Verified Test Bank Scientific Measurements Chapter 1 - Solution Bank | Chemistry Molecular Nature 8e by Neil D. Jespersen. DOCX document preview.
Chemistry: Molecular Nature of Matter, 8e (Jespersen)
Chapter 1 Scientific Measurements
1) A tentative explanation used to explain observed facts or predict future results is called
A) the scientific method.
B) a scientific law.
C) a theory.
D) a hypothesis.
E) an empirical fact.
Diff: 1
Section: 1.1
2) A broad generalization based on the results of many experiments over time is called
A) the scientific method.
B) a scientific law.
C) a theory.
D) a hypothesis.
E) an empirical fact.
Diff: 1
Section: 1.1
3) Which of the following is false?
A) Theories can be revised as more data becomes available.
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.
Diff: 2
Section: 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.
Diff: 1
Section: 1.1
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.
Diff: 2
Section: 1.1
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.
Diff: 2
Section: 1.1
7) An example of an element is
A) tin metal, Sn.
B) water, H2O.
C) benzene, C6H6.
D) carbon dioxide gas, CO2.
E) ammonium nitrate, NH4NO3.
Diff: 1
Section: 1.2
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.
Diff: 1
Section: 1.2
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.
Diff: 1
Section: 1.2
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.
Diff: 1
Section: 1.2
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 oxygen
E) The table salt in the warehouse container had very large chunks in it.
Diff: 2
Section: 1.2
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.
Diff: 2
Section: 1.2
13) Which is an example of a physical change?
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.
Diff: 2
Section: 1.2
14) Which is an example of a chemical change?
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.
Diff: 2
Section: 1.2
15) Which is an example of a physical change?
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.
Diff: 2
Section: 1.2
16) Which is an example of a physical change?
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.
Diff: 2
Section: 1.2
17) Which is an example of both a physical and a chemical change?
Hint: Think about the what is occurring over the course of time in each choice. Remember, phase change is physical.
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.
Diff: 3
Section: 1.2
18) Which is an example of both a physical and a chemical change?
Hint: Think about where the wax could have gone and how.
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) As a candle burns the wax melts down the side. When the candle is done burning, much of the wax is gone.
Diff: 3
Section: 1.2
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.
Diff: 2
Section: 1.2
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.
Diff: 1
Section: 1.2
21) Which is an example of a chemical change?
A) the separation of air into oxygen, nitrogen, and other components
B) the separation of a compound into its elements
C) the separation of gases from liquids
D) the separation of a mixture into its components
E) the separation of solids from liquids
Diff: 2
Section: 1.2
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 for a period of time, sugar turns dark brown.
E) Grape juice left in an open, unrefrigerated container turns sour.
Diff: 1
Section: 1.2
23) Which is an example of a physical change?
A) A piece of '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 a stain on a white shirt.
D) Bubbles form on an egg shell when it is placed in vinegar.
E) A portion of a figurine dissolves after being placed in the container of acid.
Diff: 1
Section: 1.2
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 that 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.
Diff: 1
Section: 1.2
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.
Diff: 1
Section: 1.2
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.
Diff: 1
Section: 1.2
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.
Diff: 1
Section: 1.2
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.
Diff: 1
Section: 1.3
29) Which is an example of a physical property?
A) corrosiveness of sulfuric acid
B) toxicity of cyanide
C) flammability of gasoline
D) neutralization of stomach acid with an antacid
E) Lead becomes a liquid when heated to 601 °C.
Diff: 2
Section: 1.3
30) Which is an example of a physical property?
A) Dynamite explodes.
B) Meat rots if it is not refrigerated.
C) Honey tastes sweet.
D) Ice floats on top of liquid water.
E) A silver platter tarnishes over time.
Diff: 1
Section: 1.3
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) If solid sodium is put in ethanol, it will produce hydrogen gas.
Diff: 2
Section: 1.3
32) Water can also exist as a gas that is called
A) ice.
B) steam.
C) evaporation.
D) molecules.
E) atomic water.
Diff: 2
Section: 1.3
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 in composition that a substance undergoes.
D) A property which cannot be seen.
E) A property which is considered hypothetical.
Diff: 2
Section: 1.3
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.
Diff: 2
Section: 1.3
35) Which is an example of a chemical property?
A) combustibility
B) volatility
C) viscosity
D) malleability
E) ductility
Diff: 2
Section: 1.3
36) Which is an example of an intensive property of matter?
