, SOLUTION MANUAL FOR
Chemistry for Engineering Students 5th Edition Brown
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, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution and Answer Guide
LARRY BROWN & TOM HOLME, CHEMISTRY FOR ENGINEERING STUDENTS, 5E 2025,
9780357974803; CHAPTER 1: INTRODUCTION TO CHEMISTRY
TABLE OF CONTENTS
Critical Materials ...................................................................................................................1
The Study of Chemistry ....................................................................................................... 2
Observations, Models, and Systems ................................................................................... 4
Numbers and Measurements ............................................................................................... 6
Problem Solving in Chemistry and Engineering ................................................................ 11
Touchscreen Technology ....................................................................................................17
Conceptual Problems ..........................................................................................................18
Focus on Problem Solving Exercises ................................................................................ 20
CRITICAL MATERIALS
1.1 Are the elements designated as critical materials all rare? Explain your answer.
Solution:
While some critical materials may be rare, the classification considers factors beyond
just rarity: primarily an element’s importance and the risk associated with its supply.
1.2 In what country is most of the world’s cobalt mined? What events in that country
dramatically affected the price of cobalt?
Solution:
More than 50% of the world’s annual cobalt production originates from the Democratic
Republic of Congo. Historically, political instability in the region significantly impacted
cobalt prices. Political unrest in the early 1980s caused cobalt price spikes of up to
600%.
1.3 In what types of technology do the elements designated as critical materials generally
play important roles?
Solution:
They are important in batteries, magnetism, and a variety of applications associated
with clean energy and electronics.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 1
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
1.4 Based on the information in Figure 1.1, which three elements would you argue are the
most critical among the “critical materials”? Justify your answer.
Solution:
Dysprosium, iridium, and neodynium. These elements rank the highest in supply risk
and are high in importance to energy. Although lithium, nickel, and cobalt rank higher
in importance, they rank lower in supply risk.
1.5 In what region of the periodic table are most of the elements that are listed as critical
materials found?
Solution:
Most of the critical elements are located in the middle of the periodic table,
specifically the region known as the lanthanide series and to a lesser extent the
transition elements.
1.6 What agency of the U.S. government is responsible for identifying an element as a
critical material? What sorts of applications are the primary concern of this agency?
Solution:
The Department of Energy (DOE). Primary concerns are energy-related technologies,
especially clean energy applications such as wind and solar energy and electric cars.
THE STUDY OF CHEMISTRY
1.7 When making observations in the laboratory, which perspective of chemistry are we
normally using?
Solution:
We make observations in the laboratory using the macroscopic perspective of
chemistry, unless very sophisticated instruments are used.
1.8 Which of the following items are matter and which are not? (a) a flashlight,
(b) sunlight, (c) an echo, (d) air at sea level, (e) air at the top of Mount Everest
Solution:
(a) matter, (b) not matter, (c) not matter, (d) matter, (e) matter
1.9 Which macroscopic characteristics differentiate solids, liquids, and gases? (List as
many as possible.)
Solution:
Shape and Volume:
Solids: Solids retain their own shape and volume, resisting deformation. Even when
placed in a container, a solid maintains its shape rather than taking the shape of the
container.
Liquids: Liquids take the shape of their container but maintain a relatively constant
volume.
Gases: Gases expand to fill the entire volume of their container, meaning they do not
maintain a fixed shape or volume.
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accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Compressibility:
Solids: Solids are generally incompressible, meaning their volume changes very little
under pressure.
Liquids: Liquids are also generally considered incompressible, although they can be
slightly compressed under very high pressure.
Gases: Gases are highly compressible. Their volume can be significantly reduced under
pressure.
Flow:
Solids: Solids do not flow. They resist deformation and maintain a fixed shape.
Liquids: Liquids flow readily and take the shape of their container.
Gases: Gases flow readily and expand to fill any space they occupy.
1.10 Do the terms element and atom mean the same thing? If not, how do they differ?
Solution:
No. An element is a pure substance, but the naturally occurring form of the element
may contain more than one atom. An example of this is elemental nitrogen (N2). In this
case the element has two atoms.
1.11 Label each of the following as either a physical process or a chemical process: (a)
rusting of an iron bridge, (b) melting of ice, (c) burning of a wooden stick, (d) digestion
of a baked potato, (e) dissolving of sugar in water.
