中五 化學試卷 (F5 Chemistry Past Paper)

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S5 Final Term Exam
GENERAL INSTRUCTIONS
HONG KONG DIPLOMA OF SECONDARY EDUCATION EXAMINATION
(SECONDARY FIVE FINAL TERM
EXAMINATION PAPER)
A Periodic Table is printed on the back of Question-Answer Book B. Atomic numbers and relative
atomic masses of elements can be obtained from the Periodic Table.
Time allowed: 2 hours 30 minutes
This paper must be answered in English.
INSTRUCTIONS FOR SECTION A (MULTIPLE-CHOICE QUESTIONS)
There are TWO sections, A and B, in this Paper. You are advised to finish Section A in about 45
Section A consists of multiple-choice questions in this question paper, while Section B contains
conventional questions printed separately in Question-Answer Book B.
Answers to Section A should be marked on the Multiple-choice Answer Sheet while answers to Section
B should be written in the spaces provided in Question-Answer Book B. The Answer Sheet for Section
A and the Question-Answer Book for Section B will be collected separately at the end of the
examination.
Read carefully the instructions on the Answer Sheet. Write your name, class and class number in the
space provided.
When told to open this book, you should check that all the questions are there. Look for the words
'END OF SECTION A' after the last question.
All questions carry equal marks.
ANSWER ALL QUESTIONS. You are advised to use an HB pencil to mark all the answers on the
Answer Sheet, so that wrong marks can be completely erased with a clean rubber. You must mark the
answers clearly; otherwise you will lose marks if the answers cannot be captured.
You should mark only ONE answer for each question. If you mark more than one answer, you will
receive NO MARKS for that question.
No marks will be deducted for wrong answers.
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S5 Final Term Exam
S5 Final Term Exam
28. Consider the following information:
W(g) + X(g) = Y(g)
2Y(g) = Z(g)
What is the equilibrium constant expression for the following reaction in terms of Ke1 and Ke2?
Z(g) = 2W(g) + 2X(g)
(K₁) ² × K c2
(K1)² × Kc2
29. Consider the following conversion:
K₂Cr₂O₁/H+
K₂Cr₂O7/H+
30. Consider the following conversion:
101 uit ionowil
Hydrogenation
Hydrogenation
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7 indicates tie
K₂Cr₂O7/H+
K₂Cr₂O7/H+
ired in each step?
conc. H₂SO4
conc. H₂SO4
conc. H₂SO4
actions in Step 1 and Step 2?
Condensation
Substitution
Substitution
Condensation
S5 Final Term Exam
S5 Final Term Exam
31. How many acyclic isomers may the molecular formula C4H,Br represent?
32. Geraniol is a compound that can be found in some plants. Its structure is shown below:
Which of the following statements about geraniol is/are correct?
(1) Geraniol is highly soluble in water.
(2) The systematic name of geraniol is 3,7-dimethylocta-2,6-dien-1-ol.
(3) Geraniol can turn orange acidified potassium dichromate solution green.
A. (1) only
(1) and (3) only
(2) and (3) only
33. The structure of vitamin C is shown below:
A. (1) only
(1) and (3) only
(2) and (3) only
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Which of the following statements about vitamin C is/are correct?
(1) Its empirical formula is CHgO6.
(2) It can decolorize acidified potassium permanganate solution.
(3) It contains three chiral centres.
S5 Final Term Exam
S5 Final Term Exam
34. Which of the following properties of manganese characterize(s) it as a transition metal?
It forms an ion with a charge of +2.
(2) It forms coloured ions in aqueous solutions.
It tarnishes in air.
B. (2) only
C. (1) and (3) only
D. (2) and (3) only
35. Consider the following equilibrium system in a closed container:
N₂O4(g) ⇒ 2NO₂(g)
Which of the following statements is/are correct when the volume of the container decreases at
constant temperature?
(1) The value of K. remains unchanged.
(2) The concentration of NO₂ decreases.
The rate of forward reaction decreases.
