complete the following: 1 g = __ kg?

a. 103 b. 2.010-9

c. 10-3

d. 0.1 e. 1012


60. What is the number needed to complete the following: 1 g = __ g?

a. 106 b. 10-9

c. 10-3

d. 0.1 e. 10-2


1-20

61. The boiling point of chlorine is -34.6 °C. This temperature expressed in Kelvin is

a. -30.3 Kb. 177.4 Kc. 238.6 Kd. 243.0 Ke. 307.6 K


62. Convert 25.4 K to oC.

a. -30.3 oCb. -247.8 oCc. -38.6 oCd. -13.8 oCe. -107.6 oC


63. Convert 79.0°F to oC.

a. 79.0 oCb. 26.1 oCc. 352 oCd. 45 oCe. 111 oC


1-21

64. Ammonia boils at -33.4°C. What temperature is this in °F?

a. -60.1 oFb. -92.1 oFc. -28.1 oFd. -18.5 oFe. 13.5 oF


65. The boiling point of barium is 725 °C. Determine the equivalent value in °F.

a. 435 °Fb. 1337 °Fc. 1247 °Fd. 1392 °Fe. 1273 °F


66. The melting point of a metal is listed in one handbook as 630.5 °C. Determine the equivalent value in °F.

a. 382.41 °Fb. 1103.3 °Fc. 1077.7 °Fd. 1166.9 °Fe. 1192.9 °F


1-22

67. The melting point of lead acetate, a white solid, is 280 °C. Determine the melting point of this compound in units of °F.

a. 446 °Fb. 472 °Fc. 504 °Fd. 536 °Fe. 562 °F


68. Convert 60.0°F to Kelvin.

a. 289 Kb. 15.6 Kc. 140 Kd. 413 Ke. 333 K


69. On a day in the summer of 1992, the temperature fell from 98 °F to 75 °F in just three hours. The temperature drop expressed in Celsius degrees (°C) was

a. 13 °Cb. 41 °Cc. 45 °Cd. 9 °Ce. 75 °C

Answer: aSection 1.4Difficulty Level: hard

1-23

70. On a day in the summer of 1976, the temperature fell from 95 °F to 75 °F in just three hours. The temperature drop expressed in Celsius degrees (°C) was

a. 11 °Cb. 13 °Cc. 18 °Cd. 20 °Ce. -12 °C


71. The melting point of antimony is listed in one handbook as 1167.3 °F. Expressed in Kelvin this temperature would be

a. 357.6 Kb. 496.8 Kc. 583.7 Kd. 894.2 Ke. 903.9 K


72. The highest temperature recorded in the athletic field house when the cooling units were being replaced and upgraded was 122.0 °F. Express this temperature in Kelvin.

a. 323.2 Kb. 337.6 K c. 341.0 Kd. 435.2 Ke. 492.8 K


1-24

73. A metal alloy melts at 874 K. What is this temperature in °F?

a. 302 °Fb. 365 °Fc. 1050 °Fd. 1082 °Fe. 1114 °F


74. The boiling point of carbonyl selenide is 251.4 K. What is this temperature in °F?

a. - 7.1 °Fb. - 44.1 °Fc. - 96.7 °Fd. 0.00 °Fe. +18.5 °F


75. A number resulting from a measurement was properly expressed in scientific notation as 3.170 10-2 meters (m). The number could also be written correctly as

a. 0.0317 mb. 0.03170 mc. 0.032 md. 317 me. 317.0 m


1-25

76. How many significant figures does the number 1.030 x 107 have?

a. 2b. 3c. 4d. 7e. 1


77. How many significant figures are in 5100.0 L?

a. 1b. 2c. 3d. 4e. 5


78. An electronic balance used in the mailroom displays tenths of a kilogram from 0 to 140 kg. How many significant figures should be used to express the mass of a package which has a mass between 80.2 and 83.5 kg?

a. 3b. 5c. 4d. 2e. 1


1-26

79. Which response gives the correct number of significant figures for all three of the following measurements? 7.103 cm, 0.00005 inch, and 1.3400 10-4 dm3

a. 3, 5, and 4b. 3, 1, and 3 c. 4, 1, and 3d. 4, 1, and 5e. 4, 5, and 5


80. How many significant figures should be displayed in the result of the operation, 8.5201 + 1.93?

a. 1b. 2c. 3d. 4e. 5


81. The number 0.0030600 is properly expressed in scientific notation as

a. 3.0600 10-2

b. 0.30600 10-2

c. 0.306 10-2

d. 3.06 10-3

e. 3.0600 10-3


1-27

82. The number 0.02100 is properly expressed in scientific notation as

a. 0.21 10-1

b. 2.1 10-2

c. 2.100 10-2

d. 21.0 10-3

e. 2.10 10-2


83. After evaluating the expression, 13 .726 + 0 . 027

8.221how many significant figures should be displayed in the result?

