college of engineering putrajaya campus final...

COLLEGE OF ENGINEERING

PUTRAJAYA CAMPUS

FINAL EXAMINATION

TRIMESTER 2, 2010/2011

PROGRAMME : Foundation in Engineering

SUBJECT CODE : CHEF 114

COURSE CODE : Chemistry I

DATE : 7 February 2011

DURATION : 2.30pm – 5.30pm (3 hours)

INSTRUCTIONS TO CANDIDATES:

1. Answer ALL the questions in Sections A and B and any FOUR (4) out of FIVE (5)

questions from Section C.

2. Please mark the answers for Section A in the answer sheet.

3. Write the answers for Sections B and C in the answer booklet.

4. All calculations in Sections B and C must be shown clearly (wherever applicable) in

order to get full marks.

5. Please detach the answer sheet for Section A from this question booklet and fasten it

together with the answer booklet containing answers from Sections B and C.

6. Periodic Table of elements and Standard Reduction Potential Table are provided.

7. No reference books, papers and mobile phones are allowed into the examination hall.

THIS QUESTION PAPER CONSISTS OF24 PRINTED PAGES INCLUDING THIS COVER PAGE

Marking scheme for CHEF 114, Trimester2 2010/2011

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SECTION A

Multiple Choice Questions. There is ONE best response to each question. Read all responses,

choose the best one and write it on your answer booklet. Blacken the circle on the answer

sheet on page 24 corresponding to this answer.

Answer ALL questions. (1 mark for each question)

1. The oxidation state for the P in the formula KH2PO4 is.

A. 3+

B. 5+

C. 4+

D. 2+

E. 0

2. Which of the following is the correct name for HClO4(aq)?

A. Chloric acid

B. Hydrochloric acid

C. Perchloric acid

D. Chlorous acid

E. Hypochlorous acid

3. The mole can be defined as

A. The mass of the atom in atomic mass units

B. The mass exactly equal to one-twelfth the mass of one 12

C atom

C. The amount of substance that contains as many elementary entities such as

atoms in 12 g of 12

C.

D. The mass in gram of one mole of atoms or molecules of a substance.

E. The percent by mass of each element in a compound.


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4. In the following redox reaction

4NH3 + 3Ca(ClO)2 2N2 + 6H2O + 3CaCl2

which element is oxidized and which is reduced?

A. H is oxidized and N is reduced D. Cl is oxidized and O is reduced

B. N is oxidized and Cl is reduced E. Cl is oxidized and N is reduced

C. N is oxidized and O is reduced

5. Which of these properties is/are characteristic(s) of gases?

A. High compressibility

B. Relatively large distances between molecules

C. Formation of homogeneous mixtures regardless of the nature of gases

D. A and B

E. A, B, and C

6. If equal masses of O2(g) and HBr(g) are in separate containers of equal volume and

temperature, which one of these statements is TRUE?

A. The pressure in the O2 container is greater than that in the HBr container.

B. There are more HBr molecules than O2 molecules

C. The average velocity of the O2 molecules is less than that of the HBr

molecules

D. The average kinetic energy of HBr molecules is greater than that of O2

molecules

E. The pressures of both gases are the same


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7. An endothermic reaction causes the surroundings to

A. warm up. D. decrease in temperature.

B. become acidic. E. release CO2.

C. condense.

8. A beaker contains 115 g of ethanol at 18.2°C. If the ethanol absorbs 1125 J of heat

without losing heat to the surroundings, what will be the final temperature of the ethanol?

The specific heat of ethanol is 2.46 J/g.oC.

A. 4.08°C B. 14.1°C C. 18.4°C

D. 22.2°C E. 36.4°C

9. Complete this sentence: Atoms emit visible and ultraviolet light

A. as electrons jump from lower energy levels to higher levels

B. as the atoms condense from a gas to a liquid

C. as electrons jump from higher energy levels to lower levels

D. as they are heated and the solid melts to form a liquid

E. as the electrons move about the atom within an orbit

10. Transition metal elements have atoms or ions with partially filled

A. s subshells D. f subshells

B. p subshells E. g subshells

C. d subshells

11. Which of the following is the general electron configuration for the outermost electrons

of elements in the alkaline earth group?

