TECHNICAL SCIENCES P2 - docscientia.co.za · (4) 3.4 Compounds C and D are of similar molecular size. The boiling point of compound D is higher than that of compound C as shown in

Technical Sciences P2 1 FS/September 2019 Grade 12 Prep. Exam.

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PREPARATORY EXAMINATION

GRADE 12

TECHNICAL SCIENCES P2

SEPTEMBER 2019

MARKS: 150

TIME: 3 HOURS

This paper consists of 15 pages and 4 information sheets.



INSTRUCTIONS AND INFORMATION 1. Write your name and other information in the appropriate spaces on the

ANSWER BOOK. 2. This question paper consists of TEN questions. Answer ALL questions in the

ANSWER BOOK. 3. Start EACH question on a NEW page in the ANSWER BOOK. 4. Number the answers correctly according to the numbering system used in this

question paper. 5. Leave one line between two sub-questions, for example between

QUESTION 2.1 and QUESTION 2.2. 6. You may use a non-programmable pocket calculator. 7. You may use appropriate mathematical instruments. 8. You are advised to use the attached DATA SHEETS. 9. Show ALL formulae and substitutions in ALL calculations. 10. Round off your FINAL numerical answers to a minimum of TWO decimal

places. 11. Give brief motivations, discussions, et cetera where required. 12. Write neatly and legibly.



QUESTION 1: MULTIPLE CHOICE QUESTIONS Four options are provided as possible answers to the following questions. Each question has only ONE correct answer. Choose the answer and write only the letter (A – D) next to the question number (1.1 – 1.10) in the ANSWER BOOK, for example 1.11 E. 1.1 Which ONE of the following statements regarding ALKANES is correct?

All alkanes …

A are unsaturated hydrocarbons.

B are saturated hydrocarbons.

C contain at least one double bond between carbon atoms.

D contain at least one triple bond between carbon atoms. (2) 1.2 Which ONE of the following homologous series contains a CARBONYL

group?

A Alkynes

B Alkenes

C Alcohols

D Aldehydes (2) 1.3 The temperature at which the vapour pressure of a substance is equal to the

atmospheric pressure is known as …

A evaporation.

B freezing point.

C melting point.

D boiling point. (2)



1.4 Consider the organic compound represented below. The above compound is …

A saturated and branched.

B unsaturated and branched.

C saturated and straight chained.

D unsaturated and straight chained. (2) 1.5 Which ONE of the following represents the energy conversion that takes

place in an ELECTROLYTIC cell?

A Chemical to mechanical

B Mechanical to chemical

C Chemical to electrical

D Electrical to chemical (2) 1.6 The oxidation number of Mn in KMnO4 is:

A +1

B +2

C +5

D +7 (2)

C C C

C

H

H

H H

H

H

H

H



1.7 Which ONE of the following half-reactions takes place at the CATHODE of a Cu-Zn galvanic cell?

A Cu2+ + 2e- → Cu

B Zn2+ + 2e- → Zn

C Cu → Cu2+ + 2e-

D Zn → Zn2+ + 2e- (2) 1.8 The image formed through a CONCAVE lens is always …

A upright and real.

B upright and virtual.

C inverted and real.

D inverted and virtual. (2) 1.9 The part of a lens through which a light ray passes through without changing direction is the …

A pole.

B focal point.

C optical centre.

D centre of curvature. (2)



1.10 The diagram below shows a light ray travelling into a semi-circular glass block. In which ONE of the following diagrams does θ represent the CRITICAL ANGLE for glass?

A

B

C

D

(2) [20]

θ

θ θ

θ θ



QUESTION 2 (Start on new page.)

Consider organic compounds represented by the letters A to F below and answer the questions that follow.

