1. Vanessa N. Prasad-Permaul Valencia Community College
Chapter 3
The Metric System
Vanessa N. Prasad-Permaul
CHM 1025
Valencia Community College

2. The Metric System
The English system was used primarily in the British Empire and wasn’t very standardized.
The French organized a committee to devise a universal measuring system.
After about 10 years, the committee designed and agreed on the metric system.
The metric system offers simplicity with a single base unit for each measurement.

3. Original Metric Unit Definitions
A meter was defined as 1/10,000,000 of the distance from the North Pole to the equator.
A kilogram (1000 grams) was equal to the mass of a cube of water measuring 0.1 m on each side.
A liter was set equal to the volume of one kilogram of water at 4 C.

4. Metric System Basic Units

5. Metric System Advantage
Another advantage of the metric system is that it is a decimal system.
It uses prefixes to enlarge or reduce the basic units.
For example:
A kilometer is 1000 meters.
A millimeter is 1/1000 of a meter.

6. Metric System Prefixes
The following table lists the common prefixes used in the metric system:

7. Metric Prefixes, Continued
For example, the prefix kilo- increases a base unit by 1000:
1 kilogram is 1000 grams.
The prefix milli- decreases a base unit by a factor of 1000:
There are 1000 millimeters in 1 meter.

8. EXAMPLE 3.1 Metric Basic Units and Prefixes
Give the symbol for each of the following metric units and state the quantity measured by each unit:
(a) gigameter (b) kilogram
(c) centiliter (d) microsecond
Solution
We compose the symbol for each unit by combining the prefix symbol and the basic unit symbol. If we refer to Tables 3.1 and 3.2, we have the following:
(a) Gm, length (b) kg, mass (c) cL, volume
(d) s, time

9. EXERCISE 3.1 Metric Basic Units and Prefixes
Give the symbol for each of the following metric units and state the quantity measured by each unit:
(a) nanosecond (b) microiliter
(c) kilogram (d) millimeter
Practice Exercise
What is the basic unit of length, mass, and volume in the metric system?
Concept Exercise

10. Metric Symbols
The names of metric units are abbreviated using symbols. Use the prefix symbol followed by the symbol for the base unit, so:
Nanometer is abbreviated nm.
Microgram is abbreviated mg.
Deciliter is abbreviated dL.
Gigasecond is abbreviated Gs.

11. Nanotechnology
Nanotechnology refers to devices and processes on the 1–100 nm scale.
For reference, a human hair is about 100,000 nm thick!
A DNA helix is a nanoscale substance, with a diameter of about 1 nm.
Nanoscale hollow tubes, called carbon nanotubes, have slippery inner surfaces that allow for the easy flow of fluids.

12. Metric Equivalents
We can write unit equations for the conversion between different metric units.
The prefix kilo- means 1000 basic units, so 1 kilometer is 1000 meters.
The unit equation is 1 km = 1000 m.
Similarly, a millimeter is 1/1000 of a meter, so the unit equation is 1000 mm = 1 m.

13. Metric Unit Factors
Since 1000 m = 1 km, we can write the following unit factors for converting between meters and kilometers:
1 km or m
1000 m km
Since 1000 mm = 1 m, we can write the following unit factors:
1000 mm or m
1 m mm

14. EXAMPLE 3.2 Metric Unit Equations
Complete the unit equation for each of the following exact metric equivalents:
(a) 1 Mm = ? m (b) 1 kg = ? g
(c) 1 L = ? dL (d) 1 s = ? ns
We can refer to Table 3.2 as necessary.
The prefix mega- means 1,000,000 basic units; thus, 1 Mm = 1,000,000 m.
1 Mm = 1  106 m
The prefix kilo- means 1000 basic units; thus, 1 kg = 1000 g.
1 kg = 1  103 g
The prefix deci- means 0.1 of a basic unit, thus, 1 L = 10 dL.
1 L = 1  101 dL
The prefix nano- means of a basic unit, thus; 1 s = 1,000,000,000 ns.
1 s = 1  109 ns
Solution

15. EXERCISE 3.2 Metric Unit Equations
Complete the unit equation for each of the following
exact metric equivalents:
(a) 1 nm = ? m (b) 1 g = ? mg
(c) 1 L = ? L (d) 1 s = ? Ms
Practice Exercise

