SPM-Kimia-jul12.pdf

CHEMISTRY 1 SPM 2012

4541 CHEMISTRY

CHAPTER 2 : STRUCTURE OF ATOM

1 Diagram 1.1 shows the arrangement of particles of substance X at different temperatures.

(a) What is the physical state of substance X at

(i) 60 oC : .........................................................................

(ii) 90 oC : .........................................................................

[2 marks]

(b) State the movement of particles of substance X at 60 oC.

....………………………………………………………………………………………........……….

[1 mark]

(c) Graph 1.2 shows the graph of temperature against time when substance X is heated

from 60 oC to 90

oC.

(i) What is meant by melting point?

……………………………………………………………………………………………..

………………………………………………………………………………………………

[1 mark]

(ii) Based on Graph 3.1, state the melting point of substance X.

………………………………………………………………………………………………

[1 mark]

Diagram 1.1 90

oC 60

oC

Temperature /oC

Time /s

Masa/s Graph 3.1

60

78

90

t0 t1 t2 t3


4541 CHEMISTRY

(iii) Explain why the temperature remains constant from t1 to t2.

....………………………………………………………………………………………........

....………………………………………………………………………………………........

[2 marks]

(d) (i) Substance X cannot conduct electricity in any state.

State the type of particles of substance X.

....………………………………………………………………………………………........

[1 mark]

(ii) Table 1.3 shows two substances.

Magnesium oxide, MgO

Carbon dioxide, CO2

Which substance has the same type of particles as substance X?

Tick (√ ) the correct answer. [1 mark]

2 Table 2 shows the incomplete information about 3 atoms; X, Y and Z.

Atom Proton number Number of neutron Number of electron

X 8 6

Y 6 6

Z 17 17

Table 2

(a) State the name of subatomic particles that are found in nucleus of an atom.

……………………………………………………………………………………………………….

[1 mark]

(b) (i) What is the term of the total number of protons and neutrons in an atom?

……………………………………………………………………………………………..

[1 mark]

(ii) The total number of protons and neutrons for atom Z is 35.

What is the number of neutron in atom Z?

……………………………………………………………………………………………..

[1 mark]

Table 1.3


4541 CHEMISTRY

(iii) Write the symbol for atom Z in the form of A X.

Z

………………………………………………………………………………………………

[1 mark]

(iv) Draw the atomic structure of atom Z.

[1 mark]

(c) Atom X and atom Y are isotopes of an element.

(i) What is the proton number of atom X?

…………………………………………………………………………………….

[1 mark]

(ii) Write the electron arrangement of atom Y.

……………………………………………………………………………………..

[1 mark]

(iii) What is valence electron of atom X?

……………………………………………………………………………………..

[1 mark]

(iv) Why atom X and atom Y has same chemical properties?

……………………………………………………………………………………..

[1 mark]

(v) State the one use of isotope X in archaeology field.

……………………………………………………………………………………..

[1 mark]


4541 CHEMISTRY

3 Diagram 3 shows the chemical symbols which represent three elements X, Y and Z.

The letters used are not the actual symbols of the elements.

9

X 4

32

Y 15

31

Z 15

Diagram 3

(a) (i) What is meant by proton number?

………………………………………………………………………………………………..

[1 mark]

(ii) State the proton number of atom X.

………………………………………………………………………………………………..

[1 mark]

(b) What is represented by the number 32 for the element Y?

……….……………………………………………………………………………………………..

[1 mark]

(c) (i) Atom Y and Z are isotopes. State the difference between the two atoms.

..…………………………………………………………………………………………………

[1 mark]

(ii) State one use of any isotopes in daily life.

……………….…………………………………………………………………………………

[1 mark]

(d) (i) Write the electron arrangement of atom Y.

………………………………………………………………………………………………..

[1 mark]

(ii) Determine the number of valence electron for atom Y.

………………………………………………………………………………………………..

[1 mark]

(iii) Draw the electron arrangement for atom Z.

[2 marks]


4541 CHEMISTRY

CHAPTER 3 : CHEMICAL FORMULAE & EQUATIONS

4 (a) Diagram 4 shows that a magnesium atom is two times heavier compare to a carbon atom.

Relative atomic mass of carbon is 12.

Diagram 4

(i) Complete this equation :

Relative atomic mass = The average mass of one atom of an element

× the mass of an atom of carbon-12

[1 mark]

(ii) One atom of element X is two times heavier than one magnesium atom.

What is the relative atomic mass of element X?

……………………………………………………………………….................................................

[1 mark]

(b) A student heats 20 g of calcium carbonate strongly. It decomposes according to the equation below.

CaCO3 → CaO + CO2

(i) State the name of the products.

……………………………………………………………………………………………………….

[2 marks]

(ii) Describe the chemical equation in terms of quantitative aspect.

……………………………………………………………………………………………………….

……………………………………………………………………………………………………….

[2 marks]

Carbon atoms

Atom karbon

Magnesium atom

Atom magnesium

……

…


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(iii) Calculate the mass of calcium oxide produced.

[ Relative atomic mass; C = 12 ; O = 16 ; Ca = 40 ]

[3 marks]

(iv) Calculate the volume of carbon dioxide produced at room conditions.

[Molar volume of gas = 24 dm3 mol

-1 at room conditions]

[2 marks]

CHAPTER 4 & 5 : PERIODIC TABLE + CHEMICAL BOND

5 Diagram 5 shows the symbols of the atoms of element X, Y and Z.

The letters used are not the actual symbols of the elements.