A C C CH

O H

HH

H

H

B

C

D

C C CH

H

C

H

HH

H

O

H

H

H

H

E Ethyl ethanoate F Propanal

2.1 Define the term homologous series. (2)

2.2 Write down the letter(s) that represents the following:

2.2.1 An alkane (1)

2.2.2 An ester (1)

2.2.3 A hydrocarbon (1)

2.2.4 An alcohol (1)

2.2.5 An aldehyde (1)

2.3 Write down the:

2.3.1 NAME of the homologous series to which compound A belongs (1)

2.3.2 IUPAC name of compound C (2)

2.3.3 Structural formula of compound E (2)

2.4 Compound B has a chain isomer.

2.4.1 Define the term chain isomer. (2)

2.4.2 Write down the IUPAC name of the CHAIN ISOMER of compound B.(2) [16]

C C C

H

H

H

H

H

C

H

H

H

H

H

C C C CH

H

H H

H H

H

H



QUESTION 3 (Start on new page.) The boiling points of four organic compounds, A to D, are shown in the table below.

COMPOUND BOILING

POINT (°C)

A CH4 -164

B CH3CH3 -89

C CH3CH2CH3 -42

D CH3CH2OH 78

3.1 Define the term functional group. (2) 3.2 Write down the NAME of the functional group of alcohols. (1) 3.3 The boiling points of compounds A, B and C are compared. 3.3.1 In what phase are these compounds at room temperature (25 °C)? Choose from GASES, LIQUIDS or SOLIDS. (1) 3.3.2 Name the TYPE of intermolecular forces in these compounds. (1) 3.3.3 STATE and fully EXPLAIN the trend in the boiling points from compound A to compound C. (4) 3.4 Compounds C and D are of similar molecular size. The boiling point of

compound D is higher than that of compound C as shown in the table above.

3.4.1 Give a reason why it is fair to compare the boiling points of these

two compounds. (1) 3.4.2 Name the TYPE of intermolecular forces in compound D which are

mainly responsible for the huge difference in boiling points. (1) 3.5 Define the term vapour pressure. (2) 3.6 Which one of the compounds (A, B, C or D) has the HIGHEST vapour pressure? Refer to the data in the table above to give a reason for the answer. (2)

[15]



QUESTION 4 (Start on new page.) The diagram below shows how ETHENE can be converted into other organic compounds. The letters A, B, C, D and E represent different organic reactions. 4.1 Write down the type of addition reaction represented by:

4.1.1 A (1)

4.1.2 C (1)

4.2 Consider reaction A. Write down the NAME or FORMULA of the:

4.2.1 Inorganic reactant needed (1)

4.2.2 Catalyst needed (1)

4.3 Consider reaction B. Write down the:

4.3.1 Type of reaction of which it is an example (1)

4.3.2 IUPAC name of compound Y (2) 4.4 Reaction D represents a polymerisation reaction.

4.4.1 Define the term polymerisation. (2)

4.4.2 Write down the IUPAC name of the MONOMER used in reaction D. (1)

4.4.3 Write down the IUPAC name of polymer Z. (1)

4.4.4 Write down the structural formula of polymer Z. (2) 4.5 Reaction E represents a hydrolysis reaction. Write down TWO reaction

conditions needed for this reaction. (2) [15]

C

A

E

B Ethane Compound Y

HBr

D

Polymer Z



Nickel (Ni) rod AgNO3(aq)

QUESTION 5 (Start on new page.) 5.1 A nickel (Ni) rod is placed in a beaker containing a silver nitrate solution, AgNO3(aq), and a reaction takes place. 5.1.1 Define an oxidising agent in terms of electron transfer. (2)

Write down the:

5.1.2 NAME or FORMULA of the reducing agent (1)

5.1.3 Reduction half-reaction that takes place (2) 5.2 A galvanic cell is now set up using a nickel half-cell and a silver half-cell as shown below.

5.2.1 For component Q, write down its:

(a) Name (1)

(b) Function (1) 5.2.1 State TWO standard conditions under which this cell operates. (2) 5.2.3 Which electrode, Ni or Ag, must be connected to the negative terminal of the voltmeter? Give a reason for the answer. (2) 5.2.4 Write down the cell notation for this cell. (3) 5.2.5 Calculate the initial reading on the voltmeter if the cell operates under standard conditions. (4)

Ag

V

Ni

Ni2+(aq) Ag+(aq)

Q



5.3 The development of FUEL CELLS is a huge improvement over internal combustion engines which produces harmful by-products. In a fuel cell, oxygen, O2(g), which is readily available in the atmosphere, and hydrogen, H2(g), reacts to produce energy. 5.3.1 State the energy conversion that takes place in a fuel cell. (1) 5.3.2 Write down the NAME or FORMULA of the emission product formed in a fuel cell. (1) 5.3.3 State ONE disadvantage of fuel cells. (1)

