1 Diagram 1 shows a safety equipment in the laboratory. What is the function of this equipment? star A A specially designed equipment to carry out experiments that release toxic vapours, flammable or pungent smells B Used to wash and clean the body when an accident occurs on parts of the body C Used for extinguishing fire in the laboratory D Used to remove chemical substances, oil, dirt and microorganisms from the hands T4 Chapter 1.3 Usage, Management and Handling of Apparatus and Materials
2 Chemists use the concept of relative atomic mass by comparing the mass of atom of an element to the mass of atom of another element that is chosen as the standard. In 1961, chemists across the world agreed to use one of the isotopic atoms of carbon as the standard atom. Which of the following isotopic atom of carbon chosen as standard atom? star A Carbon - 12 B Carbon - 13 C Carbon - 14 T4 Chapter 3.1 Relative Atomic Mass and Relative Molecular Mass
3 Which of the following is the property of covalent compound? star A Dissolve in water B High melting and boiling points C Conducts electricity in aqueous state D Does not conduct electricity in solid state T4 Chapter 5.7 Properties of Ionic Compounds and Covalent Compounds
4 Which statement exactly explains the meaning of rate of reaction? star A The decreases of the quantity of the product per unit time B The increases of the quantity of the reactant per unit time C The changes in the quantity of the reactant per unit time or the changes in the quantity of product per unit time T4 Chapter 7.1 Determining Rate of Reaction
5 Which of the following is true about an oxidation reaction? star A Oxidation reaction takes place when a reactant loses oxygen B Oxidation reaction takes place when a reactant gains hydrogen C Oxidation reaction takes place when a reactant loses electron D Oxidation reaction takes place when the oxidation number of an element in the reactant decreases T5 Chapter 1.1 Oxidation and Reduction
6 Which statement exactly explains the meaning of the heat of neutralisation? star A The heat of neutralisation is the heat released when one mole of salt is formed from the reaction between an acid and an alkali B The heat of neutralisation is the heat absorbed when one mole of water is formed from the reaction between an acid and an alkali C The heat of neutralisation is the heat change when one mole of salt is formed from the reaction between an acid and an alkali D The heat of neutralisation is the heat change when one mole of water is formed from the reaction between an acid and an alkali T5 Chapter 3.2 Heat of Reaction
7 Which statement explains the effectiveness of the cleansing action of soap? star A Effective in acidic water B Less effective in hard water C Not effective in soft water T5 Chapter 5.2 Cleaning Agents
8 A calcium atom has 20 protons and its nucleon number is 40. A calcium ion, Ca^2+ is formed when a calcium atom donates 2 electrons. How many neutrons in a calcium ion, Ca^2+? star A 20 B 22 C 18 D 40 T4 Chapter 2.3 Atomic Structure
9 Noble gases are chemically unreactive due to I noble gases exist as monoatoms II noble gases have valence shells that are fully filled with electrons III noble gases have achieved a stable duplet or octet electron arrangement IV atoms of noble gases do not donate, accept or share electrons with the atoms of other elements star A I and II B II, III and IV C I, II and IV D II and IV T4 Chapter 4.3 Elements in Group 18 T4 Chapter 5.1 Basics of Compound Formation
10 Which substance has high degree of ionisation when ionises in water? star A KOH B NH_3 C HCOOH D H_2CO_3 T4 Chapter 6.3 Strength of Acids and Alkalis
