Chapter 3
The Metric
System
Vanessa N. Prasad-Permaul
CHM 1025
Valencia Community College
1
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.
2
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.
3
Metric System Basic Units
4
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.
5
Metric System Prefixes
The following table lists the common prefixes used
in the metric system:
6
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.
7
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
EXERCISE 3.1 Metric Basic Units and Prefixes
Practice Exercise
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
Concept Exercise
What is the basic unit of length, mass, and volume in
the metric system?
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 g.
 Deciliter is abbreviated dL.
 Gigasecond is abbreviated Gs.
10
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.
11
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.
12
Metric Unit Factors
 Since 1000 m = 1 km, we can write the
following unit factors for converting between
meters and kilometers:
1 km
or
1000 m
1000 m
1 km
 Since 1000 mm = 1 m, we can write the
following unit factors:
1000 mm
1m
or
1m
1000 mm
13
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
Solution
We can refer to Table 3.2 as necessary.
(a) The prefix mega- means 1,000,000 basic units; thus, 1 Mm = 1,000,000 m.
1 Mm = 1  106 m
(b) The prefix kilo- means 1000 basic units; thus, 1 kg = 1000 g.
1 kg = 1  103 g
(c) The prefix deci- means 0.1 of a basic unit, thus, 1 L = 10 dL.
1 L = 1  101 dL
(d) The prefix nano- means 0.000 000 001 of a basic unit, thus; 1 s =
1,000,000,000 ns.
1 s = 1  109 ns
EXERCISE 3.2 Metric Unit Equations
Practice Exercise
Complete the unit equation for each of the following
exact metric equivalents:
(a) 1 nm = ? m
(c) 1 L = ? L
(b) 1 g = ? mg
(d) 1 s = ? Ms
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
Solution
We start by writing the unit equation to generate the
two unit factors.
(a) 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
EXERCISE 3.3 Metric Unit Factors
Practice Exercise
Write two unit factors for each of the following metric
relationships:
(a) liters and microliters (b)milliseconds and seconds
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:
1. Write down the unit asked for in the answer.
2. Write down the given value related to the
answer.
3. Apply unit factor(s) to convert the given unit
to the units desired in the answer.
18
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.
1g
325 mg x
= 0.325 g
1000 mg
19
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 1000 mL
10 dL
1L
20
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.
1 L x 1000 mL
125 dL x
= 12,500 mL
10 dL
1L
21
EXERCISE 3.4 Metric-Metric Conversions
Practice Exercise
A dermatology patient is treated with ultraviolet light
having a wavelength of 305 nm. What is the
wavelength expressed in meters? In micrometers?
Concept Exercise
Express the volume of a cube 1 cm on a side in
milliliters.
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
1000 g
1 Mg
x
kg ×
= 5.98 x 1019 Mg
1 kg
1000000 g
23
EXERCISE 3.5 Metric–Metric Conversion
Practice Exercise
Light travels through the universe at a velocity of
3.00  1010 cm/s. How many megameters does light
travel in one second?
Concept Exercise
How many significant digits are in the following unit
factor?
1 g/1000 mg
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.
25
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 = 0.914 m).
0.914 m
120 yd x
= 110 m
1 yd
26
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.
1 qt x 946 mL
64.0 fl oz x
= 1,890 mL
32 fl oz
1 qt
27
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
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.
,
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
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?
Concept Exercise
How many significant digits are in the following unit
factor?
1 kg/2.20 lb
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.
1. First, miles → meters
2. Next, hours → seconds
32
Compound Unit Problem
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.
75 km x 1000 m x 1 hr
= 21 m/s
1 km
hr
3600 s
33
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
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.
EXERCISE 3.8 Conversion of a Unit Ratio
Practice Exercise
If a runner completes a 10K race in 32.50 minutes
(min), what is the 10.0 km pace in miles per hour
(given that 1 mi = 1.61 km)?
Concept Exercise
Which speed is faster: 65 mi/h or 65 km/h?
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).
37
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?
Solution
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.
EXERCISE 3.9 Volume Calculation for a Rectangular
Solid
Practice Exercise
If a rectangular brass solid measures 52.0 mm by
25.0 mm by 15.0 mm, what is the volume in cubic
millimeters?
Concept Exercise
Express the volume of a cube 10 cm on a side in liters.
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?
Solution
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.
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 0.001 m
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.
42
Cubic and Liquid Volume
Units
 1 liter is equal to 1000 cubic centimeters.
 10 cm x 10 cm x 10 cm = 1000 cm3
 1000 cm3 = 1 L = 1000 mL.
 Therefore, 1 cm3 = 1 mL.
43
EXAMPLE 3.11 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.
498
cm3
1 in x 1 in x 1 in
x
= 30.4 in3
2.54 cm 2.54 cm 2.54 cm
44
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.
Concept Exercise
Which of the following is the greater volume?
500 mL or 500 cm3
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.
46
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.
47
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.
48
EXAMPLE 3.12: Volume by Displacement
A quartz stone weighing 30.475 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?
Solution
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
EXERCISE 3.12: Volume by Displacement
Practice Exercise
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 105.5 mL, what is the volume of oxygen gas?
Concept Exercise
Which of the following has the greater volume?
1 mL or 1 cm3
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.
mass
= density
volume
51
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.
52
Densities of Common Substances
53
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.
54
EXAMPLE EXERCISE 3.13 Density Calculation
Calculating Density
What is the density of a platinum nugget that
has a mass of 224.50 g and a volume of 10.0
cm3 ? Recall, density is mass/volume.
224.50 g
10.0 cm3
= 22.5 g/cm3
55
EXERCISE 3.13: Density Calculation
Practice Exercise
Carbon tetrachloride is a solvent used for degreasing
electronic parts. If 40.0 mL of carbon tetrachloride
has a mass of 39.75 g, what is the density of the
liquid?
Concept Exercise
Which of the following has the greater density: ice or
water?
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
1.84 g
= 2350 g
mL
57
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.)
Concept Exercise
Which of the following is the greater density?
1 g/mL or 1 kg/L
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
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.
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
1312.5 g. What is the density of silver?
Concept Exercise
If some humans float in water and other sink, what is
the approximate density of the human body?
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)?
3.784 L x 730. g
At 0 ºC: 1.00 gal x
= 2760 g
L
1 gal
3.784 L x 713 g
At 25 ºC: 1.00 gal x
= 2700 g
L
1 gal
 The difference is about 60 grams (about 2 %).
62
Temperature