A. ns1 B. ns

2 C. ns

2np

4 D. ns

2np

5 E. ns

2np

6(n -1)d

6

12. Which one of the following is NOT isoelectronic with Kr?

A. As3+

B. Se2–

C. Rb+ D. Sr

2+ E. Br

–


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13. Which has the shortest bond?

A. C-C B. H-H C. O-H D. Cl-Cl E. Br-I.

14. In which of the following does a bromine atom have a partial negative charge?

A. ClBr B. IBr C. BrO3- D. Br2 E. OBr2

15. Based on the following thermochemical equation:

2Li+(g) + 2F

-(g) → 2LiF(s) H = -2034 kJ

What would be the lattice energy of LiF?

A. -2034 kJ/mol

B. +2034 kJ/mol

C. +1017 kJ/mol

D. -1017 kJ/mol

E. None of the above

16. Which of the following is NOT a linear structure?

A. I2 B. I3-

C. CO2 D. H2S E. C2H2

17. Consider an electrochemical cell constructed from the following half cells, linked by a

KCl salt bridge.

• a Fe electrode in 1.0 M FeCl2 solution

• a Ni electrode in 1.0 M Ni(NO3)2 solution

When the cell is running spontaneously, which choice includes only TRUE statements

and no false ones?

A. The nickel electrode loses mass and the nickel electrode is the cathode

B. The nickel electrode gains mass and the nickel electrode is the cathode

C. The iron electrode gains mass and the iron electrode is the anode

D. The iron electrode loses mass and the iron electrode is the cathode

E. The iron electrode gains mass and the iron electrode is the cathode


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18. Given the following notation for an electrochemical cell

Pt(s) | H2(g) | H+(aq) || Ag

+(aq) | Ag(s)

what is the balanced overall (net) cell reaction?

A. 2H+(aq) + 2Ag

+(aq) H2(g) + 2Ag(s)

B. H2(g) + 2Ag(s) H+(aq) + 2Ag

+(aq)

C. 2H+(aq) + 2Ag(s) H2(g) + 2Ag

+(aq)

D. H2(g) + Ag+(aq) H

+(aq) + Ag(s)

E. H2(g) + 2Ag+(aq) 2H

+(aq) + 2Ag(s)

19. The systematic name for the compound represented below is

A. 4,5-diethylheptane D. 3-methyl-4-propylheptane

B. 3-propyl-4-ethylhexane E. 2-ethyl-4-propylhexane

C. 3-ethyl-4-propylhexane

20. Which one of these choices is the formula for an aldehyde?

A. CH3CHO B. CH3OCH3 C. CH3COCH3

D. CH3COOH E. HCCH


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SECTION B

Answer ALL the questions in this section.

Show your working clearly.

Start your answer for each new question on a fresh sheet of paper.

(40 marks)

QUESTION 1 [10 marks]

(a) (i) Draw 2 possible Lewis structures of the sulfite ion (SO32-

).

(ii) Assign formal charges to each atom on the ion.

[3 marks]

Ans:

Formal charges: ¼ x 6 = 1 ½

¾ ¾

b) TCDD or 2, 3, 7, 8-tetrachlorodibenzo-p-dioxin, is a highly toxic compound.

How many -bonds and -bonds does TCDD have?

[2 marks]

Ans:

bonds = 24; -bonds = 6 +


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c) Use the thermochemical equation and bond energies given in the table below to calculate

the C-Br bond energy.

CH3CH2OH + HBr → CH3CH2Br + H2O Hreaction = -14 kJ/mol

Given:

Bond Bond energy (kJ/mol) Bond Bond energy (kJ/mol)

C-O 351 C-C 347

H-Br 366 C-H 414

H-O 460 C-Br ?

[5 marks]

Ans:

½ ¼ ½ ¼

1 ½ mark for Lewis structures

Bonds broken (reactants)

Bond Number Bond energy (kJ/mol) Total (kJ)

C-C 1 347 347

C-H 5 414 2070

C-O 1 351 351

O-H 1 460 460

H-Br 1 366 366

Total 3594


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Bonds formed (products)

Bond Number Bond energy (kJ/mol) Total (kJ)

C-C 1 347 347

C-H 5 414 2070

C-Br 1 X X

O-H 2 2 x 460 920

Total 3337 + X

Hreaction = ∑Bonds broken – ∑Bonds formed ½

-14 - (3337 + X ) ½

-14 = 257 -X

X = 271 kJ

C-Br bond energy = 271 kJ ½


(a) (i) Draw the Lewis structure for F3SiH (Si is the central atom). [2 marks]

(ii) What is the arrangement of electron pairs around the central atom? [1 mark]

(iii) What is the molecular geometry of F3SiH? [1 mark]

(iv) Is F3SiH polar or non-polar? Show the resultant dipole moment if it is polar.

