Download AP Chemistry Summer Preparation Work 2014

AP Chemistry Summer Preparation Work 2014
Mrs. Alicia Schwartz – Lemon Bay High School
[email protected]
http://agundry.coursesites.com/
Dear future AP Chemistry student:
I am very happy to welcome you to advanced placement chemistry even before the new school year has
begun. I am really excited about the coming year and I hope you are too. Many people consider AP chemistry one
of the hardest AP classes. I believe that if you work hard this class will be a real pleasure and very easy for you.
The benefits of passing this class and scoring high in the AP exam make the effort worth it. If you pass the AP
exam with a 5 most schools in the country will award you 8 credits of chemistry. That includes the first two
college semesters of chemistry and the two laboratory classes that come with it. This is a great time and money
saver for college. Even if your college does not accept these credits, you will have gained knowledge of the topics
covered and you will breeze through freshman chem. The fundamentals in this class are essential to anyone
planning on being an engineer, a scientist, a doctor, a nurse, a psychologist, even a chef!
If you love science like I do, there is also the bonus of learning how matter works and how our universe
can be explained by understanding the interactions between matter and energy. You will also get to perform some
neat laboratory experiments at the college level.
For your summer assignment, I want you all to get through all of Chapters 1, 2, and 3 (not section 3.11)
from the Zumdahl textbook. I also want you to read a book by Peter Atkins. Atkins has written many chemistry
books that provide an easy to understand, concise breakdown of a topic. The specific Atkins book I want you to
read is called “What is Chemistry?” (ISBN: 0199683987) and lays a solid foundational knowledge, while
generating interest in the discipline. This book is available on Amazon.com for approximately $15 for a new print
version, or $10 for an electronic version. I believe that this book will be a nice start to your AP Chemistry career.
With the textbook, you will be able to download practice problems that go with the textbook. Besides the
packet, you will be able to find study guides for each of the first 3 chapters full of information, as well as practice
problems, you are to complete these practice problems.
I also suggest that you begin a notebook full of notes that you take while reading the textbook. If you did
not pick up a textbook from the school, you can download a pdf copy of it from blackboard. Also on blackboard is
an older copy of the 5 steps to a 5 review book for your download and use.
To succeed in this class it is important to have a solid background in basic high school chemistry. If you
are in this class, it is because you have had a great experience in honors chemistry and want to learn more. This
summer work will help you refresh some of the fundamentals needed to succeed in AP chem. When we return
from summer break, I will be giving you an exam on this material to assess your strengths and weaknesses. This
test will be based on the information from the textbook and reading, so if you work with it throughout the summer,
you will have no problem. If you feel that you remember everything and get the problems right then don’t kill
yourself, enjoy your summer. If you don’t remember how to do some of the problems then spend the time figuring
it out. If you have any questions while working, feel free to contact me, or use the discussion feature on
blackboard. I believe that many of you can help each other work through the problems.
**So in summary, your summer assignment is to learn the first three chapters of the textbook (minus section 3.11).
You will have online submissions periodically due throughout the summer to ensure that the assignment is
completed in a timely manner and not done in the last two nights of summer.
The timeline for summer is as follows: (Due to me by 11 pm of that day):
5/30/14- Email me @ [email protected] so I can invite you to register for blackboard.
6/20/14- Chapter 1 material is due. You need to email me your written work from the Ch. 1 Study Guide. There are
40 problems that cover material from this chapter. You can either scan this work in to me or email me a
high resolution picture (by high resolution, I mean that if you have an iphone, either choose the “actual” or
“large” size option). Please ensure that I can read the document.
7/11/14- Chapter 2 material is due. You need to email me your written work from the Ch. 2 Study Guide. There are
37 problems that cover material from this chapter. You can either scan this work in to me or email me a
high resolution picture (by high resolution, I mean that if you have an iphone, either choose the “actual” or
“large” size option). Please ensure that I can read the document.
7/25/14- The first half of the Chapter 3 material is due. You need to email me your written work from the Ch. 3
Study Guide, numbers 1-35, covering sections 3.1-3.5. You can either scan this work in to me or email me
a high resolution picture (by high resolution, I mean that if you have an iphone, either choose the “actual”
or “large” size option). Please ensure that I can read the document.
