Chapter 11 Railroad Tracks
1. How many atoms are in 15.6 moles of carbon?
=
2. How many moles are 2.4 x 1025 atoms of carbon?
=
3. How many grams are 3.2 moles of nitrogen?
=
4. How many moles are 198 grams of nitrogen?
=
5. How many atoms are 160 grams of calcium?
=
6. How many grams are 3.20 x 1024 atoms of calcium?
=
Name
Date
CHAPTER
11
Class
CHAPTER ASSESSMENT
Understanding Main Ideas (Part A)
Circle the letter of the choice that best completes the statement or answers the question.
1. A mole of potassium chloride (KCl) contains 6.02 1023
a. atoms KCl.
b. formula units KCl.
c. ions KCl.
d. molecules KCl.
c. mole.
d. mole/gram.
2. The SI unit of molar mass is the
a. gram.
b. gram/mole.
3. Which conversion factor would you use to calculate correctly the mass of 2 moles of the
element titanium?
1 g Ti
47.88 mol Ti
a. 1 mol Ti
47.88 g Ti
b. 47.88 mol Ti
1 g Ti
c. 4. How many moles of oxygen atoms do 1.5 moles of CO2 contain?
a. 1 mol
b. 1.5 mol
c. 2 mol
47.88 g Ti
1 mol Ti
d. d. 3 mol
5. Which compound has the smallest molar mass?
a. CO
b. CO2
c. H2O
d. H2O2
6. One mole of silicon (Si) has a mass of 28.086 g, and one mole of carbon has a mass of
12.011 g. What is the mass of one mole of silicon carbide (SiC)?
b. 16.075 g
c. 40.097 g
d. 3.3734 102 g
7. Methane (CH4) contains 75% carbon. What percentage of methane is hydrogen?
a. 4%
b. 6%
c. 25%
d. 33%
8. The mole ratio of the elements in a compound’s molecular formula is
a. a multiple of the mole ratio of the elements in its empirical formula.
b. less than the mole ratio of the elements in its empirical formula.
c. not related to the mole ratio of the elements in its empirical formula.
d. the same as the mole ratio of the elements in its empirical formula.
9. Sodium bromide dihydrate is correctly written as
a. NaBrH2.
b. (NaBr)2H2O.
c. NaBr(HO)2.
d. NaBr2H2O.
c. mass.
d. temperature.
10. As a hydrated compound is heated, it decreases in
a. brightness.
62
b. color.
Chemistry: Matter and Change • Chapter 11
Chapter Assessment
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
a. 2.340 g
Name
Date
11
CHAPTER
Class
CHAPTER ASSESSMENT
Applying Scientific Methods
Each time Lisa visited a grocery store in the neighborhood, she noticed a small vial hanging
on the wall. The vial was filled with a compound that appeared blue at times and pink at other
times. One day she questioned the woman who ran the store about the vial. The woman said it
was part of an old weather gadget, but could not remember how it worked. Lisa asked if she
could borrow the vial to find out more about the compound.
In the following weeks, Lisa made daily observations of the contents, the temperature,
and the relative humidity (a measure of the amount of water vapor in the air). Her observations are summarized in the following table and graph.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Week 1
Week 2
Day
Compound color
Day
Compound color
Mon
Light blue
Mon
Pink
Tue
Light blue
Tue
Pink
Wed
Pink
Wed
Light blue
Thu
Pink
Thu
Light blue
Fri
Pink
Fri
Light blue
Sat
Pink
Sat
Light blue
Sun
Pink
Sun
Light blue
Graph 1
90
80
70
60
50
40
30
20
10
0
Daily Relative Humidity (%)
Daily High Temperature (°C)
Mon
Tue
Wed
Thu
Fri
Sat
Sun
Mon
Tue
Wed
Thu
Fri
Sat
Sun
1. What effect do temperature and relative humidity have on the color of the compound in
the vial?
2. What can you infer from Lisa’s observations about the type of compound that is in the
vial? Explain your reasoning.
Chapter Assessment
Chemistry: Matter and Change • Chapter 11
65
Name
Date
CHAPTER
Section 11.3
11
Class
STUDY GUIDE FOR CONTENT MASTERY
Moles of Compounds
In your textbook, read about chemical formulas and the mole, the molar mass of compounds, and conversions among mass, moles, and number of particles.
