EdExcel IGCSE Chemistry Past Paper Questions 2013

Islamia English School

Chemistry past Paper Questions First Term

2013

Guided By Sir.Sadiq Amin

Paper References Acids, Bases, Salts and Titration Calculation Year

Month

Paper

Question Number

Part

2000

January

1

1 4

c a b c d c a b d a b

2000

2001 2001 2002 2004

May

January May May January

1

6 1

1 1 1 1

8 7 13 8

2004

May

1

14 9 14

2005

May

1

15

2006 2006

January May

1 1

2007 2008 2009

May May January

1 1 1

Sub Part

I, ii, iii

a b

I, ii, ii, ii, iv

a a b c d a b

i

iii, iv

7 12 14 15 11 14 1

2009 2010 2010 2011

May January May January

1 1 1 1

2011

May

1

2012

2013

January

1

2012

May

January

1

10 13 3 7 12 3 6 10 11 3 4 1 2 3 8 3

a

I, ii

d e 1 b

Acids, Bases, Salts and Titration Calculation Year

Month

Paper

Question Number

Part

2003

May

2

3

a

2004

January

2

4

a

Sub Part

b 2005

January

2

a b

2005

May

2

6

2006

January

2

2

c

2007

January

2

6

a

I, iii 2

2007

May

2

1

2008

January

2

5

2008

May

2

7

c

7

a

8

b

2009

January

2

8

a

2009

May

2

1

a

7

d

6

a

2010

January

2

I,ii

iii

I, ii

b c 9

a b

2010

May

2

3 5

2011

January

2

3

b

2011

May

2

8

a

i

b d 2012

January

2

3 8

2012

May

2

3

a

2013

January

2

3

c

5 3

7

Halogens Year

Month

Paper

Question Number

Part

2000

January

1

6

a

Sub Part

b 2001

January

1

7

2004

January

1

11

2006

January

1

9

2008

January

1

8

b

a b c

2008

May

1

5

2011

May

1

5

a

2012

May

1

4

d

I, ii, iii

e

Halogens Year

Month

Paper

Question Number

Part

2005

January

2

6

2006

January

2

2

2007

January

2

4

2009

January

2

4

2009

May

2

9

b

2010

January

2

9

b

Sub Part

a

4

2010

May

2

7

b

Reversible Reactions Year

Month

Paper

Question Number

Part

2000

January

1

8

c

2001

January

1

5

a

2001

May

1

3

a

Sub Part

b c 2006

January

1

13

2007

January

1

7

2008

January

1

11

2010

January

1

10

2012

January

1

3

2013

January

1

8

a

I, ii, iii

c

Reversible Reactions Year

Month

Paper

Question Number

Part

2003

May

2

2

b

Sub Part

c 4

d e 5

2004

January

2

6

d

2004

May

2

4

c

I,ii

d 2005

January

2

9

a

2006

May

2

7

a

2007

January

2

5

a b

2007

May

2

7

a

2009

May

2

7

a

2012

May

2

5

d

I,ii

6

7

8

9

Paper 1 Acid, Alkali and Salts and Titration Calculation Monday 17 January 2000 Q1 (c) Describe a chemical test to distinguish between a solution of hydrogen chloride in methylbenzene and a solution of hydrogen chloride in water. Describe the result with each solution.

(3 marks) 4. The acid concentration in red wine can be determined by titration against 0.010 mol dm-3 sodium hydroxide solution. The colour of the red wine is first removed by the use of activated charcoal. One acid present is tartaric acid, which like sulphuric acid has a molecule containing two replaceable protons. (a) Name a suitable indicator for an acid-alkali titration. State the colour of this indicator in acid and alkali solutions. Indicator Color in acid Color in alkali (3 marks) (b) Why is the color of the wine removed before titration?

(1mark) (c) In a titration, 10cm3 of 0.010mol dm-3 sodium hydroxide solution were required to neutralize 25 cm3 of wine. Given that two moles of sodium hydroxide will neutralize one mole of tartaric acid calculate (i) The number of moles of sodium hydroxide used in the titration;

10

(ii) The number of moles of tartaric acid in the volume of wine used in the titration, and the concentration of tartaric acid in mol dm-3.

