TIME

1 hour 15 minutes.

INSTRUCTIONS TO CANDIDATES

Write your Centre Number and Candidate Number in the spaces provided at the top of this page.Write your answers in the spaces provided in this question paper.Answer all nine questions.

INFORMATION FOR CANDIDATES

The total mark for this paper is 90.Figures in brackets printed down the right-hand side of pages indicate the marks awarded to each question or part question.Quality of written communication will be assessed in Questions 3(a) and 9(a).A Data Leaflet, which includes a Periodic Table of the Elements,is included in this question paper.

12123

For Examiner’suse only

Question Number Marks

1

2

3

4

5

6

7

8

9

TotalMarks

General Certificate of Secondary Education2017–2018

Centre Number

Candidate Number

Double Award Science: Chemistry

Unit C2 Higher Tier

[GSD52]TUESDAY 13 NOVEMBER 2018, MORNING

GSD

52

Examiner Only

Marks Remark

12123 2

1 This question is about the reactivity series of metals.

(a) (i) Describe three things you would observe when potassium metal reacts with cold water.

1.

2.

3.

[3]

(ii) Name the solution formed when potassium reacts with water.

[1]

(b) Iron does not react readily with cold water but does react with steam.

(i) Complete the word equation for the reaction of iron with steam.

iron + steam + [2]

(ii) What colour is the solid product from the reaction of iron with steam?

Circle the correct answer.

black white blue yellow [1]

(iii) Name one other metal which reacts with steam but not with cold water.

[1]

(iv) Name a metal which does not react with steam or water.

[1]

Examiner Only

Marks Remark

12123 3 [Turn over

(c) Magnesium ribbon burns in air. The product is magnesium oxide.

(i) Describe how you would safely carry out this experiment in the laboratory.

[2]

(ii) State two things you would see when magnesium ribbon burns in air.

1.

2. [2]

Examiner Only

Marks Remark

12123 4

2 This question is about the non-metals carbon and sulfur and their compounds.

(a) Carbon dioxide is dissolved in water to make it fizzy.

(i) Complete the symbol equation for the reaction between carbon dioxide and water.

CO2 + H2O [1]

(ii) What colour will be observed if universal indicator is added to water containing dissolved carbon dioxide?

Circle the correct colour.

blue green orange [1]

(b) Sulfur will burn in oxygen to form the gas sulfur dioxide.

(i) What colour is the flame produced when sulfur burns in oxygen?

[1]

(ii) What word can be used to describe the smell of the gas sulfur dioxide?

Circle the correct answer.

odourless pungent sweet toxic

[1]

(c) Sulfur dioxide reacts with rain water to form acid rain.

State three different effects of acid rain.

1.

2.

3. [3]

Examiner Only

Marks Remark

12123 5 [Turn over

3 (a) A new limestone quarry is to be created on the outskirts of a scenic village.

The limestone will be blasted from the quarry rock and then taken in dumper trucks to a nearby crushing plant. The crushed limestone will then be carried in heavy lorries for use in various parts of the country.

Describe the advantages and disadvantages, to the local village

people, of having a quarry situated near to where they live.

In this question you will be assessed on your written communication skills including the use of specialist scientific terms.

Advantages:

Disadvantages:

[6]

(b) When limestone is broken down using heat, bonds are broken and new bonds are made. What energy change occurs when a chemical bond is made?

[1]

Examiner Only

Marks Remark

12123 6

4 This question is about hard water and soft water.

(a) Water can be described as soft water, temporary hard water or permanent hard water.

(i) Describe an experiment to show that a sample of water is soft water.

[2]

(ii) Describe an experiment to show that a sample of hard water is temporary hard water.

[3]

(b) Explain in terms of the ions present, how hard water, containing dissolved calcium ions, can be softened using sodium carbonate.

[3]

Examiner Only

Marks Remark

12123 7 [Turn over

5 This question is about relative formula masses and using and understanding the term mole.

(a) Calculate the relative formula mass (RFM) of each of the following substances.

(relative atomic masses: H = 1, N = 14, O = 16, S = 32, Ag = 108)

(i) silver nitrate AgNO3

[1]

(ii) ammonium sulfate (NH4)2SO4

[1]

(b) What do you understand by the term “a mole of a substance”?

A mole of a substance is

[2]

(c) The relative formula mass of aluminium oxide is 102.

