This document outlines various laboratory experiments designed to investigate chemical properties and reactions of elements and compounds, including the reactivity of alkali metals with water, comparison of halogens' reactivity with hot iron, acid-base properties of oxides across period 3, and effects of electrodes and electrolyte concentration in electrolysis. Each experiment includes a statement of the problem, hypotheses, manipulated and responding variables, materials, procedures, and methods for data tabulation. The aim is to understand key concepts in chemistry through practical application and observation.

1. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
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PERIODIC TABLE OF ELEMENTS
1.
Using the suitable apparatus and materials, you are required to design a laboratory experiment to
investigate / determine the reactivity of above mentioned elements when they react with
water.
Statement of problem:
How does the reactivity of lithium, sodium and potassium/group 1 elements change when
they react with water?
Variables:
Manipulated : Different types of alkali metals // Lithium, sodium, potassium
Responding : Reactivity of alkali metals with water
Constant variable: Size of alkali metals, water
Hypothesis:
When going down Group 1, the reactivity of the metals with water increases.
Lists of substances and apparatus
Lithium, sodium, potassium, water, small knife, forcep, basin, filter paper
Procedure:
1. Fill a basin / trough with water
2. Cut a small piece of lithium using a knife and forceps
3. Dry the oil on the surface of the lithium with filter paper
4. Place the lithium slowly onto water surface in a basin / trough
5. Record your observations
6. Repeat steps 1 – 5 using sodium and potassium to replace lithium one by one
Tabulation of data:
Alkali Metals Observations
Lithium
Sodium
Potassium
Three elements of group 1 in the Periodic Table
Lithium Sodium Potassium

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2. Chlorine and bromine show similar chemical properties but differ the reactivity.
By using a suitable reaction, plan an experiment to compare the reactivity of these elements.
Problem statement:
How does the reactivity of chlorine and bromine differ when they react with hot iron wool?
Variable:
Manipulated: Type of halogens // chlorine and bromine
Responding: reactivity of reaction (towards hot iron wool)
Fixed: iron wool
Hypothesis:
Chlorine is more reactive than bromine towards hot iron.
Apparatus and substances:
Combustion tube, delivery tubes, Bunsen burner, retort stand and clamp, stoppers
Chlorine gas, liquid bromine, iron wool, soda lime
Procedure:
1. Clamp combustion tube horizontally to the retort stand.
2. Place iron wool in the middle of the combustion tube.
3. Heat the iron wool in the combustion tube strongly.
4. Pass through chlorine gas over the hot iron wool until no further change occur.
5. The excess chlorine gas is absorbed by soda lime.
6. Record the observation.
7. Repeat the experiment by using bromine.
Tabulation of data
Halogens Observation
Chlorine gas
Liquid bromine

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3. Oxides can be classified into basic oxide, acidic oxide and amphoteric oxide. An oxide that
dissolves in acid only is a basic oxide. An oxide that dissolves in alkali only is an acid oxide. An
oxide that dissolves in both acid and alkali is an amphoteric oxide.
Plan a laboratory experiment to study the properties // acid-base properties of oxides of elements in
Period 3.
Problem statement:
How does the acid-base properties // pH values of oxides of elements change across Period 3?
Hypothesis :
An acidic property of the oxides of elements increases where as basic properties of the oxides of
elements decrease across period 3.
Variables :
Manipulated : oxides of element of Period 3
Responding variables: pH values in water // solubility in acid or alkali
Fixed : water // universal indicator // pH meter // nictric acid // sodium hydroxide solution
Apparatus :
Test tube, test tube rack, gas jar, gas jar cover, 100 cm3
measuring cylinder.
Material:
Sodium oxide, magnesium oxide, aluminium oxide, silicon (IV) oxide, phosphorus pentoxide,
sulphur dioxide gas, 1.0 mol dm-3
nictric acid and 1.0 mol dm-3
sodium hydroxide solution.
Procedure:
1. A small piece of sodium oxide is put into a test tube half filled with distilled water.
2. The mixture is shaken.
3. Three drop of universal indicator are added to the mixture using dropper // pH meter is dipped
into the mixture.
4. The colour of the mixture is observed and the pH value is recorded.
5. The procedure is repeated for the other oxides.
Tabulation of data:
Oxides Solubility in water and pH values

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(a)
Procedure:
1. A little / 0.5 g // half spatula R2O3 powder is put into two separate test tubes.
2. 5 cm3
of 1.0 mol dm-3
sodium hydroxide solution is added into the first test tube.
3. 5 cm3
of 1.0 mol dm-3
nitric acid is added into the second test tube.
4. Both test tubes are heated slowly.
5. Repeat step 1-4 for MO and TO2.
6. Record the observations.
(b) Variables:
manipulated: oxide R2O3, MO and TO2
Responding : acid-base properties
Fixed : sodium hydroxide solution, nitric acid
(c) R2O3 – amphoteric oxide
MO – basic oxide
TO2 – Acidic oxide
(d) M, R, T
(e) MO insoluble in water

