Chemistry Perfect Score Module 20121 BAHAGIAN PENGURUSAN SEKOLAH
BERASRAMA PENUH DAN SEKOLAH KECEMERLANGAN MODULPERFECT SCORE &
X A-PLUS SEKOLAH BERASRAMA PENUH TAHUN 2012 PANEL PENYEDIA DAN
PEMURNI: Pn. Wan Noor Afifah Binti Wan Yusoff (Ketua)SBPI GOMBAK Tn
Hj Ja'afar B BajuriSMS SULTAN MAHMUD Pn. Norini Binti JaafarSEKOLAH
SULTAN ALAM SHAH Tn HjChe Malik Bin MamatSBPI BATU RAKIT Pn.
Rossita Binti RadzakSMS TUANKU MUNAWIR Pn. Aishah Peong Binti
AbdullahSBPI TEMERLOH En Jong Kak YingSMS KUCHING En Ooi Yoong
SeangSMS MUAR Che Ramli B Che IsmailSMS FARIS PETRA Pn Masodiah Bt
MahfodzSMS HULU SELANGOR Pn. Noraini Binti ZakariaSMS SULTAN
MOHAMAD JIWA Chemistry Perfect Score Module 20122 CHEMISTRY PERFECT
SCORE MODULE 2012 CONTENT 1 Guidelines & Anwering Techniques
Format of an instrument of chemistry Construct requirement
Guidelines for answering paper 1 Guidelines for answering paper 2
Guidelines for answering paper 3 The common command words in paper
22Set 1 The structure of Atom Chemical Formulae and equations
Periodic Table of Elements Chemical Bonds 3Set 2 Electrochemistry
Oxidation and Reduction 4Set 3 Acids and Bases Salts Rate of
reaction Thermochemistry 5Set 4 Carbon compounds Manufactured
Substance in Industry Chemicals for Consumers 6Set 5 Paper 3 set 1
Paper 3 set 2 Paper 3 set 3 Chemistry Perfect Score Module 20123
CHEMISTRYPERFECT SCORE MODULE GUIDELINES & ANSWERING TECHNIQUES
CHEMISTRY SPM Chemistry Perfect Score Module 20124 GUIDELINES AND
ANSWERING TECHNIQUES FOR SPM CHEMISTRY PAPER 1.0 FORMAT OF AN
INSTRUMENT OF CHEMISTRY BEGINNING SPM 2003 NoItemPaper 1 (4541/1)
Paper 2 (4541/2) Paper 3 (4541/3) 1Type of instrumentObjective
testSubjective testWritten Practical Test 2 Type of itemObjective
itSection A :Structured Item Section B : Essay restricted response
Item Section C : Essay extended response Item Subjective Item :
Structured ItemExtended Response Item: (Planning an experiment) 3
Number of question 50 (answers all)Section A : 6 (answer all)
Section B : 2 (choose one) Section C : 2 (choose one) Structured
Item :1/2 items (answer all)Extended Response Item : 1 item 5
Duration of time1 hour 15 minutes 2 hour 30 minutes1 hour 30
minutes 2.0CONSTRUCT REQUIREMENT ConstructPaper1Paper 2Paper3
Knowledge20 m ( No 1- 20)14 - Understanding15 m ( No 21 35)21 -
Application15 m ( No 36 50)29 - Analysis-21 - Synthesizing-15 -
Science process--50Total mark5010050 3.0TIPS TO SCORE A CHEMISTRY
3.1Master the topics that contains the basic concepts of chemistry
: 1.The structure of the atom 2.Chemical Formulae And Equations
3.Periodic Table 4.Chemical Bond
3.2FamiliarizewithdifferenttypesofquestionsaslistedbelowandcompletethepreviousSPM
papers:1.Objectives questions (MCQ) (Paper 1)2.Structured questions
( Paper 2 & 3)3.Essays (Paper 2) 4.Planning an experiment (
Paper 3)5.Draw and label the diagram6.Writing chemical equation(
balanced equation, ionic equation, half equation)
3.3Try to get :- 40 marks above for paper 160 marks above for
paper 2 40 marks above for paper 3 (Total = 180/2=80 , A+ in SPM)
Chemistry Perfect Score Module 20125 4.0GUIDELINE FOR ANSWERING
PAPER 1 4.1Paper 1 questions test students on 1. Knowledge ( Number
1 20) 2.Understanding( Number 21 35) 3.Application( Number 36 50 )
4.2Score in paper 1 Indicates students level of understanding in
chemistry: Less than 20 very weak 20 25 - weak 26 30 - average31
39- good 40 45- very good 46 50- excellent. 4.3Answer all SPM
objective questions (2003 2010). Objective questions for each
yearcontain all topics. If your score in paper 1 is 40 and above,
you will able to answerquestions in paper 2 & 3 easily.
5.0GUIDELINE FOR ANSWERING PAPER 2 (STRUCTURE AND ESSAY)5.1Paper
2 questions test student on1.Knowledge
2.understanding3.analyzing4.synthesizing5.2Steps taken
are:1.Underline the command word and marks allocated for each
question. 2.Match the command word to the mark allocated for each
question. 1 point is awarded 1 mark. 3.Follow the needs of the
question (Refer to the command words, page .) 4.Unnecessary
repetition of the statement in the question is not required.
5.3Three types of questions which involve experiments in paper 2:
I.Type1 Describe an experiment onInclude a labeled diagram in your
answer
1.Diagram2.Procedure3.Observation/example/data/calculation/equation/sketch
of graph/conclusionII.Type2 Describe an experiment( The diagram
will support your answer.) 1.Nomark is allocatedfor a
diagram2.Procedures3.Observation/example/calculation/equation/sketch
of graph/conclusionIII.Type 3 Describe a chemical/confirmatory test
for . 1.Procedure 2.Observation 3.Conclusion 6.0GUIDELINE FOR
ANSWERING PAPER 36.1Structure Question 1/2 test the mastery of 11
Scientific Skills 1.Observing2.Classifying 3.Inferring 4.Measuring
(burette , stopwatch, thermometer, voltmeter) 5.Predicting
6.Communicating( e.gconstruct table and draw graph) 7.Space-Time
Relationship 8.Interpreting Data Chemistry Perfect Score Module
20126 9.Defining Operationally 10.Controlling Variables
11.Hypothesizing Each answer is allocated mark as follows: 3
marks/2 marks/1 mark/0 Score : 11 X 3 = 33 Example of operational
definition: 1. what you do 2. what you observe correctly Example:
1. When acid is added into latex, white solid is formed. When acid
is added into latex, latex coagulated.- wrong2. When the higher the
concentration sodium thiosulphate solution is added into sulphuric
acid, time taken for `X~ mark to disappear from sight is shorter.
3. When iron nail is coiled with copper and immersed into jelly
mixed with potassium hexacyanoferrate(III) and phenolphthalein
solution, blue spot/colouration isformed. Operational definition
forWhat you doWhat is observed 1.Rusting of ironWhen an iron nail
coiled with a less electropositive metal is immersed in hot
agar-agar added with potassium hexacyanoferrate (III) solution,
Blue spots are formed 2.Coagulation of latexWhen acid is added to
latexWhite solid is formed 3.Reactivity of Group 1 elements When a
metal which is lower in Group 1 is put in a basin half filled with
water Brighter flame is formed 4.Precipitation of silver chloride
When silver nitrate solution is added to sodium chloride solution
White solid is formed 5.Voltaic cellWhen two different metals are
dipped into an electrolyte The needle of the voltmeter deflects
6.An acidWhena blue litmus paper is dipped into a substancewhich is
dissolved in water, Blue litmus paper turns red Hypothesis: Relate
manipulated variable followed by responding variable with
direction. Example:1.The higher temperature of the reactant the
higher the rate of reaction 3 marks The temperature of the reactant
affect the rate of reaction 2 marks 2. Hexene decolourised brown
bromine water but hexane does not decolourised brown bromine water.
3. When acid is added into latex, latex coagulates, when ammonia is
added into latex, latex cannot coagulates 4.Question 3 (essay) Test
The Mastery of Planning Experiment. Planning should include the
following aspects: 1.Aim of the experiment/Statement of the problem
2.All the variables3.Statement of the hypothesis 4.List of
substances/material and apparatus should be separated 5.Procedure
of the experiment 6.Tabulation of dataScore : (5 X 3) + 2 = 17
The question normally starts with certain situation related to
daily life.Problem statement/ aim of the experiment / hypothesis
and variable can be concluded from thesituation given. State all
the variables Manipulated variable :Responding variable : Constant
variable: list down all the fixed variables to ensure the outcome
of the respondingvariable is related only to the manipulated
variables. Chemistry Perfect Score Module 20127 Separatethe
substances and apparatus -Separatethe substances and
apparatus-Apparatus : list down the apparatus for the experiment.
Example:Rate of reaction stop watch Termochemistry - thermometer
Procedure : All the steps taken in the procedure must include the
apparatus used, quantity and type ofsubstance (powder, solution,
lumps etc). No mark is allocated for the diagram. The complete
labeled diagram can help students in :I.Writingthe steps taken in
the procedureII.Listing the apparatus and materials Tabulation of
data: The number of columns and rows in the table is related to the
manipulated and responding variables Units must be written for all
the titles in each row and column of the table DO NOT WRITE the
observation/inference/conclusion in the table. 7.0THE COMMON
COMMAND WORDS IN PAPER 2 & PAPER 3 CHEMISTRYThe question
normally starts with a commandword. Students must know the meaning
of the command word to make sure that the answer given is according
to the questions requirement. Match the command word to the mark
allocated for each question.CommandwordExplanation/example
Name/State the name (paper 2 & 3) Give the name , not the
formula. Example: Name the main element added to copper to form
bronze. Wrong answer:Sn. Correctanswer :TinState (paper 2 & 3)
Give brief answer only. Explanation is not required. Example :State
one substance which can conduct electricity in solid state. Answer
:Copper State the observation (Paper 2 & 3) Write what is
observed physically. Example 1 :State one observation when
magnesium powder is added to hydrochloricacid.[ 1 mark] Wrong
answer:Hydrogen gasis released. Correct answer :Gas bubbles are
released Indicate the change of colour , give the initial and final
colour of the substance/chemical. Example 2:What is the colour
change of copper(II) suphatesolution.[2 marks] Wrong answer:The
solution becomes colourless Correct answer :The blue colour of the
solution becomes colourless Explain (Paper 2 & 3) Give the
answer with reasons to explain certain statement / fact /
observation/ principal. Example 1 : Explain why bronze is harder
than pure copper[4 marks]Correct answer :-Copper atoms in pure
copper are allof the same size and ...........1 - they are arranged
in layers that can slide easily when force is
applied...........1-The presence of tin atoms in bronze that are
different in size disturb theorderly arrangement of atoms in
bronze............1 -This reduces the layer of atoms from sliding.
