AP Chemistry
Ch.1 – Matter and Measurement
Name:
Date:
Period:
STUDY QUESTIONS and PROBLEMS
1.
2.
4.
Identify the following changes as physical or chemical changes:
a.
Baking soda reacts with vinegar to produce carbon dioxide.
b.
The copper sheath on the Statue of Liberty turns green.
c.
Addition of salt melts ice on the highway.
d.
Steam condenses on the windowpane.
e.
Epoxy resin cures and hardens.
f.
Sugar dissolves in a cup of coffee.
g.
Natural gas burns in a furnace.
a.
Calculate the density of lead if a 10. kg block has a volume of 885 cm3.
b.
What is the volume of a 100. g bar of aluminum if its density is 2.70 g·cm-3?
c.
Calculate the mass of 100. cm3 of uranium (density 19.07 g·cm-3).
Convert:
a.
6.
7.
Which of the following physical properties are extensive?
a.
heat of fusion
d. viscosity
b.
melting point
e. conductivity
c.
color
f.
N
b. Ca
c.
K
d.
P
e.
V
Write the symbols for the following elements:
a. silicon
9.
density
Write the names of the following elements:
a.
8.
25C to K
b. chlorine
c. iron
d. sodium
e. silver
f. sulfur
Convert:
a.
1342 mL into L
b.
3.26 x 10-6 km into mm
c.
8,768 mg into g
d.
400 cm3 into m3
e.
3600 sq. in. into sq. ft.
10. Write the following numbers in scientific notation with the correct number of significant figures:
a.
1,327
b. 0.00562
c. 2.76
d. 0.166
e. 0.09911
11. Measurements of the boiling point of a liquid were taken by two laboratory technicians (A and B). The
actual boiling point was 92.3. Which technician achieved the most accurate result and which technician
was the most precise?
A:
92.0
92.1
92.4
92.2
B:
91.9
92.5
92.6
92.0
12. Match the prefix with the correct multiplier:
milli
mega
kilo
micro
centi
pico
10-6
103
10-2
106
10-12
10-3
13. Evaluate the following expressions. Express the answers in scientific notation with the correct number of
significant figures and the correct units.
a.
0.0045 in + 1.0098 in + 0.987 in + 23.08 in
b.
(3.45 cm3 x 2.70 g·cm-3) + (7.433 cm3 x 1.677 g·cm-3)
c.
2.703 g/(1.376 cm x 2.45 cm x 3.78 cm)
14. A 12.3 g block of an unknown metal is immersed in water in a graduated cylinder. The level of water in
the cylinder rose. The level of water in the cylinder rose exactly the same distance when 17.4 grams of
aluminum (density 2.70 g·cm-3) was added to the same cylinder. What is the unknown metal’s density?
15. If one pound is 453.59 grams, how many grams are there in one ounce? How many ounces are there in
one kilogram?
16. A sample of gold alloy contains 5.6% silver by mass. How many grams of silver are there in 1 kilogram of
the alloy?
AP Chemistry
Ch.2 – The Nuclear Atom
Name:
Date:
Period:
ALL of the answers to this worksheet can be logically figured out by looking at the Schematic Diagrams for
Various Atoms , the Periodic Table, and discussing with your partners. All of the information you need is
here somewhere. Determine each answer and be able to give convincing reasons for each answer. Good
luck.
1.
How many protons are found in
12
13
13
2.
How many neutrons are found in
12
13
13
3.
How many electrons are found in
12
13
13
4.
Based on the model,
a)
what do all carbon atoms (and ions) have in common?
b)
C?
C-1?
C?
C?
C-1?
C?
C?
C-1?
C?
what do all hydrogen atoms (and ions) have in common?
5.
What is the significance of the atomic number, Z, above each atomic symbol in the periodic chart?
6.
What do all nickel (Ni) atoms have in common?
7.
How is the mass number, A, (left-hand superscript next to the atomic symbol) determined?
8.
What structural feature is different in isotopes of a particular element?
9.
a)
What feature distinguishes a neutral atom from an ion?
b)
How is the charge on an ion determined?