A) color
B) volume
C) mass
D) weight
E) length
Diff: 2
Section: 1.3
37) Which is an example of an intensive property of matter?
A) height
B) volume
C) length
D) weight
E) melting point
Diff: 2
Section: 1.3
38) Which is an example of an extensive property of matter?
A) color
B) density
C) mass
D) melting point
E) flash point
Diff: 2
Section: 1.3
39) Which is an example of an extensive property of matter?
A) surface area
B) boiling point
C) density
D) hardness
E) freezing point
Diff: 2
Section: 1.3
40) The kilo is
A) 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).
Diff: 2
Section: 1.3
41) The SI base units of temperature and mass, respectively, are
A) degree and gram.
B) kelvin and kilogram.
C) degree Celsius and milligram.
D) degree and kilogram.
E) kelvin and gram.
Diff: 1
Section: 1.4
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.
Diff: 2
Section: 1.4
43) Which of the following is an SI base unit?
A) degree Fahrenheit
B) foot
C) milliliter
D) ampere
E) gram
Diff: 2
Section: 1.4
44) Which is a unit of surface area of a spherical object?
A) pascal
B) joule
C) square meter
D) cubic centimeter
E) kilometer
Diff: 2
Section: 1.4
45) The SI derived unit for area is
A) square centimeter.
B) square yard.
C) square kilometer.
D) square meter.
E) pascal.
Diff: 1
Section: 1.4
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/s
C) kg/m3
D) m/s2
E) pounds per cubic inches
Diff: 2
Section: 1.4
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/s
C) g m/s
D) m/s2
E) pounds per inch
Diff: 2
Section: 1.4
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) cg m/s
C) g m/s2
D) m/s2
E) pounds per inches squared
Diff: 2
Section: 1.4
49) The volume of a cylinder is π r2h, where r is the radius and h is the height. What is the derived SI unit for the volume of a cylinder?
Hint: The SI unit for length is the meter, m.
A) kg m/s3
B) liter
C) cm3
D) m3
E) cubic inches
Diff: 3
Section: 1.4
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
Diff: 2
Section: 1.4
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
Diff: 1
Section: 1.4
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
Diff: 1
Section: 1.4
53) Which is the longest measurement?
A) 10 mm
B) 10 dm
C) 10 cm
D) 10 μm
E) They are all the same measurement.
Diff: 1
Section: 1.4
54) Which is the shortest measurement?
A) 10 mm
B) 1 km
C) 10 cm
D) 10 μm
E) They are all the same measurement.
Diff: 2
Section: 1.4
55) Which is the shortest measurement?
A) 10 mm
B) 1 km
C) 10 cm
D) 10 in
E) They are all the same measurement.
Diff: 2
Section: 1.4
56) Which is the longest measurement?
A) 10 mm
B) 10 dm
C) 10 cm
D) 10 in
E) They are all the same measurement.
Diff: 2
Section: 1.4
57) What is the number needed to complete the following: 1 dm = ________ m?
Hint: Think about the prefix deci (d) and what it means.
A) 10
B) 20
C) 1
D) 0.1
E) 0.01
Diff: 3
Section: 1.4
58) What is the number needed to complete the following: 1 m = ________ pm?
A) 10-6
B) 2.0 × 10-9
C) 10-12
D) 0.1
E) 1012
Diff: 2
Section: 1.4
59) What is the number needed to complete the following: 1 g = ________ kg?
A) 103
B) 2.0 × 10-9
C) 10-3
D) 0.1
E) 1012
Diff: 2
Section: 1.4
60) What is the number needed to complete the following: 1 g = ________ μg?
A) 106
B) 10-9
C) 10-3
D) 0.1
E) 10-2
Diff: 2
Section: 1.4
61) The boiling point of chlorine is 34.6 °C. This temperature expressed in Kelvin is
A) 30.3 K
B) 177.4 K
C) 238.6 K
D) 243.0 K
E) 307.6 K
Diff: 2
Section: 1.4
62) Convert 25.4 K to °C.
A) 30.3 °C
B) -247.8 °C
C) -38.6 °C
D) -13.8 °C
E) -107.6 °C
Diff: 1
Section: 1.4
63) Convert 79.0°F to °C.
A) 79.0 °C
B) 26.1 °C
C) 352 °C
D) 45 °C
E) 111 °C
Diff: 1
Section: 1.4
64) Ammonia boils at -33.4°C. What temperature is this in °F?
