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SOALAN ULANGKAJI SPM 2009PMPMPMPMPMPMPMPMPPPM

Analsis Kertas Soalan 2004 - 2008TOPICS PAPER 1 PAPER 2 PAPER 3

04 05 06 07 08 04 05 06 07 08 04 05 06 07 08

FORM 4

Introduction To Chemistry

The Structure of The Atom

7 6 4 6 5 1 1 1 ½ 1 1 1

Chemical Formulae and question

4 6 6 6 4 ½ 1 1 ½

Periodic Table of elements

2 3 3 3 5 1 1 ½ 1

Chemical Bonds 2 1 2 1 4 1 1 1 ½

Electrochemistry 3 3 5 3 5 ½ 1 1 1

Acids and Bases 5 4 3 4 5 1 1 ½

Salts 1 0 2 0 2 1 1 ½

Manufactured Substances In Industry

4 3 4 3 1 1 1 1 1

F O R M 5

Rate of Reaction 4 5 4 4 2 1 1 1 1

Carbon compounds 6 7 6 7 3 1 1 1 1 1 1

Oxidation and reduction

6 7 4 6 5 1 1 1 1

Thermo Chemistry 4 4 5 5 3 1 2 1 1

Chemical For Consumer

2 1 2 2 3 1 1 1 1

TOTAL 50 50 50 50 50 7 7 6 9 6 4 4 3 3 2

SPM2009

[ 45411 ] [ 4541/2 ] [ 4541/3 ]

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1. After making observations, a chemist should try to

A make hypothesisB make inference C collect data D identify problems

2. Which of the following is a molecule? A NeonB Ammonia C Sodium chlorideD Potassium hexacyanoferate(III)

3 The nucleus of an atom contains

A electrons only B neutrons only C both protons and neutrons D both protons and electrons

4 The diagram shows a model of an atom.

Who introduced this model?

A Neils BohrB J.J ThomsonC James Chadwick D Ernest Rutherford

5 Which of following is the electron arrangement of a non-metal?

A 2.1B 2.2C 2.8.3 D 2.8.7

6 What can be deduced from the symbol ?

I The electron arrangement of aluminium atom is 2.8.3II Aluminium atom has 13 protons and 27 neutrons.III Aluminium atom has a proton number of 27 and 14 neutrons.IV The total number of proton and neutron of aluminium atom is 27.

A I and III B II and IV C II and III D I and IV

7. When 1.52 g of a metal oxide of Z is reduced, 1.04 g of the metal is obtained. Determine the empirical formula of the metal oxide. [RAM: O,16; Z,52].

A Z2O B Z3O2 C Z2O3 D ZO2

8 Which of the following chemical equation is balanced?

A KI + Pb(NO3)2 PbI2 + KNO3

B 2Cu(NO3)2 2CuO + 4NO2 + O2 C 2NH4Cl + Ca(OH)2 CaCl2 + 2NH3 + H2O D CuCO3 + HNO3 Cu(NO3)2 + CO2 + H2O

9 Which of the following electron arrangement of an atom has eight electrons valence?

A 2.8.2 B 2.6 C 2.8.8 D 2.8.8.2

10 What is the relative molecular mass of hydrated magnesium sulphate, MgSO4.7H2O?

[Relative atomic mass: Mg, 24; S,32; O,16; H,1]

A 356 B 246 C 145 D 305

11. In a chemical reaction of calcium carbonate with hydrochloric acid, 36cm3 of carbon dioxide gas is collected at room temperature. What is number of mole of carbon dioxide collected?

A 0.0015 mol B 0.067 mol C 1.50 mol D 1.61 mol

12 Which noble gases given below is used to fill airships and weather balloons ?

A Argon B Neon C Helium D Xenon

13 X, Y and Z are three different elements in the same period of The Periodic Table of the Elements. X is a non metal, Y is a metal and Z is a transition metal. Which is the correct order of these elements in The Periodic Table of Elements across the period from left to right?

A X, Y, Z B X, Z, Y C Y, Z, X D Z, Y, X

Electron

Shell

Nucleus that contains proton and neutrons

Al2713

SOALAN ULANGKAJI SPM 2009CHEMISTRY

Kertas 1

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20 Calculate the volume of sodium hydroxide of concentration 0.5 mol dm-3 needed to neutralise 25.0 cm3 sulphuric acid of concentration 0.20 mol dm-3.

A 10 cm3 B 20 cm3 C 25 cm3

D 50 cm3

21 The distilled water is added to 20 cm3 of 1.0 mol dm-3 sodium hydroxide solution to produce 250 cm3 of sodium hydroxide solution. What is the concentration of the sodium hydroxide solution produced?