a. 1b. 2c. 3d. 4e. 5


84. Give the correct answer for the following problem with the correct number of significant figures.

(13.7 + 0.027)

a. 1.7b. 1.67c. 1.670d. 1.703e. 1.699


1-28

85. Give the correct answer for the following problem with the correct number of significant figures.

(1.5 x 10-4 x 61.3)

a. 2.0192b. 2.0c. 2.019d. 2.02e. 2.019195


86. Which of the following numbers has exactly three significant figures as written?

a. 300b. 12.0c. 4021d. 0.12e. 0.005


87. Which of the following numbers has exactly four significant figures as written?

a. 3150b. 0.921c. 4020d. 0.0068e. 170.0


1-29

88. When the expression, 412.272 + 0.00031 - 1.00797 + 0.000024 + 12.8, is evaluated, the result should be expressed as

a. 424b. 424.0c. 424.1d. 424.06e. 424.064364


89. When the expression, 16.0200 + 0.00048 - 11.184 - 221.1, is evaluated, the result should be expressed as

a. -216.3b. -216.26c. -216.2635d. -216.26352e. -2.2 102


90. Evaluate the expression to the correct number of significant figures.

0 .04616 × 0 . 082057 × 293. 300 . 654

a. 1.69b. 1.70c. 1.699d. 1.6987e. 1.69870


1-30

91. Evaluate the expression to the correct number of significant figures.

4 .268 × 0 .082057 × 373. 15744 .6760 .0

× 2 .688

a. 49.623b. 49.631c. 49.62d. 49.64e. 49.623202


92. 1657.3 grams of a compound are to be divided between 12 students. How many grams should each student receive? Express your answer with the correct number of significant figures.

a. 138.108 gb. 138.11 gc. 138.1 gd. 138 ge. 1.4 x 102 g


1-31

93. An instructor gives a student a 103.1 g sample of a compound. A student takes this sample and using one of the laboratory balances measures the sample 4 times. He got the following results:

105.1 g 104.9 g 105.2 g 105.1 gBased on these results, how would the student’s measurements best be characterized? Assume that the sample’s mass is actually 103.1 g.

a. The measurements are both accurate and precise.b. The measurements are accurate but not precise.c. The measurements are precise, but not accurate.d. The measurements are neither accurate nor precise.e. The measurements say nothing about accuracy or precision.


94. An instructor gives a student a 103.1 g sample of a compound. A student takes this sample and using one of the laboratory balances measures the sample 4 times. He got the following results:

108.1 g 105.9 g 101.2 g 107.1 gBased on these results, how would the student’s measurements best be characterized? Assume that the sample’s mass is actually 103.1 g.

a. The measurements are both accurate and precise.b. The measurements are accurate but not precise.c. The measurements are precise, but not accurate.d. The measurements are neither accurate nor precise.e. The measurements say nothing about accuracy or precision.


95. A distance of 1.8 10-2 meters is equal to

a. 1.8 micrometers.b. 1.8 millimeters.c. 0.18 meters.d. 1.8 centimeters.e. 18 kilometers.

Answer: dSection 1.6

1-32

Difficulty Level: medium

96. The diameter of a certain atom was found to be 2.35 10-8 cm. How many nanometers is this?

a. 2.35 101 nmb. 2.35 10-19 nmc. 2.35 10-15 nmd. 2.35 10-1 nme. 2.35 10-10 nm


97. How many micrometers are there in 3.672 km?

a. 3.672 106 micrometersb. 2.723 10-7 micrometersc. 2.723 10-4 micrometersd. 3.672 109 micrometerse. 3.672 103 micrometers


98. How many mm (millimeters) are there in 6.3 km?

a. 6.3 10-5 mmb. 6300 mmc. 6.3 104 mmd. 6.3 105 mme. 6.3 106 mm


1-33

99. How many cm3 are in 0.00424 dm3?

a. 0.0424 cm3

b. 0.424 cm3

c. 4.24 cm3

d. 0.00000424 cm3

e. 424 cm3


100. How many cubic inches are in 1.00 dm3? 1 in. = 2.54 cm.

a. 61.0 in3 b. 155 in3 c. 394 in3 d. 1.64 104 in3 e. 3.83 103 in3


101. Which one of the following represents the smallest distance?

a. 4.5 mmb. 0.20 inchc. 0.83 cmd. 0.73 me. 0.30 yard


1-34

102. How many m3 are in a 1.5 L bottle of soda?

a. 1.5 101 m3

b. 0.0015 m3

c. 0.015 m3

d. 0.00015 m3

e. 1.5 m3


103.One radio station operates on an assigned frequency of 96.3 megahertz while another one operates on an assigned frequency of 1280 kilohertz. What is the ratio of the larger to the smaller value?