(3marks) (d) Even if the titration is carried out without experimental error, it gives a too high a value for the real concentration of tartaric acid in the wine. Suggest a reason for this

(1 mark) 6 (c) A sample of sea water contains 0.1g dm-3 of bromide ions. (i)

What volume of sea water produces one mole of bromine molecules?

(ii)

What volume of chlorine gas is required to produce 8g of bromine from this sea water?

(5 marks) 11

Tuesday 23 May 2000 1. This question is about four acids: Ethanoic acid

hydrochloric acid

nitric acid

sulphuric acid

(a) Which of these acids is a weak acid? Explain why this acid is regarded as weak.

(2 marks) (b) Which one of these acids can be used to prepare an acid salt? Give the name of an acid salt and write an equation for its preparation.

(3 marks) (d) In a titration, 25.0 cm3 of sodium hydroxide solution of concentration 1.0 mol dm-3 were exactly neutralized by 20.0 cm3 of dilute nitric acid. NaOH (aq) + HNO 3 (aq) → NaNO 3 (aq) + H 2 O R

(l)

(i) How many moles of sodium hydroxide are in 25.0 cm3 of sodium hydroxide solution of concentration 1.0 mol dm-3?

(ii) Calculate the concentration, in mol dm-3, of the dilute nitric acid.

(iii) What volume of this dilute nitric acid would contain exactly 1 mole of hydrogen ions?

(3 marks) 12

Tuesday 16 January 2001 8 (a) Describe how you could use a 0.10 mol dm-3 solution of sodium hydroxide to determine the concentration of a solution of sulphuric acid?

(12 marks) 13

Tuesday 22 May 2001 7 (b) Copper powders do not react with dilute sulphuric acid. Starting with copper powder and dilute sulphuric acid, describe how you would obtain pure dry sample of blue (hydrated) copper (II) sulphate.

(10 marks) 14

Tuesday 21 May 2002 13. The following equation represents the reaction between magnesium oxide and dilute sulphuric acid. MgO (s) + H 2 SO 4(aq) → MgSO 4 (aq) + H 2 O (l) R

(a) What is the relative formula mass of magnesium oxide?

(b) How many moles of sulphuric acid react with 2.0 g of magnesium oxide?

(c) What volume of 2.0mol dm-3 sulphuric acid, in cm3, would be needed to react with 2.0 g of magnesium oxide?

(d) Calculate the mass, in g, of magnesium sulphate crystals, MgSO 4 .7H 2 O, that would be formed by the reaction of 2.0g of magnesium oxide and an excess of dilute sulphuric acid.

(e) Calculate the percentage by mass of magnesium in magnesium sulphate crystals.

(7 marks)

Tuesday 13 January 2004 8 (a) Ammonia can be prepared using an ammonium salt and a strong alkali. (i) Name a suitable strong alkali.

(ii) Write an equation for a reaction that could be used to prepare ammonia gas.

(iii) Concentrated sulphuric acid is a common drying agent for gases. Why it is it not used to dry ammonia?

(iv) Name a suitable drying agent for ammonia. 15

(b) The reaction between ammonia and nitric acid is represented by the equation NH 3 (g) +HNO 3 (aq) → NH 4 NO 3 (aq) R

Calculate the mass of ammonia, in grams that would be required to neutralize 50 cm3 of nitric acid of concentration of 2 mol dm-3. (i) Number of moles of nitric acid in 50 cm3 =

(ii) Mass of ammonia =

14. A student was asked to find the relative molecular mass of a solid acid. She weighed out accurately a sample of the acid and then made 250 cm3 of solution in a graduated flask. She took 25.0 cm3 portions of the solution and titrated them against aqueous sodium hydroxide of concentration 0.20 mol dm-3 which was contained in a burette. Phenolphthalein was used as the indicator. (a) (i) What would have been the colour change for phenolphthalein at the end – point?

(ii) Why was phenolphthalein used rather than universal indicator?

(iii) Give the name of the piece of apparatus that the student would have used to accurately transfer 25.0 cm3 of acid from the graduated flask.