Study the table and the diagram of a methane molecule and a trichloromethane
molecule. Then answer the following questions.
Element
H
Molar Mass (g/mol)
Hydrogen
1.01
Carbon
12.01
Chlorine
35.45
H
H
Cl
C
C
Cl
H
H
Cl
CH4
CHCl3
1. What elements and how many atoms of each does a molecule of methane contain?
2. What elements and how many atoms of each does a molecule of trichloromethane
contain?
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
3. How many moles of each element are in a mole of methane?
4. How many moles of each element are in a mole of trichloromethane?
5. Which of the following values represents the number of carbon atoms in one mole of
methane? 6.02 1023; 12.0 1023; 18.1 1023; 24.1 1023
6. Which of the following values represents the number of chlorine atoms in one mole of
trichloromethane? 6.02 1023; 1.20 1024; 1.81 1024; 2.41 1023
7. Which of the following values represents the molar mass of methane? 13.02 g/mol;
16.05 g/mol; 52.08 g/mol; 119.37 g/mol
8. Chloromethane (CH3Cl) has a molar mass of 50.49 g/mol. Which of the following values
represents the number of molecules of CH3Cl in 101 grams of the substance?
3.01 1023; 6.02 1023; 1.20 1024; 6.08 1026
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 11
63
Name
Date
CHAPTER
Section 11.4
11
Class
STUDY GUIDE FOR CONTENT MASTERY
Empirical and Molecular Formulas
In your textbook, read about percent composition.
Answer the following questions.
1. What is the percent composition of a compound?
2. Describe how to find the percent composition of a compound if you know the mass of a
sample of a compound and the mass of each element in the sample.
In your textbook, read about empirical and molecular formulas.
Circle the letter of the choice that best answers the question.
3. Which information about a compound can you use to begin to determine the empirical
and molecular formulas of the compound?
a. mass of the compound
c. percent composition of the compound
b. number of elements in the compound
d. volume of the compound
0.600 moles of oxygen. What must you do to determine the mole ratio of the elements in
the empirical formula of the compound?
a. Multiply each mole value by 0.300 mol.
c. Divide each mole value by 0.300 mol.
b. Multiply each mole value by 0.600 mol.
d. Divide each mole value by 0.600 mol.
5. The mole ratio of carbon to hydrogen to oxygen in a compound is
1 mol C : 2 mol H : 1 mol O. What is the empirical formula of the compound?
a. CHO
b. CH2O
c. C2HO2
d. C2H2O2
6. You calculate the mole ratio of oxygen to aluminum in a compound to be
1.5 mol O : 1 mol Al. What should you do to determine the mole ratio in the
empirical formula of the compound?
a. Multiply each mole value by 1.5.
c. Divide each mole value by 1.5.
b. Multiply each mole value by 2.
d. Divide each mole value by 2.
7. What is the relationship between the molecular formula and the empirical formula of a
compound?
a. (molecular formula)(empirical formula) n
empirical formula
n
c. molecular formula (empirical formula)n
n
d. molecular formula empirical formula
b. molecular formula 64
Chemistry: Matter and Change • Chapter 11
Study Guide for Content Mastery
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
4. You have determined that a compound is composed of 0.300 moles of carbon and
Name
CHAPTER
Date
11
Class
STUDY GUIDE FOR CONTENT MASTERY
Section 11.4 continued
8. You know that the empirical formula of a compound has a molar mass of 30.0 g/mol. The
experimental molar mass of this compound is 60.0 g/mol. What must you do to determine the value of n in the relationship between the molecular formula and the empirical
formula?
a. Add 30.0 g/mol and 60.0 g/mol.
c. Divide 60.0 g/mol by 30.0 g/mol.
b. Divide 30.0 g/mol by 60.0 g/mol.
d. Multiply 30.0 g/mol by 60.0 g/mol.
9. You know that the experimental molar mass of a compound is three times the molar mass
of its empirical formula. If the compound’s empirical formula is NO2, what is its molecular formula?
a. NO2
b. NO6
c. N3O2
d. N3O6
Solve the following problem. Show your work in the space provided.