...........1
What is meant by.. (Definition) (Paper 2 & 3) Give the exact
meaning Example:What is meant by hydrocarbon. Wrong answer: A
compound that contains carbon and hydrogen Correct answer:A
compound that contains carbon hydrogen only Describe chemical test
(Paper 2 & 3) Statethe method to conduct the test , observation
and conclusion. Example:Describe how to identifythe ion present in
the solution . [3 marks] Answer :- Pour in 2 cm3 of the solution in
a test tube. Add a few drops of sodium hydroxide solution and the
test tube is shake the test tube...........1 Chemistry Perfect
Score Module 20128 - A reddish brown precipitate formed.
...........1 - Fe3+ ions present 1Describe gas test.(Paper 2 &
3) State the method to conduct the test observation and conclusion.
Example: Describe the confirmatory test for gas released at the
anode (oxygen). [3 marks] Wrong answer:Test with a glowing wooden
splinter. Correct answer:-Place a glowing wooden splinter to the
mouth of the test tube ...1 -The glowing wooden splinter is lighted
up ...1 - Oxygen gas is released ...1 Describe an experiment (8 -
10 marks) (Paper 2)
-Nomarkisawardedforthediagram.Thediagramcanhelpstudentswritethesteps
taken in the procedure.-List of materials1m -List of apparatus
1m-Procedure( 5 8 m) -Observation/tabulation of data/
calculation/sketch of the graph/ chemical equation /ionic equation
/conclusion etc.-Any additional details relevant derived from the
question. Planan experiment( 17 marks) ( Paper 3)Answer the
question according the requirement : Problem statement/Aim of
experimentHyphotesisVariables List of substances and apparatus
Procedure Tabulation of dataNote: For question 3, unlike PEKA
reportstudents only needto answer according to what is stated inthe
question.
-Nomarkforthediagram.Diagramcanhelpstudentwritingthestepstakeninthe
procedure. Describe the process Describe the structure . Describe
and writeequation Describe how (Paper 2 & 3)
Give relevant details derived from the question. Predict (Paper
2 & 3) Make a prediction for something that mighthappen based
on facts Example:Experiment 1 is repeated using a larger beaker.
Predict the increase in temperatureAnswer : The increase in
temperature is lower than experiment 1. Compare (Paper 2) Give the
similarities and differences between two items/ situations
Differentiate(Paper 2) Give differences between two
items/situations Example : State three differences between ionic
and covalent compound. Answer : State three properties of ionic
compound and three properties covalent compound Draw a labeled
diagram of the apparatus(Paper 2) Drawa complete set up of
apparatus (i)Functional set up of apparatus(ii)Complete label
(iii)Shade solid, liquid and gas correctly. (iv)Draw an arrow and
label heat if the experiment involvesheating Drawa diagramto
showthe bonding formed in the compound(Paper 2) (i)Ionic compound
The number of electrons in each shell is correct, 2 electrons in
the first shell and 8 electrons in the second and third shell. Show
the charge of each particle. Write the symbol of each element at
the centre of the ion. (ii)Covalent compound The number of
electrons in each shell is correct, 2 electrons in the first shell
and 8 electrons in the second and third shell. The number of atoms
sharing pair of electrons is correct. Can be obtained from the
diagram Chemistry Perfect Score Module 20129 Write the symbol of
each element at the center of each atom in the molecule. Draw graph
(Paper 3) Draw graph as follows : Label the two axis with the
correct unit Choose suitable scale, the size of the graph should be
at least of the size of the graph paper. Plot all the points
correctly Smooth graph ( curve or straight line ) Forthe
determination of the rate of reaction (i)Draw a tangent at the
curve. (ii)Draw a triangle at the tangent Calculate the gradient of
the tangent Draw the energy level diagram ( Paper 2) Draw an arrow
for the vertical axis only and label with energy. Draw two
horizontal lines for the reactants and products Draw the
arrangement of particles in solid, liquid and gas. (Paper 2) Solid:
Draw at least three layers of particles closely packed in orderly
manner and they are not overlap. Liquid : The particles packed
closely but not in orderly manner Gas: The particles are very far
apart from each otherDraw the direction of electron flow (Paper 2
/3) Draw the direction for the flow of electrons on the circuit,
not through the solution. Write chemical equation (Paper 2 & 3)
Write the balanced chemical equation Differentiate : (i)Balanced
chemical equation (ii)Ionic equation (iii)Half equation for
oxidation (iv)Half equation for reduction Calculate (Paper 2 &
3) Show all the steps takenGive final answer with unit. Classify
(Paper 3) Draw table to represent the classification. Chemistry
Perfect Score/X A-Plus Module 2012 10 CHEMISTRY MODULE SET 1.The
Structure of Atom 2.Chemical Formulae and Equations 3.Periodic
Table of Elements 4.Chemical Bonds Chemistry Perfect Score/X A-Plus
Module 2012 11 SECTION A 1.Table 1 shows the proton number and
nucleon number for atoms L, M and N. AtomProton numberNucleon
number L1632 M1735 N1737 Table 1 (a)(i) What is meant by proton
number ? [1 mark ] (ii) What is the number of neutrons in atom M ?
[1 mark ] (b)Which atoms are isotopes ? Explain your answer. [2
marks] (c)(i) Write the electron arrangement for atom L. [1 mark ]
(ii) State the position of atom L in the Periodic Table [1 mark ]
(iii)Explain your answer in c (ii) .. . [2 marks ](d)Write the
formula of ion formed from atom M [1 mark ] Chemistry Perfect
Score/X A-Plus Module 2012 12 2Diagram 2 shows part of the Periodic
Table of Elements.T, U, V, W, X, Y and Z do not represent the
actual symbol of the elements. 118 21314151617 VXWZ UY T
Diagram 2 (a)Write the electron arrangement ofU atom.
............................. [1 mark ] (b)(i)Which of the element
exist as a monoatomic gas ?
.......................................................................................................................
[1 mark ](ii)Explain your answer in (b)(i). ..
...............................................................................................................
[2 marks ] (c)V reacts with W to form a compound. (i)Write the
formula for the compound formed. [1 mark ] (ii) Draw the electron
arrangement for the compound formed in (c)(i).
[2 marks ] (d)(i) Choose an element that is a halogen. [1 mark ]
(ii) Which element forms an amphoteric oxide ? . [1 mark] (iii)
Choose the element which form a coloured ion orcompound . [1 mark ]
Chemistry Perfect Score/X A-Plus Module 2012 13 3 Table 3 shows the
element in Period 3 with their respective proton numbers.
ElementNaMgAlSiPSClAr Proton number1112131415161718 Table 3
(a)(i)Write the electron arrangement ofsulphur atom, [1 mark ]
(ii)In which group of the Periodic Table is Sulphur, S located
?
.....................................................................................................................................
[1 mark ] (b) (i) How does the atomic size change when going across
the Periodfrom left to right ?
...........................................................................................................................................
[1 mark ] (ii) Explain your answer in 2(b)(i)
...........................................................................................................................................
............................................................................................................................................
[2 marks ](c)Argon, Ar is chemically unreactive. Explain why ?
.............................................................................................................................................
............................................................................................................................................
[2 marks ] (d)Which of the element when reacts with oxygen produces
an amphoteric oxide ?
...........................................................................................................................
[1 mark ] (e) Write the chemical equation when sodium react with
water.
.........................................................................................................................................
[2 marks ]
4.Table 4 shows the electron arrangement of atoms ofelements
J,K,L,M and N. Element Electron arrangement of atom J1 K2.8.1
L2.8.6 M2.8.7 N2.8.8 Table 4 (a)State one element in Table 4 which
ismetal and non-metal? Metal
:.......................................................................................................
Non-
metal:........................................................................................................
[2 marks] Chemistry Perfect Score/X A-Plus Module 2012 14
(b)(i)State an element thatexist as a diatomic gas. Explain your
answer. ...... [1 mark ] (ii) Explain your answer in (b)(i) .... [3
marks] (c)(i)What is the Proton Number for atom M
......................................................................................................................................
[1 mark ] (ii) Which group is atom M located in the Periodic Table
? Explain your answer.
.....................................................................................................................................
....................................................................................................................................
[2 marks ] (d)Arrange atomsK, L and M in increasing atomic size
.......................................................................................................................................
[1 mark ](e)Write the formula forK ion.
......................................................................................................................................
[1 mark ] (f)Kand M react to form an ionic compound.State the
formula for this compound.
.....................................................................................................................................
[1 mark ] 5(a)Table 5 shows three substances and their respective
chemical formulae. Name of substanceChemical formula ChlorineCl2
MagnesiumMg Magnesium chlorideMgCl2 Table 5 Use information from
Table 1 to answer the following questions : (i)State one substance
which exists as an atom. ..[1 mark] (ii)Write the ionic formula for
the substance in (a) (i). .. [1 mark] (iii)Which substance has the
lowest melting point? .. [1 mark] Chemistry Perfect Score/X A-Plus
Module 2012 15 (iv)What is the state of matter of chlorine at room
temperature? .. [1 mark] (v)Magnesium chloride can conduct
electricity in aqueous solution. Give a reason. .. [1 mark]
(b)Graph 1 shows the temperature against time when molten of
acetamide, C2H5NO is cooled.
Graph 1 (i)State the type of compound of acetamide. ..........
