1 Which substance is an atom? star A Neon B Hydrogen C Oxygen D Nitrogen T4 Chapter 4.3 Elements in Group 18
2 Which of the following shows deposition process? star A Naphthalene ball in cupboard becomes smaller B Bromine vapour spreads throughout gas jar C Saturated copper(II) sulfate solution turns into crystals D Iodine vapor turns into an iodine solid when it comes into contact with glass T4 Chapter 2.1 Basic Concepts of Matter
3 Which of the following statements is true regarding the modern Periodic Table of Elements? star A There are 18 periods in the Periodic Table of Elements. B The elements are arranged in ascending order of atomic mass C Elements with a proton number of 13 are placed in group 13 D Horizontal rows in the Periodic Table of Elements are called groups. T4 Chapter 4.2 The Arrangement in the Periodic Table of Elements
4 ### Diagram 4 - Arranging elements according to increasing atomic mass - Stated the Law of Octaves Who is the scientist who presented the theory as in diagram 4? star A Dmitri Mendeleev B Henry Moseley C John Newlands D Lothar Meyer T4 Chapter 4.1 The Development of the Periodic Table of Elements
5 What does chemical bond mean? star A Bonds formed when new compounds are formed. B A bond formed when an electron in an atom is transferred to an atom of another element. C A bond formed when an atom of a metal element combines with an atom of a non-metal element. D Bonds formed between atoms that transfer or share electrons to form a compound. T4 Chapter 5.1 Basics of Compound Formation
6 What ionic compounds are used in the production of fertilizer? star A Ammonium nitrate and potassium chloride B Magnesium carbonate and calcium chloride C Aluminium oxide and calcium phosphate D Iron(II) sulphate and sodium oxide T4 Chapter 6.8 Salts, Crystals and Their Uses in Daily Life
7 ### Diagram 7 What salt solution can be used to replace Pb(NO3)2 solution to produce salts that has the same solubility as salt X? star A Mg(NO3)2 B Ca(NO3)2 C Fe(NO3)2 D Cu(NO3)2 T4 Chapter 6.9 Preparation of Salts
8 Farhan added 2 cm^3 of 0.1 mol dm^-3 nitric acid into a test tube containing 2 cm^3 of 0.1 mol dm^-3 potassium hydroxide solution. Identify the salt produced and its solubility in water. star A KNO_2, Insoluble B KNO_2, Soluble C KNO_3, Insoluble D KNO_3, Soluble T4 Chapter 6.7 Neutralisation T4 Chapter 6.9 Preparation of Salts
9 ### Diagram 9 Which of the following statements explains the observation? star A Reacting particles in set A move faster B More particles of calcium carbonate are present in set B C Total surface area of calcium carbonate in set B is larger. D More reacting particles achieve low activation energy in set A T4 Chapter 7.2 Factors Affecting Rate of Reactions
10 ### Diagram 10 What is the most suitable change that can be measured by Anas to determine the rate of reaction in the experiment? star A Increase of the volume of sodium sulphate solution B Formation of barium sulphate C Change in colour of the mixture D Decrease of the concentration of sodium sulphate solution T4 Chapter 7.1 Determining Rate of Reaction T4 Chapter 7.2 Factors Affecting Rate of Reactions
11 Alloy X has the following composition: - 73% Iron - 18% Chromium - 8% Nickel - 1% Carbon What is alloy X? star A Pewter B Brass C Duralumin D Stainless steel T4 Chapter 8.1 Alloy and Its Importance
12 ### Diagram 12 What is the substance added and the new property of the glass? star A Boron oxide and aluminium oxide, High expansion coefficient B Boron oxide and aluminium oxide, Low expansion coefficient C Sodium carbonate and lead(II) oxide, High expansion coefficient D Sodium carbonate and lead(II) oxide, Low expansion coefficient T4 Chapter 8.2 Composition of Glass and Its Uses
13 A redox reaction can be represented by the following equation. X_2 + 2KBr → 2KX + Br_2 Element X is in Group 17 in the Periodic Table of Elements. What can be observed if element X is replaced with iodine? star A Brown gas is produced B No change is observed C Colourless solution is produced D Brown colour of the iodine is decolourized T4 Chapter 4.5 Elements in Group 17 T5 Chapter 1.1 Oxidation and Reduction