Solution:
A chemical change involves a change in the composition of matter; that is, some new
substances are formed. A physical change only involves a change
in the physical state of matter; no new substances are formed.
(a) rusting of an iron bridge Chemical, rust forms when iron and oxygen
react chemically.
(b) melting of ice Physical, change from the solid to the liquid
state.
(c) burning of a wooden stick Chemical, the carbon, oxygen and hydrogen
in the wood are transformed into carbon
dioxide and water during combustion.
(d) digestion of a baked potato Chemical, digestion breaks down larger
complex carbohydrate molecules into
simple molecules (like sugars) through
chemical reactions involving enzymes.
(e) dissolving of sugar in water Physical, the sugar molecules are not
changed, they just become surrounded by
water molecules in solution.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 3
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
1.12 Why do physical properties play a role in chemistry if they do not involve any chemical
changes?
Solution:
While physical properties do not involve changes in the chemical composition of
substances, they are essential to understanding and predicting how substances behave
in chemical contexts.
1.13 Physical properties may change because of a chemical change. For example, the color
of an egg “white” changes from clear to white because of a chemical change when it is
cooked. What is another common situation in which a chemical change also leads to a
physical change?
Solution:
The “rusting” of iron is a chemical change. A chemical reaction changes the metal to a
new compound. The rust formed is a brittle, orange-red compound with very different
properties than iron.
1.14 Which part of the description of a compound or element refers to its physical
properties and which to its chemical properties?
(a) Calcium carbonate is a white solid with a density of 2.71 g/cm3. It reacts readily
with an acid to produce gaseous carbon dioxide.
(b) Gray powdered zinc metal reacts with purple iodine to give a white compound.
Solution:
(a) The first sentence describes physical properties; the second sentence describes a
chemical property.
(b) The sentence generally describes a chemical property; however, the stated colors
are physical properties.
OBSERVATIONS, MODELS, AND SYSTEMS
1.15 We used the example of attendance at a football game to emphasize the nature of
observations. Describe another example where deciding how to “count” subjects of
interest could affect the observation.
Solution:
The number of cities located in a state depends on how a city is defined. We would
need to specify what population size makes a city. Our results would vary depending
on that size.
1.16 Complete the following statement: Data that have a small random error but otherwise
fall in a narrow range are (a) accurate, (b) precise, or (c) neither.
Solution:
These data could be precise but not necessarily accurate.
1.17 Complete the following statement: Data that have a large systematic error are (a)
accurate, (b) precise, (c) neither.
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accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution:
Data that have a large systematic error are (c) neither accurate nor precise. Large
systematic error indicates a consistent bias in the measurements, pushing them
consistently higher or lower than the true value. Accuracy reflects how close a
measurement is to its true value. Systematic errors directly contradict accuracy by
introducing a persistent deviation from the true value. Precision describes the closeness
of multiple measurements to each other. While precise measurements exhibit minimal
scatter, a large systematic error means those measurements are consistently off-target,
even if tightly grouped.
1.18 Two golfers are practicing shots around a putting green. Each golfer takes
20 shots. Golfer 1 has 7 shots within 1 meter of the hole, and the other
13 shots are scattered around the green. Golfer 2 has 17 shots go into a small sand
trap near the green and three just on the green near the trap. Which golfer is more
precise? Which is more accurate?
Solution:
Golfer 2 is more precise because his efforts are grouped more tightly around
a central point (mean) even if it’s not the intended spot. Golfer 1 is more accurate as
there are more shots very close to the accepted “value” (the hole).
1.19 Use your own words to explain the difference between deductive and inductive
reasoning.
Solution:
Deductive reasoning moves from general principles to specific conclusions, ensuring
certainty if the premises hold true. Inductive reasoning moves from specific
observations to general conclusions, providing probable but not absolute certainty.
1.20 Suppose you are waiting at a corner for a bus. Three different routes pass this
particular corner. You see buses pass by from the two routes you are not interested in
taking. When you say to yourself, “My bus must be next,” what type of reasoning
(deductive or inductive) are you using? Explain your answer.
Solution:
Deductive reasoning is being applied in this case. The first two buses represent pieces
of information that are processed and lead to the conclusion that the “desired” bus
must be next.