[21] QUESTION 6 (Start on new page.) The simplified diagram below represents an electrolytic cell used for the decomposition of copper(II) chloride, CuCℓ2. A and B represent two carbon electrodes. 6.1 Define the term electrolytic cell. (2) 6.2 In which direction do electrons flow in the external circuit of this cell? Choose from A to B or B to A. (1) 6.3 Which electrode, A or B, is the anode? Give a reason for the answer. (2) 6.4 CuCℓ2(aq) is the electrolyte in the above cell. 6.4.1 Define the term electrolyte. (2) 6.4.2 Write down the SYMBOL of the cation (positive ion) in the electrolyte. (1) 6.4.3 Write down the SYMBOL of the anion (negative ion) in the electrolyte. (1)

A B

CuCℓ2(aq)



6.5 When the cell is functioning, electrode B is coated with a reddish-brown layer. Write down the NAME or SYMBOL of the substance responsible for this layer. (1) 6.6 What observation can be made at electrode A whilst the cell is functioning? (1) 6.7 Explain the answer to QUESTION 6.6 with the aid of a relevant half-reaction. (3) 6.8 State ONE use of electrolytic cells in the industry. (1)

[15]

QUESTION 7 (Start on new page.) In an experiment to demonstrate both REFRACTION and REFLECTION of light, a group of learners allows a light ray to move from medium A to medium B as shown in the diagram below. The optical density of medium A DIFFERS from that of medium B. 7.1 Explain the difference between refraction and reflection of light. (4) 7.2 State the law of reflection. (2) 7.3 Refer to the above diagram and write down the NAME of: 7.3.1 Angle θ (1) 7.3.2 Angle α (1) 7.3.3 Ray 1 (1) 7.3.4 Ray 2 (1) 7.4 Which medium (A or B) in the above diagram has the HIGHER optical density? (1) 7.5 Give a reason for the answer to QUESTION 7.4 by referring to the diagram above. (1)

Medium B α

θ Medium A

Ray 1

Ray 2

n



The learners now aim light ray 1 onto medium B as shown below. X, Y and Z represent three points on the path of the light ray. β represents an angle. 7.6 Define total internal reflection. (2) 7.7 Identify the point (X, Y or Z) on the path of the light ray where each of the following takes place: 7.7.1 Total internal reflection (1) 7.7.2 Refraction (1) 7.8 How does angle β compare to the critical angle for medium B? Choose from GREATER THAN, SMALLER THAN or EQUAL TO. (1) 7.9 Name ONE optical instrument that makes use of total internal reflection. (1)

[18] QUESTION 8 (Start on new page.) The dispersion of white light is illustrated in the diagram below. Light rays 1 to 7 represent a colour band. 8.1 Define the term dispersion of white light. (2)

8.2 State the wave phenomenon responsible for dispersion. (1) 8.3 What is the observed colour band called? (1)

Medium B Ray 1

Medium A

Z

n

n

Y

n

β

X

1

7

Glass prism Air

Witlig



8.4 Which colour in white light is represented by:

8.4.1 Ray 1 (1) 8.4.2 Ray 7 (1) 8.5 Briefly explain why the direction of light ray 7 changes more than that of light ray 1 when they move through the glass prism. (2)

[8] QUESTION 9 (Start on new page.) 9.1 Consider the image formed below to answer the questions that follow.

9.1.1 What type of the lens is used? Choose from CONVEX or CONCAVE. (1)

9.1.2 Give a reason for the answer to QUESTION 9.1.1. (1) 9.1.3 At which position with respect to the lens should an object be placed to obtain the image shown above? Choose from P, Q, R or S as described below. (1)

P Between f and the lens

Q On f

R Between f and 2f

S Beyond 2f


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9.2 An object is placed between f and 2f of a convex lens as shown below.

