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SPM2008

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ChemistryAnalisisMata Pelajaran

SOALAN ULANGKAJI SPM 2008134JA

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YEARTOPICS

PAPER 1 PAPER 2 PAPER 304 05 06 07 04 05 06 07 04 05 06 07

Form 4Introduction to chemistryThe structure of the atom 7 6 4 6 1 1 1 1 1 1Chemical formulae and questions 4 6 6 6 ½ 1 1 Periodic table of elements 2 3 3 3 1 1 Chemical bonds 2 1 2 1 1 1Electrochemistry 3 3 5 3 1 ½ 1 1 1Acids and bases 5 4 3 4 1 ½ Salts 1 - 2 - 1 1 1 ½Manufactured substances in industry 4 3 4 3 1 1 1 Form 5Rate of reaction 4 5 4 4 1 1 1Carbon compounds 6 7 6 7 1 1 1 1Oxidation and reduction 6 7 4 6 1 1 1 1Thermo chemistry 4 4 5 5 1 2 1Chemical for consumer 2 1 2 2 1 1 1 1

Analysis of Chemistry( 2004 - 2007 )

http://cikguadura.wordpress.com/


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SOALAN ULANGKAJI SPM 2008

TIMES HIGHER EDUCATION

SOALAN ULANGKAJI SPM 2008CHEMISTRY

Paper 1Nov./Dis

DO NOT OPEN UNTILL INTSRUCTED TO

1. Answer all the questions

2. Think thoroughly before answering any of the questions. If you need to change your answer, erase the answer properly and thoroughly before remarking the question sheet.

This question paper contains 7 printed pages and 0 non printed pages


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Instruction : For Question 1 to 50, each question is followed by four options, A, B, C and D. Choose one correct answer for each question and blacken the corresponding space in your objective answer sheet.

1. Diagram 1 shows the set-up of the apparatus for electrolysis

Which of the following compounds could be used as an electrolyte ?A Ethanol C Naphthalene B Kerosene D Ethanoic acid

2. Which of the following is true about acids.A Acids react with metal to produce salt and waterB Acids react with bases to produce salt and hydrogen gasC Acids react with metal oxide to produce salt, water, and hydrogen gasD Acids react with carbonates of metals to produce salt, water, and carbon dioxide gas.

3. Which of the following substance is a non electrolyte?A Molten lead (ii) oxideB Aqueous silver nitrateC Molten nanphthaleneD Ammonia in water

4. Glacial ethanoic acid is put into four test tubes A, B, C and D. In which test tube does a reaction occur?

5. Which of the following is a strong alkali ?A Magnesium hydroxideB Calcium hydroxideC Aqueous ammoniaD Potassium hydroxide

6. Diagram2 shows the formation of ammonia through the Haber process

Hyrogen Nitrogen

Ammonia

Catalyst XTemperature YPressure Z

Which of the following represent catalyst X, temperature Y and pressure Z?

Catalyst X Temperature Y, ºC

PressureZ/atm

A Vanadium(V) oxide 550 200B Nickel 300 100C Iron 200 450D Iron 450 300

7.

The figure above represents the manufacture of sulphuric acid by the Contact Process. What do the letters X, Y and Z represent ?

SO2 SO3 H2S2O H2SO4

X Y Z

X Y ZA Oxygen Concentrated

sulfuric acidWater

B Oxygen concentrated sulphuric acid

Catalyst

C Oxygen Water Concentrated sulfuric acid

D Catalyst Oxygen Concentrated sulfuric acid

Diagram 1

Calcium

Diagram 2


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8. Which of the following substances can be used to compare the chemical properties of hexane and hexene?I Lime waterII Liquid Bromine III Dilute sulphuric acidIV Acidified potassium manganate (VII)

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

9. Ethanol undergoes complete combustion when it burns in excess air to produce

A Water and carbon dioxide gasB Water, carbon and carbon dioxide gasC Water, carbon monoxide gas and carbon dioxide gasD Water, carbon, carbon monoxide gas and carbon dioxide gas

10. Diagram 3 shows the change of the state of matter

Which of the following is process Y?A Sublimation C FreezingB Boiling D Condensation

Diagram 3

11. Which of the following has the same number of molecules as 80 g of magnesium oxide?A 44 g carbon dioxide gasB 4 g hydrogen gasC 6 g helium gasD 58.5 g sodium chloride

12. Which of the following contains 6.02 x 1023 molecules?[Relative atomic mass : H,1; N, 14; O, 16, Avogadro constant: 6.02 x 1023]I 1.5 g of hydrogen gasII 1.8 g of waterIII 32 g of oxygen gasIV 17 g of ammonia gas

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

13. What is the meaning of heat of reaction?A The change in the energy needed to break the chemical bondB The change in the energy contained in the products and in the reactantsC The energy needed to start a reactionD The energy involved when the change of state of the matter happens

14. Which of these chemicals equation is not balanced?I 2Pb3O4 → 6PbO + O2

II Mg + Fe2O3 → MgO + 2FeIII H2 + S → H2SIV H2SO4 + NaHCO3 → Na2SO4 + H2O + CO2

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

15. 10.4g of a sample of chloride of metal M contains 6.85g of metal M. Determine the formula of the metal M chloride. (Relative atomic mass : m,137;cl,35.5

Which of these following statement is true?A MClB MCl2C M2ClD M2Cl3

16. Which of the following correctly matches the type of glass and its composition ?

Glass Main composition

I Lead glass Lead(II) oxide II Borosilicate glass Boron oxide III Fused glass Sodium oxide IV Soda-lime glass Aluminium oxide

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

17. Soap is produced in the saporification reaction by

A heating carboxylic acid with ethanolB heating ethanol with acidic potassium dichromate(VI)C heating animal oil with sodium hydroxide solutionD heating palm oil with hydrochloric acid

18. Diagram 4 shows the atomic symbol of element X.

7 X 3

Duagram 4Which of the following is true about the sub-atomic particles of element X?