10. A sample of a compound contains 7.89 g potassium, 2.42 g carbon, and 9.69 g oxygen.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Determine the empirical and molecular formulas of this compound, which has a molar
mass of 198.22 g/mol.
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 11
65
CHAPTER
11
SUPPLEMENTAL PROBLEMS
The Mole
1. Identify and calculate the number of representa-
tive particles in each of the following quantities.
a. 2.15 moles of gold
b. 0.151 mole of nitrogen oxide
6. Which quantity has the greatest mass?
a. 4.16 1023 atoms of radium
b. 1.50 1020 atoms of cadmium
c. 1.33 1024 atoms of argon
c. 11.5 moles of potassium bromide
7. Calculate the number of moles in each of the
2. Calculate the number of moles of the substance
that contains the following number of representative particles.
a. 8.92 1023 atoms of barium
b. 5.50 1025 molecules of carbon monoxide
following quantities.
a. atoms of each element in 3.35 moles of
aspirin (C9H8O4)
b. positive and negative ions in 1.75 moles of
calcium fluoride (CaF2)
c. 2.66 1022 formula units of potassium
iodide
8. Determine the molar mass of each of the
following compounds.
3. Determine the mass in grams of each of the
following quantities.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
a. 1.24 moles of beryllium
b. 3.35 moles of calcium
c. 0.155 mole of sulfur
a. formic acid (CH2O2)
b. ammonium dichromate ((NH4)2Cr2O7)
9. What is the mass in grams of each of the
following quantities?
a. 2.53 moles of lead(II) nitrate (Pb(NO3)2)
4. Calculate the number of moles in each of the
b. 4.62 moles of magnesium bromide (MgBr2)
following quantities.
a. 6.35 g lithium
10. Calculate the number of moles in each of the
b. 346 g zinc
following samples.
c. 115 g nickel
a. 3.75 g calcium carbide (CaC2)
b. 245 g aluminum nitrite (Al(NO2)3)
5. How many atoms are in the following samples?
a. 1.24 g cobalt
11. Determine the percent composition of each of
the following compounds.
b. 0.575 g cesium
a. manganese oxide (MnO)
c. 65.6 g silicon
b. propanol (C3H8O)
c. calcium phosphate (Ca3(PO4)2)
Supplemental Problems
Chemistry: Matter and Change • Chapter 11
13
Name
Date
12
CHAPTER
Class
STUDY GUIDE FOR CONTENT MASTERY
Stoichiometry
Section 12.1
What is stoichiometry?
In your textbook, read about stoichiometry and the balanced equation.
For each statement below, write true or false.
1. The study of the quantitative relationships between the amounts of
reactants used and the amounts of products formed by a chemical reaction
is called stoichiometry.
2. Stoichiometry is based on the law of conservation of mass.
3. In any chemical reaction, the mass of the products is less than the mass of
the reactants.
4. The coefficients in a chemical equation represent not only the number of
individual particles but also the number of moles of particles.
5. The mass of each reactant and product is related to its coefficient in the
balanced chemical equation for the reaction by its molar mass.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Complete the table below, using information represented in the chemical equation for
the combustion of methanol, an alcohol.
methanol oxygen 0 carbon dioxide water
2CH3OH(l) 3O2 (g) 0 2CO2(g) 4H2O(g)
Substance
Molar Mass (g/mol)
6. Methanol
32.05
7. Oxygen gas
32.00
8. Carbon dioxide
44.01
9. Water
18.02
Number of
Molecules
Number of
Moles (mol)
Mass (g)
10. What are the reactants?
11. What are the products?
12. What is the total mass of the reactants?
13. What is the total mass of the products?
14. How do the total masses of the reactants and products compare?
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 12
67
Name
Date
CHAPTER
12
Class
CHALLENGE PROBLEMS
Mole Relationships in
Chemical Reactions
Use with Chapter 12,
Section 12.2
T
he mole provides a convenient way of finding the amounts of the substances in a chemical
reaction. The diagram below shows how this concept can be applied to the reaction
between carbon monoxide (CO) and oxygen (O2), shown in the following balanced equation.