A. (1) only
(1) and (3) only
D. (2) and (3) only
36. Consider the following statements and choose the best answer:
1st statement
The progress of the reaction between
magnesium and dilute sulphuric acid can
be monitored by measuring the change in
pressure in the reaction flask.
A. Both statements are true and the 2nd statement is a correct explanation of the 1st
B. Both statements are true but the 2nd statement is NOT a correct explanation of the
1st statement.
The 1st statement is false but the 2nd statement is true.
D. Both statements are false.
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2nd statement
The reaction of magnesium with dilute
sulphuric acid produces a gas.
END OF SECTION A
S5 Final Term Exam
S5 Final Term Exam
HONG KONG DIPLOMA OF SECONDARY EDUCATION
EXAMINATION
(SECONDARY FIVE FINAL TERM
EXAMINATION PAPER)
SECTION B: Question-Answer Book B
This paper must be answered in English.
INSTRUCTIONS FOR SECTION B
(1) Write your name, class and class number in the space
provided on this page.
(2) Refer to the general instructions on the cover of the
Question Paper for Section A.
(3) This section consists of TWO parts, Part I and Part II.
(4) Answer ALL questions in both Parts I and II. Write
your answers in the spaces provided in this
Question-Answer Book. Do not write in the margins.
Answers written in the margins will not be marked.
(5) An asterisk (*) has been put next to the questions
where one mark will be awarded for effective
communication.
(6) Supplementary answer sheets will be provided on
request. Write your name, class, class number and
question number on the answer sheets and fasten
them with a string INSIDE this Question-Answer Book.
(7) No extra time will be given to you for filling in your
name, class and class number in the
Question-Answer Book after the 'Time
'Time is up'
announcement.
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S5 Final Term Exam
S5 Final Term Exam
Answer ALL questions. Write your answers in the spaces provided.
1. When ammonia dissolves in water, it ionizes to give ammonium ions and hydroxide ions.
(a) Write an equation for the ionization of ammonia in water.
(b) Ammonium ion is an example for illustrating the formation of dative covalent bond.
(i) What is the meaning of the term 'dative covalent bond'?
(ii) Draw the electron diagram for ammonium ion, showing electrons in the outermost
shells only.
(c) Ammonium salts react with alkalis to form ammonia. In an experiment, a mixture of
ammonium chloride solution and sodium hydroxide solution is heated.
(i) Write a chemical equation for the reaction involved.
(ii) Suggest a test to show that ammonia is an alkaline gas.
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S5 Final Term Exam
S5 Final Term Exam
2. Consider the following two experiments.
(a) A copper wire is added to concentrated nitric acid.
(i) State one expected observable change.
(ii) Write the ionic equation for the reaction involved.
(b) A few drops of bromine (dissolved in CC14) are added to hexane and the reaction mixture
is put under sunlight.
(i) Name the type of reaction involved.
(ii) State one expected observable change.
(iii) Write the structural formulae of TWO of the organic products formed.
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S5 Final Term Exam
S5 Final Term Exam
3. Natural gas is a fossil fuel. It consists of a mixture of hydrocarbons with low molecular masses
such as methane, ethane and propane.
(a) Consider the following statement:
(i) Give one reason to support the above statement.
'Natural gas is an environmentally friendly fuel.'
(ii) Give one reason to oppose the above statement.
(b) Methane is the most abundant component in natural gas. It is widely used in the chemical
(i) Draw the three-dimensional structure of methane.
(ii) Suggest a physical method to isolate methane from natural gas.
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S5 Final Term Exam
S5 Final Term Exam
3. (b) (iii) Industrially, carbon disulphide is produced from the reaction between methane and
(1) Given that:
2CH4(g) + 8S(s) → 2CS₂(1) + 4H₂S(g)
AH [CH4(g)] = -74.8 kJ mol-¹
AHCS₂(1)] = +89.0 kJ mol-¹
AHH₂S(g)] = -19.6 kJ mol¯¹
Calculate the standard enthalpy change of the above reaction.
(2) Carbon disulphide is commonly used as a non-polar solvent. Based on the
structure of the carbon disulphide molecule, explain why it is non-polar.