16. EXAMPLE 3.3 Metric Unit Factors
Write two unit factors for each of the following metric relationships:
(a) kilometers and meters (b)grams and decigrams
We start by writing the unit equation to generate the
two unit factors.
The prefix kilo- means 1000 basic units; thus, 1 km = 1000 m. The two unit factors are
(b) The prefix deci- means 0.1 basic unit; thus, 1 g = 10 dg. The two unit factors are
Solution

17. EXERCISE 3.3 Metric Unit Factors
Write two unit factors for each of the following metric relationships:
(a) liters and microliters (b)milliseconds and seconds
Practice Exercise

18. Metric–Metric Conversions
We will use the unit analysis method we learned in Chapter 2 to do metric–metric conversion problems.
Remember, there are three steps:
Write down the unit asked for in the answer.
Write down the given value related to the answer.
Apply unit factor(s) to convert the given unit to the units desired in the answer.

19. Metric–Metric Conversion Problem
What is the mass in grams of a 325 mg aspirin tablet?
Step 1: We want grams.
Step 2: We write down the given: 325 mg.
Step 3: We apply a unit factor (1000 mg = 1 g) and round to three significant figures.
325 mg x
= g
1000 mg
1 g

20. Two Metric–Metric Conversions
EXAMPLE 3.4 Metric Unit Factors
Two Metric–Metric Conversions
A hospital has 125 deciliters of blood plasma. What is the volume in milliliters?
Step 1: We want the answer in mL.
Step 2: We have 125 dL.
Step 3: We need to first convert dL to L and then convert L to mL:
1 L and mL
10 dL L

21. EXAMPLE 3.4 Metric Unit Factors
Continued…
Apply both unit factors, and round the answer to three significant digits.
Notice that both dL and L units cancel, leaving us with units of mL.
125 dL x
= 12,500 mL x
10 dL
1 L
1000 mL

22. EXERCISE 3.4 Metric-Metric Conversions
A dermatology patient is treated with ultraviolet light having a wavelength of 305 nm. What is the wavelength expressed in meters? In micrometers?
Practice Exercise
Express the volume of a cube 1 cm on a side in
milliliters.
Concept Exercise

23. EXAMPLE EXERCISE 3.5 Metric–Metric Conversion
Another Example
The mass of the Earth’s moon is 7.35 × 1022 kg. What is the mass expressed in megagrams, Mg?
We want Mg; we have 7.35 x 1022 kg.
Convert kilograms to grams, and then grams to megagrams.
7.35 x 1022 kg ×
= 5.98 x 1019 Mg x
1 kg
1000 g
1 Mg g

24. EXERCISE 3.5 Metric–Metric Conversion
Light travels through the universe at a velocity of 3.00  1010 cm/s. How many megameters does light travel in one second?
Practice Exercise
How many significant digits are in the following unit
factor?
1 g/1000 mg
Concept Exercise

25. Metric and English Units
The English system is still very common in the United States.
We often have to convert between English and metric units.

26. Metric–English Conversion
The length of an American football field, including
the end zones, is 120 yards. What is the length in
meters?
Convert 120 yd to meters
(given that 1 yd = m).
120 yd x
= 110 m
1 yd
0.914 m

27. English–Metric Conversion
EXAMPLE EXERCISE 3.6 Metric–English Conversion
English–Metric Conversion
A half-gallon carton contains 64.0 fl oz of milk.
How many milliliters of milk are in a carton?
We want mL; we have 64.0 fl oz.
Use 1 qt = 32.0 fl oz, and 1 qt = 946 mL.
64.0 fl oz x
= 1,890 mL x
32 fl oz
1 qt
946 mL

28. EXERCISE 3.6 Metric–English Conversion
Practice Exercise
A plastic bottle contains 4.00 gallons of distilled water. How many liters of distilled water are in the bottle (given that 1 gal = 4 qt)?
Concept Exercise
How many significant digits are in the following unit
factor?
1 qt/946 mL

29. EXAMPLE 3.7 Metric–English Conversion
We apply the unit factor 1 lb/16 oz to cancel ounces , and 454 g/1 lb to cancel pounds
The given value, 2.0 oz, limits the answer to two significant digits. Unit factor 1 has no effect as it is derived from an exact equivalent, and unit factor 2 has three significant digits.