1.21 When a scientist looks at an experiment and then predicts the results of other related
experiments, which type of reasoning is she using? Explain your answer.
Solution:
This is inductive reasoning. A scientist makes predictions and then tries to prove the
prediction by later observations. Deductive reasoning involves starting with facts and
then drawing conclusions from those.
1.22 What is the difference between a hypothesis and a question?
Solution:
A hypothesis is a statement related to observation(s). The hypothesis is either
accepted or rejected based upon experimentation. A question is simply posed and
prompts an investigation.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 5
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
1.23 Should the words theory and model be used interchangeably in the context of science?
Defend your answer using web information.
Solution:
The word theory implies something more advanced and supported than a model. When
a model makes predictions and all observations are consistent with these
observations, then the model may be described as a theory.
1.24 What is a law of nature? Are all scientific laws examples of laws of nature?
Solution:
A law of nature is an irrefutable, self-evident fact. Not all scientific laws are examples
of laws of nature.
NUMBERS AND MEASUREMENTS
1.25 Describe a miscommunication that can arise because units are not included as part of
the information.
Solution:
Discussing the time of day and omitting p.m. or a.m. If you are supposed to meet
someone at 9:00 but they didn’t say in the evening or in the morning, the meeting
might not occur. Another example might be negotiating a price while trying to buy
something.
1.26 What is the difference between a qualitative and a quantitative measurement?
Solution:
A quantitative measurement provides information as to how much analyte is present. A
qualitative measurement answers the question, “Is the analyte present?”
1.27 Identify which of the following units are base units in the SI system: grams, meters,
joules, liters, and amperes.
Solution:
Meters and amperes are base units. The other base units are: kilograms, seconds,
kelvin, moles, and candelas. Therefore, grams are not a base unit. Joules and liters are
both derived units.
1.28 What is a “derived” unit?
Solution:
A derived unit is a unit that is made up of two or more base units.
1.29 Rank the following prefixes in order of increasing size of the number they represent:
centi-, giga-, nano-, and kilo-.
Solution:
In order of smallest to largest: nano- (10−9), centi- (10−2), kilo- (103), giga- (109).
1.30 The largest computers now include disk storage space measured in petabytes. How
many bytes are in a petabyte? (Recall that in computer terminology, the prefix is only
“close” to the value it designates in the metric system.)
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 6
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution:
1 petabyte = 1,000,000,000,000,000 bytes (1015 bytes)
1.31 Historically, some unit differences reflected the belief that the quantity measured was
different when it was later revealed to be a single entity. Use the web to look up the
origins of the energy units erg and calorie, and describe how they represent an
example of this type of historical development.
Solution:
The erg was an energy unit associated with work done, while the calorie was an energy
unit associated with heat. At the time scientists thought heat and work were different
things—instead of forms of energy used in different ways.
1.32 Use the web to determine how the Btu was initially established. For the engineering
applications where this unit is still used today, why is it a sensible unit?
Solution:
The amount of energy required to raise one pound of liquid water 1 degree Fahrenheit
at its maximum density (occurs at 39.1 °F). It is sensible because of the associated
temperature change that can be sensed or measured.
1.33 How many micrograms are equal to one gram?
Solution:
The prefix micro- represents the power 10−6. One microgram (µg) is therefore equal to
1
gram. There are one million micrograms in one gram.
1, 000, 000
1.34 Convert the value 0.120 ppb into ppm.
Solution:
Parts per billion are ppb and parts per million are ppm. There is 1000 ppb for one ppm.
0.120 ppb ÷ 1000 = 1.20 × 10–4 ppm
1.35 How was the Fahrenheit temperature scale calibrated? Describe how this calibration
process reflects measurement errors that were evident when the temperature scale
was devised.
Solution:
Initially, body temperature was designated as 100°F. This choice, as the source points out,
clearly prioritized convenience over precision, as human body temperature can fluctuate
significantly. The second reference point was the lowest temperature achievable by adding
salt to ice water, which was set as 0°F. This method, wh0ile seemingly objective, suffers
from variability in the salt concentration and ambient conditions, potentially leading to
inconsistent results.