9.2.1 Copy the above diagram in your ANSWER BOOK. Use two basic

rays to show how the image observed through the lens is formed. (5) 9.2.2 Is the image formed through the lens REAL or VIRTUAL? (1)

[9] QUESTION 10 (Start on new page.) Electromagnetic radiation consists of different types of radiation that can transmit energy without the need of a medium. 10.1 Define the term electromagnetic waves. (2) 10.2 Consider the illustrations A to C below to answer QUESTIONS 10.2.1 to 10.2.3. Write down the following:

10.2.1 The invisible radiation released by the elements in appliance A (1)

10.2.2 The type of radiation responsible for the damage illustrated in B (1)

10.2.3 The type of radiation transmitted in C (1)

10.3 The energy of a photon in a microwave is 3,44 × 10-23 J.

10.3.1 Define the term photon. (2)

10.3.2 Calculate the frequency of the microwave. (3)

10.3.2 Calculate the wavelength of the microwave. (3) [13]

GRAND TOTAL: 150

A B

f

f 2f

2f

Lens Object

C

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https://www.google.co.za/url?sa=i&rct=j&q=&esrc=s&source=images&cd=&ved=2ahUKEwjigsO-mIfjAhUL2aQKHewRBYcQjRx6BAgBEAU&url=https://www.stem.org.uk/resources/elibrary/resource/31372/heat&psig=AOvVaw0A6LAAUTFzJxYLRji4LYCU&ust=1561639999696637

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https://previsecare.files.wordpress.com/2013/04/uvauvbellen.jpg

https://sweetclipart.com/multisite/sweetclipart/files/satellite_dish_outline_0.png

https://sweetclipart.com/multisite/sweetclipart/files/satellite_dish_outline_0.png

Technical Sciences P2 FS/September 2019 Grade 12 Prep. Exam.


INFORMATION SHEETS – PAPER 2 GEGEWENSBLAAIE – VRAESTEL 2

TABLE 1/TABEL 1: PHYSICAL CONSTANTS/FISIESE KONSTANTES

NAME/NAAM SYMBOL/SIMBOOL VALUE/WAARDE

Standard pressure Standaarddruk 1,01 x 105 Pa

Standard temperature Standaardtemperatuur 273 K

Speed of light in a vacuum Spoed van lig in 'n vakuum

c 3,0 x 108 m·s-1

Planck's constant Planck se konstante

h 6,63 x 10-34 J·s

TABLE 2/TABEL 2: WAVES, SOUND AND LIGHT/GOLWE, KLANK EN LIG

or

TABLE 3/TABEL 3: FORMULAE/FORMULES

θ

anode

θ

cathode

θ

cell EEE / θ

anode

θ

katode

θ

sel EEE

θ

oxidation

θ

reduction

θ

cell EEE / θ

oksidasie

θ

reduksie

θ

sel EEE

θ

agent reducing

θ

agent oxidising

θ

cell EEE / θ

ddelreduseermi

θ

ddeloksideermi

θ

sel EEE

p

T

fvf

1T

hfE

c

hE



TABLE 3: THE PERIODIC TABLE OF ELEMENTS TABEL 3: DIE PERIODIEKE TABEL VAN ELEMENTE

1 (I)

2 (II)

3

4

5

6

7

8

9

10

11

12

13 (III)

14 (IV)

15 (V)

16 (VI)

17 (VII)

18 (VIII)