10.
Where is most of the mass of an atom, within the nucleus or outside of the nucleus?
Explain your reasoning.
11.
Complete the following table:
Isotope
31
P
Atomic
Number
Z
Mass
Number
A
15
18
O
8
19
58
Ni2+
Number of
electrons
39
58
18
AP Chemistry
Ch.2 – Isotopes
Name:
Date:
Period:
Answer the following questions on a separate piece of paper. Show your work when necessary.
1. Give the mass number of each of the following atoms:
(a) an iron atom with 30 neutrons
(b) an americium atom with 148 neutrons
(c) a tungsten atom with 110 neutrons
2. Give the complete symbol ( AZ X ) for each of the following atoms:
(a) nitrogen with 8 neutrons
(b) zinc with 34 neutrons
(c) xenon with 75 neutrons
3. How many electrons, protons, and neutrons are there in an atom of:
(a) carbon-13, 13 C
(b) copper-63, 63 Cu
(c) bismuth-205, 205 Bi
4. Fill in the blanks in the table (one column per element).
65
86
Symbol
Cu
Kr
Number of protons
Number of neutrons
Number of electrons
in the neutral atom
Name of element
78
117
46
36
5. Radioactive americium-241 is used in household smoke detectors and in bone mineral analysis. Give
the number of electrons, protons, and neutrons in an atom of americium-241.
6. Which of the following are isotopes of element X, with atomic number of 9:
19
9
X , 209 X , 189 X , and
21
9
X.
7. Verify that the atomic mass of magnesium is 24.31 amu, given the following information:
24
Mg , mass = 23.985042 amu; percent abundance = 78.99%
25
Mg , mass = 24.985837 amu; percent abundance = 10.00%
26
Mg , mass = 25.982593 amu; percent abundance = 11.01%
8. Copper has two stable isotopes, 63 Cu and
65
Cu , with masses of 62.939598 amu and 64.927793 amu,
respectively. Calculate the percent abundances of these isotopes of copper.
9. Strontium has four stable isotopes, Strontium-84 has a very low natural abundance, but
88
86
Sr , 87 Sr , and
Sr are all reasonably abundant. Which of these more abundant isotopes predominates?
AP Chemistry
Ch.2 – Study Questions
Name:
Date:
Period:
“The one quality which sets one man apart from another — the key which lifts one to every aspiration while others are
caught up in the mire of mediocrity — is not talent, formal education, nor brightness — it is self-discipline. With selfdiscipline, all things are possible. Without it, even the simplest goal can seem like the impossible dream.” Theodore
Roosevelt (1858-1919)
1.
a)
b)
c)
2.
3.
Explain, at an atomic or molecular level, what happens when
water freezes to form ice
copper and tin combine to form bronze
rainwater evaporates from the pavement
Which of the following atoms are isotopes of the same element? Identify the elements of these
isotopes and describe the number of protons and neutrons in the nucleus of them all.
15
12
13
18
14
14
16
13
17
7 X
6 X
7 X
8 X
7 X
6 X
8 X
6 X
8 X
There are three naturally occurring isotopes of neon:
neon-20 mass 19.9924 amu
neon-21 mass 20.9940 amu
neon-22 mass 21.9914 amu
abundance 90.84%
abundance 0.260%
abundance 8.90%
a) Without calculation, what is the approximate atomic mass of neon?
b) Calculate the actual atomic mass.
4.
Uranium has an atomic mass equal to 238.0289. It consists of two isotopes: uranium-235 with an
isotopic mass of 235.044 amu and uranium-238 with an isotopic mass of 238.051. Calculate the %
abundance of the uranium-235 isotope.
5.
From amongst the elements sodium, chlorine, nickel, argon, calcium, uranium, and oxygen, select the
alkali metal, the alkaline earth metal, the transition metal, the actinide, the halogen, the noble gas,
and the chalcogen (Group 6A).
6.