A 0.08 mol dm-3 B 0.04 mol dm-3

C 0.06 mol dm-3

D 0.02 mol dm-3

22 Which of the following solutions has the highest concentration of hydrogen ion?A 50 cm3 of 1.0 mol dm-3 H2SO4 solutionB 150 cm3 of 1.0 mol dm-3 H2SO4 solution C 100 cm3 of 1.0 mol dm-3 H2SO4 solutionD 50 cm3 of 2.0 mol dm-3 H2SO4 solution

23

Which of the following elements may be D?

A Aluminium B Magnesium C Sulphur D Phosphorus

24 An alloy is harder than its pure metal because the foreign atoms in the alloy

A increases the bond strength between the atoms.B increases the empty spaces between the atoms.C react with the pure metal atoms to form a compound.D reduces the ability of the atoms to slide across each other.

25 The main element present in glass is A Lead B Sodium C Silicon D Boron

26 Ceramic is made from

A Silica, SiO2

B Cement C Marmar D Aluminosilicate hydrate

27 The diagram shows the arrangement of atoms in steel.

Element Electron arrangement

W 2.4

X 2.8.2

Y 2.6

Z 2.8.7

An oxide of D can reacts with both hydrochloric acid and sodium hydroxide solution

Iron atom

X atom

14 Which of the following substances is a covalent compound?

A CopperB Ammonia C Lead(II) oxideD Sodium chloride

15 The table shows the electron arrangement for elements W, X, Y and Z.

Which of the following elements react to form an ionic compound?

A Y and X B W and YC Y and ZD W and Z

16 The ions present in aqueous copper(II) chloride solution are

A Cu2+ and Cl- B Cu2+, Cl-, H+ and O2-

C Cu2+, Cl-, H+ and OH D Cu2+, Cl- , H3O+ and O2

17 Which of the following substances is an electrolyte?

A Glucose solution B Molten aluminium oxide C Hydrogen chloride in methyl benzeneD Copper(II) carbonate powder

18 The diagram shows the electrolysis of molten lead(II) bromide using carbon electrodes.

Carbon

Lead (II) bromide

Heat

What are the products at the anode and the cathode?

Anode CathodeA Bromine LeadB Oxygen HydrogenC Bromine HydrogenD Oxygen Lead

19 Which of the following is a weak alkali?

A Potassium hydroxide B Cooper(II) hydroxide C Aqueous ammonia D Lithium hydroxide

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What is X?A ZincB CopperC Carbon D Tin

28 Which of the following reactions occurs at the highest rate?

A Photosynthesis B Rusting of ironC Combustion of hydrogen in oxygenD Combustion of magnesium in oxygen

29 Which of the following is the meaning of activation energy?

A The maximum energy that the particles need to produce effective collision

B The minimum amount of energy that particles must have in order to react

C The amount of energy used by the particles during a collision

D The amount of kinetic energy of molecules during a collision

30 The graph shows the maximum volume of carbon dioxide gas evolved when calcium carbonate react with hydrochloric acid.

35

Time/s 120

What is the rate of reaction at 120 s?A 0.00 cm3 s-1 B 0.15 cm3 s-1

C 0.29 cm3 s-1

D 0.35 cm3 s-1

31 The rate of reaction depends on

A the activation energy for the reaction B the density of the reactantsC the heat of reactionD the volume of solution at the same concentration

32 A catalyst

A always slows down a chemical reactionB is not used up in the chemical reaction C can catalyst many chemical reactionsD always doubles the rate of a chemical reaction

33 Unsaturated fats can be converted to saturated fats through

A hydrogenation B esterificationC neutralizationD fermentation

34 Which of the following structural formulae shows an unsaturated hydrocarbon?

A

B

C

D

35 Which of the following pairs of substances are not isomers ?

A Hexane and 2,3-dimethyl pentane B 1-butene and 2-methylpropene C Pentane and 2,2-dimethylpropane D 2-chloropentane and 3-chloropentane 36 Pentyl propanoate is a food flavouring with apricot taste. This

substance can be obtained from the reaction between

A C3H7OH and C4H9COOH B C4H9OH and C2H5COOH C C5H11OH and C2H5COOH D C5H11OH and CH3COOH

37 Which of the following substance is found in crude oil?

A Ethanoic acid B Polythene C Ethanol D Butane

38 Which of the following is an oxidation process?

A Propene changes into propane B Lead(II) oxide loses its oxygen C Magnesium atom forms magnesium ion. D Chlorine molecule gains electrons.

