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CONTOH SOALAN DAN JAWAPAN ESEI KERTAS 3

PERIODIC TABLE OF ELEMENTS

1.

Using the suitable apparatus and materials, you are required to design a laboratory experiment to

investigate / determine the reactivit o! a"ove mentioned e#ements $hen the react $ith $ater%

Statement o! &ro"#em'

How does the reactivity of lithium, sodium and potassium/group 1 elements change when

they react with water?

(aria"#es'

anipulated ! "ifferent types of al#ali metals // $ithium, sodium, potassium%esponding ! %eactivity of al#ali metals with water

&onstant variable! 'i(e of al#ali metals, water

Hy&othesis'

)hen going down *roup 1, the reactivity of the metals with water increases.

$ists of substances and apparatus

$ithium, sodium, potassium, water, small #nife, forcep, basin, filter paper

Proced)re'

1. +ill a basin / trough with water

. &ut a small piece of lithium using a #nife and forceps

-. "ry the oil on the surface of the lithium with filter paper

. lace the lithium slowly onto water surface in a basin / trough

0. %ecord your observations

. %epeat steps 1 2 0 using sodium and potassium to replace lithium one by one

Ta")#ation o! data'

3l#ali etals 4bservations

$ithium

'odium

otassium

. &hlorine and bromine show simi#ar chemica# &ro&erties ")t di!!er the reactivit .

1

5hree elements of group 1 in the eriodic 5able

Lithi)m Sodi)m Potassi)m


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6y using a suitable reaction, plan an experiment to compare the reactivity of these elements.

Pro"#em statement'

How does the reactivity of chlorine and bromine differ when they react with hot iron wool?

(aria"#e'

anipulated! 5ype of halogens // chlorine and bromine

%esponding! reactivity of reaction 7towards hot iron wool8

+ixed! iron wool

*&othesis'

&hlorine is more reactive than bromine towards hot iron.

A&&arat)s and s)"stances'

&ombustion tube, delivery tubes, 6unsen burner, retort stand and clamp, stoppers

&hlorine gas, liquid bromine, iron wool, soda lime

Proced)re'

1. &lamp combustion tube hori(ontally to the retort stand.

. lace iron wool in the middle of the combustion tube.-. Heat the iron wool in the combustion tube strongly.

. ass through chlorine gas over the hot iron wool until no further change occur.

0. 5he excess chlorine gas is absorbed by soda lime.

. %ecord the observation.

9. %epeat the experiment by using bromine.

Ta")#ation o! data

Halogens 4bservation

&hlorine gas

$iquid bromine

2


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-. 4xides can be classified into basic oxide, acidic oxide and amphoteric oxide. 3n oxide that

dissolves in acid only is a basic oxide. 3n oxide that dissolves in al#ali only is an acid oxide. 3n

oxide that dissolves in both acid and al#ali is an am&hoteric o+ide.

lan a laboratory experiment to study the properties // acid:base properties of oxides of elements in

eriod -.

Pro"#em statement'

How does the acid:base properties // pH values of oxides of elements change across eriod -?

*&othesis '

3n acidic property of the oxides of elements increases where as basic properties of the oxides of

elements decrease across period -.

(aria"#es '

anipulated ! oxides of element of eriod -

%esponding variables! pH values in water // solubility in acid or al#ali+ixed ! water // universal indicator // pH meter // nictric acid // sodium hydroxide solution

A&&arat)s '

5est tube, test tube rac#, gas ;ar, gas ;ar cover, 18 oxide, phosphorus pentoxide,

sulphur dioxide gas, 1.< mol dm:-nictric acid and 1.< mol dm:-sodium hydroxide solution.

Proced)re'

1. 3 small piece of sodium oxide is put into a test tube half filled with distilled water.. 5he mixture is sha#en.

-. 5hree drop of universal indicator are added to the mixture using dropper // pH meter is dipped

into the mixture.

. 5he colour of the mixture is observed and the pH value is recorded.

0. 5he procedure is repeated for the other oxides.

Ta")#ation o! data'

4xides 'olubility in water and pH values

3


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7a8

Proced)re'

1. 3 little /


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TOPIC' C*EMICAL BONDS

Diagram

. "iagram shows the apparatus set:up for an experiment to compare the electrical conductivity

between two types of chemical compound, and .