Proton Number

Number of Neutron

Number of electron

A 7 7 10B 7 7 7C 3 4 3D 3 4 2

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23.

Diagram 7

Diagram 7 shows energy level of reaction which is represented by V + W X + Y ∆ H = P kJ mol-1

Calculate the value of the heat of reaction

A + 120 kJ mol-1 C - 120 kJ mol-1

B + 150 kJ mol-1 D -150 kJ mol-1

22. Diagram 6 shows a simple voltaic cell. P and Q are electrodes of the an hour for the reaction to occur

Voltmeter P Q

Copper (II)Zinc sulphate solution sulphate solution Diagram 6

Which of the following is/are true about the cell?I Porous pot is used to capture electronsII Electrode Q becomes thickerIII Electrons flow from Q to PIV Oxidation process occurs at P

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

19. Chlorine and bromine are in the same Group in the Periodic Table because

A their physical properties are the sameB Both of them are gases at room temperatureC Both of them have 7 valence electronsD Both of them dissolve in water at the same rate

20. Diagram 5 shows three different alkali metals burning at different rates in bromine gas. Bromine vapour Gas jar spoon Gas jar cover Gas jar Diagram 5

R S TA Potassium Lithium SodiumB Sodium Potassium LithiumC Lithium Sodium PotassiumD Sodium Potassium Lithium

21. The sub-atomic particles that are present in an atom areI electron III neutronII proton IV nucleon

A 1, II and IV only B 1, II and III onlyC I, III and IV only D I, II, III and IV

150kJ

30kJV + W

X + Y

24. When excess zinc powder is put into 50 cm3 1.0 mol dm-3 copper (II) sulphate solution, the temperature of the mixture rises by T ºC. What is the displacement heat for one mole copper displaced ? [ Relative formula mass: CuS04 , 160; Specific heat capacity of solution, c: 4.2 J g -1 oC -1 ]A 50 x T x 4.2 1000

B 50 x T x 4.2 x 160 0.5 x 1000

C 50 x T x 4.2 x 1 0.05 x 1000

D 50 x T x 4.2 x 0.05 1000

kJ mol-1

kJ mol-1

kJ mol-1

kJ mol-1

25. Below is the half-equation of a reaction. Cu2+ + 2e → Cu

What is meant by reduction reaction based on the equation ?A Electrons are received by copperB Electrons are donated by copperC Electrons are received by copper (II) ionsD Electrons are donated by copper (II) ions

By observing the brightness and colour of the flames, which metals are present in gas jars R, S and T respectively?

R - ReddishS - Bright YellowishT - Very bright purplish

R S T

26. Which of the following cannot be prepared by double decomposition method?

I Silver bromide II Calcium carbonate III Lead(II) nitrate IV Lead(II) chloride

V

CuZa

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26. Which of the following cannot be prepared by double decomposition method?

I Silver bromide II Calcium carbonate III Lead(II) nitrate IV Lead(II) chloride

27. Sodium hydroxide solution is added in excess to a solution containing lead ion, magnesium ion, iron(II)ion and aluminium ion in four separate test tubes and shaken. Which of the following is the correct observation?

Catalyst X ObservationA Aluminium White precipitate. Does not

dilute in excess NaOHB Magnesium White precipitate. Does not

dilute in excess NaOHC Lead White precipitate. Does not

dilute in excess NaOHD Iron (II) Brown precipitate. Does not

dilute in excess NaOH

28. Diagram 8 shows the electron arrangement of a compound formed between atoms P and Q .

Diagram 8Which of the following statements is true about the compound?

A There is a strong intermolecular force between particles P and QB The compound is formed by sharing the electronsC The compound conducts electricity in molten state D It is a covalent compound

2+ 2-

P Q

29. Diagram 9 shows the set-up of the apparatus used to purify impure copper Stripe.

A

+ –

Diagram 9

Anode Cathode ElectrolyteA Impure copper Pure copper Dilute hydrochloric

acidB Impure copper Pure copper Copper (II) Chloride

solutionC Impure copper Carbon Dilute hydrochloric

acidD Impure copper Carbon Copper (II) Chloride

solution

Which of the following set is suitable to make the process work?

31.

Based on diagram 10, what is observation after 10 minutes? A Gas bubbles are released B Grey precipitate is formed C Blue colour solution turns colourless D The concentration of copper ion decreases

30. The following represents the structural formula of a carbon compound 0 ||

CH3 C 0 CH2 CH2 CH3

The compound is produced by the reaction betweenA ethanol and propanoic acidB ethanol and butanoic acidC propanol and ethanoic acidD butanol and ethanoic acid

32. The tables shows the heat of combustion of three alcohols.

Which of the following factors increases the heat of combustion of alcohols?

A Size of molecules decreasesB Number of carbon atoms per molecule increasesC Number of oxygen atoms per molecule increasesD Number of hydrogen atoms per molecule decreases

Alcohol Heat of combustion/kJ mol-1

CH3OH -710C2H5OH -1370C4H9OH -2670

Diagram 10

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33. Which of the following compounds is an isomer of heptane?