(b) The following results were recorded:

Table 1 Mass of weighing bottle + sample of acid Mass of weighing bottle empty Mass of sample acid Final burette reading/ cm3 Initial burette reading/ cm3 Volume of NaOH added/cm3

23.45 0.00

= = =

Table 2 23.75 1.20

23.10 0.65

16

(i) Complete Tables 1 and 2 to show the mass of acid used and the volume of sodium hydroxide in each titration. (ii) Decide which titration figures should be used to calculate the most accurate mean value for the volume sodium hydroxide added and then perform the calculation.

Titration figures used to calculate the mean:

Mean Value:

(c) Using A to represent the anion of the acid, the equation for the reaction is H 2 A + 2NaOH → Na 2 A + 2H 2 O

(i) The concentration of sodium hydroxide was 0.20 mol dm-3. How many moles of sodium hydroxide were present in the mean volume?

(ii) Use the mole ratio from the equation to determine how many moles of acids reacted with this number of sodium hydroxide. The value obtained is equal to the number of moles of acid in 25.0 cm3 of solution.

(iii) How many moles of acids were present in 250 cm3 of solution?

(iv) Use the number moles of acid in 250 cm3 of solution and the mass of the acid to calculate the relative formula mass.

(12 marks)

17

Tuesday 18 May 2004 9 (b) Two solutions of hydrogen chloride were prepared. Solution X was a solution in methylbenzene, an organic solvent. Solution Y was a solution in water. (i) Solid sodium chloride was added to a sample of each solution. No reaction was observed with solution X but effervescence occurred with solution Y. Explain the difference in behavior of the two solutions.

14.In an experiment, two plugs of cotton wool soaked respectively in concentrated aqueous ammonia and concentrated hydrochloric acid was placed at either end of a long glass tube. After a short time, white ‘smoke’ was observed in the tube.

(a) Ammonia gas is produced at the plug of cotton wool soaked in concentrated aqueous ammonia. Name the gas produced at the plug of cotton wool soaked in concentrated hydrochloric acid.

(b) Name the process by which the gases move through the tube.

(c) Write a sentence comparing the relative speeds with which the gases move along the tube.

(d) Give the formula of the chemical responsible for the white smoke.

18

Tuesday 18 January 2005  (No questions related to Acids, bases, salts and titration calculation.)

Tuesday 17 May 2005 15 (a) Magnesium react with dilute sulphuric acid to produce hydrogen gas. Write an equation for this reaction.

(b) In an experiment, x g of magnesium was added to excess dilute sulphuric acid of concentration 1moldm-3. The reaction stopped after 100 s and produced 120 cm3 of hydrogen gas measured at room temperature and normal atmospheric pressure. (iii) Calculate the value of x.

(iv) Calculate the volume of dilute sulphuric acid of concentration 1 mol dm-3 that reacted with x g of magnesium in the experiment.

Tuesday 17 January 2006 7. Sulphamic acid, NH 2 SO 3 H, is a weak acid that is used to remove lime scale, calcium carbonate from shower heads. The equation for the reaction is: CaCO 3 (s) + 2NH 2 SO 3 H (aq) → Ca(NH 2 SO 3 ) 2 (aq) + CO 2 (g) + H 2 O (l) R

(a) Describe a test to show that the Sulphamic acid is a weak acid.

(b) Describe a test to show that the gas evolved is carbon dioxide.

(c) Calculate the relative atomic mass of Sulphamic acid. 19

(d) Calculate the mass of Sulphamic acid needed to remove 1.0g of lime scale.

(Total 7 marks)

Tuesday 16 May 2006 12. A group two metal carbonate, MCO 3 reacts with dilute hydrochloric acid according to the following equation. MCO 3 + 2HCl → MCl 2 + H 2 O + CO 2

When 2.5 g of the metal carbonate was added to an excess of dilute hydrochloric acid, 600 cm3 of carbon dioxide gas was produced, measured at room temperature and atmospheric pressure. (a) How many moles of carbon dioxide were formed?

(b) Use your answer to (a) and the equation to deduce how many moles of the metal carbonate are equivalent to 2.5 g.

(c) Calculate the mass of one mole of MCO 3.

(d) Find the relative atomic mass of M and identify the metal.

(e) Give details of simple test you would carry out to confirm the identity of metal M.