[1mark] (ii)State the melting point of acetamide. . [1 mark]
(iii)Describe the movement of the particles of acetamide between A
and B during cooling. [1 mark] (iv)Draw the arrangement of
particles of acetamide at stage CD. [1 mark] Temperature / 0C
Time / s T1 T2 T3 A B C D Chemistry Perfect Score/X A-Plus
Module 2012 16 Heat 6(a)In a close container, contains 3.0 dm3 of
carbon dioxide gas at room temperature. (i)How many molecules are
there in3.0 dm3 of carbon dioxide gas, CO2 ? [Avogadros number =
6.02 x 1023 mol-1] [1 mole of gas occupies 24 dm3 atroom
temperature] Use: Number of mole =Number of particles 6.02 x 1023
mol-1 [2 marks] (ii)Calculate the mass of carbon dioxide gas in the
container[Relative molecularmass for CO2 = 44] Use: Number of mole
=mass molar mass [1 mark] (b)Diagram 6 shows the set-up of
apparatus for an experiment to determine the empirical formula of
magnesium oxide.. Diagram 6 Table 1 shows the results of this
experiment DescriptionMass (g) Mass of crucible + lid34.0 Mass of
crucible + lid + magnesium ribbon36.4 Mass of crucible + lid +
magnesium oxide38.0 Table 1 (b)(i)What is the meaning of emperical
formula . .. [1 mark] Magnesium ribbon Chemistry Perfect Score/X
A-Plus Module 2012 17 (ii)Base on table 1, calculate the mass of:
Magnesium : Oxygen : [2 marks] (iii)Calculate the ratio of mole of
magnesium atoms to oxygen atoms. [Relative atomic mass: O=16, Mg
=24] [1 mark] (iv)Determine the empirical formula of magnesium
oxide. [1 mark] (v)Why was the crucible lidopened once in a while
during the experiment? .... [1 mark] (v)State why the empirical
formula ofcopper oxide cannot be determine by using the same
technique. .... [1 mark] 7. (a) What is the meaning of molecular
formula? ... .. [1 mark] (b)Diagram 7.1 shows an incomplete
equation which is one of the steps involved in determining the
empirical formula. Complete this equation. Diagram 7.1 MassRelative
atomic mass = Chemistry Perfect Score/X A-Plus Module 2012 18
(c)Diagram 7.2 shows the apparatus set-up for two methods used to
determine the empirical formula oftwo compounds. Method 1Method II
Diagram 7.2 (i)Which method is suitable to be used to determine the
empirical formula of magnesium oxide? . [1 mark] (ii)Why did you
choose the method in 2(c)(i)?
. [1 mark] (iii) When carrying out an experiment using Method I,
why does the crucible lid need to be opened once a while? [1 mark]
(d) Diagram 7.3 shows the results for an experiment to determine
the empirical formula of lead oxide. Diagram 7.3 Based on Diagram
2.3, determine the values of the following [Relative atomic mass of
O =16 , Pb = 207] (i)Mass of lead = g [1 mark] (ii) Number of moles
of lead. = mol [1 mark] (iii) Mass of oxygen
= ..g [1 mark] (iv)Number of moles of oxygen. = mol [1 mark]
(v)Empirical formula of oxide of lead. = [1 mark] Mass of
combustion tube + porcelain dish = 54.00 g Mass of combustion tube
+ porcelain dish +lead oxide = 107.52 g Mass of combustion tube +
porcelain dish + lead = 103.68 g Chemistry Perfect Score/X A-Plus
Module 2012 19 8. Diagram 8 shows the apparatus set-up to determine
the empirical formula of copper oxide. Diagram 8 Table 8 shows the
result of this experiment. DescriptionMass(g) Combustion tube +
porcelain dish42.25 Combustion tube + porcelain dish + copper
oxide52.25 Combustion tube + porcelain dish + copper 50.25 Table 8
(a) (i) What is the meaning of empirical formula? [1 mark] (ii)
State the function of the anhydrous calcium chloride. .. [1 mark]
(b) (i) Based on Table 8, determine the mass of: Copper: =..g
Oxygen: = ..g [2 marks] (ii) Calculate the ratio of moles of copper
atoms to oxygen atoms. [Relative atomic mass: O = 16 ; Cu = 64] [1
mark] Chemistry Perfect Score/X A-Plus Module 2012 20 (iii)
Determine the empirical formula of copper oxide. [1 mark] (c) (i)
Why is hydrogen gas passed through the combustion tube after
heating has stopped? . . [1 mark] (ii) State how to determine that
the reaction between copper oxide with hydrogen has completed. [1
mark] (d)(i) State why the empirical formula of magnesium oxide
cannot be determined by using the same technique. [1 mark] (ii)
State the name of another metal oxide whose empirical formula can
bedetermine using the same technique. .. [1 mark] SECTION B 9(a)
Diagram 9.1 shows the atomic structure of two carbonisotopes.
Diagram 9.1 (a)Compare the two isotopes above in terms of number of
proton, number of electron, nucleon number,physical properties and
chemical properties. [6 marks] Nucleus 6 neutrons Nucleus8 neutrons
Chemistry Perfect Score/X A-Plus Module 2012 21 (b)Diagram 9.2
shows the set up of apparatus used in experiment to determine the
melting points ofX. Diagram 9.2 (i)Suggest one example of substance
X. [1 mark] (ii) State the name of P. Explain why P is used? [2
marks] (iii)Graph 9 shows the heating curve of X. Graph 9 Describe
Graph 9 in terms of state of matter, particles arrangement, kinetic
energy ofparticles and attractionforces between particles. [10
marks] (iv) After t3 minutes, Xis cooled at room temperature.
Sketch a graphoftemperature against time for cooling process. .[2
marks] Temperature / 0C Suhu / 0C Time/ minutes Masa / minit
100
30 t1 t2 t3 80 0 Q X Heat P Chemistry Perfect Score/X A-Plus
Module 2012 22 10(a)Helium,He42exists as a monoatomic gas whereas
chlorine,Cl3517exists as a diatomic gas. Explain why. [6 marks]
(b)Table 10.1 shows the proton number of magnesium, chlorine and
carbon. Element Magnesium ChlorineCarbonProton number12176 Table
10.1 (i)Carbon reacts with chlorine to form a compound.What type of
the compound formed?Draw the electron arrangement to show the
chemical bond in the compound. [3 marks] (ii)Explain how ionic bond
is formed between magnesium and chlorine atoms. [7 marks]
(c)Diagram 10 shows the set-up of apparatus to investigate the
electrical conductivity of naphthalene and sodium chloride
solution. Diagram 10 Table 10.2 shows the result of the
experiments. Compound Observation Naphthalene Bulb does not light
upSodium chloride solution Bulb lights up Table 10.2 Explain the
electrical conductivity of the two compounds. [4 marks] Bulb Carbon
electrode Compound Chemistry Perfect Score/X A-Plus Module 2012 23
Empirical formula is CH2O. Relative molecular mass is 60. Reacts
with calcium carbonate to produce a type of gas that turns lime
water chalky. 11. (a) The following are the formulae of two
compounds. Al2O3PbO2 (i) Based on the two formulae, write the
formula forion aluminiumand ion lead[2 marks] (ii) Name both
compounds based on the IUPAC nomenclature system. [2marks]
(b) The following information is about an organic compound,
K.
Based on the information given: (i) Determine the molecular
formula of K. [Relative atomic mass : H = 1, C = 12, O = 16] [3
marks] (ii) Write a balanced chemical equation for the reaction of
compound K with calcium carbonate. [2 marks] (c) Diagram 11 shows
the apparatus set up for experiment of decomposition of copper(II)
carbonate. In this experiment copper(II) oxide and carbon dioxide
gas are formed.
Based on Diagram 11 (i) State two observations. [2 marks] (ii)
Write a balanced chemical equation for the reaction [2 marks] (iii)
) State two informations from the chemical equation in (c)(ii). [2
marks] Diagram 11 Copper(II) carbonate powder Lime water Heat
Chemistry Perfect Score/X A-Plus Module 2012 24 (v)Calculate the
mass of the copper(II) oxide formed from the decomposition of12.4 g
of copper(II) carbonate. [ Relative atomic mass of C = 12; O = 16;
Cu = 64] [3 marks] (vi)In other experiment 4.0 g copper(II) oxide
is reacted with hydrogen gas to produce copper and water. If the
mass of copper in copper(II) oxide is 3.2 g, calculate the mass of
oxygen and the simplest mole ratio for the copper atoms to oxygen
atoms [ Relative atomic mass of O = 16; Cu = 64] [2 marks] 12.
Table 12 shows the positive and negative ions in three salts
solution. Name of saltPositive ionNegative ion Iron(III)
chlorideFe3+Cl- Potassium sulphateK+ SO42- Lead(II) nitratePb2+NO3-
Table 12 Use the information in Table 12 to answer the following
questions. (a) (i) What areanother name for a positively charged
ion and negatively charged ion? [2 marks] (ii) Name the ions in
iron(III) chloride. [2 marks] (iii) Write the formula for potassium
sulphate. [1mark] (b) When 10 cm3 of 0.5 mol dm-3 potassium
sulphate solution is added to excess lead(II) nitrate solution, a
white precipitate is formed. (i) Name the white precipitate and
write the chemical equation for the reaction. [3 marks] (ii)
Describe the chemical equation in (b)(i). [1 mark] (iii) Calculate
the mass of precipitate formed. [Relative atomic mass of O = 16; S
= 32; Pb = 207] [4 marks] (c) The information below is regarding an
organic compound Z.
Relative molecular mass is 46 Carbon : 52.2%Hydrogen : 13.0%
Oxygen : 34.8% Relative atomic mass of H = 1; C = 12 and O = 16
Based on the information of the organic compound Z: (i) Determine
the molecular formula for compound Z and[6 marks] (ii) Draw its
structural formula. [1 mark] Chemistry Perfect Score/X A-Plus
Module 2012 25 SECTION C 13 (a) An experiment is carried out using
Group 1 elements;X, Y and Z reactwith oxygen gas.The set-up of
apparatus and observations of the reaction are shown in Table 13.
SetSet-up of apparatusObservation I Burns slowly andwhite fumes
formed II Burns vigorously and white fumes formed III Burns rapidly
and white fumes formed Table 13 (i)Based on the observation in
Table 13, compare the reactivity of element X and Y. Explain your
answer. [5 marks] (ii) Suggest the name of element Z. Using the
symbol of element suggested, write the chemical equation for the
reaction in set III. [3 marks] (b)State how elements of Group 1 are
stored in laboratory and give a reason. [2 marks] (c) Using an
example of Group 1 element, describe an experiment to prove above
statement.Your description shouldinclude the following : List of
material and apparatus Procedures of the experiment Observation
Chemical equation [10 marks] Group 1 elements react with water to
produce alkaline solution. Z X Y Chemistry Perfect Score/X A-Plus
Module 2012 26 14Table 14 shows the melting point, boiling point
and electrical conductivity of compoundPQ2 and compound XY.