a. 13.3b. 13.29c. 75.2d. 75.23e. 13.2918


104.One radio station operates on an assigned frequency of 88.1 megahertz while another one operates on an assigned frequency of 1460 kilohertz. What is the ratio of the larger to the smaller value?

a. 16.5b. 16.57c. 16.57208d. 60.3 e. 60.342


1-35

105.An industrial container was filled with 210.8 liters of a solvent. How many gallons of solvent does this container contain? 1 pint (pt) = 473.2 mL, 1 gallon (gal) = 8 pt.

a. 55.00 galb. 55.69 galc. 59.15 gald. 179.1 gal e. 798.0 gal


106.How many square meters are in a rectangular piece of carpet which measures 12.0 feet by 22.0 feet? 1 m = 39.37 in., 1 ft = 12 in.

a. 24.5 m2

b. 28.4 m2

c. 866 m2

d. 80.5 m2

e. 966 m2


107.How many square meters of floor space are in a room which has 225.0 square yards of floor space? 1 m = 39.37 in., 1 yard = 36 in.

a. 188.1 square metersb. 269.0 square metersc. 246.0 square metersd. 205.7 square meterse. 172.0 square meters


1-36

108.If a car has an EPA mileage rating of 3.0 101 miles per gallon, what is this rating in m L-1? 1 liter = 1 dm3, 1 gallon = 3.785 liter, 1 mile = 1.609 meter.

a. 13 m L-1

b. 200 m L-1

c. 180 m L-1

d. 70 m L-1

e. 11 m L-1


109.The diameter of a carbon atom is approximately 1 x 10-8 cm. What is this diameter when expressed in nanometers?

a. 1 x 10-19 nmb. 1 x 10-15 nmc. 1 x 101 nmd. 1 x 10-10 nme. 1 x 10-1 nm


110.How many milliliters are in 0.0050 L?

a. 0.50 mLb. 5.0 mLc. 0.50 mLd. 5.0 x 10-6 mLe. 5.0 x 103 mL


1-37

111.The density of gold, expressed in non-SI units is 19.3 g/cm3. In SI units, the density is

a. 0.0193 kg/cm3

b. 1.93 104 kg/cm3 c. 1.93 104 kg/m3 d. 193 kg/m3 e. 1.93 10-2 kg/m3


112. What is the volume of a 52.5 gram sample of nickel, if its density = 8.90 g/cm3?

a. 467 cm3

b. 0.170 cm3

c. 5.90 cm3

d. 43.6 cm3

e. 61.4 cm3


113. What is the volume of a 66.7 gram sample of vanadium (density = 6.11 g/cm3)?

a. 11.9 cm3

b. 9.92 cm3 c. 60.6 cm3

d. 10.9 cm3

e. 0.0916 cm3


1-38

114.A sample of zinc metal (density = 7.14 g/cm3) was submerged in a graduated cylinder containing water. The water level in the cylinder rose from 162.5 cm3 to 186.0 cm3. How many grams did the sample weigh?

a. 168 gb. 22.7 gc. 26.1 gd. 48.8 ge. 3.29 g


115.A sample of an alloy (density = 9.62 g/cm3) was submerged in a graduated cylinder containing water. The water level in the cylinder rose from 166.5 cm3 to 182.0 cm3. How many grams did the sample weigh?

a. 0.621 gb. 175 gc. 18.9 gd. 17.8 ge. 149 g


116."Isooctane", a fuel used in gasoline engines because it has an antiknock octane rating of 100, has a density of 0.6919 g/cm3. How many pounds would 20.4 gallons of this fuel (a typical full tank) weigh? 1 gallon = 3785 cm3 = 4 quart; 1 pound = 453.6 g

a. 77.2 poundsb. 246 poundsc. 118 poundsd. 24.2 poundse. 50.6 pounds


1-39

117.Mercury, which has a density of 13.595 g/cm3, is usually stored in iron vessels for shipment. These vessels typically have a capacity of 2.60 liters. How many pounds of mercury would a filled container hold? 1 pound = 0.4536 kg, 1 liter = 1 dm3 = 1000 cm3.