14 Fe²⁺ ion in solution can be converted to Fe³⁺ ions by adding zinc powder. Which of the following can replace zinc powder in this reaction? star A Bromine water B Potassium iodide solution C Potassium hexacyanoferrate(II) solution D Acidified potassium manganate(VII) solution T5 Chapter 1.1 Oxidation and Reduction
15 ### Diagram 15 What is the general formula for the carbon compound? star A CnH2n B CnH2n+1OH C CnH2n+1COOH D CnH2n+1COOCmH2m+1 T5 Chapter 2.2 Homologous Series
16 What are the values for X, Y and Z? star A X=9/2, Y=6, Z=8 B X=9, Y=3, Z=4 C X=9/2, Y=6, Z=4 D X=9, Y=6, Z=8 T4 Chapter 3.4 Chemical Equation
17 What type of reaction occurs at the hands feel cold when the disinfectant liquid containing alcohol evaporates while sanitizing the hands? star A Endothermic B Exothermic C Neutralisation D Displacement T5 Chapter 3.3 Application of Exothermic and Endothermic Reactions in Daily Life
18 ### Diagram 18 Which of the following statements correctly describes the energy level diagram in diagram 18? star A During the reaction, the temperature of the mixture decreases. B ∆H has a negative sign for chemical reactions that absorb heat from the environment. C When 1 mole of Mg reacts with 1 mole of H_2SO_4 to form 1 mole of MgSO_4 and 1 mole of H_2 gas, 467 kJ of heat energy is absorbed from the environment. D The reaction between magnesium, Mg and sulphuric acid, H_2SO_4 forms magnesium sulphate, MgSO_4 and hydrogen gas, H_2 is an exothermic reaction. T5 Chapter 3.1 Heat Change in Reactions
19 ### Diagram 19 Which of the following is the similarity between the monomer and its polymer? star A Molecular formula is C_2H_4 B Have double bond between carbon atoms C Contain carbon atom and hydrogen atom D Number of carbon atoms in the molecule T5 Chapter 4.1 Polymer
20 Which substance speeds up the coagulation of latex? star A Water B Ethanol C Ammonia solution D Ethanoic acid T5 Chapter 4.2 Natural Rubber
21 Which the following is the correct pair of glass and its use? star A Soda-lime glass B Lead crystal glass C Borosilicate glass D Fused silica glass T4 Chapter 8.2 Composition of Glass and Its Uses
22 ### Diagram 22 Which of the following properties best suits its use? star A Easy to break B Electrical insulation C Chemically inert D Resistant to thermal shock T4 Chapter 8.3 Composition of Ceramics and Its Uses
23 The following information is about an atom Q. - The number of protons is 12 - The nucleon number is 24 Which following, shows the diagram of electron arrangement for the ion Q? star A A Figure B B Figure C C Figure D D Figure T4 Chapter 2.3 Atomic Structure
24 The empirical formula of a hydrocarbon is CH_2. What is the molecular formula of the hydrocarbon? [Relative atomic mass: C = 12, H = 1; Molar mass of hydrocarbon = 56 g mol^-1] star A C_3H_6 B C_4H_10 C C_2H_4 D C_2H_6 T4 Chapter 3.3 Chemical Formula
25 A scientist has conducted a field study on a mountain. While conducting the research he found a blue rock. After studying the types of compounds that exist in the rocks, he has found an element that causes the rocks to be colored. As a chemistry student, where would you place the element in the Periodic Table of Elements? star A A B B C C D D T4 Chapter 4.7 Transition Elements
26 ### Diagram 26 Which of the following chemical compounds can form a compound that has the same chemical formula with Q atom and R atom? star A Aluminium chloride B Magnesium oxide C Iron(II) bromide D Calcium chloride T4 Chapter 3.3 Chemical Formula
27 Which of the following has the largest volume of gas at room condition? [Relative atomic mass: H=1, C=12, N=14, O=16; Molar volume: 24 dm^3 mol^-1 at room condition] star A 42 g of carbon monoxide, CO B 23 g of nitrogen dioxide, NO_2 C 17 g of ammonia, NH_3 D 12 g of steam, H_2O T4 Chapter 3.2 Mole Concept
28 ### Diagram 28 What is the average rate of reaction for the reaction above? star A 0.1375 g s^-1 B 0.0688 g s^-1 C 0.0375 g s^-1 D 0.0188 g s^-1 T4 Chapter 7.1 Determining Rate of Reaction
29 ### Diagram 29 Name the resulting compound and the oxidizing agent Q used. star A Ethene, Acidified potassium dichromate(VI) B Ethene, Potassium hexacyanoferrate(II) C Ethanoic acid, Acidified potassium manganate(VI) D Ethanoic acid, Potassium thiocyanate T5 Chapter 1.1 Oxidation and Reduction T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
30 ### Diagram 30 Which equation occurs at the anode? star A Fe → Fe^2+ + 2e B O_2 + 2H_2O + 4e → 4OH^- C Fe^2+ + 2OH^- → Fe(OH)_2 D 4Fe + 3O_2 + 2xH_2O → 2Fe_2O_3.xH_2O T5 Chapter 1.3 Voltaic Cell