(Total 8 marks)

20

14. When hydrated zinc sulphate is heated, it loses water to become anhydrous zinc sulphate. ZnSO 4 .xH 2 O → ZnSO 4 + xH 2 O

A sample of hydrated zinc sulphate was placed in an evaporating basin and heated until all the water had been lost. The following masses were recorded. Mass of evaporating dish when empty = 34.63 g Mass of evaporating basin +hydrated zinc sulphate = 40.37 Mass of evaporating basin + anhydrous zinc sulphate = 37.85 g (a) Calculate the relative formula mass of anhydrous zinc sulphate, ZnSO 4.

(b) (i) What mass of anhydrous zinc sulphate was formed?

(ii) What mass of water was lost?

(iii) Calculate the value of x in the formula ZnSO 4 .xH 2 O.

(Total 6 marks)

Tuesday 18 January 2007  (No questions related to Acids, bases, salts and titration calculation.)

21

Tuesday 15 May 2007

22

23

Monday 14 January 2008  (No questions related to Acids, bases, salts and titration calculation.)

Tuesday 13 May 2008

24

Wednesday 14 January 2009

25

Wednesday 20 May 2009

26

Wednesday 13 January 2010

27

28

Tuesday 25 May 2010

Wednesday 12 January 2011

29

30

31

32

Wednesday 25 May 2011

33

34

35

36

37

38

39

Friday 13 January 2012

40

41

42

Monday 21 May 2012

43

44

45

46

47

48

Monday 14 January 2013

49

50

Paper 2 Acid, Alkali and Salts and Titration Calculation Thursday 22 May 2003 3. Silver nitrate solution is used as a reagent in the laboratory. (a) Starting with solid silver nitrate, describe how you would prepare exactly 100 cm3 of silver nitrate solution of concentration 0.01 mol dm-3. You should give sufficient detail to allow another chemist to repeat your method.

(5 marks)

Thursday 15 January 2004 4. Nickel, Ni, is a transition metal in the same row of the Periodic Table as copper. (a) Describe, giving essential details, how you could prepare crystals of nickel (II) sulphate, NiSO 4 .6H 2 O, starting from nickel (II) oxide and dilute sulphuric acid. (Diagrams not required) Method

51

(5 marks) (b) The overall equation for the preparation is: NiO (s) + H 2 SO 4 (aq) 5H 2 O (l) → NiSO 4 .6H 2 O (s) R

Use the equation to calculate the maximum mass, in grams, of nickel (II) sulphate crystals that could be obtained from 3.75g of nickel (II) oxide.

(3 marks)

Thursday 20 May 2004  (No questions related to Acids, bases, salts and titration calculation.)

Thursday 20 January 2005 8 (a) (i) Describe, giving essential practical details, how you would perform a titration to find the concentration, in mol dm-3, of a solution of sulphuric acid. You are provided with aqueous sodium hydroxide of concentration 0.50 mol dm-3 and phenolphthalein indicator.

52

(ii) The equation for the reaction between sodium hydroxide and sulphuric acid is H 2 SO 4 + 2NaOH → Na 2 SO 4 + 2H 2 O

In a titration, 25.0 cm3 of H 2 SO 4 required 26.5 cm3 of 0.50 mol dm-3 NaOH for neutralization. Calculate the concentration of H 2 SO 4 in mol dm-3.

(iii) Sodium sulphate forms crystals of formula Na 2 SO 4 .x2H 2 O. Describe briefly how a sample of the pure, dry crystals can be obtained (use the information given in (ii) above).

(16 marks) (b) 6.44g of Na 2 SO 4. x2H 2 O was heated to remove the water of crystallization and a loss in mass of 3.60g was recorded. Use these figures to calculate the number of moles of water of crystallization, x, in 1 mole of Na 2 SO 4. x2H 2 O.

53

(4 marks)

Thursday May 2005

54

55

Thursday 19 January 2006 2.

56

Thursday 18 May 2006  (No questions related to Acids, bases, salts and titration calculation.)

Monday 22 January 2007

57

Thursday 17 May 2007

58

Thursday 17 January 2008 59

60

61

7.

62

Thursday 15 May 2008

63

8.

64

Monday 19 January 2009 8.