7a8 Pro"#em statement'

How does the type of compounds affect the electrical conductivity?

7b8 (aria"#e'

anipulated ! 5ype of chemical compound

%esponding ! @lectrical conductivity / the light of the bulb

&ontrolled ! carbon electrode / ass of the substance

7c8 *&othesis '

=onic compound can conduct electricity while covalent compound does not conduct

electricity in molten state.

7d8 Materia#s

solid lead7==8bromide , naphthalene, &1


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TOPIC' ELECTROC*EMISTR,

0. lan a laboratory experiment to construct the electrochemical series based on the potential

difference between two metals. Cou are given copper 7==8 sulphate solution, g, Dn, +e, b and &u

strips.

7a8 Aim'

5o construct the @lectrochemical series based on the potential difference between twometals.


How does the @lectrochemical series be constructed based on the potential difference

between two metals?

7b8 (aria"#e

anipulated ! pair of metal

%esponding ! potential difference / voltmeter reading/ voltage value

+ixed ! electrolyte 7copper 7==8 sulphate solution/ / positive 7copper8

7c8 *&othesis '

5he further the distance between two metals in the @lectrochemical series, the higher the

potential differences/ voltage/ voltmeter reading.

7d8 S)"stances! copper 7==8 sulphate solution


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"iagram .1 6attery Evoltaic cell / electrochemical cellF

. "iagram shows several electrochemical cells with different voltages. =dentify the factors that

influence the differences in the voltage.

lan a laboratory experiment to construct an electrochemical cell to determine one factor that

influences the differences in the voltage.

7a8 Statement o! &ro"#em'

How does //"oes the position /distance between two metals in electrochemical series affect

the voltmeter reading / voltage/ potential difference?

7b8 (aria"#e

anipulated ! pair of metal

%esponding ! potential difference / voltmeter reading/ voltage value

+ixed ! electrolyte 7name8 / positive terminal 7name8 /

volume and concentration of electrolyte

7c8 *&othesis '

5he further the distance between two metals electrode in the @lectrochemical 'eries,

the higher the potential differences/ voltage/ voltmeter reading.

d8 S)"stances ! copper 7==8 sulphate solution


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9. "iagram .1 and . show @xperiment = and @xperiment == to investigate the effect of type of

electrodes on the products formed at the electrodes.

E+&eriment I

E+&eriment II

6ased on "iagram .1 and "iagram . above, plan a laboratory experiment to investigate the effect

of the type of electrode to the product at anode.

7a8 Aim '

5o 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.

7b8 (aria"#e'

anipulated variable!

5ype of electrodes//&arbon electrodes and copper electrodes

%esponding variable!

roduct formed at anode

+ixed variable!

@lectrolyte// copper7==8sulpahte solution

7c8 *&othesis'

)hen carbon electrodes are used, bubbles/oxygen gas released at anode, when copper

electrodes are used, anode becomes thinner/ionised

8

Diagram -%.

&arbon electrodes


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7d8 Materia#s'

&opper7==8 sulphate solution 7


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0% 5he concentration o! the e#ectro#tewill affect the products formed at the electrodes during

electrolysis.

6y using different concentration of sodium chloride solution, design an experiment to investigate

the above statement.

Pro"#em statement'

How does the concentration of the electrolyte 7sodium chloride solution8 will affect theproducts formed at the anode electrode during electrolysis?

(aria"#e'

Mani&)#ated' concentration of the electrolyte 7sodium chloride solution8

Res&onding'products formed at the anode

Fi+ed'carbon electrodes, sodium chloride solution, blue litmus paper

*&othesis'

)hen 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.

A&&arat)s and S)"stances'

&arbon rods, electrolytic cell, battery, ammeter, connecting wires, test tubes

1.< mol dm:- sodium chloride solution,


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G. 5he displacement reaction is a chemical change which ta#es place when a metal placed higher in

the electrochemical series displaces a metal below it from its salt solution.

=ron displaces copper from its salt solution because it is placed higher than copper in the

electrochemical series. 6ased on this principle, plan a laboratory to construct the electrochemical

series.

Pro"#em statement'

How to construct the electrochemical series of metals based on the displacement of metals?