A) -60.1 °F
B) -92.1 °F
C) -28.1 °F
D) -18.5 °F
E) 13.5 °F
Diff: 2
Section: 1.4
65) The boiling point of barium is 725 °C. Determine the equivalent value in °F.
A) 435 °F
B) 1337 °F
C) 1247 °F
D) 1392 °F
E) 1273 °F
Diff: 2
Section: 1.4
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 °F
B) 1103.3 °F
C) 1077.7 °F
D) 1166.9 °F
E) 1192.9 °F
Diff: 2
Section: 1.4
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 °F
B) 472 °F
C) 504 °F
D) 536 °F
E) 562 °F
Diff: 2
Section: 1.4
68) Convert 60.0°F to Kelvin.
A) 289 K
B) 15.6 K
C) 140 K
D) 413 K
E) 333 K
Diff: 2
Section: 1.4
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
Hint: You must convert the temperatures before taking the difference.
A) 13 °C
B) 41 °C
C) 45 °C
D) 9 °C
E) 75 °C
Diff: 3
Section: 1.4
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
Hint: You must convert the temperatures before taking the difference.
A) 11 °C.
B) 13 °C.
C) 18 °C.
D) 20 °C.
E) -12 °C.
Diff: 3
Section: 1.4
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 K.
B) 496.8 K.
C) 583.7 K.
D) 894.2 K.
E) 903.9 K.
Diff: 2
Section: 1.4
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 K
B) 337.6 K
C) 341.0 K
D) 435.2 K
E) 492.8 K
Diff: 2
Section: 1.4
73) A metal alloy melts at 874 K. What is this temperature in °F?
A) 302 °F
B) 365 °F
C) 1050 °F
D) 1082 °F
E) 1114 °F
Diff: 2
Section: 1.4
74) The boiling point of carbonyl selenide is 251.4 K. What is this temperature in °F?
A) -7.2 °F
B) 44.1 °F
C) 96.7 °F
D) 0.00 °F
E) +18.5 °F
Diff: 2
Section: 1.4
75) A number resulting from a measurement was properly expressed in scientific notation as 
. The number could also be written correctly as
A) 0.0317 m
B) 0.03170 m
C) 0.032 m
D) 317 m
E) 317.0 m
Diff: 2
Section: 1.4
76) How many significant figures does the number 1.030 × 107 have?
A) 2
B) 3
C) 4
D) 7
E) 1
Diff: 2
Section: 1.5
77) How many significant figures are in 5100.0 L?
A) 1
B) 2
C) 3
D) 4
E) 5
Diff: 1
Section: 1.5
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) 3
B) 5
C) 4
D) 2
E) 1
Diff: 1
Section: 1.5
79) Which response gives the correct number of significant figures for each of the three following measurements, in order? 7.103 cm, 0.00005 inch, and 1.3400 × 104 dm3
A) 3, 5, and 4
B) 3, 1, and 3
C) 4, 1, and 3
D) 4, 1, and 5
E) 4, 5, and 5
Diff: 1
Section: 1.5
80) How many significant figures should be displayed in the result of the operation, 8.5201 + 1.93?
A) 1
B) 2
C) 3
D) 4
E) 5
Diff: 1
Section: 1.5
81) The number 0.0030600 is properly expressed in scientific notation as
A) 3.0600 × 102.
B) 0.30600 × 102.
C) 0.306 × 102.
D) 3.06 × 103.
E) 3.0600 × 103.
Diff: 1
Section: 1.5
82) The number 0.02100 is properly expressed in scientific notation as
A) 0.21 × 101.
B) 2.1 × 102.
C) 2.100 × 102.
D) 21.0 × 103.
E) 2.10 × 102.
Diff: 1
Section: 1.5
83) After evaluating the expression,
how many significant figures should be displayed in the result?
A) 1
B) 2
C) 3
D) 4
E) 5
Diff: 1
Section: 1.5
84) Give the correct answer for the following problem with the correct number of significant figures.
(13.7 + 0.027) ÷ 8.221
A) 1.7
B) 1.67
C) 1.670
D) 1.703
E) 1.699
Diff: 2
Section: 1.5
85) Give the correct answer for the following problem with the correct number of significant figures.