1.36 Superconductors are materials that have no resistance to the flow of electricity, and
they hold great promise in many engineering applications. But to date,
superconductivity has only been observed under cryogenic conditions. As of 2022, the
highest temperature at which superconductivity has been observed is 250 K. Convert
this temperature to both °C and °F.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 7
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution:
°C = 250 K – 273.15 = –23°C; °F = 1.8(–23.15°C) + 32 = –9.7°F
1.37 Express each of the following temperatures in kelvins:
(a) −10.°C
(b) 0.00°C
(c) 280.°C
(d) 1.4 × 103°C
Solution:
(a) kelvins = −10°C + 273.15 = 263 K
(b) kelvins = 0.00°C + 273.15 = 273.15 K
(c) kelvins = 280°C + 273.15 = 553 K
(d) kelvins = 1400°C + 273.15 = 1673 K
To convert from the Celsius to the Kelvin scale, we add 273.15. The unit size is the
same, making this conversion easier. Note: We do not write the degree symbol with
kelvins.
1.38 Express (a) 275°C in K, (b) 25.55 K in °C, (c) –47.0°C in °F, and (d) 100.0°F in K.
Solution:
(a) 275°C + 273.15 = 548 K
(b) 25.55 K – 273.15 = –247.60°C
(c) 1.8(–47.0°C) +32 = –52.6°F
(d) (100.0°F – 32) ÷ 1.8 = + 273.15 = 310.9 K
1.39 Express each of the following numbers in scientific notation:
(a) 62.13
(b) 0.000414
(c) 0.0000051
(d) 871,000,000
(e) 9100
Solution:
(a) 6.213 × 101
(b) 4.14 × 10−4
(c) 5.1 × 10−6
(d) 8.71 × 108
(e) 9.1 × 103
Scientific notation expresses a number factoring out all powers of 10 and writing a
number between 1 and 10 multiplied by some power of 10. It makes writing very small
or very large numbers much easier.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 8
accessible website, in whole or in part.
Chemistry for Engineering Students 5th Edition Brown
Important Notes
The file includes the complete test bank, organized chapter by chapter.
A sample of selected pages has been provided for preview.
All available appendices and Excel files (if included in the original resources) are
provided.
We continuously update our files to ensure you receive the latest and most accurate
editions.
New editions are added regularly – stay connected for updates!
Purchase Guarantee
If you believe you have purchased the wrong file, don’t worry. Contact us anytime and we
will gladly replace it with the correct version.
Contact Email:
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution and Answer Guide
LARRY BROWN & TOM HOLME, CHEMISTRY FOR ENGINEERING STUDENTS, 5E 2025,
9780357974803; CHAPTER 1: INTRODUCTION TO CHEMISTRY
TABLE OF CONTENTS
Critical Materials ...................................................................................................................1
The Study of Chemistry ....................................................................................................... 2
Observations, Models, and Systems ................................................................................... 4
Numbers and Measurements ............................................................................................... 6
Problem Solving in Chemistry and Engineering ................................................................ 11
Touchscreen Technology ....................................................................................................17
Conceptual Problems ..........................................................................................................18
Focus on Problem Solving Exercises ................................................................................ 20
CRITICAL MATERIALS
1.1 Are the elements designated as critical materials all rare? Explain your answer.
Solution:
While some critical materials may be rare, the classification considers factors beyond
just rarity: primarily an element’s importance and the risk associated with its supply.
1.2 In what country is most of the world’s cobalt mined? What events in that country
dramatically affected the price of cobalt?
Solution:
More than 50% of the world’s annual cobalt production originates from the Democratic
Republic of Congo. Historically, political instability in the region significantly impacted
cobalt prices. Political unrest in the early 1980s caused cobalt price spikes of up to
600%.
1.3 In what types of technology do the elements designated as critical materials generally
play important roles?
Solution:
They are important in batteries, magnetism, and a variety of applications associated
with clean energy and electronics.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 1
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
1.4 Based on the information in Figure 1.1, which three elements would you argue are the
most critical among the “critical materials”? Justify your answer.
Solution:
Dysprosium, iridium, and neodynium. These elements rank the highest in supply risk
and are high in importance to energy. Although lithium, nickel, and cobalt rank higher
in importance, they rank lower in supply risk.
1.5 In what region of the periodic table are most of the elements that are listed as critical
materials found?
Solution:
Most of the critical elements are located in the middle of the periodic table,
specifically the region known as the lanthanide series and to a lesser extent the
transition elements.
