chapter 11 railroad tracks - birdville isd / · pdf filechapter 11 railroad tracks 1. ......

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?

=

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62 Chemistry: Matter and Change • Chapter 11 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.

2. The SI unit of molar mass is the

a. gram. b. gram/mole. c. mole. d. mole/gram.

3. Which conversion factor would you use to calculate correctly the mass of 2 moles of theelement titanium?

a. b. c. d.

4. How many moles of oxygen atoms do 1.5 moles of CO2 contain?

a. 1 mol b. 1.5 mol c. 2 mol 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 of12.011 g. What is the mass of one mole of silicon carbide (SiC)?

a. 2.340 g 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)2�H2O. c. NaBr�(HO)2. d. NaBr�2H2O.

10. As a hydrated compound is heated, it decreases in

a. brightness. b. color. c. mass. d. temperature.

47.88 g Ti��1 mol Ti

47.88 mol Ti��1 g Ti

1 mol Ti��47.88 g Ti

1 g Ti��47.88 mol Ti

CHAPTER ASSESSMENTCHAPTER 11

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Chapter Assessment Chemistry: Matter and Change • Chapter 11 65

Applying Scientific MethodsEach time Lisa visited a grocery store in the neighborhood, she noticed a small vial hangingon the wall. The vial was filled with a compound that appeared blue at times and pink at othertimes. One day she questioned the woman who ran the store about the vial. The woman said itwas part of an old weather gadget, but could not remember how it worked. Lisa asked if shecould 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 observa-tions are summarized in the following table and graph.

1. What effect do temperature and relative humidity have on the color of the compound inthe vial?

2. What can you infer from Lisa’s observations about the type of compound that is in thevial? Explain your reasoning.

0102030405060708090

Mon Tue Wed Thu Fri Sat Sun

Daily Relative Humidity (%)

Daily High Temperature (°C)

Graph 1

Mon Tue Wed Thu Fri Sat Sun

CHAPTER ASSESSMENTCHAPTER 11

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

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Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 11 63

Section 11.3 Moles of CompoundsIn your textbook, read about chemical formulas and the mole, the molar mass of com-pounds, 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.

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?

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 ofmethane? 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 oftrichloromethane? 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 valuesrepresents 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 MASTERYCHAPTER 11

Element Molar Mass (g/mol)

Hydrogen 1.01

Carbon 12.01

Chlorine 35.45

HC

H

HCH4

C

H

Cl

Cl

Cl

CHCl3

H

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64 Chemistry: Matter and Change • Chapter 11 Study Guide for Content Mastery

Section 11.4 Empirical and Molecular FormulasIn 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 asample 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 empiricaland 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

4. You have determined that a compound is composed of 0.300 moles of carbon and 0.600 moles of oxygen. What must you do to determine the mole ratio of the elements inthe 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 acompound?

a. (molecular formula)(empirical formula) � n

b. molecular formula �

c. molecular formula � (empirical formula)n

d. molecular formula �n

��empirical formula

empirical formula��n


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8. You know that the empirical formula of a compound has a molar mass of 30.0 g/mol. Theexperimental molar mass of this compound is 60.0 g/mol. What must you do to deter-mine the value of n in the relationship between the molecular formula and the empiricalformula?

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 massof its empirical formula. If the compound’s empirical formula is NO2, what is its molecu-lar 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.Determine the empirical and molecular formulas of this compound, which has a molarmass of 198.22 g/mol.


