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IGCSE Chemistry Past Paper Discussion

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Published in: Chemistry
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Discussed the EdExcel - IGCSE Chemistry Paper Completely

Salman F / Doha

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Qualification: Post Graduate in Chemistry, BSc in Chemistry, MS in Chemistry, Bachelors degree in Education

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  1. Please check the examination details below before entering your candidate information Candidate surname Centre Number Other names Candidate Number Pearson Edexcel International GCSE (9-1 ) Tuesday 14 November 2023 Morning (Time: 2 hours) Chemistry UNIT: 4CH1 Paper 4CH1/1C 4SDO/1C reference Science (Double Award) 4SDO PAPER: IC Instructions • Use black ink or ball-point pen. • Fill in the boxes at the top of this page with your name, centre number and candidate number. • Answer all questions. • Answer the questions in the spaces provided - there may be more space than you need. • Show all the steps in any calculations and state the units. Information • The total mark for this paper is 110. • The marks for each question are shown in brackets - use this as a guide as to how much time to spend on each question. Advice • Read each question carefully before you start to answer it. • Write your answers neatly and in good English. • Try to answer every question. • Check your answers if you have time at the end. P73423A •2023 4 2 3 'N C) 128 Turn over Pearson
  2. The Periodic Table of the Elements 14 16 He 20 Ne 23 11 Be Mg 12 relative atomic mass atomic symbol atomic (proton) number 11 12 eeeeaa eeeeeeeeaeeeaeaeee eeeeeeeeeeaeeaeaea aeeeaaaaaeaeeeeeee [223] 87 [226] 88 [227] 89 [2611 104 [262] Db 105 [2661 sg 106 [2641 107 [277] Hs 108 [2681 109 [2721 [271] 110 111 Elements with atomic numbers 112—116 have been reported but not fully The lanthanoids (atomic numbers 58—71) and the actinoids (atomic numbers 90—103) have been omitted. The relative atomic masses of copper and chlorine have not been rounded to the nearest whole number. vauv SIU NI ION oa vauv NI ION oa authenticated vauv SIHI NI ION oa
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  4. Answer ALL questions. Some questions must be answered with a cross in a box X. If you change your mind about an answer, put a line through the box and then mark your new answer with a cross X. 1 A substance can exist in three states of matter, solid, liquid or gas. When a liquid evaporates at room temperature it changes into a gas. (a) Complete the diagram to show the arrangement of another four particles in a gas. o (b) Explain why heating a liquid causes it to evaporate more quickly. (c) When the temperature decreases, water in the gas state changes to a liquid. (i) Give the name of this change of state. (ii) Write an equation, including state symbols, to show the change of state of water from a gas to a liquid. 4 p 73 4 2 3 'N e 428 (1) (2) (1) z O z z o z O
  5. (d) Describe the arrangement and movement of particles in a solid. (2) (Total for Question 1 = 7 marks) Turn over p 73 4 2 3 'N e 528
  6. 2 (a) Table 1 shows some relative masses and charges of subatomic particles. Complete table 1 by giving the missing information. (2) Neutron Electron 0.0005 Proton Relative mass Relative charge Table 1 (b) Table 2 gives the number of protons, neutrons and electrons in atoms and ions of some elements. The letters are not the symbols of the elements. Atom or ion Protons Neutrons Electrons 10 Table 2 (i) What is the atomic number of P in table 2? p 73 4 2 3 'N e 628
  7. (ii) What is the mass number of U in table 2? A c D 8 16 18 26 (1) May-a z z z z o z z (c) (iii) Give the letter in table 2 that represents an element in Group 5 of the Periodic Table. (1) Q and R represent isotopes of the same element. Explain, in terms of subatomic particles, why Q and R are isotopes. (2) A sample containing the isotopes Q and R has this percentage composition by mass. Q = 20.6% •p R = 79.4% Calculate the relative atomic mass (A) of this sample of the element. Give your answer to one decimal place. (3) (Total for Question 2 = 10 marks) p 73 42 3 7 Turn over