1.6 What agency of the U.S. government is responsible for identifying an element as a
critical material? What sorts of applications are the primary concern of this agency?
Solution:
The Department of Energy (DOE). Primary concerns are energy-related technologies,
especially clean energy applications such as wind and solar energy and electric cars.
THE STUDY OF CHEMISTRY
1.7 When making observations in the laboratory, which perspective of chemistry are we
normally using?
Solution:
We make observations in the laboratory using the macroscopic perspective of
chemistry, unless very sophisticated instruments are used.
1.8 Which of the following items are matter and which are not? (a) a flashlight,
(b) sunlight, (c) an echo, (d) air at sea level, (e) air at the top of Mount Everest
Solution:
(a) matter, (b) not matter, (c) not matter, (d) matter, (e) matter
1.9 Which macroscopic characteristics differentiate solids, liquids, and gases? (List as
many as possible.)
Solution:
Shape and Volume:
Solids: Solids retain their own shape and volume, resisting deformation. Even when
placed in a container, a solid maintains its shape rather than taking the shape of the
container.
Liquids: Liquids take the shape of their container but maintain a relatively constant
volume.
Gases: Gases expand to fill the entire volume of their container, meaning they do not
maintain a fixed shape or volume.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 2
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Compressibility:
Solids: Solids are generally incompressible, meaning their volume changes very little
under pressure.
Liquids: Liquids are also generally considered incompressible, although they can be
slightly compressed under very high pressure.
Gases: Gases are highly compressible. Their volume can be significantly reduced under
pressure.
Flow:
Solids: Solids do not flow. They resist deformation and maintain a fixed shape.
Liquids: Liquids flow readily and take the shape of their container.
Gases: Gases flow readily and expand to fill any space they occupy.
1.10 Do the terms element and atom mean the same thing? If not, how do they differ?
Solution:
No. An element is a pure substance, but the naturally occurring form of the element
may contain more than one atom. An example of this is elemental nitrogen (N2). In this
case the element has two atoms.
1.11 Label each of the following as either a physical process or a chemical process: (a)
rusting of an iron bridge, (b) melting of ice, (c) burning of a wooden stick, (d) digestion
of a baked potato, (e) dissolving of sugar in water.
Solution:
A chemical change involves a change in the composition of matter; that is, some new
substances are formed. A physical change only involves a change
in the physical state of matter; no new substances are formed.
(a) rusting of an iron bridge Chemical, rust forms when iron and oxygen
react chemically.
(b) melting of ice Physical, change from the solid to the liquid
state.
(c) burning of a wooden stick Chemical, the carbon, oxygen and hydrogen
in the wood are transformed into carbon
dioxide and water during combustion.
(d) digestion of a baked potato Chemical, digestion breaks down larger
complex carbohydrate molecules into
simple molecules (like sugars) through
chemical reactions involving enzymes.
(e) dissolving of sugar in water Physical, the sugar molecules are not
changed, they just become surrounded by
water molecules in solution.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 3
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
1.12 Why do physical properties play a role in chemistry if they do not involve any chemical
changes?
Solution:
While physical properties do not involve changes in the chemical composition of
substances, they are essential to understanding and predicting how substances behave
in chemical contexts.
1.13 Physical properties may change because of a chemical change. For example, the color
of an egg “white” changes from clear to white because of a chemical change when it is
cooked. What is another common situation in which a chemical change also leads to a
physical change?
Solution:
The “rusting” of iron is a chemical change. A chemical reaction changes the metal to a
new compound. The rust formed is a brittle, orange-red compound with very different
properties than iron.
1.14 Which part of the description of a compound or element refers to its physical
properties and which to its chemical properties?
(a) Calcium carbonate is a white solid with a density of 2.71 g/cm3. It reacts readily
with an acid to produce gaseous carbon dioxide.
(b) Gray powdered zinc metal reacts with purple iodine to give a white compound.
Solution:
(a) The first sentence describes physical properties; the second sentence describes a
chemical property.
(b) The sentence generally describes a chemical property; however, the stated colors
are physical properties.
OBSERVATIONS, MODELS, AND SYSTEMS
1.15 We used the example of attendance at a football game to emphasize the nature of
observations. Describe another example where deciding how to “count” subjects of
interest could affect the observation.