A 2-methyl pentane C 2,3-dimethyl pentaneB 2-methyl heptane D 3,3-dimethye hexane

34. Protein is a polymer that is made up of many units of……A glycerols C amino acidsB fatty acids D monosaccharides

35. Diagram 11 shows information about two types of particle._______________________________________________ Particle Proton Electron Number configuration _______________________________________________ X 9 2.8 Y 17 2.8.8_______________________________________________

Diagram 11

Based on the information in the table, both particles X and Y areA inert gasesB negative ions C atoms of metals D isotopes of the same element

36. Which of the following are uses of an alloy?I To make ornamentsII To produce superconductorsIII To build the bodies of aircrafts

A I and II only C II and III onlyB I and III only D I, II and III

37. What is the number of molecules in 12 dm-3 of oxygen gas, O2 ? [1 mole of gas occupies 24 dm-3 at room temperature and pressure; Avogadro constant 6.0 x 1023 particles]A 1.5 x 1022 moleculesB 1.5 x 1023 moleculesC 3 x 1023 moleculesD 3x 1022 molecules

38. The equation shows the reaction between sulphuric acid and sodium hydroxide. H2SO4 + 2NaOH Na2SO4 + 2H2OWhat is the volume of 1.0 mol dm-3 sodium hydroxide solution which can neutralize 50 cm3 of 0.5 mol dm-3 sulphuric acid ?A 25 cm3 B 30 cm3

C 50 cm3 D 75 cm3

41. The following chemical equation shows the reaction between stearate ions, CH3(CH2)16COO- and alkyl sulphate ions, ROSO3- with calcium ions, Ca2+ in hard water. R represents the hydrocarbon long chain.

2CH3( CH2 )16COO-( aq ) + Ca2+( aq )

[ CH3( CH2 )16COO]2Ca( s )

ROSO3- Na+(aq) + Ca2+(aq)

( ROSO3- )2 Ca2+( aq ) + 2Na2+( aq )

What is the effect of the addition of calcium ion on the concentration of stearate ion or alkyl sulphate ion?A The concentration of stearate ion increasesB The concentration of stearate ion decreasesC The concentration of alkyl sulphate ion increasesD The concentration of alkyl sulphate ion decreases

42. Diagram 13 shows the set up of the apparatus to plate an iron spoon with silver.

Silver rodIron spoonSilver nitrate solution

Diagram 13

40. Diaram 12 shows the change of ethanol through step I, II and III.

Which of the following processes are applicable for step I, II and III?

R S TA Oxidation Dehydration HydrogenationB Reduction Hydration HydrogenationC Esterification Dehydration HydrationD Dehydration Oxidation Reduction

C2H4 C2H6

CH3COOHC2H5OHStep I

Step III

Step II

Diagram 12

39. When sodium metal is left exposed to the air, the grey metal turns white. What inference can be made from this observation?A Sodium does not rustB Sodium undergoes oxidation by receiving electronsC Sodium resistant to corrosionD Sodium corrodes and gets tarnished

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After 30 minute it was found that no plating took place on the iron spoon. What should be done ?

A Increase the cell voltage B Interchange the terminals in the cellC Rub the ion spoon with sand paperD Use iron(II) sulphate solution as the electrolyte

43. A dibasic acid, H2J has the concentration of 0.5 mol dm-3.Letter J is not the actual symbol of the element. What is the volume of potassium hydroxide, KOH, 1.0 mol dm-3 that can neutralize 25.0 cm3 of the H2J acid solution?

A 6.25 cm3 C 25.00 cm3

B 12.50 cm3 D 50.00 cm3

44.

Diagram 14Diagram 14 shows the energy level for a neutralization reaction. Which of the following statements is correct?A Reaction between A and B is an endothermic reaction.B T2 is the total heat energy releasedC The temperature of this reaction decreasesD T1 is the Heat of reaction

45. In an experiment, 25 cm3 of ethanoic acid was added to 20 cm3 of aqueous ammonia. The temperature of mixture increased by 5oC. How much was the heat energy released?[The specific heat capacity of mixture=4.2 Jg-1oC-1; density of mixture = 1 gcm-3]A 840 J B 900 JC 945 J D 1000 J

A + B

C + DT2

T1

Energy

46. Which of the following chemical reactions are representing a redox reaction? I H2SO4 + 2NaOH Na2SO4 + 2H2O11 Cu + 2AgN03 Cu(N03)2 + 2AgIII Pb(NO3)2 + Na2CO3 PbCO3 + 2NaNO3

IV 2Al + Fe203 Al203 + 2Fe A I and II only C III and IV onlyB I,II and IV only D II and IV only

47. What is the structure of the product of reaction when propane is passed into liquid bromine?

A CH3-CH2-CH2Br solutionB CH2=CH-CH2-CH2Br C CH3-CH2-CHBr-CH2BrD CH3- CHBr-CH2Br

48. Diagram 15 shows the experiment to study the effect of different metals on the rusting of iron when in contact with iron.

The iron bar in which beaker will not rust?

A Beaker IV C Beaker IIB Beaker III D Beaker I

49. Which of the following has the lowest pH?

A 0.01 mol dm-3 of ammonia solutionB 0.01 mol dm-3 of sulphuric acid solutionC 0.001 mol dm-3 of ethanoic acid solutionD 0.001 mol dm-3 of ammonia solution

50. Diagram 16 shows the graph obtained when an experiment was repeated with the change of one variable.

Which of the following statements is true to describe the above graph? A The rate of reaction of Experiment I is higher than experiment IIB The rate of reaction of Experiment II is higher because catalyst was used in Experiment IIC The difference in temperatures is not the factor affecting the rate of reaction of Experiment I and IID The time taken for reaction in Experiment I to stop is shorter than reaction in Experiment II

Nace solution

Zinc LeadIron Iron

TinIronCopper

Beaker I Beaker II

Beaker III Beaker IV

Diagram 15

Volume of carbon dioxide

(cm3)

Diagram 16Time (s)

Experiment II

Experiment I


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Paper 2Nov./Dis

1 hour 30 minutes






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Switch

Section A (60 marks)

Answer all questions in this Section. You are advised to spend 90 minutes on this section1. Diagram below shows the set-up of apparatus to investigate the redox reaction in a chemical cell.

