PRACTICE TEST I r99

PRACTICE TEST 1

Time: 60 minutes

Note: Unless otherwise stated, for all statements involving chemical equations and/or solutions, assume that the system isin pure water.

Part A

Directions: Each of the following sets of lettered choices refers to the numbered formulas or statements immediatelybelow it. For each numbered item, choose the one lettered choice that fits it best. Then fill in the corresponding oval onthe answer sheet. Each choice in a set may be used once, more than once, or not at all.

aucstisnil=a

(A) Anions

(B) Cations

(C) Element

(D) Isorope

(E) Atom

A positive ion

An atom of the same element that differs by the num-ber of neutrons

Cannot be broken down chemically

Will migrate through a salt bridge to the anode halfcell

l.

2.

4.

200

Ouestions 5-7

5.

6.

"1.

(A) Calorimeter

(B) Geiger Counter

(C) Burette

(D) Funnel

(E) Bunsen burner

Used to detect radioactivitY

Used to deliver acids and bases in a titration

Can be lined with moist filter paper to catch insoluble

solids

Oue$ia$-8=10

(A) Anhenius acid

(B) Anhenius base

(C) Lewis acid

(D) Lewis base

(E) Brgnsted-Lowry acid

Yields hydroxide ions as the only negative ions in

solution

Electron pair accePtor

Proton donor

PART IV / FOUR FULT.LENGTH PRACTICE TESTS

PRACTICE TEST- C ontinue d

a-ucsdals-lLia

(A) Purple solution

(B) Brown-orange liquid

(C) Green gas

(D) Silver-gray liquid

(E) Yellow-orange when burned

in a flame

11. Potassiumpermanganate

12. Sodium salt

13. Chlorine

14. Mercury

9.

r0.

PRACTICE TEST I 20r

PRACTICE TEST- C ontinue d

15.

16.

t7.

Ouestions 15-17

(A) E'is positive

(B) AS is negative

(C) AG is positive

(D) K, is greater than I

(E) K" is very large

Indicates a strong acid

A reaction is nonspontaneous

Less chaos, disorder, and randomness

Ouestions 18-21

(A) Alkali metals

(B) Alkaline earth metals

(C) Transition metals

(D) Halogens

(E) Noble or inert gases

18. Group 1

19. Group 10

20. Contains elements in the solid, liquid, and gas phases

21. Will form chlorides with the formula of MClz

Ouestions 22-25

(A) 1+

(B) 1-

(c) 0

(D) 2+

(E) 3+

22. Oxidation numberof O in H2O2

23. Oxidation number of F in HF

24, Oxidation number of O in Or

25. Oxidation number of calcium in calcium phosphate

204PART IV / FOUR FUIL.I.ENGTH PRACTICE TESTS

PRACTICE TEST- C o ntinued

Pafi C

Directions: Each of the multiple-choice questions or incomplete sentences below is followed by five answers or comple-tions' select the one answer that is best in each case and then fill in the corresponding oval on th. unrr", sheet provided.

28.

26. Which of the following would not be attracted ordeflected while traveling through an electric field?

I. Gamma ray

II. Beta particle

III. Neutron

(A) I only(B) II only(C) I and II only(D) I and III onty(E) I, II, and III

2'7. Which substance below is resonance stabilized bydelocalized pi electrons?

(A) Benzene

(B) Hydrochloric acid(C) Hydrogen gas

(D) Methane(E) Potassium bromide

Which of the following is true about a solution that has

[Ofi'-, = 1.0 x 10-6 M?

(A) The pH is 8 and the solution is acidic.(B) The [H'l = 1.0 x l0{ M andthe soturion is

basic.

(C) The pH is 6 and rhe solurion is acidic.(D) The [Hr-] = 1.0 x 10-6 M andthe solution is

basic.

(E) The [Ht.l = 1.0 x l}-ta M and the solution isneutral.

What will be the products of the following doublereplacement? (NH1)3PO4 + Ba(NO.,), -(A) Ammonium nitrate and barium nitrate(B) Barium nitrate and ammonium phosphate(C) Barium phosphate and sodium nitrate(D) Ammonium nitrate and barium phosphate(E) Ammonium nitrite and barium nitrate

30. Which Ko value is that of an acid that is the weakestelectrolyte?

(A) 1.7 x l0-7

(B) 2.7 x 10 8

(C) 6.6 x 10 ro

(D) 4.9 x 10-3

(E) 5.2 x 10-a

31. A student perf,orms a titration using 1.00 M NaOH tofind the unknown molarity of a solution of HCl. Thestudent records the data as shown below. What is themolarity of the solution of HCI?

@) a.js M(B) 0.s0 M(c) 0.2s M(D) 0.10M(E) 2.00 M

32. Which of the following is not a synthetic polymer?

(A) Polyvinylchloride(B) Plasric

(C) Polystyrene

(D) Polyethylene(E) Cellulose

29.

