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UK GCSE 2006 : Higher Tier, Chemistry Paper 1

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Centre Number 71 Candidate Number General Certificate of Secondary Education 2006 Paper 1 Higher Tier G1403 Science: Chemistry [G1403] WEDNESDAY 14 JUNE, MORNING TIME 1 hour 30 minutes. INSTRUCTIONS TO CANDIDATES Write your Centre Number and Candidate Number in the spaces provided at the top of this page. Write your answers in the spaces provided in this question paper. Answer all five questions. INFORMATION FOR CANDIDATES The total mark for this paper is 120. Quality of written communication will be assessed in question 5(a)(ii). Figures in brackets printed down the right-hand side of pages indicate the marks awarded to each question or part question. A Data Leaflet which includes a Periodic Table of the Elements is provided. For Examiner s use only Question Number 1 2 3 4 5 Total Marks G141H6 876 Marks BLANK PAGE G141H6 876 2 [Turn over 1 Magnesium metal does not occur uncombined in nature. It was first isolated by Sir Humphrey Davy in 1808 by passing an electric current through molten magnesium chloride. Copper metal does occur in nature and has been known for thousands of years. Examiner Only Marks Remark (a) Explain why magnesium metal does not occur uncombined in nature but copper metal does. _________________________________________________________ ______________________________________________________ [2] (b) Copper and magnesium are typical metals and show similar physical properties. Both conduct electricity and copper s use in electrical wiring is also due to the fact that it is ductile. (i) What is meant by the term ductile? ______________________________________________________ ___________________________________________________ [1] (ii) Explain why metals conduct electricity. ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] (iii) Give two other physical properties of metals. 1. _________________________________________________ [1] 2. _________________________________________________ [1] G141H6 876 3 [Turn over (c) Compounds of copper vary in their colour. Examiner Only Marks Remark Complete the table below, giving the colour of the substances listed. Substance Colour copper(II) carbonate [2] copper(II) sulphate solution (d) Magnesium metal burns in air with a bright white flame as shown below. Source: http//www.uncp.edu/home/mcclurem/ptable/mg_2.jpg The product of the reaction is mainly magnesium oxide with about 10% magnesium nitride. (i) Describe the appearance of magnesium oxide. ___________________________________________________ [2] (ii) Write a balanced symbol equation for the formation of the magnesium oxide. ___________________________________________________ [3] (iii) Give the formula of magnesium nitride. ___________________________________________________ [1] G141H6 876 4 [Turn over (e) Magnesium metal reacts with dilute hydrochloric acid. Examiner Only Marks Remark (i) What would you observe when magnesium reacts with dilute hydrochloric acid? ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] (ii) Write a balanced symbol equation for the reaction between magnesium and dilute hydrochloric acid. ___________________________________________________ [3] (iii) Name one other metal which reacts safely with dilute hydrochloric acid. ___________________________________________________ [1] G141H6 876 5 [Turn over 2 Sodium thiosulphate solution, Na2S2O3(aq), reacts with dilute hydrochloric acid according to the following equation: Examiner Only Marks Remark Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + S(s) + SO2(g) + H2O(l) The diagram below shows the apparatus used to investigate the effect of changing the concentration of sodium thiosulphate solution on the rate of this reaction. Look down at cross from above white paper reactants cross A precipitate is produced which causes the solution to become cloudy. The rate of this reaction can be investigated by timing how long it takes for the cross drawn on the white paper to disappear from view. (a) Which product causes the solution to become cloudy? ______________________________________________________ [1] G141H6 876 6 [Turn over (b) A series of experiments carried out to investigate the effect of concentration of sodium thiosulphate solution on the rate of reaction produced the following results: Concentration of sodium thiosulphate solution (mol/dm3) Time taken for cross to disappear (s) Rate of reaction (s 1) 1 time 1 0.4 105 0.0095 2 0.8 79 0.0127 3 1.2 54 0.0185 4 1.6 32 Experiment ( ) Examiner Only Marks Remark (i) State two precautions which should be taken to ensure a fair test. ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] (ii) Calculate the rate of reaction for experiment 4 and insert the value into the results table. [1] (iii) From the results of the experiments, state the effect of increasing the concentration of sodium thiosulphate solution on the rate of the reaction. ______________________________________________________ ___________________________________________________ [1] G141H6 876 7 [Turn over (iv) Explain, as fully as possible in terms of particles, how an increase in concentration of sodium thiosulphate solution has this effect on the rate of reaction. Examiner Only Marks Remark ______________________________________________________ ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [4] (v) Name two other factors apart from concentration of sodium thiosulphate solution that will affect the rate of this reaction. 1. ____________________________________________________ 2. _________________________________________________ [2] (c) The Haber Process is used to produce ammonia in industry. (i) Write a balanced symbol equation for this reaction. ___________________________________________________ [3] G141H6 876 8 [Turn over The amount of ammonia gas produced (% yield) from this reaction is affected by both the temperature and the pressure at which the process is carried out. The graph below shows how the amount of ammonia produced from the reaction changes with both temperature and pressure. 60 350 C 55 50 % yield of ammonia 45 40 450 C 35 30 25 550 C 20 15 10 5 0 0 50 100 150 200 250 300 350 400 450 Pressure (atm) Examiner Only Marks Use the graph to answer the following questions. Remark (ii) What happens to the percentage yield of ammonia if the pressure is increased at constant temperature? ___________________________________________________ [1] (iii) State the temperature and pressure at which the greatest yield of ammonia gas is produced. Temperature ___________ C [1] Pressure [1] ___________ atm (iv) The conditions usually used in the production of ammonia are a temperature of 450 C and a pressure of 200 atmospheres. What is the percentage yield of ammonia using these conditions? ___________________________________________________ [1] G141H6 876 9 [Turn over (v) Suggest two reasons why industry compromises by using these conditions when it is possible to obtain a higher yield of ammonia using a lower temperature and a higher pressure. Examiner Only Marks Remark ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] G141H6 876 10 [Turn over 3 Organic compounds are used in medicine and first aid. Examiner Only Marks Remark (a) One of the first anaesthetics to be used in surgery was ethene. However, ethene is flammable and halothane, CF3CHBrCl, is now used instead. (i) Draw the structural formula of ethene. [2] (ii) Describe a chemical test which could be used to show that ethene is unsaturated. Give the observations which would occur. Test: _______________________________________________ [1] Observations: __________________________________________ ___________________________________________________ [2] (iii) Explain why halothane is not a hydrocarbon. ______________________________________________________ ___________________________________________________ [1] (iv) Write a balanced symbol equation for the burning of ethene in excess air. ___________________________________________________ [3] (v) At room temperature and pressure, what is the physical state of ethene? ___________________________________________________ [1] G141H6 876 11 [Turn over (b) Hip and shoulder joints which have been damaged by arthritis can be replaced during surgery by a metal bone which fits into a polythene cup. Polythene is a polymer made from ethene. Examiner Only Marks Remark (i) State one property of polythene which makes it suitable for this use. ___________________________________________________ [1] (ii) What is meant by the term polymer? ______________________________________________________ ___________________________________________________ [2] (iii) Draw the structure of polythene. [2] (c) Surgical spirit is used to sterilise surfaces and to cleanse cuts in the skin. It contains ethanol and a small amount of methanol. (i) Draw the structural formula of ethanol. [2] G141H6 876 12 [Turn over (ii) The ethanol in surgical spirit is produced in industry from ethene. Write a balanced symbol equation for the production of ethanol from ethene. Examiner Only Marks Remark ___________________________________________________ [2] (iii) Alcoholic drinks also contain ethanol, which is produced by fermentation. Explain the process of fermentation. ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] (d) In first aid ethanoic acid is used to treat wasp stings which are alkaline. (i) Draw the structural formula of ethanoic acid. [2] (ii) State another use of ethanoic acid. ___________________________________________________ [1] (iii) Ethyl ethanoate is formed when ethanoic acid reacts with ethanol. Draw the structural formula of ethyl ethanoate. [2] G141H6 876 13 [Turn over BLANK PAGE G141H6 876 14 [Turn over 4 (a) Hydrochloric acid reacts with zinc hydroxide and potassium hydroxide. These reactions produce salts. Zinc hydroxide is a base. Potassium hydroxide is an alkali. Examiner Only Marks Remark (i) Name one other base. ___________________________________________________ [1] (ii) What is meant by the term alkali? ___________________________________________________ [2] (b) Zinc hydroxide acts as a base with hydrochloric acid. However, it also reacts with alkalis like potassium hydroxide. (i) What term is used for substances like zinc hydroxide which react with both acids and alkalis? ___________________________________________________ [1] (ii) Name one other metal hydroxide which behaves in this way. ___________________________________________________ [1] (iii) Write balanced symbol equations for the reactions between: (1) zinc hydroxide and hydrochloric acid; ________________________________________________ [3] (2) zinc hydroxide and potassium hydroxide. ________________________________________________ [3] G141H6 876 15 [Turn over (c) The reaction between zinc carbonate and hydrochloric acid produces the salt zinc chloride. The diagram below details how pure, dry crystals of zinc chloride may be produced. Measure 25 cm3 of dilute hydrochloric acid and place in a conical flask Add zinc carbonate to the hydrochloric acid until it is in excess Filter the solution Heat the filtered solution to make it more concentrated Leave aside to cool and crystallise Filter crystals from solution Dry the crystals G141H6 876 16 [Turn over (i) What piece of apparatus would you use to measure 25 cm3 of hydrochloric acid? Examiner Only Marks Remark __________________________________________________ [1] (ii) Explain why the zinc carbonate is added until it is in excess. _____________________________________________________ __________________________________________________ [1] (iii) Give one way in which you would know the zinc carbonate is in excess. _____________________________________________________ __________________________________________________ [1] (iv) What is the general name given to the solid trapped by the filter paper? __________________________________________________ [1] (v) What is the general name given to the filtered solution? __________________________________________________ [1] (vi) Explain why crystals form as the solution is cooled. _____________________________________________________ _____________________________________________________ __________________________________________________ [2] (vii) Give two methods of drying the crystals. 1. ___________________________________________________ 2. ________________________________________________ [2] G141H6 876 17 [Turn over (d) Zinc chloride consists of zinc ions and chloride ions. The table below describes a chemical test for zinc ions. Examiner Only Marks Remark Zinc ions Test add sodium hydroxide solution to a solution of zinc chloride Observations (i) Complete the table giving the observations for the test for zinc ions. [2] (ii) Write a balanced ionic equation for the reaction between the zinc ions in zinc chloride and the hydroxide ions in sodium hydroxide. ___________________________________________________ [3] G141H6 876 18 [Turn over 5 (a) The table below gives some information about the elements calcium and oxygen. (i) Complete the table. Element Atomic Atomic number number Calcium Oxygen Electronic arrangement Atom Ion Symbol Atom Ca2+ 2,8,8,2 8 Ion 2,8 Examiner Only Marks Remark [6] (ii) Calcium atoms react with non-metal atoms like oxygen to form calcium ions. Explain in terms of electrons, what happens when atoms of calcium form calcium ions. ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] Quality of written communication [2] (iii) Oxygen has two isotopes. Explain what is meant by the term isotope. ______________________________________________________ ___________________________________________________ [2] (iv) Atoms of oxygen, like most atoms, contain protons, neutrons and electrons. Complete the table below for each type of particle. Particle Relative charge Relative mass Number in one atom of 16O 8 Electron Neutron Proton [3] G141H6 876 19 [Turn over (v) The bonding in calcium is metallic. Explain what is meant by metallic bonding. You may use a labelled diagram to help answer this question. Examiner Only Marks Remark ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] (vi) Explain why metals like calcium are malleable. ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] G141H6 876 20 [Turn over (b) The diagram shows an atom of an element X, where: Examiner Only Marks Remark e represents an electron; n represents a neutron; and p represents a proton. ee ee 6n 5p e (i) Name the element X. __________________________ [1] (ii) State the Group to which element X belongs. __________________________ [1] (iii) What is the mass number of this atom of element X? __________________________ [1] (iv) Name the part of the atom which is shaded grey. __________________________ [1] G141H6 876 21 [Turn over THIS IS THE END OF THE QUESTION PAPER G141H6 876 22 [Turn over [Turn over Permission to reproduce all copyright material has been applied for. In some cases, efforts to contact copyright holders may have been unsuccessful and CCEA will be happy to rectify any omissions of acknowledgement in future if notified. S 5/05 5300 302507(33)

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