39 Which of the following statements refer to oxidation?

I Process of losing oxygenII Process of gaining hydrogenIII Process of losing electronsIV Process of increasing oxidation number.

A I and II onlyB III and IV only C I, II and III onlyD I, II , III and IV.

Volume of CO2 gas/ cm3

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40 In which of the following compounds is the oxidation number of nitrogen the highest?

A KNO2

B NH4Cl C N2O D HNO3

41 W, X, Y and Z are four metals. Consider the reactions below involving these metals:

Z sulphate + X → Z + X sulphateZ sulphate + W → No reactionY sulphate + W → Y + W sulphateArrange the metals W, X, Y and Z in decreasing order of reactivity.

A X, W, Z, YB Y, W, Z, X C X, Z, W, Y D Y, Z, W, X

42 When a mixture of carbon and copper(II) oxide is heated strongly

I the oxide ion loses two electrons.II the oxidation number of carbon increases from 0 to +4III the copper(II) oxide acts as the reducing agent.IV the copper(II) ion accepts two electrons A I and IIIB II and IV C II, III and IVD I, II, III and IV

43 Redox reaction between iron(II) ion and manganate(VII) ion is represented by the equation:

5 Fe 2+ + MnO 4- + 8 H+ → 5 Fe3+ + Mn2+ + 4H2O

What can be deduced from the equation? I The oxidation state of manganese changes from +7 into +2 II The oxidation state of hydrogen changes from +1 into 0 III The greenish colour of iron(II) ions solution turns to

colourless IV Electrons transfer from iron(II) ions to manganate(VII) ions

A I and III only B I and IV only C I, II and III only D I, II, III and IV

44 The diagram shows a match. By striking the match, a chemical reaction is initiated.

Which statements about the chemical reaction are correct?

A Reaction is endothermic because energy is used to strike the match

B Reaction is endothermic because energy is given out as the match burns

C Reaction is exothermic because energy is used to strike the match

D Reaction is exothermic because energy is given out as the match burns

45 The reaction between solution P and solution Q is exothermic. A student confirms this statement by mixing equal volumes of the two solutions and measuring the temperature change. Which two pieces of apparatus should the student use?

A Balance and stop watch B Balance and thermometerC Pipette and stop watch D Pipette and thermometer

46 The burning of 0.6 g of K causes the temperature of 100 cm3 water to increase by 12°C.

What is the heat of combustion of K? [ relative molecular mass of X = 60; specific heat capacity of

water = 4.2 J g-1 ° C-1]

A 50.4 kJ mol-1

B 72.0 kJ mol-1

C 302.4 kJ mol-1

D 504.0 kJ mol-1

47 Which of the following is not used as a preservative in the food industry?

A SugarB Ginger C SaltD Vinegar

48 What is the function of an analgesic?

A To relieve pain B To treat asthma C To destroy bacteria D To calm down the emotion of the patient

49 The cleansing effect of detergent is more effective in hard water compared to soap because detergent

A is more soluble in water B produces more foam than soap in hard waterC does not form insoluble salt with metal ion in hard water D has hydrocarbon chain which makes detergent dissociate

less in hard water

50 Which of the following are examples of antibiotics? I Streptomycin II Barbiturate III Cortisone IV Penicillin

A IV onlyB II and III onlyC I and IV only D I, III and IV only

END OF QUESTION PAPER

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Answer all questions in this section.The time suggested to complete Section A is 90 minutes.

1. An experiment was carried out to determine the empirical formula of lead (II) oxide.A sample of lead (II) oxide was heated in the flow of dry hydrogen gas as shown in Figure 1.

After heating,the porcelain boat and its contents are cooled in the flow of hydrogen and its mass is recorded. The heating ,cooling and weighing processes are repeated until the mass of the porcelain boat and its contents are constant.The data recorded from the experiment are as follows:

Mass of porcelain boat = 25.30g Mass of porcelain boat and lead (II) oxide before heating = 36.45g Mass porcelain boat and lead after heating = 35.65g

(a) Write one chemical equation that can produce hydrogen gas.

……………………………………………………………………………………………………………… [1 mark]

(b) State one observation that can be made from this experiment.

……………………………………………………………………………………………………………… [1 mark]

(c) Why is necessary to cool the porcelain boat and its contents in the flow of hydrogen gas?

……………………………………………………………………………………………………………… [ 1 mark]

(d) Based on the data,determine the empirical formula of lead (II) oxide. [Relative atomic mass : Pb,207; O,16]

[4 marks]

(e) Why is the process of heating,cooling and weighing repeated until a constant mass is obtained?