Solution:
The number of cities located in a state depends on how a city is defined. We would
need to specify what population size makes a city. Our results would vary depending
on that size.
1.16 Complete the following statement: Data that have a small random error but otherwise
fall in a narrow range are (a) accurate, (b) precise, or (c) neither.
Solution:
These data could be precise but not necessarily accurate.
1.17 Complete the following statement: Data that have a large systematic error are (a)
accurate, (b) precise, (c) neither.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 4
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution:
Data that have a large systematic error are (c) neither accurate nor precise. Large
systematic error indicates a consistent bias in the measurements, pushing them
consistently higher or lower than the true value. Accuracy reflects how close a
measurement is to its true value. Systematic errors directly contradict accuracy by
introducing a persistent deviation from the true value. Precision describes the closeness
of multiple measurements to each other. While precise measurements exhibit minimal
scatter, a large systematic error means those measurements are consistently off-target,
even if tightly grouped.
1.18 Two golfers are practicing shots around a putting green. Each golfer takes
20 shots. Golfer 1 has 7 shots within 1 meter of the hole, and the other
13 shots are scattered around the green. Golfer 2 has 17 shots go into a small sand
trap near the green and three just on the green near the trap. Which golfer is more
precise? Which is more accurate?
Solution:
Golfer 2 is more precise because his efforts are grouped more tightly around
a central point (mean) even if it’s not the intended spot. Golfer 1 is more accurate as
there are more shots very close to the accepted “value” (the hole).
1.19 Use your own words to explain the difference between deductive and inductive
reasoning.
Solution:
Deductive reasoning moves from general principles to specific conclusions, ensuring
certainty if the premises hold true. Inductive reasoning moves from specific
observations to general conclusions, providing probable but not absolute certainty.
1.20 Suppose you are waiting at a corner for a bus. Three different routes pass this
particular corner. You see buses pass by from the two routes you are not interested in
taking. When you say to yourself, “My bus must be next,” what type of reasoning
(deductive or inductive) are you using? Explain your answer.
Solution:
Deductive reasoning is being applied in this case. The first two buses represent pieces
of information that are processed and lead to the conclusion that the “desired” bus
must be next.
1.21 When a scientist looks at an experiment and then predicts the results of other related
experiments, which type of reasoning is she using? Explain your answer.
Solution:
This is inductive reasoning. A scientist makes predictions and then tries to prove the
prediction by later observations. Deductive reasoning involves starting with facts and
then drawing conclusions from those.
1.22 What is the difference between a hypothesis and a question?
Solution:
A hypothesis is a statement related to observation(s). The hypothesis is either
accepted or rejected based upon experimentation. A question is simply posed and
prompts an investigation.
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accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
1.23 Should the words theory and model be used interchangeably in the context of science?
Defend your answer using web information.
Solution:
The word theory implies something more advanced and supported than a model. When
a model makes predictions and all observations are consistent with these
observations, then the model may be described as a theory.
1.24 What is a law of nature? Are all scientific laws examples of laws of nature?
Solution:
A law of nature is an irrefutable, self-evident fact. Not all scientific laws are examples
of laws of nature.
NUMBERS AND MEASUREMENTS
1.25 Describe a miscommunication that can arise because units are not included as part of
the information.
Solution:
Discussing the time of day and omitting p.m. or a.m. If you are supposed to meet
someone at 9:00 but they didn’t say in the evening or in the morning, the meeting
might not occur. Another example might be negotiating a price while trying to buy
something.
1.26 What is the difference between a qualitative and a quantitative measurement?
Solution:
A quantitative measurement provides information as to how much analyte is present. A
qualitative measurement answers the question, “Is the analyte present?”
1.27 Identify which of the following units are base units in the SI system: grams, meters,
joules, liters, and amperes.
Solution:
Meters and amperes are base units. The other base units are: kilograms, seconds,
kelvin, moles, and candelas. Therefore, grams are not a base unit. Joules and liters are
both derived units.
1.28 What is a “derived” unit?
Solution:
A derived unit is a unit that is made up of two or more base units.
1.29 Rank the following prefixes in order of increasing size of the number they represent:
centi-, giga-, nano-, and kilo-.
Solution:
In order of smallest to largest: nano- (10−9), centi- (10−2), kilo- (103), giga- (109).