11 Diagram 2 shows a steel ball bearing on the surface of the copper block using a cellophane tape, next, a weight of 1 kg is released onto the steel ball bearing. Diameter of the dent formed on the surface of the copper block is recorded. Which of the following block will form a less deep dent as compared to copper block? star A Zinc B Lead C Bronze D Iron T4 Chapter 8.1 Alloy and Its Importance
12 ### Table 1 | Hydrocarbon | Hexane | Heptane | Octane | | Boiling point | 69 °C | 98 °C | 126 °C | The boiling point of hexane is the lowest. Which statement exactly explains this phenomenon? star A The covalent bonds between hexane molecules are weaker B The covalent bonds between carbon atoms and hydrogen atoms in hexane molecules are weak C The atomic size of hexane is the smallest D Van der Waals forces between hexane molecules are weaker T5 Chapter 2.2 Homologous Series
13 Diagram 3 shows the structural of terylene. How many types of monomers are needed to produce this polymer? star A 1 B 2 C 3 D 4 T5 Chapter 4.1 Polymer
14 Discovered neutral particles, that are neutrons in the nucleus. Neutrons contribute almost half of the mass of an atom. The statements above show the information of an atomic structure model. Who are the scientists who identify this? star A J.J Thomson B Ernest Rutherford C James Chadwick D Niels Bohr T4 Chapter 2.2 The Development of the Atomic Model
15 Diagram 4 shows electric bulb which is filled with one of the elements in Group 18. What is the element? star A Helium B Neon C Krypton D Argon T4 Chapter 4.3 Elements in Group 18
16 Which of the following reagent is used to test the presence of cations in the salt? star A Sodium hydroxide B Sulphuric acid C Silver chloride D Barium chloride T4 Chapter 6.11 Qualitative Analysis
17 An alloy is a mixture of two or more elements where the main element is a metal. Scientists change the elemental composition to produce alloys with different properties. Which of the following elements are found in duralumin? star A Copper, Magnesium, Manganese B Aluminium, Carbon, Magnesium, Manganese C Aluminium, Copper, Magnesium, Manganese D Antimony, Copper, Magnesium, Manganese T4 Chapter 8.1 Alloy and Its Importance
18 Which of the following is the molecular formula for propanoic acid? star A C_4H_8O_2 B C_3H_8O C C_3H_6O D C_3H_6O_2 T5 Chapter 2.2 Homologous Series
19 Which of the following is the illustration of vulcanised rubber? star A A Figure B B Figure C C Figure D D Figure T5 Chapter 4.2 Natural Rubber
20 Chemical equation can be interpreted qualitatively and quantitatively. Which of the following is the balanced chemical equation for the following reactions? Sodium metal reacts with water to produce aqueous solution of sodium hydroxide and hydrogen gas. star A Na_2 + 2H_2O -> 2NaOH + 2H B 2Na + 2H_2O -> 2NaOH + H_2 C Na + H_2O -> NaOH + H D Na + H_2O -> NaOH + H_2 T4 Chapter 3.4 Chemical Equation T4 Chapter 4.4 Elements in Group 1
21 Ethanol, C_2H_5OH is soluble in water. Which of the following statement explains the solubility of ethanol in water correctly? star A The oxygen atom in ethanol molecule can form a hydrogen bond with the hydrogen atom from water molecule B The hydrogen atom which is bonded to carbon atom in ethanol molecule can form a hydrogen bond with the oxygen atom from water molecule C All hydrogen atoms in ethanol molecule can form a hydrogen bond with the oxygen atom from water molecule D Ethanol molecule can form Van der Waals forces with water molecule T4 Chapter 5.4 Hydrogen Bond