Base: final burette reading 21.05 mL

Base: initial burette reading 6.05 mL

mL of base used

Aci9: final burette reading 44. 15 mL

Acid: initial burette reading 14.1-5 mL

mL of acid used

PRACTICE TEST I

PRACTICE TEST- C ontinue d

Which process is represented by the arrow on the fol- 3'l .

lowing phase diagram? (See Figure t.)

Figure 1

(A) Evaporation

(B) Deposition

(C) Condensation

(D) Freezing 38.

(E) Sublimation

Whatisthe mo\ar mass of Ca3(POa)21

(A) 310 grams/mole

(B) 154 grams/mole

(C) 67 grams/mole

(D) 83 grams/mole

(E) 115 grams/mole

What is the percent composition of oxygen in C6H12O6 39.(molar mass = 180)?

(A) 25Eo

(B) 33Eo

(c) 40Ea

(D) 53Eo

(E) 1s%

The following reaction occurs at STP: 2H2O(l) - 40.2Hr(g) + Oz(g). How many liters of hydrogen gas canbe produced by the breakd own of i2 grams of water?

(A) 5.6liters(B) I 1.2 liters(C) 2Z.4liters(D) 44.8liters(E) 89.6liters

What is the mass-action expression for the followingreaction at equilibnum?

2W(aq) + X(1) *+ 3Y(aq) + 2Z(s)

(A) lzl'lYl'twl'lxl

(B) twl'[X]lzl'lYl'

(c) lYl'IwF

(D, lr]1"]'-' lwlltl

(trr [*]l"lIzlltl

Which statement best describes the bonding found informaldehyde, CH2O?

(A) The carbon atom is sp hybndized.

\B) \here are Srree sigmabonds and one prbondpresent.

(C) The bonding gives the molecule a tetrahedralshape.

(D) The bonds between the atoms are ionic bonds.(E) All of the bonds are nonpolar bonds.

What is the molarity of a solution thathas29.25 gramsof NaCl dissolved to make 1.5 liters of solution?

(A) t9.s M(B) 3.0 M(c) t.1s M(D) 0.33 M(E) 1.0 M

A sample of a gas at STP contains 3.01 x 1023 mole-cules and has a mass of 22.0 grams. This gas is mostlikely

(A) co,(B) O'(C) N:(D) CO(E) NO

205

JJ.

34.

35.

36.

206 PART IV / FOUR FUTL.LENGTH PRACTICE TESTS

PRACTICE TEST- C ontinue d

46.4r. What is the value of AH for the reaction: X + 2Y - 22?

(W+X - 2Y AH = -200kcal)(2W + 3X - 2Z + 2Y AH = -150 kcal)

(A) -550 kcal

(B) +50 kcal

(C) -50 kcal

(D) -350 kcal

(E) +250 kcal

Which fraction would be used to find the new volume

of a gas at 760 torr under its new pressure at 900 torr

if the temperature is kept constant?

(A) 900 / 760

(B) 1.18

(c) 760 / 900

(D) 6s8.7 t198.1(E) 198.7 /658.',7

Which of the following can be classifled as a precipi-

tation reaction?

(A) HCl(aq) + NaOH(aq) *(B) KBr(aq) + NaCl(aq) -(C) AgNO:(aq) + MgCl(aq) -(D) CaCL(aq) + KI(aq) *(E) NaNO.(aQ) + HCrHiO2(aq) -

Which system at equilibrium will not be influenced by

a change in pressure?

(A) 3Oz(g) -- 2O:(8)

(B) Nz(g) + 3H:(g) *- 2NH:(8)(C) 2NO:(g) *- NuO+(g)

(D) Hr(g) + Iz(g) -- 2Hi(g)(E) 2W(g) + X(g) -- Y(g + 2Z(s)

The organic reaction: C2H6 + Cl: * HCI + CzHsCl is

best described as

1A.1 a substitution reaction

(B) an addition reaction

(C) an esterification

(D) a dehydration synthesis

(E) a fermentation

Enough CaSOa(s) is dissolved in water at 298 K toproduce a saturated solution. The concentration ofCa2* ions is found to be 3.0 x l0-3M. The K"n value forCaSO+ will be

(A) 6.0 x 10{(B) 9.0 x 10{(C) 6.0 x 10i(D) 9.0 x 10r(E) 3.0 x 10-3

Which of the following statements is not true about

acid rain?

(A) Acid rain will erode marble statues.

(B) Acid rain can change the pH of lakes and

streams.

(C) Acid rain can be formed from carbon dioxide.

(D) Acid rain creates holes in the ozone layer.

(E) Acid rain can be formed from the gases SO2

and SO3.