2CO(g) O2(g) 0 2CO2(g)
Use the equation and the diagram to answer the following questions.
Moles of
CO
3
Particles of
CO
1
6
2
4
Grams of
CO
Moles of
CO2
5
7
Particles of
CO2
Grams of
CO2
1. What information is needed to make the types of conversions shown by double-arrow 1
in the diagram?
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
2. What conversion factors would be needed to make the conversions represented by
double-arrow 2 in the diagram for CO? By double-arrow 6 for CO2?
3. What information is needed to make the types of conversions represented by
double-arrows 3 and 7 in the diagram?
4. What conversion factors would be needed to make the conversions represented by
double-arrow 3 in the diagram for CO?
5. Why is it not possible to convert between the mass of a substance and the number of
representative particles, as represented by double-arrow 4 of the diagram?
6. Why is it not possible to use the mass of one substance in a chemical reaction to find the mass
of a second substance in the reaction, as represented by double-arrow 5 in the diagram?
12
Chemistry: Matter and Change • Chapter 12
Challenge Problems
Name
CHAPTER
Section 12.3
Date
12
Class
STUDY GUIDE FOR CONTENT MASTERY
Limiting Reactants
In your textbook, read about why reactions stop and how to determine the limiting
reactant.
Study the diagram showing a chemical reaction and the chemical equation that represents the reaction. Then complete the table. Show your calculations for questions 25–27
in the space below the table.
0
O2 2NO 0 2NO2
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
The molar masses of O2, NO, and NO2 are 32.00 g/mol, 30.01 g/mol, and 46.01 g/mol,
respectively.
Amount and Name
of Excess Reactant
Amount of O2
Amount of NO
1 molecule
2 molecules
2 molecules
none
none
4 molecules
4 molecules
4 molecules
NO
2 molecules O2
2 molecules
8 molecules
Amount of NO2
Limiting Reactant
1.
2.
3.
1.00 mol
2.00 mol
4.
5.
6.
4.00 mol
4.00 mol
7.
8.
9.
5.00 mol
7.00 mol
10.
11.
12.
1.00 mol
4.00 mol
13.
14.
15.
0.500 mol
0.200 mol
16.
17.
18.
32.00 g
60.02 g
19.
20.
21.
16.00 g
80.00 g
22.
23.
24.
10.00 g
20.00 g
25.
26.
27.
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 12
71
Name
Date
CHAPTER
Section 12.4
12
Class
STUDY GUIDE FOR CONTENT MASTERY
Percent Yield
In your textbook, read about the yields of products.
Study the diagram and the example problem.
mass of product from experimental
measurement
actual yield
percent yield 100%
theoretical yield
mass of product predicted from stoichiometric calculation using
a. mass of reactant
b. 4-step mass-to-mass conversion
1. Write the balanced chemical equation.
2. Calculate the number of moles of reactant, using
molar mass.
3. Calculate the number of moles of product, using
the appropriate mole ratio.
4. Calculate the mass of product, using the reciprocal
of molar mass.
4Ga(s) 3O2(g) 0 2Ga2O3(s)
In one experiment, the reaction yielded 7.42 g of the oxide from a 7.00-g sample of gallium.
Determine the percent yield of this reaction. The molar masses of Ga and Ga2O3 are
69.72 g/mol and 187.44 g/mol, respectively.
Use the information in the diagram and example problem to evaluate each value or
expression below. If the value or expression is correct, write correct. If it is incorrect,
write the correct value or expression.
1. actual yield: unknown
2. mass of reactant: 7.00 g Ga
69.72 g Ga
1 mol Ga
3. number of moles of reactant: 7.00 g Ga 2 mol Ga2O3
1 mol Ga
4. number of moles of product: 0.100 mol Ga 187.44 g Ga2O3
5. theoretical yield: 0.0500 mol Ga2O3 1 mol Ga O
2 3
6. percent yield:
72
9.37 g Ga2O3
7.42 g Ga2O3 100
Chemistry: Matter and Change • Chapter 12
Study Guide for Content Mastery
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Example Problem: The following chemical equation represents the production of gallium
oxide, a substance used in the manufacturing of some semiconductor devices.