22 Diagram 5 shows the graph of volume of carbon dioxide gas against time for the two set experiments, I and II. Which of the following statement explains the graph in the Diagram 5 correctly? star A The quantity of reactants for set I experiment is more than set II and the rate of production of carbon dioxide gas for experiment set II is higher than set I B The quantity of reactants for set II experiment is more than set I and the rate of production of carbon dioxide gas for experiment set II is higher than set I C The quantity of reactants for both experiments are the same and the rate of production of carbon dioxide gas for experiment set I is higher than set II D The quantity of reactants for both experiments are the same and the rate of production of carbon dioxide gas for experiment set II is higher than set I T4 Chapter 7.2 Factors Affecting Rate of Reactions
23 Which statement exactly explains the following redox reaction? Cu(s) + 2AgNO_3(aq) -> Cu(NO_3)_2(aq) + 2Ag(s) star A The standard electrode potential value, Eº of Cu is more positive than Eº of Ag B Nitrate ion, NO_3^-, undergoes reduction C Copper is the oxidised substance D Silver is the oxidising agent T5 Chapter 1.1 Oxidation and Reduction
24 Diagram 6 shows the energy profile for a reaction. Which of the following explains the energy profile in Diagram 6? star A The value of activation energy is represented by II B \Delta H is represented by III C The reaction involved has a positive value of \Delta H D The total energy of reactants is represented by I T5 Chapter 3.1 Heat Change in Reactions
25 Green Technology is a technology or application developed to minimise the negative effects of harmful human activities. Green Technology is utilised in waste and wastewater management. Which of the following statement explains the reason of the treatment of leachate in solid waste disposal process? star A To prevent the pollution of underground water B To separate the solid waste C To produce a cleaner source of energy D To reduce the global warming effect T5 Chapter 5.6 Application of Green Technology in Industrial Waste Management
26 What is the number of atoms in 0.5 mol of carbon dioxide gas? [Avogadro constant = 6.02 \times 10^{23} mol^{-1}] star A 3 \times 6.02 \times 10^{23} B 0.5 \times 6.02 \times 10^{23} C 0.5 \times 3 \times 6.02 \times 10^{23} D 0.5 \times 2 \times 6.02 \times 10^{23} T4 Chapter 3.2 Mole Concept
27 Diagram 7 shows stalactites and stalagmites formed in a limestone cave. Limestone caves consist of a certain compound. The percentages of each element in the compound are recorded in the following table. | Element | Percentage (%) | | P | 40 | | Q | 12 | | R | 48 | Assume that 100 g of the limestone cave sample is used. What is the empirical formula of the compound? [Relative atomic mass: P = 40; Q = 12; R = 16] star A PQR B PQ_2R C P_2QR D PQR_3 T4 Chapter 3.3 Chemical Formula
28 Which acid contains the highest number of hydrogen ions? star A 50 cm^3 carbonic acid 1 mol dm^-3 B 50 cm^3 sulphuric acid 1 mol dm^-3 C 50 cm^3 ethanoic acid 1 mol dm^-3 D 50 cm^3 nitric acid 1 mol dm^-3 T4 Chapter 6.3 Strength of Acids and Alkalis
29 Lead(II) nitrate decomposes when heated. What is the volume of nitrogen dioxide gas is produced when 10 g of lead(II) nitrate is heated at room temperature? [Relative atomic mass: Pb = 207; N = 14; O = 16; Molar volume of gas = 24 dm^3 mol^-1 at room condition] star A 0.89 dm^3 B 1.78 dm^3 C 0.73 dm^3 D 1.45 dm^3 T4 Chapter 3.2 Mole Concept T4 Chapter 3.4 Chemical Equation T4 Chapter 6.10 Effect of Heat on Salts
30 In the presence of manganese(IV) oxide, MnO_2, hydrogen peroxide, H_2O_2 decomposes to be water and oxygen. The oxygen gas released is collected in a syringe and the volume of gas recorded at intervals of 0.5 minute. The data collected is shown in Table 2. | Time (min) | 0 | 0.5 | 1.0 | 1.5 | 2.0 | 2.5 | 3.0 | 3.5 | | Volume of gas (cm^3) | 0.0 | 5.4 | 9.5 | 12.8 | 15.0 | 16.3 | 16.5 | 16.5 | Calculate the overall rate of reaction. star A 3.70 cm^3 min^-1 B 6.52 cm^3 min^-1 C 5.50 cm^3 min^-1 D 4.71 cm^3 min^-1 T4 Chapter 7.1 Determining Rate of Reaction