a. 77.9 poundsb. 86.7 poundsc. 11.5 poundsd. 16.0 poundse. 42.6 pounds


118. Iron has a density of 7.86 g/cm3. How many pounds does a block of iron with a volume of 1.650 cubic feet weigh? 1 pound = 0.4536 kg, 1 foot = 12 in., 1 in. = 2.54 cm.

a. 809.6 poundsb. 0.8715 poundsc. 871.1 poundsd. 491.2 poundse. 3.015 pounds


119.Iridium has a density of 22.65 g/cm3. A student has an iridium figurine on his desk which weighs 11.50 pounds. What is its volume, in cubic inches? 1 pound = 0.4536 kg, 1 inch = 2.54 cm.

a. 5.533 cubic inchesb. 9.410 cubic inchesc. 14.05 cubic inchesd. 35.70 cubic inchese. 90.67 cubic inches


1-40

120.The metric equivalent of a 55 gallon drum has a volume of 0.200 cubic meters. One such drum was filled with a colorless liquid, Sukanol, which has a density of 1.168 g/cm3. How many kg should this quantity of Sukanol weigh? 1000 cm3 = 1 L, 1000 L = 1 m3.

a. 24.3 kgb. 234 kgc. 243 kgd. 2.34 105 kg e. 500 kg


121.The metric equivalent of a 55 gallon drum has a volume of 0.200 cubic meters. One such drum was filled with a colorless liquid, Sukanol, which has a density of 1.168 g/cm3. How many pounds should this quantity of Sukanol weigh? 1000 cm3 = 1 L, 1000 L = 1 m3.

a. 53.6 lbb. 515 lbc. 536 lbd. 5.15 105 lb e. 1102 lb


122.A 55.25 gallon container was filled with an industrial solvent whose density is 1.146 g/cm3. How many kg should the solvent in the container weigh? 1 gallon (gal) = 3.785 liters (L) .

a. 23.9 kgb. 239.7 kgc. 239 kgd. 2.39 105 kg e. 500 kg


1-41

123.The density of iron is 7.86 g/cm3. What is the mass (in kg) of 20.00 cubic inches of iron? 1 inch = 2.54 cm, exactly.

a. 6.46 10-3 kgb. 4.17 10-2 kgc. 0.393 kgd. 2.54 kge. 2.58 kg


124.Acetone has a density of 0.791 g/mL. If 1 gallon = 3.7854 liters, how many kg should the contents of a 5.00 gallon container filled with acetone weigh?

a. 1.045 kgb. 12.6 kg c. 13.8 kg d. 15.0 kg e. 23.9 kg


125.The density of cadmium metal is 8.642 g/cm3. Given that 1 foot (ft) = 12 inches (in.), 1 in. = 2.54 cm, and 1 pound (lb) = 453.6 g, what is the density of cadmium in lb/ft3?

a. 17.70 lb/ft3

b. 141.6 lb/ft3

c. 539.5 lb/ft3

d. 263.4 lb/ft3

e. 327.7 lb/ft3


1-42

126.The density of chromium metal is 7.20 g/cm3. Given that 1 foot (ft) = 12 inches (in.), 1 in. = 2.54 cm, and 1 pound (lb) = 453.6 g, what is the density of chromium in lb/ft3?

a. 14.7 lb/ft3

b. 118 lb/ft3

c. 449 lb/ft3

d. 219 lb/ft3

e. 393 lb/ft3


127.The density of copper metal is 8.92 g/cm3. Given that 1 foot (ft) = 12 inches (in.), 1 in. = 2.54 cm, and 1 pound (lb) = 453.6 g, what is the density of copper in lb/ft3?

a. 18.3 lb/ft3

b. 146 lb/ft3

c. 557 lb/ft3

d. 272 lb/ft3

e. 317 lb/ft3


128.An empty volumetric flask, weighing 27.16 grams, has a volume of 100.4 cm3. How much would it weigh when filled with bromine, an element that has a density of 3.1028 g/cm3?

a. 59.51 gb. 284.4 gc. 311.5 gd. 338.7 ge. 395.8 g


1-43

129.Gold has a density of 19.3 g/cm3. How many pounds does a gold sphere weigh if it has a diameter of 5.20 inches? 1 pound = 0.4536 kg. The volume of a sphere = 4

3( π r3 ).

a. 16.3 poundsb. 19.7 poundsc. 51.3 poundsd. 63.7 poundse. 411 pounds


130. A spherical cannonball which has a volume given by4

3(π r3)

is made of an iron alloy and has a diameter of 9.55 inches and a density of 7.89 g/cm3. How many pounds does this cannonball weigh? 1 pound = 0.4536 kg, 1 inch = 2.54 cm.