[2 marks]

Answer:

(i) Lewis structure for F3SiH:

(ii) Tetrahedral.

(iii) Tetrahedral.

(iv) F3SiH is polar.

The resultant dipole moment is:


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(b) Cysteine is one of the natural amino acids.

(i) What are the estimated values of angle 1 and angle 2? [2 marks]

(ii) What is the orbital hybridization used by the S atom? [1 mark]

(iii) What is the orbital hybridization used by the carbon 1? [ 1 mark]

Answer:

(i) Angle 1 = 104.5o ; Angle 2 = 120

o (1 mark + 1 mark)

(ii) sp3 hybridization

(iii) sp2 hybridization


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Consider the following half-reactions and Eo values:

Ag+ (aq) + e

- Ag(s) E

o= 0.80 V

Cu2+

(aq) + 2e- Cu (s) E

o= 0.34 V

Pb2+

(aq) + 2e- Pb(s) E

o= -0.13 V

(a) Which of these metals or ions is the strongest oxidizing agent? Which is the strongest

reducing agent? [2 marks]

(b) The half-reactions can be used to construct three different galvanic cells. Identify the

anode and cathode half –reactions which can deliver the highest voltage.

[2 marks]

(c) Write the overall cell reaction for part (ii), and calculate the values of Ecello at 25

oC.

[2 marks]

(d) Calculate the voltage for the cell in part (ii) if both ion concentrations are 0.010M.

[2 marks]

(e) Calculate the mass change (in grams) of the cathode after the cell supplied a constant

current of 10.0 A for 25.0 min. [2 marks]

Answer:

(i) Ag+ is the strongest oxidizing agent; Pb is the strongest reducing agent.

(ii) Anode: Pb(s) Pb2+

(aq) + 2e- E

o=0.13 V

Cathode: Ag+ (aq) + e

- Ag(s) E

o=0.80 V

(iii)Pb(s) + 2 Ag+ (aq) Pb

2+ (aq) + 2 Ag (s) Ecell

o=0.93 V

(iv)

Ecell = Ecello – (0.0257 V/n) ln ([Pb

2+]/[Ag

+]

2) (½)

= 0.93 V – (0.0257 V/2) ln ([0.010]/[0.010]2) (½)

= 0.93 V – 0.059

= 0.87 V

(v)

(½) (½)

= 16.77 g Ag

10.0 A x 25 min x x x x x 1C

1A.s

60s

1min

1F

96500 C

1 mol Ag

1F

107.87 g

1 mol Ag


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(a) Ester and carboxylic acids are isomeric. Draw the structural formula for the ester and

the carboxylic acid which has the molecular formula, C4H8O2.

[2 marks]

ANS O

║

(ester) CH3C-O-C2H5 (1)

O

║

(carboxylic acid) CH3CH2CH2-C-OH (1)

(b) Fill in the table below with the correct answers:

Compound Functional

group IUPAC name

[3marks]

ANS

Compound Functional

group IUPAC name

Ketone

3-hexanone


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Carboxylic acid

4-methylhexanoic acid

Carboxylic acid

Chloroethanoic acid

(c) The following compound exhibits geometric isomerism. Draw and name the 2

geometric isomers of CH3-CH2-CH=CH-CH3

[4 marks]

Answer

H H H CH3

C = C C = C

CH3CH2 CH3 CH3CH2 H

cis-2-pentene trans-2-pentene

(d) Below (A-E) are five different functional groups found in organic compounds. Which

one of the structures represents an ester functional group?

[1 mark]

ANS = E


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SECTION C

Answer any 4 out of 5 questions in this section.

Show your working clearly.

Start your answer for each new question on a fresh sheet of paper.

