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Contents: 18 pages Examination: 2 hours 50 multiple-choice questions Additional Time Permitted: 60 minutes © Province of British Columbia Chemistry 12 Examination Booklet 2008/09 Released Exam June 2009 Form A DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO. FOR FURTHER INSTRUCTIONS REFER TO THE RESPONSE BOOKLET.

Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

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Page 1: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Contents: 18 pages Examination: 2 hours 50 multiple-choice questions Additional Time Permitted: 60 minutes © Province of British Columbia

Chemistry 12 Examination Booklet

2008/09 Released Exam June 2009 Form A

DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.

FOR FURTHER INSTRUCTIONS REFER TO THE RESPONSE BOOKLET.

Page 2: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider
Page 3: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 1

PART A: MULTIPLE CHOICE Value: 62.5% of the examination

Suggested Time: 80 minutes

INSTRUCTIONS: For each question, select the best answer and record your choice on the Answer Sheet provided. Using an HB pencil, completely fill in the bubble that has the letter corresponding to your answer.

You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,

fill in the bubble as follows.

FA B C D E HGExam Booklet Form/Cahier d’examen

1. Which of the following would have the highest reaction rate at room temperature?

A. H2 g( ) + I2 g( ) 2HI g( )

B. H2S g( ) + Cl2 aq( ) 2HCl aq( ) + S s( )

C. Ca2 + aq( ) + C2O42

aq( ) CaC2O4 s( )

D. Mg s( ) + 2H2O( ) Mg OH( )2 aq( ) + H2 g( )

2. Consider the following experimental results:

Experiment 1 Experiment 2

Reactants powdered Cu and HCl chunk of Cu and HNO3

Temperature 20º C 10º C

Concentration of acid 0.6 M HCl 0.4 M HNO3

Rate low high

Which of the following factors would account for the lower rate in Experiment 1? A. temperature B. nature of reactants C. surface area of Cu D. concentration of acid

Page 4: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 2 Chemistry 12 – 0906 Form A

3 Which of the following describes “activation energy”? A. the amount of energy that product molecules possess B. the difference between the products PE and the reactants PE C. the amount of energy released when reactant molecules collide D. the minimum amount of energy required to start a chemical reaction 4. Consider the following PE diagram:

Progress of reaction

PE(kJ)

200

100

150

50

Which of the following is correct for the reverse reaction?

PE (activated complex) (kJ) H (kJ)

A. 50 100

B. 50 +100

C. 200 100

D. 200 +100

Page 5: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 3

5. Consider the following reaction mechanism:

Step 1: ClO + H2O HClO + OH

Step 2: I + HClO HIO + Cl

Step 3: HIO + OH IO + H2O

Which of the following is correct?

Reactant for the Overall Reaction Reaction Intermediate

A. I OH

B. ClO H2O

C. H2O HClO

D. HClO HIO

6. Which of the following is correct for all systems at equilibrium?

I The temperature is constant.

II [Reactants] = [Products]

III Forward and reverse reactions are occurring.

IV The forward and reverse reaction rates are equal.

A. I and II only B. I, III and IV only C. II, III and IV only D. III and IV only

Page 6: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 4 Chemistry 12 – 0906 Form A

7. In which of the following does entropy increase?

A. the electrolysis of Na2SO4 aq( )

B. the reaction of NaCl aq( ) with AgNO3 aq( )

C. the redox reaction of an Fe nail in CuCl2 aq( )

D. the neutralization of Sr OH( )2 aq( ) by H2SO4 aq( )

8. Considering enthalpy and entropy factors, in which of the following will equilibrium be established?

I Cl2 g( )?

Cl2 aq( ) H = 25kJ

II CO g( ) + 2H2 g( )?

CH3OH g( ) H = 91kJ

III Mg s( ) + 2HCl aq( )?

MgCl2 aq( ) + H2 g( ) H = 425kJ

IV 3CO2 g( ) + 4H2O g( )?

C3H8 g( ) + 5 O2 g( ) H = +2200 kJ

A. I and II only B. II and IV only C. III and IV only D. I, II and III only

Page 7: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 5

Use the following equilibrium to answer questions 9 and 10.

2NO g( ) N2 g( ) + O2 g( ) H = +181kJ

9. Which of the following pairs of stresses cause the same shift to the above equilibrium? A. adding a catalyst and decreasing volume

B. increasing pressure and increasing NO[ ]

C. decreasing N2[ ] and decreasing temperature

D. decreasing temperature and increasing volume 10. If some O2 is injected into the above equilibrium system, which of the following is correct?

Equilibrium Shift Net Change O2[ ]

A. left increase

B. left decrease

C. right increase

D. right decrease

11. Consider the following:

SO3 g( ) + 6HF g( ) SF6 g( ) + 3H2O g( ) Keq = 6.3 10 3

Which of the following is the value of Keq for:

2SF6 g( ) + 6H2O g( ) 12HF g( ) + 2SO3 g( )

A. 1.3 101

B. 1.6 10 2

C. 3.2 10 2

D. 2.5 10 4

Page 8: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 6 Chemistry 12 – 0906 Form A

12. Consider the following:

I C2H4 g( ) + H2 g( ) C2H6 g( ) Keq = 1.2 1019

II 2HBr g( ) H2 g( ) + Br2 g( ) Keq = 7.0 10 20

III Si s( ) + O2 g( ) SiO2 s( ) Keq = 2.0 10142

Which of the following lists these equilibria from the one that most favours products

to the one that least favours products? A. I, II, III B. I, III, II C. II, III, I D. III, I, II 13. Consider the following equilibrium system:

Ni s( ) + 4CO g( ) Ni CO( )4 g( ) H = 603 kJ

Which of the following statements is correct? A. Increasing CO[ ] will increase Keq .