Section 11.4 continued

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Supplemental Problems Chemistry: Matter and Change • Chapter 11 13

The MoleThe Mole1. 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

c. 11.5 moles of potassium bromide

2. Calculate the number of moles of the substancethat contains the following number of represen-tative particles.

a. 8.92 � 1023 atoms of barium

b. 5.50 � 1025 molecules of carbon monoxide

c. 2.66 � 1022 formula units of potassiumiodide

3. Determine the mass in grams of each of the following quantities.

a. 1.24 moles of beryllium

b. 3.35 moles of calcium

c. 0.155 mole of sulfur

4. Calculate the number of moles in each of thefollowing quantities.

a. 6.35 g lithium

b. 346 g zinc

c. 115 g nickel

5. How many atoms are in the following samples?

a. 1.24 g cobalt

b. 0.575 g cesium

c. 65.6 g silicon

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

7. Calculate the number of moles in each of thefollowing quantities.

a. atoms of each element in 3.35 moles ofaspirin (C9H8O4)

b. positive and negative ions in 1.75 moles ofcalcium fluoride (CaF2)

8. Determine the molar mass of each of the following compounds.

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)

b. 4.62 moles of magnesium bromide (MgBr2)

10. Calculate the number of moles in each of the following samples.

a. 3.75 g calcium carbide (CaC2)

b. 245 g aluminum nitrite (Al(NO2)3)

11. Determine the percent composition of each ofthe following compounds.

a. manganese oxide (MnO)

b. propanol (C3H8O)

c. calcium phosphate (Ca3(PO4)2)

SUPPLEMENTAL PROBLEMSCHAPTER 11

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StoichiometryStoichiometry

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 ofreactants used and the amounts of products formed by a chemical reactionis 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 ofthe reactants.

4. The coefficients in a chemical equation represent not only the number ofindividual particles but also the number of moles of particles.

5. The mass of each reactant and product is related to its coefficient in thebalanced chemical equation for the reaction by its molar mass.

Complete the table below, using information represented in the chemical equation forthe combustion of methanol, an alcohol.

methanol � oxygen 0 carbon dioxide � water

2CH3OH(l) � 3O2 (g) 0 2CO2(g) � 4H2O(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?


Number of Number of Substance Molar Mass (g/mol) Molecules Moles (mol) Mass (g)

6. Methanol 32.05

7. Oxygen gas 32.00

8. Carbon dioxide 44.01

9. Water 18.02

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12 Chemistry: Matter and Change • Chapter 12 Challenge Problems

Mole Relationships inChemical ReactionsMole Relationships inChemical Reactions

The 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.

CHALLENGE PROBLEMSCHAPTER 12

Use with Chapter 12,Section 12.2

1. What information is needed to make the types of conversions shown by double-arrow 1in the diagram?

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 massof a second substance in the reaction, as represented by double-arrow 5 in the diagram?

Moles ofCO

Grams ofCO

Moles ofCO2

Grams ofCO2

Particles ofCO

Particles ofCO2

1

5

2

3

46

7

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Section 12.3 Limiting ReactantsIn your textbook, read about why reactions stop and how to determine the limitingreactant.

Study the diagram showing a chemical reaction and the chemical equation that repre-sents the reaction. Then complete the table. Show your calculations for questions 25–27in the space below the table.

O2 � 2NO 0 2NO2

The molar masses of O2, NO, and NO2 are 32.00 g/mol, 30.01 g/mol, and 46.01 g/mol,respectively.

� � 0 �

Amount and Name Amount of O2 Amount of NO Amount of NO2 Limiting Reactant of Excess Reactant

1 molecule 2 molecules 2 molecules none none

4 molecules 4 molecules 4 molecules NO 2 molecules O2

2 molecules 8 molecules 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.

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72 Chemistry: Matter and Change • Chapter 12 Study Guide for Content Mastery

Section 12.4 Percent YieldIn your textbook, read about the yields of products.

Study the diagram and the example problem.

Example Problem: The following chemical equation represents the production of galliumoxide, a substance used in the manufacturing of some semiconductor devices.

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 orexpression 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

3. number of moles of reactant: 7.00 g Ga �

4. number of moles of product: 0.100 mol Ga �

5. theoretical yield: 0.0500 mol Ga2O3 �

6. percent yield: � 100 9.37 g Ga2O3��7.42 g Ga2O3

187.44 g Ga2O3��1 mol Ga2O3

2 mol Ga2O3��1 mol Ga

69.72 g Ga��1 mol Ga


percent yield � � 100%actual yield

��theoretical yield

mass of product from experimentalmeasurement

mass of product predicted from stoichiometric calculation using

a. mass of reactantb. 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.

