NATIONAL SENIOR CERTIFICATE GRADE 10 - TSHS - Physical

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NATIONAL SENIOR CERTIFICATE

GRADE 10 PHYSICAL SCIENCES P2

2007 MARKS: 150 TIME: 3 hours

This question paper consists of 13 pages, 1 periodic table and a 1-page answer sheet..

Physical Sciences/P2 DoE/ 2007 Grade 10


2

INSTRUCTIONS AND INFORMATION 1. 2. 3. 4. 5. 6. 7. 8.

Write your name and/or examination number (and centre number if applicable) in the space provided on the ANSWER SHEET and ANSWER BOOK. Answer ALL the questions. Answer SECTION A on the attached ANSWER SHEET. Answer SECTION B in the ANSWER BOOK. Non-programmable calculators may be used. Appropriate mathematical instruments may be used. Number the answers correctly according to the numbering system used in this question paper. Wherever motivation, discussion, et cetera is required, be brief.



3

SECTION A Answer this section on the attached ANSWER SHEET provided. QUESTION 1: ONE-WORD ANSWERS Give ONE word/term for each of the following descriptions. Write only the word/term next to the question number (1.1 - 1.5) on the ANSWER SHEET.

1.1 Chlorine, bromine, iodine, fluorine and astatine (1) 1.2 Atoms of the same element with different numbers of neutrons (1) 1.3 Protons and neutrons in the nucleus of an atom (1) 1.4 A reaction during which a reactant forms two or more products (1) 1.5 Rain with a pH less than 5,6 (1)

[5]



4

QUESTION 2: MATCHING ITEMS Choose an item from COLUMN B that matches the information in COLUMN A. Write only the letter (A -J) next to the question number (2.1 - 2.5) on the ANSWER SHEET.

COLUMN A COLUMN B 2.1 Group I elements A Na2SO4 2.2 Sodium sulphate B alkali earth metals 2.3 Forces between atoms in molecules C potential energy 2.4 Needed when a positive ion is formed D inter-molecular forces 2.5 Produced during the Haber process E alkali metals F ammonia G Na2SO3 H intra-molecular forces I ionisation energy J nitric acid [5] QUESTION 3: TRUE OR FALSE Indicate whether the following statements are TRUE or FALSE. Write only 'true' or 'false' next to the question number (3.1 - 3.5) on the ANSWER SHEET. If the statement is FALSE, write down the correct statement.

3.1 Salt water is an example of a heterogeneous mixture. (2) 3.2 Rutherford found that the mass of an atom is situated in the nucleus, while

electrons are responsible for the volume of an atom. (2) 3.3 The boiling point of a liquid depends on its intermolecular forces. (2) 3.4 Atoms and molecules are conserved during a chemical reaction. (2) 3.5 Evaporation of water only takes place at the boiling point of water. (2)

[10]



5

QUESTION 4: MULTIPLE-CHOICE QUESTIONS Four possible options are provided as answers to the following questions. Choose the answer and make a cross (X) in the block next to the question number (4.1 – 4.5) on the ANSWER SHEET.

4.1 The diagram below shows three test tubes, X, Y and Z, containing three

different liquids. Three identical marbles are released simultaneously at the surface of each of the three liquids in the test tubes.

Y Z X

Which ONE of the following is a correct description of the three liquids? A The viscosity of the liquid in X is higher than the viscosity of the liquid in

Z; and the liquid in Y has the lowest viscosity.

B The viscosity of the liquid in Y is higher than the viscosity of the liquid in

Z; and the liquid in X has the lowest viscosity.

C The viscosity of the liquid in Z is higher than the viscosity of the liquid in

Y; and the liquid in X has the highest viscosity.

D The viscosity of the liquid in X is lower than the viscosity of the liquid in

Z; and the liquid in Y has the lowest viscosity.