B. Increasing temperature will increase Keq .

C. Increasing temperature will decrease Keq .

D. Decreasing Ni CO( )4[ ] will decrease Keq .

Page 9: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 7

14. Consider the equilibrium:

N2 g( ) + 3H2 g( ) 2NH3 g( ) Keq = 64

A 1.0 L container is filled with 0.28 mol N2, 0.16 mol H2 and 0.54 mol NH3 .

In which direction will the reaction proceed and what will happen to the pressure of the system?

Direction Pressure

A. left decreases

B. left increases

C. right decreases

D. right increases

15. Which of the following will form a saturated solution? A. 0.10 mol CaSO4 added to 1.0 L of water

B. 0.10 mol Cs2SO4 added to 1.0 L of water

C. 0.20 mol MgSO4 added to 2.0 L of water

D. 0.50 mol Pb NO3( )2 added to 2.0 L of water

16. Which of the following would be an appropriate measure of solubility? A. moles of solute per volume of solute B. mass of solute per volume of solution C. volume of solvent per mass of solvent D. moles of solute at a specific temperature 17. What is the complete ionic equation for the precipitation reaction between

MgS aq( ) and Sr OH( )2 aq( ) ? A. Mg 2+ aq( ) + 2OH aq( ) Mg OH( )2 s( )

B. MgS aq( ) + Sr OH( )2 aq( ) SrS aq( ) + Mg OH( )2 s( )

C. Mg2+ aq( ) + S2 aq( ) + Sr2+ aq( ) + 2OH aq( ) Mg2+ aq( ) + 2OH aq( ) + Sr S s( )

D. Mg2+ aq( ) + S2 aq( ) + Sr2+ aq( ) + 2OH aq( ) Sr2+ aq( ) + S2 aq( ) + Mg OH( )2 s( )

Page 10: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 8 Chemistry 12 – 0906 Form A

18. What is the Ksp expression for the low solubility salt formed when K2SO3 aq( )

and AlCl3 aq( ) are mixed?

A. Ksp = SO32[ ]

B. Ksp = K+[ ] Cl[ ]

C. Ksp = Al3+[ ]2

SO32[ ]

3

D. Ksp = Al 3+[ ]3

SO32[ ]

2

19. Which compound has the lowest solubility? A. ZnS

B. CuS

C. AgCl

D. SrSO4

20. What is the solubility of the salt PbCl2 ? A. 1.4 10 2 M

B. 2.4 10 3 M

C. 3.5 10 3 M

D. 1.2 10 5 M

21. A solution is found to contain a Pb2 +[ ] of 0.10M. What is the maximum SO 42

[ ] that can exist in

this solution before a precipitate forms?

A. SO 42

[ ] = 1.8 10 9 M

B. SO 42

[ ] = 1.8 10 8 M

C. SO 42

[ ] = 1.8 10 7 M

D. SO 42

[ ] = 1.3 10 4 M

Page 11: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 9

22. Which of the following represents the results of tests using an acidic solution?

Reaction

with Mg s( ) Colour in

Phenol Red

A. yes yellow

B. yes red

C. no yellow

D. no red

23. Identify the reactant acid and its conjugate base in the equilibrium below.

Al H2O( )63+

+ HS H2S + Al H2O( )5 OH( )2+

Reactant Acid Conjugate Base

A. HS H2S

B. H2S Al H2O( )63+

C. Al H2O( )63+ HS

D. Al H2O( )63+ Al H2O( )5 OH( )

2+

24. Which of the following is the weakest acid? A. 0.10 M CH3COOH

B. 0.50 M HClO4

C. 1.0 M HIO3

D. 1.5M HCN

Page 12: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 10 Chemistry 12 – 0906 Form A

25. Which of the following is the correct sequence of relative acid strengths?

A. HO2 > HCO3 > H2O2 > H2CO3

B. H2CO3 > HCO3 > H2O2 > HO2

C. H2CO3 > H2O2 > HCO3 > HO2

D. HCO3 > H2O2 > H2CO3 > HO2

26. Water reacts most completely as an acid with which of the following?

A. HO2

B. CO32

C. C2O42

D. HPO42

27. Which of the following equations represents the ionization of water?

A.

H2O( ) H2 aq( ) + 12 O2 aq( )

B. 2H2O( ) H3O

+ aq( ) + O2 aq( )

C. H2O( ) + H2O( ) H+ aq( ) + OH aq( )

D. H2O( ) + H2O( ) H3O

+ aq( ) + OH aq( )

28. The ionization of water is endothermic. Which of the following is a suitable

value of Kw if the temperature of water is lower than 25º C ?

A. 6.8 10 15

B. 2.0 10 14

C. 1.0 10 14

D. 1.6 10 13

Page 13: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 11

29. What is the pOH of 0.30 M HI ?

A. 3.3 10 14

B. 0.52

C. 0.52

D. 13.48

30. What is the equilibrium constant expression for the predominant equilibrium in HCO3 aq( ) ?

A. H2CO3 OH

HCO3

B. H3O+ CO3

2

HCO3

C. HCO3 aq( ) + H2O( ) H2CO3 aq( ) + OH aq( )

D. HCO3 aq( ) + H2O( ) H3O+ aq( ) + CO3

2 aq( )

31. Which of the following 0.10 M solutions would have the lowest pH? A. HF

B. NH3

C. HNO3

D. H2CO3

Page 14: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 12 Chemistry 12 – 0906 Form A

32. Which of the following describes the predominant hydrolysis reaction that occurs in Na2HPO4 aq( )?

A. Na2HPO4 aq( ) 2Na+ aq( ) + HPO42 aq( )

B. PO4

3 aq( ) + H2O( ) HPO42 aq( ) + OH aq( )

C. HPO4

2 aq( ) + H2O( ) H3O+ aq( ) + PO43 aq( )

D. HPO4

2 aq( ) + H2O( ) H2PO4 aq( ) + OH aq( )

33. Which of the following represents a basic salt solution? A. NaI aq( )

B. NH4Cl aq( )

C. Na2CO 3 aq( )

D. NaHSO4 aq( )

34. The term “equivalence point” typically applies to A. buffer solutions. B. titration reactions. C. saturated solutions. D. chemical indicators.