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TOPIC: CHEMICAL BONDS
Diagram
4. Diagram shows the apparatus set-up for an experiment to compare the electrical conductivity
between two types of chemical compound, P and Q.
(a) Problem statement:
How does the type of compounds affect the electrical conductivity?
(b) Variable:
Manipulated : Type of chemical compound
Responding : Electrical conductivity / the light of the bulb
Controlled : carbon electrode / Mass of the substance
(c) Hypothesis :
Ionic compound can conduct electricity while covalent compound does not conduct
electricity in molten state.
(d) Materials
solid lead(II)bromide , naphthalene, C10H8
Apparatus
Crucible, Batteries, Bulb, Carbon electrodes, Tripod stand, Bunsen burner, Pipe-clay
triangle, Connecting wire and crocodile clip.
(e) Procedure :
1 Fill a crucible with a solid lead(II)bromide, PbBr2 until it is half full.
2 Connect the carbon electrodes to the batteries and bulb.
3 Heat the solid lead(II)bromide until it melts.
4 Dip /place/ immerse carbon electrodes into the molten lead(II)bromide, PbBr2
5 Record the observation.
6 Repeat steps 1 to 5 / experiment using naphthalene, C10H8
(f) Tabulation of data:
Chemical compound Observation
Lead(II)bromide
Naphthalene
P

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TOPIC: ELECTROCHEMISTRY
5. Plan a laboratory experiment to construct the electrochemical series based on the potential
difference between two metals. You are given copper (II) sulphate solution, Mg, Zn, Fe, Pb and Cu
strips.
(a) Aim:
To construct the Electrochemical series based on the potential difference between two
metals.
Statement of problem:
How does the Electrochemical series be constructed based on the potential difference
between two metals?
(b) Variable
Manipulated : pair of metal
Responding : potential difference / voltmeter reading/ voltage value
Fixed : electrolyte (copper (II) sulphate solution/ / positive (copper)
(c) Hypothesis :
The further the distance between two metals in the Electrochemical series, the higher the
potential differences/ voltage/ voltmeter reading.
(d) Substances : copper (II) sulphate solution 0.5 mol dm-3
, Mg, Zn, Fe, Pb and Cu strips, sand
paper
Apparatus: beaker, connecting wire with crocodile clip, voltmeter
(e) Procedure : 1. Clean the metals with sandpaper
2. Pour 50.0 cm3
copper (II) sulphate solution into a beaker.
3. Dip / immerse the Mg and Cu strip into the beaker.
4. Complete the circuit // connect the electrodes to a voltmeter using connecting
wire with crocodile clip.
5. Record the potential difference / voltmeter reading.
6. Repeat steps 1 to 5 using Zn, Fe and Pb to replace Mg.
(f) Tabulation of data:
Pair of metal Potential difference, V
Zn and Cu
Mg and Cu
Fe and Cu
Pb and Cu

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Diagram 2.1 Battery [voltaic cell / electrochemical cell]
6. Diagram shows several electrochemical cells with different voltages. Identify the factors that
influence the differences in the voltage.
Plan a laboratory experiment to construct an electrochemical cell to determine one factor that
influences the differences in the voltage.
(a) Statement of problem:
How does //Does the position /distance between two metals in electrochemical series affect
the voltmeter reading / voltage/ potential difference?
(b) Variable
Manipulated : pair of metal
Responding : potential difference / voltmeter reading/ voltage value
Fixed : electrolyte (name) / positive terminal (name) /
volume and concentration of electrolyte
(c) Hypothesis :
The further the distance between two metals electrode in the Electrochemical Series,
the higher the potential differences/ voltage/ voltmeter reading.
d) Substances : copper (II) sulphate solution 0.5 mol dm-3
, Mg,Zn, Fe, Pb and Cu strips, sand paper
Apparatus : beaker, connecting wire with crocodile clip, voltmeter
(e) Procedure : 1. Clean the metals with sandpaper
2. Pour 50.0 cm3
copper (II) sulphate solution into a beaker.
3. Dip / immerse the Mg and Cu strip into the beaker.
4. Complete the circuit // connect the electrodes to a voltmeter using connecting
wire with crocodile clip.
5. Record the potential difference / voltmeter reading.
6. Repeat steps 1 to 5 using Zn, Fe and Pb to replace Mg.
(f) Tabulation of data:
Pair of metal/electrode Potential difference, V
Zn and Cu
Mg and Cu
Fe and Cu
Pb and Cu

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7. Diagram 6.1 and 6.2 show Experiment I and Experiment II to investigate the effect of type of
electrodes on the products formed at the electrodes.
Experiment I
Experiment II
Based on Diagram 6.1 and Diagram 6.2 above, plan a laboratory experiment to investigate the effect
of the type of electrode to the product at anode.
(a) Aim :
To determine the effect of type of electrode on the selection of ions to be discharged at the
anode/ on the product formed at the anode.
(b) Variable:
Manipulated variable:
Type of electrodes//Carbon electrodes and copper electrodes
Responding variable:
Product formed at anode
Fixed variable:
Electrolyte// copper(II)sulpahte solution
(c) Hypothesis:
When carbon electrodes are used, bubbles/oxygen gas released at anode, when copper
electrodes are used, anode becomes thinner/ionised
Diagram 6.1
After 30 minutes
Carbon electrodes Carbon electrodes
After 30 minutes
Copper electrodes
0.01 mol dm-3
copper(II)
sulphate solution
Diagram 6.2
0.01 mol dm-3
copper(II)
sulphate solution
0.01 mol dm-3
copper(II)
sulphate solution