7 23 39

X Y Z 3 11 19

Diagram 5

(a) What is the number of valence electron of the atom of element X?

…………………………………………………………………………………………..........................

[1 mark]

(b) (i) Identify the position of element Y in the Periodic Table of Elements.

…………………………………………………………………………………………................

[1 mark]


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(ii) Explain why element Y is placed at the position identified in (b) (i).

…………………………………………………………………………………………................

…………………………………………………………………………………………................

[2 marks]

(c) Element X, Y and Z can react with water.

(i) Which of the element is the most reactive in their reactions with water?

…………………………………………………………………………………………................

[1 mark]

(ii) Explain your answer in (c) (i).

…………………………………………………………………………………………................

…………………………………………………………………………………………................

…………………………………………………………………………………………................

[3 marks]

(iii) Write the chemical equation for the reaction between element that you choose in (c) (i) and

water.

…………………………………………………………………………………………................

[2 marks]

(d) Argon is placed at the same period with element Y in the Periodic Table of Elements.

(i) Compare the atomic size argon and element Y.

[ Given that proton number of argon is 18 ]

…………………………………………………………………………………………................

[1 mark]

(ii) Explain your answer in (d) (i).

…………………………………………………………………………………………................

…………………………………………………………………………………………................

[2 marks]


4541 CHEMISTRY

6 Diagram 6 shows part of the Periodic Table of the Elements.

Q, T, X, Y and Z do not represent the actual symbol of the elements.

.

3

Q

7

4

T

9

6

X

12

7

Y

14

8

Z

16

Transition Elements

Diagram 6

By using the letters in the Periodic Table of the Elements in Diagram 6, answer the following questions.

(a) (i) Write the electron arrangement of atom Q.

..............................................................................................................................................................

[1 mark]

(ii) Write the formula of ion Q.

..............................................................................................................................................................

[1 mark]

(b) State one element which exists as a diatomic molecule.

..……………………………………….. ...............................................................................................

[1 mark]

(c) (i) Arrange the elements Q, T, X, Y and Z according to the atomic size in descending order.

………………….…………………………………………………………………............................

[1 mark]

(ii) Explain your answer in (c) (i) based on nuclei attraction force on the valence electrons.

………………….…………………………………………………………………............................

………………….…………………………………………………………………............................

………………….…………………………………………………………………............................

[ 2 marks]


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(d) X reacts with Z to form a compound.

(i) What is the type of the compound formed?

………………….…………………………………………………………………............................

[1 mark]

(ii) State one physical property of the compound formed.

………………….…………………………………………………………………............................

[1 mark]

(iii) Draw the electron arrangement for the compound formed.

[2 marks]

7 (a) Element X reacted with oxygen to form a compound which cannot conduct electricity at

any state. Suggest one example of element X.

Write chemical equation between element X and oxygen.

[3 marks]

(b) Table 7 shows the proton number of elements P, Q and R.

Element Proton Number

P 6

Q 11

R 17

Table 7

State the elements that combined together to form a compound that has a high melting point.

Explain the formation of the compound.

[6 marks]


4541 CHEMISTRY

(c)

[Proton number of : C = 6 ; O = 8 ; Na = 11 ; Cl = 17]

(i) State the type of compound, type of bond and type of particles of two substances.

(ii) Explain the formation of carbon dioxide and draw the diagram of electron arrangement of

the compound formed.

(d)

Identify U and solvent V. Explain the differences between two solutions.

8 Table 8.1 shows the electron arrangement of elements U, V and W.

Element Electron arrangement

U 2.6

V 2.1

W 2.8.1

(a) Based on the Table 8.1,

(i) Identify one metal and one non-metal element. [2 marks]

(ii) State the group and period of element W in the Periodic Table of Elements. [2 marks]

(iii) The reaction between element U and W produces a compound.

State one property for the compound.

Draw the electron arrangement for the compound formed. [3 marks]

Table 8.1

Carbon dioxide, CO2 Sodium chloride, NaCl

U

Solution Z

Cannot conduct electricity

No colour change on litmus paper

Solution Y

Can conduct electricity

Change the colour of red litmus

paper to blue

+ water + solvent V


4541 CHEMISTRY

(b) Table 8.2 shows the observations of element V and element W when react with water.

Element Observation

V

Element V

water

Element V, moves slowly at random on the water surface with a little ‘hissing’

sound.

The solution formed turns the colour of red litmus paper to blue.

W

Element W

water

Element W, moves rapidly at random on the surface of the water with a louder

‘hissing’ sound.

The solution formed turns the colour of red litmus paper to blue.

(i) Write the chemical equation when element V reacts with water. [3 marks]

(ii) Compare the reactivity of elements V and W when react with water.

Explain your answer. [4 marks]

(c) Diagram 8.3 show the set up apparatus used to compare the electrical conductivity of solution P

and solution Q.

Based on the observations in Diagram 8.3,

(i) Identify the type of compound of solution P and solution Q. [2 marks]

(ii) Explain why there is a difference in the observations. [4 marks]

Table 8.2

Solution Q

Carbon electrode

Solution P

Bulb lights up Bulb does not light up

Diagram 8.3


4541 CHEMISTRY

CHAPTER 6 : ELECTROCHEMISTRY

9 (a) Table 9.1 show the set up of apparatus of two experiments to investigate electrolysis

process by using different electrodes.