Page 15: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 13

35. A solution is tested with two indicators and the following results are obtained:

Indicator Colour

chlorophenol red red

phenolphthalein colourless

What is the approximate pH of the solution? A. 4.0 B. 6.0 C. 7.0 D. 10.0 36. What is the net ionic equation for the reaction of hydrochloric acid with NaOH aq( ) ? A.

H + aq( ) + OH aq( ) H2O( )

B. HCl aq( ) + NaOH aq( ) NaCl aq( ) + H2O( )

C. HCl aq( ) + NaOH aq( ) + H2O( ) NaCl aq( ) + H3O+ aq( ) + OH aq( )

D. H + aq( ) + Cl aq( ) + Na+ aq( ) + OH aq( ) Na+ aq( ) + Cl aq( ) + H2O( )

37. Consider the following buffer equilibrium system:

HCN aq( ) + H2O( ) H3O

+ aq( ) + CN aq( )

What is the net result of adding a small amount of KOH ? A. The pH increases slightly.

B. The pH decreases slightly.

C. The HCN[ ] increases slightly.

D. The CN[ ] decreases slightly.

Page 16: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 14 Chemistry 12 – 0906 Form A

38. An oxide of which of the following elements will form a basic solution? A. P B. N C. K D. C 39. A reducing agent in a chemical reaction can best be described as a substance that A. loses electrons and has a decrease in oxidation number. B. gains electrons and has a decrease in oxidation number. C. loses electrons and has an increase in oxidation number. D. gains electrons and has an increase in oxidation number. 40. What happens to the oxidation number of O as MgO2 undergoes a reaction in which

H2O2 is formed? A. It decreases by 1. B. It increases by 1. C. It increases by 2. D. It does not change. 41. Consider the following redox equation:

K2Cr2O7 + 7H2SO4 + 6KBr 3Br2 + 4K2SO4 + Cr2 SO4( )3 + 7H2O

Which chemical species is oxidized? A. Br in KBr

B. S in H2SO4

C. H in H2SO4

D. Cr in K2Cr2O7

Page 17: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 15

42. Consider the following spontaneous redox reactions:

X + Y X + Y

Y + Z Y + Z

Which of the following describes the relative strengths of the reducing agents? A. X > Y > Z

B. Z > Y > X

C. X > Y > Z

D. Z > Y > X 43. The following half-reaction can be balanced in acidic solution:

N2O5 NH4+

Which of the following appear in the balanced equation?

A. 13e

B. 14e

C. 16e

D. 18e 44. Consider the following redox reaction:

2MnO4 + 16H++ 10 I 2Mn2+

+ 8H2O + 5 I2

A 10.0 mL sample of an iodide solution is titrated with 15.7mL of acidified 0.0106 M MnO4 .

What is the I[ ] of the sample?

A. 3.33 10 3 M

B. 1.66 10 2 M

C. 3.24 10 2 M

D. 8.32 10 2 M

Page 18: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 16 Chemistry 12 – 0906 Form A

45. Consider the following diagram of a standard electrochemical cell:

1.0 M Zn(NO3)

Cu(s)Zn(s)

21.0 M Cu(NO3)2

e–Object 1e–

Which of the following is correct?

Object 1 Zn s( )

A. light bulb cathode

B. light bulb anode

C. power supply cathode

D. power supply anode

Page 19: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Form A Page 17

Use the following diagram to answer questions 46, 47 and 48.

1.0 M HCl 1.0 M AgNO3

Ag

H2(g)

Pt (inert)

Volts

PorousBarrier

46. What is the overall cell reaction?

A. Ag++ H+ H2 + Ag

B. 2Ag + 2H+ 2Ag++ H2

C. 2Ag++ H2 2H+

+ 2Ag

D. Ag++ H2 Ag + 2H+

+ e

47. Which of the following is correct as the cell operates?

Direction of NO3 Migration pH near the Pt Electrode

A. towards Pt increases

B. towards Pt decreases

C. towards Ag increases

D. towards Ag decreases

48. Which of the following describes the direction of electron flow and the change in mass of the Ag electrode as the cell operates?

Direction of Electron Flow Mass of Ag Electrode

A. from Pt to Ag increases

B. from Pt to Ag decreases

C. from Ag to Pt increases

D. from Ag to Pt decreases

Page 20: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 18 Chemistry 12 – 0906 Form A

49. An iron pipeline can be protected from rusting by connecting it to a A. silver electrode buried beside the pipeline. B. copper electrode buried beside the pipeline. C. positive terminal of a direct current power supply. D. negative terminal of a direct current power supply. 50. The electrolysis of molten NaCl is an industrial process. What does the electrolysis produce? A. Na and Cl2

B. H2 and O2

C. Na + and Cl

D. NaOH and Cl2 You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,

ensure you filled in the bubble as follows.

FA B C D E HGExam Booklet Form/Cahier d’examen

This is the end of the multiple-choice section. Answer the remaining questions in the Response Booklet.

Page 21: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider
Page 22: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider
Page 23: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 Data Page 1

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tein

ium

(252

)

6 8 Er

Erb i

u m

167.

3

100

Fm

Ferm

ium

(25 7

)

69 Tm

Thul

ium

168.

9

101

Md

Men

dele

vium

(258

)

70 Yb

Ytte

rbiu

m

173.

0

102

No

Nob

eliu

m

(259

)

71 Lu

Lute

tium

175.

0

103

Lr

Law

renc

ium

(262

)

1 HH

ydro

gen

1.0

46 Pd

Palla

dium

106 .