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(d) Materials:
Copper(II) sulphate solution (0.5 – 2.0) mol dm-3
, copper rods,
Apparatus:
Carbon rods, electrolytic cell, battery, ammeter, connecting wires, test tube
(e) Procedure:
1. Half filled the electrolytic cell/beaker with copper(II) sulphate solution
2. A test tube filled with copper(II) sulphate solution is inverted over the anode carbon
electrode
3. Both electrodes are connected to the batteries using connecting wires//Complete the circuit
4. Record the observations at the anode
(f) Tabulation of data:
Type of electrodes Observation at anode
Carbon
Copper

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8. The concentration of the electrolyte will affect the products formed at the electrodes during
electrolysis.
By using different concentration of sodium chloride solution, design an experiment to investigate
the above statement.
Problem statement:
How does the concentration of the electrolyte (sodium chloride solution) will affect the
products formed at the anode electrode during electrolysis?
Variable:
Manipulated: concentration of the electrolyte (sodium chloride solution)
Responding: products formed at the anode
Fixed: carbon electrodes, sodium chloride solution, blue litmus paper
Hypothesis:
When concentrated sodium chloride solution is used, greenish yellow gas released at the
anode, when diluted sodium chloride solution is used, colourless gas released at the anode.
Apparatus and Substances:
Carbon rods, electrolytic cell, battery, ammeter, connecting wires, test tubes
1.0 mol dm-3
sodium chloride solution, 0.0001 mol dm-3
sodium chloride solution, litmus paper
Procedure:
1. Half filled the electrolytic cell/beaker with 1.0 mol dm-3
sodium chloride solution.
2. A test tube filled with 1.0 mol dm-3
sodium chloride solution is inverted over the anode
carbon electrode.
3. Both electrodes are connected to the batteries using connecting wires//Complete the circuit
4. Record the observations at the anode.
5. Repeat step 1-4 by using 0.0001 mol dm-3
sodium chloride solution.
(f) Tabulation of data:
Concentration electrolyte /
sodium chloride solution
Observation at anode // Product at anode
1.0 mol dm-3
0.0001 mol dm-3

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9. The displacement reaction is a chemical change which takes place when a metal placed higher in
the electrochemical series displaces a metal below it from its salt solution.
Iron displaces copper from its salt solution because it is placed higher than copper in the
electrochemical series. Based on this principle, plan a laboratory to construct the electrochemical
series.
Problem statement:
How to construct the electrochemical series of metals based on the displacement of metals?
Hypothesis:
The greater the number of metals that can be displaced by a metal from their solutions, the higher is
its position in the electrochemical series.
Variables :
Manipulated : pair of metal and salts solution used
Responding : the number of displacement reactions occurred
fixed : concentration and volume of solution.
Apparatus: test tube, test tube rack
Materials: 1 mol dm-3
of magnesium nitrate, zinc nitrate, lead(II)nitrate, copper(II)nitrate solution.
Magnesium, zinc, lead, and copper strip.
Procedure:
1. Pour 5 cm3
1 mol dm-3
of magnesium nitrate, zinc nitrate, lead(II)nitrate, copper(II)nitrate
solution solutions into four separate test tubes.
2. Place a strip of magnesium ribbon into each test tube.
3. Record the observation.
4. Repeat step 1-3 using zinc, lead and copper to replace the magnesium strip. For each repetition,
use a fresh salt solution.
5. Record all observations.
Tabulation Data:
solution
salt
Metal
Magnesium
nitrate
Zinc nitrate Lead(II) nitrate Copper(II)
nitrate
Mg
Zn
Pb
Cu

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TOPIC: ACIDS AND BASES
10.
Plan a laboratory experiment to investigate the role of water in showing the properties of acids.
(a) Statement of problem:
Does an acid need water to show its acidic properties?
(b) Variable
Manipulated : type of solvents (water and tetrachloromethane/ propanone)
Responding : properties of acid / change in colour of blue litmus paper
Fixed : type of acid (ethanoic acid), litmus paper
(c) Hypothesis :
Water is needed for an acid to show its acidic properties // An acid will show its acidic
properties when dissolved in water.
* Operational definition: Blue litmus paper turning red when water is added to glacial
ethanoic acid indicates acidic properties.
(d) Materials:
Glacial ethanoic acid, distilled water and tetrachloromethane/ propanone, blue itmus paper
Apparatus:
Test tube, droppers, test tube rack
(e) Procedure:
1. Label three test tubes as A, B and C. Place the test tube in a test tube rack.
2. Put 2 cm3
glacial ethanoic acid into each test tube using dropper.
3. Add 2 cm3
distilled water in test tube B
4. Add 2 cm3
tetrachloromethane/ propanone in test tube C.
5. Place dry blue litmus paper into the test tubes.
6. Record the observation.
(f) Tabulation of data
Test tube / solvents Observation
A
B / distilled water
C/ tetrachloromethane/ propanone
Glacial ethanoic acid, CH3COOH is dry. It only shows
acidic properties when water is added to it.