Friday 22 May 2009

65

7.

66

Monday 18 January 2010

67

68

69

Friday 28 May 2010

70

71

72

Monday 17 January 2011 3.

73

Wednesday 15 June 2011

74

75

76

Friday 20 January 2012

77

78

Tuesday 29 May 2012

79

Wednesday 16 January 2013 3.

80

81

82

83

84

85

Paper 1 Halogens Monday 17 January 2000

(5 marks)

Tuesday 23 May 2000  (No questions related to Halogens.)

86

Tuesday 16 January 2001 7.

Tuesday 22 May 2001  (No questions related to Halogens.)

Tuesday 21 May 2002  (No questions related to Halogens.)

Tuesday 20 May 2003  (No questions related to Halogens.)

Tuesday 13 January 2004

87

Tuesday 18 May 2004  (No questions related to Halogens.)

Tuesday 18 January 2005  (No questions related to Halogens.)

Tuesday 17 January 2006

(Total 5 marks)

Tuesday 16 May 2006  (No questions related to Halogens.)

88

Thursday 18 January 2007  (No questions related to Halogens.)

Tuesday 15 May 2007  (No questions related to Halogens.)

Monday 14 January 2008

89

Tuesday 13 May 2008

90

Wednesday 14 January 2009  (No questions related to Halogens.)

Wednesday 20 May 2009  (No questions related to Halogens.)

Wednesday 13 January 2010  (No questions related to Halogens.)

Tuesday 25 May 2010  (No questions related to Halogens.)

Wednesday 12 January 2011  (No questions related to Halogens.)

Wednesday 25 May 2011

91

Friday 13 January 2012  (No questions related to Halogens.)

Monday 21 May 2012 4.

Monday 14 January 2013  (No questions related to Halogens.)

92

Paper 2 Halogens

Thursday 22 May 2003  (No questions related to Halogens.)

Thursday 15 January 2004  (No questions related to Halogens.)

Thursday 20 May 2004  (No questions related to Halogens.)

Thursday 20 January 2005

93

94

(25 MARKS)

Thursday 19 May 2005  (No questions related to Halogens.)

Thursday 19 January 2006

Thursday May 2006  (No questions related to Halogens.)

95

Monday 22 January 2007

96

Thursday 17 May 2007  (No questions related to Halogens.)

Thursday 17 January 2008  (No questions related to Halogens.)

Thursday 15 May 2008  (No questions related to Halogens.)

Monday 19 January 2009

97

Friday 22 May 2009

98

Monday 18 January 2010

99

Friday 18 May 2010 7.

Monday 17 January 2011  (No questions related to Halogens.)

Wednesday 15 June 2011  (No questions related to Halogens.)

Friday 20 January 2012  (No questions related to Halogens.)

Tuesday 29 May 2012  (No questions related to Halogens.)

Wednesday 16 January 2013  (No questions related to Halogens.)

100

Paper 1 Reversible Reactions

Monday 17 January 2000 8.

Tuesday 23 May 2000  (No questions related to Reversible Reactions.)

Tuesday 16 January 2001

101

Tuesday 22 May 2001

102

Tuesday 21 May 2002  (No questions related to Reversible Reactions.)

Tuesday 20 May 2003  (No questions related to Reversible Reactions.)

Tuesday 13 January 2004  (No questions related to Reversible Reactions.)

Tuesday 18 January 2003  (No questions related to Reversible Reactions.)

Tuesday 17 May 2005  (No questions related to Reversible Reactions.)

Tuesday 17 January 2006

103

(Total 10 Marks)

Tuesday 16 May 2006  (No questions related to Reversible Reactions.)

Thursday 18 January 2007

104

Tuesday 15 May 2007  (No questions related to Reversible Reactions.)

Monday 14 January 2008

105

Tuesday 13 May 2008  (No questions related to Reversible Reactions.)

Wednesday 14 January 2009  (No questions related to Reversible Reactions.)

Wednesday 20 May 2009  (No questions related to Reversible Reactions.)

Wednesday 13 January 2010

106

Tuesday 25 May 2010  (No questions related to Reversible Reactions.)

Wednesday 12 January 2011  (No questions related to Reversible Reactions.) 107

Wednesday 25 May 2011  (No questions related to Reversible Reactions.)

