test 1 2011 kimia march

8/13/2019 Test 1 2011 Kimia March

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TEST 1FEB 2011

CHEMISTRY FORM 5(1 HOUR)

NAME: ................................................CLASS:.........................

SECTION A : Each question is followed by four option A, B, C and D. Choose the best optionfor each question.

BAHAGIAN A : Setiap soalan diikuti dengan empat pilihan awapan A, B, C and D. !ilihawapan yang terbaik bagi

setiap soalan.

". #he following are units of the rate of reactione$ceptA g s%"B g min%"C mol s%"

D mol dm%"

&. #he graph below shows the 'olume of gasproduced plotted against time.

Based on the graph, find the a'erage rate of reactionfor the first two minutes.A "(.( cm)min%"

B &(.( cm)min%"

C )(.( cm)min%"D *(.( cm)min%"

). +hich of the following cannotbe used to

determine the rate of reaction- olume of gas released per unit time-- Change of colour intensity per unit time--- /ass of precipitate produced per unit time- -ncrease in the mass of reactant per unit

timeA --- onlyB - onlyC - and -- onlyD --- and - only

Volume of gas (cm3)

60

40

20

Time (minute)1 2 3

50

30

10


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*. #he graph below shows the 'olume of carbondio$ide gas liberated plotted against time for thereaction between marble and !c""hydrochloric acid.

#he 'olume of carbon dio$ide remains constantafter * minutes becauseA the mass of catalyst decreasesB all the marble has been used upC all the hydrochloric has been used upD the rate of reaction remained

constant

0. +hich of the following #"tdescribe theproperties of catalyst- A catalyst increases the rate of collision-- A catalyst increases a quantity of product--- A positi'e catalyst is used to accelerate

reactions- 1nly a small amount of catalyst is

needed to cataly2e a reactionsA - and -- onlyB - and --- onlyC -- and - onlyD --- and - only

3. +hen the temperature decreases, thenumber of effecti'e collisions also decreasesbecauseA the acti'ation energy increasesB the a'erage kinetic energy decreasesC the number of atoms increases when the

bonds are brokenD the particles collide more often increasesthe acti'ation energy

4. 5inc powder reacts faster with hydrochloricacid than a 2inc strip becauseA there is a layer of 2inc o$ide on the

2inc stripB the 2inc powder has a larger total

surface areaC the particles of 2inc powder ha'e

more kinetic energyD the particles in the 2inc strip packed

more closely together

6. #he diagram shows an energy profilediagram.

Based on the abo'e energy profile diagram, theamount of acti'ation energy is..A 78 9 :; k< mol%"

B : k< mol%"

C 7: 9 8; k< mol%"$ 8 k< mol%"

=. 0 g magnesium carbonate is placed in a

conical flask on an electronic balance and &0cm)dilute hydrochloric acid is added. #hechange in mass is recoded at )( s inter'als. #heresults of the e$periment are shown in thediagram below.

At what time was the rate of reaction thehighestA "( minB &( min

C )( min$ *( min

"(. -n an e$periment, 2inc metal is mi$ed with 0(cm)of acid. +hich of the following mi$ture willyield gas with the lowest initial rate of reactionA 3 g of granulated 2inc with

(.* mol dm%)ethanoic acid.B 3 g 2inc powder with (.* mol dm%)

hydrochloric acid.C "& g granulated 2inc with (.& mol dm%)

sulphuric acid.

$ "& g of 2inc powder with (.& mol dm%)

hydrochlporic acid.

"". Cur'e > in the following graph shows thedecomposition of )( cm)of (.0( moldm%)of hydrogen pero$ide by using (.& g of

Volume of carbon

dioxide gas (cm3)

2 4 6 Time (s)

Energy

eactants

! "# mol$1

% "# mol$1

&roducts

'las" contents

30

20

10

0

40

10 20 30 40

Time (s)


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manganese7-; o$ide as catalyst at atemperature of )( oC.

+hich of the following e$periments will producecur'e S

Volume ofH2O2/ cm3 Concentration ofH2O2/ mol dm

-3

A )( (.3(

B "0 (.3(

C )( (.*(

$ *( (.*(

"&. +hich of the following statements about thecharacteristic of a catalyst are t%&I >eacts specifically for a certain

reaction only.II ?ormally used in small quantity.III At the end of reaction catalyst may

change their physical character.I' #he catalyst use only to speed the

rate of reactionA -- and - onlyB -, -- and - onlyC -, -- and --- only$ -, --, --- and -

"). #he best definition for a catalyst is achemical compound that can change the rate ofchemical reaction andA is used widely in industrial fields.B does not change chemically at the end

of a reaction.C does not take part directly in a reaction.$ is a comple$ molecule that is produced

by plants.

"*. +hich of the following statements gi'es the#"t e$planation for the statement gi'en abo'eA @inetic energy of molecules decreases.B Bonds are easier to break.C Acti'ation energy is lowered.$ Chances to ha'e effecti'e collisions are

increased.