30. EXAMPLE 3.7 Metric–English Conversion
If a tennis ball weighs 2.0 oz, what is the mass of the tennis ball in grams?
Unit Analysis Map

31. EXERCISE 3.7 Metric–English Conversion
Practice Exercise
If a tennis ball has a diameter of 2.5 inches, what is the diameter in millimeters?
How many significant digits are in the following unit
factor?
1 kg/2.20 lb
Concept Exercise

32. Compound Units Some measurements have a ratio of units.
For example, the speed limit on many highways is 55 miles per hour. How would you convert this to meters per second?
Convert one unit at a time using unit factors.
First, miles → meters
Next, hours → seconds

33. Compound Unit Problem = 21 m/s 1 km 1000 m 1 hr 3600 s 75 km hr
A motorcycle is traveling at 75 km/hour. What is
the speed in meters per second?
We have km/h; we want m/s.
Use 1 km = 1000 m and 1 h = 3600 s.
= 21 m/s x
1 km
1000 m
1 hr
3600 s
75 km hr

34. EXAMPLE 3.8 Conversion of a Unit Ratio
If a Mazda Miata is traveling at 95 km/h, what is the speed in meters per second (given that 1 km = 1000 m, and 1 h = 3600 s)?
Unit Analysis Map

35. EXAMPLE 3.8 Conversion of a Unit Ratio
Solution
We apply the unit factor 1000 m/1 km to cancel kilometers , and 1 h/3600 s to cancel hours
The given value has two significant digits, so the answer is limited to two digits. Since each unit factor is derived from an exact equivalent, neither affects the number of significant digits in the answer.

36. EXERCISE 3.8 Conversion of a Unit Ratio
If a runner completes a 10K race in minutes (min), what is the 10.0 km pace in miles per hour (given that 1 mi = 1.61 km)?
Practice Exercise
Which speed is faster: 65 mi/h or 65 km/h?
Concept Exercise

37. Volume by Calculation
The volume of an object is calculated by multiplying the length (l) by the width (w) by the thickness (t).
volume = l x w x t
All three measurements must be in the same units.
If an object measures 3 cm by 2 cm by 1 cm, the volume is 6 cm3 (cm3 is cubic centimeters).

38. EXAMPLE 3.9 Volume Calculation for a Rectangular Solid
If a stainless steel rectangular solid measures 5.55 cm long, 3.75 cm wide, and 2.25 cm thick, what is the volume in cubic centimeters?
We can calculate the volume of the rectangular solid by multiplying length times width times thickness: l  w  t.
5.55 cm  3.75 cm  2.25 cm = 46.8 cm3
The answer is rounded off to three significant digits because each given value has three significant digits.
Solution

39. EXERCISE 3.9 Volume Calculation for a Rectangular Solid
If a rectangular brass solid measures 52.0 mm by 25.0 mm by 15.0 mm, what is the volume in cubic millimeters?
Practice Exercise
Express the volume of a cube 10 cm on a side in liters.
Concept Exercise

40. EXAMPLE 3.10: Thickness Calculation for a Rectangular Solid
A sheet of aluminum foil measures 25.0 mm by 10.0 mm, and the volume is 3.75 mm3. What is the thickness of the foil in millimeters?
We can calculate the thickness of the foil by dividing the volume by length and width. Since the unit of volume is mm3, we obtain the thickness in mm by unit cancellation.
The answer is rounded off to three significant digits because each given value has three significant digits.
Solution

41. EXERCISE 3.10: Thickness Calculation for a Rectangular Solid
Practice Exercise
A sheet of aluminum foil measures 35.0 cm by 25.0 cm, and the volume is 1.36 cm3. What is the thickness of the foil in centimeters?
Aluminum foil :A thin sheet of aluminum foil.
Concept Exercise
Which of the following is the greatest thickness?
1 mm, 0.1 cm, or m

42. Cubic Volume and Liquid Volume
The liter (L) is the basic unit of volume in the metric system.
One liter is defined as the volume occupied by a cube that is 10 cm on each side.

43. Cubic and Liquid Volume Units
1 liter is equal to 1000 cubic centimeters.
10 cm x 10 cm x 10 cm = cm3
1000 cm3 = 1 L = 1000 mL.
Therefore, 1 cm3 = 1 mL.