Compound Melting point and Boiling point Electrical conductivity
SolidMolten PLow No NoQHigh NoYesTable 14 (a)Suggest one possible
compound for P. State the type of compound for P. Explain why P has
low melting and boiling points. [4 marks] (b)Chemical formula of
compound P is XY. Suggest one possible electron arrangement of atom
X and atom Y. State the type of chemical bond and explain how the
bond is formed between atom X and atom Y. [7 marks] (c)Plan one
laboratory experiment to investigate the electrical conductivityof
compound Q. Your answer should include the following : A list of
material and apparatus Procedure of the experiment Observation of
the experiment A labeled diagram showing the apparatus set-up [9
marks] 15 (a)Metal P has the following characteristics:- Based on
the information above, state the method used to determine the
empirical formula of oxide of metal P.Give a reason for your
answer. [2 marks] (b) Diagram 15 shows the set up of apparatus for
an experiment to determine the empirical formula of the oxideof
metal Y. Diagram 15 The results are obtained as follows:
Table 15 Grey in colour Can react with steam Reactive metal Dry
hydrogen Oxide of metal Y Combustion tube Mass of combustion tube +
Porcelain dish = 54.30 gMass of combustion tube + Porcelain dish
+Oxide of Metal Y =56.69 g Mass of combustion tube + Porcelain dish
+Metal Y=56.37 g Chemistry Perfect Score/X A-Plus Module 2012 27
(i)Based on the above information, determine the empirical formula
of oxide ofmetal Y Given that the relative atomic mass of O = 16, Y
= 207 [4 marks]
(ii) Describe the steps that should be taken to ensure that all
the air in the combustion tube has been expelled . [3 marks]
(b)Describe an experiment on how to determine the empirical formula
of magnesium oxide. In your description, state the precautions
should be taken during the experiment and show how the empirical
formula of magnesium oxide is obtained. [Relative atomic mass: O =
16; Mg = 24] [11 marks] 16. (a) The following is the chemical
formula of a compound. SO3 Name the compound and describe the
composition of this compound. [3 marks] (b) Excess calcium
carbonate chips is added to 30 cm3 of 0.5 mol dm-3 acid HX. The
chemical equation below shows the reaction between calcium
carbonate and acid HX. CaCO3+ nHXCaX2 +CO2+H2O Given that the
relative atomic mass of C = 12, O = 16 , Ca = 40 and the molar
volume of any gas is 24 dm3 mol-1 at room temperature and pressure.
(i) Suggest acid HX and name salt CaX2 Determine the value of n [3
marks] (ii) Calculate the maximum volume of carbon dioxide gas
produced. [4 marks] (c) You are provided with a sample of M oxide
powder. The colour of the M oxide powder is greenwhile the colour
of metal M is grey. When it is heated with hydrogen, the M oxide is
reduced to M metal. Based on the information given, describe an
experiment to determine the empirical formula of the M oxide. In
your description, include the precautions that should be taken and
show how the empirical formula of M oxide is obtained. [Relative
atomic mass of O = 16 and M = 56][10 marks] Chemistry Perfect
Score/X A-Plus Module 2012 28 CHEMISTRYMODULE SET
1.Electrochemistry 2.Oxidation and Reduction Chemistry Perfect
Score/X A-Plus Module 2012 29 SECTION A 1Diagram 1 shows the set-up
of apparatus ofa voltaic cell.
Diagram 1 Based on Diagram 1 , answer the following questions.
(a)What is theenergy change that occurs in the voltaic cell?
..................................................................................................................................
[1 mark] (b)Write the formula of all ions in copper(II) sulphate
solution.
..................................................................................................................................
[1 mark] (i)State the name ofthe negative terminal of the voltaic
cell.
...............................................................................................................................
[1 mark] (ii)Give a reason for your answer in (c)(i).
.....................................................................................................................
[1 mark] (d) (i)State one observation at copper plate.
.....................................................................................................................
[1 mark] (ii)Write the halfequation for the reaction occurat
thecopper plate.
.....................................................................................................................
[1 mark] (e)What is the colour change of the copper(II) sulphate
solution? Give a reason.
..................................................................................................................................
..................................................................................................................................
[2 marks] (f)Another experiment is carried out by replacing the
zinc plate with P , Q and R metals.Table 1 shows the results. .Pair
of metalVoltage/VNegative terminal P/Cu2.7PQ/Cu2.0Q R/Cu0.5R Table
1 Copper(II) nitrate solutionCopper plateZincplateV Chemistry
Perfect Score/X A-Plus Module 2012 30 (i)Arrange P, Q, R and Cu
metal in accending order of electropositivity.
..................................................................................................................................
[1 mark] (ii)Predict the voltage for pair of Q/R.
..................................................................................................................................
[1 mark] 2.Diagram 2 shows the set-up of apparatus to investigate
the reaction occurred in test tubesX and Y. (a)Based on test tube
X, (i)Name the reaction occurred. [1 mark] (ii)Write the ionic
equation for the reaction. [2 marks] (iii)Describe a chemical test
to verify the product formed.
........................................................................................................
..........................................................................................................
[2 marks] (b)Based on test tube Y,
(i)State the observation involved.
................................................................................................................
[1 mark] (ii)Experiment is repeated by using copper to replace
zinc.State the observation involved.
..................................................................................................................
[1 mark] (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] Test tube X Test tube Y Agar solution + Potassium
hexacyanoferrate(III) solution+Phenolphthalein Iron nail coiled
with zinc Diagram 2 Zinc Iron(III) sulphate solution Heat Chemistry
Perfect Score/X A-Plus Module 2012 31 SECTION B 3 Diagram 3.1 shows
the set-up of apparatus to investigate the electrolysis of
magnesium chloride 1.0mol dm-3 solution. Diagram 3.1 (a) (i)Based
on Diagram 3.1;State the name of the products at the cathode and
the anode.Explain the reaction at cathode and anode. Include the
following in your explanation: Listthe ions attracted to cathode
and anode. Statethe ions selectively discharged at cathode and
anode. The reason why the ions are selectively discharged. Half
equation for the reaction at cathode and anode. [10 marks]
(ii)Predict the product at anode and cathode if magnesium chloride
1.0 mol dm-3 solution is replaced by magnesium chloride 0.0001 mol
dm-3 solution. [2 marks] (b)Diagram 3.2 shows the set up of
apparatus when cell X is combined with cell Y. Compare and contrast
cell X and cell Yin terms of following: Types of cells
Energychanges Name of electrodes Ions in the electrolyte Half
equations Observations . [8 marks] Copper plate Copper(II) sulphate
solution Magnesium plate
Cell XCell Y Copper plate Diagram 3.2 V Magnesium chloride 1.0
mol dm-3 A Carbon electrodes Chemistry Perfect Score/X A-Plus
Module 2012 32 4 (a) The following are the formulae of two
compounds. Na2O PbO2 (i)Based on the two formulae , state the
oxidation number for sodium and lead. [ 2 marks] (ii)State the name
ofthe compoundsbased on the IUPAC nomenclature. [ 2 marks]
(b)Diagram 4 shows the observation of two experiment to study the
effect of metal P and metal Q on the rusting of iron.
ExperimentObservation Experiment 1 Large amount of dark blue
precipitate Experiment 2 No dark blue precipitate. Solution turns
pink. Diagram 4 (i)Suggest metal P and metal Q. (ii)Explain the
observationsand write the chemical equation for the reaction in the
experiment 1 and experiment 2. [ 10 marks] (c)The equation shows a
redoxreaction. M is a metal. X(s)+ CuSO4 (aq)XSO4 (aq) + Cu(s)
Suggest metal X and explain the redox reaction in terms of the
transfer of electrons .[6 marks] SECTION C 5 Diagram 5 shows the
set-up of apparatus for electrolysis of 1.0 mol dm-3 sodium
sulphate solution.
Diagram 5 (a)State the name of gas produced at electrode X and
electrode Y. [2 marks] Carbon electrode Y Carbon electrode X 1.0
moldm-3 sodium sulphate solution Chemistry Perfect Score/X A-Plus
Module 2012 33 (b)Explain the reaction at electrode X and electrode
Y. Include the following inyour explanation. List of ion attracted
to each electrodes, X and Y. State the name of the ions selectively
discharged at each electrode. The reason why the ion are
selectively discharged. [5 marks] (c)Whensodium sulphate solution
is replaced bya solution of substance Zwith same concentration, the
equal gas produced at electrode X and electrode Y . Suggest the
substance Z. Write the half equation for the reaction at electrode
X. [3 marks] (d)Zinc is placed above metal A in the electrochemical
series. Zinc and metal A can be used to build a chemical cell,
using suitable apparatus and the following chemicals ; Zinc Zinc
nitrate solution Metal A A nitrate solution By naming metal A and A
nitrate solution, describe how you build the chemical cell. Include
a labelled diagram in your answer. On your diagram, mark the
direction of electron flow, the positive terminal and the negative
terminal. [ 10 marks] 6 (a)The following are the equations of two
reactions: Determine which reaction is a redox reaction.Explain
your answer in terms of oxidation number. [4 marks] (b)Table 6
shows the observations of two experiments to determine the position
of carbon in the reactivity series of metal.
ExperimentReactantsObservation ICarbon + oxide of metal P A flame
spreads to the whole mixture.A brown residue is formed.IICarbon +
oxide of metal QNo change IIICarbon + oxide of metal R A glow
spreads to the whole mixture. A grey residue is formed. Based on
observations in Table 6, arrange the reactivity of metals P, Q, and
R in descending order. Explain your answer.[6 marks] (c) By using a
named metal as a reducing agent and a named halogen as an oxidising
agent, describe briefly how you would carry out these two
conversion. Describe a test to show that each conversion has taken
place. [ 10 marks] Reaction I:NaOH+HCl NaCl + H2O Reaction
II:Mg+Zn(NO3)2Mg(NO3)2 + Zn Table 6 Iron(II) ions can be converted
to iron(III) ions and iron(III) ions can be converted back to
iron(II) ions. Chemistry Perfect Score/X A-Plus Module 2012 34
CHEMISTRY MODULE SET 1.Acids and Bases 2.Salts 3.Rate of reaction
4.Thermochemistry Chemistry Perfect Score/X A-Plus Module 2012 35
SECTION A 1.Diagram 1 shows four test tubeslabeled A,B,C and D
which are used to study therelationship betweenpHvalue of acid and
alkali with themolarity. pH paper ABCD 5 cm3HCl 5 cm3HCl5 cm3 NaOH
5 cm3NaOH 0.1 mol dm-30.01 mol dm-3 0.1 mol dm-30.01 moldm-3
(a)Determine which solution has(i) highest pH value. ` ......... [1
mark] (ii)lowest pH value. Give a reason for your answer.