To illustrate Robert Millikan’s determination of the charge on an electron, suppose that you were
given the task of determining the mass of a single jelly bean given the following experimental data:
Various scoops of jelly beans were weighed and the following masses determined. The number of jelly
beans in each scoop was not known.
Masses (in grams) of ten different scoops:
4.96
8.68
13.64
7.44
21.08
16.12
9.92
19.84
6.20
12.40
7.
Reorder this list to match the name of the scientist with his or her contribution to our understanding of
the nature of matter:
J.J. Thompson
_______________
developed the idea of the atomic nature of matter
James Chadwick
_______________
established the law of conservation of matter
Robert Millikan
_______________
characterized positive and negative electrical charges
Henry Moseley
_______________
suggested that atoms could disintegrate
Michael Faraday
_______________
experimented with electrolysis
Dmitri Mendeleev
_______________
proved the existence of the electron
John Dalton
_______________
developed the idea of a nuclear atom
Henri Becquerel
_______________
discovered the neutron
Democritus
_______________
developed the first periodic table of elements
Joseph Proust
_______________
showed that periodicity depended upon atomic number
Antoine Lavoisier
_______________
formulated the laws of constant composition
Ernest Rutherford
_______________
determined the charge on a single electron
Marie Curie
_______________
revived the atomic theory
Benjamin Franklin
_______________
discovered radioactivity
8.
Identify the following elements:
a) The most abundant metal in the earth’s crust
b) Combined with chlorine, it produces a compound essential to life.
c) A metal that occurs in vast limestone deposits and combines with oxygen to form an oxide with a
formula MO.
d) The transition element at the center of hemoglobin.
e) Used in smoke detectors and named for the United States.
f)
A component of washing powder mined in Death Valley.
g) The basis for the compounds that make up all living things.
h) Primary constituent of pencil lead.
i)
The last element in the Periodic Table that is not radioactive.
j)
Exists as X4 molecules.
k) The element named after the sun, where it was first detected.
AP Chemistry
40 Ions to Memorize
aluminum
Al3+
strontium
Sr2+
ammonium
NH4+
stannous
Sn2+
barium
Ba2+
stannic
Sn4+
calcium
Ca2+
zinc
Zn2+
cuprous
Cu+
acetate
C2H3O2 or CH3COO
cupric
Cu2+
bromide
Br
ferrous
Fe2+
carbonate
CO32
ferric
Fe3+
chlorate
ClO3
hydrogen
H+
chloride
Cl
hydronium
H3O+
chromate
CrO42
lead
Pb2+
dichromate
Cr2O72
lithium
Li+
fluoride
F
magnesium
Mg2+
hydroxide
OH
manganese
Mn2+
iodide
I
mercurous
Hg22+
nitrate
NO3
mercuric
Hg2+
oxide
O2
nickel
Ni2+
permanganate
MnO4
potassium
K+
phosphate
PO43
silver
Ag+
sulfate
SO42
sodium
Na+
sulfide
S2
P Chemistry
Ch.2 - Organize Your Ions
Name:
Date:
I
Period:
VIII
H
II
III
Li
V
VI
VII
O
F
S
Cl
Na
Mg
K
Ca
Br
Sr
I
Ba
Al
IV
2- ions
1+ ions
3- ions
“ates”
2+ ions
Elements with two different ion names / charges
3+ ions
4+ ions
1- ions
AP Chemistry
Name:
Ch.2 – Writing Formulas and Naming Compounds
Introduction
Writing formulas and naming compounds can be confusing because there are different types of compounds
that follow different rules. Additionally, some compounds (H2O, NH3, CH4, etc.) simply have common names
that must be memorized.
The two types of compounds we will focus on first are ionic compounds (formed from positive and negative
ions) and binary nonmetal compounds (molecular compounds). Later we will add acids. So… you must
recognize the type of compound before you try to name it. [Note: + ion = “cation” and – ion = “anion”.]
Ionic
+ ion before – ion
Formula
ex: NaCl (NH4)2SO4 Al2S3
Name of cation + name of anion
Naming
I.
sodium chloride
ammonium sulfate
aluminum sulfide
Binary Nonmetal
usually the less electronegative atom is first
ex: CO
CO2
N2O
Indicate the number (mono, di, tri, and kind of atoms.
