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Final Exam
Name: Date:
1. Different arrangements of atoms are shown in thefigures below.
3.
Which figure represents a mixture?
A. Figure 1 B. Figure 2
C. Figure 3 D. Figure 4
2. The following equations represent chemicalreactions.
Which equation shows that the total mass during achemical reaction stays the same?
A. 1 B. 2 C. 3 D. 4
The above picture shows a light bulb connected toa battery with the circuit interrupted by a solution.When dissolved in the water to form a 1.0 molar
complete a circuit allowing the bulb to light except
A. hydrochloric acid. B. sodium nitrate.
C. sucrose. D. ammonium sulfate.
4. H2O2, hydrogen peroxide, naturally breaks downinto H2O and O2 over time. MnO2, manganesedioxide, can be used to lower the energy ofactivation needed for this reaction to take placeand, thus, increase the rate of reaction. What typeof substance is MnO2?
A. a catalyst B. an enhancer
C. an inhibitor D. a reactant
page 1
solution, all of the following substances will
5. In which of the following reactions involvinggases would the forward reaction be favored by anincrease in pressure?
A. A + B (+ AB B. A + B (+ C + D
C. 2A + B (+ C 2D D. AC (+ A
6.
Which action will drive the reaction to the right?
A. heating the equilibrium mixture
B. adding water to the system
8. In a sealed bottle that is half full of water,equilibrium will be attained when water molecules
A. cease to evaporate.
B. begin to condense.
C. are equal in number for both the liquid and
the gas phase.
D. evaporate and condense at equal rates.
9. C3H8 + O2 ! CO2 + H2O
This chemical equation represents the combustion
coefficient for water isC. decreasing the oxygen concentration
D. increasing the system’s pressure
7. NO2(g) + CO(g) (+ NO(g) + CO2(g)
The reaction shown above occurs inside a closedflask. What action will shift the reaction to theleft?
A. pumping CO gas into the closed flask
B. raising the total pressure inside the flask
C. increasing the NO concentration in the flask
D. venting some CO2 gas from the flask
A. 2. B. 4. C. 8. D. 16.
10. Hydrazine, N2H4, and dinitrogen tetroxide, N2O4,react to form gaseous nitrogen and water. Whichof these represents a properly balanced equationfor this reaction?
A. N2H4 + N2O4 ! N2 + H2O
B. 2N2H4 + N2O4 ! 2N2 + 4H2O
C. 2N2H4 + N2O4 ! 3N2 + 4H2O
D. 2N2H4 + 3N2O4 ! 5N2 + 6H2O
page 2 Final Exam
of propane. When correctly balanced, the
11. When methane (CH4) gas is burned in the presenceof oxygen, the following chemical reaction occurs.
CH4 + 2O2 ! CO2 + 2H2O
If 1 mole of methane reacts with 2 moles ofoxygen, then
A. 6.02 × 1023 molecules of CO2 and 6.02 × 1023
B. 1.2 × 1024 molecules of CO2 and 1.2 × 1024molecules of H2O are produced.
C. 6.02 × 1023 molecules of CO2 and 1.2 × 1024molecules of H2O are produced.
D. 1.2 × 1024 molecules of CO2 and 6.02 × 1023molecules of H2O are produced.
12. How many moles of CH4 are contained in96.0 grams of CH4?
A. 3.00 moles B. 6.00 moles
C. 12.0 moles D. 16.0 moles
13. The reaction of element X ( ) with element Y(O) is represented in the following diagram:
Which equation properly describes the reactionbetween X and Y?
A. 3X + 8Y ! X3Y8
B. 3X + 6Y ! X3Y6
C. X + 2Y ! XY2
D. 3X + 8Y ! 3XY2 + 2Y
14. A balanced chemical equation reflects the idea thatthe mass of the products
A. is greater than the mass of the reactants.
B. is less than the mass of the reactants.
C. equals the mass of the reactants.
D. is not related to the mass of the reactants.
page 3 Final Exam
molecules of H2O are produced.