(a) What is the energy change that occurrs in the experiment? (1 mark)

(b) What is the function of potassium nitrate solution in the above experiment? (1 mark)(c) State one observation that can be made in the above experiment. Explain why. (2 marks)(d) (i) Name the process that occurrs in electrode A. (1 mark)

Diagram 1

(ii) Write an ionic equation for the reaction that occurrs in electrode A. ( 1 mark)(e) State the negative terminal for this cell. Explain your answer. (2 marks)(f) Write a complete ionic equation for the reaction that occurrs in this experiment. (2 marks)

Paper 2

A B

Silver Rod

Silver nitrate solution

Zinc Rod

Zinc Sulphate solution

Potassium nitrate solution

2.

Diagram 2

Copper plate

Porous pot

Copper (II) sulphate solution

Zinc

Zinc nitrate solution

VoltmeterV

Diagram 2 shows a chemical cell.(a) Write the formula of zinc nitrate [1 mark]

(b) Write the half ionic equation for reactions at (i) negative terminal (ii) positive terminal [2 marks]

(c) Name the reaction that occurs at (i) negative terminal (ii) positive terminal [2 marks]

(d) State one observation in the experiment [1 mark]

(e) (i) Shows the direction of electron flow in Diagram 2 [1 mark](ii) State the change in energy in this experiment [1 mark]

(f) State the change in oxidation number for copper in this reaction [1 mark]

A


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3.

Diagram 3 shows a series of changes involving glucose. (a) Liquid A has a structural formula of C2H6O and the functional group – OH. Draw the structural formula for liquid A. _____________________________________________________________________________________________ [1 mark]

(b) Liquid B produces carbon dioxide gas when it reacts with sodium carbonate. (i) What is liquid B? _____________________________________________________________________________________________ [1 mark]

(ii) Write the molecular formula for liquid B _____________________________________________________________________________________________ [1 mark] (c) Liquid C has a sweet, fruity smell (i) Name catalyst Y.

_____________________________________________________________________________________________ [1 mark]

(ii) Name the homologous series for liquid C. _____________________________________________________________________________________________

[1 mark]

(d) When gas D is passed through bromine water, the brown colour of bromine water is decolourised (i) Name gas D. _____________________________________________________________________________________________ [1 mark] (ii) Write down the molecular formula for the compound that is produced when gas D reacts with bromine water. _____________________________________________________________________________________________ [1 mark]

(e) i) Write the equation for the reaction involving the combustion of liquid A. _____________________________________________________________________________________________

[1 mark](ii) What is the volume of oxygen at room temperature needed to burn 2.3 g of liquid A completely? [Atomic relative mass : H,2 ; C,12 ; O,16. Volume of 1 mole of gas at room temperature is 24 dm3 ]

_____________________________________________________________________________________________

Diagram 3

Liquid A Gas DHeat

Glucose

Liquid B Liquid C

Yeast Distillation

Porcelain chips

Liquid A + Catalyst Y

Reflux

Acidified K2Cr2O7 solution

(10 marks)

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B

4. Diagram 4 shows part of the Periodic Table of Element. A, B, C, D, E, F, G and H do not represent the actual symbol of elements

E

H

FC D

A

G

Diagram 4

Using the letters in the Periodic Table of Elements in Diagram 4, answer the following questions.

(a) (i) State the number of proton of atom G. _____________________________________________________________________________________________ [1 mark]

(ii) Write the formula of ion of atom G. _____________________________________________________________________________________________ [1 mark]

(b) 12 C is one isotope of C. 6 (i) Name another isotope of C _____________________________________________________________________________________________ (ii) Both isotopes have same chemicals properties. Eaplain why. _____________________________________________________________________________________________ [2 marks](c) Atom D is more electronegative compared to atom C. Explain why. _____________________________________________________________________________________________ _____________________________________________________________________________________________ [3 marks]

(d) E reacts with G to form a compound (i) Write the chemical equation for the reaction. _____________________________________________________________________________________________ [1 mark]

(ii) Draw the diagram of electron arrangement for the compound that is formed between E and G. _____________________________________________________________________________________________ _____________________________________________________________________________________________ [2 marks]

(10 marks)

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5. An experiment is carried out to determine the rate of reaction for the reaction between 50 cm3 of dilute sulphuric acid and excess copper(II) carbonate powder. Table 1 shows the results of the volume of carbon dioxide gas collected at regularintervals of 30 seconds.

Time, s 0 30 60 90 120 150 180 210 240Volume of CO2, cm3 0.0 20.0 29.0 36.0 41.0 44.0 45.0 45.0 45.0

Diagram 5

(a) Draw a labeled diagram for a set-up of the apparatus used in this experiment. _____________________________________________________________________________________________ _____________________________________________________________________________________________ [2 marks]

(b) Plot the graph of volume of carbon dioxide gas collected against time for this experiment. _____________________________________________________________________________________________

[4 marks]

(c) Based on the graph plotted, determine (i) the average rate of reaction in this experiment

_____________________________________________________________________________________________ _____________________________________________________________________________________________

(ii) the instantaneous rates of reaction at 2 minutes. _____________________________________________________________________________________________ _____________________________________________________________________________________________

[3 marks]

(d) Explain why the rate of reaction decreases with time. _____________________________________________________________________________________________

[1 mark]

(10 marks)

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6.