Which mole sample of the solids below is best for

melting a 500-gram sheet of ice on a sidewalk?

(A) NaCl

(B) CaCl,

(C) KBr(D) AgNo:(E) NaCzHrOz

Given this reaction that occurs in plants: 6COz +

6HrO - C6Hr2O6 + 602. If 54 grams of water are con-

sumed by the plant, how many grams C6H12O6 (molar

mass is 180 grams/mole) can be made? Assume an

unlimited supply of carbon dioxide for the plant to

consume as well.

(A) 54 grams

(B) 180 grams

(C) 540 grams

(D) 3 grams

(E) 90 grams

41.1a+L.

43.48.

44.49.

45.

PRACTICE TEST I 207

54.50. Which of the following will nor be changed by rhe

addition of a catalyst to a reaction at equilibrium?

I. The point of equilibriumII. The heat of reaction, AH

III. The potential energy ofthe products

(A) I only(B) II only

(C) I and II only(D) II and III only(E) I, II, and III

According to the reaction Pb(s) + S(s) - PbS(s), when20.7 grams of lead are reacted with 6.4 grams of sulfur

(A) there will be an excess of 20.7 grams of lead(B) the sulfur will be in excess by 3.2 grams

(C) the lead and sulfur will react completely with-out any excess reactants

(D) the sulfur will be the limiting factor in thereaction

(E) there will be an excess of 10.35 grams of lead

Which of the following statements is not part of the

kinetic molecular theory?

(A) The average kinetic energy of gas molecules isproportional to temperature.

(B) Attractive and repulsive forces are present

between gas molecules.

(C) Collisions between gas molecules are perfectlyelastic.

(D) Gas molecules travel in a continuous, random

motion.

(E) The volume that gas molecules occupy is mini-.mal compared to the volume in which the gas is

contained.

A student is performing an experiment where a bluesalt is being heated to dryness in order to determinethe percent of water in the salt. Which pieces of labo-ratory equipment would be used to help determinethis percentage?

I. A crucible and cover

II. Tongs

IIL A triple beam balance

(A) II only(B) III only

(C) I and III only(D) II and III only(E) I, II, and III

PRACTICE TEST- C ontinued

(A)

(B)

(c)(D)(E)

Which of the following is considered to be a danger-

ous procedure in the laboratory setting?

(A) Pouring all liquids, especially acids and bases,

over the sink(B) Wearing goggles

(C) Pushing glass tubing, thermometers, or glass

thistle tubes through a rubber cork(D) Pointing the mouth of a test rube thar is being

heated away from you and others(E) Knowing where the fire extinguisher and eye-

wash stations are located

Given a 4-gram sample of each Hr(g) and He(g), each

in separate containers, which of the following state-

ments is true? (Assume STP.)

(A) The sample of hydrogen gas will occupy44.8 liters and the sample of helium will con-tain 6.02 x 1023 molecules.

(B) The sample of hydrogen gas will occupy22.4 liters and the sample of helium will con-tain3.02 x 1023 molecules.

(C) The sample of hydrogen gas will occupy44.8 liters and the sample of helium will con-tain L202 x 102a molecules.

(D) The sample of helium will occupy 44.8 litersand the sample of hydrogen gas will contain6.02 x 1023 molecules.

(E) None of the above statements is correct.

The diagram shows a solid being heated from belowits freezing point. Which line segment shows the gas and

liquid phases existing at the same time? (See Figure 2.)

TimeFigure 2

51.

55.

52.

56.

t<

(.)qE

F

53.

AB

C

D

E

208 PART IV / FOUR FUTL.LENGTH PRACTICE TESTS

PRACTICE TEST- C ontinued

62.57. Which of the following statements is/are correct

regarding molecular geometries?

I. CH4 is trigonal pyramidal in shape.

[. BF3 is trigonal planar in shape.

IIL XeFo is tetrahedral in shape.

(A) I only

(B) II only

(C) III only(D) I and III only

(E) I, II, andIII

When Uranium-238 undergoes one alpha decay and

then one beta decay, the resulting isotope is

(A) Th-234

(B) U-234

(C) Pa-234

(D) rh-230(E) Ra-226

Which compound is matched up with its correct name?

(A) CO-monocarbonmonoxide(B) CaFz-calcium difluoride

(C) CCl+-carbontetrachloride(D) PCl-potassium trichloride(E) TiF,r-tin(IV)fluoride

Of the statements below, which best explains why CHa

is a gas at STP, while C3Hrs is a liquid and C20Ha2 is

a solid?

(A) C20H42 has the greatest ionic interaction

between its molecules.

(B) C20H42 has a greater amount of hydrogen bond-

itrg than CHa or CrH'r.

(C) There is more dipole-dipole interaction between

molecules of greater mass.