8/15/14- The rest of the Chapter 3 material is due. You need to email me your written work from the Ch. 3 Study
Guide, numbers 36-72. You can either scan this work in to me or email me a high resolution picture (by
high resolution, I mean that if you have an iphone, either choose the “actual” or “large” size option). Please
ensure that I can read the document.
Ch. 1- Chemical Foundations:
1.1 Chemistry: An overview
1.2 The Scientific Method
1.3 Units of Measurement
1.4 Uncertainty in Measurement
1.5 Significant Figures and Calculations
1.6 Dimensional Analysis
1.7 Temperature
1.8 Density
1.9 Classification of Matter
Ch. 2- Atoms, Molecules, and Ions
2.1 The Early History of Chemistry
2.2 Fundamental Chemical Laws
2.3 Dalton’s Atomic Theory
2.4 Early Experiments that Characterize the Atom
2.5 The Modern View of Atomic Structure: An Introduction
2.6 Molecules and Ions
2.7 An Introduction to the Periodic Table
2.8 Naming Simple Compounds
Ch. 3 Stoichiometry
3.1 Counting by Weighing
3.2 Atomic Masses
3.3 The Mole
3.4 Molar Mass
3.5 Learning to Solve Problems
3.6 Percent Composition of Compounds
3.7 Determining the Formula of a Compound
3.8 Chemical Equations
3.9 Balancing Chemical Equations
3.10 Stoichiometric Calculations
XX 3.11 The Concept of Limiting Reagent
After registering for blackboard, please check the e-mail that you provided me with periodically (at least twice a
week), so I can keep you updated on any changes.
Thank you again for accepting the challenge of AP Chemistry. I hope you have a great summer and I look forward
to seeing you in August.
Mrs. Schwartz
Ch. 1 Study Guide
Section 1.2
1. In a simulated boxing match done on a computer several years ago, Joe Louis (champion in the 1940s) defeated Muhammad
Ali (champion in the 1960s) in 15 rounds. The computer simulation took into account the fighters’ heights, weights, styles,
punching power, and speed. (1)Was the simulation realistic? (2)What other variables would have to be included to make the
simulation more valid?
2. If your chemistry teacher said she knew that the Earth is flat and challenged you to prove, using scientific tests, that she was
wrong, what tests might you perform?
Section 1.3
3. List the fundamental units that you would combine to get the following derived units (you may need to look up the meaning
of some of the terms):
a. velocity
c. volume
e. density
b. acceleration
d. specific heat
f. pressure
4. Put the following prefixes in order, from smallest to largest: femto, tera, mega, deci, kilo, atto, exa.
5. Put the following prefixes in order, from smallest to largest: giga, hecto, micro, peta, milli, nano, pico.
6. A student was shopping for additional computer memory. She saw a display with 3 memory chips that had these labels. (The
price per byte for each chip was the same.)
50 gigabytes
50 terabytes
50 megabytes.
a. If price were no object, which memory chip should she buy?
b. If price were the most important consideration, which memory chip should she buy?
Section 1.4
7. Three students weighed the same sample of copper shot five times. Their results were as follows:
a. Calculate the mean (average) mass of the sample determined by each student.
b. The average deviation (a.d.) is a measure of precision. It is calculated by the formula:
That means that you take each of the values in a data set (5 total values), subtract the mean, and
take the absolute value. Add all 5 absolute values and divide the total by 5. That number is your
a.d. Calculate the average deviation for each student’s data.
c. If the true mass of copper shot is 15.384 g, which student was most accurate? Which was most precise? What could be
the possible sources of error in the determinations?
8. A student weighed 15 pennies on a balance and recorded the following masses:
3.078
3.055
3.060
3.066
3.102
2.107
3.121
2.518
3.052
2.476
2.546
3.050
3.073
3.080
3.128
a. Calculate the mean mass.
b. What might cause the difference in weights?
9. Define the following terms:
a. accuracy
c. random error
b. precision
d. systematic error
10. A student had purchased an “official” quatloo from its owners on the planet Triskelion. Its mass is listed on the box as 83.4
grams. The student weighed the quatloo and got these readings for mass: 71.97 g, 71.69 g, and 71.80 g.
a. What is the average mass of the quatloo, according to the student’s measurement?
b. If we assume that the mass of the quatloo is what the seller claimed, was the mass measurement made by the student
accurate, precise, both, or neither?
