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UK GCSE 2010 : Higher Tier, Chemistry Paper 2

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Centre Number 71 Candidate Number General Certificate of Secondary Education Paper 2 Higher Tier [G1404] WEDNESDAY 9 JUNE, AFTERNOON G1404 Science: Chemistry *G1404* 2010 TIME 2 hours. 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 seven questions. INFORMATION FOR CANDIDATES The total mark for this paper is 160. Quality of written communication will be assessed in question 1(c). 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 6 7 Total Marks 5474 Marks 1 Neutralisation occurs when an acid and an alkali react to form a salt and water. (a) (i) Examiner Only Marks Remark Complete the table below to give the names and formulae of the ions present in all acids and alkalis. Name Formula Ion present in all acids Ion present in all alkalis [4] (ii) Write an ionic equation for neutralisation. Include state symbols. ___________________________________________________ [2] (b) Sulphuric acid can be neutralised using an alkali such as sodium hydroxide or by adding an insoluble base such as copper(II) oxide. (i) Name the salt formed when sodium hydroxide reacts with sulphuric acid. ___________________________________________________ [1] (ii) Write a balanced symbol equation for the reaction between copper(II) oxide and sulphuric acid. ___________________________________________________ [2] 5474 2 [Turn over (c) In the preparation of copper(II) sulphate crystals, an excess of copper(II) oxide was added to warm dilute sulphuric acid. The excess copper(II) oxide was removed by filtration. Describe how you would obtain pure dry crystals of copper(II) sulphate from the filtrate collected. Examiner Only Marks Remark _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] Quality of written communication (d) (i) [2] To prove that the copper(II) sulphate salt produced in (c) contained copper(II) ions, Cu 2+, two different tests were carried out on a sample of the salt. Test 1 used a solid sample of the salt and Test 2 used a solution of the salt. Complete the table by stating what you would observe for Test 1, Test 2(a) and Test 2(b). Test 1 Observations Flame test 2 (a) Add a few drops of ammonia solution to the salt solution (b) Add excess ammonia solution to the result of Test 2(a) [5] 5474 3 [Turn over (ii) Reagent: Result: Name the reagent used to test for the presence of the sulphate ion in a solution of copper(II) sulphate and state the result for a positive test. Examiner Only Marks Remark ______________________________________________ _______________________________________________ _____________________________________________________ ___________________________________________________ [3] (iii) To identify the ions present in an unknown salt A the following tests were carried out and the observations are recorded in the table below. Use these results to complete the table by giving the identity of the ions present and suggest the formula for salt A. Test 1. Flame test 2. Dissolve half a spatula-measure of A in 2 cm3 of dilute nitric acid. Add2 cm3 of silver nitrate solution. Formula 5474 Observations Ion present lilac flame yellow precipitate of salt A ____________________________________ [3] 4 [Turn over BLANK PAGE (Questions continue overleaf) 5474 5 [Turn over 2 (a) Hydrogen is a powerful rocket fuel. The diagram shows the reaction which occurs in the combustion chamber of a rocket. Key hydrogen atom oxygen atom Examiner Only Marks Remark Combustion chamber NASA http://www1.dfrc.nasa.gov/Gallery/Graphics/STS/Large/EG-0076-04.gif (i) Explain what you understand by the term combustion. _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] (ii) Explain why hydrogen is considered to be a clean fuel. _____________________________________________________ ___________________________________________________ [1] 5474 6 [Turn over (iii) The equation for the reaction which occurs in the combustion chamber is: Examiner Only Marks Remark 2H2 + O 2 2H2O Explain, in terms of bonds, why the reaction in the combustion chamber is exothermic. _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [5] 5474 7 [Turn over (b) Hydrogen is also a powerful reducing agent. The diagram shows the apparatus which could be used in the laboratory to reduce copper(II) oxide using hydrogen. Examiner Only Marks Remark excess hydrogen burning hydrogen copper(II) oxide HEAT (i) State two observations made during this reaction. 