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11. An experiment is carried out to measure the pH values of hydrochloric acid having different
molarities.
Plan a laboratory experiment to investigate the relationship between pH values and molarity of the
acids.
Sample answer:
Statement of the problem:
How does the molarity of the acids affect the pH values?
Variable:
Manipulated : molarity of acid
Responding : pH value
Fixed : hydrochloric acid, pH meter
Hypothesis : When the molarity of the acid increases, the pH value decreases.
Materials : 0.1 mol dm-3
, 0.01 mol dm-3
, 0.001 mol dm-3
hydrochloric acid
Apparatus : beaker, pH meter, measuring cylinder.
Procedure:
1. pour 50 cm3
of 0.1 mol dm-3
hydrochloric acid into a beaker,
2. Dip pH meter into the acid.
3. Record the pH meter reading.
4. Repeat step 1 to 3 by using 0.01 mol dm-3
, 0.001 mol dm-3
hydrochloric acid.
Tabulation data:
Molarity of acid, mol dm-3
pH value
0.1
0.01
0.001

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TOPIC : SALTS
Diagram shows seven test tube containing lead(II)chromate(VI) precipitate which is formed when
lead(II)nitrate solution reacts with potassium chromate(VI) solution. Based on diagram, paln one
laboratory experiment to construct the ionic equation for the formation of lead (II) chromate(VI).
12. Aim : To construct the ionic equation for the formation of lead (II) chromate(VI)
Problem Statement:
How does an ionic equation for the formation of lead chromate (VI) can be constructed? // How to
construct an equation for the formation of lead chromate (VI)?
Hypothesis :
As the volume potassium chromate (VI) used is increases, the height of the yellow precipitate
increases until it achieves a maximum height // constant// no change
Variables:
Manipulated : Volumes of 0.5 mol dm-3
potassium chromate (VI) solution.
Responding : Height of yellow precipitate.
Fixed : Size of test tubes, volume and concentration of lead (II) nitrate solution,
concentration of potassium chromate (VI) solution.
Apparatus : Test tubes of the same size, test tube rack, burette, retort stand with
clamp, ruler, glass rod, dropper.
Material : 0.5 mol dm-3
potassium chromate (VI) solution, 0.5 mol dm-3
lead (II)
nitrate solution.
Procedure :
1. Seven test tubes of the same size were labelled from number 1 to 7. They were placed in a
test tube rack.
2. A burette was filled 0.5 mol dm-3
lead (II) nitrate solution, 5.00 cm3
of the lead (II)
nitrate solution was run into each the seven tubes.
3. Another burette was filled with 0.5 mol dm-3
potassium chromate (VI) solution.
4. 1 cm3
of potassium chromate (VI) solution from the burette was added into the first test
tubes
5. Repeat the experiment with different volume of potassium chromate(VI) solution. The
mixture in each test tube was stirred with a clean glass rod.
6. The test tubes were left aside for about an hour.
7. The height of the precipitate in each test tube was measured and recorded.
Results:
Test tube 1 2 3 4 5 6 7
Volume of 0.5 mol dm-3
K2Cr O4 /cm3
1.00 2.00 3.00 4.00 5.00 6.00 7.00
Height of precipitate (cm)

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Garden snail
13. The soft body of the garden snail is protected by its cone-shaped shell. What kind of chemical
compound found in the shell to give it its hardness and waterproof nature? Actually the above
mentioned shell consists of calcium carbonate, CaCO3. It is an insoluble salt. Referring to the
situation above, plan a laboratory experiment to compare the solubility of nitrate, sulphate,
carbonate and chloride salt in water.
Sample answer:
Problem statement:
How does solubility of nitrate, sulphate, carbonate and chloride salt in water? //
Does all nitrate, sulphate, carbonate and chloride salt soluble in water?
Variables
Manipulated: nitrate, sulphate, carbonate and chloride salt // Type of salts
Responding: solubility of salt
Fixed: volume and temperature of water // quantity of salt powder
Hypothesis:
Some of salts soluble in water but other salts insoluble in water //
Some of salts soluble in water, while some are not.
Material:
Any suitable nitrate, sulpahte, chloride and carbonate salts soluble and insoluble in water
distilled water.
Apparatus:
Test tube, test tube rack and spatula.
Procedure:
1. Half spatula of zinc nitrate powder is put into a test tube.
2. Pour 5 cm3
of distilled water into the test tube.
3. Stir the mixture / shake the test tube
4. Observe and record the solubility of salt.
5. Repeat step 1 to 4 by using various salt powder.
Tabulation of data:
Salt Solubility in water / observation
Zinc nitrate
Calcium sulphate
Potassium carbonate
Lead(II)chloride
Magnesium chloride
Copper(II) carbonate
Copper (II)sulphate

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TOPIC: MANUFACTURED SUBSTANCES IN INDUSTRY
14 . Copper wire in electric cable can be easily bent by hand. A coin cent made of an alloy of
copper with tin and zinc cannot be bent easily.
Referring to the situation above, plan a laboratory experiment to investigate the effect of alloy
formation on the hardness of a metal.
(a) Statement of problem:
Does the formation of alloy increase the hardness of a metal?
(b) Variable
Manipulated : copper and bronze / copper and brass
Responding : size of the dent made by the metal ball bearing on the block
Fixed : mass of the weight // type of metal ball // the height of the thread
(c) Hypothesis : Bronze is harder than copper
Operational definition: If smaller dent produced when I kg weights is dropped on the metal
block, then the metal block is harder.
(d) List of apparatus: copper block, bronze/ brass block, steel ball bearing, weight 1 kg, ruler,
rope, retort stand.
(e) Procedure
1. Put the steel ball bearing on the copper block.
2. Pull the rope that tied to the weight until the weight is 60 cm high on the copper block.
3. Drop the weight onto the steel ball bearing.
4. Measure the diameter of the dent made on the copper block and records it.
5. Repeat the activity 3/5 times.
6. Repeat step 1 to 5 by using the bronze block, replacing the copper block.
(f) Tabulation of data
Name of metal Diameter of the dent (cm) Average ,
cm1 2 3 4 5
Metal/ copper
Alloy / bronze