First element is simply name of element. Second
element name ends with “ide”
carbon monoxide
carbon dioxide
dinitrogen monoxide
Writing Ionic Formulas
Cl-
NO3-
S2-
CO32-
N3-
PO43-
Na+
NH4+
Sn2+
Hg22+
Al3+
Sn4+
II.
Naming Ionic Compounds
Cation
Anion
Cu2+
OH-
Ba2+
SO42-
NH4+
Cr2O72-
Ag+
C2H3O2-
Fe3+
S2-
Formula
Name
OH-
mono
III.
di
tri
tetra
hexa
hepta
octa
nona
deca
Writing Formulas of Binary Nonmetal Compounds
Name
IV.
Formula
Name
Formula
nitrogen trifluoride
phosphorus trichloride
nitrogen monoxide
phosphorus pentachloride
nitrogen dioxide
sulfur hexafluoride
dinitrogen tetroxide
disulfur decafluoride
dinitrogen monoxide
xenon tetrafluoride
Naming Binary Nonmetal Compounds
Name
V.
penta
Formula
Name
Formula
CCl4
HBr
P4O10
N2F4
ClF3
XeF3
BCl3
PI3
SF4
SCl2
Practice for Both Types of Compounds
Formula
Name
Formula
Name
HCl
carbon dioxide
PCl5
ammonium carbonate
K2S
sulfur dichloride
NiSO4
calcium iodide
ClF3
boron trifluoride
OF2
phosphorus triiodide
Al(OH)3
magnesium perchlorate
NCl3
potassium permanganate
(NH4)3PO4
aluminum phosphate
S2Cl2
dioxygen difluoride
AP Chemistry
Ch. 2 – Study Questions
Name:
Date:
You will need to answer the questions below on a separate piece of paper. Show your work whenever
necessary – remember to include units in your answers when required.
1.
a. The structural formula for acetic acid is CH3CO2H. What is its empirical formula; what is its molecular
formula?
b. The molecular formula of acrylonitrile is C3H3N. Look up in the text, and draw, its structural formula.
c. The molecular formula of aspartame (nutrasweet) is C14H18O5N2. Look up in the text, and draw, its
structural formula.
2.
The formulas for ethanol and ammonium nitrate are C2H5OH and NH4NO3. In what respects are these
formulas and compounds different?
3.
The molecular formula for both butanol and diethylether is C4H10O. Write structural formulas for both and
show how they are different. Are any other structures possible?
4.
Name the polyatomic ions:
CH3CO2H2PO4SO32-
5.
What are the formulas of the polyatomic ions:
phosphate
sulfate
bisulfite
HCO3Cr2O72ClO4-
nitrite
cyanide
chlorite
6.
Write the ions present in the following salts and predict their formulas:
potassium bromide
calcium carbonate
magnesium iodide
lithium oxide
aluminum sulfate
ammonium chlorate
beryllium phosphate
7.
Name the following ionic salts:
(NH4)2SO4
KHCO3
Ca(NO3)2
8.
9.
Co2(SO4)3
NiSO4
AlPO4
Name the following binary compounds of the nonmetals:
CS2
SiCl4
SF6
GeH4
IF5
P4O10
N2H4
S4N4
PCl5
OF2
Cl2O7
IF7
What are the formulas for the following binary compounds?
silicon dioxide
phosphine
boron trifluoride
silicon carbide
xenon tetroxide
phosphorus tribromide
dinitrogen pentoxide
disulfur dichloride
bromine trifluroide
hydrogen selenide
carbon tetrachloride
10.
a.
b.
c.
d.
e.
f.
g.
h.
i.
How many moles are present in 128 grams of sulfur dioxide?
What is the mass of 3 moles of oxygen molecules?
If 5 moles of a metallic element have a mass of 200 grams, which element is it?
What is the molar mass of methane CH4?
What is the mass of 9 moles of fluorine molecules?