1. ___________________________________________________ 2. _________________________________________________ [2] (ii) Write a balanced symbol equation for the reduction of copper(II) oxide using hydrogen. ___________________________________________________ [2] (iii) Explain why this reaction is described as reduction. _____________________________________________________ _____________________________________________________ ___________________________________________________ [2] 5474 8 [Turn over (c) Before the use of electronic built-in flashes, most cameras needed flash bulbs to create a flash of artificial light. The diagram below represents a flash bulb which works by the reaction of very thin magnesium wires with oxygen. Examiner Only Marks Remark Very thin magnesium wire in oxygen gas Thin glass wall Electrical connectors (i) Explain why very thin magnesium wires are used instead of magnesium ribbon. _____________________________________________________ ___________________________________________________ [2] (ii) Write a balanced symbol equation for the reaction which occurs inside the flash bulb. ___________________________________________________ [3] (iii) State one observation made during this reaction. ___________________________________________________ [1] (iv) Complete the ionic half equation below and use it to explain, in terms of electrons, why this reaction is described as oxidation. Mg Mg2+ _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] 5474 9 [Turn over 3 Barium hydroxide is a Group II metal hydroxide which is often found in drain cleaners. Examiner Only Marks Remark Drain Cleaner To determine the concentration of a solution of barium hydroxide Ba(OH) 2 25.0 cm3 of the solution was placed in a conical flask with a few drops of phenolphthalein indicator and titrated with a solution of hydrochloric acid of concentration 0.2 mol/dm3 (moles per litre). The balanced symbol equation for the reaction is: Ba(OH)2 + 2HCl (a) (i) BaCl 2 + 2H 2O Describe in detail, stating precautions to ensure safety and accuracy, how you would place 25.0 cm3 of barium hydroxide solution into the conical flask. _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [4] (ii) State the colour change of the phenolphthalein indicator at the end point. From _____________________ to _____________________ 5474 10 [2] [Turn over (b) The results of the titration are shown in the table below . Initial burette reading (cm3) Volume of hydrochloric acid used (titre) (cm3) Rough titration 0.0 22.8 22.8 1st accurate titration 0.0 22.4 22.4 2nd accurate titration (i) Final burette reading (cm3) 0.0 22.5 22.5 Examiner Only Calculate the average titre. Marks Remark [2] (ii) Calculate the number of moles of hydrochloric acid used in this titration. [2] (iii) Use the balanced symbol equation to deduce the number of moles of barium hydroxide which reacted with the hydrochloric acid. [2] (iv) Calculate the concentration of the barium hydroxide solution in mol/dm3 (moles per litre). [2] 5474 11 [Turn over (c) Calcium is a Group II metal which reacts with nitric acid according to the balanced symbol equation: Ca + 2HNO 3 Ca(NO 3)2 +H Examiner Only Marks Remark 2 (Relative atomic masses: H = 1; N = 14; O = 16; Ca = 40) (i) 0.2 g of calcium metal was reacted with excess nitric acid. Calculate the volume of hydrogen gas which was produced in this reaction. (1 mole of any gas occupies 24 dm3). _______________ dm3 [5] (ii) If the concentration of the nitric acid was 2.0 mol/dm3 (moles per litre) calculate the volume of nitric acid needed to completely react with the 0.2 g of calcium. [4] (iii) The calcium nitrate produced in this reaction is often used in fertilisers. Calculate the percentage of nitrogen, by mass, present in calcium nitrate. [3] 5474 12 [Turn over 4 (a) Calcium carbonate thermally decomposes to form calcium oxide. Calcium oxide (lime) has a high melting point and can be heated to a high temperature without melting so that it emits white light, called limelight. Examiner Only Marks Remark Adam Hart-Davis/Science Photo Library (i) Explain what is meant by thermal decomposition. _____________________________________________________ ___________________________________________________ [2] (ii) Write a balanced symbol equation for the thermal decomposition of calcium carbonate. ___________________________________________________ [2] (iii) Explain why calcium oxide has a high melting point. _____________________________________________________ _____________________________________________________ ___________________________________________________ [2] (iv) Calcium oxide must be kept dry because when it comes into contact with even the slightest amount of moisture, it rapidly becomes hot and hisses, releasing a lar ge amount of steam. Write a balanced symbol equation for the reaction of calcium oxide with water. ___________________________________________________ [2] 5474 13 [Turn over (b) Calcium carbonate reacts with acids such as hydrochloric acid and sulphuric acid. It is used in many antacid tablets, where it reacts with excess acid in the stomach, reducing acidity and relieving heartburn . Examiner Only Marks Remark drflet/istockphoto (i) Write a balanced symbol equation for the reaction between calcium carbonate and hydrochloric acid. ___________________________________________________ [3] (ii) State two observations for this reaction. 1. ___________________________________________________ 2. _________________________________________________ [2] (iii) Write a balanced symbol equation for the reaction between calcium carbonate and sulphuric acid. ___________________________________________________ [2] 5474 14 [Turn over (c) Another compound used in antacid tablets is aluminium hydroxide. (i) Examiner Only Marks Remark Write a balanced symbol equation for the reaction between aluminium hydroxide and hydrochloric acid. ___________________________________________________ [3] (ii) Aluminium hydroxide is amphoteric. Explain what you understand by the term amphoteric. _____________________________________________________ ___________________________________________________ [1] 5474 15 [Turn over 5 (a) Compounds are formed when two or more dif ferent elements chemically bond together. (i) Examiner Only Marks Remark Explain what you understand by the term element. _____________________________________________________ _____________________________________________________ ___________________________________________________ [2] (ii) Using full electronic configurations, draw diagrams to show how atoms of magnesium combine with atoms of oxygen to form magnesium oxide. [6] (iii) State the type of bonding which is present in magnesium oxide. ___________________________________________________ [1] 5474 16 [Turn over (b) Substances containing covalent bonds can have very dif ferent physical properties. Graphite, which is an allotrope of the element carbon, contains covalent bonds. Examiner Only Marks Remark (i) Explain what you understand by the term allotrope. _____________________________________________________ ___________________________________________________ [2] (ii) Draw a labelled diagram to show the structure and bonding in graphite. [4] (iii) Diamond is another allotrope of carbon and it is the hardest naturally occurring substance on Earth. Explain why diamond is so hard. _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [2] 5474 17 [Turn over (c) Carbon dioxide also contains covalent bonds. The melting point of carbon dioxide is 78 C. Examiner Only Marks Remark (i) Explain what you understand by the term covalent bond. _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] (ii) Explain why the melting point of carbon dioxide is very low . _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] 5474 18 [Turn over BLANK PAGE (Questions continue overleaf) 5474 19 [Turn over 6 The blast furnace is used to produce iron from its ore. The diagram below represents the materials added to, and removed from, the blast furnace. Examiner Only Marks Remark CHARGE made up of: IRON ORE LIMESTONE COKE EXHAUST GASES BLAST FURNACE HOT AIR MOLTEN SLAG MOLTEN IRON (a) Iron ore is reduced to iron. The reducing agent is carbon monoxide. Carbon monoxide is formed from carbon in two reactions which are shown as word equations below. Reaction 1: carbon + oxygen Reaction 2: carbon (i) dioxide + carbon carbon dioxide carbon monoxide Name the material added to the blast furnace which is composed mainly of carbon. ___________________________________________________ [1] (ii) What is the source of oxygen in the blast furnace? ___________________________________________________ [1] (iii) Write balanced symbol equations for reactions 1 and 2 which are given above. Reaction 1: __________________________________________ [2] Reaction 2: __________________________________________ [3] (iv) Write a balanced symbol equation for the reduction of iron ore to iron in the blast furnace. ___________________________________________________ [3] 5474 20 [Turn over (b) The flow diagram below represents the formation of slag in the blast furnace. Substances