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S5 Final Term Exam
S5 Final Term Exam
4. In traditional gold extraction process, gold-containing ores are ground into smaller pieces
before mixing with calcium cyanide solution. Air or pure oxygen will then be bubbled into the
mixture. 'Gold cyanidation' occurs accordingly:
4Au(s) + 8CN (aq) + O₂(g) + 2H₂O(1) → 4[Au(CN)₂] (aq) + 4OH(aq)
Insoluble solids is then removed and the resultant solution is collected. Finally, zinc powder is
added to the resultant solution to recover gold.
(a) State the importance of grinding the ores into smaller pieces before 'gold cyanidation'.
(b) The calcium cyanide solution used in 'gold cyanidation' is produced by the reaction
between hydrocyanic acid (HCN(aq)) and calcium hydroxide solution.
(i) Draw the electron diagram for hydrogen cyanide molecule, showing electrons in the
outermost shells only.
(ii) Write a chemical equation for the reaction between hydrocyanic acid and calcium
hydroxide solution.
(c) Draw a labelled diagram to show how to remove the insoluble solids in 'gold cyanidation'.
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S5 Final Term Exam
S5 Final Term Exam
4. (d) With reference to 'gold cyanidation', identify the species undergoing oxidation and
reduction respectively. Explain your answers in terms of changes in oxidation numbers.
(e) Explain why zinc can recover gold from the resultant solution.
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S5 Final Term Exam
S5 Final Term Exam
This section consists of two parts. There are 24 questions in PART I and 12 questions in PART
Choose the best answer for each question.
Candidates may refer to the Periodic Table printed on the back of Question-Answer Book B.
1. The electron diagram of Y₂ is shown below:
Which of the following is the structural formula for the compound formed between element Y
and chlorine?
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Which of the following is made up of discrete molecules?
In which of the following species does chlorine has the highest oxidation number?
Which of the following processes would produce a colourless gas?
A. Passing steam over heated zinc granules
B. Adding a magnesium ribbon to cold water
C. Adding calcium oxide powder to dilute hydrochloric acid
Heating copper(II) oxide strongly
S5 Final Term Exam
S5 Final Term Exam
5. Copper is widely used to make electrical wires which utilize its high electrical conductivity.
Crude copper is not suitable as impurities greatly reduce its electrical conductivity. Purification
of copper is achieved by electrolytic refining as illustrated in the diagram below.
Impure copper r
impure copper rod
electrolyte
(b) With the h
electrolytic
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(c) It is known that the impure copper rods contain zinc. Explain whether zinc will deposit on
the thin sheets of pure copper.
› copper serve as the cathodes.
thin sheet of
pure copper
mpure copper can be purified by
S5 Final Term Exam
S5 Final Term Exam
*6. State the environmental problems associated with the popular use of batteries in modern life,
and suggest a method to reduce the problems.
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S5 Final Term Exam
S5 Final Term Exam
7. Account for each of the following:
(a) HF has a higher boiling point than HCl.
(b) Metals are malleable.
(c) Carbon can form a large number of compounds.
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S5 Final Term Exam
S5 Final Term Exam
8. When sodium nitrate (NaNO3) is heated strongly in a boiling tube, it melts and effervescence
occurs. When a glowing splint is put at the mouth of the boiling tube, the glowing splint
relights. Upon cooling, a white solid is left in the boiling tube.
(a) Suggest the gas that causes effervescence.
(b) Analysis shows that the white solid left contains 33.3% sodium, 20.3% nitrogen and
46.4% oxygen by mass. Determine the empirical formula of the white solid.
(Relative atomic masses: N = 14.0, O = 16.0, Na = 23.0)
(c) Deduce the equation for the thermal decomposition of sodium nitrate.
(d) Predict, with explanation, whether the white solid is soluble in water.