(1.5 × 10-4 × 61.3) + 2.01
A) 2.0192
B) 2.0
C) 2.019
D) 2.02
E) 2.019195
Diff: 2
Section: 1.5
86) Which of the following numbers has exactly three significant figures as written?
A) 300
B) 12.0
C) 4021
D) 0.12
E) 0.005
Diff: 2
Section: 1.5
87) Which of the following numbers has exactly four significant figures as written?
A) 3150
B) 0.921
C) 4020
D) 0.0068
E) 170.0
Diff: 2
Section: 1.5
88) When the expression, 412.272 + 0.00031 - 1.00797 + 0.000024 + 12.8, is evaluated, the result should be expressed as
A) 424
B) 424.0
C) 424.1
D) 424.06
E) 424.064364
Diff: 2
Section: 1.5
89) When the expression, 16.0200 + 0.00048 11.184 221.1, is evaluated, the result should be expressed as
A) 216.3
B) 216.26
C) 216.2635
D) 216.26352
E) 2.2 × 102
Diff: 2
Section: 1.5
90) Evaluate the expression to the correct number of significant figures.
A) 1.69
B) 1.70
C) 1.699
D) 1.6987
E) 1.69870
Diff: 2
Section: 1.5
91) Evaluate the expression to the correct number of significant figures.
A) 49.623
B) 49.631
C) 49.62
D) 49.64
E) 49.623202
Diff: 2
Section: 1.5
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 g
B) 138.11 g
C) 138.1 g
D) 138 g
E) 1.4 × 102 g
Diff: 2
Section: 1.5
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 g
Based on these results, how would the student's measurements best be characterized? Assume that the sample's mass is actually 102.1 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.
Diff: 2
Section: 1.5
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 g
Based 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.
Diff: 2
Section: 1.5
95) A distance of 1.8 × 102 meters is equal to
A) 1.8 micrometers.
B) 1.8 millimeters.
C) 0.18 meters.
D) 1.8 centimeters.
E) 18 kilometers.
Diff: 1
Section: 1.5
96) The diameter of a certain atom was found to be 2.35 × 108 cm. How many nanometers is this?
A) 2.35 × 101 nm
B) 2.35 × 10-19 nm
C) 2.35 × 10-15 nm
D) 2.35 × 10-1 nm
E) 2.35 × 10-10 nm
Diff: 2
Section: 1.6
97) How many micrometers are there in 3.672 km?
A) 3.672 × 106 micrometers
B) 2.723 × 10-7 micrometers
C) 2.723 × 10-4 micrometers
D) 3.672 × 109 micrometers
E) 3.672 × 103 micrometers
Diff: 2
Section: 1.6
98) How many mm (millimeters) are there in 6.3 km?
A) 6.3 × 10-5 mm
B) 6300 mm
C) 6.3 × 104 mm
D) 6.3 × 105 mm
E) 6.3 × 106 mm
Diff: 2
Section: 1.6
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
Diff: 2
Section: 1.6
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
Diff: 2
Section: 1.6
101) Which one of the following represents the smallest distance?
A) 4.5 mm
B) 0.20 inch
C) 0.83 cm
D) 0.73 m
E) 0.30 yard
Diff: 2
Section: 1.6
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
Diff: 2
Section: 1.6
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) 13.3
B) 13.29
C) 75.2
D) 75.23
E) 13.2918
Diff: 2
Section: 1.6
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) 16.5
B) 16.57
C) 16.57208
D) 60.3
E) 60.342
Diff: 2
Section: 1.6
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 gal
B) 55.69 gal
C) 59.15 gal
D) 179.1 gal
E) 798.0 gal
Diff: 2
Section: 1.6
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.
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 24.5 m2
B) 28.4 m2
C) 866 m2
D) 80.5 m2
E) 966 m2
Diff: 3
Section: 1.6
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.
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 188.1 square meters
B) 269.0 square meters
C) 246.0 square meters
D) 205.7 square meters
E) 172.0 square meters
Diff: 3
Section: 1.6
108) If a car has an EPA mileage rating of 3.0 × 101 miles per gallon, what is this rating in
km L-1? 1 liter = 1 dm3, 1 gallon = 3.785 liter, 1 mile = 1.609 kilometer.
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 13 km L-1
B) 200 km L-1
C) 180 km L-1
D) 70 km L-1
E) 11 km L-1
Diff: 3
Section: 1.6
109) The diameter of a carbon atom is approximately 1 × 10-8 cm. What is this diameter when expressed in nanometers?