Section 1.5
11. How many significant figures are there in each of the following values?
a. 6.07 × 10-15
c. 17.00
e. 463.8052
b. 0.003840
d. 8 × 108
12. How many significant figures are there in each of the following values?
a. 1406.20
c. 1600.0
e. 1.250 × 10-3
b. 0.0007
d. 0.0261140
13. Which value has more significant figures, 7.63 × 10-11 or 0.00076?
14. Use exponential notation to express the number 37,100,000 with:
a. one sig fig
b. two sig figs
c. three sig figs
d. six sig figs
15. Perform the indicated calculations on the following measured values, giving the final answer with the correct number of
significant figures.
a. 16.81 + 3.2257
c. (3.8 × 10-12 + 4 × 10-13)/(4 × 1012 + 6.3 × 1013)
b. 324.6 × 815.991
d. 3.14159 × 68 / (5.18 × 10-11 - 6 × 10-4)
16. Perform the indicated calculations on the following measured values, giving the final answer with the correct number of
significant figures.
a. 2.85 + 3.4621 + 1.3
b. 7.442 - 7.429
c. 1.65 × 14 × 100.0
d. 27/4.148
e. [(3.901 - 3.887)/3.901]
f. 6.404 × 2.91 × (18.7 - 17.1)
Section 1.7
17. Using the conversion factors in the inside back cover of your textbook, convert 3.5 quarts to:
a. liters (L)
b. milliliters (mL)c. microliters (μL)
d. cubic centimeters (cm3)
18. Using the conversion factors in the inside back cover of your textbook, convert 4.2 yards to:
a. meters
b. centimeters
c. micrometers
d. kilometers
19. If you put 8 gallons of gas in your car and it cost you a total of $19.04, what is the cost of gas per liter?
20. A runner can run a 5.0 kilometer race in a time of 21 minutes and 22 seconds.
a. What is the runner’s speed in miles per hour?
b. How long, on the average, did it take for the runner to run one mile?
21. A student made the 27.0 kilometer drive to school in 16 minutes.
a. How many miles did the student drive?
b. If the speed limit is 55 mph, was the student speeding? How fast was the student driving?
22. A radio station broadcasts at a frequency of 107.9 megahertz (MHz), (cycles per second).
a. How many seconds per cycle are there in 107.9 MHz?
b. What is the broadcast frequency in gigahertz (GHz)?
23. A 5-lb bag of flour costs $0.89. What is the cost of flour per kilogram?
24. A “joule,” like a calorie, is a unit of energy. There are 4.184 joules per calorie. How many joules of energy are available in
one ounce of Frosted Flakes®, which has 120,000 calories? (Note: a “food calorie” (called a Calorie, with a capital “C”) = 1000
energy calories.)
25. If you have to eat 20 tablespoonfuls of cereal to eat the entire ounce of dry Frosted Flakes® (discussed in the previous
problem) and there are 3 teaspoon measures in one tablespoon, how many food calories of Frosted Flakes® are in each
teaspoonful?
26. During a recent baseball game, a pitcher threw a fastball that had a velocity of 93.7 mph.
a. Calculate the velocity in meters/second.
b. Calculate how long it took this pitch to travel from the mound to home plate (60 ft 6 in).
27. Which of the following is greater:
a. 35 kg or 3500 g?
b. 6 × 104 mL or 6 × 103 L?
28. A chemical manufacturing plant wishes to scale up a process to make aspirin. In doing so, it needs to increase the amount of
a reactant from kilograms per day to gigagrams per day. The production staff finished its calculation, they found they needed
352,600 kilograms per day to scale up. How many gigagrams per day did they require?