102 grams of a gas contains 6 moles. What is its molar mass?
How many grams are there in one mole of benzene C6H6?
How many moles of nitrogen atoms are there in 6 moles of TNT (trinitrotoluene CH3C6H2(NO2)3)?
What is the molar mass of TNT?
11.
What is the percent by mass of nitrogen in ammonium nitrate?
12.
The hydrocarbons ethylene (molar mass 28 g/mol), cyclobutane (molar mass 56 g/mol), pentene (molar
mass 70 g/mol), and cyclohexane (molar mass 84 g/mol), all have the same empirical formula. What is it?
Write the molecular formulas for these four compounds.
13.
A compound was analyzed and found to contain 76.57% carbon, 6.43% hydrogen, and 17.00% oxygen
by mass. Calculate the empirical formula of the compound. If the molar mass of the compound is
94.11g/mol, what is the molecular formula of the compound?
14.
A compound was analyzed and found to contain 53.30% carbon, 11.19% hydrogen, and 35.51% oxygen
by mass. Calculate the empirical formula of the compound. If the molar mass of the compound is 90.12
g/mol, what is the molecular formula of the compound?
15.
A 15.67 g sample of a hydrate of magnesium carbonate was carefully heated, without decomposing the
carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
16.
Anhydrous lithium perchlorate (4.78 g) was dissolved in water and re-crystallized. Care was taken to
isolate all the lithium perchlorate as its hydrate. The mass of the hydrated salt obtained was 7.21 g. What
hydrate is it?
AP Chemistry
Name:
Ch.3 - Molar Mass & Percent Composition Date:
Period:
I. Molar Masses
Given a periodic table, you should be able to calculate the molecular mass (in u’s) or the molar mass
(in grams) for any element or compound.
Examples: (give answers to two decimal places)
H2SO4
Cl2
CO2
N2O
Ca(OH)2
HC2H3O2
NaOCl
Al2S3
II. Fraction and Percent Composition
It is useful to determine how much of a compound’s mass is made up of each element. Water, H 2O,
for example has a molar mass of 18.02 g. The H’s mass is 2(1.0079) = 2.02 g. The O’s mass is
16.00 g.
We can set up fractions for each element:
H=
2.02
= 0.112 = 11.2%.
18.02
O=
16.00
= 0.888 = 88.8%.
18.02
This is called the percent composition. The fraction composition is a good in-between step.
Determine the fraction and percent composition of each element below (answer to one decimal
place):
1. H2SO4
2. Ca(OH)2
3. HC2H3O2
4. CO2
5. N2O
6. NaOCl
7. Al2S3
AP Chemistry
Mole Calculations - Difficulty Level 1
Name:
Date:
Period:
1 mole = 6.02 x 1023 molecules = 22.4 L (@ STP)
In each question, there is a “given” (G) and a “determine” (D). For each problem, I have outlined the
number of conversions necessary to solve for the determined. You need to fill in the blanks and solve
using dimensional analysis.
1.
Calculate the mass of 1.58 moles CH4. [molar mass CH4 = 16.0 g/mol]
G: 1.58 moles CH4
D: ? g CH4
1.58 moles CH4
=
2.
What volume will 7.29 moles of CO2 gas occupy at STP?
G: 7.29 moles CO2
D: ? L CO2
7.29 moles CO2
=
3.
How many molecules are there in a 0.00583 mole sample of H2O?
G: 0.00583 moles H2O
D: ? molecules H2O
0.00583 moles H2O
=
4.
What mass of CO2 gas occupies a volume of 100. Liters at STP? [molar mass CO2 = 44.0
g/mol]
G: 100. Liters CO2
D: ? g CO2
100. Liters CO2
=
5.
How many molecules are in a 35.0 gram sample of H2O? [molar mass H2O = 18.0 g/mol]
G: 35.0 g H2O
D: ? molecules H2O
35.0 g H2O
=
6.
What volume will 5.25 x 1022 molecules of CH4 occupy at STP?