A) 1 × 10-19 nm
B) 1 × 10-15 nm
C) 1 × 101 nm
D) 1 × 10-10 nm
E) 1 × 10-1 nm
Diff: 3
Section: 1.6
110) How many milliliters are in 0.0050 L?
A) 0.50 mL
B) 5.0 mL
C) 0.050 mL
D) 5.0 × 10-6 mL
E) 5.0 × 103 mL
Diff: 2
Section: 1.6
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
Diff: 1
Section: 1.6
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
Diff: 2
Section: 1.7
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
Diff: 2
Section: 1.7
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. What was the mass of the zinc sample?
A) 168 g
B) 22.7 g
C) 26.1 g
D) 48.8 g
E) 3.29 g
Diff: 2
Section: 1.7
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. What was the mass of the sample?
A) 0.621 g
B) 175 g
C) 18.9 g
D) 17.8 g
E) 149 g
Diff: 2
Section: 1.7
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 pounds
B) 246 pounds
C) 118 pounds
D) 24.2 pounds
E) 50.6 pounds
Diff: 2
Section: 1.7
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 pounds
B) 86.7 pounds
C) 11.5 pounds
D) 16.0 pounds
E) 42.6 pounds
Diff: 2
Section: 1.7
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 pounds
B) 0.8715 pounds
C) 871.1 pounds
D) 491.2 pounds
E) 3.015 pounds
Diff: 2
Section: 1.7
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 inches
B) 9.410 cubic inches
C) 14.05 cubic inches
D) 35.70 cubic inches
E) 90.67 cubic inches
Diff: 2
Section: 1.7
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 kg
B) 234 kg
C) 243 kg
D) 2.34 × 105 kg
E) 500 kg
Diff: 2
Section: 1.7
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, 1 pound = 0.4536 kg.
A) 53.6 lb
B) 515 lb
C) 536 lb
D) 5.15 × 105 lb
E) 1102 lb
Diff: 2
Section: 1.7
122) A 55.25 gallon container was filled with an industrial solvent whose density is 1.146 g/cm3. How many kg of solvent are in the container? 1 gallon (gal) = 3.785 liters (L).
A) 23.9 kg
B) 239.7 kg
C) 239 kg
D) 2.39 × 105 kg
E) 500 kg
Diff: 2
Section: 1.7
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
A) 6.46 × 103 kg
B) 4.17 × 102 kg
C) 0.393 kg
D) 2.54 kg
E) 2.58 kg
Diff: 2
Section: 1.7
124) Acetone has a density of 0.791 g/mL. If 1 gallon = 3.7854 liters, how many kg of acetone are in a 5.00 gallon container filled with acetone?
A) 1.045 kg
B) 12.6 kg
C) 13.8 kg
D) 15.0 kg
E) 23.9 kg
Diff: 2
Section: 1.7
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?
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
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
Diff: 3
Section: 1.7
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?
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 14.7 lb/ft3
B) 118 lb/ft3
C) 449 lb/ft3
D) 219 lb/ft3
E) 393 lb/ft3
Diff: 3
Section: 1.7
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?
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 18.3 lb/ft3
B) 146 lb/ft3
C) 557 lb/ft3
D) 272 lb/ft3
E) 317 lb/ft3
Diff: 3
Section: 1.7
128) An empty volumetric flask, weighing 27.16 grams, has a volume of 100.4 cm3. What is the flask's mass when filled with bromine, an element that has a density of 3.1028 g/cm3?
Hint: The mass of the flask itself will not change but must be considered in the final answer.
A) 59.51 g
B) 284.4 g
C) 311.5 g
D) 338.7 g
E) 395.8 g
Diff: 3
Section: 1.7
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 = 
(πr3)
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 16.3 pounds
B) 19.7 pounds
C) 51.3 pounds
D) 63.7 pounds
E) 411 pounds
Diff: 3
Section: 1.7
130) A spherical cannonball, which has a volume given by
(πr3)
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.
Hint: Recall the diameter is twice the radius. Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 59.0 pounds
B) 1.30 × 102 pounds
C) 41.4 pounds
D) 1.24 × 103 pounds
E) 21.0 pounds
Diff: 3
Section: 1.7
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
Diff: 2
Section: 1.7
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/mL
B) 0.095 g/mL
C) 0.09526 g/mL
D) 1.3409 g/mL
E) 10.485 g/mL
Diff: 2
Section: 1.7
133) In determining the density of a rectangular metal bar, a student made the following measurements:
length = 8.56 cm
width = 2.0 cm
height = 1.865 cm
mass = 52.7064 g
Calculate the density of the metal to the correct number of significant figures.