(3)

4.2 Which ONE of the following pairs of elements contains the same number of

neutrons? A He4

2 and H21

B C146 and N14

7

C H11 and H3

1

D He42 and H3

1 (3)



6

4.3 Which ONE of the following has the same electron configuration as a

potassium ion? A Na+

B Mg2+

C Aℓ3+

D Cℓ- (3)

4.4 Temperature is a measurement of the … of the particles of a substance. A potential energy

B average kinetic energy

C internal energy

D kinetic energy (3)

4.5 Which ONE of the following pairs of compounds is an example of the law of

multiple proportions? A NH3 and N2

B NO and NO2

C NaCℓ and NaCℓ2

D H2 and O2 (3) [15]

TOTAL SECTION A: 35



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SECTION B INSTRUCTIONS 1. 2. 3.

Answer this section in the ANSWER BOOK. In ALL calculations, formulae and substitutions must be shown. Round off your answers to TWO decimal places.

QUESTION 5 5.1 Four classes of materials are shown below:

metals ceramics glass plastics Choose from the above list the class to which each of the following materials belongs:

5.1.1 A is flexible, easily melted, can be moulded and does not conduct

electricity. (2)

5.1.2 B is strong, hard, can be bent and is a good conductor of both heat and electricity.

(2)

5.1.3 C is hard, transparent, strong when compressed, but weak when stretched. It is brittle.

(2)

5.2 A learner wants to determine which of a wooden ruler, a strip of aluminium foil

or a polystyrene strip will conduct electricity. The learner is supplied with the following apparatus: Two 1,5 V cells, a light bulb, conducting wires with at least two crocodile clips.

Write an experimental plan that the learner can follow to conduct this investigation. Include the following steps in the experimental plan:

• Investigative question • Hypothesis • Method –steps that the learner can follow to perform the investigation • Circuit diagram – include a circuit diagram to support the method • Results – include a table that the learner can use to record the results • Conclusion – how to use/interpret the results to draw a conclusion

(16)[22]

2 x 1,5 V cells

Light bulb Conducting wires with crocodile clips



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QUESTION 6 During a practical investigation the solubility of potassium nitrate and sodium chloride in water were compared at different temperatures. 6.1 Write down the formulae for sodium chloride and potassium nitrate. (2) The graph below shows the results obtained during the investigation

▪

▪

▪

▪

▪

▪

0 0

50

100

150

200

250

20 40 60 80 100

▪ ▪ ▪ ▪▪▪

Sol

ubili

ty (g

/100

g H

2O)

Temperature (°C)

Sodium chloride

Potassium nitrate

(2) Use the graph to answer the following questions: 6.2 Write down the factor that was kept constant during the investigation. (2) 6.3 Which ONE of the two substances is more soluble at room temperature

(25 °C)? (2) 6.4 Write down the temperature at which the solubility of these substances is

equal. (2) 6.5 What mass of potassium nitrate dissolved at 50 °C? (2) 6.6 What conclusion can be drawn from the graph? (2)

[12]



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QUESTION 7 During a demonstration to illustrate the difference between a chemical and a physical change, the following experiments are performed: Experiment A: Sugar is dissolved in boiling water. Experiment B: Sugar is heated on the stove until a brown syrup is formed.

7.1 Classify each of the changes during the above experiments as a physical or a

chemical change. (2)

7.2 Give ONE reason for your answers to QUESTION 7.1. (2) 7.3

In the northern Kalahari the most commonly used poison for the arrows of the San was made from the larva and pupae of chrysomelid beetles. The contents of the larvae/pupae were squeezed directly on to the arrows. The arrows were then dried over a fire. Is this an example of a chemical or a physical change?

(2) [6]

QUESTION 8 The reaction of metals with oxygen, such as the rusting of iron, is an undesirable chemical reaction. Annually a lot of money is spent to protect steel structures from rusting. Rust is iron(III) oxide, formed when iron reacts with oxygen in the air. Besides oxygen, moisture is necessary for the rusting process.