Temperature is a measure of the average
kinetic energy of the individual particles in a
sample.

There are three temperature scales:
1. Celsius
2. Fahrenheit
3. Kelvin

Kelvin is the absolute temperature scale.
63
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.
64
Temperature Scales
65
Temperature Conversions
 This is the equation for converting °C to °F.
°C x
(
180°F
100°C
) = °F
 This is the equation for converting °F to °C.
(°F - 32°F) x
(
100°C
180°F
) = °C
 To convert from °C to K, add 273.
°C + 273 = K or K – 273 = oC
66
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?
(98.6°F - 32°F) x
(
100°C
180°F
)
= 37.0°C
K = °C + 273 = 37.0 °C + 273 = 310 K
67
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
Concept Exercise
What is the relationship between the Celsius and
centigrade temperature scales?
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 + 273 = 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.
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?
Concept Exercise
Which of the following temperatures does not exist?
–100 °F, –100 °C, –100 K
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).
71
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.
72
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
= 4.184 kJ).
Unit Analysis Map
EXAMPLE 3.18 Energy Conversion
Solution
We apply the unit factor 4.184 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.
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 = 4.184 kJ).
Concept Exercise
If an aerosol can feels cold after releasing the spray, is
heat flowing from the can or from your hand?
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.
76
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
EXAMPLE 3.19 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.
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?
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.
80
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.
81
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.
82
Give the symbol for microliter.
a.
b.
c.
d.
mL
miL
ML
μL
Give the symbol for microliter.
a.
b.
c.
d.
mL
miL
ML
μL
2.00 microliters = ? liters
a.
b.
c.
d.
2.00 × 10–9 L
2.00 × 10–6 L
2.00 × 10–3 L
2.00 × 103 L
2.00 microliters = ? liters
a.
b.
c.
d.
2.00 × 10–9 L
2.00 × 10–6 L
2.00 × 10–3 L
2.00 × 103 L
Given that 1 yd = 0.914 m and 1 mi
= 1760 yd, which Olympic track
event covers a distance that is
closest to a half mile?
a.
b.
c.
d.
200 m
400 m
800 m
1000 m
Given that 1 yd = 0.914 m and 1 mi
= 1760 yd, which Olympic track
event covers a distance that is
closest to a half mile?
a.
b.
c.
d.
200 m
400 m
800 m
1000 m
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 0.500 cubic centimeters in
cubic inches?
a.
b.
c.
d.
0.0122 cubic inches
0.0305 cubic inches
0.0775 cubic inches
0.197 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 0.500 cubic centimeters in
cubic inches?
a.
b.
c.
d.
0.0122 cubic inches
0.0305 cubic inches
0.0775 cubic inches
0.197 cubic inches
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?
a.
b.
c.
d.
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
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?
a.
b.
c.
d.
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