A) 0.607 g/cm3
B) 1.7 g/cm3
C) 1.647 g/cm3
D) 0.60714 g/cm3
E) 0.61 g/cm3
Diff: 2
Section: 1.7
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 have a mass of 44.5 kg? (1.0 kg = 2.20 pounds)
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 2.04 ft3
B) 0.853 ft3
C) 13.0 ft3
D) 1.55 ft3
E) 0.0154 ft3
Diff: 2
Section: 1.7
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)
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
A) 4.15 ft3
B) 0.180 ft3
C) 0.397 ft3
D) 0.872 ft3
E) 48.7 ft3
Diff: 3
Section: 1.7
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?
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
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
Diff: 3
Section: 1.7
137) A statement that describes something seen, heard, or smelled, is called a(n) ________.
Diff: 1
Section: 1.1
138) A statement based on a series of observations is a(n) ________.
Diff: 1
Section: 1.1
139) A broad generalization based on the results from many experiments is called a(n) ________.
Diff: 2
Section: 1.1
140) Chemistry is particularly about the way substances undergo changes in ________.
Diff: 2
Section: 1.1
141) All the objects around us are examples of what is called ________.
Diff: 1
Section: 1.2
142) Substances that cannot be decomposed into simpler substances by chemical reactions are examples of ________.
Diff: 1
Section: 1.2
143) An abbreviation used to represent the name of an element is a(n) ________.
Diff: 1
Section: 1.2
144) The melting of lithium chloride is an example of a(n) ________ change.
Diff: 1
Section: 1.2
145) The burning of sulfur is an example of a ________ change.
Diff: 1
Section: 1.2
146) The dissolving of glucose in water is a ________ change.
Diff: 1
Section: 1.2
147) The evaporation of water from a saltwater solution until only salt is left is a ________ change.
Diff: 1
Section: 1.2
148) Bleaching of hair is a ________ change.
Diff: 1
Section: 1.2
149) Water has a freezing point of 0°C. This is a ________ property of water.
Diff: 1
Section: 1.2
150) Sodium metal reacts violently with water. This is a ________ property of sodium metal.
Diff: 1
Section: 1.3
151) Aluminum metal reacts with oxygen to form an aluminum oxide. This is a ________ of aluminum metal.
Diff: 1
Section: 1.3
152) Gold metal can be pressed into very thin sheets or foils. This is a ________ property of aluminum metal.
Diff: 1
Section: 1.3
153) Antimony has a high density of 6.697 g/cm3. This is a ________ property of antimony.
Diff: 1
Section: 1.3
154) Neon gas does not react with any metal at room temperature. This is a ________ property of neon.
Diff: 1
Section: 1.3
155) The SI prefix micro indicates ________.
Diff: 1
Section: 1.3
156) A kilometer is ________ times longer than a centimeter.
Diff: 2
Section: 1.4
157) A 201 g sample has a mass of ________ mg. (Answer in scientific notation.)
Diff: 2
Section: 1.4
158) A 1.54 L sample contains ________ mL. (Answer in scientific notation.)
Diff: 2
Section: 1.4
159) A 405 nm is equivalent to ________ cm. (Answer in scientific notation.)
Diff: 1
Section: 1.4
160) Express the mass 2.34 × 10-9 g, without scientific notation, and using the appropriate SI prefix for the answer to have two decimal places. ________
Diff: 2
Section: 1.4
161) Many home freezers maintain a temperature of 0.0 °F. Express this temperature in °C. ________
Diff: 2
Section: 1.4
162) Many home freezers maintain a temperature of 0.0 oF. Express this temperature in Kelvin. ________
Diff: 2
Section: 1.4
163) Antimony melts at 630.63°C. Express this temperature in °F. ________
Diff: 2
Section: 1.4
164) How many significant figures does the number 30.340 contain? ________
Diff: 2
Section: 1.4
165) How many significant figures are there in the number 1.050 × 109? ________
Diff: 1
Section: 2.3
166) How many significant figures are there in the number 0.070120? ________
Diff: 2
Section: 1.5
167) Express the result of the operation, 8.520 + 2.7 - 1.03, to the proper number of significant figures. ________
Diff: 2
Section: 1.5
168) Express the result of the operation, (8.317 s 2.7 × 3.159)/4.19, to the proper number of significant figures. ________
Diff: 2
Section: 1.5
169) Express the result of the operation, 95.17 + 5.311 + 0.01275, to the proper number of significant figures. ________
Diff: 2
Section: 1.5
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? ________
Diff: 2
Section: 1.5
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? ________
Diff: 2
Section: 2.4
172) A spot on a microchip which is 7500 nm in diameter is ________ pm in diameter.