29. If a student weighs 185 lb, what is his mass in μg?
Section 1.8
30. Which is the higher temperature, 42°C or 92°F?
31. Perform the following temperature conversions:
a. 300. K to °F
b. 300.°F to K
c. −40.°F to °C
d. −100.°C to K
e. 1555 K to °C f. 0.0 K to °F
32. Perform the following temperature conversions:
a. 16°C to °F
b. 305 K to °F
c. 0.0°F to °C
d. 150°F to K
e. −45°C to K
f. 920 K to °C
Section 1.9
33. A sample of motor oil with a mass of 440 g occupies 500 mL. What is the density of the motor oil?
34. A worker at the United States Mint wants to know if a batch of 100 pennies was minted before 1982 (100% copper) or after
1982 (3% copper and 97% zinc). Assuming that both groups of pennies had the same dimensions, would she get her answer by
weighing the coins? Explain.
35. The density of an object is 1.63 g/mL. Its volume is 0.27 L. What is the mass of the object?
36. An object weighing 4.0 lbs occupies 1700 mL. What is the density of the object in g/mL?
37. The density of the Earth is about 3.5 g/cm3. If the Earth has a radius of 7000 miles, what’s its mass? (volume = [4πr3/3])
38. Which of the following is less:
a. 8.7 g/mL or 6.1 μg/μL?
b. 4 × 10-2 kg/cm3 or 4 × 10-1 mg/cm3?
39. Which is greater:
a. 16.1 pounds per cubic inch, or 704 grams per cm3?
b. 22 miles per second, or 3.8 × 105 km per hour?
Section 1.10
40. Define the following:
a. mixture
b. pure substance
c. homogeneous
d. heterogeneous
41. List five physical methods of separating mixtures.
Ch. 2 Study Guide
Section 2.2
1. In an exothermic (heat producing) reaction, chlorine reacts with 2.0200 g of hydrogen to form 72.926 g of hydrogen chloride
gas. How many grams of chlorine reacted with hydrogen?
2. Sulfur and oxygen can react to form both sulfur dioxide and sulfur trioxide. In sulfur dioxide, there are 32.06 g of sulfur and
32.00 g of oxygen. In sulfur trioxide, 32.06 g of sulfur are combined with 48.00 g of oxygen.
a. What is the ratio of the weights of oxygen that combine with 32.06 g of sulfur?
b. How do these data illustrate the law of multiple proportions?
3. By experiment it has been found that 2.18 g of zinc metal combines with oxygen to yield 2.71 g of zinc oxide. How many
grams of oxygen reacted with zinc metal?
4. A sample of H2SO4 contains 2.02 g of hydrogen, 32.07 g of sulfur, and 64 g of oxygen. How many grams of sulfur and grams
of oxygen are present in a second sample of H2SO4 containing 7.27 g of hydrogen?
Section 2.3
5. Describe what part of Dalton's atomic theory each chemical statement relates to.
a. H2 + Cl2 → 2HCl
b. There are 3.01 × 1023 atoms in 20.04 g of calcium.
c. Lead does not change to chromium when it forms lead hydroxide.
Section 2.5
6. Identify each of the following elements:
7. Identify each of the following elements:
8. How many protons and neutrons are in each of the following elements?
9. How many protons and neutrons are in each of the following elements?
Section 2.6
10. How many protons, neutrons, and electrons are in each of the following ions?
11. How many protons, neutrons, and electrons are in each of the following?
12. Fill in the missing information in the following table:
13. Fill in the missing information in the following table:
Section 2.7
14. Name the family to which each of the following elements belongs:
a. Fe
b. Ar
c. Rb
d. Cl
e. Sr
f. Nd
15. Are the following elements metals or nonmetals?
a. Mg
b. Br
c. Co
d. P
e. O
f. Mo
g. Hg
h. Bi
i. Xe
16. Name the family to which each of the following elements belongs:
a. Es
b. Yb
c. Fr
d. I
e. Kr
f. Ca
g. Au
17. Given the position in the periodic table, what is the likely oxidation state that each element will have when forming an ion?
a. Cs
b. N
c. Br
d. K
e. Al
f. S
Section 2.8
18. Would you expect the following atoms to gain or lose electrons when forming ions? If so, how many will be gained or lost?
a. Be
b. Cl
c. Al
d. O
e. F
f. Li
g. P
19. An element combines with 2 atoms of chlorine to form an ionic compound. The element has 20 neutrons in its most
abundant form. Write the formula of the compound.
20. An element combines with two atoms of oxygen to form a covalent compound. The element is in the same group as oxygen
but has less than 20 protons, and is in the same period as one that combines with chlorine to form a white solid that we
shake on our food. Identify the element, and give the formula of the compound.