1.30 The largest computers now include disk storage space measured in petabytes. How
many bytes are in a petabyte? (Recall that in computer terminology, the prefix is only
“close” to the value it designates in the metric system.)
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 6
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution:
1 petabyte = 1,000,000,000,000,000 bytes (1015 bytes)
1.31 Historically, some unit differences reflected the belief that the quantity measured was
different when it was later revealed to be a single entity. Use the web to look up the
origins of the energy units erg and calorie, and describe how they represent an
example of this type of historical development.
Solution:
The erg was an energy unit associated with work done, while the calorie was an energy
unit associated with heat. At the time scientists thought heat and work were different
things—instead of forms of energy used in different ways.
1.32 Use the web to determine how the Btu was initially established. For the engineering
applications where this unit is still used today, why is it a sensible unit?
Solution:
The amount of energy required to raise one pound of liquid water 1 degree Fahrenheit
at its maximum density (occurs at 39.1 °F). It is sensible because of the associated
temperature change that can be sensed or measured.
1.33 How many micrograms are equal to one gram?
Solution:
The prefix micro- represents the power 10−6. One microgram (µg) is therefore equal to
1
gram. There are one million micrograms in one gram.
1, 000, 000
1.34 Convert the value 0.120 ppb into ppm.
Solution:
Parts per billion are ppb and parts per million are ppm. There is 1000 ppb for one ppm.
0.120 ppb ÷ 1000 = 1.20 × 10–4 ppm
1.35 How was the Fahrenheit temperature scale calibrated? Describe how this calibration
process reflects measurement errors that were evident when the temperature scale
was devised.
Solution:
Initially, body temperature was designated as 100°F. This choice, as the source points out,
clearly prioritized convenience over precision, as human body temperature can fluctuate
significantly. The second reference point was the lowest temperature achievable by adding
salt to ice water, which was set as 0°F. This method, wh0ile seemingly objective, suffers
from variability in the salt concentration and ambient conditions, potentially leading to
inconsistent results.
1.36 Superconductors are materials that have no resistance to the flow of electricity, and
they hold great promise in many engineering applications. But to date,
superconductivity has only been observed under cryogenic conditions. As of 2022, the
highest temperature at which superconductivity has been observed is 250 K. Convert
this temperature to both °C and °F.
© 2025 Cengage Learning, Inc. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly 7
accessible website, in whole or in part.
, Solution and Answer Guide: Larry Brown & Tom Holme, Chemistry For Engineering Students, 5e 2025,
9780357974803; Chapter 1: Introduction to Chemistry
Solution:
°C = 250 K – 273.15 = –23°C; °F = 1.8(–23.15°C) + 32 = –9.7°F
1.37 Express each of the following temperatures in kelvins:
(a) −10.°C
(b) 0.00°C
(c) 280.°C
(d) 1.4 × 103°C
Solution:
(a) kelvins = −10°C + 273.15 = 263 K
(b) kelvins = 0.00°C + 273.15 = 273.15 K
(c) kelvins = 280°C + 273.15 = 553 K
(d) kelvins = 1400°C + 273.15 = 1673 K
To convert from the Celsius to the Kelvin scale, we add 273.15. The unit size is the
same, making this conversion easier. Note: We do not write the degree symbol with
kelvins.
1.38 Express (a) 275°C in K, (b) 25.55 K in °C, (c) –47.0°C in °F, and (d) 100.0°F in K.
Solution:
(a) 275°C + 273.15 = 548 K
(b) 25.55 K – 273.15 = –247.60°C
(c) 1.8(–47.0°C) +32 = –52.6°F
(d) (100.0°F – 32) ÷ 1.8 = + 273.15 = 310.9 K
1.39 Express each of the following numbers in scientific notation:
(a) 62.13
(b) 0.000414
(c) 0.0000051
(d) 871,000,000
(e) 9100
Solution:
(a) 6.213 × 101
(b) 4.14 × 10−4
(c) 5.1 × 10−6
(d) 8.71 × 108
(e) 9.1 × 103
Scientific notation expresses a number factoring out all powers of 10 and writing a
number between 1 and 10 multiplied by some power of 10. It makes writing very small
or very large numbers much easier.
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accessible website, in whole or in part.