2,1

1 H 1

2 He 4

1,0

3 Li 7

1,5

4 Be 9

2,0

5 B 11

2,5

6 C 12

3,0

7 N 14

3,5

8 O 16

4,0

9 F 19

10 Ne 20

0,9

11 Na 23

1,2

12 Mg 24

1,5

13 Aℓ 27

1,8

14 Si 28

2,1

15 P 31

2,5

16 S 32

3,0

17 Cℓ

35,5

18 Ar 40

0,8

19 K 39

1,0

20 Ca 40

1,3

21 Sc 45

1,5

22 Ti 48

1,6

23 V 51

1,6

24 Cr 52

1,5

25 Mn 55

1,8

26 Fe 56

1,8

27 Co 59

1,8

28 Ni 59

1,9

29 Cu

63,5

1,6

30 Zn 65

1,6

31 Ga 70

1,8

32 Ge 73

2,0

33 As 75

2,4

34 Se 79

2,8

35 Br 80

36 Kr 84

0,8

37 Rb 86

1,0

38 Sr 88

1,2

39 Y 89

1,4

40 Zr 91

41 Nb 92

1,8

42 Mo 96

1,9

43 Tc

2

,2 44

Ru 101

2,2

45 Rh 103

2,2

46 Pd 106

1,9

47 Ag 108

1,7

48 Cd 112

1,7

49 In

115

1,8

50 Sn 119

1,9

51 Sb 122

2,1

52 Te 128

2,5

53 I

127

54 Xe 131

0,7

55 Cs 133

0,9

56 Ba 137

57 La 139

1,6

72 Hf

179

73 Ta 181

74 W

184

75 Re 186

76 Os 190

77 Ir

192

78 Pt

195

79 Au 197

80 Hg 201

1,8

81 Tℓ

204

1,8

82 Pb 207

1,9

83 Bi

209

2,0

84 Po

2,5

85 At

86 Rn

0,7

87 Fr

0,9

88 Ra 226

89 Ac

58 Ce 140

59 Pr

141

60 Nd 144

61 Pm

62 Sm 150

63 Eu 152

64 Gd 157

65 Tb 159

66 Dy 163

67 Ho 165

68 Er

167

69 Tm 169

70 Yb 173

71 Lu 175

90 Th 232

91 Pa

92 U

238

93 Np

94 Pu

95 Am

96 Cm

97 Bk

98 Cf

99 Es

100 Fm

101 Md

102 No

103 Lr

29

Cu 63,5

1,9

Symbol Simbool

Electronegativity Elektronegatiwiteit

Approximate relative atomic mass Benaderde relatiewe atoommassa

Atomic number Atoomgetal

KEY/SLEUTEL



TABLE 4A: STANDARD REDUCTION POTENTIALS TABEL 4A: STANDAARD-REDUKSIEPOTENSIALE

Half-reactions / Halfreaksies (V)