*&othesis'

5he greater the number of metals that can be displaced by a metal from their solutions, the higher isits position in the electrochemical series.

(aria"#es '

anipulated ! pair of metal and salts solution used

%esponding ! the number of displacement reactions occurred

fixed ! concentration and volume of solution.

A&&arat)s' test tube, test tube rac#

aterials! 1 mol dm:-of magnesium nitrate, (inc nitrate, lead7==8nitrate, copper7==8nitrate solution.

agnesium, (inc, lead, and copper strip.

Proced)re'

1. our 0 cm-1 mol dm:-of magnesium nitrate, (inc nitrate, lead7==8nitrate, copper7==8nitrate

solution solutions into four separate test tubes.

. lace a strip of magnesium ribbon into each test tube.

-. %ecord the observation.

. %epeat step 1:- using (inc, lead and copper to replace the magnesium strip. +or each repetition,

use a fresh salt solution.

0. %ecord all observations.

Ta")#ation Data!

so#)tion

sa#t

Meta#

agnesium

nitrate

Dinc nitrate $ead7==8 nitrate &opper7==8

nitrate

Mg

1n

P"

C)

11


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TOPIC' ACIDS AND BASES

1


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11. 3n experiment is carried out to measure the pH values of hydrochloric acid having different

molarities.

lan a laboratory experiment to investigate the relationship between pH values and molarity of the

acids.

Same ans$er'

Statement o! the &ro"#em'

*o$ doesthe molarity of the acids affect the pH values?

(aria"#e'

anipulated ! molarity of acid

%esponding ! pH value

+ixed ! hydrochloric acid, pH meter

*&othesis ')hen the molarity of the acid increases, the pH value decreases.

Materia#s !


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"iagram shows seven test tube containing lead7==8chromate7>=8 precipitate which is formed when

lead7==8nitrate solution reacts with potassium chromate7>=8 solution. 6ased on diagram, paln onelaboratory experiment to construct the ionic equation for the formation of lead 7==8 chromate7>=8.

.% Aim '5o construct the ionic equation for the formation of lead 7==8 chromate7>=8

Pro"#em Statement'

*o$ doesan ionic equation for the formation of lead chromate 7>=8 can be constructed? // *o$to

construct an equation for the formation of lead chromate 7>=8?

*&othesis '

3s the volume potassium chromate 7>=8 used is increases, the height of the yellow precipitate

increases until it achieves a maximum height // constant// no change

(aria"#es'

Mani&)#ated ' >olumes of =8 solution.

Res&onding ' Height of yellow precipitate.

Fi+ed ' 'i(e of test tubes, vo#)me and concentrationof lead 7==8 nitrate solution,

concentrationof potassium chromate 7>=8 solution.

A&&arat)s ' 5est tubes of the same si(e, test tube rac#, burette, retort stand with

clamp, ruler, glass rod, dropper.

Materia# '=8 solution, =8 solution from the burette was added into the first testtubes

0. %epeat the experiment with different volume of potassium chromate7>=8 solution. 5he

mixture in each test tube was stirred with a clean glass rod.

. 5he test tubes were left aside for about an hour.

9. 5he height of the precipitate in each test tube was measured and recorded.

Res)#ts'

Test t)"e . 6 : 4 - ;

>olume of


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.:. &opper wire in electric cable can be easily bent by hand. 3 coin cent made of an alloy of copper

with tin and (inc cannot be bent easily.

%eferring to the situation above, plan a laboratory experiment to investigate the effect of alloy

formation on the hardness of a metal.


"oes the formation of alloy increase the hardness of a metal?

7b8 (aria"#e

anipulated ! copper and bron(e / copper and brass

%esponding ! si(e of the dent made by the metal ball bearing on the bloc#

+ixed ! mass of the weight // type of metal ball // the height of the thread

7c8 *&othesis ! 6ron(e is harder than copper

O&erationa# de!inition' =f smaller dent produced when = #g weights is dropped on the metal

bloc#, then the metal bloc# is harder.

7d8 List o! a&&arat)s! copper bloc#, bron(e/ brass bloc#, steel ball bearing, weight 1 #g, ruler,

rope, retort stand.

7e8 Proced)re

1. ut the steel ball bearing on the copper bloc#.

. ull the rope that tied to the weight until the weight is < cm high on the copper bloc#.