4

38 Sr

Stro

ntiu

m

87.6

3 Li

Lith

ium

6.9

14

Si

Si

li

co

n

28.1

Ato

mic

Num

ber

Sym

bol

Nam

eA

tom

ic M

ass

14 Si

Silic

on

28.1

Page 24: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Data Page 2 Chemistry 12

ATOMIC MASSES OF THE ELEMENTSBased on mass of C12 at 12.00.

Values in parentheses are the mass number of the most stable or bestknown isotopes for elements that do not occur naturally.

ActiniumAluminumAmericiumAntimonyArgonArsenicAstatineBariumBerkeliumBerylliumBismuthBoronBromineCadmiumCalciumCaliforniumCarbonCeriumCesiumChlorineChromiumCobaltCopperCuriumDubniumDysprosiumEinsteiniumErbiumEuropiumFermiumFluorineFranciumGadoliniumGalliumGermaniumGoldHafniumHeliumHolmiumHydrogenIndiumIodineIridiumIronKryptonLanthanumLawrenciumLeadLithiumLutetiumMagnesiumManganeseMendelevium

AcAlAmSbArAsAtBaBkBeBiBBrCdCaCfCCeCsClCrCoCuCmDbDyEsErEuFmFFrGdGaGeAuHfHeHoHInIIrFeKrLaLrPbLiLuMgMnMd

89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 105 66 99 68 63 100 9 87 64 31 32 79 72 2 67 1 49 53 77 26 36 57 103 82 3 71 12 25 101

(227) 27.0 (243) 121.8 39.9 74.9 (210) 137.3 (247) 9.0 209.0 10.8 79.9 112.4 40.1 (251) 12.0 140.1 132.9 35.5 52.0 58.9 63.5 (247) (262) 162.5 (252) 167.3 152.0 (257) 19.0 (223) 157.3 69.7 72.6 197.0 178.5 4.0 164.9 1.0 114.8 126.9 192.2 55.8 83.8 138.9 (262) 207.2 6.9 175.0 24.3 54.9 (258)

MercuryMolybdenumNeodymiumNeonNeptuniumNickelNiobiumNitrogenNobeliumOsmiumOxygenPalladiumPhosphorusPlatinumPlutoniumPoloniumPotassiumPraseodymiumPromethiumProtactiniumRadiumRadonRheniumRhodiumRubidiumRutheniumRutherfordiumSamariumScandiumSeleniumSiliconSilverSodiumStrontiumSulphurTantalumTechnetiumTelluriumTerbiumThalliumThoriumThuliumTinTitaniumTungstenUraniumVanadiumXenonYtterbiumYttriumZincZirconium

HgMoNdNeNpNiNbNNoOsOPdPPtPuPoKPrPmPaRaRnReRhRbRuRfSmScSeSiAgNaSrSTaTcTeTbTlThTmSnTiWUVXeYbYZnZr

804260109328417

102768

461578948419596191888675453744

10462213414471138167343526581906950227492235470393040

200.6 95.9 144.2 20.2 (237) 58.7 92.9 14.0 (259) 190.2 16.0 106.4 31.0 195.1 (244) (209) 39.1 140.9 (145) 231.0 (226) (222) 186.2 102.9 85.5 101.1 (261) 150.4 45.0 79.0 28.1 107.9 23.0 87.6 32.1 180.9 (98) 127.6 158.9 204.4 232.0 168.9 118.7 47.9 183.8 238.0 50.9 131.3 173.0 88.9 65.4 91.2

Element Symbol Atomic Number

AtomicMass Element Symbol Atomic

NumberAtomicMass

Page 25: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 Data Page �

NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air.** Not stable in aqueous solutions.

Negative Ions(Anions)

Po s i t i v e I o n s( C a t i o n s )

Aluminum

Ammonium

Barium

Calcium

Chromium(II), chromous

Chromium(III), chromic

Copper(I)*, cuprous

Copper(II), cupric

Hydrogen

Hydronium

Iron(II)*, ferrous

Iron(III), ferric

Lead(II), plumbous

Al3+

NH4+

Ba2+

Ca2+

Cr2+

Cr3+

Cu+

Cu2+

H+

H3O+

Fe2+

Fe3+

Pb2+

Hydroxide

Hypochlorite

Iodide

Monohydrogen phosphate

Nitrate

Nitrite

Oxalate

Oxide**

Perchlorate

Permanganate

Phosphate

Sulphate

Sulphide

Sulphite

Thiocyanate

OH–

ClO–

I–

HPO42–

NO3–

NO2–

C2O42–

O2–

ClO4–

MnO4–

PO4?–

SO42–

S2–

SO32–

SCN–

Bromide

Carbonate

Chlorate

Chloride

Chlorite

Chromate

Cyanide

Dichromate

Dihydrogen phosphate

Ethanoate, acetate

Fluoride

Hydrogen carbonate, bicarbonate

Hydrogen oxalate, binoxalate

Hydrogen sulphate, bisulphate

Hydrogen sulphide, bisulphide

Hydrogen sulphite, bisulphite

Br–

CO32–

ClO3–

Cl–

ClO2–

CrO42–

CN–

Cr2O72–

H2PO4–

CH3COO–

F–

HCO3–

HC2O4–

HSO4–

HS–

HSO3–

Lead(IV), plumbic

Lithium

Magnesium

Manganese(II), manganous

Manganese(IV)

Mercury(I)*, mercurous

Mercury(II), mercuric

Potassium

Silver

Sodium

Tin(II)*, stannous

Tin(IV), stannic

Zinc

Pb4+

Li+

Mg2+

Mn2+

Mn4+

Hg22+

Hg2+

K+

Ag+

Na+

Sn2+

Sn4+

Zn2+

Page 26: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Data Page � Chemistry 12

SOLUBILITY OF COMMON COMPOUNDS IN WATER

The term soluble here means > 0.1 mol/L at 25°C.