15. Corey found that when he added a certainchemical to water, the water would heat up. Hethen performed an experiment in which he mixeddifferent amounts of the chemical with water ina test tube and measured the temperature of thewater. The results of his experiment are shown in
16. The law of conservation of mass can bedemonstrated by a chemical reaction. Which ofthe following models of a chemical reaction bestrepresents the law of conservation of mass?
A.
Trial Amountof Water
Amount ofChemical
Temperatureof Water
before AddingChemical
Temperatureof Water2 minutes
after AddingChemical
1 100mL 0 grams ◦ C ◦ C2 100mL 5 grams ◦ C ◦ C3 100mL 10 grams ◦ C ◦ C4 100mL 15 grams ◦ C ◦ C
5 100mL 20 grams ◦ C ◦ C
B.
Which of these is a valid conclusion based on theresults of Corey’s experiment?
A. Adding more of the chemical will always heatthe water to a greater temperature.
B. The chemical always heats water to the sametemperature.
C. The temperature of water is not affected bythe amount of the chemical.
D. Adding more of the chemical will heat thewater but only up to a certain temperature.
C.
D.
page 4 Final Exam
2127323535
2121212121
the table below.
17. Students in a biology laboratory are monitoringthe rate at which hydrogen peroxide breaks downto produce water and oxygen gas. They beginmonitoring a sample of hydrogen peroxide andthen add catalase, an enzyme that speeds up itsbreakdown. Their data are shown in the tablebelow.
19. A student heated a 10g sample of a compound inan open container. A chemical reaction occurred.The mass of the sample was measured againand found to be less than before. Which of thefollowing explains the change in mass of thesample?
Time(min)
Rate of HydrogenPeroxide Breakdown(molecules per min)
0.0 00.5 0.0301.0 0.0321.5 4,970,0002.0 5,001,0002.5 4,985,300
3.0 5,021,700
A. The heat caused the compound to becomeless dense.
B. The reaction gave off more heat than wasadded.
C. Some of the lighter atoms were converted toenergy.
D. One of the reaction products was a gas.
Based on the data in this table, during which ofthe following time periods did the students add the
catalase to the hydrogen peroxide?
A. between 0.0 and 0.5 min
B. between 1.0 and 1.5 min
C. between 2.0 and 2.5 min
D. between 2.5 and 3.0 min
18. Copper in the compound CuSO4 can be isolatedin the following reaction with iron.
Fe + CuSO4 ! FeSO4 + Cu
What type of reaction is shown above?
A. decomposition
B. synthesis
C. single displacement
D. double displacement
20. Which of the following represents a doubledisplacement reaction?
A. ABC ! AB + C
B. A + B ! AB
C. AB + CD ! AD + CB
D. A + BC ! AC + B
page 5 Final Exam
21. Fluorine gas is produced according to the followingreaction.
2BrF5(g) (+ Br2(g) + 5F2(g)
Under which of the following conditions willmaximum production of fluorine gas occur?
A. The temperature is reduced until the BrFcondenses.
B. The reaction takes place in the presence ofbromine gas.
C. Additional fluorine gas is continuouslypumped into the container.
D. Fluorine gas is removed from the system as itis formed.
22. The figure below represents a reaction.
What type of reaction is shown?
A. synthesis
B. decomposition
C. single displacement
D. double displacement
23. The equation below shows the formation ofnitrogen monoxide.
N2 + O2 + energy ! 2NO
The graph below shows how potential energychanges as nitrogen and oxygen react to formnitrogen monoxide.
Which of the following conclusions about thereaction is supported by this graph?
A. It is an exothermic reaction.
B. It is an endothermic reaction.
C. It is a decomposition reaction.
D. It is a single displacement reaction.
page 6 Final Exam
24. A student dissolves 10.0g of ammonium nitrate(NH4NO3) crystals in a calorimeter containing100.0g of water. The equation for the dissolutionprocess is shown below.