CHAPTER 11
The Mole
Name:
1
Date:
How many moles of nitrogen atoms are contained in
one mole of Ba(NO3)2?
A
1
B
2
C
6
D
9
4
5
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
The molecular formula of a compound is X6Y3. What
is the empirical formula for this compound?
amu
B
mass
C
molecule
D
particle
What is the total number of atoms contained in 2.00
moles of helium?
A
15.999
A
X6Y
B
32.0
B
XY3
C
6.02 1023
C
X2Y
D
1.20 1024
D
XY2
This question covers TEKS 2C. This question tests
the material that was covered in the textbook on
page 311.
This question covers TEKS 2D and 11C. This
question tests the material that was covered in the
textbook on page 331.
6
3
A
This question covers TEKS 2D. This question tests
the material that was covered in the textbook on
page 313.
This question covers TEKS 11B and 11C. This
question tests the material that was covered in the
textbook on page 320.
2
Mole is to atom as gram is to —
Zinc is used as a coating on iron and steel to prevent
corrosion. What is the mass, in grams, of 0.0650
mol Zn?
A compound has the formula MgSO4•7H2O. Its
chemical name is —
A
aqueous magnesium sulfate
A
3.25 g
B
magnesium sulfate pentahydrate
B
3.90 g
C
magnesium sulfate heptahydrate
C
3.94 g
D
magnesium sulfate decahydrate
D
4.25 g
This question covers TEKS 2C and 10B. This
question tests the material that was covered in the
textbook on page 315.
Reviewing Chemistry: Mastering the TEKS
This question covers TEKS 11A. This question tests
the material that was covered in the textbook on
page 338.
Chemistry: Matter and Change
21
CHAPTER 11
The Mole, continued
Name:
7
Date:
Indium (In) is a relatively rare element
that never occurs as a free metal. It is
usually found in a compound that contains 70.48%
In and 29.52% S. What is the empirical formula for
this compound?
9
A
38.67%
A
InS
B
45.94%
B
In2S3
C
55.71%
C
In3S5
D
56.58 %
D
In6S9
This question covers TEKS 2C and 2D. This
question tests the material that was covered in the
textbook on pages 328–329.
This question covers TEKS 2C. This question tests
the material that was covered in the textbook on
pages 331–332.
10
8
Potassium nitrate, also known as saltpeter, is used in
matches. What is the percent by mass of potassium
(K) in potassium nitrate (KNO3)?
A student measures 10.0 g of hydrated sodium
carbonate (Na2CO3•xH2O) and places it in
a crucible. After heating, 3.7 g of anhydrous
sodium carbonate (Na2CO3) remains. What is
the formula for the hydrate?
Na2CO3•2H2O
B
Na2CO3•5H2O
C
Na2CO3•8H2O
D
Na2CO3•10H2O
This question covers TEKS 2C and 11B. This
question tests the material that was covered in the
textbook on page 339.
A
63.2 g
B
84 g
C
210 g
D
231 g
This question covers TEKS 2C and 10B. This
question tests the material that was covered in the
textbook on page 323.
11
A mole of
12
C
6
A
12 kg
B
12 g
C
12 amu
D
6 amu
atoms will have a total mass of —
This question covers TEKS 4B. This question tests
the material that was covered in the textbook on
pages 313.
22
Chemistry: Matter and Change
Reviewing Chemistry: Mastering the TEKS
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
A
Baking soda is the common name for sodium
hydrogen carbonate (NaHCO3). What is the mass in
grams of 2.75 moles of sodium hydrogen carbonate?
CHAPTER 12
Stoichiometry
Name:
A chemist is about to synthesize tetraphosphorus
decoxide by combining X grams of phosphorus with
sufficient oxygen to react completely with the
phosphorus. If he wants to determine the amount of
tetraphosphorus decoxide that will be produced, all
of the following need to be answered before
initiating the experiment EXCEPT —
A
Use the graph below to answer question 4.
Number of Mole Ratios
per Number of Reactants and Products
Number of Mole Ratios
1
Date:
100
What is the balanced chemical equation for this
reaction?
B
What are the number of moles for each reactant?