…………………………………………………………………………………...………………………… …………………………………………………………………………………...………………………… [1 mark]

(f) State two precautionary steps to be taken while conducting this experiment.

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [2 marks]

SOALAN ULANGKAJI SPM 2009CHEMISTRY

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2. Figure 2 shows the flow chart for the fermentation process of a type of fruit juice.

Gas A

Heating with Porcelain chips

Fruit juice Compound B C2H6O

Process Y

Compound C Reflux Compound D C2H4O2

Compound X H2SO4

Figure 2

(a) Name compound B.

……………………………………………………………………………………………………… [1 mark]

(b) Name process Y. ……………………………………………………………………………………………………… [1 mark]

(c) Gas A is produced when compound B is strongly heated in the presence of porcelain chips. (i) Name gas A.

……………………………………………………………………………………………………… [1 mark] (ii) What can be observed when gas A is channeled into the acidified potassium manganate (VII) solution ?

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [1 mark]

(iii) Write a chemical equation for reaction in (c)(i) to produce gas A.

……………………………………………………………………………………………………… [1 mark]

(d) (i) Name the formation process of compound D from compound C.

……………………………………………………………………………………………………… [1 mark]

(ii) Write the chemical equation for the formation of compound D.

……………………………………………………………………………………………………… [1 mark] (iii) Give two chemical properties for the compound C.

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [2 marks]

(e) Give one characteristic of the compound D.

……………………………………………………………………………………………………… [1 mark]

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3. Substance X is heated in a test tube as shown in Figure 3. The limewater contained in another test tube turns milky.The residue left after substance X is heated is yellow when hot and white when cold.

Figure 3

(a) What is substance X?

……………………………………………………………………………………………………… [1 mark]

(b) Write an equation for the reaction.

……………………………………………………………………………………………………… [1 mark]

(c) What other substance will decompose when heated to give the same residue as that produced when substance X is heated?

……………………………………………………………………………………………………… [1 mark]

(d) What other substances are produced when the substance referred to in (c) is heated?

……………………………………………………………………………………………………… [2 marks]

(e) Write an equation for the reaction that occurs when the substance referred to in (c) is heated.

……………………………………………………………………………………………………… [1 mark]

(f) The residue left in the test tube is dissolved in dilute hydrochloric acid. Write an equation for the reaction of the residue with dilute hydrochloric acid .

……………………………………………………………………………………………………… [1 mark]

(g) i.) A few drops of of sodium hydroxide solution are added to the solution obtained in (f).What can be observed?

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [1 mark]

ii) More sodium hydroxide solution is added to the product obtained in (g)i. until no more changes occur. What can be observed?

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [1 mark]

(h) What conclusion can be drawn from the observations in (g)i. and (g)ii.?

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [1 mark]

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4.

Figure 4

(a) Write half equations for the reactions at the cathode and the anode.

Cathode :………………………….........................................................................

Anode :…………………………………………………………………………. [2 marks]

(b) State two observations during the electrolysis.

1. …………………………………………………………………………………... 2…………………………………………………………………………………… [2 marks]

(c) Is the resulting solution,after the electrolysis,acidic,neutral or basic? Explain your answer.

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [.2 marks]

(d) The product formed from the anode goes into the potassium iodide solution. Describe what you would see.

……………………………………………………………………………………………………… [ 1 mark]

(e) Write the ionic equation for the reaction taking place in test tube X.

……………………………………………………………………………………………………… [1 mark]

(f) Another electrolysis is carried out using diluted copper (II) chloride solution. The observation stated in (d) are not seen at the anode?Explain why.

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [1 mark]

(g) Identify a test to verify the product formed at the anode for experiment in (f).

……………………………………………………………………………………………………… [1 mark]

Potassium solution

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5. Figure 5 shows the arrangement of the apparatus used to study redox reactions.

Figure 5

(a ) Name one chemical substance that can be used to replace 1.0 mol dm-3 potassium nitrate.

……………………………………………………………………………………………………… [1 mark]

(b) Write the change of oxidation number for zinc in the reaction .

……………………………………………………………………………………………………… [1 mark]

(c) State which metal foil serves as the anode. Explain your answer.