Experiment Apparatus set-up

I

II

Compare and contrast Experiment I and Experiment II. Include in your answer,

the observations at the anode and cathode,

the name of the products formed at the anode and cathode and

half

equations for the reactions at the electrodes in both cells. [10 marks]

(b) A student intends to electroplate an iron spoon with copper to prevent it from rusting.

Design a laboratory experiment to electroplate the iron spoon.

Your answer should consist of the following :

procedures of the experiment.

a labelled diagram showing the set up of apparatus.

half equations for the reactions at both electrodes.

observation at both electrodes [8 marks]

Table 9.1

Copper electrodes

Elektrod kuprum

Elektrod kuprum

Copper(II) sulphate solution

A

Copper(II) sulphate solution

Carbon electrodes

A


4541 CHEMISTRY

10 Diagram 10.1 shows the set-up of apparatus to investigate the electrolysis of magnesium chloride 1.0 mol

dm-3

solution.

Diagram 10.1

(a) (i) Based on Diagram 10.1, state the name of the products at the cathode and the anode.

Explain your answer in term of factor that affects discharge of ion.

[8 marks]

(ii) Predict the product at anode and cathode if magnesium chloride 1.0 mol dm-3

solution is

replace by magnesium chloride 0.0001 mol dm-3

solution.

[2 marks]

(b) Diagram 10.2 shows the set up of apparatus when cell X is combined with cell Y.

Compare cell X and cell Y base on ;

the name of the cells,

energy conversion,

the observations and half equations for the reactions at the electrodes in both cells.

. [10 marks]

Magnesium chloride 1.0 mol dm-3

A A

Carbon

electrodes

Copper plate

Magnesium

plate

P Q R S

Cell X Cell Y

Copper plate

Diagram 10.2

V

0.5 mol dm-3

Copper(II)

sulphate solution


4541 CHEMISTRY

CHAPTER 7 : ACIDS AND BASES

11 (a) Diagram 11.1 show the observation in test tube I and test tube II when hydrogen chloride in

tetrachloromethane and hydrogen chloride in water are reacted with zinc powder.

Test tube I II

Apparatus set-up

Hydrogen chloride in

tetrachloromethane

+ zinc powder

Hydrogen chloride in water

+ zinc powder

Observation No change. Bubbles of gas are produced.

Diagram 11.1

(i) State the ion that causes an acid shows its acidic properties.

……………………………………………………………………………………........................

[1 mark]

(ii) Explain why the differences in observation in test tube I and II.

……………………………………………………………………………………........................

……………………………………………………………………………………........................

[2 marks]

(iii) State the name of the gas produced in test tube II.

……………………………………………………………………………………........................

[1 mark]

(iv) Write the chemical equation for the reaction between zinc and hydrochloric acid.

……………………………………………………………………………………........................

[2 marks]

(b) Table 11.2 shows the information of the solution A, solution B and solution C.


4541 CHEMISTRY

Solution of A, B and C might be an acid or an alkali.

Solution Information

A Ionises completely.

The solution remains colourless when phenolphthalein is added.

B Ionises partially.

The solution remains colourless when phenolphthalein is added.

C Ionises completely.

The solution turns to pink when phenolphthalein is added.

Table 11.2

(i) Give an example for each of the solution.

(a) .........................................................................

(b) .........................................................................

(c) .........................................................................

[1 mark]

(ii) Which solution has the lowest pH?

……………………………………………………………………………………………………….

[1 mark]

(iii) Give a reason for your answer in (b) (i).

……………………………………………………………………………………………………….

[1 mark]

(iv) Vinegar consists of an ethanoic acid. Describe a chemical test to verify the acid without using an

indicator.

……………………………………………………………………………………………………….

……………………………………………………………………………………………………….

[2 marks]


4541 CHEMISTRY

12 Hydrochloric acid, HCl is a strong acid. Table 12.1 shows two solutions of hydrochloric acid, HCl with

different concentration.

Solution Concentration /

mol dm-3

pH

A 1.0 1.0

B 0.001 3.0

Table 12.1

(a) What is meant by acid?

……………………………………………………………………………………………………….

……………………………………………………………………………………………………….

[1 mark]

(b) pH value of the solution A and B are different. Explain why.

……………………………………………………………………………………………………….

……………………………………………………………………………………………………….

……………………………………………………………………………………………………….

[3 marks]

(c) Diagram 12.2 shows the set-up of apparatus for titration of 25 cm3 of 1.0 mol dm

-3 sodium hydroxide

solution with solution A, using phenolphthalein as indicator.

Solution A

25 cm3 of 1.0 mol dm

-3

sodium hydroxide solution

+ phenolphthalein indicator

Diagram 12.2


4541 CHEMISTRY

(i) State the colour change of the solution in the conical flask at the end point.

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

[1 mark]

(ii) State the type of the reaction occurred.

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

[1 mark]

(iii) Write the chemical equation for the reaction.

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

[1 mark]

(iv) Calculate the volume of solution A needed to neutralise the sodium hydroxide solution.

[3 marks]


4541 CHEMISTRY

CHAPTER 8 : SALT

13 (a) A student has carried out an experiment to construct an ionic equation for the formation of lead(II)

iodide.

Seven test tubes of the same size were labelled 1 to 7. A fixed volume of 5.0 cm3 of 1.0 mol dm

-3

potassium iodide solution was placed in each test tube.

0.5 cm3 of 1.0 mol dm

-3 lead(II) nitrate solution was added into test tube 1, 1.0 cm

3 into test tube 2

and so on until 3.5 cm3 was added into test tube 7.