31 Hydrogen gas is released when excess zinc granules are added into dilute nitric acid. The volume of hydrogen gas released is recorded at intervals of 30 seconds. The graph of volume of hydrogen gas against time is shown in Diagram 8. Calculate the rate of reaction at the 60 s? star A 0.46 cm³ s⁻¹ B 0.67 cm³ s⁻¹ C 0.31 cm³ s⁻¹ D 0.25 cm³ s⁻¹ T4 Chapter 7.1 Determining Rate of Reaction
32 The following thermochemical equation represents a metal displacement reaction. Fe(s) + CuSO_4(aq) -> FeSO_4(aq) + Cu(s) ∆H = -250 kJ mol⁻¹ Calculate the heat released when excess iron powder is added to 100 cm³ of 2 mol dm⁻³ copper(II) sulphate solution. star A 50 000 kJ B 50 kJ C 500 kJ D 5 000 kJ T5 Chapter 3.2 Heat of Reaction
33 Diagram 9 shows the structural formulae of a hydrocarbon. H H H H | | | | H-C-C-C-C-H | | | | H H H H What is the name for the hydrocarbon? star A Butane B Butene C Butyne T5 Chapter 2.4 Isomers and Naming Based on IUPAC Nomenclature
34 Which pair of monomer and polymer is correct? | | Monomer | Polymer | | A | Starch | Glucose | | B | Amino acid | Protein | | C | Styrene | Natural rubber | | D | Cellulose | Glucose | star A Starch, Glucose B Amino acid, Protein C Styrene, Natural rubber D Cellulose, Glucose T5 Chapter 4.1 Polymer
35 Diagram 10 shows the bond formed in and between water molecules. What is bond X? star A Dative bond B Covalent bond C Hydrogen bond D Ionic bond T4 Chapter 5.4 Hydrogen Bond
36 Which of the following tests are suitable to use to differentiate between alkane and alkene? I Reaction with bromine water under sunlight II Reaction with acidified potassium manganate(VII) solution III Reaction with acidified potassium dichromate(VI) solution IV Sootiness of flame star A I and II B II and III C I, II and IV D II, III and IV T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
37 Most chemical reactions involve reactants in aqueous solution. In that case, the preparation of aqueous solution with specific concentrations is very important. Standard solution is a solution with known concentration. However, sodium hydroxide is not suitable to be used for the preparation of a standard solution. Which of the following statement exactly explains this phenomenon? star A Because sodium hydroxide is alkaline B Because sodium hydroxide is hygroscopic C Because it is difficult to determine the exact mass of sodium hydroxide D Because sodium hydroxide insoluble in water T4 Chapter 6.6 Standard Solution
38 Table 3 shows standard electrode potential, Eº for lead, magnesium and iron. | System | Half-cell reaction | Eº / V | | I | Pb²⁺(aq) + 2e⁻ ⇌ Pb(s) | -0.13 | | II | Mg²⁺(aq) + 2e⁻ ⇌ Mg(s) | -2.38 | | III | Fe²⁺(aq) + 2e⁻ ⇌ Fe(s) | -0.44 | Which of the following cell notation represents the voltaic cell that produces the highest voltage? star A Fe(s) | Fe²⁺(aq) || Mg²⁺(aq) | Mg(s) B Mg(s) | Mg²⁺(aq) || Fe²⁺(aq) | Fe(s) C Mg(s) | Mg²⁺(aq) || Pb²⁺(aq) | Pb(s) D Pb(s) | Pb²⁺(aq) || Mg²⁺(aq) | Mg(s) T5 Chapter 1.3 Voltaic Cell
39 Diagram 11 shows the conversion of compound C_2H_6O into compound C_2H_4O_2. Compound C_2H_6O is a colourless liquid, easy volatile and soluble in water. Reaction between compound C_2H_6O and compound C_2H_4O_2 produces compound X. What is compound X? star A Ethyl ethanoate B Ethyl propanoate C Methyl propanoate D Propyl methanoate T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
40 Diagram 12 shows energy level for the neutralisation reaction between sodium hydroxide and hydrochloric acid. How much heat is released when 50 cm^3 of 0.1 mol dm^-3 sodium hydroxide solution is reacted with 50 cm^3 of 0.2 mol dm^-3 hydrochloric acid? star A 0.29 J B 0.57 J C 570 J D 285 J T5 Chapter 3.2 Heat of Reaction