  8. 3 Crude oil is an important source of organic compounds. (a) The diagram shows how crude oil can be separated into useful mixtures of hydrocarbons. x crude oil (i) Give the name of this method of separation. (ii) State what happens to the crude oil when it is in X. (iii) Give the letter of the mixture that is most likely to contain a hydrocarbon with six carbon atoms. (iv) Give the name of mixture D. (v) Give a use for mixture B. 8 p 73 4 2 3 'N e 828 (1) (1) (1) (1) z O z z o z O
  9. (b) Explain, in terms of intermolecular forces, why a hydrocarbon in mixture B has a higher boiling point than a hydrocarbon in mixture D. (c) Catalytic cracking can be used to break down long-chain hydrocarbons to produce shorter-chain alkanes and alkenes. (i) Give the name of a catalyst used in catalytic cracking. z-ao--Q-R (ii) Complete the equation to show two different alkenes that could be produced in this cracking reaction. C15H32 C8H18 + (iii) Give one important use for short-chain alkenes. (Total for Question 3 = 12 marks) p 73 42 3 A e 928 (3) (1) (2) Turn over
  10. 4 This question is about gases. (a) The table gives information about five gases. Name of gas Formula of gas Mr of gas argon 40 carbon hydrogen dioxide C02 2 oxygen 02 32 Use information from the table to answer these questions. Each gas may be used once, more than once or not at all. (i) Give the name of the gas that is about 79% of the atmosphere by volume. 2- (ii) Give the name of the gas that is a compound. (iii) Give the name of the least reactive gas. (iv) Give the name of the gas that is not normally found in the atmosphere. (v) Give the name of the gas that affects global warming. (vi) Calculate the Mr for carbon dioxide. (vii) Give a reason why it is not possible to give information for air in the table. (1) p 73 28 nitrogen 28 (1) (1) (1) (1) (1) (1) z O z z o z O 10
  11. (b) When copper(ll) carbonate is heated, the products are copper(ll) oxide and carbon dioxide. (i) Give the name for this type of reaction. (1) (ii) Give the colour change that occurs during this reaction. to (iii) Give a chemical equation for this reaction. (Total for Question 4 = 11 marks) p 73 423 e I (2) (1) 11 Turn over
  12. This question is about alkanes and alkenes. 5 (a) The alkane C4H10 exists as two isomers. (i) State what is meant by the term isomers. (ii) Draw the displayed formulae for the two isomers of C4H10 Isomer 1 —9 (b) Ethane (C2H6) can react with bromine. (i) State the condition needed for ethane to react with bromine. (ii) Complete the equation for this reaction. C2H6 + (iii) Give the name for this type of reaction. 12 p 73 423 A e 12 28 Isomer 2 (2) (2) (1)
  13. (c) Explain why ethane is described as a saturated compound. (2) (d) State what you would observe when ethane and ethene are added separately to two samples of bromine water. (2) ethane ethene (e) Explain why straight-chain alkenes always have the same empirical formula, but straight-chain alkanes have different empirical formulae. Refer to the molecular formulae of the alkanes C2H6 and C4H10 in your answer. (3) 13 Turn over p 73 28
  14. (f) An organic compound has this percentage composition by mass. C = 19.2% H = 4.0% 64.0% Calculate the empirica formula of this compound. (3) empirical formula = (Total for Question 5 = 17 marks) 14 p 73 28
  15. 6 A student uses this apparatus to investigate the decomposition of z z z z o z z hydrogen peroxide solution. 2 hydrogen peroxide solution 40 60 80 100 oxygen 00 0 manganese(lV) oxide This is the equation for the reaction. 214202 21420 + 02 a) Give the test for oxygen. ) Complete the dot-and-cross diagram for a molecule of hydrogen peroxide. Show outer electrons only. H o (1) (2) 15 Turn over p 73 28
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  17. (d) (i) Explain in terms of particle collision theory how decreasing the concentration affects the rate of a reaction. (ii) The student repeats the experiment using the same volume of hydrogen peroxide solution but with half the original concentration. All other conditions are kept the same. On the grid, draw the curve you would expect the student to obtain. (e) In this reaction, the manganese(lV) oxide acts as a catalyst. Explain how a catalyst works. (Total for Question 6 = 12 marks) p 73 423 A 2 (3) (2) (2) 17 Turn over