The heights of the precipitate formed in each test tube were measured.

The results are shown in Table 13.1

Test tube 1 2 3 4 5 6 7

Volume of 1.0 moldm-3

lead(II) nitrate solution

/ cm3

0.5 1.0 1.5 2.0 2.5 3.0 3.5

Height of precipitate /cm 1.1 2.2 3.4 4.4 5.5 5.5 5.5

Table 13.1

(i) Based on Table 13.1, plot a graph of the height of the precipitate against volume of lead(II)

nitrate solution on a graph paper..

[3 marks]

(ii) Determine the volume of lead(II)nitrate solution that had reacted completely with 5.0 cm3 of

1.0 mol dm-3

potassium iodide.

[1 mark]

(iii) Using the volume obtained in (a) (ii), calculate the number of moles of lead(II) ions and iodide

ions that are required for the formation of lead(II) iodide.

Then, calculate the number of moles of iodide ions that has reacted with 1 mol of lead(II) ions.

[4 marks]

(iv) Write the ionic equation for the formation of lead(II) iodide.

[2 marks]


4541 CHEMISTRY

(b) Diagram 13.2 shows a series of reactions for compound A.

Compound A is insoluble in water.

(i) State the name of substances A , B , C and D. [4 marks]

(ii) State the ion presence in solution D that give the blue colour.

Describe a chemical test to verify the ion. [3 marks]

(iii) Why does gas B turns lime water milky?

Write the chemical equation for the reaction occurred. [3 marks]

14 Diagram 14 shows a series of reaction starting from lead(II) carbonate, PbCO3.

(a) Based on Diagram 14 :

Identify gas Y. Describe a chemical test to verify gas Y.

Describe a chemical test to determine the presence of anion in the solution X.

Compare and contrast the observation when solid X and lead(II) carbonate, PbCO3 are

heated.

Solution X + Gas Y + H2O

Diagram 14

Solid X

HNO3

PbO + Gas Y

Heat Crystallisation

PbCO3 +

Diagram 13.2

Compound A

(Green powder)

Colourless gas B

turns lime water

milky

Black powder C

Blue solution D

+

+

Colourless gas B

turns lime water

milky

Heat

+ Hydrochloric acid


4541 CHEMISTRY

CHAPTER 9 : MANUFACTURED SUBSTANCES IN INDUSTRY

15 (a) Diagram 15.1 shows the production of ammonium sulphate from the reaction between

substance X and substance Y. Substance X is produced from Contact process

whereas substance Y from Haber process.

Diagram 15.1

(i) State the name of substance X and substance Y.

X : …………………………………………………………………………

Y : ………………………………………………………………………… [2 marks]

(ii) State one use of ammonium sulphate in agriculture field.

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

(iii) Write the chemical equation for the reaction between substance X and substance Y.

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

(b) Diagram 15.2 shows the structure formula of a polymer.

H Cl

C C

H H

n

Diagram 15.2

(i) State the name of the polymer.

……………………………………………………………………………………………..

[1 mark]

Contact process

Haber process

X

Y

Ammonium sulphate


4541 CHEMISTRY

(ii) Draw the structure formula of it monomer.

[1 mark]

(iii) Disposal of the polymer by burning is not suitable. Give a reason.

……………………………………………………………………………………………..

[1 mark]

(iv) The polymer is not suitable to be buried for disposing. Give a reason.

……………………………………………………………………………………………..

[1 mark]

(v) Suggest how to solve the problems in (b) (iii) and (b) (iv).

……………………………………………………………………………………………..

[1 mark]

(c) There are four types of glasses that are used in our daily lives.

(i) Name the major component of glass.

……………………………………………………………………………………………..

[1 mark]

(ii) Table 15.3 shows three types of glasses and their uses.

Complete the table.

Type of glass Uses

Borosilicate glass Cookware

Laboratory glassware

............................................. Decorative lamp

Prism

............................................. Bottles

Mirrors

[2 marks]

(iii) Why is borosilicate glass suitable to make cookware and laboratory glassware?

……………………………………………………………………………………………..

[1 mark]

Table 15.3


4541 CHEMISTRY

16 Diagram 16 shows railway tracks and the arrangement of atom in alloy that made the railway tracks.

(a) State the name of the alloy X

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

[1 mark]

(b) State the name of atom M.

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

[1 mark]

(c) (i) Draw the arrangement of atoms in pure iron.

[1 mark]

(d) Explain the difference of hardness of alloy Y and pure iron.

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

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

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

[2 marks]

Alloy X

Atom iron

Atom M

Diagram 16


4541 CHEMISTRY

CHAPTER 10 : RATE OF REACTION

17 The following equation shows the decomposition of hydrogen peroxide at room condition using a

catalyst.

2H2O2 → 2H2O + O2

Oxygen gas was collected and the result shown in Table 17.

Time (s) Volume of oxygen gas (cm3)

0 0.0

10 15.0

20 25.0

30 32.5

40 38.0

50 42.0

60 45.5

70 47.5

80 49.0

90 50.0

100 50.0

Table 17

(a) Plot the graph of the volume of oxygen gas against time on a graph paper. [3 marks]

(b) Based on your graph in (a), calculate the rate of reaction at 20 s.

[2 marks]


4541 CHEMISTRY

(c) Why does the decomposition of hydrogen peroxide decreases with time?

..................……………………………………………………………………………………………..

[1 mark]

(d) (i) State one suitable substance that can be used as catalyst for this reaction.