NH4NO3(s) ! +(aq) −3 (aq)The student records the temperature of the solutionevery 5s. The table below shows the collected
data.
26. A reaction yields 6.26g of a product. What is thepercent yield if the theoretical yield is 18.81g?
A. 3.00% B. 10.6% C. 33.3% D. 56.1%
Time (s) Temperature (◦C)0 22.25 17.510 17.015 16.6
20 16.6
27. Calcium and boron react to form calcium boride,as represented by the chemical equation below.
Ca + 6B ! CaB6
Which type of reaction is shown by this equation?
Which of the following conclusions aboutdissolving the crystals can be made based on thedata?
A. Dissolution added energy to the water, so theprocess is exothermic.
B. Dissolution added energy to the water, so theprocess is endothermic.
C. Dissolution absorbed energy from the water,so the process is exothermic.
D. Dissolution absorbed energy from the water,so the process is endothermic.
25. The balanced equation below represents thereaction of NaOH with H3PO4.
NaOH + H3PO4 ! NaH2PO4 + H2O
When 20g of NaOH reacts with 49g of H3PO4,
9g of water is produced. How many grams of
A. 11g B. 60g C. 69g D. 78g
A. synthesis
B. decomposition
C. double displacement
D. single displacement
28. In places that have cold winters, people spread salton icy roads and sidewalks.
Which of these does the salt do to the ice?
A. It raises the density of ice, causing it to be
less slippery.
B. It destroys the matter of ice, causing the iceto break apart.
C. It lowers the freezing point of water, causingthe ice to melt.
D. It increases the boiling point of ice, causingit to turn into water.
page 7 Final Exam
NaH2PO4 are produced?
29. The following equation represents a balancedchemical reaction.
2Al2O3 + 3C ! 4Al + 3CO2
According to the law of conservation of mass,how many aluminum atoms will be produced if1,000 molecules of aluminum oxide are used inthe reaction?
A. 500 B. 1,000 C. 2,000 D. 4,000
30. How is this reaction classified?
CaO + H2O ! Ca(OH)2 + heat
A. endothermic B. exothermic
C. decomposition D. double replacement
31. This graph represents the change in energy for twolaboratory trials of the same reaction.
Which factor could explain the energy differencebetween the trials?
A. Heat was added to trial #2.
B. A catalyst was added to trial #2.
C. Trial #1 was stirred.
D. Trial #1 was cooled.
page 8 Final Exam
32. Use the graph below to answer the followingquestion(s).
In the graph, which of the following is representedby the letter L?
A. reaction heat
B. progress of reaction
C. catalytic effect
D. activation energy
33. The reaction represented in the graph is bestdescribed by which of the following terms?
A. unreactive B. nonreversible
C. exothermic D. endothermic
34. How does increasing temperature affect thecollisions of reactant molecules in a chemicalreaction?
A. The reactant molecules collide more frequentlywith greater energy per collision.
B. The reactant molecules collide more frequentlywith less energy per collision.
C. The reactant molecules collide less frequentlywith less energy per collision.
D. The reactant molecules collide less frequentlywith greater energy per collision.
page 9 Final Exam
35. The graph below shows the potential energy levelsof products and reactants during a reaction.
Potential Energy LevelsDuring a Reaction
Which statement best describes the reaction shownin the graph?
A. The reaction is exothermic because theproducts have less energy than the reactants.
B. The reaction is endothermic because thereactants have more energy than the products.
C. The reaction is endothermic because theproducts have more energy than the reactants.
D. The reaction is exothermic because thereactants have less energy than the products.
36. Which substance would most neutralize an acidicfood?
A. dairy (pH 5–7)
B. water (pH 6–7)
C. citrus fruit (pH 2–3)
D. baking soda (pH 8–9)
37. The table below shows the pH and reaction tolitmus of four body fluids.
These data indicate that gastric juice is
A. very acidic. B. very basic.
C. positively charged. D. negatively charged.
page 10 Final Exam
38. Red Cabbage pH Indicator Investigation
Red cabbage contains a water-soluble pigment. In a highly acidic solution, the pigment turns bright red, and ina moderately acidic solution, it turns pinkish. In a highly basic solution, the pigment turns yellow, and in a
moderately basic solution, it turns bluish.