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [2 marks]

(d) State the change that occurs at the

(i) copper foil:

……………………………………………………………………………………………………… [1 mark]

(ii) zinc foil:

……………………………………………………………………………………………………… [1 mark]

(e) In the reaction,which substance is

(i) oxidized:

……………………………………………………………………………………………………… [1 mark]

(ii) the oxidizing agent:

……………………………………………………………………………………………………… [1 mark]

(f) Write half equation s for the reaction at

(i) copper foil

……………………………………………………………………………………………………… [1 mark]

(ii) zinc foil

……………………………………………………………………………………………………… [1mark]

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(g) Table 1 shows two experiments conducted at room condition.

Table 1

The volume of hydrogen gas is recorded every 30 seconds.

(a) Write the equation for the reaction.

……………………………………………………………………………………………………… [1 mark]

(b) Calculate the maximum volume of hydrogen gas produced in [RAM : Zn, 65 ; 1 mol of gas occupies 24 dm3 at room condition]

(i) Experiment I

[2 marks]

(ii) Experiment II

[2 marks]

(c) State the experiment that gives the highest rate of hydrogen gas release.

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [2 marks]

(d) Plot a graph of the volume of hydrogen gas against time for Experiment I and Experiment II on the same axis.

[3 marks]

(e) State one way to increase the rate of reaction of the two experiments.

……………………………………………………………………………………………………… [1 mark]

Experiment I Experiment II

5.0 g of zinc powder + 50cm3

of 0.2 mol dm-3 sulphuric acid5.0 g of zinc powder + 50 cm3 of 1.0 mol dm-3

sulphuric acid

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Section B[20 marks]

Answer any one question from this section.The time suggested to complete Section B is 30 minutes.

(h) (a) The speed of reaction is important in industry and everyday life. State the five factors affecting the rate of reaction. [5 marks]

(c) The use of catalyst is increasing in importance in industry.

(i) What are the four essential features of catalyst? [4 marks]

(ii) Describe the effect of catalysts on the rate of reaction. [5 marks]

(iii) Give three catalyst with suitable examples,used in the manufacture of chemicals. [6 marks]

(i) Table 3 shows the proton number of atoms of elements P,Q and R.

(a) Compare the atomic size of atom T and U .Explain your answer. [ 4 marks]

(b) S and T burn vigorously in oxygen gas. Compare the reactivity between S and T .Explain your answer. [ 5 marks]

(c) Gas U can react with iron to form a brown solid. With the help of a labeled diagram,describe how the experiment can be carried out in the laboratory. Your description should include the chemical equation for the reaction. [ 6 marks]

(d) Describe the location of S in the Periodic Table. [ 5 marks]

Section C

[20 marks]

Answer any one question.The time suggested to answer this section is 30 minutes.

9. Salts may be prepared by the following methods:

Method A: reaction between metal oxide and acid. Method B: double decomposition involving two solutions of salts.

Rosmah has been asked to prepare lead (II) sulphate and copper (II) sulphate.

(a) Select suitable methods to prepare the dry salts. Explain your choice of method for each salt. [6 marks](b) Describe a laboratory experiment each to prepare the salts.In your description,include the chemical

equations involved. [14 marks]

10. The properties of compound R are as follows:

∙ Has melting point of 78°C ∙ Colourless solid ∙ Insoluble in water

(a) What type of compound is R? Explain your answer. [3 marks]

(b) R has a melting point of 78°C. Explain. [3 marks]

(c) Q is an ionic compound. State three differences of the physical properties of Q compared to R [3 marks]

(d ) Describe briefly an experiment to prove that Q can conduct electricity in a molten state but R cannot. [9 marks]

(e) R cannot conduct electricity in molten or solid state. Explain why. [ 2 marks]

Element Proton number

S 3

T 11

U 17

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1. A student conducted two experiments and obtained the following results.

Time(min) 0 30 60 90 120 150 180 210 240 270 300 330

Experimen XTemperature (oC)

61 65 67 71 74 76 80 80 80 83 87 89

Experiment YTemperature (oC)

87 84 83 81 80 80 80 76 73 69 66 64

In Experiment X, naphthalene powder is put in a boiling tube and placed in a water bath. The water is heated until 60oC, then the temperature of naphthalene is recorded at every 30 seconds interval until the temperature reaches about 90oC. The substance is stirred gently with the thermometer throughout the heating process.In Experiment Y,the hot boiling tube is cooled down.

(a) Write the hypothesis of:

(i) Experiment X:

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [3 marks]

(ii) Experiment Y:

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [3 marks]

(b) During the cooling of naphthalene,explain why the naphthalene must be stirred continuously.