…....................................................................................................................................................

[1 mark]

(ii) With reference to the collision theory, explain how does catalyst in (d) (i) affects the rate of

decomposition of hydrogen peroxide.

…....................................................................................................................................................

…....................................................................................................................................................

…....................................................................................................................................................

…....................................................................................................................................................

[3 marks]

18 Diagram 18 shows the set-up of apparatus to study the rate of reaction between hydrochloric acid with

sodium thiosulphate solution.

In this reaction, a 250 cm3 conical flask contained 50 cm

3 of 0.2 mol dm

-3 sodium thiosulphate solution,

Na2S2O3 is placed on a white paper marked with the ‘X’ sign.

5.0 cm3 of 2.0 mol dm

-3 hydrochloric acid was added to the sodium thiosulphate solution and the mixture is

swirled. At the same time the stopwatch was started. The time is taken as soon as the ‘X’ sign is no longer

visible.

Observer eye

‘X’ sign White paper

Sodium thiosulphate solution

+ Hydrochloric acid

250 cm3 conical flask

Diagram 17


4541 CHEMISTRY

(a) In this reaction, a precipitate is formed. What is the colour of the precipitate?

………………………………………………………………………………………………………….

[1 mark]

(b) Calculate the number of moles of HCl and the number of moles of Na2S2O3 used in the experiment.

[2 marks]

(c) The chemical equation for the reaction occurred in this reaction is :

Na2S2O3 + 2HCl → 2NaCl + S + SO2 + H2O

Based on the calculation in (b) and the chemical equation above, calculate the mass of the precipitate

formed.

[Given that the relative atomic mass of S = 32]

[2 marks]

(d) (i) State two factors that affect the rate of reaction in this experiment.

…………………………………………………………………………………………................

…………………………………………………………………………………………................

[2 marks]


4541 CHEMISTRY

(ii) By using any one of the factor that you are stated in (d) (i), explain how the factor that you are

stated in (d) (i) affect the rate of reaction.

…………………………………………………………………………………………................

…………………………………………………………………………………………................

…………………………………………………………………………………………................

…………………………………………………………………………………………................

…………………………………………………………………………………………................

[4 marks]

19 (a) Table 19 shows the data from three experiments that were carried out to investigate the factors that

affects the rate of reaction.

Experiment Reactants Temperature /0C

Time taken for all the

magnesium to dissolve

/s

I Excess hydrochloric acid

+ 0.2 g magnesium ribbon 30 50

II Excess hydrochloric acid

+ 0.2 g magnesium ribbon 40 20

III

Excess hydrochloric acid

+ 0.2 g magnesium ribbon

+ copper(II) sulphate solution

40 15

Table 19

(i) Write the chemical equation for the reaction between magnesium and hydrochloric acid.

Calculate the maximum volume of hydrogen gas produced.

[ Relative atomic mass : Mg =24 ; Molar gas volume : 24 dm3 mol

-1 at room condition ]

[5 marks]

(ii) Compare the rate of reaction between Experiment I and Experiment II or Experiment II and

Experiment III.

With reference to collision theory, explain why there is difference in the rate of reaction.

[5 marks]

(b) By using either the factor of size of reactant or concentration, describe an experiment how this factor

affecting the rate of reaction.

[10 marks]


4541 CHEMISTRY

CHAPTER 11 : CARBON COMPOUND

20 Diagram 20 shows the flow chart of reaction for compound J with molecular formula C3H7OH.

Based on the information in Diagram 20, answer the following questions :

(a) State the name of the compound J

…………………………………………………………………………………..............................................

[1 mark]

(b) State the name of the type of reaction occurring in Step I.

…………………………………………………………………………………..............................................

[1 mark]

(c) (i) State the name of the substance L which is used in Steps III and IV

……………………………………………………………………………............................................

[1 mark]

(i) What can you observe in Step III

……………………………………………………………………………............................................

[2 marks]

Compound J

C3H7OH

C3H6 gas

Substance P

C3H6(OH)2

Compound Q

C2H5COOH

Compound R

I II

Polymerisation

III IV

Porcelain chips

Heat

Substance L

Heat

V Compound J

Reflux with concentrated

sulphuric acid

Diagram 20

Substance L

Heat


4541 CHEMISTRY

(d) Draw the structural formulae of

(i) substance P formed in Step II

(ii) Compound Q formed in step IV

[2 marks]

(e) In step V, a mixture of compound Q, compound J and a few drops of concentrated sulphuric acid is

boiled under reflux for a few minutes.

(i) Draw the set up of the apparatus for this reaction.

[2 marks]

(ii) Write a chemical equation for this reaction.

…………………………………………………………………………….........................................

[1 mark]


4541 CHEMISTRY

21 Diagram 21.1 shows five structural formula of carbon compound.

Diagram 21.1

(a) Choose any one of the compound in Diagram 21.1, state the products formed when the compound

burn completely in excess oxygen gas. Write the chemical equation involve.

(b) State the name of two compounds in Diagram 21.1 that are isomer. Explain your answer.

(c) Describe a chemical test to differentiate between compound A and compound B.

(d) Diagram 21.2 shows the reaction between compound E and carboxylic acid.

Diagram 21.2

(i) Name an example of of carboxylic acid member that can be used in this reaction.

State the name of the ester formed when the carboxylic acid react with compound E.

Draw the structural formula of name the carboxylic acid and the ester that formed.