-. "rop the weight onto the steel ball bearing.

. easure the diameter of the dent made on the co&&erbloc# and records it%

0. %epeat the activity -/0 times.

. %epeat step 1 to 0 by using the "ron>ebloc#, replacing the co&&erbloc#.

7f8Ta")#ation o! data

Bame of metal "iameter of the dent 7cm8 3verage ,

cm1 - 0

etal/ copper

3lloy / bron(e

.4%Cou have learnt the stee#is an alloy of iron. 'teel is harder than &)re iron.

6oth iron and steel can r)stwhen exposed to air and $ater. Do the r)st at the same rate?

16


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Aim '5o com&are the rate of rusting between iron, steel and stainless steel

Pro"#em Statement'

*o$ doesthe rate of rusting between iron, steel and stainless steel differ?

*&othesis=ron rust faster than steel and steel rust faster than stainless steel.

O&erationa# de!inition !or r)sting'5he more the blue colour produced, when the metal is placed

in test tube containing the mixture of hot ;elly and &otassi)m he+acano!errate 7III8solution, the

higher the rate of rusting.

(aria"#es

Mani&)#ated' =ron, steel and stainless steel.

Res&onding ' intensity / amount of dar# blue colour / rate o! r)sting

Fi+ed ' si(e of nail, concentration of solution, duration of rusting

A&&arat)s'

test tube, test tube rac#

Materia#s'

iron nail, steel nail, stainless steel nail, mixture of hot ;elly and &otassi)m he+acano!errate 7III8

solution.

Proced)re'

1. &lean the nails with sand paper 7to remove the rust from all the nails8.

. lace the iron nail, steel nail and stainless steel nail into the test tube 3, 6 and & respectively.

-. repare a 0 I ;elly solution by adding 0 g ;elly to 1


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1. "iagram shows two reagent bottles containing two colourless liquid of carbon compounds and

respectively.

5hese two liquid are hexene and ethanioc acid.

Using suitable reagent, plan a laboratory experiment to identify the colourless liquid.

Pro"#em statement'

How to determine and identify hexane and ethanoic acid 7liquid and liquid 8?

(aria"#es'

anipulated variable! Hexene and ethanoic acid // $iquid and

%esponding variable! &olour change of reagent // gas bubbles release

&onstant variable: >olume of hexene and ethanoic acid // acidified potassium

manganate7>==8 // magnesium ribbon// (inc powder // calcium carbonate

*&othesis

=f liquid decolourised purple colour of acidified potassium manganate7>==8, so liquid is

hexene // 3cid will produce gas bubbles with agnesium 7&alcium carbonate8

A&&arat)s

5est tube, dropper, and stopper

Materia#s$iquid , $iquid , acidified potassium manganate7>==8 solution / agnesium ribbon, (inc

power or calcium carbonate chips8

Proced)re'

1. cm-liquid and liquid are poured into two different test tubes.

. 5hree 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 7>==8 are added into the test

tubes // a piece of magnesium ribbon are dipped into the test tubes.

-. 5he test tubes are closed with stoppers.

. 5he mixtures are sha#en.

0. 5he observations are recorded.

Ta")#ation o! data'

$iquid 4bservation

18


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.;%

Aim '5o compare the elasticity of vulcanised and unvulcanised rubber

Pro"#em statement!

How does 7the elasticity of8 vulcanised rubber differ from unvulcanised rubber?

*&othesis'>ulcanised rubber is more elastic than unvulcanised rubber

(aria"#e

Mani&)#ated ! vulcanised rubber and unvulcanised rubber

Res&onding ! length of rubber strip / elasticity

Fi+ed ! mass of weight, si(e of rubber

Materia# and a&&arat)s!

%etort stand, bulldog clip, meter ruler, weight, vulcanised and unvulcanised rubber

Proced)re'

1 Hang both rubber strips to the retort stand with bulldog clip.

easure the initial length of both rubber strips and record%

- Hang 0< g weight to the end of each rubber using bulldog clip. %emove the weight and measure the length of both rubber strips and record.//

0 %ecord all the data obtained.

Res)#t / Data

5ype of rubber =nitial length , cm $ength after removal of weight ,cm

vulcanised

unvulcanised

1A.