Diagram 6

Diagram 6 shows an electrolytic cell that is used to electrolyse copper (II) chloride, CuCl2. (a) Name the electrode where oxidation occurs. _____________________________________________________________________________________________ (1 mark)

(b) Describe the transfer of electrons in this electrolysis. _____________________________________________________________________________________________ _____________________________________________________________________________________________ (2 marks)

(c) i) Name the ion that is reduced. _____________________________________________________________________________________________ (1 mark) ii) Write the reduction half-equation _____________________________________________________________________________________________ (1 mark)

iii) State the change in the oxidation number during the reduction. _____________________________________________________________________________________________ _____________________________________________________________________________________________ (2 marks)

d) i) State an observation at Y electrode. _____________________________________________________________________________________________ (1 mark)

ii) Name the reaction that occurs at Y _____________________________________________________________________________________________ (1 mark)

e) Write the ionic equation for this experiment _____________________________________________________________________________________________ _____________________________________________________________________________________________ (2 marks)

X Y

electrode carbon

Copper (II) chloride

crucible

(11 marks)

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SECTION B (20 MARKS)

Answer One question in this section. The time suggested to answer this question is 30 minutes

7. (a) Benzene, C6H6 is an unsaturated hydrocarbon. Benzene burns completely in excess air.

(i) Write a balanced chemical equation to show the burning process above. [3 marks]

(ii) The relative molecular mass of benzene is 78’. What is meant by this statement ? [3 marks]

(iii) When 7.8 g of benzene is completely burned, determine the volume of oxygen gas evolved in cm3. [1 mole of gas occupies 24 dm3 at room temperature and pressure] [4 marks]

(b) The diagram below shows a molecular formula of 2-methyl propan-2-ol.

(i) Draw the structural formula of 2-methylpropan-2-ol.

(ii) Draw and name other isomers of 2-methylpropan-2-ol.

(iii) Compare the physical and chemical properties between the isomers [10 marks]

C4H9OH

8. Diagram below shows three symbols for the elements X, Y and Z

7 12 35 X Y Z3 6 17

(a) Compare the subatomic particles between any two of the elements. [4 marks] (b) Element X reacts with element Z to form a compound. Based on a labeled diagram, explain the formation of the compound [10 marks]

(c) Element Y also can react with element Z to form a compound. Explain how the compound is formed [3 marks]

(d) Compare the melting point of compound in (b) and (c). Explain your answer [3 marks]

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Section C (20 marks)

Instructions: Answer any one question from this section. The time suggested to complete this section is 30 minutes.9. (a) “ A chef who makes cakes for his restaurant wants to make the food tastier, last longer and of course look better.”

State the food additives that can help the chef with the above purpose. Explain how the additives act. (6 marks)

(b) “A fish seller washes his oily hands using soap” Explain the cleansing action of the soap on the oily dirt on the hand. (6 marks)

c) “Ionic compounds can conduct electricity in molten state but cannot conduct electricity in solid state. Covalent compounds cannot conduct electricity in solid and molten states.” Describe an experiment to prove the above statements. In your description, include all the chemicals apparatus and observations involved. (8 marks)

10. Diagram 7.1 and Diagram 7.2 show the electron arrangement for atoms of two elements from Group 17 in the Periodic Table of Elements.

(a) Based on Diagram 7.1: (i) Write the electron arrangement for the atom of the element and name the element. [2 marks] (ii) Write a chemical equation for the reaction between these elements and sodium hydroxide. [3 marks](b) Compare the attractive forces between the nuclei and the valence electrons in the atoms in Diagram 7.1 and Diagram 7.2 and relate this to their respective reactivity. [6 marks](c) Another element in Group17 is a black coloured solid. Predict the reactivity of this element in its reaction with sodium hydroxide compared to that of the element in Diagram 7.2 [1 mark]

Diagram 7.1 Diagram 7.2

(d) Diagram 7.3 shows the set up of the apparatus to investigate the reaction of an element from Group 17 with iron metal

Iron woolChlorine gasConcentrated

hydrochloric acid

Potassium manganate (VII) chips

Heat

Sodium hydroxide solution

Part G Part H

(i) State two safety precautions that are needed to be taken when carrying out the experiment [2 mark]

(ii) Explain and write down the chemical equations for the reactions occurring in Part G and Part H. [6 mark]

Diagram 7.3


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Paper 3Nov./Dis

1 hour 30 minutes






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Table 1 Shows the data obtained by a student fromm two experiments that were carried out to study the decomposition of hydrogen peroxide.In Experiment I, 8 cm3 of 2.0 mol dm-3 hydrogen peroxide solution was added to 42 cm3 of distilled water and 2 chips of manganese(IV) oxide. The total volume of gas produced was recorded at regular intervals.In Experiment II, 8 cm3 of 3.0 mol dm-3 hydrogen peroxide solution was added to 42 cm3 of distilled water and 2 chips of manganese(IV) oxide. The total volume of gas produced was recorded at regular intervals.

(a) Name the gas produced in the above experiments.

_____________________________________________________________________________________________

(b) (i) State the manipulated variable and the responding variable in the experiment. Manipulated variable : _____________________________________________________________________________

Responding variable : _____________________________________________________________________________

(ii) State the hypothesis of the experiment. _____________________________________________________________________________________________ _____________________________________________________________________________________________

Diagram 1 shows the initial burette reading at 0 minute and the final burette reading after 5 minutes.Determine the value of X, which is the volume of gas collected at the 5th minute.

_____________________________________________________________________________________________ _____________________________________________________________________________________________

Time/minutes 0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5 6.0 6.5 7.0Experiment I(volume of gas/cm3)

0 3.0 5.5 8.0 10.5 13.0 15.0 16.5 18.0 19.5 20.5 21.5 22.5 23.5 24.5

Experiment II(volume of gas/cm3)

0 6.0 10.5 15.5 18.5 21.5 24.5 27.0 29.0 31.0 x 34.0 35.0 36.0 37.0

Table 1

Diagram 1

Time : 1 hour 30 minutesAnswer all Questions

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(d) (i) Plot the graphs of the volume of gas against time for Experiment I and Experiment II on the graph paper below by using the same axes

(ii) Predict the volume of the gas produced at the 7.5th minute of Experiment II from the graph in (d)(i).