Name: Date:

1 How many moles of nitrogen atoms are contained inone mole of Ba(NO3)2?

A 1

B 2

C 6

D 9

2 The molecular formula of a compound is X6Y3. Whatis the empirical formula for this compound?

A X6Y

B XY3

C X2Y

D XY2

3 Zinc is used as a coating on iron and steel to preventcorrosion. What is the mass, in grams, of 0.0650 mol Zn?

A 3.25 g

B 3.90 g

C 3.94 g

D 4.25 g

4 Mole is to atom as gram is to —

A amu

B mass

C molecule

D particle

5 What is the total number of atoms contained in 2.00moles of helium?

A 15.999

B 32.0

C 6.02 � 1023

D 1.20 � 1024

6 A compound has the formula MgSO4•7H2O. Itschemical name is —

A aqueous magnesium sulfate

B magnesium sulfate pentahydrate

C magnesium sulfate heptahydrate

D magnesium sulfate decahydrate

The Mole CHAPTER 11

21

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Reviewing Chemistry: Mastering the TEKS Chemistry: Matter and Change

This question covers TEKS 11B and 11C. Thisquestion tests the material that was covered in thetextbook on page 320.

This question covers TEKS 2D and 11C. Thisquestion tests the material that was covered in thetextbook on page 331.

This question covers TEKS 2C and 10B. Thisquestion tests the material that was covered in thetextbook on page 315.

This question covers TEKS 2D. This question teststhe material that was covered in the textbook onpage 313.

This question covers TEKS 2C. This question teststhe material that was covered in the textbook onpage 311.

This question covers TEKS 11A. This question teststhe material that was covered in the textbook onpage 338.

7 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 forthis compound?

A InS

B In2S3

C In3S5

D In6S9

8 A student measures 10.0 g of hydrated sodiumcarbonate (Na2CO3•xH2O) and places it in a crucible. After heating, 3.7 g of anhydroussodium carbonate (Na2CO3) remains. What is the formula for the hydrate?

A Na2CO3•2H2O

B Na2CO3•5H2O

C Na2CO3•8H2O

D Na2CO3•10H2O

9 Potassium nitrate, also known as saltpeter, is used inmatches. What is the percent by mass of potassium(K) in potassium nitrate (KNO3)?

A 38.67%

B 45.94%

C 55.71%

D 56.58 %

10 Baking soda is the common name for sodiumhydrogen carbonate (NaHCO3). What is the mass ingrams of 2.75 moles of sodium hydrogen carbonate?

A 63.2 g

B 84 g

C 210 g

D 231 g

11 A mole of C atoms will have a total mass of —

A 12 kg

B 12 g

C 12 amu

D 6 amu

12 6

22

CHAPTER 11 The Mole, continued

Reviewing Chemistry: Mastering the TEKS

Copyright ©

Glencoe/M

cGraw

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he McG

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panies, Inc.

Name: Date:

Chemistry: Matter and Change

This question covers TEKS 2C. This question teststhe material that was covered in the textbook onpages 331–332.


This question covers TEKS 2C and 2D. Thisquestion tests the material that was covered in thetextbook on pages 328–329.

This question covers TEKS 4B. This question teststhe material that was covered in the textbook onpages 313.


Stoichiometry

Name: Date:

1 A chemist is about to synthesize tetraphosphorusdecoxide by combining X grams of phosphorus withsufficient oxygen to react completely with thephosphorus. If he wants to determine the amount oftetraphosphorus decoxide that will be produced, allof the following need to be answered beforeinitiating the experiment EXCEPT —

A What is the balanced chemical equation for thisreaction?

B What are the number of moles for each reactant?

C What is the mole ratio of the two reactants?

D Which is the limiting reactant and which is theexcess reactant?