............. [2 marks] (b)If the hydrochloric acid in test tube B
is replaced with 5 cm3 of 0 .01 mol dm-3ethanoic acid, predict the
pH value of the solution. Explain your answer ..... . [3 marks]
(c)Excess of magnesium powder is added to 5 cm3 of 0.1moldm-3
hydrochloric acid in test tube A (i)State the name of the products
formed. . ..... [1 mark] (ii)Write the chemical equation for the
reaction in test tube A [1 mark] (iii) Calculate volume of hydrogen
gas released at room conditions in test tube A [1 mol ofgas
occupies 24 dm3 at room conditions] [3 marks] Diagram 1 Chemistry
Perfect Score/X A-Plus Module 2012 36 Add water (d)If the solution
in test tube C is added to lead(II) nitrate solution. State the
observation from the reaction. . [1 mark] 2.(a)Diagram 2.1 shows
the pH value of glacial ethanoic acid in solvent P and solvent Q
respectively. (i)SuggestsolventP and solvent Q. Solvent P: ....
Solvent Q: . [2 marks] (ii)If magnesium ribbon is added into beaker
containing glacial ethanoic acid and solventP, what can be
observed? . [1 mark] (iii)Explain why ethanoic acid in solvent Pand
solvent Q hasdifferent the pH value. . . . ... [3 marks] (b)Diagram
2.2 shows the concentration of hydrochloric acid in volumetric
flask when a certain volume of hydrochloric from the beaker is
transferredto the volumetric flask and added with water
7.0 4.8 Glacial ethanoic acid+ solvent P Glacial ethanoic acid
+solvent Q 100 cm3 of 0.5 moldm-3 hydrochloricacid Diagram 2.1
Diagram 2.2 250 cm3 of0.04 moldm-3 hydrochloricacid Chemistry
Perfect Score/X A-Plus Module 2012 37 (i)What happen to the pH
value of the hydrochloric acid when water is added to the acid?Give
areason for your answer. . . [2 marks] (ii)Calculate the volume of
hydrochloric acid that is needed to prepare 250cm3 of 0.04 mol dm-3
hydrochloric acid. [2 marks] 3.A student carried out an experiment
to investigate the properties of three solutions. Diagram 3 shows
the results of the experiments. Test tubePQR Set-up of apparatus
Observation The red litmus paper turned blue. No change Diagram 3
(a)What is meant by strong alkali?
.......................................................................................................................................
[1 mark] (b)What is the property of the solution in test tube P?
.......................................................................................................................................
[1 mark](c)What are the types of particles that exist in the test
tubes P and Q? Particles in the test tube P:
..........................................................................................
Particles in the test tube Q:
.........................................................................................
[2 marks] (d)Is there any changes of colour of the litmus paper in
test tube Q? Give a reason to your answer.
......................................................................................................................................
......................................................................................................................................
[2 marks] Ammoniagas dissolved in water Red litmusPaper Ammonia gas
dissolved in propanone Red litmusPaper Hydrogen chloride gas
dissolved in water Magnesium Chemistry Perfect Score/X A-Plus
Module 2012 38 (e)(i) What can beobserved in test tube R?
......................................................................................................................................
[1 mark] (ii) Write a chemical equation for the reaction in test
tube R.
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[2 marks] (iii) 2.4 g of magnesium is reacted completely with the
solution in test tube R.Calculate the volume of the hydrogen gas
produced at room condition [Relative atomic mass: Mg,24; 1 mol of
gas occupies 24 dm3 at room conditions] [2 marks]
4Diagram4showstheapparatusset-upfortheneutralisationreactionbetweensulphuricacidandpotassium
hydroxide solution for preparation of salt X. Diagram 4 (a)(i)State
the colour change of the solution in the conical flask at the end
point. . [1 mark] (ii)Write a chemical equation for the above
reaction. . [2 marks] (iii)Calculate the concentration of potassium
hydroxide used. [2 marks] (b)(i) State the name of salt X. .. 25.0
cm3potassium hydroxide solution + phenolphthalein indicator 15
cm3of0.1mol dm-3 sulphuric acid Chemistry Perfect Score/X A-Plus
Module 2012 39 [1 marks] (ii) Calculate the maximum mass of salt X
formed. [Molar mass of salt X = 174 g mol-1] [3 marks] (c)(i) The
experiment is repeated with 0.1 mol dm-3 nitric acid to replace
sulphuric acid. Predict the volume of nitric acid neededto
neutralize completely potassium hydroxide .. [1 mark] (iii)Explain
your answer in (c) (i).
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......................................................................................................................................................
[2marks] 5.Diagram5 shows a series reaction ofcopper compound.
(a)Copper(II) nitrate solution reacts with sodium carbonate
solution to form copper(II) carbonate precipitate.(i)What is the
colour ofcopper(II) carbonate? ............. [1 mark] (ii)State the
name of the reaction.
.........................................................................................................................................................
[1 mark] (b) Heating of copper(II) carbonate producescopper(II)
oxide and gas X. (i)State the name of gas X. .. [1 mark] (ii)Write
the chemical equation of the reaction.
...................................................................
[2 mark] Copper(II) carbonate Copper(II) oxide Sodium carbonate
Copper(II) nitrate Copper(II) sulphate Diagram 5 Acid Y HeatGas X +
Chemistry Perfect Score/X A-Plus Module 2012 40 (iv)Draw a labeled
diagram for the heating ofcopper(II) carbonate to producecopper(II)
oxideand gas X. In your diagram show how gas X is tested. [2 marks]
(c)Copper(II) carbonate reacts withacid Y to produce copper(II)
sulphate. The chemical equation is shownbelow. CuCO3+Acid Y
CuSO4+CO2 + H2O (i)What is acid Y? [1 mark] (ii)12.4 gcopper(II)
carbonate reacts completely with excess acid Y. Calculate the mass
ofcopper(II) sulphate formed. [Relative atomic mass:C = 12,O=16 , S
= 32, Cu = 64] [3 marks] 6.Three experiments were conducted to
investigate factors affecting the rate of reaction. The results are
shown in the Table 6 ExperimentReactantsTemperature / 0C Time taken
for all the magnesium to dissolve/s I 0.4g magnesium ribbon and 50
cm3 1 moldm-3 hydrochloric acid 30100 II 0.4g magnesium powder and
50 cm3 1 moldm-3 hydrochloric acid 3060 III 0.4g magnesium ribbon
and 50 cm3 1 moldm-3 hydrochloric acid and copper(II) sulphate
solution 3045 Table 6 (a)Write a chemical equation to show the
reaction between magnesium and hydrochloric acid. [2
marks](b)Calculate the number of mole of (i)Magnesium [Relative
atomic mass of Mg = 24] [1 mark] (ii)Hydrochloric acid [1 mark]
Chemistry Perfect Score/X A-Plus Module 2012 41 (c)Ifhydrochloric
acid used is excess, calculate the maximum volume of hydrogen gas
produce at room temperature and pressure.[1 mole of gas occupies
the volume of 24 dm3 at room temperature and pressure] [2 marks]
(d)Calculate the average rate of reaction for(i)Experiment I [1
mark] (ii)Experiment II. [1 mark] (iii)What is the purpose of using
copper(II) sulphate? . [1 mark] (f) The factor that affects the
rate of reaction in this experiment is total surface area and the
use of catalyst. State two other factors that affect the rate
reaction in this experiment. .. [2 marks] 7.Diagram7shows two
experiments to investigate one of the factors that affect the rate
of reaction between zinc and hydrochloric acid Diagram 7 (a)(i)
Based on Diagram 7, state the factor that affect the rate of
reaction in this experiment. . [1 mark] 50 cm3 1 mol dm-3HCl
Hydrogen gas Excess zincgranules Experiment I 50 cm3 1 mol dm-3HCl
+ copper(II) sulphate solution Hydrogen gas Excess zincgranules
Experiment II Chemistry Perfect Score/X A-Plus Module 2012 42 (ii)
Besides measuring the change of volume of gas released at certain
time interval, suggest another measurable change to determine the
rate of reaction? .. [1 mark] (b)In Experiment II, 2.0 cm3 0.5
moldm-3copper(II) sulphate solution is added. The maximum volume of
hydrogen gas releasedin Experiment I is V cm3.(i)Compare the volume
of gas released in Experiment I andExperiment II.Give a reason for
your answer. .. . [2 marks] (ii)The graph of volume of hydrogen gas
released against time in Experiment I is shown below. Sketch the
curve for Experiment II on the same axes in the graph above. [2
marks] (iii)With reference to collision theory, explain how
copper(II) sulphate solution affect the rate of reaction in this
experiment. [3 marks] (c)Table 7.1 shows three experiments done by
a student. ExperimentReactants A Excess calcium carbonate chips +
25 cm3 1.0 mol dm-3 hydrochloric acid B Excess calcium carbonate
chips + 25 cm3 0.5 mol dm-3 hydrochloric acid C Excess calcium
carbonate chips + 100 cm3 0.5 mol dm-3 hydrochloric acid Table 7.1
Time / s Volume of gas released/ cm3 Key : Experiment I :
Experiment II : .. Chemistry Perfect Score/X A-Plus Module 2012 43
The graph of volume of carbon dioxide released against time is
sketched as shown in graph 7 Based on theabove table andgraph,
determine which curve represents the resultsfor experiment B and C.
Write your answers in the boxes provided. [1 mark] 8. An experiment
is conducted to study the heat of displacement for reaction between
copper(II) sulphate and excess magnesium 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 magnesium
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;
(a)What is the meaning of heat of displacement in this experiment?
............................................................................................................................
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[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.
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[2 marks] (d)(i)Based on the experiment, calculate the heat
energyreleased. [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. [3 marks] Time/s Volume of carbon dioxide /cm3 Experiment
A Graph 7 Chemistry Perfect Score/X A-Plus Module 2012 44 5 g of
zinc powder 50 cm3 of 0.2 mol dm-3 copper(II) sulphate solution
Plastic cup (f)Why polystyrene cup is used in this experiment? [1
mark]
9.Diagram9showstheapparatusset-uptodetermineheatofdisplacementofcopperbyusingzinc
powder. The result of the experiment is recorded in the Table 9.
Diagram 9 Initial temperature of copper(II) sulphate solution (oC)
30.0 Highest temperature of the mixture (oC) 38.0 Table 9 (a)What
is the meaning of heat of displacement? [1 mark] (b) (c) Why
plastic cupis used in this experiment. [1 mark] State the type of
reaction that occurs based on the temperature change. [1 mark]
(d)Calculate :(i)the heat change for the reaction [Specific heat
capacity of solution = 4.2 J g-1 oC-1; Density of solution = 1 g
cm-3] [1 mark] (ii)the heat of displacement for the reaction. [2
marks] (e)Draw energy level diagram for the reaction. [3 marks]
Chemistry Perfect Score/X A-Plus Module 2012 45 (f)Experiment is
repeated by using 100 cm3 of 0.2 mol dm-3 of copper(II) sulphate
solution. (i)Predict the temperature change in the experiment. .