_____________________________________________________________________________________________

(iii) Determine the rate of reaction in Experiments I and II at the 3rd minute using the graph in (d)(i).

Rate of reaction in Experiment I at the 3rd minute

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Rate of reaction in Experiment II at the 3rd minute

_____________________________________________________________________________________________

(e) What is the factor that caused the difference in the rates of reaction for the two experiments in (d)(iii)?

_____________________________________________________________________________________________

(f) Why does the rate of decomposition of hydrogen peroxide decrease with time ?

_____________________________________________________________________________________________

(g) What is the function of manganese(IV) oxide in both the experiments?

_____________________________________________________________________________________________

(h) The total volume of gas released with 7 minutes in Experiments II is greater than that in Experiment I. Give your reason. _____________________________________________________________________________________________

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(i) Write a balanced chemical equation for the decomposition of hydrogen peroxide.

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2. Diagram 2 below displays the set-up of the apparatus of an experiment to determine the heat of neutralization between aqueous sodium hydroxide and dilute hydrochloric acid.

The respective initial temperatures of the two reactants and the maximum temperature of the mixture are displayed by the thermometer readings in the figure below.

200 cm3 of 1 mol dm-3 dilute hydrochloride acid

200 cm3 of 1 mol dm-3

aqueous sodium hydroxide

Plastic cup

(a) Based on the figure above, write the temperature readings of each of the solutions in the appropriate spaces in the table below.

Initial temperature of aqueous sodium hydroxide/ oCInitial temperature of dilute hydrochloric acid/ oCMaximum temperature of the mixture/ oC

(b) (i) Write the equation for this neutralization reaction.

_____________________________________________________________________________________________ (ii) Calculate the total energy that was released from this reaction. [The specific heat capacity of water = 4.2 J g-1 oC-1; Density of the solution = 1.0 g cm-3]

(c) (i) Calculate the heat of neutralization for this reaction

_____________________________________________________________________________________________ (ii) Draw the energy level diagram of this reaction.

_____________________________________________________________________________________________

40

30

20

40

30

20

40

30

20

Initial temperature of aqueous sodium hydroxide

Initial temperature of dilute hydrochloric acid

Maximum temperature of the mixture

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Diagram 2

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(d) (i) Write the observation noted in this experiment other than changes in the temperature.

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(ii) What is the inference deduced from the observation above?

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(e) What are the precautions to be taken for this experiment.

_____________________________________________________________________________________________ _____________________________________________________________________________________________

3. Food that is kept in a refrigerator will last longer than that of food being kept at room temperature.Based on the above statement, plan a laboratory experiment to investigate the effect of temperature on the rate of reaction between magnesium ribbon and dilute sulphuric acid.

Your planning should include the following aspect : (a) Statement of the problem

(b) All the variables involved

(c) Hypothesis

(d) List of apparatus and materials

(e) Procedure

(f) Tabulation of data

END OF QUESTION PAPER

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1.2.3.4.5.6.7.8.9.

10.11.12.13.14.15.16.17.18.19.20.21.22.23.24.25.

26.27.28.29.30.31.32.33.34.35.36.37.38.39.40.41.42.43.44.45.46.47.48.49.50.

DDCDDDABACBBBCBACCCCBBCCC

CBABCCBCCBBCCDABBCBCDDDBC

Chemistry[ 4541/1 ] [ 4541/2 ] [ 4541/3 ]

Kertas 1


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JawapanSoalan UlangkajiKertas 2

Soalan Butiran

1. (a)

(b)

(c)

(d) (i)

(ii)

(e)

(f)

2. (a)

(b) (i)

(ii)

(c) (i)

(ii)

(d)

(e) (i)

(ii)

(f)

SECTION A

A change from chemical energy to electrical energy

It serves as the salt bridge to complete the electric circuit so that ions can move through it.

The mass of zinc rod decreases gradually. Zinc rod gives up its electrons to silver rod.

Oxidation

Zn → Zn2+ + 2e-

Zinc rod is the negative terminal. Zinc is more electropositive than silver and its position is higher than silver in the electrochemical series. It has a greater tendency to donate its electrons.

Zn + 2Ag+ → Zn2+ + 2Ag

Zn(NO3)2

Zn → Zn2+ + 2e-

Cu2+ + 2e- → Cu Oxidation Reduction The blue colour of copper (II) sulphate solution diminishes gradually.

A change from chemical energy to electrical energy. A change from 0 to +2

Chemistry[ 4541/1 ] [ 4541/2 ] [ 4541/3 ]

copper (II) sulphate solution

Zinc nitrate solution

Zinc

Switch Voltmeter

porous pot

copper plate


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JawapanSoalan UlangkajiKertas 2

Soalan Butiran3. (a)

(b) (i)

(ii)

(c) (i)

(ii)

(d) (i)

(ii)

(e) (i)

(ii)

4.(a)(i)

(ii)

(b) (i)

(ii)

(c)

(d) (i)

(ii)

H H H H

H C C H H C C OH

H OH H H Ethanoic acid CH3COOH / C2H4O2 Concentrated sulphuric acid Ester Ethene C2H4Br2 C2H5OH + 3O2 → 2CO2 + 3H2O (complete combustion) 2.3 g of ethanol = 2.3/46 = 0.05 mol

(to react with) 0.05 x 3 = 0.15 mol of oxygen gas Volume of oxygen is 0.15/1 x 24 dm3 = 3.6 dm3

17 Cl-

Carbon-13 Both have the same number of valence electrons which is 4. Hence, they demonstrate similar reactivity. Atom D has 6 valence electrons compared to atom C which has 4. Atom D requires only 2 more electrons to reach its octet stability. Therefore, it is more electronegative. Mg + Cl2 → MgCl2

Chemistry[ 4541/1 ] [ 4541/2 ] [ 4541/3 ]

Cl mg Cl

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JawapanSoalan UlangkajiChemistry[ 4541/1 ] [ 4541/2 ] [ 4541/3 ]


(b)

(c) (i)

(ii)

(d)

6. (a)

(b)

(c) (i)

(ii)

(iii)

(d) (i)

(ii)

(e)

45/180 = 0.25 cm3 s-1 19/141 = 0.135 cm3 s-1 The rate of reaction in inversely proportional to the time taken. This means the longer the time taken, the lower the rate of reaction.