8.1 Write a balanced chemical equation for the reaction of iron with oxygen to

form iron(III) oxide. (3) 8.2 Classify the reaction in QUESTION 8.1 as a synthesis or a decomposition

reaction. (2) 8.3 Use relative atomic masses and calculate the mass of the reactants and the

products in QUESTION 8.1. Write down an observation on these masses. (4) 8.4 Name the law illustrated in QUESTION 8.3. (2) 8.5 Although South Africa is rich in iron ore, we still have to protect products

made from iron against rust. The available resources will not last for ever and if not protected, we might find ourselves back in the Stone Age in future. Suggest TWO ways in which we can protect iron products from rusting.

(2) [13]



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QUESTION 9 Food production for a growing world population depends heavily on fertilisers. Nitric acid is used for the production of ammonium nitrate, a fertiliser with a high nitrogen content. Word equations for three reactions during the industrial preparation of nitric acid are given below. Write balanced chemical equations for each of these reactions.

9.1 ammonia + oxygen nitrogen monoxide + water (3) 9.2 nitrogen monoxide + oxygen nitrogen(IV) oxide (3) 9.3 nitrogen(IV) oxide + oxygen + water nitric acid (3)

[9] QUESTION 10 Between 1928 and 1937 hydrogen-filled airships were used to transport people between Europe and New York. When the Hindenburg docked at Lakehurst in the USA, in May 1937, the hydrogen in its balloon burst into flames, engulfing the airship in fire and killing 35 of the 97 people on board. The Hindenburg disaster put an end to the use of hydrogen in air travel. Hydrogen on its own will not explode. Even a mixture of hydrogen with air or pure oxygen gives no reaction. However, when this mixture is ignited a fast reaction takes place during which water is produced.

2H2(g) +O2(g) 2H2O(g)

10.1 What is represented by the (g) in the above chemical equation? (2) 10.2 Is the reaction of hydrogen with oxygen exothermic or endothermic? Motivate

your answer with information from the passage. (3)

10.3 During an experiment 2 dm3 of H2(g) reacts with enough O2(g) to produce

H2O(g).

10.3.1 What volume of H2O(g) will be produced during this reaction?

Show your reasoning clearly. (3)

10.3.2 What volume of O2(g) is needed to react with the 2 dm3 of H2(g)? (2) 10.4 Balloons filled with hydrogen gas will rise easily because hydrogen is the least

dense gas. Why is helium the preferred gas when filling balloons to entertain children?

(2) [12]



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QUESTION 11 Water is an exceptional liquid in many ways and makes life on earth possible. The heating curve for water is illustrated below.

100

20

0

80

60

40

Tem

pera

ture

(°C

)

B

D E

C

Time

Application of heat A -20

11.1 Which letter on the graph represents water in the liquid phase? (2) 11.2 Write down the phase change represented by the letter D. (2) 11.3 The temperature does not increase during the phase change mentioned in

QUESTION 11.2. Write down a reason for this observation. (2)

11.4 Explain the meaning of the concept latent heat. (2) 11.5 Name the latent heat required during the phase change represented by the

letter B. (2)

11.6 We normally experience cold weather when the snow on mountains starts to

melt. Give a reason for this phenomenon. (2)

11.7 Which letter, A or C, represents the phase of water with the lower density? (2) 11.8 Refer to your answer to QUESTION 11.7 and briefly explain the impact of this

phenomenon on the environment. (2) [16]



12

QUESTION 12 The diagram below shows activities and industries based on a large river.

Town

Sewage works

Source of river

Water treatment

Power station

Fertiliser Factory

Farms

P

Q R

S

Samples of water were collected at sites P, Q, R and S. The table below shows the temperature and pH of the water, as well as the amount of dissolved oxygen in the water.

Temperature

(°C) pH Oxygen dissolved (parts per million)

Sample from P 4 7 15

Sample from Q 6 8 14

Sample from R 14 6 10

Sample from S 11 6 3

12.1 Give ONE reason why the water supply of the town is taken from the river at

Point P and not closer to the town. (2)

12.2 Give a reason for the big difference in temperature between Points Q and R. (2) 12.3 The river at Point S is becoming choked with fast growing algae. Give

THREE reasons for this observation. (3)

12.4 Despite the presence of enough plant food, no fish is found in the river at and

around point S. Give a reason for this. (2)

Physical Sciences/P2 13 DoE/ 2007 Grade 10

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12.5 Farmers on the farms around point S were told that the water may be a health

risk for humans.