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S5 Final Term Exam
S5 Final Term Exam
9. To determine the molarity of sulphuric acid in a rust remover, a sample of rust remover was
titrated against 2.05 M NaOH(aq). The diagram below shows the set-up of the titration:
2.05 M NaOH(aq)
³ of NaOH(aq) are added to 10.0 cm³ of rust
reacts with NaOH(aq) accordingly, and the
1 mixture is recorded by the data-logger. The graph below shows
volume of NaOH(aq) added (cm³)
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re the experiment.
S5 Final Term Exam
S5 Final Term Exam
9. (b) Explain the variation of the temperature with the volume of NaOH(aq) added.
(c) (i) Determine the volume of NaOH(aq) needed to completely neutralize the sulphuric
acid in the rust remover.
(ii) Calculate the molarity of sulphuric acid in the rust remover.
(d) It is known that the rust remover is purple in colour. Suggest another method to determine
the end point of the titration.
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END OF PART I
S5 Final Term Exam
S5 Final Term Exam
*10. You are provided with common laboratory apparatus, a magnesium ribbon and dilute
hydrochloric acid. Outline how you would perform an experiment to determine the molar
volume of hydrogen gas under the experimental conditions.
11. (a) Consider the following oxides:
Na₂O, MgO, Al2O3, SiO2, P4O10, SO2, C1₂O
(i) Which of these oxides can dissolve well in water to form an alkaline solution?
(ii) Which of these oxides can react with sodium hydroxide?
(b) State and explain which Period 3 element has the highest electrical conductivity.
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S5 Final Term Exam
S5 Final Term Exam
12. The structures of fructose, mannose and mannitol are shown below:
(ii) Name the type of reaction involved.
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(a) In the above diagram, label ALL chiral carbon atom(s) in the structure of fructose by using
(b) Fructose and mannose are isomers. Name the type of isomerism involved.
(c) Mannitol can be used as a sweetener. It can be synthesized from fructose:
fructose →→→ mannitol
(i) Suggest the reagents required for the conversion.
A student suggested that mannitol can be converted to mannose by heating with acidified
K₂Cr₂O₂(aq) under reflux. Comment on the suggestion.
S5 Final Term Exam
S5 Final Term Exam
13. The structural formula of 2-chlorobutane is shown below:
CH3CH₂CHCH3
(a) 2-chlorobutane exists in two isomeric compounds.
(i) Draw the three-dimensional structures for the two compounds.
(ii) State one difference in physical property of the two compounds.
(b) Outline a synthetic route, with no more than three steps, to accomplish the conversion of
butanal to 2-chlorobutane. For each step, give the reagent(s), reaction conditions (as
appropriate) and structure of the intermediate.
CH₂CH₂CHCH₂
2-chlorobutane
CH₂CH₂CH₂CH
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S5 Final Term Exam
S5 Final Term Exam
14. CF3COOH is a weak acid. It undergoes incomplete ionization in water:
CF3COOH(aq) ⇒ CF3COO¯(aq) + H*(aq) K = 0.302 mol dm³ at 298K
(a) What is the systematic name of CF3COOH?
(b) Write an expression for the equilibrium constant (Kc) for the ionization of CF3COOH in
(c) 0.01 mol of CF3COOH is dissolved in water to form a 250.0 cm³ of solution. Calculate the
equilibrium concentration of H*(aq) and hence determine the pH value of the solution.
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S5 Final Term Exam
S5 Final Term Exam
5. Which of the following statements about 50.0 cm³ of 0.10 M sulphuric acid is correct?
(Relative atomic mass: Mg = 24.3)
Its pH value is 1.
It contains H*(aq), OH (aq) and SO² (aq).
0.2 g of magnesium can completely dissolve in it.
D. It is a weaker acid than 1.0 M sulphuric acid.
Which of the following experiments would give a clear colourless solution?
B. Adding limestone to excess sulphuric acid
C. Adding silver nitrate solution to excess sodium chloride solution
D. Adding magnesium hydroxide to excess hydrochloric acid
Which of the following combinations is INCORRECT?