Electrode Y Electrons are transferred from the anode (electrode Y) to the cathode (electrode X)

Copper ion Cu2+ + 2e- → Cu The oxidation number of copper decreases from +2 to 0 Greenish-yellow gas is evolved. Oxidation CuCl2 → Cu2+ + 2Cl-

Kertas 2

SPM2008



Soalan Butiran7.(a)(i)

(ii)

(iii)

(b) (i)

(ii)

(iii)

SECTION B

General formula CxHy CxHy + (x + y/4)O2 → xCO2 + y/2 H2O C6H6 + 7½ → 6CO2 + 3H2O Relative atomic mass: H,1 ; C,12 (12x6) + (1x6) = 78 78 is the relative molecular mass of one molecule of benzene, which means, it is 78 times heavier than one twelfth (1/12) of the mass of carbon-12 atom. 7.8 g/78 g x 1 mol = 0.1 mol 0.1 mol/1 mol x 24 dm3 = 2.4 dm3

2-methylpropan-2-ol has a branched carbon chain and the hydroxyl (OH) group is positioned at carbon 2.Butan-2-ol has a straight carbon chain and the hydroxyl (OH) group is positioned at carbon 2.2-methylpropan-1-ol has a branched carbon chain and the hydroxyl (OH) group is positioned at carbon 1.The isomers have different physical properties such as melting and boiling points because they have different molecular structures; but they have the same chemical properties because they belong to the same homologous series.

Kertas 2

SPM2008




(b)

(c)

(d)

9. (a)

(b)

Subatomic particles Element X Element Y Electron 3 6 Proton 3 6 Neutron 4 6

Element X reacts with element Z to produce a compound with formation of ionic bond.

The electronic configuration of atom X is 2.1 and the electronic configuration of atom Z is 2.8.7. To attain the stable duplet electron arrangement, atom X donates one electron to form a positive ion. X → X+ + e-Atom Z will receive an electron to form Z- ion and attains the stable octet electron arrangement with 8 electrons in the valence electron shell. Z + e- → Z- The X+ ion and Z- ion will attract each other with a strong electrostatic force and form an ionic compound with the formula XZ. Element Y reacts with element Z to form a compound with formation of covalent bond.To attain the stable octet electron arrangement with 8 electrons in the valence electron shell, atom Y shares electrons with atom Z. One atom Y contributes 4 electrons and four atom Z contribute one electron each. Atom Y shares 4 pairs of electrons with four atom Z to form a covalent compound with the formula YZ. Compound XZ has a higher melting point than compound YZ. In compound XZ, the electrostatic force of attraction between oppositely charged ions is very strong and a lot of heat energy is required to overcome it. In compound YZ, the intermolecular force of attraction between molecules is weak and a little heat energy is required to overcome it.

For those purposes, the chef can use flavouring agents, preservatives, antioxidants and colouring agents.Flavoring agents are added to food to make it taste better. The agents are of two types: artificial flavours and flavour enhancers. Artificial flavours include sweeteners and others such as peppermint or vanilla. Examples are aspartame and saccharin. These two are actually substitutes for sugar to enhance the sweetness of food. Flavour enhancers are chemicals added to food to bring out the flavours or to enhance the taste, for example, monosodium glutamate (MSG).Preservatives and antioxidants protect food from being spoiled by bacterial and fungal attack, and atmospheric oxidation, respectively. Preservatives, for example sodium nitrite, benzoic acid and sodium benzoate, retard or prevent growth of microorganisms so that food can be kept longer.Examples of antioxidants include sulphur dioxide and sodium sulphite. They are added to food to prevent oxidation of fats and oils by oxygen in air.Colouring agents are synthetic dyes used to restore the colour of food lost during processing and enhance natural colours to increase attractiveness. Examples are azo and triphenyl compounds.

Soap molecules contain hydrophilic and fat insoluble heads and hydrophobic hydrocarbon tails.When soap is used on oily wetted hands, the negatively charged heads of soap ions dissolve in water, whereas, the hydrocarbon tails dissolve in the layer of oil. During washing, the oily dirt is lifted and washed away from the hands.Soap also can emulsify the oily dirt by breaking large drops of oil into smaller droplets. If the hands are dipped in water, the oily droplets repel one another because they carry the same charge. As a result, the oil is suspended.During washing, the droplets will be carried away.

Kertas 2

SPM2008



Soalan Butiran(c)

10. (a) (i)

(ii)

(b)

(c)

(d) (i)

(ii)

To investigate the electrical conductivity of compoundsApparatusCrucible, spatula, graphite rods, batteries, light bulb, switch, connecting wires, tripod stand, clay triangle and Bunsen burner.

MaterialsLead (II) bromide and naphthalene. Methods1. Three spatula of lead (II) bromide solid is put in a crucible.2. Two graphite rods are dipped in the lead (II) bromide solid and the circuit is completed by connecting to the batteries and switch.3. The switch is turned on and the bulb is checked if it lights up.4. Lead (II) bromide is heated strongly until it melts. The switch is turned on again to check if the bulb lights up.5. Steps 1 to 4 are repeated using naphthalene to replace lead (II) bromide.