... [1 mark] (ii)Explain your answer in (e) (i). ... ... ... [2
marks] 10. Theequation for combustion of propanol in excess oxygen
is given below.
(a)What is meant by heat ofcombustion in this reaction?
.......................................... [1 mark] (b)Statetwo
information that can be obtained from the equation
........................................... [2 mark] (c)Heat given
out from the complete combustion of 1.2 g propanol is used to heat
200 cm3 of water. Calculate: (i)The heat energy given out in the
reaction. [Molar mass of propanol, C3H7OH = 60 gmol-1] [2 marks]
(ii) The temperature change in the reaction. [Spesific heat
capacity of water=4.2 Jg-1oC-1; Density of water = 1 gcm-3] [2
marks] (d)Draw the energy level diagram for this reaction. [3
marks] C3H7OH +9 O2 3CO2+ 4H2O , H =-2015 kJ mol-1 2 2 Chemistry
Perfect Score/X A-Plus Module 2012 46 (e)The value of the heat of
combustion of propanol obtained from the experiment is lessthan the
theoretical value. Suggest one precaution step that should be taken
in order to get a more accurate result.
............................................................................................................................................................
[1 mark] (f)Table 10 show s the molecular formula and the heat of
combustion for methanol andethanol. AlcoholMolecular formulaHeat of
combustion/kJmol-1 MethanolCH3OH-728 EthanolC2H5OH-1376 Based on
the information in Table 10, explain why there is a difference in
the value of heat of combustion between methanol and ethanol.
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[3 marks] SECTION B 11.(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 labeled 1 to 7.A
fixed volume of 5.0 cm3 of 1.0 mol dm-3 potassium iodide solution
was poured in each test tube.The volume of 1.0 mol dm-3lead(II)
nitrate solution that added are shown in Table 11.The height of
precipitate formed in each test tube was measured.The results are
shown in Table 11. Table 11 (i)Based on Table 11, plot a graph of
the height of precipitate against volume of lead(II) nitrate
solution. [3 marks] (ii)Determine the number of moles oflead(II)
ions and iodide ions that are required for the formation of
lead(II) iodide.Your answer shouldconsist of the following: the
volume of lead(II) nitrate solution that had reacted completely
with 5.0 cm3 of 1.0 mol dm-3 potassium iodide calclate the number
of moles of lead(II) ions and iodide ions calculate the number of
moles of iodide ions that has reacted with 1 mol oflead(II) ions.
write the ionic equation for the formation of lead(II) iodide. [7
marks] Test tube1234567 Volume of 1.0 moldm-3 lead(II) nitrate
solution /cm3 0.51.01.52.02.53.03.5 Height of precipitate
/cm1.12.23.44.45.55.55.5 Table 10 Chemistry Perfect Score/X A-Plus
Module 2012 47 (b)Diagram 11 shows the flow chart of reaction of
salt J.X oxide which is brown when hot and yellow when cold is
formed when salt J is heated strongly.Salt J dissolves in water to
form colourless solution.The solution formed is tested with
potassium iodide, KI solution. + + H2O Diagram 11 Based on the
information in Diagram 11: (i)Identify salt J,X oxide, brown gas Y,
colourless gas Z and yellow precipitate L. [5 marks] (ii)State the
name of the anion present in salt J. Then describe one chemical
test to determine the presence of anion in salt J. [5 marks]
12.Diagram 12.1 shows a series of reaction for salt S which is a
green colour compound. Salt S is heated strongly to produce black
residue of compound T and gas U. Compound T reacts with sulphuric
acid to form blue solution of compound W. Diagram 12.1 Based on
Diargram 12.1: (a)(i)Suggest one formula of the anion in salt S. [1
mark] (ii)Identify salt S, compound T, gas U and compound W. [4
marks] (b)Write a chemical equation for the reaction between
compound T and sulphuric acid. [2 marks] (c)Compound W is a soluble
salt. Describe chemical test to verify the cation and anion in
compound W. [5 marks] Salt JX OxideBrown gas Y Colourless gas Z
Salt J solutionYellow precipitate L Potassium iodide solution Heat
+ Salt SCompound T Gas U Compound W + H2SO4 Lime water turns cloudy
Pass through lime water Chemistry Perfect Score/X A-Plus Module
2012 48 (d)Diagram 12.2 shows the chemical equation for the
reaction between blue solution of compound W and barium nitrate
solution. Diagram 12.2 Based on Diagram 12.2: (i)State the name of
salt X and salt Y. [2 marks] (ii)State one observation and name the
type of reaction occurred. [2 marks] (iii)Compound W reacts with 50
cm3 of 0.1 mol dm-3 barium nitrate solution.Write the ionic
equation for the reaction and calculate the mass of salt X
produced. [Relative molecular mass of salt X: 233] [4 marks] 13
(a)Table 13 shows the incomplete observation for two experiments to
construct balanced chemical equation.
ExperimentProcedureObservation ACopper(II) carbonate is heated and
the gas produced is passed through lime water.. Green solid turns
black.The lime water turns milky. BPotassium iodide solution is
added to lead(II) nitrate solution. Table 13 (i)Based on the
observation, state the name of the products in experiment A and
write the chemical equation for the reaction. [3 marks ] (ii)State
one observation in experiment B and state the name of the products
formed. Write the chemical equation for the reaction. [4 marks ]
(b)You are given aluminiumnitrate solution and zinc nitrate
solution.Describe chemical tests that can be used to verify the
cations and anion in each solutions. [8 marks] (c)Excess of solid
copper(II) oxide is added to 25 cm3 of 1.0 mol dm-3sulphuric acid
to form copper(II) sulphate. [Relative atomic mass, Cu=64, S=32,
O=16] (i)Write the chemical equation for the reaction (ii)Calculate
the mass of copper (II) sulphate produced [5 marks] Compound
W(aq)+Ba(NO3)2(aq) Salt X(s)+ Salt Y(aq) Chemistry Perfect Score/X
A-Plus Module 2012 49 14 (a) (i) Rate of a givenreaction is
important in industries and in our everyday lives. State the four
factors that affect the rate of reaction. [4 marks] (ii)What are
the conditions required for the production of ammonia in Haber
Process? [3 marks] (b)A student carried out two experiments to
investigate the effect of concentration on the rate of reaction.
Diagram 3.1 shows the set-up of apparatus of the experiments.
Experiment Set-up of apparatus I Diagram 14.1 Table 14.2 shows the
result of the experiments. Time /s0306090120150180210 Volume of gas
ofExperiment I /cm3 0.005.0010.0014.2018.0021.3024.0026.00 Volume
of gas of Experiment II /cm3
0.0010.0017.0023.0025.0026.0026.0026.00 Table 14.2 (i) Plot the
graph of the volume of carbon dioxide gas against time for
Experiment I and II on the same axes on the graph paper provided .
[4 marks] (ii) Calculate the average rate of reaction for
Experiment I and II. [4 marks] (iii) Compare the rate of reaction
between Experiment I and Experiment II. Explain the differences in
the rate of reaction with reference to the collision theory. [5
marks] 0.2 g calcium carbonate powder Excess hydrochloric
acid0.2mol dm-3 Water Air 0.2 g calcium carbonate powder Excess
hydrochloric acid0.5mol dm-3 Water Air II Chemistry Perfect Score/X
A-Plus Module 2012 50 Question 14 (b) (i) Chemistry Perfect Score/X
A-Plus Module 2012 51 15. (a) A fixed mass of magnesium is added to
50 cm3 0.5 mol dm-3 of excess sulphuric acid . State 3 ways to
shorten the time for the magnesium to dissolve completely. [3
marks] (b) When potassium chlorate(V) is heated, it decomposedto
release oxygen gas according to the equation below. 2KClO3 2 KCl
+3O2 (i)Name a suitable catalyst that can be used to increase the
rate of decomposition of potassium chlorate(V) [1 mark] (ii)State 2
characteristics of a catalyst [2 marks] (iii) Contact Process is an
industrial process to manufacture sulphuric acid in large scale.
State and justify any two of the conditions involved in this
process . [4 marks] (c)The graph below shows the change of rate of
reaction with time when excesscalcium carbonate granules is reacted
with dilute hydrochloric acid. State and explain how the rate of
reaction changes with time. [3 marks] (d)Describe an experiment to
study the effect of catalystmanganese(IV) oxide on the rate of
decomposition of hydrogen peroxide.[7 marks] 16.(a)Diagram 16.1 and
16.2 show energy level diagrams.
(i)Compare both the energy level diagrams above. Your
explanation should include the followingionic equationstype of
chemical reactionsenergy content of reactants and products [6
marks]
(ii)Basedondiagram16.1,calculatethechangeintemperatureofthesolutionifexcess
magnesium powder is added to 50 cm3 of 0.2 mol dm-3 iron(II)
sulphate solution. [Given thatSpecific heat capacity of solution :
4.2 J g -1oC-1] [3 marks] (b)Explain why the heat of reaction
between 1.0 mole of silver nitrate solution and 1.0 mole of sodium
chloride solution is the same as the heat of reaction between 1.0
mole of silver nitrate solution and 0.5 mole of magnesium chloride
solution. [4 marks] Diagram16.1 Diagram16.2 Time / s Rate of
reaction MgSO4+Fe Mg(s)+ FeSO4 Energy H= - 200 kJmol-1 Energy
CaCl2+ Na2CO3 CaCO3+ 2NaCl H= + 12.6 kJmol-1 Chemistry Perfect
Score/X A-Plus Module 2012 52 (c)A student carried out an
experiment to determine the heat of neutralisation for the reaction
between 50 cm3 of 2.0 mol dm-3 hydrochloric acid and100 cm3 of2.0
mol dm-3 sodium hydroxide solution. The following data was
obtained:Initial temperature of hydrochloric acid =30.2 oC Initial
temperature of sodium hydroxide solution=30.2 oC Highest
temperature of the mixture of the solutions =42.2 oC (i)Calculate
the heat of neutralisation for this reaction. [Given that specific
heat capacity of solution = 4.2 J g -1oC -1] [3 marks] (ii)If the
experimentis repeatedusing 100 cm3 of 2.0 mol dm-3 hydrochloric
acid and 100 cm3 of 2.0 mol dm-3 sodiumhydroxide solution and all
other conditions are the same, predict the increase in temperature.