"0. #he diagram shows an energy le'el for

the reaction ! S. +hat is the acti'ationenergy for this reactionA ")( k< mol%"

B )0( k< mol%"

C *6( k< mol%"

$ 6)( k< mol%"

"3. #he equation abo'e represents the aberprocess. #he rate of reaction increases ifpressure increases becauseA the kinetic energy of nitrogen gas

molecules and hydrogen gas moleculesincreases.

B the acti'ation energy is lowered under

high pressure.C the co'alent bonds in molecules ?&and

&are easily broken under highpressure.

$ the concentration of nitrogen gas andhydrogen gas increases under highpressure.

"4. +hich of the following will change Eato Ea

A ?egati'e catalyst

B !ositi'e catalyst

C !ressure

$ !romoter

Volume of oxygen (cm3)

Time (min)

Reducing the size of reactants will

increase the rate of reaction

Energy

& *

4+0 "#350 "#

N2 (g) + 3H

2(g) 2NH

3(g)

Energy

& *

Ea

Ea,


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"6. ood is stored in a refrigerator last longerthan food stored in a kitchen cabinet becauseF.A the food particles ha'e less kinetic

energyB the dehydration of food decreases the

temperature of foodC the concentration of food decreases

the surface areas of food$ the lower temperature decreases the

rate of the reaction of bacteria onfood.

"=. +hich of the following statements is nottrue about the collision theoryA All the collisions of the particles will

produce a reaction.B #he reaction will only occur when the

particles possess energy equal ormore than Ea.

C A greater surface area will producemore effecti'e collisions among theparticles.

$ #he rate of collision increases with atemperature rise.

&(. & g magnesium ribbon is dissol'ed in ane$cess of (." mol dm%)of hydrochloric acid toproduce magnesium chloride and hydrogen.+hich of the following factors will produce agreater 'olume of hydrogen gasA Gse ) g magnesium ribbon.

B Gse concentrated hydrochloric acid

C +arm the solution of the mi$ture.

$ Gse & g of magnesium powder.

An"% Fo% Scton A

Question

Answer Question Answer

1 11

2 12

3 13

4 14


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5 15

6 16

7 17

1

! 1!

1" 2"

Scton B#nstruction$ Answer all t%e &uestions in s'ace 'ro(ided)

". An e$periment was conducted to study the effect of temperature on the rate of reaction between 0( cm)

of sodium thiosulphate solution (.& mol dm%)and 0 cm) of sulphuric acid ".( mol dm%)to form a yellowprecipitate. Diagram " shows the set%up of apparatus for the e$periment.

#he e$periment was repeated fi'etimes using different temperatures.#able " shows the temperatureand time taken for mark H: todisappear from 'iew.

E$periment #emperatureIoC #imeIs

" &6.( 00

& *(.( ))) 0(.( &)

* 3(.( "4

0 4(.( ")

7a; Draw a graph oftemperature against time forthis e$periment. J* marksK

7b; rom the graph, calculate the rate of reaction in

7i; E$periment &

J& marksK

7ii; E$periment *

0( cm)of sodium thiosulphatesolution (.& mol dm%) 0 cm)ofsulphuric acid " mol dm%)


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J& marksK

7c; Compare the rate of reaction between E$periment & and E$periment *. E$plain your answer by using the Collision #heory. FFFF.

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J0 marksK

7d; +rite the chemical equation for the reaction.

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J" markK7e; ?ame the yellow precipitate formed.

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J" markK7f; State one other factor that can affect the rate of reaction for this e$periment.

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J" markK

2- T.o ex/eriments are carried out to study te effect of te sie of calcium carbonate on te rate of

reaction-

Ex/eriment 1 g of calcium carbonate ci/s react .it 20-0 cm3 of 0-2 mol dm$3 ydrocloric acid

Ex/eriment 1 g of calcium carbonate /o.der react .it 20-0 cm3 of 0-2 mol dm$3 ydrocloric

acidTe rate of reaction is determined by measuring te olume of of carbon dioxide gas gien off against time

using te do.n.ard dis/lacement of .ater metod- Te olume of gas released is recorded in Table 2-1

and Table 2-2 belo.-

Ex/eriment 1

Times 0 60 120 1+0 240 300 360

urette reading cm3 50-00 7-50 +-00 +-00

Volume of gas cm3 0-00

Table 2-1

Ex/eriment

Times 0 60 120 1+0 240 300 360

urette reading cm3 50-00 22-00 13-50 7-00 +-00 +-00 +-00

Volume of gas cm3 0-00

Table 2-2


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Diagram below shows the burette reading for E$periment - at 3(, "&( and "6( seconds.7a; >ecord the burette reading and the 'olume of gas released at 3(, "&( and "6( seconds in #able &.".

J) marksK7b; >ecordthe 'olumeof gasreleased in

bothe$perimentsin #able &."and #able&.&.

J3 marksK

7c; 7i; State the 'ariables in'ol'ed in this e$periment. /anipulated 'ariable

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J) marksK 7ii; State the hypothesis for these e$periments.

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J" markK7d; !redict the 'olume of gas released at *&( seconds in E$periment --.

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L11D MGC@ A?D #>8 81G> BES#

SECTION A 20

SECTION B 30

TOTAL MARKS 50

test 1 2011 kimia march

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