21. An element combines with two atoms of oxygen to form a covalent substance that is, technically, not a compound. Rather,
we can most correctly call it a molecule. The element is in the same group as oxygen but and has less than 20 protons.
What is are the common name and formula for this molecule?
22. Predict the formula and state the name of a compound likely to be formed from the following pairs of elements:
a. sodium and fluorine
b. aluminum and oxygen
23. Predict the formula and state the name of the compound likely to be formed from the following substances:
a. calcium and phosphate ion
b. potassium and nitrate ion
24. Predict the formula and state the name of the compound likely to be formed from these elements:
a. Fe2+ and oxygen
b. cesium and the nitrate ion
25. What are the name and formula of the compound formed by the combination of carbon in its most negative oxidation state
and hydrogen in its most positive oxidation state?
26. Name each of the following compounds:
a. PbI2
e. CsCl
i. K2Cr2O7
b. NH4Cl
f. OsO4
j. Na2SO4
c. Fe2O3
g. Cr(OH) 3
k. KH2PO4
d. LiH
h. NaC2H3O2
27. Name each of the following compounds:
a. MgSO4
d. KMnO4
g. Fe(IO4)3
b. N2O3
e. NiO
h. SO3
c. Ce2O3
f. BaSO4
i. KClO4
28. Name each of the following compounds:
a. NI3
c. CO
e. N2O4
b. PCl5
d. P4O10
f. NH3
29. Name each of the following compounds:
a. P4O6
c. AgNO3
e. AgCl
b. N2
d. BF3
f. KHCO3
30. Name each of the following compounds:
a. HIO3
c. HCN
e. K2SO3
b. HNO2
d. NaNO2
f. NaHSO3
31. Name each of the following compounds:
a. UF6
c. SF6
e. SnCl2
b. Cu(NO3)2
d. H3PO4
f. Na2CO3
32. Write formulas for each of the following compounds:
a. sodium cyanide
c. lead(II) nitrate
e. sodium hydrogen sulfate
b. tin(II) fluoride
d. iron(III) oxide
f. sodium bromate
33. Write formulas for each of the following compounds:
a. sodium sulfate
d. potassium hypochlorite
g. magnesium oxide
b. manganese(IV) oxide
e. lithium aluminum hydride
h. copper(I) oxide
c. potassium chlorate
f. barium chloride
i. hydroiodic acid
34. Write formulas for each of the following compounds:
a. potassium carbonate
f. rubidium nitrate
k. sulfurous acid
b. magnesium hydroxide
g. potassium chlorate
l. potassium hydrogen phosphate
c. dinitrogen tetroxide
h. carbon tetrachloride
m. ammonium acetate
d. hypoiodous acid
i. sodium iodate
n. ammonium dichromate
e. iron(III) chloride
j. potassium permanganate
o. tin(IV) oxide
35. Give the names of the following acids:
a. H2SO3
c. HBr
e. H3PO4
b. HI
d. HNO2
f. HCl
36. Give formulas for the following acids:
a. nitric acid
c. sulfuric acid
e. hydrosulfuric acid
b. hydrofluoric acid
d. hydrocyanic acid
f. acetic acid
37. Give the alternate or common name for each of the following compounds or cations:
a. sodium hydrogen carbonate (NaHCO3)
d. iron(II) (Fe2+)
b. dinitrogen monoxide (N2O)
e. tin(IV) (Sn4+)
c. nitrogen monoxide (NO)
f. lead(II) (Pb2+)
Ch. 3 Study Guide
Section 3.2
1. An element "E" is present as 10E with a mass value of 10.01 amu, and as 11E with a mass value of 11.01 amu. The natural
abundances of 10E and 11E are 19.78% and 80.22% respectively. What is the average atomic mass of the element? What is
the element?
2. Naturally occurring sulfur consists of four isotopes, 32S (95.0%), 33S (0.76%), 34S (4.22%), and 36S (0.014%). Using these
data, calculate the atomic weight of naturally occurring sulfur. The masses of the isotopes are given in the table below.