12.5.1 Which ions in the water are most probably responsible for the

health risk? (2)

12.5.2 Briefly describe the effects that the ions mentioned in QUESTION 12.5.1 can have on humans.

(2) [13]

QUESTION 13 A family moved from a town to a farm outside the town. After six months on the farm, they found a white solid forming a layer in the kettle used to boil water. They were very surprised, because this never happened during their stay in town. They realised that the problem must be with the water on the farm. During the analysis of the water on the farm, they were told that the water is hard.

13.1 Explain the term 'hard water'. (2) 13.2 Write down the formula of the solid that precipitated in the kettle. (2) 13.3 Suggest a household substance that the family can use to dissolve the solid

on the inside of the kettle. (2)

13.4 Write down TWO other problems, besides the solid in the kettle, that hard

water can cause for the family. (2)

13.5 The analyst indicated to the family that the hard water can be an advantage

as well. Write down ONE advantage that hard water can have for the family. (2)

13.6 The town gets water from the same source as the farm. The municipality of

the town softens the water using ion exchange. Briefly describes how ion exchange softens the water.

(2) [12]

TOTAL SECTION B:

GRAND TOTAL:

115 150

ciences/P2 DoE/2007 Grade 10

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THE PERIODIC TABLE OF ELEMENTS 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 Aℓ27

1,8

14 Si28

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 Sc45

1,5

22 Ti 48

1,6

23 V 51

1,6

24 Cr52

1,5

25 Mn55

1,8

26 Fe56

1,8

27 Co59

1,8

28 Ni 59

1,9

29 Cu63,5

1,6

30 Zn65

1,6

31 Ga70

1,8

32 Ge73

2,0

33 As75

2,4

34 Se79

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 Nb92

1,8

42 Mo96

1,9

43 Tc

2,

2

44 Ru101

2,2

45 Rh103

2,2

46 Pd 106

1,9

47 Ag108

1,7

48 Cd112

1,7

49 In115

1,8

50 Sn119

1,9

51 Sb122

2,1

52 Te128

2,5

53 I

127

54 Xe 131

0,7

55 Cs 133

0,9

56 Ba 137

57 La139

1,6

72 Hf 179

73 Ta181

74 W184

75 Re186

76 Os190

77 Ir

192

78 Pt 195

79 Au197

80 Hg201

1,8

81 Tℓ204

1,8

82 Pb207

1,9

83 Bi209

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 Sm150

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

Approximate relative atomic mass Benaderde relatiewe atoommassa

Symbol Simbool

Atomic number Atoomgetal

29 Cu 63,5

1,9 Electronegativity

Elektronegatiwiteit

KEY / SLEUTEL

Physical S

Copyri

Physical Sciences/P2 DoE/2007 Grade 10

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EXAM NO: NAME:

PHYSICAL SCIENCES GRADE 10 ANSWER SHEET

FISIESE WETENSKAPPE GRAAD 10 ANTWOORDBLAD QUESTION 1 / VRAAG 1 QUESTION 2 / VRAAG 2

1.1

(1)

2.1

(1)

1.2

(1)

2.2

(1)

1.3

(1)

2.3

(1)

1.4

(1)

2.4

(1)

1.5

(1)

2.5

(1) [5] [5] QUESTION 3 / VRAAG 3

3.1

(2)

3.2

(2)

3.3

(2)

3.4

(2)

3.5

(2)[10]

QUESTION 4 / VRAAG 4 4.1 A B C D 4.2 A B C D 4.3 A B C D 4.4 A B C D 4.5 A B C D [5 x 3 = 15]

TOTAL SECTION A / TOTAAL AFDELING A: 35

NATIONAL SENIOR CERTIFICATE GRADE 10 - TSHS - Physical

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