a. 59.0 poundsb. 1.30 102 poundsc. 41.4 poundsd. 1.24 103 poundse. 21.0 pounds


131. A piece of silver (Ag) metal weighing 194.3 g is placed in a graduated cylinder containing 242.0 mL of water. The volume of water now reads 260.5 mL. From this data calculate the density of silver.

a. 10.5 g/cm3

b. 0.10 g/cm3

c. 0.0952 g/cm3

d. 1.34 g/cm3

e. 0.0134 g/cm3


1-44

132. A piece of silver (Ag) metal weighing 194.29 g is placed in a graduated cylinder containing 242.0 mL of water. The volume of water now reads 260.53 mL. From this data calculate the density of silver with the correct number of significant figures.

a. 10.49 g/mLb. 0.095 g/mLc. 0.09526 g/mLd. 1.3409 g/mLe. 10.485 g/mL


133. In determining the density of a rectangular metal bar, a student made the following measurements:length = 8.56 cmwidth = 2.0 cmheight = 1.865 cmmass = 52.7064 gCalculate the density of the metal to the correct number of significant figures.

a. 0.607 g/cm3

b. 1.6 g/cm3

c. 1.647 g/cm3

d. 0.60714 g/cm3

e. 0.61 g/cm3


1-45

134. Sulfuric acid has a specific gravity of 1.84 at a certain temperature. If the density of water at the same temperature is 62.4 pounds per cubic foot, how many cubic feet of the acid will weigh 44.5 kg? (1.0 kg = 2.20 pounds)

a. 2.04 ft3

b. 0.853 ft3 c. 13.0 ft3 d. 1.55 ft3 e. 0.0154 ft3


135. Ethanol has a specific gravity of 0.78 at a certain temperature. If the density of water at the same temperature is 62.4 pounds per cubic foot, how many cubic feet of the ethanol will weigh 19.3 kg? (1.0 kg = 2.20 pounds)

a. 4.15 ft3

b. 0.180 ft3 c. 0.397 ft3 d. 0.872 ft3 e. 48.7 ft3


136. Ethanol has a specific gravity of 0.78 at a certain temperature. If the density of water at the same temperature is 62.4 pounds per cubic foot, what is the density of ethanol at this temperature?

a. 4.15 lbs/ft3

b. 48.672 lbs/ft3 c. 0.0125 lbs/ft3 d. 80.0 lbs/ft3 e. 13.7 lbs/ft3


1-46

Fill-in-the-Blank Questions

137.A statement that describes something seen, heard, or smelled, is called an ____________.

Answer: observationSection 1.1 Difficulty Level: easy

138.A statement based on a series of observations is a ____________.

Answer: conclusionSection 1.1Difficulty Level: medium

139.A broad generalization based on the results from many experiments is called a__________.

Answer: scientific lawSection 1.1Difficulty Level: medium

140.Chemistry is particularly about the way substances undergo changes in ___________.

Answer: chemical reactionsSection 1.2Difficulty Level: easy

141.All the objects around us are examples of what are called __________.

Answer: matterSection 1.2Difficulty Level: easy

142.Substances that cannot be decomposed into simpler substances by chemical reactions are examples of __________ .

Answer: elementsSection 1.2Difficulty Level: easy

1-47

143.An abbreviation used to represent the name of an element is a __________ .

Answer: chemical symbolSection 1.2Difficulty Level: easy

144. The melting of lithium chloride is an example of a____________ .

Answer: physical changeSection 1.2Difficulty Level: easy

145. The burning of sulfur is an example of a____________ .

Answer: chemical changeSection 1.2Difficulty Level: easy

146. The dissolving of glucose in water is a ___________.


147. The evaporation of water from a saltwater solution until only salt is left is a ___________.


148. Bleaching of hair is a ___________.

Answer: chemical changeSection 1.2Difficulty Level: easy

1-48

149. Water has a freezing point of 0oC. This is a __________ of water.

Answer: physical property Section 1.3Difficulty Level: easy

150. Sodium metal reacts violently with water. This is a __________ of sodium metal.

Answer: chemical property Section 1.3Difficulty Level: easy

151.Aluminum metal reacts with oxygen to form an aluminum oxide. This is a __________ of aluminum metal.


152.Gold metal can be pressed into very thin sheets or foils. This is a __________ of aluminum metal.


153. Antimony has a high density of 6.697 g/cm3. This is a __________ of antimony.


154.Neon gas does not react with any metal at room temperature. This is a __________ of neon.