Explain your answer. [4 marks] SECTION C 17.(a) Acid HX is a
monoprotic acid while H2X is a diprotic acid. Both acid HX and H2X
are strong acid. Using suitable examples, explain what is meant by
(i)diprotic acid(ii)strong acid[ 4 marks ] (b)Table 9 shows the pH
value of sodium hydroxide and aqueous ammonia of the same
concentration Explain why sodium hydroxide solution and aqueous
ammonia of the same concentration have different pH value.[ 6 marks
] (c)Describe how to prepare 250 cm3 of 1.0 mol dm-3 potassium
hydroxide starting from solid potassium hydroxide. State the size
of volumetric flask used and calculate mass of potassium hydroxide
needed. [Relative atomic mass: H, 1; O, 16; K, 39] [ 10 marks ]
18(a)Salts is widely used in various fields. Name one example of
salt and its uses in each of the following fields: (i)agriculture
(ii)food preparation (iii)medicine [6 marks]
(b)Byusingallthechemicalsubstancesgivenbellowandsuitableapparatus,describealaboratory
experiment to prepare dry zinc sulphate salt. In your description,
include chemical equations involved. [12marks] AlkaliConcentration
/ moldm-3pH Sodium hydroxide solutiom0.1 13 Ammonia
aqueoussolutiom0.1 11 zinc nitrate solutionDilute sulphuric acid
sodium carbonate solution Chemistry Perfect Score/X A-Plus Module
2012 53 19 (a) Write an ionic equation to represent the reaction
given in the box above. [2 marks] (b)The rate of the above reaction
can be measured based on the mass of sulphur produced. Based on
this statement,state the meaning of the rate of reaction. [2 marks]
(c)Suggest two factors that can affect the rate of reaction stated
above and state the respective effects on the rate of reaction. [4
marks] (d)You are given a conical flask, a piece of white paper and
all other common apparatus found in normal school laboratory.
Describean experiment to show the effect of one ofthe factors that
you have given in (b).In your answer, you are required to show how
the data obtained can be analysedto help you draw the conclusion
for your experiment. [12 marks] 20.Table 20.1 shows the data from
Experiment I andExperimentII that were carried out to study the
rate of reaction ofmagnesium ribbon with two acids,X and Y .
ExperimentReactantsProducts IExcess ofmagnesium ribbon and50 cm3 of
acidX1.0 mol dm-3 Magnesium chloride and hydrogen gas IIExcess
ofmagnesium ribbon and50 cm3 of acid Y 1.0 mol dm-3 Magnesium
sulphate and hydrogen gas Table20.1 (a)(i) State the name ofacidsX
and Y. Write the chemical equation for the reaction of acid X with
magnesium. [3 marks] (ii)Calculate the number of mol of acid X or
acid Y that react with excess magnesium ribbon. [1 mark] (iii)Based
on this experiment what is meant by the rate of reaction? [1 mark]
(b)(i) At the same axis, sketch the graph of volume of gas against
time for experiment I and experiment II.[2 marks] (ii) Compare
therate of reaction in experiment I and II . Explain your answer
based on collision theory. [5 marks] (c)Describe one laboratory
experiment to conduct the Experiment I or Experiment II to
determinethe rate of reaction. Your answer should include the
following : -A labeled diagram showing the apparatus set-up
-Proceduresof the experiment -A table to collect the data [8 marks]
Sodium thiosulphate solution reacts with hydrochloric acid to form
sulphur, pungent gas sulphur dioxide, water and salt Chemistry
Perfect Score/X A-Plus Module 2012 54 21(a) A student carried out
an experiment in the laboratory to determine the heat of
precipitation of silver chloride, AgCl using the following chemical
substances : Table 21.1 shows the result of the experiment :
Initial temperature of silver nitrate, AgNO3 solution 29.0 oC
Initial temperature of sodium chloride, NaCl solution29.0 oC
Highest temperature of reaction mixture33.0 oC Table 21.1
(i)Calculate the heat of precipitation of silver chloride [
Specific heat capacity for all solution is 4.2 Jg-1oC-1and the
density of all solution is 1.0 g cm-3] (ii)Draw an energy level
diagram for the reaction between silver nitrate and sodium
chloride. [4 marks] (b)Table 10.2 shows the heat released for
Experiment I, II and III using different acid that has been reacted
with sodium hydroxide solution. ExperimentChemical EquationHeat
released IHCl+NaOHNaCl+H2O57 IICH3COOH+NaOHCH3COONa+H2O54
IIIH2SO4+2NaOHNa2SO4+2H2O 114 Based on Table 21.2, 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] 25 cm3 of 0.5 mol dm-3 silver nitrate
solution 25 cm3 of 0.5 mol dm-3 sodium chloride solution Chemistry
Perfect Score/X A-Plus Module 2012 55 22 (a)What is meant by
exothermic and endothermic reaction? Compare the changes in energy
content of the reactants and products for both of the reactions.[4
marks] (b)Diagram represent the energy level diagram for a chemical
reaction State four information that can be obtained from the above
diagram. [4 marks] (c)Reaction I and II below are the
thermochemical equation for the heat of precipitation. Reaction
I:AgNO3+NaCl AgCl + NaNO3 H = - 210kJmol-1 Reaction II :AgNO3+KCl
AgCl + KNO3 H = - 210kJmol-1 Explain why the value of heat of
precipitation in reactions I and II are the same.
[4 marks] d) Describe a laboratory experiment to determine the
heat of reaction for the above reaction. In your answer, include
the following : chemicals required procedures of the experiment
results and calculation involved[8 marks] 23. The thermochemical
equation for the combustion of butanol is given as follows:
C4H9OH+6O2 4CO2+ 5H2O H=-2679 kJmol-1 [Relative atomic mass : H=1,
C=12, O=16,specific heat capacity of water = 4.2 Jg-1 oC-1]
(a)State three information that can be obtained from the above
equation. [3 marks] (b)Calculate the mass of butanol that must be
burnt to raise the temperature of 400 cm3 of water by 25C.[3 marks]
(c) Describe an experiment to determine the heat of combustion of
butanol. Your answer should include: (i) apparatus set-up [2 marks]
(ii)procedure of the experiment[6 marks] (iii)data obtained from
the experiment[2 marks] (iv)calculation of heat of combustion of
butanol.[4 marks] Energy A + B C+D H= + xkJ mol-3 Ca2+(aq)+CO32-
(aq) CaCO3 (s) H = + 12.6 kJmol-1 Chemistry Perfect Score/X A-Plus
Module 2012 56 CHEMISTRY MODULE SET 1.Carbon Compounds
2.Manufactured Substances in Industry 3.Chemicals for Consumers
Chemistry Perfect Score/X A-Plus Module 2012 57 SECTION A 1.Diagram
1 shows the structural formula of compound X. Diagram 1 (a)
Compound X is an unsaturated hydrocarbon. What is the meaning of
unsaturated hydrocarbon?
....................................................................................
[2 marks] (b) State the homologous series for compound X.
............................................................................................
[1 mark] (c)Name the compound X.
............................................................................................
[1 mark] (d)At 180 oC and in the presence of nickel as catalyst,
compound X can be changed into saturated hydrocarbon compound. (i)
Name the reaction.
............................................................................................
[1 mark] (ii)Draw the structural formula for the compound formed.
[1 mark] (e)Compound X burns completely in excess oxygen. (i)Write
a balanced chemical equation for the complete combustion of X.
..............................................................................................................................................
[2 marks](ii)2.1 g of compound X undergoes complete combustion at
room conditions. Calculate the volume of carbon dioxide gas
released. [1 mol of gas occupies 24 dm3 at room conditions;
Relative atomic mass: H = 1; C = 12] [2 marks] Chemistry Perfect
Score/X A-Plus Module 2012 58 2.Diagram 2 shows a series of
reactions.Compound P with the molecular formula C2H6O, can be
prepared through fermentation of glucose solution. Diagram 2
(a)Name the compound P. .........................................
[1 mark] (b)State the functional group of compound P.
.........................................[1 mark] (c) In the
reaction I, compound Q is produced when an acidified potassium
dichromate (VI) solution is added into a test tube containing
compound P. (i)Name the reaction I.
.................................... [1 mark] (ii) State one
observation for this reaction. ................................. [1
mark] (iii) Draw the structural formula of compound Q.
[1 mark] (d)In the reaction II, compound R is formed when
compound P reacts with compound Q in the presence of concentrated
sulphuric acid. (i) Name the reaction II.
.................................... [1 mark] (ii)Name the compound
R. .................................. [1 mark] (iii)Give one
special physical property of compound R.
.................................... [1 mark] (iv)Write the
chemical equation for the reaction II.
........................................ [2 marks] Glucose
Compound P C2H6O Compound Q Compound R Reaction II Reaction I
Chemistry Perfect Score/X A-Plus Module 2012 59 3. Diagram 3 shows
a series of reactions involving compound Q, C2H6O. Diagram 3
(a)(i)State the name of reaction I. ..... [1 mark] (ii)State the
name of compound Q. .......... [1 mark] (iii) Draw the structural
formula for compound Q. [1 mark] (b)Write a chemical equation for
the complete combustion of compound Q. ... [2 marks] (c)(i)State
the name of gas R that produced in reaction III. ..... [1 mark]
(ii)Draw the set-up of apparatus to carry out reaction III in the
laboratory. [2 marks] (d)State the change of colour of acidified
potassium manganate(VII) solution in reaction IV. [1 mark] Glucose
Gas P Compound Q, C2H6OGas R Compound S, C2H4O2 Compound T Water
Yeast Combustion I + II III pieces of porcelain Acidified potassium
manganate(VII) solution IV Concentrated sulphuric acid, refluxed
with compound Q. V Chemistry Perfect Score/X A-Plus Module 2012 60
(e) (i) State the name of reaction V. . [1 mark] (ii) State the
name of compound T. . [1 mark] 4.(a) The following flow chart shows
the steps involved in the manufacture of an industrialsubstance L
and the production of fertiliser M. (i)What is substance L? .. [1
mark] (ii)Name the industrial process to produce substance L. .. [1
mark] iii)What is substance K? ... [1 mark] (iv) The conversion of
sulphur dioxide to substance M is very slow. Catalyst and high
temperature are usedto overcome these problems. State the catalyst
and the temperature used. [2 marks] (v)What is fertiliser M? . [1
mark] (b) Table 4 shows the manufactured substances in industries.