……………………………………………………………………………………………………… ……………………………………………………………………………………………………… [3 marks]

(c) In the space given below,draw the apparatus showing the (i) heating of naphthalene

[3 marks](ii) cooling of naphthalene

[ 3 marks]

(d) State two important steps involved in this experiment.(i) ………………………………………………………………………………………………………(ii) ……………………………………………………………………………………………………… [3 marks]

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(e) State the three types of variables in Experiment X and Experiment Y.

(i) Manipulated variable

……………………………………………………………………………………………………… ………………………………………………………………………………………………………

(ii) Responding variable

……………………………………………………………………………………………………… ………………………………………………………………………………………………………

(iii) Constant variable:

……………………………………………………………………………………………………… [3 marks]

(f) Using scale of 1 cm to represent 30 s on the x-axis and 2 cm to represent 10oC on the y-axis, draw the temperature against time graphs for

(i) Experiment X

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(i) Experiment y

(g) What conclusion can you draw regarding the melting and freezing points of naphthalene from the graphs?

……………………………………………………………………………………………………… [3 marks]

2. Iron (II) ions can be oxidized to iron by a strong oxidizing agent like chlorine through the transfer of electrons at a distance.

Plan and explain how you would conduct an experiment in the laboratory to test the statement given above. Your planning should include the following aspects:

(a) Hypothesis(b) All the variables(c) List of substances and apparatus(d) Procedure of the experiment(e) Tabulation of data(f) Conclusion [17 marks]

END OF QUESTION PAPER

SKEMA JAWAPANSOALAN ULANGKAJI SPM

2009

Chemistry

255262264274

M l i1

CONTENTS

2

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SOALAN ULANGKAJI SPM 2009PMPMPMPMPMPMPMPMPPPM

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PAPER 1

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SPM2009

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Chemistryhttp://cikguadura.wordpress.com/

SOALAN ULANGKAJI SPM 2009 265

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Question Answer Mark1.(a) Zn + 2HCl ZnCl2 1m (b) Yellow powder changes to grey solid. 1m (c) To avoid the hot lead metal from being oxidised to form lead

(II) oxide again.1m

(d) Element Pb OMass/g 35.65-25.30=10.35 36.45-35.65=0.8Number of moles 10.35÷207=0.05 0.8÷16=0.05Ratio of moles 1 1

Empirical Formula: PbO

1m

(e) To ensure that all the lead (II) oxide has been reduced to lead completely

1m

(f) Allow the hydrogen gas to flow through the apparatus for an interval of time before heating.Continue the flow of hydrogen gas after heating until the hot deposited is cooled.

1m1m

Total: 10m2.(a) Ethanol 1m (b) Oxidation 1m

(c)(i) Ethene gas 1m (c)(ii) The purple solution of potassium manganate (VII) is

discoloured.1m

(c)(iii) Porcelain chipsC2H5OH C2H4 + H2O

1m

(d)(i) Esterification 1m (ii) C2H5OH + CH3COOH CH3COOC2H5 + H2O 1m (iii) 1. Ethanoic acid (compound C) reacts with metal carbonates

to form salts,carbon dioxide and water.2. Ethanoic acid reacts with bases to form salts and water.

1m

1m (e) Compound D have sweet odour. 1m

Total:10m3.(a) Zinc carbonate 1m (b) ZnCO3 ZnO + CO2 1m (c) Zinc nitrate 1m (d) Nitrogen dioxide,

Oxygen1m 1m

(e) 2Zn(NO3) 2ZnO + 4NO2 +O2 1m (f) ZnO + 2HCl ZnCl2 + H2O 1m

(g)(i) A white precipitate is produced 1m (ii) The white precipitate dissolves. 1m (h) The solution obtained in (f) contains zinc ions (Zn2+) 1m

Total:10m

PAPER 2SECTION A http://cikguadura.wordpress.com/

SOALAN ULANGKAJI SPM 2009266JAWAPAN

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4.(a) Cathode:Cu2+ + 2e CuAnode : 2Cl- Cl2 + 2e

1m1m

(b) 1. Pinkish brown solid ,copper is deposited at the copper electrode.2. Green copper (II) chloride solution fades and decolourises.

1m

1m (c) Neutral.

Cu2+ ions and Cl- ions are discharged at the electrodes.The resulting solution contains H+ and OH- ions which are water molecules.Thus,it is neutral.

1m1m

(d) The colourless solution of potassium iodide turns brown. 1m (e) Cl2 + 2I- 2Cl- + I2 1m (f) OH- ions, being more concentrated than Cl- ions, are

selectively discharged at the anode to produce oxygen gas and water molecule.

1m

(g) Use a glowing wooden splinter.Oxygen gas relights the glowing wooden splinter.