Negative Ions(Anions)

Positive Ions(Cations)

Solubility ofCompounds

All

All

All

Soluble

Soluble

Soluble

All Soluble

Soluble

Low Solubility

All others

Soluble

Low Solubility

Soluble

Low Solubility

Soluble

Low Solubility

Soluble

Low Solubility

All others

All others

All others

All others

or

or

or

or

14243

14253

123

123

123

Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+

Ammonium ion: NH4+

Chloride, Cl–

Bromide, Br–

Iodide, I–

Nitrate, NO3–

Hydrogen ion: H+

Ag+, Pb2+, Cu+

Sulphide, S2–Alkali ions, H+, NH4

+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+

Sulphate, SO42–

Hydroxide, OH–Alkali ions, H+, NH4

+, Sr2+ ?

Sulphite, SO32–

Phosphate, PO43–

Carbonate, CO32–

Alkali ions, H+, NH4+

Ag+, Ca2+, Sr2+, Ba2+, Pb2+

Page 27: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 Data Page �

SOLUBILITY PRODUCT CONSTANTS AT 25°C

Name Formula

Barium carbonate

Barium chromate

Barium sulphate

Calcium carbonate

Calcium oxalate

Calcium sulphate

Copper(I) iodide

Copper(II) iodate

Copper(II) sulphide

Iron(II) hydroxide

Iron(II) sulphide

Iron(III) hydroxide

Lead(II) bromide

Lead(II) chloride

Lead(II) iodate

Lead(II) iodide

Lead(II) sulphate

Magnesium carbonate

Magnesium hydroxide

Silver bromate

Silver bromide

Silver carbonate

Silver chloride

Silver chromate

Silver iodate

Silver iodide

Strontium carbonate

Strontium fluoride

Strontium sulphate

Zinc sulphide

BaCO3

BaCrO4

BaSO4

CaCO3

CaC2O4

CaSO4

CuI

Cu(IO3)2

CuS

Fe(OH)2

FeS

Fe(OH)3

PbBr2

PbCl2

Pb(IO3)2

PbI2

PbSO4

MgCO3

Mg(OH)2

AgBrO3

AgBr

Ag2CO3

AgCl

Ag2CrO4

AgIO3

AgI

SrCO3

SrF2

SrSO4

ZnS

2.6 10–9

1.2 10–10

1.1 10–10

5.0 10–9

2.3 10–9

7.1 10–5

1.3 10–12

6.9 10–8

6.0 10–37

4.9 10–17

6.0 10–19

2.6 10–39

6.6 10–6

1.2 10–5

3.7 10–13

8.5 10–9

1.8 10–8

6.8 10–6

5.6 10–12

5.3 10–5

5.4 10–13

8.5 10–12

1.8 10–10

1.1 10–12

3.2 10–8

8.5 10–17

5.6 10–10

4.3 10–9

3.4 10–7

2.0 10–25

K sp

Page 28: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Data Page � Chemistry 12

Perchloric HClO H ClO

Hydriodic HI H I

Hydrobromic HBr H Br

Hydrochloric HCl H Cl

Nitric HNO H NO

Sulphuric H SO H HSO

4 4

3 3

2 4 4

→ +

→ +

→ +

→ +

→ +

→ +

+ −

+ −

+ −

+ −

+ −

+ −

very large

very large

very large

very large

very large

very large

Hydronium Ion H O H H O

Iodic HIO H IO

Oxalic H C O H HC O

Sulphurous SO H O H SO H HSO

Hydrogen sulphate ion HSO H SO

3 2

3 31

2 2 4 2 42

2 2 2 3 32

4 42 2

1 0

1 7 10

5 9 10

1 5 10

1 2 10

+ +

+ − −

+ − −

+ − −

− + − −

→← +→← + ×→← + ×

+( ) →← + ×→← + ×

.

.

.

.

.

Phosphoric H PO H H PO

Hexaaquoiron ion iron ion Fe H O H Fe H O OH

Citric H C H O H H C H O

Nitrous HNO H NO

Hydrofluoric HF

III

3 4 2 43

2 63

2 52 3

3 6 5 7 2 6 5 74

2 24

7 5 10

6 0 10

7 1 10

4 6 10

→← + ×

( ) →← + ( ) ( ) ×→← + ×→← + ×

+ − −

+ + + −

+ − −

+ − −

.

, .

.

.

( )

→→← + ×+ − −H F 3 5 10 4.

Methanoic formic HCOOH H HCOO

Hexaaquochromium ion chromium ion Cr H O H Cr H O OH

Benzoic C H COOH H C H COO

Hydrogen oxalate ion HC O H C O

Ethanoic acetic

III

, .

, .

.

.

,

( )

→← + ×

( ) →← + ( ) ( ) ×→← + ×→← + ×

+ − −

+ + + −

+ − −

− + − −

1 8 10

1 5 10

6 5 10

6 4 10

4

2 63

2 52 4

6 5 6 55

2 4 2 42 5

CHCH COOH H CH COO3 351 8 10→← + ×+ − −.

Dihydrogen citrate ion H C H O H HC H O

Al H O H Al H O OH

Carbonic CO H O H CO H HCO

Monohydrogen citrate ion HC H O H

2 6 5 7 6 5 72 5

2 63

2 52 5

2 2 2 3 37

6 5 72

1 7 10

1 4 10

4 3 10

− + − −

+ + + −

+ − −

− +

→← + ×

( ) →← + ( ) ( ) ×

+( ) →← + ×→←

.

.

.

Hexaaquoaluminum ion, aluminum ion

++ ×→← + ×

− −

− + − −

C H O

Hydrogen sulphite ion HSO H SO

6 5 73 7

3 32 7

4 1 10

1 0 10

.

.