(40 marks)


(a) When 0.684 g of an organic compound containing only carbon, hydrogen and oxygen

was burned in oxygen, 1.312 g CO2 and 0.805 g H2O were obtained. What is the

empirical formula of the compound?

[7 marks]

Answer:

All of the carbon is converted to carbon dioxide so,

(1)

(½)

All of the hydrogen is converted to H2O, so

(1)

(½)

The amount of O in the compound is determined by substracting the mass of C and the mass of H

from the sample.

(1)

(½)

The relative mole ratios are:


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(½)

(½)

(½)

The empirical formula C2H6O (1)

(b) Complete and balance the following question.

Write the molecular, ionic and net ionic equations.

Ca(OH)2 (aq) + HNO3 (aq)

[3 marks]

Answer

(1)

(1)

(1)


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(a) Ethane burns in air according to the equation below:

2 C2H6 (g) + 7 O2 (g) 4 CO2 (g) + 6 H2O (g)

(i) There are four gases involved in this reaction. Place them in order of

INCREASING velocity at 25 °C. [1 mark]

(ii) If 2.00 g C2H6 is burned in excess oxygen and the products (CO2 and H2O) are

collected in a 15.0 L flask at 25oC, what is the total pressure of the gases ( in atm)

in the flask? [4 marks]

(b) From the following reactions:

H2 (g) + ½ O2 (g) H2O (ℓ) ∆H = –285.8 kJ

C (graphite) + O2 (g) CO2 (g) ∆H = –393.5 kJ

CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (ℓ) ∆H = –890.4 kJ

calculate the enthalpy of formation of methane, CH4 from its elements.

C (graphite) + 2 H2 (g) CH4 (g) [5 marks]

Answer:

(a) (i) CO2 < O2 < C2H6 < H2O

(ii)


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(b) Eq (1) x 2:

2 H2 (g) + O2 (g) 2 H2O (ℓ) ∆H = –571.6 kJ

Eq (2):

C (graphite) + O2 (g) CO2 (g) ∆H = –393.5 kJ

Eq (3) inverse:

CO2 (g) + 2 H2O (ℓ) CH4 (g) + 2 O2 (g) ∆H = 890.4 kJ

C (graphite) + 2 H2 (g) CH4 (g)

∆Hrxn = (–571.6 kJ) + (– 393.5 kJ) + 890.4 kJ = –74.7 kJ


(a) How many subshells and orbitals are contained within the principle shell n=4?

[1 mark]

Answer: 4 subshells and 16 orbitals. (½) + (½)

(b) Based on their positions in the periodic table, arrange these ions in order of increasing

radius: Cl-, K

+, S

2-, Se

2-, Ar [1 mark]

Answer: K+

< Ar < Cl- < S

2-< Se

2-

(c) Arrange these elements in order of increasing electronegativity and classify each as a

metal, nonmetal, or metalloid: Ge, N, O, Rb, Zr [2 marks]

Answer: Rb < Zr < Ge < N < O.

Metals (Rb, Zr), Metalloid (Ge), Nonmetal (N,O)


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d) The compound Fe3O4 was called lodestone in ancient times, because it responds to

Earth’s magnetic field and can be used to construct a primitive compass. Today Fe3O4 is

commonly called magnetite, because it contains both Fe2+

and Fe3+

, and the unpaired

electrons on these ions align to form tiny magnets.

(i) How many unpaired electrons does each ion have? [2 marks]

(ii) Would you expect compounds containing Zn2+

to be paramagnetic or

diamagnetic? Explain your answer. [2 marks]

(iii) Would you expect Fe or Zn to have the lower third ionization energy? Please give

your reason. [2 marks]

Answer:

(i) Fe2+

has 4 unpaired electrons, and Fe3+

has 5 unpaired electrons. +

(ii) Compounds of Zn2+

do not exhibit magnetic behavior because the Zn2+

ion has no

unpaired electrons. +

(iii) The third ionization potential of Zn is larger than that of Fe, because removing a

third electron from Zn requires breaking into the closed 3d10

subshell.