A student makes a pH indicator from red cabbage that has a reddish-purple color with a pH of approximately 7.The student pours the same amount of the cabbage solution into each of four different beakers. He then adds adifferent household solution to each of the four beakers until a color change is obtained. His results are shown inthe table below.
Household Solution Color of Mixture
lemon juice bright pink
club soda light pink
window cleaner light blue
drain cleaner greenish-yellow
The student finds the following chart online from someone else’s cabbage pH indicator investigation.
pH 2 4 6 8 10 12
Color red pink purple blue green yellow
Comparing his results to the chart above, what logical conclusion can the student make regarding the substances hetested?
A. Lemon juice has a pH between 0 and 2.
B. Drain cleaner has a pH between 10 and 12.
C. Window cleaner and club soda are both neutral solutions.
D. Window cleaner can be used to completely neutralize drain cleaner.
39. The equation below represents the reaction ofhydrogen iodide with water.
HI + H2O ! H3O+ + I−
Which reactant in this equation acts as a Br nstedbase?
A. HI B. H2O C. HO+3 D. −
40. Which of the following substances has the highestconcentration of hydrogen ions in solution?
A. bleach – pH 13
B. water – pH 7
C. tomato juice – pH 4
D. vinegar – pH 3
page 11 Final Exam
I
41. The equation below shows ammonia dissolving inwater.
NH3(aq) + H2O(l) (+ NH+4 (aq) + OH−(aq)
Why is water considered an acid when ammoniais dissolved in it?
A. Water acts as a proton donor.
B. Water acts as a proton acceptor.
C. Water contains hydrogen atoms.
D. Water has a 2 : 1 ratio of hydrogen to oxygen.
42. In the reaction of hydrobromic acid (HBr) andammonia (NH3), ammonia acts as a Brønsted base.Which of the following ions is formed?
44. Why is sulfuric acid (H2SO4) considered aBronsted acid?
A. It has a pH greater than 7.
B. It is able to donate protons.
C. It contains a hydroxide ion.
D. It reacts with hydronium ions.
45. Bee venom contains acids and other compoundsthat cause the pain and itching from a bee sting.Calamine lotion, which is a mild base, helpsrelieve the symptoms. Which best explains how
the calamine lotion relieves a bee sting?
A. The calamine lotion hydrates the skin aroundthe bee sting.
B. The calamine lotion neutralizes the acids inthe bee venom.
A. N+ B. NH2− C. − D. NH+ C. The calamine lotion decreases the pH of the
bee venom.D. The calamine lotion repairs the cells damaged
by the bee sting.
43. Which of the following characteristics allows bloodto resist changes in pH?
A. acidity B. basicity
C. buffering capacity D. clotting factors
46. Which substance can act as either an acid or abase according to the Brφnsted-Lowry definition?
A. H3O1+ B. NH1+
C. HOH D. HCl
page 12 Final Exam
NH2 4
4
47. What is the [H+] of an HCl solution if the pH is
measured to be 6?
A. 1 × 10−7 M B. 1 × 10−6 M
C. 6 × 10−6 M D. 8 × 10−1 M
48. The chart below shows the characteristics ofseveral common acid-base indicators.
Characteristics of Common Acid-Base Indicators
49. Water is a polar solvent, while hexane is anonpolar solvent.
Which of the examples above illustrates a nonpolarsolute in a polar solvent?