  18. 7 (a) A technician needs to identify the solution in an unlabelled bottle. The technician knows that the solution contains one of these compounds. iron(ll) bromide iron(ll) chloride iron(lll) bromide iron(lll) chloride Describe how the technician can use chemical tests to identify the compound. 18 p 73 423 A e 18 28
  19. (b) When chlorine gas is passed over heated iron powder, iron(lll) chloride forms. This is the equation for the reaction. 2Fe + 3C12 + 2FeC13 0.060 mol of chlorine gas is passed over 2.8g of iron powder. Show by calculation that the iron powder is in excess. (c) When iron(lll) chloride dissolves in water, an acidic solution forms. (i) Give the colour of litmus in this solution. (ii) Give the formula of the ion that causes the solution to be acidic. (3) (1) (Total for Question 7 = 11 marks) 19 Turn over p 73 423 28
  20. 8 Diamond and graphite are made of carbon atoms, joined together by covalent bonds. The diagram shows their structures. diamond graphite (a) State, in terms of electrostatic attractions, what is meant by a covalent bond. (2) (b) Explain why diamond has a high melting point. (3) (c) Explain why graphite is a good conductor of electricity. (2) 20 p 73 4 2 3 'N e 2 e 28
  21. (d) C60 fullerene is a molecule made of 60 carbon atoms. The diagram shows the structure of fullerene. One mole of atoms contains 6.0 x 1023 atoms. Determine the number of atoms in one mole of C60 fullerene. Give your answer in standard form. (2) number of atoms = (Total for Question 8 = 9 marks) Turn over p 73 423
  22. 9 A scientist uses this apparatus in an experiment to reduce a metal oxide to a metal. metal oxide hydrogen heat hydrogen burning tube Before heating the mass of the empty tube and the mass of the tube and the metal oxide are recorded. After heating, the tube is allowed to cool and the mass of the tube and its contents is recorded again. (a) (i) State why the reaction of the metal oxide to form a metal is described as a reduction reaction. (1) (ii) State why it is important to relight the hydrogen at the end of the tube if the flame goes out. (1) (iii) Explain why it is important to continue passing hydrogen into the tube and burning the hydrogen at the end of the tube until the contents have cooled. (2) 22 p 73 423 z O z z o z O
  23. z z o z z o z z (iv) Describe what should be done next to ensure that all the metal oxide has been converted into the metal. (b) In this experimenta mass of 4.14g of metal is formed from 4.46g of the metal oxide. Calculate the amount, in moles, of oxygen atoms in the sample of the metal oxide. amount of oxygen atoms = The formula of the metal oxide is MO, where M represents the symbol of (i ii) (iv) the metal. Deduce the amount, in moles, of M in the sample of the metal oxide. amount of M = Calculate the relative atomic mass of M. relative atomic mass of M = Use the Periodic Table to identify metal M. (Total for Question 9 = 12 marks) Turn over p 73 4 2 3 'N e 2328 (2) (2) mol (1) mol (2) (1)
  24. 10 This method is used in an experiment to produce hydrated zinc nitrate crystals. pour 50 cm3 of dilute nitric acid into a beaker add a spatula of zinc powder to the acid add more zinc until it is in excess filter the mixture obtain crystals of zinc nitrate from the filtrate (a) State why the mixture is filtered. (1) (b) Describe how a pure, dry sample of hydrated zinc nitrate crystals could be obtained from the filtrate. (4) p 73 4 2 3 'N e 2 428
  25. (c) This equation represents the formation of hydrated zinc nitrate in the experiment. zn(s) + 2HN03(aq) + 6H20(l) + + H2(g) (i) In another experiment, 9.75g of zinc is completely reacted with nitric acid. Show that the maximum possible mass of hydrated zinc nitrate crystals that could be formed is approximately 45 g. [for Zn(N03b.6H20, Mr = 297] (2) (ii) The actual yield of hydrated zinc nitrate crystals is 36.4 g. Calculate the percentage yield of hydrated zinc nitrate crystals. (2) percentage yield = (Total for Question 10 = 9 marks) TOTAL FOR PAPER = 110 MARKS 25 p 73 4 2 3 'N e 2528
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