1mTotal:10m

5. (a) Dilute sulphuric acid 1m (b) 0 to +2 1m (c) Zinc foil

because zinc is more electropositive than copper1m1m

(d)(i) Copper foil becomes thicker. 1m (ii) Zinc foil becomes thinner. 1m (e)(i) Zinc foil. 1m (ii) Copper (II) ion 1m (f)(i) Zn Zn2+ + 2e 1m

(ii) Cu2+ + 2e Cu 1mTotal: 10m

6. (a) Zn + H2SO4 ZnSO4 + H2 1m (b)(i) Number of moles of H2SO4 that reacts

= 50 x 0.2 1000= 0.01 molFrom the equation in (a),1mol of sulphuric acid that reacts will release 24dm3 of

Hydrogen gas at room condition.-Therefore If 0.01mol of sulphuric acid reacts the volume of hydrogen released= 0.01 x 24 = 2.4dm3

1m

1m

1m

SOALAN ULANGKAJI SPM 2009 267

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(b)(ii) Number of mol H2SO4 that reacts=50x0.1 1000=0.005 molFrom the equation in (a), 1 mol of sulphuric acid that reacts will released 24 dm3 of hydrogen gas at room condition.Therefore,If 0.005 mol of sulphuric acid reacts the volume of hydrogen gas released.=0.005 mol x 24 dm3

=0.12 dm3.

1m

1m (c) Experiment 1

Because the concentration of sulphuric acid used is higher.1m1m

(d) Volume of hydrogen gas/cm3

240 Experimen 1

Experimen 2

0 Time/minutes 2m

(e) Using a hotter dilute sulphuric acid. 1mTotal:10m

Question Answer Mark7(a) 1.Size of solid particles

2. Concentration of the solution3. Temperature4. Pressure5. Catalyst

1m1m1m1m1m

Total: 5m

ANSWER SCHEME: SECTION B

SOALAN ULANGKAJI SPM 2009268JAWAPAN

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7(b) (i) 1. They speeds up reactions. 2. They are chemically unchanged at the end of reaction. 3. Only a small amount of catalyst is required. 4. Most catalysts are very specific and only catalyse a particular reaction.

(ii)- When reactions take place,bonds in the reactants must be broken before new bonds can be formed in the products. - This bond breaking requires a minimum energy which is called the activation energy. - In a catalysed reaction, the activation energy is lowered and less energy is required to break the bonds. - As a result,more effective collision occur and bond breaking takes place more easily. - Hence ,catalysed reactions are faster.

(iii) Process CatalystContact process Vanadium (VI) oxideHaber process IronCracking of petroleum Platinum

1m1m1m

1mTotal : 4m

1m

1m

1m

1m

1mTotal: 5m

6m

8.(a) - Atom U is smaller in size than atom T- Atom U has more protons in the nucleus- Attractive forces between the nucleus and the electrons in the shells are stronger.- Therefore,the electron filled shells are attracted closer to the nucleus.

1m1m

1m

1mTotal: 4 m

8(b) - T is more reactive .- The electron arrangement of T is 2.8.1 and S is 2.1- The valence electron of atom T is further from its nucleus.- The attractive forces between the nucleus of atom T towards the nucleus of atom T towards the valence electron is weaker.- Therefore the tendency of atom T to donate the valence electron is higher.

1m1m1m

1m

1mTotal: 5m

SOALAN ULANGKAJI SPM 2009 269

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8(c)

Procedure:

1. A spatula of iron filings is put into the combustion tube.2. Gas U is passed over the hot iron filings.3. The iron filings are heated very strongly.

Observation:

- The iron filings glow brightly and a brown solid is formed.

Chemical equation:

2Fe + 3 U2 2FeU3

1m

1m1m1m

1m

1m

Total: 6m8(d) - S has the electron arrangement of 2.1.

- S is located in Group 1- because S has 1 valence electron.- S is located in Period 2.- because S has 2 electron filled shells.

1m1m1m1m1m

Total: 5m

Question Answer Mark9(a) ∙ Copper (II) sulphate is prepared using Method A

∙ Copper (II) sulphate is a soluble salt which requires crystallisation to obtain the salt.∙ Lead (II) sulphate is prepared using Method B as lead (II) sulphate is an insoluble salt.∙ Using method A for preparation of lead (II) sulphate would result in incomplete reaction as salt form ed will be deposited on metal oxide,reducing the surface area of the reactants and eventually will stop the reaction.