(i) What is the mass of 0.40 moles of aluminium oxide?

g [1]

(ii) Scale is important in industrial chemistry. How many moles are there in 51 kg of aluminium oxide?

Show your working out.

[2]

Examiner Only

Marks Remark

12123 8

(d) The final part of this question is about concentrations of solution, the effect that dilution or mixing has on the concentration of a solution and the number of moles in the solution.

(i) If 600 cm3 of water is added to 400 cm3 of a 2 mol/dm3 solution of sulfuric acid, what happens to the concentration of acid in the solution? Tick (3) the correct answer.

It stays the same

It becomes 40% of its original value

It becomes 60% of its original value [1]

(ii) If 600 cm3 of water is added to 400 cm3 of a 2 mol/dm3 solution of sulfuric acid, what happens to the number of moles of acid in the solution? Tick (3) the correct answer.

It stays the same

It becomes 40% of its original value

It becomes 60% of its original value [1]

(iii) 0.5 dm3 of a 2 mol/dm3 solution of sulfuric acid is added to another 0.5 dm3 of a 2 mol/dm3 solution of sulfuric acid. What is the concentration of the new 1 dm3 solution?

Tick (3) the correct answer.

1 mol/dm3

2 mol/dm3

4 mol/dm3 [1]

Examiner Only

Marks Remark

12123 9 [Turn over

6 This question is about oxidation, reduction and redox reactions.

(a) Listed below are four chemical equations. Place a tick (3) beside the two equations that show oxidation reactions.

Tick (3)

2HBr H2 + Br2

CuSO4 + 5H2O CuSO4.5H2O

CH4 + 2O2 CO2 + 2H2O

HCl + NaOH NaCl + H2O [2]

(b) The reaction of lead nitrate solution and aluminium powder can be represented by the two half equations shown below.

Pb2+ + 2e– Pb

Al Al3+ + 3e–

Explain in terms of electron transfer the oxidation and reduction reactions that are happening.

[2]

(c) The manufacture of iron can be represented by the following chemical equation.

Fe2O3 + 3CO 2Fe + 3CO2

Using your knowledge and the equation, identify what is being oxidised and what is being reduced.

being oxidised:

being reduced: [2]

Examiner Only

Marks Remark

12123 10

7 This question is about rates of reaction and factors that affect rate.

(a) A group of students were investigating how surface area affects the rate of the reaction between excess dilute hydrochloric acid and 0.25 g of calcium carbonate lumps.

They collected the following results for the reaction carried out at 20 ºC and presented the information in the graph below.

Time/s 0 20 40 60 80 100 120 140 160 180 200

Volume of gas/cm3 0 16 30 40 48 54 56 58 60 60 60

0

10

20

30

40

50

60

70

80

40 80 120 1600

volu

me

of g

as/c

m3

20 60 100 140 180

time/s

200

Use the graph and your knowledge to answer the following questions.

(i) What volume of gas was formed in the first 50 seconds?

[1]

(ii) How many seconds did it take for all of the solid to react?

[1]

Examiner Only

Marks Remark

12123 11 [Turn over

(iii) The students repeated the experiment using 0.25 g of powdered calcium carbonate.

On the same axes draw the curve you would expect to get for the reaction carried out using 0.25 g of powdered calcium carbonate. You should assume that all other variables were kept the same as in the original experiment. [2]

(b) Use collision theory to explain why increasing the temperature and increasing the concentration will increase the rate of a reaction.

(i) Increasing the temperature of the reaction mixture.

[3]

(ii) Increasing the concentration of an acid.

[2]

(c) Two students are reacting sulfuric acid with an excess of powdered magnesium to form hydrogen gas.

Student A uses 500 cm3 of 0.5 mol/dm3 sulfuric acid. Student B uses 250 cm3 of 1.0 mol/dm3 sulfuric acid.

What difference, if any, will there be between the reactions carried out by student A and student B? Your answer should refer to both the rate of the reaction and the volume of hydrogen gas produced.

rate of reaction:

volume of hydrogen gas:

[2]

Examiner Only

Marks Remark

12123 12

8 This question is about nitrogen gas and ammonia gas.

(a) (i) Give two physical properties of nitrogen gas.

1.

2. [2]

(ii) Nitrogen gas can be used to make ammonia. Give one other use of nitrogen gas.

[1]

(b) Ammonia is produced from nitrogen and hydrogen gas in the Haber process.

(i) Name the catalyst used in the Haber process.