3. An unknown sample of mystery element "T" is injected into the mass spectrometer. According to the mass spectrum, 7.42%
of the element is present as 6T, and 92.58% is present as 7T. The mass values are 6.02 amu for 6T and 7.02 amu for 7T.
Calculate the average atomic mass, and identify the mystery element.
4. A noble gas consists of three isotopes of masses 19.99 amu, 20.99 amu, and 21.99 amu. The relative abundance of these
isotopes is 90.92%, 0.257%, and 8.82% respectively. What is the average atomic mass of this noble gas? What noble gas is
this?
5. Chlorine has two stable isotopes. The mass of one isotope is 34.97 amu. Its relative abundance is 75.53%. What is the mass
of the other stable isotope?
6. Complete the following table of isotopic information for the element neon (Ne).
7. Silicon has three stable isotopes in nature as shown in the table below. Fill in the missing information.
8. Gallium has two stable isotopes of masses 68.93 amu (69Ga) and 70.92 amu (71Ga). What are the relative abundances of the
two isotopes?
9. Magnesium exists as three isotopes in nature. One isotope (25Mg) has a mass of 24.99 amu and a relative abundance of
10.13%. The other two isotopes have masses of 23.99 amu (24Mg) and 25.98 amu (26Mg). What are their relative
abundances? (atomic mass Mg = 24.305 amu)
10. An element “X” has 5 major isotopes, listed below along with their abundances. What is the element? Does the atomic mass
that you calculate based on these data agree with that listed in your periodic table?
Section 3.3
11. How many moles are in a sample of 300 atoms of nitrogen? How many grams?
12. How many atoms of gold does it take to make 1 gram of gold?
13. How many atoms of yttrium does it take to make 5.00 × 10-22 moles of yttrium?
14. An atom of sodium has a mass that is about ¼ the mass of an atom of yttrium. How would the number of atoms change if
we wanted 5.00 × 10-22 moles of sodium instead of yttrium, as in the previous problem?
15. If you buy 38.9 moles of M&M's®, how many M&M's® do you have? (1 mole of M&M's® = 6.022 x 1023 M&M's®)
16. A sample of sulfur has a mass of 5.37 g. How many moles are in the sample? How many atoms?
17. Give the number of moles of each element present in 1.0 mole of each of the following substances:
a. Hg2I2
c. PbCO3
e. RbOH·2H2O
b. LiH
d. Ba3(AsO4)2
f. H2SiF6
22
18. How many grams of zinc are in 1.16 x 10 atoms of zinc?
19. How many amu are in 3.68 moles of iron?
Section 3.4
20. Calculate the molar masses of each of the following:
a. Cu2SO4
c. C10H16O
e. Ca2Fe(CN)6·12H2O
b. NH4OH
d. Zr(SeO3)2
f. Cr4(P2O7)3
21. Calculate the molar mass of
a. Zn(CN)4
b. Cu(NH3)4•8H2O
22. What is the mass of 4.28 x 1022 molecules of water?
23. What is the mass of 4.89 x 1023 atoms of the element “X” described in problem # 10?
24. How many milligrams of Br2 are in 4.8 x 1020 molecules of Br2?
25. How many sodium ions are present in each of the following:
a. 2 moles of sodium phosphate
b. 5.8 grams of sodium chloride
c. a mixture containing 14.2 grams of sodium sulfate and 2.9 grams of sodium chloride?
26. How many potassium ions are present in each of the following:
a. 3 moles of potassium chloride
b. 6.2 grams of potassium nitrate
c. a mixture containing 12.6 grams of potassium phosphate and 5.4 grams of potassium chloride?
27. What is the weight in grams of
a. 0.4 moles of CH4
b. 11 moles of SO4-2
c. 5 moles of Mg(OH)2?
28. Determine the molar mass of KAl(SO4)2·12H2O.
29. How many moles of cadmium bromide, CdBr2, are in a 39.25 g sample?
30. A sample of calcium chloride, CaCl2, has a mass of 23.8 g. How many moles of calcium chloride is this?
31. If 0.172 moles of baking soda, NaHCO3, were used to bake a chocolate cherry cake, how many grams of baking soda would
the recipe call for?
32. How many moles are there in a sample of barium sulfate, BaSO4, weighing 9.90 x 10-7 g?
33. How many grams are there in 0.36 moles of cobalt (III) acetate, Co(C2H3O2)3? How many grams of cobalt are in this
sample? How many atoms of cobalt?