Diff: 2
Section: 1.6
173) An object weighing 450 kg, expressed in megagrams (Mg), is ________ Mg.
Diff: 2
Section: 1.6
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 be the mass, in kg, of a person weighing 14.9 stone? (1 kg = 2.20 lbs)
Diff: 2
Section: 1.6
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?
Diff: 2
Section: 1.6
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?
Diff: 1
Section: 1.7
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?
Diff: 1
Section: 1.7
178) A metal ball has a radius of 1.42 inches, and a density of 3.94 g/cm3. What is the mass of the ball, in grams? 2.54 cm = 1 inch
Hint: You need to calculate the volume of the ball to answer this question.
Diff: 3
Section: 1.7
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? ________
Hint: You need to calculate the volume of the box to answer this question.
Diff: 3
Section: 1.7
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
Diff: 2
Section: 1.7
181) The following equation, Pressure = Constant/Volume, is an example of a theory.
Diff: 2
Section: 1.1
182) Theoretical models are used to help in explaining laws.
Diff: 2
Section: 1.1
183) The observations made during an experiment are known as conclusions.
Diff: 2
Section: 1.1
184) A sample of a pure compound contains two or more phases.
Diff: 2
Section: 1.1
185) Mass indicates how much matter is in a given object.
Diff: 1
Section: 1.2
186) A compound is an example of a mixture which can have variable composition.
Diff: 1
Section: 1.2
187) A homogeneous mixture consists of only one chemical substance.
Diff: 1
Section: 1.2
188) A mixture always contains more than one chemical substance.
Diff: 1
Section: 1.2
189) There are 90 elements on the periodic table.
Diff: 1
Section: 1.2
190) The mass of a water molecule is the same on the moon as it is on the earth.
Diff: 1
Section: 1.2
191) A heterogeneous mixture can exist as only a single phase.
Diff: 2
Section: 1.2
192) A homogeneous mixture can exist as only a single phase.
Diff: 2
Section: 1.2
193) The evaporation of rubbing alcohol is a chemical change.
Diff: 2
Section: 1.2
194) The combustion of gasoline into carbon dioxide gas and water vapor is both a chemical and physical change.
Diff: 2
Section: 1.2
195) Density is one of the extensive properties of matter.
Diff: 2
Section: 1.2
196) The volume of a sample is an extensive property of matter.
Diff: 2
Section: 1.3
197) The density of water is a physical property of water.
Diff: 2
Section: 1.3
198) The combustibility of octane is a physical property of octane.
Diff: 2
Section: 1.3
199) A liter of carbon tetrachloride is smaller than a quart of the same substance.
Diff: 2
Section: 1.3
200) An increase of one Kelvin in temperature, is a smaller change than an increase of one degree Fahrenheit.
Diff: 2
Section: 1.4
201) The measurement, 7.05 × 10-12 m, is the same measurement as 7.05 pm.
Diff: 2
Section: 1.4
202) A large crowd attending a celebration in a metropolitan area was described in the morning newspaper the next day as about 450,000 people. 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 chemistry student is correct in how to represent the crowd size using scientific notation.
Diff: 2
Section: 1.4
203) Any number known accurately to six or more significant figures is defined as an exact number.
Diff: 2
Section: 1.5
204) In determining the number of significant digits in the result of a calculation, exact numbers are considered as having a value represented by zeros as significant figures.
Diff: 1
Section: 1.5
205) Ambiguity in the number of significant figures in a number being expressed can be eliminated by proper use of scientific notation.
Diff: 1
Section: 1.5
206) The result of the operation 8.52010 × 7.90, should be expressed as 67.3088.
Diff: 2
Section: 1.5
207) A 15 km run is a shorter run than a 10 mile run.
Diff: 2
Section: 1.5
208) A 5.00 pound bag of sugar weighs more than a 2.50 kg bag of sugar.