44. Cubic–Liquid Volume Conversion
EXAMPLE Metric–English Volume Conversion
Cubic–Liquid Volume Conversion
An automobile engine displaces a volume of
498 cm3 in each cylinder. What is the displacement of a cylinder in cubic inches, in3?
We want in3; we have 498 cm3.
Use 1 in = 2.54 cm three times.
= 30.4 in3 x
1 in
2.54 cm
498 cm3 x

45. EXERCISE 3.11: Metric–English Volume Conversion
Practice Exercise
Given that an SUV has a 304 in.3 engine, express the engine volume in liters.
Which of the following is the greater volume?
500 mL or 500 cm3
Concept Exercise

46. Volume by Displacement
If a solid has an irregular shape, its volume cannot be determined by measuring its dimensions.
You can determine its volume indirectly by measuring the amount of water it displaces.
This technique is called volume by displacement.
Volume by displacement can also be used to determine the volume of a gas.

47. Solid Volume by Displacement
You want to measure the volume of an irregularly
shaped piece of jade.
Partially fill a volumetric flask with water and measure the volume of the water.
Add the jade, and measure the difference in volume.
The volume of the jade is 10.5 mL.

48. Gas Volume by Displacement
You want to measure the volume of gas given off
in a chemical reaction.
The gas produced displaces the water in the flask into the beaker. The volume of water displaced is equal to the volume of gas.

49. EXAMPLE 3.12: Volume by Displacement
A quartz stone weighing g is dropped into a graduated cylinder. If the water level increases from 25.0 mL to 36.5 mL, what is the volume of the quartz stone?
We can calculate the displaced volume in milliliters by subtracting the initial volume from the final volume.
36.5 mL – 25.0 mL = 11.5 mL
Solution

50. EXERCISE 3.12: Volume by Displacement
Hydrogen peroxide decomposes to give oxygen gas, which displaces a volume of water into a beaker. If the water level in the beaker increases from 50.0 mL to mL, what is the volume of oxygen gas?
Practice Exercise
Which of the following has the greater volume?
1 mL or 1 cm3
Concept Exercise

51. The Density Concept
The density of an object is a measure of its concentration of mass.
Density is defined as the mass of an object divided by the volume of the object.
= density
volume
mass

52. Density
Density is expressed in different units. It is usually grams per milliliter (g/mL) for liquids, grams per cubic centimeter (g/cm3) for solids, and grams per liter (g/L) for gases.

53. Densities of Common Substances

54. Estimating Density
We can estimate the density of a substance by comparing it to another object.
A solid object will float on top of a liquid with a higher density.
Object S1 has a density less than that of water, but larger than that of L1.
Object S2 has a density less than that of L2, but larger than that of water.

55. EXAMPLE EXERCISE 3.13 Density Calculation
Calculating Density
What is the density of a platinum nugget that has a mass of g and a volume of 10.0 cm3 ? Recall, density is mass/volume.
= g/cm3
10.0 cm3 g

56. EXERCISE 3.13: Density Calculation
Carbon tetrachloride is a solvent used for degreasing electronic parts. If 40.0 mL of carbon tetrachloride has a mass of g, what is the density of the liquid?
Practice Exercise
Which of the following has the greater density: ice or water?
Concept Exercise

57. Density as a Unit Factor
EXAMPLE EXERCISE 3.14 Density as a Unit Factor
Density as a Unit Factor
We can use density as a unit factor for conversions between mass and volume.
An automobile battery contains 1275 mL of acid. If the density of battery acid is 1.84 g/mL, how many grams of acid are in an automobile battery?
– We have 1275 mL; we want grams:
1275 mL x
= g mL
1.84 g

58. EXERCISE 3.14: Density as a Unit Factor
Practice Exercise
The most abundant gases in our atmosphere are nitrogen, oxygen, and argon. What is the volume of 1.00 kg of air? (Assume the density of air is 1.29 g/L.)
Which of the following is the greater density?
1 g/mL or 1 kg/L
Concept Exercise

59. EXAMPLE 3.15: Density as a Unit Factor
A 1.00-in. cube of copper measures 2.54 cm on a side. What is the mass of the copper cube (given that d of copper = 8.96 g/cm3)?
Unit Analysis Map

60. EXAMPLE 3.15:Density as a Unit Factor
Solution
First, we find the volume of the copper cube. We obtain the volume of the cube, 16.4 cm3, by multiplying (2.54 cm) (2.54 cm) (2.54 cm). We use the given density, 8.96 g/1 cm3, as a unit factor to cancel cubic centimeters , which appears in the
denominator.
The given value and unit factor each has three
significant digits, so the answer is rounded off
to three significant digits.
Copper Metal A 1.00-inch cube of copper metal.