G: 5.25 x 1022 molecules CH4
D: ? L
22
5.25 x 10 molecules CH4
=
AP Chemistry
Mole Calculations - Difficulty Level 2
Name:
Date:
Period:
1 mole = 6.02 x 1023 molecules = 22.4 L (@ STP)
In each question, there is a “given” (G) and a “determine” (D). For each problem, I have outlined the
number of conversions necessary to solve for the determined but you will need to decide what “G”
and “D” are, and then you need to fill in the blanks and solve using dimensional analysis.
1.
Calculate the mass of 2.19 moles CH4. [molar mass CH4 = 16.0 g/mol]
G:
D:
=
2.
What volume will 2.22 moles of CO2 gas occupy at STP?
G:
D:
=
3.
How many molecules are there in a 0.127 mole sample of H2O?
G:
D:
=
4.
What mass of CO2 gas occupies a volume of 395 Liters at STP? [molar mass CO2 = 44.0 g/mol]
G:
D:
=
5.
How many molecules are in a 0.250 gram sample of H2O? [molar mass H2O = 18.0 g/mol]
G:
D:
=
6.
What volume will 3.01 x 1022 molecules of CH4 occupy at STP?
G:
D:
=
AP Chemistry
Mole Calculations - Difficulty Level 3
Name:
Date:
Period:
1 mole = 6.02 x 1023 molecules = 22.4 L (@ STP)
In each question, there is a “given” (G) and a “determine” (D). For each problem, you will need to
decide what “G” and “D” are, and then you need to solve using dimensional analysis.
1.
Calculate the mass of 7.23 moles CH4. [molar mass CH4 = 16.0 g/mol]
G:
D:
2.
What volume will 9.35 moles of CO2 gas occupy at STP?
G:
D:
3.
How many molecules are there in a 0.0752 mole sample of H2O?
G:
D:
4.
What mass of CO2 gas occupies a volume of 10.8 Liters at STP? [molar mass CO2 = 44.0
g/mol]
G:
D:
5.
How many molecules are in a 1.44 gram sample of H2O? [molar mass H2O = 18.0 g/mol]
G:
D:
6.
What volume will 1.21 x 1024 molecules of CH4 occupy at STP?
G:
D:
AP Chemistry
Ch.3: Composition of Hydrates
Name:
Date:
Period:
1.
Cupric chloride, CuCl2, when heated to 100C is dehydrated. If 0.235 g of CuCl2 · x H2O gives 0.185 g of
CuCl2 on heating, what is the value of x?
2.
The “alum” used in cooking is potassium aluminum sulfate hydrate, KAl(SO4)2 · x H2O . To find the value
of x, you can heat a sample of the compound to drive off all of the water and leave only KAl(SO4)2.
Assume you heat 4.74 g of the hydrated compound and that the sample loses 2.16 g of water. What is
the value of x?
3.
If “Epsom salt,” MgSO4 · x H2O is heated to 250C, all the water of hydration is lost. On heating a 1.687-g
sample of the hydrate, 0.824 g of MgSO4 remains. What is the formula of Epsom salt?
4.
When CaSO4 · x H2O is heated, all of the water is driven off. If 34.0 g of CaSO4 (molar mass = 136) is
formed from 43.0 g of CaSO4 · x H2O, what is the value of x?
AP Chemistry
Name:
Ch. 3 – Chemical Equations & Stoichiometry
Date:
STUDY QUESTIONS AND PROBLEMS
1. Balance the following equations:
a.
__C4H6(g) + __O2(g)  __CO2(g) + __H2O(l)
3.
b.
__NH3(g) + __O2(g)  __NO2(g) + __H2O(l)
c.
__PCl3(l) + __H2O(l)  __H3PO3(aq) + __HCl(aq)
d.
__Ca3P2(s) + __H2O(l)  __Ca(OH)2(aq) + __PH3(g)
e.
__C4H8(OH)2(l) + __O2(g)  __CO2(g) + __H2O(l)
f.
__NH3(g) + __NO(g)  __N2(g) + __H2O(l)
g.