Hydrogen sulphide H S H HS

Dihydrogen phosphate ion H PO H HPO

Boric H BO H H BO

Ammonium ion NH H NH

Hydrocyanic HCN H CN

28

2 4 42 8

3 3 2 310

4 310

10

9 1 10

6 2 10

7 3 10

5 6 10

4 9 10

→← + ×→← + ×→← + ×→← + ×→← + ×

+ − −

− + − −

+ − −

+ + −

+ − −

.

.

.

.

.

Phenol C H OH H C H O

Hydrogen carbonate ion HCO H CO

Hydrogen peroxide H O H HO

Monohydrogen phosphate ion HPO H PO

Water H O H OH

Hydroxide ion OH

6 5 6 510

3 32 11

2 2 212

42

43 13

214

1 3 10

5 6 10

2 4 10

2 2 10

1 0 10

→← + ×→← + ×→← + ×→← + ×→← + ×

+ − −

− + − −

+ − −

− + − −

+ − −

.

.

.

.

.

←← +

← +

+ −

+ −

H O very small

Ammonia NH H NH very small

2

3 2

RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASESin aqueous solution at room temperature.

Name of Acid Base Acid Ka

ST

RO

NG

WE

AK

ST

RO

NG

WE

AK

ST

RE

NG

TH

OF

AC

IDS

TR

EN

GT

H O

F B

AS

E

Page 29: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 Data Page �

ACID-BASE INDICATORS

Indicator

yellow to blue

red to yellow

red to yellow

red to yellow

yellow to blue

red to yellow

yellow to red

yellow to blue

yellow to red

red to amber

yellow to blue

colourless to pink

colourless to blue

yellow to red

blue to yellow

Methyl violet

Thymol blue

Orange IV

Methyl orange

Bromcresol green

Methyl red

Chlorophenol red

Bromthymol blue

Phenol red

Neutral red

Thymol blue

Phenolphthalein

Thymolphthalein

Alizarin yellow

Indigo carmine

pH Range in WhichColour Change Occurs

Colour Changeas pH Increases

0.0 – 1.6

1.2 – 2.8

1.4 – 2.8

3.2 – 4.4

3.8 – 5.4

4.8 – 6.0

5.2 – 6.8

6.0 – 7.6

6.6 – 8.0

6.8 – 8.0

8.0 – 9.6

8.2 – 10.0

9.4 – 10.6

10.1 – 12.0

11.4 – 13.0

Page 30: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Data Page � Chemistry 12

F g e F

S O e SO

H O H e H O

MnO H e Mn H O

Au e Au s

2

2 82

42

2 2 2

42

23

2 2 2 87

2 2 2 01

2 2 2 1 78

8 5 4 1 51

3 1 50

( ) + →← +

+ →← +

+ + →← +

+ + →← + +

+ →← ( ) +

− −

− − −

+ −

− + − +

+ −

.

.

.

.

.

BrO H e Br H O

ClO H e Cl H O

Cl g e Cl

Cr O H e Cr H O

O g H e

312 2 2

4 2

2

2 72 3

2

12 2

6 5 3 1 48

8 8 4 1 39

2 2 1 36

14 6 2 7 1 23

2 2

− + −

− + − −

− −

− + − +

+ −

+ + →← ( ) + +

+ + →← + +

( ) + →← +

+ + →← + +

( ) + + →

l .

.

.

.

←← +H O2 1 23.

MnO s H e Mn H O

IO H e I s H O

Br e Br

AuCl e Au s Cl

NO H e NO g H

22

2

312 2 2

2

4

3 2

4 2 2 1 22

6 5 3 1 20

2 2 1 09

3 4 1 00

4 3 2

( ) + + →← + +

+ + →← ( ) + +

( ) + →← +

+ →← ( ) + +

+ + →← ( ) +

+ − +

− + −

− −

− − −

− + −

.

.

.

.

l

OO +0 96.

Fe e Fe

O g H e H O

MnO H O e MnO s OH

I s e I

Cu e Cu s

3 2

2 2 2

4 2 2

2

0 77

2 2 0 70

2 3 4 0 60

2 2 0 54

0 52

+ − +

+ −

− − −

− −

+ −

+ →← +

( ) + + →← +

+ + →← ( ) + +

( ) + →← +

+ →← ( ) +

.

.

.

.

.

H SO H e S s H O

Cu e Cu s

SO H e H SO H O

Cu e Cu

Sn e Sn

2 3 22

42

2 3 22

4 2

4 4 3 0 45

2 0 34

4 2 0 17

0 15

2 0 15

+ + →← ( ) + +

+ →← ( ) +

+ + →← + +

+ →← +

+ →← +

+ −

+ −

− + −

+ − +

+ − +

.

.

.

.

.

S s H e H S g

H e H g

Pb e Pb s

Sn e Sn s

Ni e Ni s

( ) + + →← ( ) +

+ →← ( ) +

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ −

+ −

+ −

+ −

+ −

2 2 0 14

2 2 0 00

2 0 13

2 0 14

2 0 26

2

22

2

2

.

.

.

.

.

H PO H e H PO H O

Co e Co s

Se s H e H Se

Cr e Cr

H O e H OH M

3 4 3 3 22

23 2

2 27

2 2 0 28

2 0 28

2 2 0 40

0 41

2 2 2 10 0 41

+ + →← + −

+ →← ( ) −

( ) + + →← −

+ →← −

+ →← + ( ) −

+ −

+ −

+ −

+ − +

− − −

.

.

.

.

.

Fe e Fe s

Ag S s e Ag s S

Cr e Cr s

Zn e Zn s

Te s H e H Te

2

22

3

2

2

2 0 45

2 2 0 69

3 0 74

2 0 76

2 2 0 79

+ −

− −

+ −

+ −

+ −

+ →← ( ) −

( ) + →← ( ) + −

+ →← ( ) −

+ →← ( ) −

( ) + + →← −

.