34. How many milligrams of chlorine are there in a sample of 3.9 x 1019 molecules of chlorine gas, Cl2? How many atoms of
chlorine?
35. Bauxite, the principle ore used in the production of aluminum cans, has a molecular formula of Al2O3•2H2O.
a. Determine the molar mass of bauxite.
b. How many grams of Al are in 0.58 moles of bauxite?
c. How many atoms of Al are in 0.58 moles of bauxite?
d. What is the mass in grams of 2.1 x 1024 formula units of bauxite?
Section 3.6
36. Calculate the mass percent of Cl in each of the following compounds:
a. ClF
b. CuCl2
c. HClO2
d. PuOCl
37. Calculate the mass percent of each element in C5H10O.
38. Calculate the mass percent of each element in potassium ferricyanide, K3Fe(CN)6.
39. Calculate the mass percent of each element in barium sulfite, BaSO3.
40. Calculate the mass percent of each element in natural lucite, KAlSi2O6.
41. Calculate the mass percent of silver in each of the following compounds:
a. AgCl
b. AgCN
c. AgNO3
42. Chlorophyll a is essential for photosynthesis. It contains 2.72% magnesium by mass. What is the molar mass of chlorophyll
a assuming there is one atom of magnesium in every molecule of chlorophyll a?
43. Calculate the mass percent of each of the elements in Nicotine, C10H14N2.
Section 3.7
44. Which of the following formulas can be empirical?
a. CH4
d. N2O5
g. Sb2S3
b. CH2
e. B2H6
h. N2O4
c. KMnO4
f. NH4Cl
i. CH2O
45. Determine the empirical and molecular formulas of a compound that has a mass of 31.04 g/mole and contains the following
percentages of elements by mass: C = 38.66%, H = 16.24%, N = 45.10%
46. The analysis of a rocket fuel showed that it contained 87.4% nitrogen and 12.6% hydrogen by weight. Mass spectral
analysis showed the fuel to have a molar mass of 32.05 grams. What are the empirical and molecular formulas of the fuel?
47. A compound is found, by mass spectral analysis, to contain the following percentages of elements by mass: M= 289.9
g/mole C = 49.67%, Cl = 48.92%, H = 1.39% Determine the empirical and molecular formula of the compound.
48. Vanillin, the pleasant smelling ingredient used to bake chocolate chip cookies, is often used in the production of vanilla
extract. Vanillin has a mass of 152.08 g/mole and contains the following percentages of elements by mass: C = 63.18%, H
= 5.26%, O = 31.56%
Determine the empirical and molecular formula of vanillin.
49. Determine the empirical formula of a compound that contains the following percentages of elements by mass:
Mo = 43.95%, O = 7.33%, Cl = 48.72%
50. A molecule with a molecular weight of approximately 110 g/mole is analyzed. The results show that it contains 10.05% of
carbon, 0.84% of hydrogen, and 89.10% of chloride. Calculate the molecular formula of this compound.
51. Using the data provided, calculate the empirical formulas for the compounds indicated:
a. an oxide of nitrogen, a sample of which contains 6.35 g of nitrogen and 3.65 g of oxygen
b. an oxide of copper, one gram of which contains 0.7989 g of copper
c. an oxide of carbon that contains 42.84% carbon
d. a compound of potassium, chloride, and oxygen containing K = 31.97%, O = 39.34%
e. a compound of hydrogen, carbon, and nitrogen containing H = 3.70%, C = 44.44%, and N = 51.85%.
Section 3.8
52. How many grams of product are formed in each of the following reactions?
a. Two moles of H2 react with one mole of O2.
b. One mole of silver nitrate reacts with one mole of sodium chloride.
c. Three moles of sodium hydroxide react with one mole of phosphoric acid.
53. How many moles of hydrogen can react with 8.30 moles of nitrogen? How many grams of ammonia, NH3, will be formed?
3H2 + N2 → 2NH3
54. What mass of hydrogen is required to produce 652 grams of ammonia? 3H2 + N2 → 2NH3
55. The following reaction was performed: Fe2O3(s) + 2X(s) → 2Fe(s) + X2O3(s)
It was found that 79.847 g of Fe2O3 reacted with "X" to form 55.847 g of Fe and 50.982 g of X2O3. Identify element X.
