2024 Fuhua Sec 4E Chemistry P1

Candidate Name: Class: Index No.: FUHUA SECONDARY SCHOOL Secondary Four Express PRELIMINARY EXAMINATION 2024 4E Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School Fuhua Secondary School CHEMISTRY 6092/01 Paper 1 Multiple Choice Additional Material: Optical Mark Recognition (OMR) DATE 28 August 2024 TIME 0800 – 0900 DURATION 1 hour READ THESE INSTRUCTIONS FIRST Write in soft pencil. Do not use staples, paper clips, glue or correction fluid. Write your name, class, index number on the OMR and this question booklet. There are forty questions on this paper. Answer all questions. For each question, there are four possible answers A, B, C and D. Choose the one you consider correct and record your choice in soft pencil on the separate OMR. Each correct answer will score one mark. A mark will not be deducted for a wrong answer. Any rough working should be done on this paper. A copy of the Periodic Table is printed on page 15. The use of an approved scientific calculator is expected, where appropriate. FOR EXAMINER’S USE PARENT’S SIGNATURE 40 Setter: Mr Nicholas Liu Vetter: Mdm Hia Soo Ching This document consists of 15 printed pages, including this page.

2 1 Nitrogen dioxide gas is almost twice as dense as nitrogen gas. A gas jar of nitrogen dioxide was placed on top of a gas jar of nitrogen gas with the open ends together. After half an hour, which of these statements would be true? A Both gases would not have mixed. B The bottom gas jar contained nitrogen gas only. C The top gas jar contained nitrogen dioxide gas only. D Some of each gas would have moved into the other gas jar. 2 The diagram shows the apparatus used to separate hexane (boiling point 70oC) and water. Which graph would be obtained if the temperature at point T was plotted against the total volume of distillate collected? 70 80 90 100 temperature/°C total volume of distillate 70 80 90 100 temperature/°C total volume of distillate C 70 80 90 100 temperature/°C Total volume of distillate D 70 80 90 100 temperature/°C total volume of distillate A B T

3 3 A student titrated 25.0 cm3 of sodium hydroxide with hydrochloric acid. The diagram shows the volume of hydrochloric acid in the burette at the start and the end of the titration. What volume of hydrochloric acid was added from the burette? A 29.00 cm3 B 29.60 cm3 C 31.30 cm3 D 32.70 cm3 4 The formulae of the ions of some elements are shown below: P3- S2- Cl- Li+ Mg2+ Which of the following statements about these ions is correct? A They all have more electrons than protons. B They all have the same number of electron shells. C They all have the same number of neutrons in their nuclei. D They all have the same electronic structures as noble gases. 5 Ethanol has the structure shown. How many of the electrons in a molecule of ethanol are not involved in bonding? A 4 B 6 C 8 D 10

4 6 J, K and L are three different elements in the Periodic Table. The ‘dot and cross’ diagram (showing only the valence electrons) of the compound formed between J, K and L is shown: Which of the following statements is/are correct? 1 Element L is hydrogen. 2 Element J belongs to Group 2 of the Periodic Table. 3 Elements J, K and L are bonded together by ionic bonds only. A 1 only B 1 and 2 C 2 and 3 D 3 only 7 Elements X and Y form an ionic compound of formula X3Y. What could the atomic numbers of X and Y be? X Y A 3 1 B 8 4 C 11 7 D 13 9 8 Magnesium oxide has a similar structure to that of sodium chloride. Which of the following statements is true? A Magnesium oxide has a lower melting point than sodium chloride. B Magnesium oxide and sodium chloride can conduct electricity in the molten state only. C In a lattice structure, each magnesium ion is surrounded by six oxide ions while each oxide ion is surrounded by six magnesium ions. D When magnesium reacts with oxygen, every mole of magnesium atoms loses a mole of electrons. Likewise, every mole of oxygen molecules loses a mole of electrons. 9 Which of the following reactions shows the amphoteric property of zinc oxide? A 2ZnO + C → 2Zn + CO2 B ZnO + Mg → MgO + Zn C ZnO + 2HCl → ZnCl2 + 2H2O D ZnO + 2NaOH → Na2ZnO2 + H2O

5 10 The following statements about dilute sulfuric acid are all correct. 1 It reacts with copper(II) oxide, forming a blue solution. 2 It turns anhydrous copper(II) sulfate from white to blue. 3 A white precipitate is formed when aqueous barium nitrate is added. 4 Addition of methyl orange shows that the solution has a pH value of less than 4.0. Which two statements confirm the acidic nature of the solution? A 1 and 2 B 1 and 4 C 2 and 3 D 3 and 4 11 A titration method can be used to prepare aqueous potassium sulfate from potassium carbonate and dilute sulfuric acid. Which of the following conclusions from this information is correct? A Potassium carbonate is an acidic salt. B Potassium carbonate is insoluble in water. C Potassium carbonate neutralises dilute sulfuric acid. D Potassium carbonate reacts more vigorously than sodium carbonate with dilute sulfuric acid. 12 Solid X is gradually added to aqueous solution Y. The changes in pH are shown in the graph below. What could X and Y be? X Y A potassium carbonate ethanoic acid B potassium oxide ethanoic acid C sodium oxide hydrochloric acid D zinc oxide hydrochloric acid 14 0 7 pH mass of solid X added/ g

6 13 An aqueous solution, Z, contains one cation and two anions. Some tests were carried out on the solution to determine the possible identities of the ions present. The observations of the tests carried out are recorded as follows: Test 1 White precipitate forms when aqueous barium nitrate is added to solution Z. Test 2 When solution Z is heated with aqueous sodium hydroxide and aluminium, a gas that turns moist red litmus blue is evolved. Test 3 No visible change is observed when dilute hydrochloric acid is added to solution Z. Which ions are likely to be present in solution Z? A Al3+, Cl-, SO42- B Al3+, NO3-, SO42- C Pb2+, NO3-, SO42- D Pb2+, Cl-, NO3- 14 G is a white powder that turns yellow upon heating and gives off a colourless gas which is slightly soluble in water to produce a solution with pH less than 7. The residue reacts with dilute nitric acid and the aqueous solution formed white precipitate that is soluble in excess aqueous ammonia. Which of the following could be the identity of G? A aluminium carbonate B aluminium oxide C zinc carbonate D zinc oxide 15 One mole of a sample of hydrated sodium sulfide contains 162 g of water of crystallisation. What is the correct formula of this compound? A Na2S.3H2O B Na2S.5H2O C Na2S.7H2O D Na2S.9H2O 16 When solid sodium hydrogencarbonate is heated strongly, the following reaction occurs. 2NaHCO3 (s) → Na2CO3 (s) + H2O (g) + CO2 (g) What is the loss in mass when 33.6 g of solid sodium hydrogencarbonate is heated? A 10.8 g B 12.4 g C 21.2 g D 24.6 g 17 1.36 g of aqueous solution XC l2 reacts wit