A. NH4Cl in water
B. C10H8 in water
C. C2H5OH in hexane
D. CO(NH2)2 in hexane
Indicator pH Range Color RangeBromocresol Green 3.8–5.4 Yellow to Blue
Congo Red 3.0–5.0 Blue to RedPhenol Red 6.8–8.2 Yellow to Red
Indigo Carmine 11.6–13.0 Blue to Yellow
50. How many moles of HNO3 are needed to prepare5.0 liters of a 2.0M solution of HNO3?
A. 2.5 B. 5 C. 10 D. 20
Which indicator would appear to be yellow ina solution with a hydrogen ion concentration of
1.0 × 10−7?
A. Bromocresol Green B. Congo Red
C. Phenol Red D. Indigo Carmine
51. Many laboratory preparations of solutions callfor stirring the solvent while adding the solute.Which of the following is always an effect of thisprocedure?
A. It decreases the reactivity of the solute.
B. It decreases the solubility of the solute.
C. It brings the solute and solvent rapidly intocontact.
D. It produces a double displacement reaction.
page 13 Final Exam
52. Which of the following solutions has the highestconcentration of solute?
A. 1.0 mol solute in 200mL solvent
B. 2.0 mol solute in 500mL solvent
C. 3.0 mol solute in 1L solvent
D. 4.0 mol solute in 1.5L solvent
54.
Which solute exhibits the least response totemperature change?
A. NH4Cl B. KCl
C. HCl D. NH3
53. A pharmacist mixes together 20g of crystals ofcompound A and 10g of crystals of compound B.The mixture is then dissolved in 120mL of waterto make cough syrup.
The mixture will most likely dissolve fastest underwhich of the following sets of conditions?
A.
B. 55. Consider this reaction:
3Ca(s)+2H3PO4(aq) ! Ca3(PO4)2(s)+3H2(g)
C. How many moles of calcium are required toproduce 3 moles of calcium phosphate?
A. 1 mole B. 3 molesD.
C. 0.33 moles D. 9 moles
page 14 Final Exam
(
(
(
(
Size of Temperature StirringCrystals (mm) ◦C) (Y/N)?
0.01–0.02 22.3 N
Size of Temperature StirringCrystals (mm) ◦C) (Y/N)?
0.1–0.2 49.9 N
Size of Temperature StirringCrystals (mm) ◦C) (Y/N)?
0.1–0.2 22.3 Y
Size of Temperature StirringCrystals (mm) ◦C) (Y/N)?
0.01–0.02 49.9 Y
56. What voume of 0.2-M potassium hydroxide (KOH)
acid (H2SO4)?
A. 20mL B. 40mL
C. 80mL D. 160mL
57. Neutralization occurs when 15.0mL of KOH reactwith 25.0mL of HNO3. If the molarity of HNO3
is 0.750M, what is the molarity of the KOH?
A. 1.67M B. 1.25M
C. 0.600M D. 0.450M
58. In an experiment, 2.62g of iron react completelywith 1.50g of sulfur. What is the empiricalformula for the compound produced?
A. FeS B. FeS2 C. Fe2S D. Fe2S3
59. Which quantity is equivalent to 39 grams of LiF?
A. 1.0 mole B. 2.0 moles
C. 0.50 mole D. 1.5 moles
60. What is the mass in grams of 1.00 mole of O2gas?
A. 11.2 B. 16.0 C. 22.4 D. 32.0
61. Which substance has the greatest molecular mass?
A. H2O2 B. NO C. CF4 D. I2
62. The molar mass of Ba(OH)2 is
A. 154.3 g B. 155.3 g
C. 171.3 g D. 308.6 g
63. A sample of nitrogen containing 1.5 × 1023
molecules has the same number of molecules as asample containing
A. 1.0 mole of H2 B. 2.0 moles of He
C. 0.25 mole of O2 D. 0.50 mole of Ne
page 15 Final Exam
is needed to neutralize 40mL if 0.2-M sulfuric
64. What mass contains 6.0 × 1023 atoms?
A. 6.0g of carbon B. 16g of sulfur
C. 3.0g of helium D. 28g of silicon
65. What is the total number of atoms contained in2.00 moles of nickel?
A. 58.9 B. 118
C. 6.02 × 1023 D. 1.20 × 1024
66. Given the reaction:
4NH3 + 5O2 ! 4NO + 6H2O
What is the maximum number of moles of H2Othat can be produced when 2.0 moles of NH3 arecompletely reacted?