Friday 13 January 2012 3.

Monday 21 May 2012  (No questions related to Reversible Reactions.)

Monday 14 January 2013

108

109

Paper 2 Reversible Reactions

Thursday 22 May 2003 2.

110

111

Thursday 15 January 2004 6.

Thursday 20 May 2004 4.

112

Thursday 20 January 2005

113

Thursday 19 May 2005  (No questions related to Reversible Reactions.)

Thursday 19 January 2006  (No questions related to Reversible Reactions.)

Thursday 18 May 2006

114

Monday 22 January 2007

115

116

Thursday 17 May 2007

Thursday 17 January 2008  (No questions related to Reversible Reactions.)

Monday 19 January 2009  (No questions related to Reversible Reactions.)

117

Friday 22 May 2009

Monday 18 January 2010  (No questions related to Reversible Reactions.)

118

Friday 28 May 2010  (No questions related to Reversible Reactions.)

Monday 17 January 2011  (No questions related to Reversible Reactions.)

Wednesday 15 June 2011  (No questions related to Reversible Reactions.)

Friday 20 January 2012  (No questions related to Reversible Reactions.)

Tuesday 29 May 2012 5.

119

Wednesday 16 January 2013  (No questions related to Reversible Reactions.)

120

Group Information

Group Leader: Abdullah Al Abid Mohammad Tofazzal Hossain Bhuyian

Also In the Group

 Abdul Haleem Abdul Kareem  Ikramullah Arifulla  Haider Ali Baqwi  Mohammad Zain Shakeel  Mohammad Anas Kareem  Ahmed Bin Rashid Irshad  Mohammad Rehan Sandhu

121

CHEMISTRY PAST PAPER QEUSTIONS AND REFERENCES FOR TERM 3 Topics from term 3  Reactivity series  Test for ions and gases 

Extraction for metals

Project Done By Hudais khan, Hamid Hasan, Hamza Shams, Ahmed Ifthikar, Israr Ahmed, Saleem Khan, Shabbir Hossain and Abdul Khaleel Talha

REACTIVITY SERIES Paper

Month

Year

Question

Sub Part

1

May

2000

5

1

May

2001

9

(b)

1

May

2004

17

(a)(b)

1

May

2005

5

1

May

2007

5

1

May

2010

6

1

May

2012

2

1

January

2013

6

2

May

2008

7

2

June

2011

1

(a)(i)(ii)(iii)

(b)

rusting of iron Paper

Month

Year

Question

Sub Part

1

May

2004

17

( c)

1

May

2006

16

1

January

2007

3

1

January

2009

9

1

May

2009

7

1

May

2011

7

1

January

2012

2

1

January

2013

4

2

January

2011

6

(b)

Oxidation & reduction Paper

Month

Year

Question

1

January

2006

9

1

January

2008

8

1

May

2008

5

1

January

2011

8

Sub Part

(a)(b)(i)(ii)

Extraction of metals Paper

Month

Year

Question

Sub Part

1

January

2000

7

(a)

1

May

2001

6

(a)(b)( c )

1

January

2001

9

(a)

1

May

2002

7

1

May

2002

14

1

January

2005

7

1

January

2007

12

1

January

2008

8

1

May

2008

12

1

May

2011

9

1

May

2012

12

(a)(b)

1

January

2013

7

(a)

2

May

2005

7

(a)

2

January

2006

6

(a)

2

May

2006

6

(a)

2

May

2007

9

(a)

2

May

2008

6

(a)

2

May

2009

6

(a)(i)(iii)

2

January

2010

8

(a)

2

May

2010

7

(a)(iii)

2

January

2011

6

(a)

2

May

2012

2

(d)

test for ions & Preparation and test for gases

Paper

Month

Year

Question

Sub Part

1

May

2000

8

(e)

1

January

2001

3

1

May

2001

2

1

May

2001

6

1

May

2003

8

1

May

2003

10

1

May

2005

13

1

May

2006

7

1

January

2008

12

1

January

2012

3

1

May

2012

11

2

May

2007

1

2

January

2009

1

2

May

2010

9

(d)(ii)

(a)(b)

(a)(b)