(ii) Describe an experiment to produce ester in (d) (i) in laboratory.

Compound E + Carboxylic acid → Ester

Sebatian E + Asid karboksilik →

ester

Compound D Compound E

Compound A Compound B Compound C


4541 CHEMISTRY

CHAPTER 12 : OXIDATION & REDUCTION

22 Diagram 22 shows the set-up of apparatus to investigate the reaction between iron(II) sulphate solution and

acidified potassium dichromate(VI) solution through the transfer of electrons at a distance.

(a) What is the colour of iron(II) sulphate solution?

………………………………………………………………………………………………………….

[1 mark]

(b) (i) Write the half equation for the reaction occur at X.

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

[1 mark]

(ii) State the change in oxidation number of iron.

…………………………………………………………………………………………...

[1 mark]

(c) The incomplete half equation occur at Y is :

Cr2O72-

+ ……. + 6e → …Cr3+

+ …H2O

Complete the equation. [1 mark]

(d) On the diagram above, show the direction of electrons flow. [1 mark]

Diagram 22


4541 CHEMISTRY

(e) You are provided with the following substances and apparatus :

(i) By using the given materials and apparatus, draw the set-up of apparatus to investigate the

redox reaction through transfer of electron at a distance.

[2 marks]

(ii) On your diagram in (e) (i), indicate the positive and negative terminal. [1 mark]

(iii) State the change in oxidation number for bromine in this reaction.

…………………………………………………………………………………………................

[1 mark]

Bromine water

Potassium iodide solution

Carbon electrodes

Beaker

Porous pot

Connecting wire


4541 CHEMISTRY

23 Diagram 23 shows the set-up of apparatus to investigate the reaction occurred in test tubes A and B.

(a) Based on test tube A,

(i) Name the reaction occurred.

................................................................................................................................................

[1 mark]

(ii) Write the ionic equation for the reaction.

................................................................................................................................................

[2 marks]

(iii) State a chemical test to verify the product formed.

................................................................................................................................................

................................................................................................................................................

[2 marks]

(b) Based on test tube B,

(i) State the observation involved.

................................................................................................................................................

[1 mark]

(ii) State the observation if the experiment is repeated by using copper to replace zinc.

................................................................................................................................................

[1 mark]

Diagram 23

Test tube A Test tube B


4541 CHEMISTRY

(c) Compare the answer in (b) (i) and (b) (ii) and explain why there is a difference in the observation.

.............................................................................................................................................................

.............................................................................................................................................................

.............................................................................................................................................................

[2 marks]

(d) When iron is exposed to water and oxygen, it rusts easily. State one method to prevent the

rusting of iron.

.............................................................................................................................................................

[1 mark]

CHAPTER 13 : THERMOCHEMISTRY

24 An experiment is conducted to study the heat of displacement for reaction between copper(II) sulphate and

excess zinc powder. 50.0 cm3 of 0.5 mol dm

-3 copper(II) sulphate solution is poured into a polystyrene cup

and the initial temperature is recorded. The excess zinc powder is added to the same polystyrene cup. The

mixture is stirred slowly and the highest temperature is recorded.

Initial temperature of copper(II) sulphate solution = 28.5 oC

Highest temperature of mixture = 33.5 oC

[Relative atomic mass : Cu=64; S=32; O=16; Zn= 65; Specific heat capacity of the solution ; 4.2 J g-1

oC

-1]

(a) What is the meaning of heat of displacement in this experiment?

.............................................................................................................................................................

.............................................................................................................................................................

[1 mark]

(b) Why does zinc in the form of powder is used in this experiment?

.............................................................................................................................................................

[1 mark]

(c) Write the ionic equation for the reaction in this experiment.

.............................................................................................................................................................

[2 marks]


4541 CHEMISTRY

(d) Based on the experiment, calculate :

(i) heat released

[1 mark]

(ii) number of mole of copper(II) sulphate that has reacted.

[1 mark]

(iii) heat of displacement in this reaction

[2 marks]

(e) Draw an energy level diagram for the reaction.

[2 marks]

(f) Why plastic cup is used in this experiment?

.............................................................................................................................................................

[1 mark]


4541 CHEMISTRY

25 (a) Diagrams 25.1 and 25.2 show two energy level diagrams.

Diagram 25.1 Diagram 25.2

(i) Compare both the energy level diagrams. Your explanation should include the following :

ionic equation

type of chemical reaction

energy content of reactants and products

[6 marks]

(ii) Based on Diagram 25.1, calculate the change in temperature of the solution if excess

magnesium powder is added to 50 cm3 of 0.2 mol dm

-3 iron(II) sulphate solution.

[Specific heat capacity of solution : 4.2 J g -1 o

C-1

]

[3 marks]

(b) Table 25.3 shows the heat released for Experiment I, II and III using different acid that has been

reacted with sodium hydroxide solution.

Experiment Chemical Equation Heat released (kJ)

I HCl + NaOH → NaCl + H2O 57

II CH3COOH + NaOH CH3COONa + H2O 54

III H2SO4 + 2NaOH Na2SO4 + 2H2O 114

Table 25.3

Based on Table 25.3, explain the difference in heat released between :

(i) Experiment I and Experiment II

(ii) Experiment I and Experiment III

[6 marks]

(c) Describe a laboratory experiment to determine the heat of displacement of metal by a more

electropositive metal. In your description, include the following aspects :

Materials and apparatus needed

Procedure of experiment

A table to collect data

Calculation method

[10 marks]

Energy

CaCl2 + Na2CO3

CaCO3 + 2NaCl

ΔH= + 12.6 kJ mol-1

MgSO4 + Fe

Mg + FeSO4

Energy

ΔH= - 200 kJ mol-1


4541 CHEMISTRY

CHAPTER 14 : CHEMICALS FOR CONSUMERS

26 (a) Diagram 26.1 shows the structure of anion parts of a soap and a detergent. These anions consist of

part A and part B as shown in the diagram.