C
What is the mole ratio of the two reactants?
Which is the limiting reactant and which is the
excess reactant?
This question covers TEKS 2A. This question tests
the material that was covered in the textbook on
pages 354–357 and 364.
80
60
40
20
0
D
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
2
Three atoms of iron (Fe) are to be combined with
four molecules of oxygen (O2). How many total iron
atoms and oxygen molecules will be combined
during the formation of Fe3O4?
A
3
B
4
C
7
D
10
This question covers TEKS 2C and
11B. This question tests the material
that was covered in the textbook on
page 354.
2Al(s) + 3Br2(l) 2AlBr3(s)
3
4
The above equation represents the reaction of
aluminum and bromine to form aluminum bromide.
Which of these is NOT a mole ratio for this
reaction?
A
2 mol Al:3 mol Br2
B
2 mol AlBr3:2 mol AlBr3
C
3 mol Br2:2 mol Al
D
2 mol AlBr3:3 mol Br2
This question covers TEKS 2C and 11B. This
question tests the material that was covered in the
textbook on pages 356–357.
Reviewing Chemistry: Mastering the TEKS
3
5
6
7
8
4
Number of Species in Equation
This graph shows the number of mole ratios that can
be determined given the number of reactants and
products of a chemical reaction. If this trend
continues, how many mole ratios can be formed with
a chemical reaction that has a sum of eight reactants
and products?
A
54
B
56
C
58
D 60
This question covers TEKS 2D and 2E. This question
tests the material that was covered in the textbook
on pages 356–357.
5
Chemists normally use an excess of one reactant in a
chemical reaction because —
A
the reaction will continue until all of the limiting
reactant is consumed
B
the reaction will continue until all of the excess
reactant is consumed
C
reactions do not take place unless there are
unequal amounts of reactants
D
reactions occur too quickly if equal amounts of
reactants are used
This question covers TEKS 3C. This question
tests the material that was covered in the
textbook on pages 368–369.
Chemistry: Matter and Change
23
CHAPTER 12
Stoichiometry, continued
Name:
Date:
Use the graph below to answer question 6.
8
Production Yield
final yield
final
yield
Time
Theoretical Yield
6
9
The symbol of the elements in the molecule
B
The atomic number of each element in
the molecule
C
The number of electrons at each energy level for
each element
D
The average atomic mass of one atom of each
element in the molecule
Three moles of carbon dioxide are produced when
one mole of propane gas is burned. How many
moles of carbon dioxide will be produced if 30
moles of propane gas are burned?
the actual yield is higher than the
theoretical yield
A
10 moles
B
the calculated percent yield of product will be
less than 100%
B
30 moles
C
the theoretical and actual yields are equal
C
90 moles
D
the percent yield of product is more than 100%
D
120 moles
This question covers TEKS 11B. This question tests
the material that was covered in the textbook on
pages 358–359.
Stoichiometry is the study of quantitative
relationships between amounts of —
A
the reactants and products of a chemical reaction
relative to time
B
the products of a chemical reaction only
C
the reactants and products of a chemical reaction
D
the reactants of a chemical reaction only
This question covers TEKS 3E. This question tests
the material that was covered in the textbook on
pages 353–354.
10
In the movie The Wacky World of Chemistry, a
chemist wrote down the following equation on a
chalkboard: Ti + C + 2Cl2 ➝ TiCl3 + C. This
equation is NOT correct because —
A
the titanium atoms are not equal on both sides of
the equation
B
there are not enough chlorine atoms on the right
side of the equation
C
the carbon atoms are equal on both sides of the
equation
D
the right side of the equation should have a
greater number of atoms than the left side
This question covers TEKS 11C. This
question tests the material that was
covered in the textbook on page 363.
24
Chemistry: Matter and Change
Reviewing Chemistry: Mastering the TEKS
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
A
This question covers TEKS 2D. This question tests
the material that was covered in the textbook on
pages 370–371.
7
A
This question covers TEKS 11B. This question tests
the material that was covered in the textbook on
pages 354–355.
Actual Yield
According to this graph, during a chemical
reaction —
Which piece of information about an element on the
periodic table is most necessary in order to compute
the mass of a given molecule?