1-49

155. The SI prefix micro indicates _________.

Answer: 10-6

Section 1.4Difficulty Level: medium

156.A kilometer is ______ times longer than a centimeter.

Answer: 105


157.A 201 g sample weighs ______ mg.

Answer: 2.01 105 mgSection 1.4Difficulty Level: medium

158.A 1.54 L sample contains ______ mL.

Answer: 1.54 x 103 mLSection 1.4Difficulty Level: easy

159.A 405 nm is equivalent to ______ cm.

Answer: 4.05 x 10-5


160. Express the mass, 2.34 10-9 g, without scientific notation, and using the appropriate SI prefix _________.

Answer: 2.34 ngSection 1.4Difficulty Level: medium

1-50

161.Many home freezers maintain a temperature of 0.0 oF. Express this temperature in °C. ______

Answer: -17.8 °CSection 1.4Difficulty Level: medium

162.Many home freezers maintain a temperature of 0.0 oF. Express this temperature in Kelvin. ______

Answer: 255.4 KSection 1.4Difficulty Level: medium

163.Antimony melts at 630.63°C. Express this temperature in °F. ______

Answer: 1167.1°FSection 1.4Difficulty Level: medium

164. How many significant figures does the number 30.340 contain? ______

Answer: 5Section 2.3 Difficulty Level: easy

165. How many significant digits are there in the number 1.050 109? ______

Answer: 4Section 1.5Difficulty Level: medium

166. How many significant digits are there in the number 0.070120? ______


1-51

167. Express the result of the operation, 8.520 + 2.7 – 1.03, to the proper number of significant digits. ______

Answer: 10.2Section 1.5Difficulty Level: medium

168. Express the result of the operation, (8.317 x 2.7 x 3.159)/4.19, to the proper number of significant digits. ______


169. Express the result of the operation, 95.17 + 5.311 + 0.01275, to the proper number of significant digits. ______


170. What will be the cost, in dollars, of gasoline for a 3170 mile trip in a car pulling a trailer that delivers 13.30 miles per gallon, if the average price of gas is $1.449 cents per gallon? ______

Answer: $345Section 2.4Difficulty Level: medium

171.What will be the cost of gasoline for a 4710 mile automobile trip if the car delivers 27.35 miles per gallon of gasoline, and the average price of gas is $1.249 per gallon? ______

Answer: $215Section 1.6Difficulty Level: medium

1-52

172. A spot on a microchip which is 7500 nm (nanometers) in diameter is ______ pm (picometers) in diameter.

Answer: 7.5 106 pmSection 1.6Difficulty Level: medium

173. An object weighing 450 kg, expressed in megagrams (Mg), is ______ Mg.

Answer: 0.45 mgSection 1.6Difficulty Level: medium

174. The stone is a unit of weight that is still used in some areas of Europe. It is equal to exactly 14 pounds. Using this information what would a person weighing 14.9 stones weigh in kg? (1 kg = 2.20 lbs)

Answer: 94.8 kgSection 1.6Difficulty Level: medium

175. An organic liquid has a mass of 23.0 g. If the volume of the liquid is 29.75 mL, what is the density of the liquid?

Answer: 0.773 g/mLSection 1.7Difficulty Level: easy

176.A certain liquid has a density of 1.76 g/mL. If 56.1 mL of this liquid is measured out, what would be the mass of this liquid?

Answer: 98.7 g Section 1.7Difficulty Level: easy

1-53

177. An organic liquid has a mass of 23.0 g. If the liquid has a density of 0.785 g/cm3, what is the volume of this liquid? ________

Answer: 29.3 mLSection 1.7Difficulty Level: medium

178. A metal ball has a radius of 1.42 inches, and a density of 3.94 g/cm3. What is the mass in grams? 2.54 cm = 1 inch ________

Answer: 774 g Section 1.7Difficulty Level: hard

179.Liquid lead has a density of 10.66 g/cm3. How many kilograms of lead could fit into a box that is 5.00 cm long, 10.0 cm wide, and 10.0 cm high? ________

Answer: 5.33 kg Section 1.7Difficulty Level: hard

180. Sulfuric acid has a specific gravity of 1.84 at a certain temperature. If the density of water at the same temperature is 62.4 pounds per cubic foot, what is the density of sulfuric acid at the same temperature?

a. 115 lbs/ft3

b. 33.9 lbs/ft3 c. 74.3 lbs/ft3 d. 0.0295 lbs/ft3 e. 52.4 lbs/ft3


1-54

True and False Questions

181. The following equation, Pressure = Constant/Volume, is an example of a theory.

Answer: FalseSection 1.1Difficulty Level: medium

182. Theoretical models are used to help in explaining laws.

Answer: TrueSection 1.1Difficulty Level: medium

183. The observations made during an experiment are known as conclusions.


184. A sample of a pure compound contains two or more phases.

Answer: FalseSection 1.2Difficulty Level: easy

185. Mass indicates how much matter is in a given object.

Answer: TrueSection 1.2Difficulty Level: easy

186. A compound is an example of a mixture which can have variable composition.


1-55

187.A homogeneous mixture consists of only one chemical substance.