61. EXERCISE 3.15: Density as a Unit Factor
Practice Exercise
A cube of silver is 8.00 cm on a side and has a mass of g. What is the density of silver?
If some humans float in water and other sink, what is
the approximate density of the human body?
Concept Exercise

62. Critical Thinking: Gasoline
The density of gasoline is 730. g/L at 0 ºC (32 ºF) and 713 g/L at 25 ºC (77 ºF). What is the mass difference of 1.00 gallon of gasoline at these two temperatures (1 gal = 3.784L)?
The difference is about 60 grams (about 2 %).
2.76 x 103g
= 2760 g x
At 0 ºC: gal x
730. g L
3.784 L
1 gal
2.70 x 103g
= 2700 g x
At 25 ºC: 1.00 gal x
713 g L
3.784 L
1 gal

63. Temperature
Temperature is a measure of the average kinetic energy of the individual particles in a sample.
There are three temperature scales:
Celsius
Fahrenheit
Kelvin
Kelvin is the absolute temperature scale.

64. Temperature Scales On the Fahrenheit scale, water freezes at 32 °F
and boils at 212 °F.
On the Celsius scale, water freezes at 0 °C and
boils at 100 °C. These are the reference points
for the Celsius scale.
Water freezes at 273 K and boils at 373 K on the Kelvin scale.

65. Temperature Scales

66. Temperature Conversions
This is the equation for converting °C to °F.
This is the equation for converting °F to °C.
To convert from °C to K, add 273.
°C = K or K – 273 = oC
= °F
°C x
100°C
180°F
( )
( )
180°F
100°C
= °C
(°F - 32°F) x

67. Fahrenheit–Celsius Conversions
EXAMPLE 3.16 °F and °C Temperature Conversions
Fahrenheit–Celsius Conversions
Body temperature is 98.6 °F. What is body temperature in degrees Celsius? In Kelvin?
K = °C = °C = 310 K
( )
180°F
100°C
= 37.0°C
(98.6°F - 32°F) x

68. EXAMPLE 3.16: °F and °C Temperature Conversions
Practice Exercise
The average surface temperature of Mars is –55 °C. What is the average temperature in degrees Fahrenheit?
Australian Stamp The cartoon illustrates that
38 °C is approximately equal to 100 °F
What is the relationship between the Celsius and
centigrade temperature scales?
Concept Exercise

69. EXAMPLE 3.17: °C and K Temperature Conversions
Dermatologists use liquid nitrogen to freeze skin tissue. If the Celsius temperature of liquid nitrogen is –196 °C, what is the Kelvin temperature?
Solution
Given the Celsius temperature, we add 273 units to find the corresponding Kelvin
temperature.
–1.96 ° C = 77 k
Liquid Nitrogen Although nitrogen is normally a gas, it liquefies at –196 °C. When liquid nitrogen is poured from a Thermos, it is cold enough to freeze the moisture in air and form a white mist.

70. EXERCISE 3.17: °C and K Temperature Conversions
Practice Exercise
The secret to “fire-walking” is to first walk barefoot through damp grass and then step lively on the red-hot coals. If the bed of coals is 1475 K, what is the Celsius temperature?
Which of the following temperatures does not exist?
–100 °F, –100 °C, –100 K
Concept Exercise

71. Heat
Heat is the flow of energy from an object of higher temperature to an object of lower temperature.
Heat measures the total energy of a system.
Temperature measures the average energy of particles in a system.
Heat is often expressed in terms of joules (J) or calories (cal).

72. Heat Versus Temperature
Although both beakers below have the same temperature (100 ºC), the beaker on the right has twice the amount of heat because it has twice the amount of water.

73. EXAMPLE 3.18 Energy Conversion
Burning one liter of natural gas produces 9.46 kcal of heat energy. Express the energy in kilojoules (given that 1 kcal = kJ).
Unit Analysis Map

74. EXAMPLE 3.18 Energy Conversion
Solution
We apply the unit factor kJ /1 kcal to cancel kilocalories , which appears in the denominator.
The given value has three significant digits, and the unit factor has four digits. Thus, we round off the answer to three significant digits.
Bunsen Burner A laboratory burner that uses natural gas for fuel.