[1]

(ii) What pressure is used in the Haber process? Include units with your answer.

[2]

(iii) Write a balanced symbol equation for the production of ammonia in the Haber process.

[4]

(iv) Give two uses of ammonia.

1.

2. [2]

Examiner Only

Marks Remark

12123 13 [Turn over

9 (a) Methanoic acid and ethanoic acid are both members of the carboxylic acid homologous series.

• Define the term homologous series. • Describe the similarities you would expect in the physical

properties and chemical reactions of methanoic acid and ethanoic acid.

In this question you will be assessed on using your written communication skills including the use of specialist science terms.

Definition of the term homologous series

Expected similarities in the physical properties and chemical reactions of methanoic acid and ethanoic acid

[6]

Examiner Only

Marks Remark

12123 14

(b) Hexane and hexene are both colourless liquids. Describe a chemical test you could carry out on both these liquids to

determine which one is the alkene. Test:

Expected result with hexene:

Expected result with hexane:

[4]

(c) Write a balanced symbol equation for the complete combustion of hexene, C6H12.

[3]

(d) Describe what you would observe if some dilute ethanoic acid was added, in excess, to a flask containing calcium carbonate powder.

[3]

THIS IS THE END OF THE QUESTION PAPER

Permission to reproduce all copyright material has been applied for.In some cases, efforts to contact copyright holders may have been unsuccessful and CCEAwill be happy to rectify any omissions of acknowledgement in future if notified.

12123

SYMBOLS OF SELECTED IONS

chemistrydouble awardsingle award

DATA LEAFLETFor the use of candidates taking

Science: Chemistry,

Science: Double Award or Science: Single Award

Copies must be free from notes or additions of any kind. No other type of data booklet or information

sheet is authorised for use in the examinations.

Contents

PagePeriodic Table of the Elements

2–3Symbols of Selected Ions

4Solubility of Common Salts

4

gcseMost chlorides, bromides and iodidesEXCEPT silver and lead chlorides, bromides and iodides

SOLUBILITY IN COLD WATER OF COMMON SALTS, HYDROXIDES AND OXIDES

Soluble

Insoluble

Most carbonatesEXCEPT sodium, potassium and ammonium carbonates

Most hydroxides EXCEPT sodium, potassium and ammonium hydroxides

Most oxides EXCEPT sodium, potassium and calcium oxides which react with water

All sodium, potassium and ammonium salts

All nitrates

Most sulfates EXCEPT lead and barium sulfatesCalcium sulfate is slightly soluble

Positive ions Negative ionsName Symbol Name Symbol

Ammonium +4NH Carbonate −2

3CO

Chromium(III) +3Cr Dichromate −272OCr

Copper(II) +2Cu Ethanoate −COOCH3

Iron(II) +2Fe Hydrogen carbonate −3HCO

Iron(III) +3Fe Hydroxide −OH

Lead(II) +2Pb Methanoate −HCOO

Silver +Ag Nitrate −3NO

Zinc +2Zn Sulfate −24SO

Sulfite −23SO

227

89

139

57

256

101

223

87

226

88

261

104

262

105

263

106

262

107

265

108

266

109

269

110

272

111

285

112

140

58

141

59

144

60

147

61

150

62

152

63

157

64

159

65

162

66

165

67

167

68

169

69

173

70

175

71232

90

231

91

238

92

237

93

242

94

243

95

247

96

245

97

251

98

254

99

253

100

254

102

257

103

133

55

137

56

178

72

181

73

184

74

186

75

190

76

192

77

195

78

197

79

201

80

89

39

91

40

103

45

85

37

88

38

93

41

96

42

99

43

101

44

106

46

108

47

112

48

131

54222

86

210

85

210

84

209

83

207

82

204

81

84

36

79

34

73

32

40

20

39

19

45

21

48

22

51

23

52

24

55

25

56

26

59

27

59

28

64

29

65

30

11

5

12

6

14

7

16

8

19

9

20

10

4

2

40

18

35.5

17

32

16

31

15

28

14

27

1370

31

75

33

80

35115

49

119

50

122

51

128

52

127

53

23

11

24

12

7

3

9

4

1

1

* 58 – 71 Lanthanum series† 90 – 103 Actinium series

a = relative atomic mass(approx)x = atomic symbolb = atomic number

THE PERIODIC TABLE OF ELEMENTSGroup

ab x

1 2 3 4 5 6 7

0

*

†