Diff: 2
Section: 1.6
209) A piece of carpet which measures 44.0 square yards is smaller than a piece of carpet which measures 44.0 square meters.
Diff: 2
Section: 1.6
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.
Diff: 2
Section: 1.6
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.
Diff: 2
Section: 1.7
212) The density of a metal reported as 1.74 g/cm3 also has a density of 1.74 kg/m3.
Diff: 2
Section: 1.7
213) The density of liquid water is inversely correlated to its temperature.
Hint: Think about what an inverse relationship looks like on a graph.
Diff: 3
Section: 1.7
214) A quick way to determine the sugar content of grapes is to determine the density of the grape juice using a hydrometer.
Diff: 2
Section: Chemistry Outside the Classroom 1.1
215) A sample of wine from grape juice can be distilled to obtain a mixture of alcohol and water.
Diff: 2
Section: Chemistry Outside the Classroom 1.1
216) One way to determine the alcohol content of wine is to determine the specific gravity of the wine using a hydrometer.
Diff: 2
Section: Chemistry Outside the Classroom 1.1
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 °Z
2) the boiling point of sulfur which is 444.60 °C = 717.75 K = 250.00 °Z
3) 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.
Hint: First, consider whether or not the temperature scales have the same magnitude increments; then you can determine the value of absolute zero.
Diff: 3
Section: Chemistry Outside the Classroom 1.1
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 °V
2) the boiling point of benzene which is 80.10 °C = 100.00 °V
3) 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.
Hint: First, consider whether or not the temperature scales have the same magnitude increments; then you can determine the value of absolute zero.
Diff: 3
Section: 1.4
219) A number resulting from a measurement was properly expressed in scientific notation as 
. The number could also be correctly written as
A) 0.0021 m
B) 0.002100 m
C) 0.00021 m
D) 2.1000 m
E) 21000 m
Diff: 1
Section: 1.4
220) Solve the following, with the correct number of significant figures:
(628.83 - 627.71) × 124 + 122.08
Diff: 2
Section: 1.5
221) Solve the following: (2.15 × 106 + 3.2 × 102)/(2.332 + 22.0005 + 0.9861)
A) 1.45 × 103
B) 48.8
C) 233.1
D) 106
E) 8.5 × 104
Diff: 2
Section: 1.5
222) If 1 meter = 39.37 inch and 1 foot = 12.00 inch, calculate the relationship to four significant figures that will convert cubic feet into cubic meters directly. 1 ft3 = ________ m3
Hint: Recall the correct order of operations and how to determine the significant figures for each kind of step.
Diff: 3
Section: 1.5
223) A home aquarium measures 17.0 inches wide, 17.0 inches long and 8.50 inches high. What is the volume in liters? (1 in = 2.54 cm and 1 cm3 = 1 ml)
Diff: 3
Section: 1.6
224) Express 109 miles per hour in meters per second. ( 1 mile = 1609.34 meters)
Hint: Remember that when converting derived units, you must convert each of the component fundamental units individually.
Diff: 3
Section: 1.6
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 g
Mass of weighing cup + metal sample = 72.943 g
Volume 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?
Hint: Remember to remove the mass of the weighing cup from the sample before performing any calculations.
A) 2.2 g cm-3
B) 3.8 g cm-3
C) 4.8 g cm-3
D) 19 g cm-3
Diff: 3
Section: 1.6
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? 1 pound = 0.4536 kg.
volume = (πr3)
Hint: Read the problem carefully. Follow the units and remember that the diameter is twice the radius.
Diff: 3
Section: 1.7
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 = (πr3)
Hint: Read the problem carefully. Follow the units and remember that the diameter is twice the radius.
Diff: 3
Section: 1.7
228) Some students in the AP chemistry class have come up with an idea they would like to have tested, which involves collaboration with several defense 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.
volume = (πr3)
Hint: Read the problem carefully. Follow the units and remember that the diameter is twice the radius.
Diff: 3
Section: 1.7
229) Iron has a density of 7.86 g/cm3. As part of their exam, students in the junior class at a school were to mass 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 = (πr3)
Hint: Read the problem carefully. Follow the units and remember that the diameter is twice the radius. Use the difference in mass to find the missing volumes.
Diff: 3
Section: 1.7
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?
Hint: Consider your units and make sure to determine volume before and after phase change. Remember, the mass doesn't change.
Diff: 3
Section: 1.766
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