__KClO3(s)  __KCl(s) + __O2(g)
h.
__Ca(OH)2(s) + __H3PO4(aq)  __Ca3(PO4)2(s) + __H2O(l)
i.
__C3H8(g) + __O2(g)  __CO2(g) + __H2O(l)
j.
__N2O(g) + __O2(g)  __NO2(g)
k.
__Al4C3(s) + _H2O(l)  __Al(OH)3(aq) + __CH4(g)
l.
__CS2(l) + __Cl2(g)  __CCl4(l) + __S2Cl2(l)
m.
__C2H5OH(l) + __PCl3(l)  __C2H5Cl(l) + __H3PO3(l)
n.
__ZnS(s) + __O2(g)  __ZnO(s) + __SO2(g)
o.
__Ag(s) + __H2S(g) + __O2(g)  __Ag2S(s) + __H2O(l)
When asked to balance the equation:
C2H6(g) + O2(g)  CO2(g) + H2O(l)
the following suggestions were made:
C2H6(g) + 5O2(g)  2CO2(g) + 3H2O(l)
C2H6(g) + 5O(g)  2CO(g) + 3H2O(l)
2C2H6(g) + 7O2(g)  4CO2(g) + 6H2O(l)
Which answer is correct and what is wrong with the others?
4.
Write balanced chemical equations for the following reactions:
a. the decomposition of ammonium nitrate to nitrogen gas, oxygen gas, and water vapor.
b. the reaction of sodium bicarbonate with sulfuric acid to produce sodium sulfate, water, and carbon
dioxide.
c. the treatment of phosphorus pentachloride with water to produce phosphoric acid and hydrogen
chloride.
5.
If the maximum amount of product possible is formed in the following reactions, what mass of the
specified product would you obtain?
a.
10 grams of sodium chloride is treated with excess silver nitrate:
AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)
How much silver chloride is precipitated?
b.
12 grams copper metal is treated with excess dilute nitric acid:
3Cu(s) + 8HNO3(aq)  3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l)
How much nitric oxide gas (NO) is produced?
c.
60 grams propane gas is burned in excess oxygen:
C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(l)
How much water is produced?
6.
A furniture dealer put together a special deal for the annual sale—an entire dining room set comprising a
table, six dining chairs, two bookshelves, a china cabinet, and a sideboard for $999. The dealer had in
stock 280 tables, 1750 chairs, 550 bookshelves, 300 china cabinets, and 325 sideboards. He asked his
assistant to figure out how many dining room sets they could sell, how much money they would make if
they sold all the sets possible, and what they would have left that could not be sold as part of the deal.
7.
Hydrazine reacts with dinitrogen tetroxide according to the equation:
2N2H4(g) + N2O4(g)  3N2(g) + 4H2O(g)
50.0 grams of hydrazine is mixed with 100.0 grams of dinitrogen tetroxide. How much nitrogen gas was
produced?
9.
7.321 mg of an organic compound containing carbon, hydrogen, and oxygen was analyzed by
combustion. The amount of carbon dioxide produced was 17.873 mg and the amount of water produced
was 7.316 mg. Determine the empirical formula of the compound.
10. 0.1101 gram of an organic compound containing carbon, hydrogen, and oxygen was analyzed by
combustion. The amount of carbon dioxide produced was 0.2503 gram and the amount of water
produced was 0.1025 gram. A determination of the molar mass of the compound indicated a value of
approximately 115 grams/mol. Determine the empirical formula and the molecular formula of the
compound.
13. Sodium metal reacts vigorously with water to produce a solution of sodium hydroxide and hydrogen gas:
2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
What mass of hydrogen gas can be produced when 10 grams of sodium is added to 15 grams of water?
14. Nitrous oxide reacts with oxygen to produce nitrogen dioxide according to the equation:
2N2O(g) + 3O2(g)  4NO2(g)
What mass of nitrogen dioxide can be made from 42 grams of nitrous oxide and 42 grams of oxygen?
15. If only 75 grams of nitrogen dioxide was produced in the reaction described in the previous question, what
was the % yield?