Adding sodium sulphite solution to excess acidified potassium permanganate
Substance Melting point / °C
The following table shows the properties of four substances:
Electrical conductivity in
solid state
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To fill airships
To make ammonia
As a refrigerant
To make table salts
Non-conducting
Non-conducting
Non-conducting
Which of the above substances is most likely to have a giant covalent structure?
Solubility in water
S5 Final Term Exam
S5 Final Term Exam
15. In an experiment, a student follows the progress of the following reaction by titration:
HCOOCH,(aq)+NaOH(aq) → HCOONa(aq) +CH,OH(aq)
The procedure of the experiment is shown below:
Titrate NaOH(aq) in the reaction mixture with dilute H₂SO4(aq), using
phenolphthalein as indicator.
Plot a graph of volume of titre against time.
(a) Suggest what apparatus should be used in step 2 to withdraw the reaction mixture.
(b) What is the purpose of adding a large amount of cold distilled water to the reaction mixture
Mix HCOOCH3(aq) with excess NaOH(aq).
Withdraw portions of the reaction mixture at fixed time intervals.
Add a large amount of cold distilled water to the reaction mixture. Record
the time (t) at which distilled water is added.
(c) State the colour change at the end point of titration in step 4.
(d) Sketch a graph of the volume of titre against time.
END OF SECTION B
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END OF PAPER
S5 Final Term Exam
© Aristo Educational Press Ltd 2018
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S5 Final Term Exam
(223) (226)
138,9 178.5
(227) (261)
140.1 140.9
232.0 (231)
180.9 183.9
atomic number RIF
relative atomic mass 相對原子質量
PERIODIC TABLE 周期表
190.2 192.2
200.6 204.4
209.0 (209) (210)
S5 Final Term Exam
S5 Final Term Exam
9. Which of the following molecules has a non-octet structure?
C. CH₂Cl₂
10. The diagram below shows an electrolytic cell:
an alloy of
zinc and iron
11. The following table shows some information about four fuels:
Standard enthalpy
change of combustion / kJ
sis, the solution around the alloy gradually turns pale green.
a mixture of zinc nitrate solution
and silver nitrate solution
s at the alloy.
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Density / g cm
Which of the following fuels releases the least amount of heat upon complete combustion?
15.0 cm³ of hexane
12.0 cm³ of octane
20.0 cm³ of methanol
18.0 cm³ of ethanol
Molar mass /
S5 Final Term Exam
S5 Final Term Exam
Directions: Questions 12 to 14 refer to the following experiment:
To determine the concentration of ethanoic acid in a vinegar sample, 25.0 cm³ of the vinegar sample
was withdrawn to apparatus Y using apparatus X and then made up to 100.0 cm³ with distilled water.
A few portions of 10.0 cm³ of the diluted vinegar were then withdrawn to apparatus Z and titrated
against 0.272 mol dm3 of NaOH(aq). The average titre was 12.30 cm³.
12. Which of the following combinations is correct?
Apparatus X
Measuring cylinder
Measuring cylinder
From pink to colourless
From yellow to orange
D. From orange to yellow
15. Refer to the following equation:
14. What is the concentration of ethanoic acid in the vinegar sample?
A. 0.13 mol dm¯³
B. 0.33 mol dm¯³
1.34 mol dm¯³
D. 2.68 mol dm¯³
Apparatus Y
Volumetric flask
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Volumetric flask
13. What would be the colour change if phenolphthalein was used to detect the end point?
A. From colourless to pink
Conical flask
Conical flask
Apparatus Z
Conical flask
Conical flask
3Mg(s) + Al₂O3(s) → 3MgO(s) + 2Al(s)
Y mole of magnesium reacts with Y mole of aluminium oxide. What is the theoretical mass of
aluminium produced?
(Relative atomic mass: Al = 27.0)
S5 Final Term Exam
S5 Final Term Exam
16. Which of the following molecules is polar and trigonal planar in shape?
17. 0.015 mol of metal X is required to completely reduce 50.0 cm³ of 0.2 M VO₂ (aq) to V²+ (aq).
Which of the following could metal X be?