.

.

.

.

2 2 2 0 83

2 1 19

3 1 66

2 2 37

2 71

2 22

3

2

H O e H g OH

Mn e Mn s

Al e Al s

Mg e Mg s

Na e Na s

+ →← ( ) + −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

− −

+ −

+ −

+ −

+ −

.

.

.

.

.

Ca e Ca s

Sr e Sr s

Ba e Ba s

K e K s

Rb e Rb s

2

2

2

2 2 87

2 2 89

2 2 91

2 93

2 98

+ −

+ −

+ −

+ −

+ −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

+ →← ( ) −

.

.

.

.

.

Cs e Cs s

Li e Li s

+ −

+ −

+ →← ( ) −

+ →← ( ) −

3 03

3 04

.

.

Hg e Hg

O g H M e H O

NO H e N O H O

Ag e Ag s

Hg e Hg

2

12 2

72

3 2 4 2

12 2

2

2 0 85

2 10 2 0 82

2 4 2 2 0 80

0 80

0 80

+ −

+ − −

− + −

+ −

+ −

+ →← ( ) +

( ) + ( ) + →← +

+ + →← + +

+ →← ( ) +

+ →← ( ) +

l

l

.

.

.

.

.

STANDARD REDUCTION POTENTIALS OF HALF-CELLSIonic concentrations are at 1M in water at 25°C.

Reducing AgentsOxidizing AgentsS

TR

ON

GW

EA

KS

TR

ON

GW

EA

K

Overpotential Effect

Overpotential Effect

ST

RE

NG

TH

OF

OX

IDIZ

ING

AG

EN

TS

TR

EN

GT

H O

F R

ED

UC

ING

AG

EN

TE° Volts( )

Page 31: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Version 0601.1

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Page 32: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Version 0601.1

D E F G H Exam Booklet Form/Cahier d examen

A B C,

814

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Question 8

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Student Instructions

1. PlaceyourPersonalEducationNumber(PEN)labelatthetopofthisBookletANDfillinthebubble(FormA,B,C,D,E,F,GorH)thatcorrespondstotheletteronyourExaminationBooklet.

2. UseapenciltofillinbubbleswhenansweringquestionsonyourAnswerSheet.

3. Useapencilorblue-orblack-inkpenwhenansweringwritten-responsequestionsinthisBooklet.

4. Whentheexaminationbegins,removetheDataPageslocatedinthecentreoftheExaminationBooklet.

5. ReadtheExaminationRulesonthebackofthisBooklet.

Instructions:

AnswerthefollowingquestionsinthespaceprovidedinthisResponse Booklet.Youareexpectedtocommunicateyourknowledgeandunderstandingofchemicalprinciplesinaclearandlogicalmanner.YourstepsandassumptionsleadingtoasolutionmustbewritteninthisResponse Booklet.Answersmustincludeunitswhereappropriateandbegiventothecorrectnumberofsignificantfigures.For questions involving calculations, full marks will NOT be given for providing only an answer.

Course Code = CH 12

Chemistry 122008/09 Released Exam

JUNE 2009

Response Booklet

Course Code = CH 2008/09 Released ExamJUNE 2009

MINISTRY USE ONLYMINISTRY USE ONLY

12

MINISTRY USE ONLY

Examination Rules

1.Thetimeallottedforthisexaminationistwohours.Youmay,however,takeupto60minutesofadditionaltimetofinish.

2.AnswersenteredintheExaminationBookletwillnotbemarked.

3.Cheatingonanexaminationwillresultinamarkofzero.TheMinistryofEducationconsiderscheatingtohaveoccurredifstudentsbreakanyofthefollowingrules:

• Studentsmustnotbeinpossessionoforhaveusedanysecureexaminationmaterialspriortotheexaminationsession.

• Studentsmustnotcommunicatewithotherstudentsduringtheexamination.

• Studentsmustnotgiveorreceiveassistanceofanykindinansweringanexaminationquestionduringanexamination,includingallowingone’spapertobeviewedbyothersorcopyinganswersfromanotherstudent’spaper.

• Studentsmustnotpossessanybook,paperoritemthatmightassistinwritinganexamination,includingadictionaryorpieceofelectronicequipment,thatisnotspecificallyauthorizedfortheexaminationbyministrypolicy.

• Studentsmustnotcopy,plagiarizeorpresentasone’sown,workdonebyanyotherperson.

• Studentsmustimmediatelyfollowtheinvigilator’sordertostopwritingattheendoftheexaminationtimeandmustnotalteranExaminationBooklet,ResponseBookletorAnswerSheetaftertheinvigilatorhasaskedstudentstohandinexaminationpapers.

• Studentsmustnotremoveanypieceoftheexaminationmaterialsfromtheexaminationroom,includingworkpages.

4.Theuseofinappropriatelanguageorcontentmayresultinamarkofzerobeingawarded.

5.Uponcompletionoftheexamination,returnallexaminationmaterialstothesupervisinginvigilator.

© Province of British Columbia

PlacePersonalEducationNumber(PEN)here. PlacePersonalEducationNumber(PEN)here.

Page 33: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Response Booklet Page 1

PART B: WRITTEN RESPONSE Value: 37.5% of the examination

Suggested Time: 40 minutes

1. (4 marks)

A student burned a paraffin candle C25H52( ) in an open beaker according to the following equation:

C25H52 s( ) + 38 O2 g( ) 25CO2 g( ) + 26H2O g( )

The following data was recorded:

Time (min) Mass of candle and beaker (g)

0.0 175.00

2.0 173.20

Calculate the rate of paraffin consumption in moles of C25H52 per minute mol C25H52 min( ) ;

then, calculate how long it would take to produce 0.70 g CO2 .