31 ### Diagram 31 | Bond | Energy Bond (kJ mol^-1) | | H-H | 436 | | Cl-Cl | 243 | | H-Cl | 432 | Calculate the X and Y values. star A X=679 kJ, Y=864 kJ B X=486 kJ, Y=432 kJ C X=185 kJ, Y=864 kJ D X=679 kJ, Y=185 kJ T5 Chapter 3.1 Heat Change in Reactions
32 A student has conducted an experiment to determine the heat of displacement for the reaction between copper, Cu and silver nitrate solution, AgNO_3. In this experiment, excess copper powder was added to 100 cm^3 of argentum nitrate solution, AgNO_3 0.5 mol dm^-3. The heat of displacement in the experiment is - 105 kJ mol^-1. Calculate the temperature change for the reaction. [Specific heat capacity = 4.2 J g^-1 °C^-1] star A 12.5 °C B 10.5 °C C 6.25 °C D 5.25 °C T5 Chapter 3.2 Heat of Reaction
33 ### Table 33 | Ion | Number of electrons | Number of neutrons | | W^+ | 10 | 12 | | X^- | 10 | 10 | | Y^2+ | 10 | 12 | | Z^2- | 10 | 8 | Which of the following shows the correct nucleon number of the ion? star A W^+, 21 B X^-, 19 C Y^2+, 18 D Z^2-, 20 T4 Chapter 2.3 Atomic Structure
34 ### Diagram 34 What is the volume of oxygen gas needed to react completely in this reaction? [Molar volume of gas at room conditions = 24 dm^3 mol^-1] star A 1.2 dm^3 B 2.2 dm^3 C 2.4 dm^3 D 4.8 dm^3 T4 Chapter 3.2 Mole Concept T4 Chapter 3.4 Chemical Equation
35 Decomposition of potassium chlorate(V) KClO_3 by heat produce potassium chloride and oxygen gas. This method is often used to produce oxygen gas in the laboratory. Assume you are a laboratory assistant. Calculate the mass of potassium chlorate(V) KClO_3 is needed to produce 48000 cm^3 oxygen gas in room condition? [Relative atomic mass: O = 16, Cl = 35.5, K = 39; Molar volume = 24 dm^3 mol^-1 at room condition] star A 2000.000 g B 666.670 g C 245.000 g D 162.925 g T4 Chapter 3.2 Mole Concept T4 Chapter 3.4 Chemical Equation
36 Reaction between sulphuric acid with 9.0 g of copper(II) oxide powder produce copper(II) sulphate and water. What is the mass of copper(II) oxide that does not react if 50 cm^3 0.5 mol dm^-3 sulphuric acid is used? [Relative atomic mass; O = 16, S = 32, Cu = 64] star A 2.00 g B 7.00 g C 9.00 g D 11.00 g T4 Chapter 3.2 Mole Concept T4 Chapter 3.4 Chemical Equation T4 Chapter 6.5 Concentration of Aqueous Solution
37 ### Table 37 | Type of acid | Concentration / mol dm^-3 | pH value | | Hydrochloric acid | 0.1 | 1 | | Ethanoic acid | 0.1 | 4 | Which of the following statements are true about both acids? I Hydrochloric acid is a weak acid while ethanoic acid is strong acid II Concentration of hydrogen ions is higher in hydrochloric acid compared with ethanoic acid. III The degree of dissociation of hydrochloric acid in water is lower than ethanoic acid. IV Both acids can neutralized an alkali to produce salt and water star A I and II B I and III C II and IV D III and IV T4 Chapter 6.2 pH Value T4 Chapter 6.3 Strength of Acids and Alkalis T4 Chapter 6.7 Neutralisation
38 ### Diagram 38 What is the reaction at copper electrod X and observation at copper electrode Y in the experiment? star A Oxidation, Thinner B Oxidation, Ticker C Reduction, Thinner D Reduction, Thicker T5 Chapter 1.4 Electrolytic Cell
39 ### Diagram 39 C_2H_5OH (l) + 3O_2 (g) -> 2CO_2(g) + 3H_2O (l) ΔH = -1376 kJ mol^-1 Calculate the mass of ethanol, C_2H_5OH needed to burn completely in excess oxygen, O_2 in order to raise the temperature of water by 50.0 °C. (Assume that no heat is lost to the surroundings) [Specific heat capacity = 4.2 J g^-1 °C^-1; Density of water = 1 g cm^-3; Molar mass of ethanol = 46 g mol^-1] star A 0.03 g B 1.38 g C 32.76 g D 46.00 g T5 Chapter 3.2 Heat of Reaction
40 ### Diagram 40 Which of the following combination of conditions take the shortest time for the mark X to disappear from sight? star A Sulphuric acid: 20 cm³, 0.5 mol dm⁻³; Sodium thiosulphate: 40 cm³, 0.5 mol dm⁻³; Temperature: 40 °C B Sulphuric acid: 10 cm³, 0.5 mol dm⁻³; Sodium thiosulphate: 50 cm³, 0.5 mol dm⁻³; Temperature: 30 °C C Sulphuric acid: 10 cm³, 1.0 mol dm⁻³; Sodium thiosulphate: 50 cm³, 0.5 mol dm⁻³; Temperature: 30 °C D Sulphuric acid: 10 cm³, 1.0 mol dm⁻³; Sodium thiosulphate: 50 cm³, 0.5 mol dm⁻³; Temperature: 40 °C T4 Chapter 7.2 Factors Affecting Rate of Reactions