Diagram 26.1

(i) Name part A and part B of the anions.

State the solubility of part A and part B in the cleansing action. [4 marks]

(ii) Compare the effectiveness of the cleansing action of the two anions shows in the Diagram 26.1

in hard water. Explain your answer.

Write an ionic equation to show the reaction of anion of soap in hard water.

[6 marks]

(b) Diagram 26.2 shows the label of soft drink.

Diagram 26.2

Based on the ingredient used, classify the type of food additives that contained in this soft drink.

[4 marks]

(c) A patient is suffering from tuberculosis for a period of time. Suggest a type of medicine that should

be taken and the prescription should be followed by the patient.

[4 marks]

Anion of a soap

Anion of a detergent

Part A Part B

Ingredient :

Water, citric acid, aspartame, octyl butanoate and tartazine. Expiry date : 03 Jan 2013


4541 CHEMISTRY

27 (a) (i) Polythene and polyvinyl chloride (PVC) is an examples of synthetic polymer.

Explain how disposal and burning of synthetic polymers causes environmental pollution.

[6 marks]

(ii) Suggest steps that can be taken to overcome environmental pollutions that stated in (a) (i).

[4 marks]

(b) (i) Composite materials are produced from combination of two or more different compounds.

Fibre glass is a type of composite compound.

Describe on fibre glass in terms of :

main component

special properties

uses

[4 marks]

(c) (i) State the main component of glass and one difference between ceramic and glass.

(ii) State the uses of ceramic in the fields of construction, electronics, medical and astronomy.

[6 marks]


4541 CHEMISTRY

4541/3 : CHEMISTRY PAPER 3

1 Table 1 shows three experiments to investigate the solubility of salts in water.

(a) Write the

observation for Experiment I, II and III in Table 1. [3 marks]

Experiment Reaction Observation

I

II

III

Table 1

water

Lead(II) nitrate

Colourless

solution

water

Calcium carbonate

water

Copper(II) sulphate

Blue

solution


4541 CHEMISTRY

(b) Based on Experiment I and III, state the operational definition of soluble salt.

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

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

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

[3 marks]

(c) When calcium nitrate solution is added into sodium carbonate solution, white precipitate calcium

carbonate is formed. If potassium carbonate solution is used to replace sodium carbonate solution,

the same salt is produced. Explain why?

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

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

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

[3 marks]

(d) Classify the following salts into soluble salts and insoluble salts.

Soluble Salt Insoluble Salt

[3 marks]

Potassium sulphate, Lead(II) sulphate, Barium sulphate, Zinc sulphate


4541 CHEMISTRY

2 Table 2 shows observation on an experiment to investigate the solubility of salts in water.

Type of salt Solubility in water

X chloride Soluble

Y sulphate Insoluble

Table 2

Based on the information in Table 2, plan a laboratory experiment to investigate the solubility of the salts

with one example for each of the salt.

Your planning should include the following :

(a) Problem statement

(b) All the variables

(c) Hypothesis

(d) List of materials and apparatus

(e) Procedure

(f) Tabulation of data

Sample Answer :

Question 2

(a) Problem statement :

Does different type of ……………. gives different ……………… in water?

(b) Variables :

Manipulated variable : …………………………………

Responding variable : …………………………………

Constant variable : Volume of water

(c) Hypothesis :

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


4541 CHEMISTRY

(d) Materials :

……………… chloride, ……………… sulphate, ………………….

Apparatus :

Beakers/Test tubes, measuring cylinder, electronic balance, glass rod, spatula

(e) Procedure :

1. 100 cm3 of distilled water is measured by using measuring cylinder.

2. The distilled water is poured into a beaker.

3. 5 g of ……………… chloride is weight .

4. The ……………… chloride is put into the beaker.

5. The mixture is stirred.

6. Solubility of the salt in water is recorded.

7. Step 1-6 is repeated using …………… sulphate.

(f) Tabulation of data :

Type of Salt Solubility (√)

Soluble Insoluble

……………… chloride

……………… sulphate

Type of Salt Observation

……………… chloride

……………… sulphate


4541 CHEMISTRY

3 An experiment is carried out to determine the heat of combustion of four alcohols, methanol (CH3OH),

ethanol (C2H5OH), propanol (C3H7OH) and butanol (C4H9O11). The initial mass of spirit lamp containing

alcohol is measured before burning the alcohol. Then, 200 cm3 of water is heated with alcohol in the spirit

lamp until the temperature of water rises by 30 °C. The final mass of lamp containing alcohol is measured

again after burning.

Diagram 3.1 shows the set up of apparatus and thermometer reading of water for the experiment with

methanol.

Diagram 3.1


4541 CHEMISTRY

(a) Give one inference based on the observation in Diagram 3.1.

……………………………………………………………………………………………………………..

……………………………………………………………………………………………………………..

[3 marks]

(b) For this experiment, state :

(i) the manipulated variable

……………………………………………………………………………………………………….

(ii) the responding variable

……………………………………………………………………………………………………….