A and B are formed by the thermal decomposition of limestone (Reaction 3) and then substance B reacts with an impurity in the iron ore to form slag. Substance A is one of the exhaust gases. Examiner Only Marks Remark Limestone Thermal decomposition (Reaction 3) A B + Impurity in iron ore Reaction 4 SLAG EXHAUST GASES (i) Name A and B. A ___________________________________________________ B _________________________________________________ [2] (ii) Name the impurity in the iron ore which reacts with B to form slag. ___________________________________________________ [1] (iii) Write a balanced symbol equation for reaction 4. ___________________________________________________ [2] (iv) Suggest the name of one other gas which could be present in the exhaust gases. ___________________________________________________ [1] 5474 21 [Turn over 7 Many chemical reactions produce gases. For a reaction which produces a gas, the rate of the reaction can be measured by two main methods. Examiner Only Marks Remark (a) The following three reactions produce a gas. Reaction A: Mg + 2HCl MgCl 2 + H Reaction B: 2H2O2 2H 2O + O Reaction C: Na2S2O3 + 2HCl 2 2 2NaCl + SO 2 +S+H 2O (i) Circle the gaseous product in each reaction. (ii) [3] H 2O2 undergoes catalytic decomposition in reaction B. What is the chemical name of H 2O2? ___________________________________________________ [1] (iii) A catalyst is required for reaction B. What is meant by the term catalyst? _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] (iv) Name the catalyst required for reaction B. ___________________________________________________ [1] 5474 22 [Turn over (b) One method of measuring the rate of a reaction in which a gas is produced is to monitor the volume of gas. The apparatus shown below is often used for this purpose. A Examiner Only Marks Remark C B conical flask hydrochloric acid marble chips in contact with acid (i) Name the pieces of apparatus labelled A, B and C A ___________________________________________________ B ___________________________________________________ C _________________________________________________ [3] (ii) Apart from safety equipment, what other piece of apparatus would be required to carry out this experiment? ___________________________________________________ [1] (iii) Why must A be below the level of the hydrochloric acid in the conical flask during the experiment? _____________________________________________________ ___________________________________________________ [1] 5474 23 [Turn over (c) The apparatus below also shows how the rate of the reaction between 1.25 g of marble chips (calcium carbonate) and 25.0 cm3 of hydrochloric acid (an excess) may be measured. This was carried out at room temperature (20 C). Examiner Only Marks Remark Cotton wool plug Conical flask containing 1.25 g of marble chips and 25.0 cm3 of hydrochloric acid Electronic balance 117.20 The mass of the flask containing the marble chips and the acid is measured against time. The results obtained were plotted on the graph shown below. 117.25 117.20 117.15 117.10 Mass/g 117.05 117.00 116.95 116.90 116.85 116.80 116.75 116.70 (i) 0 1 2 3 4 5 6 Time/minutes 7 8 9 10 Calculate the total mass lost during the experiment. _____________________________________________________ ___________________________________________________ [2] 5474 24 [Turn over (ii) What is the purpose of the cotton wool plug in the apparatus? Examiner Only Marks Remark _____________________________________________________ ___________________________________________________ [1] (iii) The experiment was repeated at 40 C and the rate of reaction increased. Sketch on the graph the curve you would expect to obtain if all other factors were kept the same. [2] (iv) Explain, in terms of particles, how increasing the temperature would increase the rate of this reaction. _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] (v) State clearly two other factors which you could change to increase the rate of this chemical reaction. 1. ___________________________________________________ 2. _________________________________________________ [2] (d) Catalysts are used in many industrial processes. Complete the blanks in the table below. Industrial Process Equation for the reaction Catalytic oxidation of ammonia 4NH3 + 5O 2 4NO + 6H 2O Haber Process Name of catalyst iron [4] 5474 25 [Turn over THIS IS THE END OF THE QUESTION P APER 5474 26 [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. 1847-031-1

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