A. 1.0 B. 2.0 C. 3.0 D. 6.0
67. A sample of a compound contains 65.4 grams ofzinc, 12.0 grams of carbon, and 48.0 grams ofoxygen. What is the empirical formula of thiscompound?
A. ZnCO B. ZnCO3
C. Zn2CO3 D. ZnC3O
68. What is the percent by mass of oxygen inmagnesium oxide, MgO?
A. 20% B. 40% C. 50% D. 60%
69. What is the percent composition by mass of sulfurin the compound MgSO4 (gram-formula mass =120. grams per mole)?
A. 20.% B. 27% C. 46% D. 53%
70. Which formulas could represent the empiricalformula and the molecular formula of a givencompound?
A. CH2O, C4H6O4 B. CHO, C6H12O6
C. CH4, C5H12 D. CH2, C3H6
71. What is the molecular formula of a compoundthat has a molecular mass of 42 and an empiricalformula of CH2?
A. CH2 B. C2H4 C. C3H6 D. C4H12
page 16 Final Exam
72. Which reaction occurs at the cathode in anelectrochemical cell?
73.
A. combustion B. neutralization
C. oxidation D. reductionNi0(s) + 2Ag+(aq) ! Ni2+ + 2Ag0(s)
In the given reaction, the Ag+ ions
A. gain electrons B. lose electrons
C. gain protons D. lose protons
page 17 Final Exam
PHYSICAL CONSTANTS AND CONVERSION FACTORS
STANDARD ELECTRODE POTENTIALSIonic Concentraion 1M Water At 298K, 1atm
Half-Reaction E0(volts)
F2(g) + 2e− ! 2F− +2.878H+ + MnO− + 5e− ! Mn2+ + 4H2O
4 +1.51Au3+ + 3e− ! Au(s) +1.50
Cl2(g) + 2e− ! 2Cl− +1.3614H+ + Cr2O2− + 6e− ! 2Cr3+ + 7H2O
7 +1.234H+ + O2(s) + 4e− ! 2H2O +1.23
4H+ + MnO2(s) + 4e− ! Mn2+ + 2H2O +1.22Br2(`) + 2e− ! 2Br− +1.09Hg2+ + 2e− ! Hg(`) +0.85Ag2+ + e− ! Ag(s) +0.80Hg2+ + 2e− ! 2Hg(`)
2 +0.80Fe3+ + e− ! Fe2+ +0.77I2(s) + 2e− ! 2I− +0.54Cu+ + e− ! Cu(s) +0.52
Cu2+ + 2e− ! Cu(s) +0.344H+ + SO2− + 2e− ! SO2(a2q) + 2H2O
4 +0.17Sn4+ + 2e− ! Sn2+ +0.152H+ + 2e− ! H2(g) 0.00Pb2+ + 2e− ! Pb(s) −0.13Sn2+ + 2e− ! Sn(s) −0.14Ni2+ + 2e− ! Ni(s) −0.26Co2+ + 2e− ! Co(s) −0.28Fe2+ + 2e− ! Fe(s) −0.45Cr3+ + 3e− ! Cr(s) −0.74Zn2+ + 2e− ! Zn(s) −0.76
2H2O + 2e− ! 2OH− + H2(g) −0.83Mn2+ + 2e− ! Mn(s) −1.19Al3+ + 3e− ! Al(s) −1.66
Mg2+ + 2e− ! Mg(s) −2.37Na+ + e− ! Na(s) −2.71
Ca2+ + 2e− ! Ca(s) −2.87Sr2+ + 2e− ! Sr(s) −2.89Ba2+ + 2e− ! Ba(s) −2.91Cs+ + e− ! Cs(s) −2.92K+ + e− ! K(s) −2.93
Rb+ + e− ! Rb(s) −2.98
Li+ + e− ! Li(s) −3.04
74. Given the reaction:
Fe(s) + Cu2+ ! Fe2+ + Cu(s)
Based on Reference Table N, what is the potential (E ◦) for the overall reaction
A. −0.11V B. +0.11V C. −0.79V D. +0.79V
page 18 Final Exam
75. Based on Reference Table N, what is thestandard electrode potential (E0) for the reaction
A. 0.45 B. −0.45 C. 0.77 D. −0.77
76. A material will be used to fill an empty beaker tolevel A, as shown in the diagram. Which material,
cause the bulb to glow brightly?