F2(g) + 2e ⇌ 2F + 2,87

Co3+ + e ⇌ Co2+ + 1,81

H2O2 + 2H+ +2e ⇌ 2H2O +1,77

MnO + 8H+ + 5e ⇌ Mn2+ + 4H2O + 1,51

Cℓ2(g) + 2e ⇌ 2Cℓ + 1,36

Cr2O + 14H+ +

6e ⇌ 2Cr3+ + 7H2O + 1,33

O2(g) + 4H+ + 4e ⇌ 2H2O + 1,23

MnO2 + 4H+ + 2e ⇌ Mn2+ + 2H2O + 1,23

Pt2+ + 2e ⇌ Pt + 1,20

Br2(ℓ) + 2e ⇌ 2Br + 1,07

NO + 4H+ + 3e ⇌ NO(g) + 2H2O + 0,96

Hg2+ + 2e ⇌ Hg(ℓ) + 0,85

Ag+ + e ⇌ Ag + 0,80

NO + 2H+ + e ⇌ NO2(g) + H2O + 0,80

Fe3+ + e ⇌ Fe2+ + 0,77

O2(g) + 2H+ + 2e ⇌ H2O2 + 0,68

I2 + 2e ⇌ 2I + 0,54

Cu+ + e ⇌ Cu + 0,52

SO2 + 4H+ + 4e ⇌ S + 2H2O + 0,45

2H2O + O2 + 4e ⇌ 4OH + 0,40

Cu2+ + 2e ⇌ Cu + 0,34

SO + 4H+ + 2e ⇌ SO2(g) + 2H2O + 0,17

Cu2+ + e ⇌ Cu+ + 0,16

Sn4+ + 2e ⇌ Sn2+ + 0,15

S + 2H+ + 2e ⇌ H2S(g) + 0,14

2H+ + 2e ⇌ H2(g) 0,00

Fe3+ + 3e ⇌ Fe 0,06

Pb2+ + 2e ⇌ Pb 0,13

Sn2+ + 2e ⇌ Sn 0,14

Ni2+ + 2e ⇌ Ni 0,27

Co2+ + 2e ⇌ Co 0,28

Cd2+ + 2e ⇌ Cd 0,40

Cr3+ + e ⇌ Cr2+ 0,41

Fe2+ + 2e ⇌ Fe 0,44

Cr3+ + 3e ⇌ Cr 0,74

Zn2+ + 2e ⇌ Zn 0,76

2H2O + 2e ⇌ H2(g) + 2OH 0,83

Cr2+ + 2e ⇌ Cr 0,91

Mn2+ + 2e ⇌ Mn 1,18

Aℓ3+ + 3e ⇌ Aℓ 1,66

Mg2+ + 2e ⇌ Mg 2,36

Na+ + e ⇌ Na 2,71

Ca2+ + 2e ⇌ Ca 2,87

Sr2+ + 2e ⇌ Sr 2,89

Ba2+ + 2e ⇌ Ba 2,90

Cs+ + e- ⇌ Cs - 2,92

K+ + e ⇌ K 2,93

Li+ + e ⇌ Li 3,05

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TABLE 4B: STANDARD REDUCTION POTENTIALS

TABEL 4B: STANDAARD-REDUKSIEPOTENSIALE

Half-reactions / Halfreaksies (V)

Li+ + e ⇌ Li 3,05

K+ + e ⇌ K 2,93

Cs+ + e ⇌ Cs 2,92

Ba2+ + 2e ⇌ Ba 2,90

Sr2+ + 2e ⇌ Sr 2,89

Ca2+ + 2e ⇌ Ca 2,87

Na+ + e ⇌ Na 2,71

Mg2+ + 2e ⇌ Mg 2,36

Aℓ3+ + 3e ⇌ Aℓ 1,66

Mn2+ + 2e ⇌ Mn 1,18

Cr2+ + 2e ⇌ Cr 0,91

2H2O + 2e ⇌ H2(g) + 2OH 0,83

Zn2+ + 2e ⇌ Zn 0,76

Cr3+ + 3e ⇌ Cr 0,74

Fe2+ + 2e ⇌ Fe 0,44

Cr3+ + e ⇌ Cr2+ 0,41

Cd2+ + 2e ⇌ Cd 0,40

Co2+ + 2e ⇌ Co 0,28

Ni2+ + 2e ⇌ Ni 0,27

Sn2+ + 2e ⇌ Sn 0,14

Pb2+ + 2e ⇌ Pb 0,13

Fe3+ + 3e ⇌ Fe 0,06

2H+ + 2e ⇌ H2(g) 0,00

S + 2H+ + 2e ⇌ H2S(g) + 0,14

Sn4+ + 2e ⇌ Sn2+ + 0,15

Cu2+ + e ⇌ Cu+ + 0,16

SO + 4H+ + 2e ⇌ SO2(g) + 2H2O + 0,17

Cu2+ + 2e ⇌ Cu + 0,34

2H2O + O2 + 4e ⇌ 4OH + 0,40

SO2 + 4H+ + 4e ⇌ S + 2H2O + 0,45

Cu+ + e ⇌ Cu + 0,52

I2 + 2e ⇌ 2I + 0,54

O2(g) + 2H+ + 2e ⇌ H2O2 + 0,68

Fe3+ + e ⇌ Fe2+ + 0,77

NO + 2H+ + e ⇌ NO2(g) + H2O + 0,80

Ag+ + e ⇌ Ag + 0,80

Hg2+ + 2e ⇌ Hg(ℓ) + 0,85

NO + 4H+ + 3e ⇌ NO(g) + 2H2O + 0,96

Br2(ℓ) + 2e ⇌ 2Br + 1,07

Pt2+ + 2 e ⇌ Pt + 1,20

MnO2 + 4H+ + 2e ⇌ Mn2+ + 2H2O + 1,23

O2(g) + 4H+ + 4e ⇌ 2H2O + 1,23

Cr2O + 14H+ + 6e ⇌ 2Cr3+ + 7H2O + 1,33

Cℓ2(g) + 2e ⇌ 2Cℓ + 1,36

MnO + 8H+ + 5e ⇌ Mn2+ + 4H2O + 1,51

H2O2 + 2H+ +2 e ⇌ 2H2O +1,77

Co3+ + e ⇌ Co2+ + 1,81

F2(g) + 2e ⇌ 2F + 2,87

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Documents

TECHNICAL SCIENCES P2 - docscientia.co.za · (4) 3.4 Compounds C and D are of similar molecular size. The boiling point of compound D is higher than that of compound C as shown in