+


(a) Copy the table below into your answer booklet and complete the blanks:

Compound Electron pairs around

central atom Arrangement of electron pairs

Molecular shape

Hybridization on central atom

No. of -bonds

No. of -bonds

Bonding Lone pair

NO3-

XeF2

[7 marks]


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Ans:

Compound Electron pairs around

central atom Arrangement of

electron pairs Molecular

shape Hybridization

on central atom No. of

-bonds

No. of

-bonds Bonding Lone pair

NO3-

3

0 Trigonal planar

Trigonal

planar

sp2

3

1

XeF2

2

3 Trigonal

bipyramidal

Linear

sp3d

2

0

½ x 14 = 7 marks

(b) For the ethylene (C2H4) molecule,

(i) Draw its Lewis structure and name the hybridization of the central atom.

[¾ mark]

(ii) Based on the VSEPR theory, predict the molecular geometry (shape) around C.

[½ mark]

(iii) Describe the bonding in the ethylene molecule.

(Hint: show the overlap of the orbitals involved in the bonding formation)

[1½ mark]

(iv) Is the ethylene molecular polar or non-polar? [¼ mark]

Ans:

(i)

½

sp2 hybridization ¼

(ii) trigonal planar around each C ½

(iii) Show sp2 hybrid orbitals on C and 1s orbital on each H; show overlap of sp2 hybrid

orbitals between the 2C atoms and sp2 hybrid orbital on C and 1s orbital on H to form


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-bonds, and the side to side overlap between unhybridized pz orbitals on each C to

form -bond.

1.5 marks

(iv) Non-polar ¼

QUESTION 5 (10 marks)

(a) The SO2 present in air is mainly responsible for the phenomenon of acid rain. The

concentration of SO2 can be determined by titrating against a standard permanganate

solution as follows:

SO2 + MnO4- SO4

2- + Mn

2+ (in acidic solution)

(i) Balance the above equation by the ion-electron method. [4 marks]

(ii) Calculate the number of grams of SO2 in a sample of air if 7.37 mL of 0.0080 M

KMnO4 solution are required for the titration.

[2 marks]

Answer:


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Oxidation: SO2 SO42-

(½)

Reduction: MnO4- Mn

2+ (½)

5e- + 8H

+ MnO4

- Mn

2+ + 4H2O (½)

2H2O + SO2 SO42-

+ 4H+ + 2e

- (½)

16H+ + 2MnO4

- 2Mn

2 + 8H2O (½)

10H2O + 5SO2 5SO42-

+ 20H+ (½)

The balanced equation is:

5SO2(g) 2MnO4(aq) 2H2O(l) 5SO4

2(aq) 2Mn

2(aq) 4H

(aq) (1)

The mass of SO2 in the water sample is given by

4 2 2

4 2

0.00800 mol KMnO 5 mol SO 64.07 g SO7.37 mL

1000 mL soln 2 mol KMnO 1 mol SO 3

29.44 10 g SO

(½) (½) (1)

b) Draw FOUR (4) structural isomers for the molecule having the formula C7H7Cl. The

molecule contains one benzene ring.

[4 marks]

The four isomers are:

CH2ClCH3

Cl

CH3CH3

Cl

Cl

(1) X 4

-END OF QUESTION PAPER-


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PERIODIC TABLE

1A

1

H 1.008

IIA

(2)

IIIA

(13)

IVA

(14)

VA

(15)

VIA

(16) VIIA

(17)

2

He 4.003

3

Li 6.941

4

Be 9.012

5

B

10.81

6

C 12.01

7

N 14.01

8

O 16.00

9

F 19.00

10

Ne 20.18

11

Na 22.99

12

Mg 24.31

IIIB

(3)

IVB

(4)

VB

(5)

VIB

(6)

VIIB

(7)

VIIIB

(8) (9) (10)

IB

(11)

1IB

(12)

13

Al 26.98

14

Si 28.09

15

P 30.97

16

S 32.06

17

Cl 35.45

18

Ar 39.95

19

K 39.10

20

Ca 40.08

21

Sc 44.96

22

Ti 47.90

23

V 50.94

24

Cr 52.00

25

Mn 54.94

26

Fe 55.85

27

Co 58.93

28

Ni 58.70

29

Cu 63.55

30

Zn 65.39

31

Ga 69.72

32

Ge 72.61

33

As 74.92

34

Se 78.96

35

Br 79.90

36

Kr 83.80

37

Rb 85.47

38

Sr 87.62

39

Y 88.91

40

Zr 91.22

41

Nb 92.91

42

Mo 95.94

43

Tc 98

44

Ru 101.1

45

Rh 102.9

46

Pd 106.4

47

Ag 107.9

48

Cd 112.4

49

In 114.8

50

Sn 118.7

51

Sb 121.8

52

Te 127.6

53

I 126.9

54

Xe 131.3

55

Cs 132.9

56

Ba 137.3.