A. C6H12O6(s) B. C6H12O6(aq)
C. KCl(s) D. KCl(aq)
77. Which statement is true about oxidation andreduction in an electrochemical cell?
A. Both occur at the anode.
B. Both occur at the cathode.
C. Oxidation occurs at the anode and reductionoccurs at the cathode.
D. Oxidation occurs at the cathode and reduction
78. Which conversion of energy always occurs in avoltaic cell?
A. light energy to chemical energy
B. electrical energy to chemical energy
C. chemical energy to light energy
D. chemical energy to electrical energy
79. Given the reaction:
HI(g) + H2O(`) (+ H3O+(aq) + I−(aq)
Which species represents the Br¨onsted-Lowry basein the forward reaction?
A. HI(g) B. H2O(`)
C. H3O+(aq) D. −(aq)
80. Given the balanced equation representing areaction:
4 (aq) + H2O(`) ! 3O + SO −(aq)
According to one acid-base theory, the H2O(`)molecules act as
A. a base because they accept H+ ions
B. a base because they donate H+ ions
C. an acid because they accept H+ ions
D. an acid because they donate H+ ions
page 19 Final Exam
I
HSO
Fe2+ ! Fe3+ + e−?
when used to fill the beaker to level A, would
occurs at the anode.
Problem-Attic format version 4.4.220c_ 2011–2014 EducAide SoftwareLicensed for use by Steve Reed
Terms of Use at www.problem-attic.com
Final Exam 05/20/20151.Answer: C
2.Answer: C
3.Answer: C
4.Answer: A
5.Answer: A
6.
Answer: D7.Answer: C
8.Answer: D
9.Answer: B
10.Answer: C
11.Answer: C
12.Answer: B
13.Answer:
14.Answer: C
15.Answer: D
16.Answer: A
17.Answer: B
18.Answer: C
19.Answer: D
20.Answer: C
21.Answer: D22.
Answer: A23.
Answer: B24.
Answer: D25.
Answer: B26.Answer: C
27.
Answer: A28.
Answer: C29.
Answer: C30.
Answer: B31.
Answer: B32.
Answer: D33.
Answer: C34.
Answer: A35.
Answer: C36.
Answer: D37.
Answer: A38.
Answer: B39.
Answer: B40.
Answer: D
Teacher’s Key Page 2
41.Answer: A
42.Answer: D
43.Answer: C44.Answer: B45.Answer: B46.Answer: C47.Answer: B48.Answer: C49.Answer: B50.
Answer: C51.
Answer: C52.
Answer: A53.Answer: D
Answer: B
Answer: D
Answer: C
Answer: B
58.Answer: A59.Answer: D
60.Answer: D
61.Answer: D
62.Answer: C
63.Answer: C
64.Answer: C65.
Answer: D66.Answer: C
67.Answer: B
68.Answer: B
69.Answer: B
70.Answer: D
71.Answer: C
72.Answer: D
73.Answer: A
74.Answer: D
75.Answer: D
76.Answer: D77.
Answer: C78.
Answer: D79.
Answer: B80.Answer: A
54.
55.
56.
57.