2 Three atoms of iron (Fe) are to be combined withfour molecules of oxygen (O2). How many total ironatoms and oxygen molecules will be combinedduring the formation of Fe3O4?

A 3

B 4

C 7

D 10

2Al(s) + 3Br2(l) � 2AlBr3(s)

3 The above equation represents the reaction ofaluminum and bromine to form aluminum bromide.Which of these is NOT a mole ratio for thisreaction?

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

Use the graph below to answer question 4.

4 This graph shows the number of mole ratios that canbe determined given the number of reactants andproducts of a chemical reaction. If this trendcontinues, how many mole ratios can be formed witha chemical reaction that has a sum of eight reactantsand products?

A 54

B 56

C 58

D 60

5 Chemists normally use an excess of one reactant in achemical reaction because —

A the reaction will continue until all of the limitingreactant is consumed

B the reaction will continue until all of the excessreactant is consumed

C reactions do not take place unless there areunequal amounts of reactants

D reactions occur too quickly if equal amounts ofreactants are used

Number of Species in Equation

100

80

60

40

20

0Num

ber

of M

ole

Rat

ios

Number of Mole Ratiosper Number of Reactants and Products

3 4 5 6 7 8

CHAPTER 12

23

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Reviewing Chemistry: Mastering the TEKS Chemistry: Matter and Change

This question covers TEKS 2A. This question teststhe material that was covered in the textbook onpages 354–357 and 364.

This question covers TEKS 2C and11B. This question tests the materialthat was covered in the textbook onpage 354.

This question covers TEKS 2C and 11B. Thisquestion tests the material that was covered in thetextbook on pages 356–357.

This question covers TEKS 2D and 2E. This questiontests the material that was covered in the textbookon pages 356–357.

This question covers TEKS 3C. This questiontests the material that was covered in thetextbook on pages 368–369.

Use the graph below to answer question 6.

6 According to this graph, during a chemical reaction —

A the actual yield is higher than the theoretical yield

B the calculated percent yield of product will beless than 100%

C the theoretical and actual yields are equal

D the percent yield of product is more than 100%

7 Stoichiometry is the study of quantitativerelationships between amounts of —

A the reactants and products of a chemical reactionrelative 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

8 Which piece of information about an element on theperiodic table is most necessary in order to computethe mass of a given molecule?

A The symbol of the elements in the molecule

B The atomic number of each element inthe molecule

C The number of electrons at each energy level foreach element

D The average atomic mass of one atom of eachelement in the molecule

9 Three moles of carbon dioxide are produced whenone mole of propane gas is burned. How manymoles of carbon dioxide will be produced if 30moles of propane gas are burned?

A 10 moles

B 30 moles

C 90 moles

D 120 moles

10 In the movie The Wacky World of Chemistry, achemist wrote down the following equation on achalkboard: Ti + C + 2Cl2 ➝ TiCl3 + C. Thisequation is NOT correct because —

A the titanium atoms are not equal on both sides ofthe equation

B there are not enough chlorine atoms on the rightside of the equation

C the carbon atoms are equal on both sides of theequation

D the right side of the equation should have agreater number of atoms than the left side

Time

Pro

duct

ion

Yie

ld

Theoretical Yield Actual Yield

final yield

finalyield

24

CHAPTER 12 Stoichiometry, continued

Reviewing Chemistry: Mastering the TEKS

Copyright ©

Glencoe/M

cGraw

-Hill, a division of T

he McG

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ill Com

panies, Inc.

Name: Date:

Chemistry: Matter and Change

This question covers TEKS 2D. This question teststhe material that was covered in the textbook onpages 370–371.

This question covers TEKS 3E. This question teststhe material that was covered in the textbook onpages 353–354.

This question covers TEKS 11B. This question teststhe material that was covered in the textbook onpages 354–355.

This question covers TEKS 11B. This question teststhe material that was covered in the textbook onpages 358–359.

This question covers TEKS 11C. Thisquestion tests the material that wascovered in the textbook on page 363.

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