(D) CH4 has the greatest intermolecular forces

while C26H.r has the least.

(E) There are more Van der Waals (dispersion)

forces between nonpolar molecules that are

greater in mass.

Which of the gases listed below would not be collected

via water displacement?

(A) co,(B) CH4

(C) 02

(D) NH3

(E) H2

Which scientist and discovery are not correctly paired?

(A) Millikan / neutron

(B) Rutherford / nucleus

(C) Charles / relationship between temperature and

pressure

(D) Curie / radioactivity(E) Mendeleyev / periodic table

Which of the following situations demonstrate(s) an

increase in entropy?

L Dissolving a salt into water

II. Sublimation

III. Heating up a liquid

(A) I only

(B) I and II only(C) II and III only

(D) I and III oniy(E) I, II, andIII

How many moles of a gas are present in a closed,

empty soda bottle that has a volume of 2.0 liters at

22'C and a pressure of 1.05 atm?

(A)(t.osatm)(z.ot-)

( o.oszo L.atm/K.mol ) ( 22'C )

(B) (o.oazo i-.at'rr/r.mot)(zosr)

@rcr (r.osa')(:.0 l)(zosr)-@

(D) (t.osut-)(z.or-)

( o.oazo L.atm/r.mot )

( zosr )

(E) (o.oszoI-.atm/K.moi)

( t.os un") (z.o r-) (zosr)

Which set of conditions below guarantees that a reac-

tion will be spontaneous?

(A) AH(+) and AS(-)(B) AH(-) and AS(+)

(C) AH(+) and AS(+) at a low temperature

(D) AH(-) and AS(-) at a high temperature

(E) AG(+)

How many moles of electrons are transferred in the

following reaction? Ce3* + Pb - Ce + Pba*

(A) 14

(B) 12

(c) 7

(D) 24

(E) 3

63.

-58.

64.59.

60.

61.

65.

66.

PRACTICE TEST I

PRACTICE TEST- C ontinued

61 . A gas is conflned in the manometer as shown. (See 69.Figure 3.) The stopcock is then opened and the high-est level of mercury inside the tube moved to a levelthat is B0 mm above its lowest level. What is the pres-sure of the gas?

209

Which indicator is correctly paired up with its propercolor if it were added to a base?

I. Litmus-blueII. Phenolphthalein-pinkIII. Methyl Orange-yellow

(A) I only(B) II only(C) III only(D) I and III only(E) I, II, and III

Which structure below demonstrates a violation of theoctet rule? (See Figure 4.)

(A) H-C=C-H(B) o

il

H-C-H

(c) oHI

O:S: O

I

OH

(D) H-N-HI

H

(E) H-C:C-HttHH

Figure 4

Hgmj760

10

68.

80 mm

Figure 3

(A) 80 mmHg(B) 160 mm Hg(C) 680 mm Hg(D) 840 mm Hg(E) The pressure cannot be determined.

Which statement best describes the density and rate ofeffusion of the following gases?

NO, CrHo Kr Xe F2

(A) Fluorine has the lowest density and the lowestrate of effusion.

(B) Xenon has the greatest rate of effusion and thelowest density.

(C) Krypton has the lowest density and greatest rateof effusion.

(D) Ethane has the greatest rate of effusion and thelowest density.

(E) Nitrogen dioxide has the highest density andthe greatest rate of effusion.

STOPIF YOU FINISH BEFORE TIME IS CALLED, GO BACK AND CHECK YOUR WORK.

ANSWERS'

!

1. B!

2. D!

3. C!

4. A!

5. B!

6. C!

7. D!

8. B!

9. C!

10. E!

11. A!

12. E!

13. C!

14. D!

15. E!

16. C!

17. B!

18. A!

19. C!

20. D!

21. B!

22. B!

23. B!

24. C!

25. D!

!

101. T,!T,!CE!

102. F,!F!

103. T,!F!

104. T,!T,!CE!

105. T,!T,!CE!

106. T,!T,!CE!

107. T,!T,!E!

108. F,!F!

109. T,!T,!CE!

110. T,!T,!CE!

111. T,!F!

112. T,!F!

113. T,!F!

114. F,!T!

115. T,!F!

!

26. D!

27. A!

28. B!

29. D!

30. C!

31. B!

32. E!

33. E!

34. A!

35. D!

36. E!

37. C!

38. B!

39. D!

40. A!

41. E!

42. C!

43. C!

44. D!

45. A!

46. B!

47. D!

48. B!

49. E!

50. E!

51. B!

52. B!

53. E!

54. C!

55. A!

56. D!

57. B!

58. C!

59. C!

60. E!

61. D!

62. A!

63. E!

64. D!

65. B!

66. B!

67. D!

68. D!

69. E!

70. C!