19


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Aim '5o compare / investigate the strengthof vulcanised and unvulcanised rubber

Pro"#em statement!

How does the strengthof vulcanised rubber differ from unvulcanised rubber?

*&othesis'

>ulcanised rubber is strongerthan unvulcanised rubber.

(aria"#e'

Mani&)#ated ! vulcanised rubber and unvulcanised rubber

Res&onding ! change in length of the rubber strip

Fi+ed ! mass of weight, si(e of rubber strips

Materia# and a&&arat)s!

%etort stand with clamp, bulldog clip, meter ruler, weight 7


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.@. 3n acid is used to coagulate latex while al#ali can prevent the coagulation of latex. 6ased on

this idea, plan a laboratory experiment to investigate the e!!ect o! acid and a#?a#ion the

coagulation of latex.

7a8 Pro"#em statement'

How does ethanoic acid and ammonia so#)tion affects the coagulation of latex?

7b8 (aria"#e

anipulated ! ethanoic acid and ammonia so#)tion

%esponding ! coagulate of latex

+ixed ! latex

7c8 *&othesis '

@thanoic acid coagulates the latex while ammonia so#)tiondoes not coagulate the latex.

7d8 Materia#s'

$atex , ethanoic acid


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.% Aim'to investigate e!!ect o! cata#ston the rate of decomposition hydrogen peroxide.

Pro"#em statement' *o$ doesa catalyst affect the rate of decomposition hydrogen peroxide?

*&othesis! manganese 7=>8 oxide, n4increases the rate of decomposition of hydrogen

peroxide

(aria"#es'

anipulated ! presence of manganese 7=>8 oxide 7n48

%esponding ! rate of reaction

+ixed ! concentration of H4// initial temperature of H4solution.

A&&arat)s! test tube, 1< cm-measuring cylinder, test tube rac#, spatula.

Materia#s'70:18 oxide 7n48 powder, wooden

splinter

Proced)res'

1. $abel two test tube as 3 and 6. Using a measuring cylinder measure 0 cm-of < 2 volume of H4solution and pour

into test tube 3.

-. 3dd K spatula 78 oxide powder into test tube 3.

. 'ha#e the test tube.

0. =mmediately place a glowing splinter into the test tube.

. 4bserve and record the changes.

9. %epeat step 7 : 8 // he same procedure for test tube 6 without n4

Ta")#ation o! data

Test t)"e O"servation3// presence of manganese 7=>8

oxide// catalyst

6// with manganese 7=>8 oxide //

catalyst

23

Meta# reacts $ith acid to !orm sa#t and hdrogen gas%


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%eferring to the situation above, plan a laboratory experiment to investigate the effect of

concentrationor cata#ston the rate of reaction between a named acidand a named meta#%

%

7i8 Pro"#em statement!How does concentration o! acidaffect the rate of reaction?

(aria"#es'

Mani&)#ated varia"#e ! &oncentration of acid 7H&l8

Res&onding varia"#e ! %ate of reaction

Constant varia"#e ' >olume of acid //mass of metal

*&othesis'

5he higher the concentration of acid 7*C#8 , the higher the rate of reaction.

Materia#s

Dinc, 7hydrochloric acid8 E


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7ii8 Pro"#em statement'

"oes the presence of cata#st9copper7==8 sulphate, increase the rate of reaction?

(aria"#e'

Mani&)#ated varia"#e ! &atalyst // copper7==8 sulphate

Res&onding varia"#e ! %ate of reaction

Constant varia"#e ' (o#)me and concentrationof acid // mass of metal

*&othesis'

5he presence of catalyst, copper7==8 sulphate , increase the rate of reaction.

Materia#s

Dinc powder, copper7==8sulphate solution, water, acid E


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TOPIC' REDO

:. 5he rusting of iron can be affected by the present of other metal that is in contact with iron.

lan a laboratory experiment to investigate the e!!ect o! meta# on the r)sting o! iron%

7a8 3im!

5o investigate the effect of different types of metals in contactwith iron on the rusting.


How does different type of metals in contact with iron affect rusting?

7b8 (aria"#e

anipulated ! metals 7agnesium and &opper8

%esponding ! the rusting of iron

+ixed ! iron nail, ;elly solution mix with potassium hexacyanoferrate7===8 and

henolphthalein.