18. Which of the following statements about fractional distillation of crude oil is/are correct?
(1) The separation of hydrocarbons involves both chemical changes and physical changes.
(2) Naphtha is collected at a higher position in the fractionating tower than petrol.
(3) Hydrocarbons are separated according to their viscosity.
A. (1) only
(1) and (3) only
D. (2) and (3) only
19. Which of the following statements about the reaction of methane with bromine under sunlight
is/are correct?
(1) A mixture of organic compounds is produced.
(2) Sunlight provides energy to break the C-H bond to initiate the reaction.
(3) The reaction stops immediately when the reaction mixture is removed from the light
A. (1) only
B. (2) only
(1) and (3) only
(2) and (3) only
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S5 Final Term Exam
S5 Final Term Exam
20. Which of the following pairs of substances can be distinguished by using bromine solution?
(1) Sodium sulphate and sodium sulphite
(2) Potassium chloride and potassium bromide
Hexane and hex-1-ene
A. (1) and (2) only
B. (1) and (3) only
C. (2) and (3) only
(1), (2) and (3)
21. Which of the following statements about tin (atomic number = 50) is/are correct?
(1) It is a transition metal.
Tin can be displaced from tin(II) nitrate solution by iron.
(3) Food cans can be protected from rusting by tin-plating.
A. (1) only
(1) and (3) only
(2) and (3) only
22. Which of the following statements are correct?
(1) For an exothermic reaction, the products have a lower enthalpy than the reactants.
(2) The heat change of a reaction in a constant volume is regarded as the enthalpy change.
(3) Mixing ethanol with hexane is an endothermic process.
A. (1) and (2) only
B. (1) and (3) only
(2) and (3) only
D. (1), (2) and (3)
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S5 Final Term Exam
S5 Final Term Exam
23. Consider the following statements and choose the best answer:
Neon has a higher boiling point than
A. Both statements are true and the 2nd statement is a correct explanation of the 1st
1st statement
Both statements are true but the 2nd statement is NOT a correct explanation of the
1st statement.
The 1st statement is false but the 2nd statement is true.
D. Both statements are false.
24. Consider the following statements and choose the best answer:
A 'corrosive' hazard warning label
should be put on the bottle that stores
1st statement
Neon has a larger relative atomic mass than
2nd statement
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Both statements are true and the 2nd statement is a correct explanation of the 1st
END OF PARTI
2nd statement
Sodium reacts with water to form a strongly
alkaline solution.
Both statements are true but the 2nd statement is NOT a correct explanation of the
1st statement.
The 1st statement is false but the 2nd statement is true.
Both statements are false.
S5 Final Term Exam
S5 Final Term Exam
25. Which of the following statements about an equilibrium system is INCORRECT?
The use of catalysts has no effect on the equilibrium position.
The rates of the forward reaction and the backward reaction are zero.
The concentrations of the reactants and products remain unchanged.
D. The equilibrium can be attained from either the forward or the backward reaction.
26. There are three gas chambers containing different gases. Consider the following information:
25.0 cm³ of CH4(g) at 1 atm and 25°C
Gas chamber W
Gas chamber X
Gas chamber Y
50.0 cm³ of CO(g) at 1 atm and 25°C
75.0 cm³ of Ar(g) at 1 atm and 25°C
Which of the following is the correct ascending order of the numbers of atoms in the gas
27. Consider the following information of two experiments:
Experiment I Adding 1.0 g of calcium carbonate to 50.0 cm³ of 0.5 M HCl(aq)
Experiment II
Adding 1.0 g of calcium carbonate to 100.0 cm³ of 0.5 M HCl(aq)
Which of the following combinations is correct?
(Relative atomic masses: C = 12.0, O = 16.0, Ca = 40.1)
Initial rate of formation of CO₂(g)
Experiment I < Experiment II
Experiment I < Experiment II
Experiment I = Experiment II
Experiment I = Experiment II
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Total volume of CO₂(g) formed
Experiment I < Experiment II
Experiment I = Experiment II
Experiment I < Experiment II
Experiment I = Experiment II
S5 Final Term Exam