ResultsCompound State Observation InferenceLead (II) bromide Solid Light bulb does not light up Conducts electricity in the molten but not in the solid state Molten Light bulb lights up Naphthalene Solid Light bulb does not light up Does not conduct electricity in any state Molten Light bulb does not light up

The electronic configuration for Diagram 7.1 is 2.8.7. The element is chlorine. Cl2 + 2NaOH → NaCl + NaOCl + H2O The distance between the nucleus and the valence electrons of atom in Diagram 7.2 is greater than that in Diagram 7.1 as the atom in Diagram 7.1 has 3 electron shells but the atom in Diagram 7.2 has 4 electron shells. Because of this, the attractive forces between the nucleus and the valence electrons become weaker in Diagram 7.2 compared to the atom in Diagram 7.1.As a result, the atom in Diagram 7.1 has a stronger attraction towards electrons compared to the atom in Diagram 7.2. The atom in Diagram 7.1 is more electronegative, therefore, it is more reactive compared to the atom in Diagram 7.2. The element in Diagram 7.2 reacts more actively with sodium hydroxide compared to the black coloured solid. 1. Concentrated acid is corrosive and the experiment must be conducted in a fume chamber.2. Make sure that the apparatus are connected tightly to prevent leakage of chlorine gas, which is poisonous. Part G Chlorine gas will react with iron wool to produce iron (III) chloride solid. 2Fe + 3Cl2 → 2FeCl2

Part H The excessive chlorine gas will flow into sodium hydroxide solution to produce sodium chloride, sodium chlorate and water. Cl2 + 2NaOH → NaCl + NaOCl + H2O

Kertas 2

SPM2008



Soalan Butiran1.(a)

(b)(i)

(b)(ii)

(c)

(d)(i)

(ii)(iii)

(e)

(f)

(g)

(h)

(i)

Oxygen gas

Manipulate variable : concentration of hydrogen peroxideResponding variable : decomposition rate of hydrogen peroxide

The higher the concentration of hydrogen peroxde, the higher is the rate of its decomposition

x= 49.5-17.0 = 32.5 cm³

38.0 cm³ (±0.5cm³)Rate of reaction of Experiment I at the 3rd minute = 3.6cm³ min (+0.2 )Rate of reaction of Experiment II at the 3rd minute = 5.6cm³ min (+0.2 )

Concentration of hydrogen peroxide in Experiment II is higher than that in Experiment I.

Concentration of hydrogen peroxide decreases with time due to occurrence of decomposition.

It acts as a catalyst.

The reason being the higher concentration of hydrogen peroxide in Experiment II compared to the concentration of hydrogen peroxide in Experiment I

2H2O2 2H2O + O2

Kertas 3

35

30

25

20

15

10

5

0 1 2 3 4 5 6 7 8

40

volume of O2 gas cm³

time/minute


SPM2008



Soalan Butiran 2.(a) (b)(i)

(ii)

(c)(i)

(ii)

d)(i) (ii)

(e)

3.(a)

(b) i. ii. iii.

(c)

(d)(i)(ii)

28°C; 28°C ; 39°CNaOH + HC1 NaC1 + H2OTotal (heat) energy released = mass of solution x specific heat capacity x rise in temperature = (200 + 200) x 4.2 x (39 – 28) = 400 x 4.2 x 11 = 18480 J

no. of moles of NaOH = (200 x 1.0) ÷ 1000 = 102molno. of moles of HCI = (200 x 1.0) ÷ 1000 = 0.2 molno. of moles of H2O produced = 0.2 molHeat Neutralisation = -[(1 ÷ 0.2) x 18.480 kJ] = - 92.40 kJ mol-1

Energy

The plastic cup becomes hotThe reaction is an exothermic reaction. 1 – A plastic cup must be used for this experiment2 – The mixture must be stirred constantly with the thermometer3 – The dilute acid must be added quickly and carefully to the alkali

Problem StatementDoes the increase in the temperature of sulphuric acid increase the rate of reaction. VariablesManipulated variable: temperature of sulphuric acidResponding variable: time take for magnesium ribbon to dissolve completely / rate of action Fixed variable: mass of magnesium ribbon; volume and concentration of sulphuric acid.

HypothesisThe higher the temperature of sulphuric acid, the shorter is the time taken for the magnesium ribbon to dissolve completely; the higher the temperature of sulphuric acid, the higher is the reaction between sulphuric acid and magnesium.

Apparatus and materialsMagnesium ribbon 0.1 mol³ dm sulphuric acidstopwatch, conical flask, electronic balance, measuring cylinder, Bunsen burner, thermometer, tripod stand, wire gauze.

Kertas 3

↑ ↑NaOH + HC1

NaCl + H20

∆H = -92.40 kj mol -1

SPM2008



Soalan Butiran(e)

(f)

Procedure1 – 25 cm³ of 0.1 mol dm³ sulphuric acid is measured and poured into a conical flask.2 – Using a thermometer, the temperature of sulphuric acid solution is measured.3 -5g of magnesium ribbon is weighed out and put into the acid in the conical flask.4 – A stop watch is started simultaneously5 – The conical flask is slowly shaken throughout the experiment6 – The time taken for the magnesium ribbon to dissolve completely in sulphuric acid is recorded.7 – Steps 1 to 6 are repeated with unchanged conditions and methods at different temperatures i.e 35°C, 40°C, 45°C, 50°C and 55°C respectively.

Tabulation Of Data

Temperature, 0C Time for magnesium ribbon to dissolve completely, SInitial Time350C400C450C500C550C

Kertas 3


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