MaterialSubstance LAlloyPolymerGlass Example Reinforced concretes
Bronze Polyvinyl chloride (PVC) Borosilicate glass Table 4 Based on
Table 4, answerthefollowingquestions. (i)State the name of
substance L. .. [1mark] (ii) Draw and label the arrangement of
atoms in bronze.
[2marks] Chemistry Perfect Score/X A-Plus Module 2012 61 (iii)
Write the chemical equation for the polymerisation process of
Polyvinyl chloride. .. [1mark] (iv) State one reason for
borosilicate glass to use in laboratory glassware. .. [1mark]
5.(a)Soap can be preparedfromthe reaction between oil and
concentrated sodium hydroxide. Diagram 5 shows the equation for the
reaction. + 3NaOH Soap Y+ R is a carbon chainwith 15 carbon atoms.
(i) State what is soap. .. [1 mark] (ii) Draw the structural
formulafor soap Yformed . On the diagram you have drawn , label the
hydrophobic and hydrophilic parts of the soap
[2 marks] (iii)Name this reaction . [1 mark] (iv) During the
preparation of soap, sodium chloride is added to the soap mixture.
Explain why? [1 mark] CH2OH O RCOCH2 CH2OH O RCOCH2 CH2OH O RCOCH2
Diagram 5 Chemistry Perfect Score/X A-Plus Module 2012 62 (b)
Medicine is often given to patients to cure or prevent diseases.
The table below shows the examples of four types of commonly used
medicines. MedicineExample AnalgesicsAspirin QPenicillin
Psychotherapeutic medicineP (i)What is the function of analgesics
medicines?
.... [1 mark] (ii)What is the negative effect of taking
aspirin.
.... [1 mark] (iii)State the type of medicine for Q.
... [1 mark] (iv) Why is it very important to follow the
prescription and to complete the dosage when taking penicillin?
....
.... [1 mark] (v) State one example of P. .. [1 mark] Chemistry
Perfect Score/X A-Plus Module 2012 63 SECTION B 6(a)Table 6 shows
some information about three members of a homologous series. Member
of homologous series Boiling point (C) PreparationOxidation product
Ethanol78C2H4 + H2O C2H5OHEthanoic acid Propanol97C3H6 + H2O
C3H7OHPropanoic acid Butanol118C4H8 + H2O C4H9OHButanoic acid Table
6 Based on Table 6, state and explain five characteristics of a
homologous series. [10 marks] (b)The following information is about
an organic compound X. Empirical formula is CH2O Relative molecular
mass is 60 Reacts with calcium carbonate to produce a type of gas
that turns lime water chalkyBased on the information given: (i)
State the molecular formula of X. (Relative atomic mass : C = 12, H
= 1, O = 16) [2 marks] (ii)State the name of the homologous series
for Xandexplain your answer. [2 marks] (iii)Write a balanced
chemical equation for the reaction of compound X with calcium
carbonate.[2 marks] (c)Diagram 6 shows the structural formulae of
hydrocarbon of compounds P and Q. Compound PCompound Q Diagram 6
Compare and contrast these two hydrocarbons based on their
structures. [4 marks] 7.(a) A hydrocarbon M, consists of 85.7% of
carbon and X% of hydrogen by mass.[Relative atomic mass: C = 12; H
= 1 , Relative molecular mass of M = 56.] (i) What is the value of
X. [1 mark] (ii)Determine the empirical formula and molecular
formula of hydrocarbon X.[5 marks] (iii) Draw the structural of the
two isomers of hydrocarbon M.Write the names for each isomer [4
marks] (iv) CompoundM burns with sootier flames as compared to
butane. Explainandprove.[3 marks] Chemistry Perfect Score/X A-Plus
Module 2012 64 (b)Natural rubber is a natural polymer. (i) Give
another two examples of natural polymer. [2 marks] (ii)Name and
draw the structural formula of the monomer of natural rubber. [2
marks] (c)The tyres of aircrafts are made from vulcanised rubber.
(i) What is vulcanised rubber? [1 marks] (ii)Explain why vulcanised
rubber is more elastic than unvulcanised rubber. [2 marks]
8(a)Diagram 8.1 shows the structural formula of two of
hydrocarbons. Hydrocarbon A Hydrocarbon B
Diagram 8.1 (i)State the type of bond, homologous series and
general formula of hydrocarbon A and hydrocarbon B. [6 marks]
(ii)Complete combustion of hydrocarbon A produces gas C and
water.State the name of gas C and write the chemical equation for
the reaction. [3 marks] (iii)Whichhydrocarbon change the colour of
bromine water from brown to colourless. Explain your answer. [3
marks] (iv)Diagram 8.2 shows the burning of hydrocarbon A and
hydrocarbon B in air. Compare the sootiness of hydrocarbon A and
hydrocarbon B.Explain your answer.[Given that the relative atomic
mass ofH = 1, C = 12] [4 marks] Diagram 8.2 Porcelain dish Filter
paper Soot Hydrocarbon AHydrocarbon BChemistry Perfect Score/X
A-Plus Module 2012 65 (b)Diagram 8.3 shows the reaction between
carboxylic acid X and alcohol Y. Diagram 8.3 Draw the structural
formula and state the name of carboxylic acid X and alcohol Y. [4
marks] 9. (a)Sulphur dioxide, SO2, is one of the by-products of the
Contact Process. It can cause environmental pollution like acid
rain. Sulphur dioxide gas dissolves in rain water to produce
sulphurous acid (i)Write the chemical equation for the reaction
between sulphur dioxide gas and rain water. (ii)State three effects
of acid rain to the environment. [4 marks] (b)Diagram 7 shows an
industry preparation of sulphuric acid by the Contact Process.
Diagram 9 (i)Name the compound X. (ii)Write the chemical equation
of the reaction at stage II. (iii) The chemical equation below
shows the reaction between sulphur and oxygen gas at stage I. S+O2
SO2 Given that the relative atomic mass of S = 32, O = 16 and the
molar volume of any gas is24 dm3mol-1 at room temperature and
pressure. Calculate the maximum volume of sulphur dioxide gas
produced if 48 g of sulphur is burnt completely in oxygen gas. [6
marks] (c)Brass is an alloy of copper. Pure copper is ductile and
malleable whereas brass is stronger and harder than copper.
(i)Explain why pure copper is ductile and malleable? [5 marks]
(ii)Name the element which is added to copper to make brass.
Explain why brass is strong and harder than copper. Draw a diagram
to show the arrangement of atoms in brass. [5 marks] SSO2 SO3 X
H2SO4 Stage IStage II Stage III Stage IV OxygenOxygenConcentrated
sulphuric acidWaterCarboxylic acid X AlcoholY +Water+ Chemistry
Perfect Score/X A-Plus Module 2012 66 10.(a) Food preservatives are
substances added to food so that the food can be kept for longer
periodsfor time. Using two suitable examples, explain how they work
as preservative. [4 marks] (b)The following is the information
about a child. 2 years old High fever Whooping cough (i)Can aspirin
be used to treat the child? Explain why.[2 marks] (ii)Name two
examples of modernmedicine that can be used to treat the child . [2
marks] (iii) Explain the effect if the precautions states in
(b)(ii) are not followed properly. [2 marks] (c ) Table 10 shows
the food additives that are added to a certain food by two chefs.
Chef WanChef Koh Turmeric Sugar, salt and spice Garlic Tartrazine
Monosodium glutamate Ascorbic acid Table 10 Based on Table 10,
categorise the food additives. Include in your answer the function
of eachtype of food additives and the disadvantages of using any
two food additives. [10 marks] Chemistry Perfect Score/X A-Plus
Module 2012 67 SECTION C 11. (a)Table 11 shows the result of two
sets of experiment to investigate the coagulation of latex. SetType
of solutionObservation ILatex + solution XLatex coagulate very
fastIILatex + solution YLatex does not coagulate Table 11 (i)
Suggest one possible substance for solution X. and Y [2 marks] (ii)
Explain the process of coagulation of latex in set I [4 marks]
(iii) Explain why latex does not coagulate in set II[2 marks]
(b)Diagram 11 shows how compound Q is formed from alkene W. Diagram
11 (i) Name the homologous series of compound Q.[1 mark] (ii)State
two chemical properties of compound Q. [2 marks] (iii)By using a
compound Q with number of carbon atom per molecule more than one,
describe an experiment to convert compound Q to alkene.Your answer
should consist of the following: Procedure of the experiment A
labelled diagram showing the apparatus set-up The test to confirm
the product is alkene[9 marks] Alkene W+H2O Compound Q Chemistry
Perfect Score/X A-Plus Module 2012 68 12.Diagram 12.1 shows five
structural formula of carbon compound. Diagram 12.1 (a)Choose any
one of the compound in Diagram 12.1, state the products formed when
the compound burn completely in excess oxygen gas. Write the
chemical equation involve. [3 marks] (b)State the name of two
compounds in Diagram 12.1 that are isomer.Explain your answer. [3
marks] (c)Describe a chemical test to differentiate between
compound A and compound B. [4 marks] (d)Diagram 10.2 shows the
reaction between compound E and carboxylic acid. Diagram12.2 (i)
State the name an example of a member of carboxylic acid and state
the name of ester that formed when the named carboxylic acid react
with compound E. Draw the structural formula of named carboxylic
acid and ester that formed. [4 marks] (ii) Describe an experiment
to produce ester in (d) (i) in laboratory. [6 marks] Compound E+
Carboxylic acidester Chemistry Perfect Score/X A-Plus Module 2012
69 13(a)Diagram 13.1 shows a structural formula of butene, Diagram
9.1 Draw structural formulae for another two isomers of butene and
names each isomer according to the IUPAC nomenclature. [4 marks]
(b)Diagram 9.2 shows the structural formula of an ester Diagram
13.2 Based on diagram 13.2: (i)Identify the two organic chemicals
needed to produce the ester above. [2 marks] (ii)State three
chemical properties for each organic chemicals that you stated in
9(b)(i). [6 marks] (c)Diagram 13.3 shows the formula of two
hydrocarbons P and Q : PQ Diagram 13.3 (i)State the name of
hydrocarbons P and Q. (ii)Describe two chemical tests to
differentiate between hydrocarbon P and Q.Your description must
include the procedure and observation.[8 marks] CCCCH HHHH H HH
CCCOH H HH HHO C H H CH H CH3(CH2)4CH3CH3(CH2)3CH = CH2 Chemistry
Perfect Score/X A-Plus Module 2012 70 14Diagram 14shows the
industrial manufacture of ammonia. Diagram14 (a) State the name of
the above process, catalyst Y and write a chemical equation for
there