1m1m1m1m1m

1mTotal=6m

ANSWER SCHEME: SECTION B

SOALAN ULANGKAJI SPM 2009270JAWAPAN

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9(b) ∙Preparation of copper (II) sulphate using method A:

- Add one spatula of copper (II) oxide to 25 cm3 of 1 mol dm-3 of hot dilute sulphuric acid.- When it has reacted,add further amounts until it can no longer dissolve.- Filter the mixture.- Evaporate the filtrate to one third of its volume or until the solution becomes saturated. - Allow the saturated solution to cool so that the salt crystallises out. - Filter to obtain the crystals.- Wash with a bit of distilled water and dry between the sheets of filter paper.

∙ Preparation of lead (II) sulphate using method B:

- Mix lead (II) nitrate solution with sodium sulphate solution.- Stir the mixture well.- Filter the mixture.- The residue is barium sulphate salt.- Wash the salt with distilled water.- Then dry the salt between sheets of filter papers.

1m

1m1m1m1m1m1m1m

1m

1m

1m1m1m1m

Total: 14m10(a) - R is a covalent compound.

- The compound has a low melting point.- and it is insoluble in water.

1m1m1m

Total: 3m10(b) - R has a low melting point.

- Attractive forces between the molecules are weak.- less heat energy is needed to overcome the weak forces of attraction.

1m1m1m

Total: 3m10(c) - (i) Q has a high melting point

-(ii) It can conduct electricity in aqueous solution or molten state.-(iii) It is soluble in water.

1m1m

1mTotal: 3m

SOALAN ULANGKAJI SPM 2009 271

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- Apparatus:

Spatula,Bunsen burner,tripod stand,batteries,carbon electrodes,electrode holder,bulb,connecting wires with crocodile clips,switch,pipe-clay triangle ,crucible

- Material: Powder R,Powder Q

- Procedure:

1. One spatula of Q powder is placed in a crucible.2. Two carbon electrodes are dipped into Q and the circuit is completed by connecting to the batteries and switch.3. Powder Q is heated until its melts and the switch is turned on again.4. Steps 1-3 are repeated by replacing powder Q with powder R.

- Observation:Compound Physical States ObservationQ Solid The bulb does not light up.

Molten The bulb lights up.R Solid The bulb does not light up.

Molten The bulb does not light up.

1m

2m

1m1m

1m

1m

2m

Total: 9m

10(e) - R consists of neutral molecules.- No ions to carry electrical charges.

1m1m

Total: 2m

SOALAN ULANGKAJI SPM 2009272JAWAPAN

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Question Answer Mark1(a)(i) The temperature [1] of naphthalene powder increases[1]

when it is heated [1]3m

1(a)(ii) When molten naphthalene is cooled down,the temperature falls.

3m

1 (b) To ensure an even temperature during the cooling of naphthalene in order to avoid supercooling

3m

1(c) (i)

1(c)(ii)

1 (d)(i) A water bath is used to heat naphthalene. 3m1 (d) (ii) Naphthalene is continuosly stirred during heating of cooling. 3m1(e)(i) Time taken to heat/cool 1m1(e)(ii) Temperature of naphthalene 1m1(e)(iii) Naphthalene 1m1(f)(i) 3m

PAPER 3ANSWER SCHEME http://cikguadura.wordpress.com/

SOALAN ULANGKAJI SPM 2009 273

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1(f)(ii) 3m

1(g) The melting point =The freezing point=80oC 3m2 (a) -Chlorine oxidises Fe2+ ions to Fe3+ ions through the transfer

of electronsat a distance from the reducing agent to the oxidising agent.

3m

2 (b) Manipulated: Chlorine and Fe2+ ions Responding : Products of reaction deflection of Galvanometer needle.Constant : Volume of oxidizing and reducing agents

3m

2 (c) Substances: Chlorine water,dilute sulphuric acid,iron (II) sulphate solution,sodium hydroxide solution.

Apparatys: U-tube,carbonelectrodes,electric wires with crocodile clips,galvanometer,stoppers,dropper

3m

2(d) Procedure of the experiment :

1. The apparatus is set up as shown in the diagram and left aside for 30 minutes.2. Observations before an after the experiment are recorded.3. At the end of the experiment, a little solution is removed from the negative terminal with a dropper and tested with sodium hydroxide solution.

2(e) Tabulation of data;Experiment ObservationDirection of electron flow Deflection of galvanometer

shows electron flow from the negative to positive terminal.

Change to FeSO4 Light green to yellow in colour.

Changes to Cl2 Greenish yellow to colourlessReaction of iron salt with NaOH

Forms brown precipitate,insoluble in excess alkali.

3m