75. EXERCISE 3.18 Energy Conversion
Practice Exercise
Burning one gram of gasoline produces 51.3 kJ of energy. Express the heat energy in kilocalories (given that 1 kcal = kJ).
Concept Exercise
If an aerosol can feels cold after releasing the spray, is heat flowing from the can or from your hand?

76. Specific Heat
The specific heat of a substance is the amount of heat required to bring about a change in temperature.
It is expressed with units of calories per gram per degree Celsius.
The larger the specific heat, the more heat is required to raise the temperature of the substance.

77. 35.0 °C, what is the mass of water (specific heat = 1.00 cal/g × °C)?
EXAMPLE 3.19 Specific Heat
An energy-efficient home may have solar panels for heating water. If 350,000 cal heat water from 20.0 °C to
35.0 °C, what is the mass of water
(specific heat = 1.00 cal/g × °C)?
Unit Analysis Map

78. We apply the unit factor to cancel calories , and
EXAMPLE Specific Heat
Solution
We apply the unit factor to cancel calories , and
(35.0 – 20.0) °C to cancel degrees Celsius
Solar Panels on Rooftop Solar panels collect light energy from the Sun, which is converted to heat energy for the home.

79. EXERCISE 3.19 Specific Heat
Practice Exercise
A 725 g steel horseshoe is heated to 425 °C and dropped into a bucket of cold water. If the horseshoe cools to 20 °C and the specific heat of steel is 0.11 cal/g  °C, how much heat is released?
Concept Exercise
If the crust of an apple pie cooks faster than the filling, which has the higher specific heat: the crust or apple filling?

80. Chapter Summary
The basic units in the metric system are grams for mass, liters for volume, and meters for distance.
The base units are modified using prefixes to reduce or enlarge the base units by factors of ten.
We can use unit factors to convert between metric units.
We can convert between metric and English units using unit factors.

81. Chapter Summary, Continued
Volume is defined as length x width x thickness.
Volume can also be determined by displacement of water.
Density is mass divided by volume.

82. Chapter Summary, Continued
Temperature is a measure of the average energy of the particles in a sample.
Heat is a measure of the total energy of a substance.
Specific heat is a measure of how much heat is required to raise the temperature of a substance.

83. Give the symbol for microliter.mL
miL ML μL

84. Give the symbol for microliter.mL
miL ML μL

85. 2.00 microliters = ? liters
2.00 × 10–9 L
2.00 × 10–6 L
2.00 × 10–3 L
2.00 × 103 L

86. 2.00 microliters = ? liters
2.00 × 10–9 L
2.00 × 10–6 L
2.00 × 10–3 L
2.00 × 103 L

87. Given that 1 yd = m and 1 mi = 1760 yd, which Olympic track event covers a distance that is closest to a half mile?
200 m
400 m
800 m
1000 m

88. Given that 1 yd = m and 1 mi = 1760 yd, which Olympic track event covers a distance that is closest to a half mile?
200 m
400 m
800 m
1000 m

89. 0.0122 cubic inches 0.0305 cubic inches 0.0775 cubic inches
Flu vaccines are usually administered using a hypodermic needle. A typical dose is 0.500cc (0.500cubic centimeters). Given that 2.54 cm = 1 in, what is cubic centimeters in cubic inches?
cubic inches
cubic inches
cubic inches
0.197 cubic inches

90. 0.0122 cubic inches 0.0305 cubic inches 0.0775 cubic inches
Flu vaccines are usually administered using a hypodermic needle. A typical dose is 0.500cc (0.500 cubic centimeters). Given that 2.54 cm = 1 in, what is cubic centimeters in cubic inches?
cubic inches
cubic inches
cubic inches
0.197 cubic inches

91. When added to a graduated cylinder containing 4. 00 mL of water, 5
When added to a graduated cylinder containing 4.00 mL of water, 5.00 g of which metal will displace the greatest volume of water?
iron, d = 7.87 g/cm3
lead, d = 11.3 g/cm3
gold d = 19.3 g/cm3
5.00 g of any of these metals will displace the same volume of water

92. When added to a graduated cylinder containing 4. 00 mL of water, 5
When added to a graduated cylinder containing 4.00 mL of water, 5.00 g of which metal will displace the greatest volume of water?
iron, d = 7.87 g/cm3
lead, d = 11.3 g/cm3
gold d = 19.3 g/cm3
5.00 g of any of these metals will displace the same volume of water