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15. You have learnt the steel is an alloy of iron. Steel is harder than pure iron.
Both iron and steel can rust when exposed to air and water. Do they rust at the same rate?
Aim : To compare the rate of rusting between iron, steel and stainless steel
Problem Statement:
How does the rate of rusting between iron, steel and stainless steel differ?
Hypothesis
Iron rust faster than steel and steel rust faster than stainless steel.
Operational definition for rusting: The more the blue colour produced, when the metal is placed
in test tube containing the mixture of hot jelly and potassium hexacyanoferrate (III) solution, the
higher the rate of rusting.
Variables
Manipulated: Iron, steel and stainless steel.
Responding : intensity / amount of dark blue colour / rate of rusting
Fixed : size of nail, concentration of solution, duration of rusting
Apparatus:
test tube, test tube rack
Materials:
iron nail, steel nail, stainless steel nail, mixture of hot jelly and potassium hexacyanoferrate (III)
solution.
Procedure:
1. Clean the nails with sand paper (to remove the rust from all the nails).
2. Place the iron nail, steel nail and stainless steel nail into the test tube A, B and C respectively.
3. Prepare a 5 % jelly solution by adding 5 g jelly to 100 cm3
of boiling water. Add a few drop of
potassium hexacyanoferrate (III) solution.
4. Pour the hot jelly into the test tubes until all the nails are fully immersed.
5. Leave the nails for 3 days.
6. Observe and record the intensity of the dark blue colour.
Test tube The intensity of the dark blue colour
A
B
C

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TOPIC: CARBON COMPOUNDS
16. Diagram shows two reagent bottles containing two colourless liquid of carbon compounds P and
Q respectively.
P Q
These two liquid are hexene and ethanioc acid.
Using suitable reagent, plan a laboratory experiment to identify the colourless liquid.
Problem statement:
How to determine and identify hexane and ethanoic acid (liquid P and liquid Q)?
Variables:
Manipulated variable: Hexene and ethanoic acid // Liquid P and Q
Responding variable: Colour change of reagent // gas bubbles release
Constant variable: Volume of hexene and ethanoic acid // acidified potassium
manganate(VII) // magnesium ribbon// zinc powder // calcium carbonate
Hypothesis
If liquid P decolourised purple colour of acidified potassium manganate(VII), so liquid P is
hexene // Acid will produce gas bubbles with Magnesium (Calcium carbonate)
Apparatus
Test tube, dropper, and stopper
Materials
Liquid P, Liquid Q, acidified potassium manganate(VII) solution / Magnesium ribbon, zinc
power or calcium carbonate chips)
Procedure:
1. 2 cm3
liquid P and liquid Q are poured into two different test tubes.
2. Three d r o p s o f a c i d i f i e d p o t a s s i u m m a n g a n a t e (VII) are added into the test
tubes // a piece of magnesium ribbon are dipped into the test tubes.
3. The test tubes are closed with stoppers.
4. The mixtures are shaken.
5. The observations are recorded.
Tabulation of data:
Liquid Observation
P
Q

19. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
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17.
Aim : To compare the elasticity of vulcanised and unvulcanised rubber
Problem statement:
How does (the elasticity of) vulcanised rubber differ from unvulcanised rubber?
Hypothesis: Vulcanised rubber is more elastic than unvulcanised rubber
Variable
Manipulated : vulcanised rubber and unvulcanised rubber
Responding : length of rubber strip / elasticity
Fixed : mass of weight, size of rubber
Material and apparatus:
Retort stand, bulldog clip, meter ruler, weight, vulcanised and unvulcanised rubber
Procedure:
1. Hang both rubber strips to the retort stand with bulldog clip.
2. Measure the initial length of both rubber strips and record.
3. Hang 50 g weight to the end of each rubber using bulldog clip.
4. Remove the weight and measure the length of both rubber strips and record.//
5. Record all the data obtained.
Result / Data
Type of rubber Initial length , cm Length after removal of weight , cm
vulcanised
unvulcanised

20. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
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18.
Aim : To compare / investigate the strength of vulcanised and unvulcanised rubber
Problem statement:
How does the strength of vulcanised rubber differ from unvulcanised rubber?
Hypothesis:
Vulcanised rubber is stronger than unvulcanised rubber.
Variable:
Manipulated : vulcanised rubber and unvulcanised rubber
Responding : change in length of the rubber strip
Fixed : mass of weight, size of rubber strips
Material and apparatus:
Retort stand with clamp, bulldog clip, meter ruler, weight (20-50 g), vulcanised and
unvulcanised rubber strips.
Procedure:
1. Hang a strip of vulcanised rubber to the retort stand with clip / bulldog clip.
2. Measure and record the initial length of the rubber strip with meter ruler.
3. Hang (20-50) g weight to the bottom end of the rubber strip using clip / bulldog clip.
4. Measure and record the length of the rubber strips.
5. Repeat step 1-4 replacing vulcanised rubber with unvulcanised rubber.
Result / Data
Type of rubber Initial length , cm Final length , cm
vulcanised
unvulcanised