57

La 138.9

72.

Hf 178.5

73

Ta 180.9

74

W 183.9

75

Re 186.2

76

Os 190.2

77

Ir 192.2

78

Pt 195.1

79

Au 197.0

80

Hg 200.6

81

Tl 204.4

82

Pb 207.2

83

Bi 209.0

84

Po (209)

85

At (210)

86

Rn (222)

87

Fr (223)

88

Ra (226)

89

Ac (227)

104

Rf (261)

105

Db (262)

106

Sg (266)

107

Bh (264)

108

Hs (269)

109

Mt (268)

110

Ds (269)

58

Ce 140.1

59

Pr 140.9

60

Nd 144.2

61

Pm (145)

62

Sm 150.4

63

Eu 152.0

64

Gd 157.3

65

Tb 158.9

66

Dy 162.5

67

Ho 164.9

68

Er 167.3

69

Tm 168.9

70

Yb 173.0

71

Lu 175.0

90

Th 232.0

91

Pa (231)

92

U 238.0

93

Np (237)

94

Pu (244)

95

Am (243)

96

Cm (247)

97

Bk (247)

98

Cf (251)

99

Es (252)

100

Fm (257)

101

Md (258)

102

No (259)

103

Lr (260)

TABLE OF CONSTANTS

Avogadro's number = 6.022 x 10 23

/mol

1 atm = 760 mmHg = 760 torr = 101,325 Pa

1 J = 1 kg. m2 / s

2

Specific heat of water = 4.184 J/g.C

1 amu = 1.49 x 10-10

J

Planck constant, h = 6.63 x 10-34

J.s

Gas constant, R = 0.0821 L.atm/ K.mol

Gas constant, R = 8.314 J/ K.mol

1 L.atm = 101.3 J

Speed of light, c = 3.00 x 108 m/s

1 kg = 6.022 x 1026

amu

Rydberg constant, RH = 2.18 x 10-18

J

VIIIA

(18)


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Standard Reduction Potentials

Half-Reaction Eo (V)

Au3+

(aq) + 3e- Au(s) 1.50

Cl2(g) + 2e- 2Cl

-(aq) 1.36

O2(g) + 4H+(aq) + 4e

- 2H2O 1.23

Br2(g) + 2e- 2Br

-(aq) 1.08

NO3- (aq) + 4H

+ + 3e

- NO(g) + 2H2O 0.96

Fe3+

(aq) + e- Fe

2+(aq) 0.77

Cu2+

(aq) + 2e- Cu(s) 0.34

2H+(aq) + 2e

- H2(g) 0.00

Sn2+

(aq) + 2e- Sn(s) -0.14

Pb2+

(aq) + 2e- Pb(s) -0.13

Ni2+

(aq) + 2e- Ni(s) -0.25

Cd2+

(aq) + 2e- Cd(s) -0.40

Fe2+

(aq) + e- Fe(s) -0.44

Zn2+

(aq) + 2e- Zn(s) -0.76

2H2O(l) + 2e- H2(g) + 2OH

-(aq) -0.83

Mn2+

(aq) + 2e- Mn(s) -1.18

Al3+

(aq) + 3e- Al(s) -1.66

Mg2+

(aq) + 2e- Mg(s) -2.37

Ca2+

(aq) + 2e-

Ca(s) -2.87

K+(aq) + e

- K(s) -2.93


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Name : __________________________ Student ID : ___________________

Section : _________________________ Lecturer : _____________________

Answer Sheet for Multiple Choice Questions (Section A).

Please use 2B pencil to fill the circle completely. Example :

1.

11.

2.

12.

3.

13.

4.

14.

5.

15.

6.

16.

7.

17.

8.

18.

9.

19.

10.

20.

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

A B C D E

B D E

A B C D E

E

A B C D E

college of engineering putrajaya campus final...

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