Page 34: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 2 Chemistry 12 – 0906 Response Booklet

2. (4 marks)

Consider the following equilibrium:

CO g( ) + 3H2 g( ) CH4 g( ) + H2O g( )

Initially, 0.200 mol CO and 0.600 mol H2 are placed in a 2.00 L container. At equilibrium, H2O[ ] = 0.039 M. Calculate the value of Keq .

Page 35: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Response Booklet Page 3

3. (4 marks)

Consider the following equilibrium:

Mg OH( )2 s( ) Mg 2+ aq( ) + 2OH aq( )

What happens to the amount of solid Mg OH( )2 when some HCl is added?

On the graph below, sketch the effect of adding HCl at time t1 .

Time (s)

Concentration(M)

t1

OH-

Mg2+

Page 36: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 4 Chemistry 12 – 0906 Response Booklet

4. (3 marks)

A solution of Sr OH( )2 aq( ) is titrated with H2SO4 . Explain what will happen to the electrical conductivity during the titration. Begin by writing the balanced formula equation, including states, to support your answer.

Page 37: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Response Booklet Page 5

5. (5 marks)

Aniline C6H5NH2( ) is a weak base with a Kb = 4.3 10 10 .

Calculate the concentration of an aniline solution that has a pH = 8.80 . Begin by writing the equation for the predominant equilibrium.

Page 38: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 6 Chemistry 12 – 0906 Response Booklet

6. (3 marks)

Calculate the OH[ ] that results when 800.0 mL of 0.010 M HCl is mixed with 1.216 g Sr OH( )2 .

(Assume no volume change on mixing.)

Page 39: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Chemistry 12 – 0906 Response Booklet Page 7

7. (4 marks)

Balance the following redox equation in acidic solution:

Te O4 + In In2 O3 + Te (acidic)

Page 40: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Page 8 Chemistry 12 – 0906 Response Booklet

8. (3 marks)

Consider the following cell diagram:

PowerSupply

1 M K2SO4

+

Cu(s)Pb(s)

Write the overall cell reaction.

Write the formula for a precipitate that forms as the cell operates.

Page 41: Chemistry 12 - School District 67old Provincial... · Experiment 1 Experiment 2 Reactants powdered Cu and HCl chunk of Cu and HNO 3 ... Page 6 Chemistry 12 – 0906 Form A 12. Consider

Version 0601.1

D E F G H Exam Booklet Form/Cahier d examen

A B C,

814

NR(.5)3210

Question 8

NR(.5)43210Question 7

NR(.5)3210

Question 6

NR(.5)543210

Question 5

NR(.5)3210

Question 4

NR(.5)43210

Question 3

NR(.5)43210

Question 2

NR(.5)43210

Question 1

Student Instructions

1. PlaceyourPersonalEducationNumber(PEN)labelatthetopofthisBookletANDfillinthebubble(FormA,B,C,D,E,F,GorH)thatcorrespondstotheletteronyourExaminationBooklet.

2. UseapenciltofillinbubbleswhenansweringquestionsonyourAnswerSheet.

3. Useapencilorblue-orblack-inkpenwhenansweringwritten-responsequestionsinthisBooklet.

4. Whentheexaminationbegins,removetheDataPageslocatedinthecentreoftheExaminationBooklet.

5. ReadtheExaminationRulesonthebackofthisBooklet.

Instructions:

AnswerthefollowingquestionsinthespaceprovidedinthisResponse Booklet.Youareexpectedtocommunicateyourknowledgeandunderstandingofchemicalprinciplesinaclearandlogicalmanner.YourstepsandassumptionsleadingtoasolutionmustbewritteninthisResponse Booklet.Answersmustincludeunitswhereappropriateandbegiventothecorrectnumberofsignificantfigures.For questions involving calculations, full marks will NOT be given for providing only an answer.

Course Code = CH 12

Chemistry 122008/09 Released Exam

JUNE 2009

Response Booklet

Course Code = CH 2008/09 Released ExamJUNE 2009

MINISTRY USE ONLYMINISTRY USE ONLY

12

MINISTRY USE ONLY

Examination Rules

1.Thetimeallottedforthisexaminationistwohours.Youmay,however,takeupto60minutesofadditionaltimetofinish.

2.AnswersenteredintheExaminationBookletwillnotbemarked.

3.Cheatingonanexaminationwillresultinamarkofzero.TheMinistryofEducationconsiderscheatingtohaveoccurredifstudentsbreakanyofthefollowingrules:

• Studentsmustnotbeinpossessionoforhaveusedanysecureexaminationmaterialspriortotheexaminationsession.

• Studentsmustnotcommunicatewithotherstudentsduringtheexamination.

• Studentsmustnotgiveorreceiveassistanceofanykindinansweringanexaminationquestionduringanexamination,includingallowingone’spapertobeviewedbyothersorcopyinganswersfromanotherstudent’spaper.

• Studentsmustnotpossessanybook,paperoritemthatmightassistinwritinganexamination,includingadictionaryorpieceofelectronicequipment,thatisnotspecificallyauthorizedfortheexaminationbyministrypolicy.

• Studentsmustnotcopy,plagiarizeorpresentasone’sown,workdonebyanyotherperson.

• Studentsmustimmediatelyfollowtheinvigilator’sordertostopwritingattheendoftheexaminationtimeandmustnotalteranExaminationBooklet,ResponseBookletorAnswerSheetaftertheinvigilatorhasaskedstudentstohandinexaminationpapers.

• Studentsmustnotremoveanypieceoftheexaminationmaterialsfromtheexaminationroom,includingworkpages.

4.Theuseofinappropriatelanguageorcontentmayresultinamarkofzerobeingawarded.

5.Uponcompletionoftheexamination,returnallexaminationmaterialstothesupervisinginvigilator.

© Province of British Columbia

PlacePersonalEducationNumber(PEN)here. PlacePersonalEducationNumber(PEN)here.