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19. An acid is used to coagulate latex while alkali can prevent the coagulation of latex. Based on
this idea, plan a laboratory experiment to investigate the effect of acid and alkali on the
coagulation of latex.
(a) Problem statement:
How does ethanoic acid and ammonia solution affects the coagulation of latex?
(b) Variable
Manipulated : ethanoic acid and ammonia solution
Responding : coagulate of latex
Fixed : latex
(c) Hypothesis :
Ethanoic acid coagulates the latex while ammonia solution does not coagulate the latex.
(d) Materials:
Latex , ethanoic acid 0.5 mol dm-3
and ammonia solution
Apparatus:
Beaker, measuring cylinder, glass rod, dropper
(e) Procedure:
1. 10 cm3
of latex is poured into a beaker.
2. ethanoic acid is added into the beaker using a dropper.
3. The mixture is stirred using glass rod.
4. The beaker is left aside.
5. Experiment is repeated using ammonia solution to replace ethanoic acid.
6. The observation is recorded.
(f) Tabulation of data
Mixture Observation
Latex + ethanoic acid
Latex + ammonia solution

22. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
22
TOPIC : RATE OF REACTION
20. Building in industrial areas are more corroded than those in housing areas. This is because the
concentration of acid in rain water is higher in industrial areas.
Referring to the situation above, plan a laboratory experiment to investigate the effect of
concentration on the rate of reaction between a named acid and a named metal.
(a) Statement of problem:
Does the increases in the concentration acid increases the rate of reaction? //
How does the concentration of acid affect the rate of reaction?
(b) Variable:
Manipulated : concentration of hydrochloric acid.
Responding : rate of reaction
Fixed : volume of hydrochloric acid / mass of zinc
(c) Hypothesis :
The higher the concentration of hydrochloric acid the higher the rate of reaction.
(d) Materials : hydrochloric acid, 0.5 mol dm-3
, zinc powder.
Apparatus : stopwatch, conical flask, beaker,
(e) Procedure:
1. 25 cm3
hydrochloric acid is measured using measuring cylinder and poured into a beaker
2. a spatula of zinc powder is put into the beaker.
3. Stopwatch is started immediately.
4. The mixture in the conical flask is swirled
5. Time is recorded for all zinc dissolve.
6. The experiment is repeated by using different concentarion of hydrochloric acid.
(f) Tabulation of data:
Concentration of hydrochloric acid,
mol dm-3
Time for all zinc dissolve, s
1.0
0.5
0.1

23. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
23
21. Aim: to investigate effect of catalyst on the rate of decomposition hydrogen peroxide.
Problem statement: How does a catalyst affect the rate of decomposition hydrogen peroxide?
Hypothesis: manganese (IV) oxide, MnO2 increases the rate of decomposition of hydrogen
peroxide
Variables:
Manipulated : presence of manganese (IV) oxide (MnO2)
Responding : rate of reaction
Fixed : concentration of H2O2 // initial temperature of H2O2 solution.
Apparatus: test tube, 10 cm3
measuring cylinder, test tube rack, spatula.
Materials: (5-10) – volume of H2O2 solution, manganese (IV) oxide (MnO2) powder, wooden
splinter
Procedures:
1. Label two test tube as A and B
2. Using a measuring cylinder measure 5 cm3
of 20 – volume of H2O2 solution and pour
into test tube A.
3. Add ½ spatula (0.1-1.0 g) of manganese (IV) oxide powder into test tube A.
4. Shake the test tube.
5. Immediately place a glowing splinter into the test tube.
6. Observe and record the changes.
7. Repeat step (2 - 6) // he same procedure for test tube B without MnO2
Tabulation of data
Test tube Observation
A// presence of manganese (IV)
oxide// catalyst
B// with manganese (IV) oxide //
catalyst

24. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
24
Referring to the situation above, plan a laboratory experiment to investigate the effect of
concentration or catalyst on the rate of reaction between a named acid and a named metal.
22.
(i) Problem statement:
How does concentration of acid affect the rate of reaction?
Variables:
Manipulated variable : Concentration of acid (HCl)
Responding variable : Rate of reaction
Constant variable : Volume of acid //mass of metal
Hypothesis:
The higher the concentration of acid (HCl) , the higher the rate of reaction.
Materials
Zinc, (hydrochloric acid) [0.5 – 2.0] mol dm-3
, distilled water
Apparatus
Conical flask, measuring cylinder, stopper, delivery tube, basin, retort stand, burette, and
stopwatch.
Procedure:
1. A burette is filled with water and inverted into a basin of water. The initial burette
reading is recorded
2. (50-100) cm3
of acid [0.5 – 2.0] mol dm-3
acid is measured and poured into a conical
flask.
3. 2 g of zinc powder is added into conical flask
4. The conical flask is closed immediately.
5. At the same time, the stopwatch is started.
6. The burette readings at intervals of 30 seconds are recorded until reaction stops.
7. The experiment is repeated using the same volume of acid with different concentration.
Tabulation of data:
Time(s) 0 30 60 90 120 150 180 210 240 270 300
Burette
Reading(cm3
)
Metal reacts with acid to form salt and hydrogen gas.

25. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
25
23.
(ii) Problem statement:
Does the presence of catalyst, copper(II) sulphate, increase the rate of reaction?
Variable:
Manipulated variable : Catalyst // copper(II) sulphate
Responding variable : Rate of reaction
Constant variable : Volume and concentration of acid // mass of metal
Hypothesis:
The presence of catalyst, copper(II) sulphate , increase the rate of reaction.
Materials
Zinc powder, copper(II)sulphate solution, water, acid [0.5 – 1.0] mol dm-3
Apparatus
Conical flask cm3
, measuring cylinder, stopper with delivery tube, basin, retort stand, burette,
stopwatch.
Procedure:
1. A burette is filled with water and inverted into a basin of water. The initial burette
reading is recorded
2. (50-100) cm3
of acid [0.5 – 1.0] mol dm-3
acid is measured and poured into a conical
flask.
3. 5 cm3
of acid 0.5 mol dm-3
copper(II)sulphate solution is added into conical flask
4. 2 g of zinc powder is added into conical flask
5. The conical flask is closed immediately.
6. At the same time, the stopwatch is started..
7. The burette readings at intervals of 30 seconds are recorded until reaction stops.
8. The experiment is repeated without adding copper(II) sulphate solution
Time(s) 0 30 60 90 120 150 180 210 240 270 300
Burette
Reading(cm3
)
Volume of
gas(cm3
)

26. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
26
TOPIC: REDOX
24. The rusting of iron can be affected by the present of other metal that is in contact with iron.
Plan a laboratory experiment to investigate the effect of metal on the rusting of iron.
(a) Aim:
To investigate the effect of different types of metals in contact with iron on the rusting.
Statement of problem:
How does different type of metals in contact with iron affect rusting?
(b) Variable
Manipulated : metals (Magnesium and Copper)
Responding : the rusting of iron
Fixed : iron nail, jelly solution mix with potassium hexacyanoferrate(III) and
Phenolphthalein.
(c) Hypothesis:
When a more electropositive metal is in contact with iron, the metal inhibits rusting.
When a less electropositive metal is in contact with iron, the metal speeds up rusting.
(d) Materials:
Iron nail, magnesium, copper strips, jelly solution mix with potassium hexacyanoferrate(III)
and phenolphthalein, sandpaper.
Apparatus:
test tube, test tube rack.
(e) Procedure:
1. Clean iron nail, magnesium and copper strip with sand paper.
2. Coil two iron nails tightly with magnesium and copper strip.
3. Place the iron nails into separate test tubes.
4. Pour the hot jelly solution mix with potassium hexacyanoferrate(III) and phenolphthalein
into the test tubes.
5. Keep the test tubes in a test tube rack and leave them aside for two days.
6. Record the observation.
(f) Tabulation of data
Pair of metal Observation
Fe-Mg
Fe-Cu

27. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
27
25. Way to store metals in laboratory depends on their reactivity with oxygen. The reactivity of the
metals is compared by observing how fast or how vigorous they react. Generally, the more vigorous
a metal burns in oxygen, the more reactive the metal is.
Based on this idea, plan a laboratory experiment to investigate the reactivity of magnesium, copper,
zinc and lead with oxygen.
Aim:
To investigate the reactivity of magnesium, copper, zinc and lead with oxygen
Variable:
manipulated: magnesium, copper, zinc and lead
responding: reactivity with oxygen
Fixed : solid potassium manganate(VII)
Hypothesis:
The higher the position of metal in reactivity series, the higher the reactivity of metal with oxygen.
Apparatus:
Boiling tube, retort stand and clamp, Bunsen burner, spatula and forceps
Material:
Magnesium, copper, zinc and lead powder, solid potassium manganate(VII), asbestos paper, glass
wool.
Procedure:
1. Put one spatula of potassium manganate(VII), KMnO4 , into a boiling tube.
2. Push some glass wool into the boiling tube and clamp horizontally.
3. Place one spatula magnesium powder on a piece of asbestos paper
and put into the boiling tube.
4. Heat magnesium powder strongly and then heat the solid KMnO4.
5. Observe and record how vigorous the reaction.
6. Repeat step 1 to 5 using copper, lead and zinc powder.
Tabulation of data:
Metal Vigour of reaction
Magnesium
Copper
Lead
Zinc

28. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
28
TOPIC: THERMOCHEMISTRY
26. Plan a laboratory experiment to compare the heat of neutralization between a named strong
acid with sodium hydroxide solution and heat of neutralization between named weak acid with
sodium hydroxide solution.
(a) Statement of problem:
Does heat of neutralization between hydrochloric acid and sodium hydroxide solution is
higher than heat of neutralization between ethanoic acid with sodium hydroxide solution?
(b) Variable
Manipulated : type of acids
Responding : heat of neutralization
Fixed : volume and concentration of acid / volume and concentration of alkali
(c) Hypothesis :
Reaction between hydrochloric acid and sodium hydroxide solution has
higher heat of neutralization than reaction between ethanoic acid with sodium
hydroxide solution.
(d) Materials / Substances:
Hydrochloric acid, 0.5 mol dm-3
and sodium hydroxide, 0.5 mol dm-3
, ethanoic acid
0.5 mol dm-3
Apparatus : polystyrene cup, measuring cylinder, thermometer
(e) Procedure :
1. 50 cm3
of sodium hydroxide solution is measured and pour into a polystyrene cup.
2. The initial temperature of the solution in measured and recorded.
3. 50 cm3
of hydrochloric acid is measured and pour into a polystyrene cup.
4. The initial temperature of the solution in measured and recorded.
5. Hydrochloric acid is poured into the sodium hydroxide solution.
6. The mixture is stirred using thermometer and the highest temperature is recorded.
7. The experiment is repeated using ethanoic acid.
(f) Tabulation of data
Acid Hydrochloric acid Ethanoic acid
initial temperature NaOH, o
C
initial temperature acid ,o
C
highest temperature of the mixer ,o
C
highest temperature of the mixer, o
C

29. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
29
27. Different type of alcohols produces different heat of combustions. When the number of
carbon per molecule of alcohol increases the heat of combustion increases. Table shows the heat
of combustion of ethanol, propanol and butanol.
Alcohol Molecular formula Heat of combustion/ kJ mol-1
Ethanol C2H5OH -1376
Propanol C3H7OH -2016
Butanol C4H9OH -2678
Plan a laboratory experiment to compare the heat of combustion of the alcohols.
The heat of combustion for alcohols
(a) Statement of problem:
` Does a different type of alcohol have different heat of combustion //
How does the number of carbon atom per molecule of alcohol affect the heat of
combustion?
(b) Manipulated variable:
Different type of alcohols //
Different alcohols such as ethanol, propanol and butanol.
Responding variable:
Heat of combustion//Increase in temperature
Fixed variable:
Volume of water // type of container/ size of container
(c) Hypothesis:
When the number of carbon per molecule of alcohol increases, the heat of
combustion increases.
(d) Materials
Methanol, Ethanol, propanol, butanol, water,.
Apparatus
copper can, spirit lamp, thermometer, weighing balance, wooden block, tripod stand,
wind shield, measuring cylinder
(e) Procedure:
1. [200 cm3
] of water is poured into a [copper can].
2. Initial temperature of the water is recorded.
3. A spirit lamp is half filled with methanol.
4. Weight the spirit lamp with ethanol and record the mass
5. The spirit lamp is put under the copper can and ignites the wick immediately.
6. The water is stirred and the flame is put off after the temperature has increased by 30o
C.
7. The highest temperature of the water is recorded
8. Immediately weight the spirit lamp and record the mass.
9. The experiment is repeated t by replacing ethanol with ethanol, propanol and butanol.
(
Table

30. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
30
f) Tabulation of data:
Types of
alcohols
Initial
temperature/o
C
Highest
temperature/o
C
Initial mass of spirit
lamp/g
Final mass of spirit
lamp/g
Methanol
Ethanol
Propanol
Butanol
TOPIC: CHEMICALS FOR CONSUMERS
28. Diagram shows the set-up of apparatus used to investigate the cleansing action of a cleaning
agent on a piece of cloth stained with oil.
Experiment Apparatus Observation
I Oil stained remains
II
Oil stained remains
Diagram
Based on the above diagram, plan one laboratory experiment to compare the effectiveness
of cleaning agents A mad B on cleansing action in hard water.
(a) Aim:
To compare the effectiveness of cleaning agents A and B on cleansing action in hard water.
(b) Variable:
Manipulated variable: Cleaning agent A and B
Responding variable: Effectiveness of cleansing action
Fixed variable: Type of water//hard water
(c) Hypothesis
Cleaning agent B is more effective than cleaning agent A in hard water
(d) Material:
Hard water, cleaning agent A and B
Apparatus:
,2 beakers, 2 pieces of cloths stained with oil, galss rod

31. CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3
31
(e) Procedure:
1. [50 - 200] cm3
of hard water is poured into a beaker
2. Cleaning agent A is added into the beaker
3. A piece of cloth stained with oil is immersed in the solution
4. The cloth is shaken/rubbed/stirred
5. Observation is recorded
6. Repeat steps 1 – 5 by using cleaning B .
(f) Tabulation of data:
Type of cleaning agent Observation
Cleaning agent A
Cleaning agent A
Example of operational definition:
Operational
definition for
What is observed What you do
Rusting of iron Blue spots are formed When an iron is coiled with a less electropositive
metal is immersed into hot jelly added with
potassium hexacyanoferrate(III) solution
Coagulation of
latex
White solid formed When acid is added to the latex
Reactivity of
Group 1 elements
Its move vigorously on
the water surface.
Brighter flame is
formed.
When a metal which is lower in Group 1 is put in
basin half filled water.
When a metal which is lower in Group 1 is burn
and put into the gas jar filled with oxygen gas.
Precipitation of
silver chloride
White solid formed. When silver nitrate solution is added to sodium
chloride solution
Voltaic cell The needle of the
voltmeter deflects/
voltmeter shows a
reading.
When two different metals connected to voltmeter
are dipped into an electrolyte
An acid Blue litmus paper turn
red
When a blue litmus paper is dipped into a
substance which is dissolved in water
Reactivity of
halogen
The brighter flame
produced/formed
When halogen gas is flow through the heated
iron wool,
The hardness of
alloy
Smaller dent produced When the weights of I kg is dropped at height of
60 cm to hit the ball bearing which is tape on the
alloy block.
Rate of reaction time taken for `X~
mark to disappear from
sight is shorter
When the higher the concentration sodium
thiosulphate solution is added into sulphuric acid,.