188.A mixture always contains more than one chemical substance. Answer: TrueSection 1.2Difficulty Level: easy

189.There is only one pure form for each element on the periodic table.


190. The mass of a water molecule is the same on the moon as it is on the earth.


191. A heterogeneous mixture can exist as only a single phase.


192. A homogeneous mixture can exist as only a single phase.


1-56

193. The evaporation of rubbing alcohol is a chemical change.


194. The combustion of gasoline into carbon dioxide gas and water vapor is both a chemical and physical change.


195. Density is one of the extensive properties of matter.


196. The volume of a sample is an extensive property of matter. Answer: TrueSection 1.3Difficulty Level: medium

197. The density of water is a physical property of water.


198. The combustibility of octane is a physical property of octane.


1-57

199. A liter of carbon tetrachloride is smaller than a quart of the same substance.


200. An increase of one Kelvin in temperature, is a smaller change than an increase of one degree Fahrenheit.


201. The measurement, 7.05 10-12 m, is the same measurement as 7.05 pm.


202. A large crowd attending a celebration in a metropolitan area was described as 450,000 in the morning newspaper the next day. A chemistry student stated that, mindful of the purpose of using scientific notation, this should be correctly expressed in scientific notation as 4.50000 105. The number expressed this way truly represents the crowd size, true or false?


203. Any number known accurately to six or more significant digits is defined as an exact number.


1-58

204. In determining the number of significant digits in the result of a calculation, exact numbers are considered as having a value to six significant digits.


205. Ambiguity in the number of significant digits in a number being expressed can be eliminated by proper use of scientific notation.


206. The result of the operation, 8.52010 7.90, should be expressed as 67.3088. Answer: FalseSection 1.5Difficulty Level: medium

207. A 15 km distance run is a shorter run than a 10 mile distance run.


208. A 5.00 pound bag of sugar weighs more than a 2.50 kg bag of sugar.


209. A piece of carpet which measures 44.0 square yards is smaller than a piece of carpet which measures 44.0 square meters.


1-59

210. A liquid which has a volume of 8.50 mL, and a mass of 7.05 g, has a density of 0.829 g/cm3.


211. A liquid has a density of 3.10 g/mL. A 17.7 g sample of this liquid has a volume of 55 mL.


212. The density of a metal reported as 1.74 g/cm3, also has a density of 1.74 kg/m3.

Answer: FalseSection 1.7Difficulty Level: hard

213. Yeast cells feed on glucose in grape juice to give ethyl alcohol and carbon dioxide during the fermentation reaction.

Answer: TrueSection: Chemistry Outside the Classroom 2.1Difficulty Level: medium

214. A very quick way to determine the sugar content of grapes is to determine the density of the grape juice using a hydrometer.


215. A sample of wine from grape juice can be distilled to obtain a mixture of alcohol and water.


1-60

216. One way to determine the alcohol content of wine is to determine the specific gravity of the wine using a hydrometer.

Answer: FalseSection: Chemistry Outside the Classroom 1.1Difficulty Level: medium

Critical Thinking Questions

217. A young high school student has invented a new temperature scale, the Zuban scale (his last name, of course). In common with the Kelvin, Celsius, and Fahrenheit scales, it is a linear scale.

According to Zuban, 1) the boiling point of water which is 100.00 °C = 373.15 K = 0.00 °Z2) the boiling point of sulfur which is 444.60 °C = 717.75 K = 250.00 °Z3) the melting point of silver which is 960.15 °C = 1233.30 K = 624.02 °Z

Calculate the value of absolute zero on the Zuban Scale. ________

Answer: -270.71 °ZSection 1.4 Difficulty Level: hard

218. Carl, a ninth grade whiz kid, has invented a new temperature scale, the Vitellan scale (his last name, of course). In common with the Kelvin, Celsius, and Fahrenheit scales, it is a linear scale. According to Carl,

1) the melting point of benzene which is 5.53 °C = 0.00 °V2) the boiling point of benzene which is 80.10 °C = 100.00 °V3) the melting point of lead which is 327.50 °C = 431.77 °V