56. Do these equations follow the conservation of matter?
1. Na2SiO3 + 6HF → SiF4 + 2NaF + 3H2O
2. 3N2O4 + 2H2O → 4HNO3 + 2NO2
Section 3.9
57. Balance the following chemical equations:
a. AgI + Na2S → Ag2S + NaI
b. (NH4)2Cr2O7 → Cr2O3 + N2 + H2O
c. Na3PO4 + HCl → NaCl + H3PO4
d. TiCl4 + H2O → TiO2 + HCl
e. Ba3N2 + H2O → Ba(OH)2 + NH3
f. HNO2 → HNO3 + NO + H2O
58. Balance the following equation:
__NH4OH(l) + __KAl(SO4)2·12H2O → __Al(OH)3(s) + __(NH4)2SO4(aq) + __KOH(aq) + __H2O(l)
59. Balance the following equation:
___Fe(s) + ___HC2H3O2(aq) → ___Fe(C2H3O2)3(aq) + ___H2(g)
60. Complete the following reactions (making sure they are balanced):
a. HNO3 + _____ → H2O + KNO3
b. ______ + Na3PO4 → Ca3(PO4)2 + NaCl
c. Mg(OH)2 + HCl → MgCl2 + ______
d. _______ + Cl2 → NaCl + Br2
61. Balance the following equations:
a. Ca + C + O2 → CaCO3
b. FeS + O2 → Fe2O3 + SO2
c. HNO2 → NO2 + H2O + NO
d. PCl5 + H2O → H3PO4 + HCl
Section 3.10
62. How many grams of water vapor can be generated from the combustion of 18.74 g of ethanol?
C2H6O(g) + O2(g) → CO2(g) + H2O(g) (unbalanced)
63. How many grams of sodium hydroxide are required to form 51.63 g of lead hydroxide?
Pb(NO3)2(aq) + NaOH(aq) → Pb(OH)2(s) + NaNO3(aq) (unbalanced)
64. How many grams of potassium iodide are necessary to completely react with 20.61 g of mercury (II) chloride?
HgCl2(aq) + KI(aq) → HgI2 + KCl(aq) (unbalanced)
65. How many grams of oxygen are necessary to completely react with 22.8 grams of methane, CH4? (combustion) (Please
write the entire reaction.)
66. If, in the previous problem, only 25.9 grams of water vapor were formed, how much methane actually reacted with oxygen?
67. What mass of calcium carbonate (CaCO3) would be formed if 248.6 g of carbon dioxide (CO2) were exhaled into limewater,
Ca(OH)2? How many grams of calcium would be needed to form that amount of calcium carbonate? Assume 100% yield
in each reaction.
68. The following reaction is used to form lead iodide crystals. What mass of crystal (PbI2) could be formed from 1.0 x 103 g of
lead (II) acetate [Pb(C2H3O2)2]?
Pb(C2H3O2)2(aq) + 2KI(aq) → PbI2(s) + 2KC2H3O2(aq)
69. How many grams of precipitate (Hg2Cl2) would be formed from a solution containing 102.9 g of mercury ions that are
reacted with chloride ions as follows?
2Hg+(aq) + 2Cl-(aq) → Hg2Cl2(s)
70. You were hired by a laboratory to recycle 6 moles of silver ions. You were given 150 g of copper. How many grams of
silver can you recover? Is this enough copper to recycle 6 moles of silver ions? 2Ag+ + Cu → 2Ag + Cu+2
71. Fermentation converts sugar into ethanol and carbon dioxide. If you were to ferment a bushel of apples containing 235 g of
sugar, what is the maximum amount of ethanol in grams that would be produced? C6H12O6 → 2C2H6O + 2CO2
72. The reaction between potassium chlorate and red phosphorus is highly exothermic and takes place when you strike a match
on a matchbox. If you were to react 52.9 g of potassium chlorate (KClO3) with red phosphorus, how many grams of
tetraphosphorus decaoxide (P4O10) would be produced?
KClO3(s) + P4(s) → P4O10(s) + KCl(s) (unbalanced)