(ii) the fixed variable

……………………………………………………………………………………………………….

[3 marks]

(c) State one hypothesis for this experiment.

……………………………………………………………………………………………………………..

……………………………………………………………………………………………………………..

……………………………………………………………………………………………………………..

[3 marks]


4541 CHEMISTRY

(d) Table 3.2 shows the initial and final readings of the electronic balance for the mass of spirit lamp before

burning and after burning of four types of alcohol.

Table 3.2

Based on Table 2, state the mass of the alcohols used in space provided into two decimal places.

[3 marks]


4541 CHEMISTRY

(e) Calculate the heat of combustion of methanol.

[Specific heat capacity of water = 4.2 J g-1

°C-1

]

[Molar mass of methanol = 32 g mol-1

]

[3 marks]

(f) Given the heat of combustion of ethanol and butanol are -1175 kJ mol-1

and -2475 kJ mol-1

respectively.

By using the answer obtained in 3 (e), plot a graph of heat of combustion against number of carbon atoms

per molecule.

[3 marks]

(g) Using the plotted graph, predict the heat of combustion of propanol.

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

[3 marks]


4541 CHEMISTRY

4 Diagram 4 (a) and 4 (b) below shows the apparatus set up to study the effects of metals X and metal Y on

the rusting of iron.

Referring to the information in the diagram above, plan an experiment to investigate the effect of a named

X and Y metals on the rusting of iron.

Your planning should include the following aspects :

(a) Aim of the experiment

(b) All the variables

(c) Hypothesis

(d) List of materials and apparatus

(e) Procedure

(f) Tabulation of data

[17 marks]

Sample Answer :

Question 4

(a) Aim of the experiment :

To investigate the effect of ………………… and ………………… on the rusting of iron.

(b) Variables :

Manipulated variable : …………………………………

Responding variable : …………………………………

Constant variable : Iron nail

Potassium hexacyanoferrate(III) solution

+ phenolphthalein solution + hot jelly

Iron nail coiled

with metal X

Iron nail coiled

with metal Y

Diagram 4 (a) Diagram 4 (b)


4541 CHEMISTRY

(c) Hypothesis :

If iron nail is coiled with ……………………, the iron nail does not rust, if iron nail is coiled

with ……………………, the iron nail rust a lot.

(d) Materials :

Iron nails, ……………… strip, …………………. strip, potassium hexacyanoferrate(III)

solution, phenolphthalein solution, hot jelly.

Apparatus :

Test tubes, test tube rack, sand paper, beaker, glass rod and dropper

(e) Procedure :

1. Clean an iron nail and ………………… strip using sand paper.

2. Coil the iron nail with the ………………… strip.

3. Put the iron nail coil with the ………………… strip into a test tube (A).

4. Put the test tube in a test tube rack.

5. Pour liquid hot jelly into a beaker.

6. Add a few drops of potassium hexacyanoferrate(III) solution and phenolphthalein solution

into the beaker and stir the mixture.

7. Pour the mixture into the test tube.

8. Repeat step 1 to 7 using …………………… strip (B) to replace …………………. strip.

9. Set aside the test tubes for 3 days and record all the observations.

(f) Tabulation of data :

Test tube Observation

A :

Iron nail coiled with

………………………

B :

Iron nail coiled with

………………………


4541 CHEMISTRY

5 An experiment was carried out to construct an ionic equation for the precipitation of silver chloride

according to the following steps :

Step I : 5.00 cm3 of 1.0 mol dm

-3 potassium chloride solution was poured into 7 test tubes

labelled P, Q, R, S, T, U and V.

Step II : 1.00 cm3 of 1.0 mol dm

-3 silver nitrate solution was added to test tube P from a burette.

Step III : Step II was repeated for test tubes Q, R, S, T, U and V using different volumes of 1.0

mol dm-3

silver nitrate solution.

Step IV : All the test tubes were shakes and put it into in a test tube rack to allow silver chloride

precipitate to settle.

Step V : The height of the precipitate in the test tubes were measured and recorded in Table 5.1

Test tube P Q R S T U V

Volume of silver nitrate

solution (cm3)

1.00 2.00 3.00 4.00 5.00 6.00 x

Height of precipitate (cm) 1.0 2.0 3.0 4.0 5.0 5.0 5.0

Table 5.1

(a) Diagram 5.2 shows the initial and final burette reading for test tube V.

Based on Diagram 5.2, determine the value of x in Table 5.1.

x = final burette reading – initial burette reading

= …………………… – ………………………

= ……………………..…… cm3

40

41

47

48

Initial burette reading Final burette reading

Diagram 5.2


4541 CHEMISTRY

(b) Based on Table 5.1, plot a graph of height of precipitate against volume of silver nitrate solution on a

graph paper.

(i) On the graph, mark and write the minimum volume of silver nitrate solution needed for

complete reaction with 5.00 cm3 of 1.0 mol dm

-3 potassium chloride solution.

(ii) Using the volume obtained in (b) (i), calculate the number of moles of silver ion and chloride

ion used.

Then, calculate the number of mole of chloride ion that will react with 1.0 mol of silver ion.

(iii) Based on the calculation in (b) (ii), write the ionic equation for the formation of silver chloride.

…………………………………………………………………………………………………….

(c) Predict the height of precipitate formed when 3.50 cm3 of silver nitrate solution is added into 5.00

cm3 of 1.0 mol dm

-3 potassium chloride solution.

…………………………………………………………………………………………………………..

END OF MODULE

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