Calculate the value for the melting point of mercury ( -38.86 °C) on the Vitellan scale. ______

Answer: -59.53 °VSection 1.4Difficulty Level: hard

1-61

219. A number resulting from a measurement was properly expressed in scientific notation as 2.1 10-3 meters (m). The number could also be correctly written as

a. 0.0021 mb. 0.002100 mc. 0.00021 md. 2.1000 me. 21000 m


220. Solve the following: (628.83 – 627.71) 124 122.08


221. Solve the following: (2.15 106 + 3.2 102)/(2.332 + 22.0005 + 0.9861)

a. 1.45b. 48.8c. 233.1d. 106e. 1,080.2


222. If 1 meter = 39.37 inch and 1 foot = 12.00 inch, calculate the relationship to four significant digits, which will convert cubic feet into cubic meters directly. 1 ft3 = ______ m3


1-62

223. A home aquarium measures 17.0 inches wide, 17.0 inches long and 8.50 inches high. What is the volume in liters?

Answer: 40.2 LSection 1.6Difficulty Level: hard

224. Express 109 miles per hour, in meters per second. Answer: 48.7 m/sSection 1.6Difficulty Level: hard

225. Consider this data from a lab, concerning the mass and the volume of water displaced in a graduated cylinder by introduction of a metal sample to the cylinder:

Mass of weighing cup = 0.452 gMass of weighing cup + metal sample = 72.943 gVolume of water in cylinder = 15.2 cm3

When the metal sample was carefully lowered into the graduated cylinder, the water above the submerged metal sample rose to the 19.0 cm3 mark. What is the density of the metal?

a. 2.2 g cm-3

b. 3.8 g cm-3

c. 4.8 g cm-3

d. 19 g cm-3

e. 19.2 g cm-3


226. A spherical cannonball made of an iron alloy has a specific gravity of 7.88, and weighs 22.12 pounds. It has a diameter of 13.46 cm. On the other hand, spent uranium (from processing which removes the commercially important rare isotope) has a specific gravity of 19.05. How many pounds would a uranium cannonball of the same dimensions as the iron cannonball weigh?

volume 4

3(π r3)

Answer: 53.5 poundsSection 1.7

1-63

Difficulty Level: hard

227. A spherical cannonball made of an iron alloy has a density of 7.86 g/cm3, and weighs 22.12 pounds. On the other hand, spent uranium (from processing which removes the commercially important rare isotope) has a density of 19.05 g/cm3. What would be the diameter, in cm, of a uranium round shot which has exactly twice the weight as the iron ball described above? 1 pound = 0.4536 kg. volume 4

3(π r3 )

Answer: 12.62 cmSection 1.7Difficulty Level: hard

228. Some students in the AP chemistry class have come up with an idea they would like to have tested which involves collaboration with two or three DOD facilities. They want to test two small muzzle loading cannons like the ones used in the 18th century. One would be using spherical cannonballs made of iron, while the other would be using spherical cannonballs made of spent uranium. Both cannons will be using cannonballs with a diameter of 5.000 inches. If uranium has a density of 19.05 g/cm3, what would be the mass, in pounds, of the

uranium cannonballs? 1 pound = 453.6 g, 1 inch = 2.54 cm exactly. volume 4

3(π r3 )

___________

Answer: 45.04 poundsSection 1.7Difficulty Level: hard

229. Iron has a density of 7.86 g/cm3. As part of their exam, students in the junior class at a boarding school were to weigh a metal sphere, measure its diameter and calculate its density. Some of the seniors sneaked into the lab the weekend before, took the iron sphere, took it downtown, and had the interior partially hollowed and the surface repaired so it wouldn't be noticed and replaced it in the cabinet late on Sunday. The junior students who had this iron sphere for their "unknown" obtained 9.30 cm for the diameter and 2.44 kg for the mass. What value should they have reported for the mass of the sphere if it had not been tampered with, and what was the volume of the hollowed out space in the interior of the

sphere? volume 4

3(π r3 )

___________________

Answer: 3.31 kg and 111 cm3

Section 1.7Difficulty Level: hard

1-64

230. Solid antimony has a density of 6.70 g/cm3. Liquid antimony has a density of 6.53 g/cm3. If a 1.34 kg sample of liquid antimony is allowed to cool into a solid by how much will the volume of the sample change?

Answer: 5.21 cm3

Section 1.7Difficulty Level: hard

1-65

Documents

testbankbyte.comtestbankbyte.com/wp-content/uploads/2016/09/ch011.docx · Web viewb.a statement describing a relationship between phenomena that is always the same under the same