7c8 *&othesis!

)hen a more electropositive metal is in contact with iron, the metal inhibits rusting.

)hen a less electropositive metal is in contact with iron, the metal speeds up rusting.

7d8 Materia#s'

=ron nail, magnesium, copper strips, ;elly solution mix with potassium hexacyanoferrate7===8

and phenolphthalein, sandpaper.

A&&arat)s'

test tube, test tube rac#.

7e8 Proced)re'

1. C#ean iron nail, magnesium and copper strip with sand paper.

. Coi# two iron nails tightly with magnesium and copper strip.

-% P#acethe iron nails into separate test tubes.

. Po)rthe hot ;elly solution mix with potassium hexacyanoferrate7===8 and phenolphthalein

into the test tubes.

0. ee&the test tubes in a test tube rac# and leave them aside for two days.

. Recordthe observation.

7f8 Ta")#ation o! data

air of metal 4bservation+e:g

+e:&u

26


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0. )ay to store metals in laboratory depends on their reactivity with oxygen. 5he reactivity of the

metals is compared by observing how fast or how vigorous they react. *enerally, the more vigorous

a metal burns in oxygen, the more reactive the metal is.

6ased on this idea, plan a laboratory experiment to investigate the reactivity of magnesium, copper,

(inc and lead with oxygen.

Aim'

5o investigate the reactivity of magnesium, copper, (inc and lead with oxygen

(aria"#e'

mani&)#ated' magnesium, copper, (inc and lead

res&onding! reactivity with oxygen

Fi+ed 'solid potassium manganate7>==8

*&othesis'

5he higher the position of metal in reactivity series, the higher the reactivity of metal with oxygen.

A&&arat)s'

6oiling tube, retort stand and clamp, 6unsen burner, spatula and forceps

Materia#'

agnesium, copper, (inc and lead powder, solid potassium manganate7>==8, asbestos paper, glass

wool.

Proced)re'

1. ut one spatula of potassium manganate7>==8, n4, into a boiling tube.

. ush some glass wool into the boiling tube and clamp hori(ontally.

-. lace one spatula magnesium powder on a piece of asbestos paper and put into the boiling tube.

.Heat magnesium powderstrong# and then heat the solid n4.

0. 4bserve and record how vigorous the reaction.

. %epeat step 1 to 0 using copper, lead and (inc powder.

Ta")#ation o! data'

etal >igour of reaction

agnesium

&opper

$eadDinc

TOPIC' T*ERMOC*EMISTR,27


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-% lan a laboratory experiment to com&arethe heat o! ne)tra#i>ationbetween a named strong

acid with sodium hydroxide solution and heat of neutrali(ation between named wea# acid with

sodium hydroxide solution.


"oes heat of neutrali(ation between hydrochloric acid and sodium hydroxide solution ishigher than heat of neutrali(ation between ethanoic acid with sodium hydroxide solution?

7b8 (aria"#e

anipulated ! type of acids

%esponding ! heat of neutrali(ation

+ixed ! volume and concentration of acid / volume and concentration of al#ali

7c8 *&othesis '

%eaction between hydrochloric acid and sodium hydroxide solution has

higher heat of neutrali(ation than reaction between ethanoic acid with sodium

hydroxide solution.

7d8 Materia#s / S)"stances'

Hydrochloric acid,


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;. "ifferent type of alcohols produces different heat of combustions. )hen the number of

carbon per molecule of alcohol increases the heat of combustion increases. 5able shows the heat

of combustion of ethanol, propanol and butanol.

3lcohol olecular formula Heat of combustion/ #L mol:1

@thanol &H04H :1-9

ropanol &-H94H :olume of water // type of container/ si(e of container

7c8 *&othesis')hen the number of carbon per molecule of alcohol increases, the heat of

combustion increases.

7d8Materia#s

ethanol, @thanol, propanol, butanol, water,.

3pparatus

copper can, spirit lamp, thermometer, weighing balance, wooden bloc#, tripod stand,

wind shield, measuring cylinder

7e8 Proced)re'

1. E


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31/32


7d8 Materia#'

Hard water, cleaning agent 3 and 6

3pparatus!

, bea#ers, pieces of cloths stained with oil, galss rod

7e8 Proced)re'

1. E0< :


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