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UK GCSE 2006 : Higher Tier, Chemistry Paper 2

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Centre Number 71 Candidate Number General Certificate of Secondary Education 2006 Paper 2 Higher Tier G1404 Science: Chemistry [G1404] THURSDAY 22 JUNE, AFTERNOON 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 2(b). 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 G142H6 880 Marks 1 (a) Complete the blanks in the paragraph below about the Periodic Table. Examiner Only Marks Remark In 1869, a Russian chemist called _______________ produced a Periodic Table very similar to the one we use today. The elements of the modern Periodic Table are arranged in order of increasing _______________ number. In the Periodic Table, the horizontal rows are called periods and the vertical columns of elements are called _______________ . Moving across a period the size of the atoms _______________ and the non-metallic character of the elements _______________. [5] (b) Sodium and potassium are both in Group I of the Periodic Table. (i) Give another name for the Group I elements. ___________________________________________________ [1] (ii) Name another element found in Group I. ___________________________________________________ [1] (iii) Which element in Group I is least reactive? ___________________________________________________ [1] (iv) In terms of electronic configuration, what do the elements of Group I have in common? Illustrate your answer giving the full electronic configuration of sodium and potassium. Electronic configuration of sodium: _________________________ Electronic configuration of potassium: _______________________ ______________________________________________________ ___________________________________________________ [3] G142H6 880 2 [Turn over (c) Use your Periodic Table to answer the following questions. Examiner Only Marks Remark (i) Give the symbol of a noble gas. ___________________________________________________ [1] (ii) Give the symbol of an element which has five electrons in its outer shell. ___________________________________________________ [1] (iii) Give the symbol of a non-metal which is solid at room temperature and pressure. ___________________________________________________ [1] (iv) Give the symbol of an element which forms an ion with a charge of 2+. ___________________________________________________ [1] (v) Give the symbol of an element in Period 3 which is best described as a semi-metal. ___________________________________________________ [1] G142H6 880 3 [Turn over 2 (a) Some football boots and leather bags have a small packet of silica gel included in the packaging. Examiner Only Marks Remark (i) What is the purpose of the silica gel? ______________________________________________________ ___________________________________________________ [1] (ii) Name another solid compound used in the laboratory for the same purpose as the silica gel. ___________________________________________________ [1] (b) When a fish is caught in a river and put into a jar of water, it survives for a long time if the jar is kept cool. However, if the water in the jar is allowed to warm up, the fish soon dies. Explain why this happens. _________________________________________________________ _________________________________________________________ _________________________________________________________ ______________________________________________________ [3] Quality of written communication G142H6 880 [2] 4 [Turn over (c) Sugar is soluble in water. It has a high solubility. Examiner Only Marks Remark (i) What is meant by the term solubility? ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [4] (ii) How does the solubility of sugar vary as the temperature of the water increases? ___________________________________________________ [1] G142H6 880 5 [Turn over (d) Potassium chloride and potassium nitrate are both soluble in water. The solubilities of the two salts at specific temperatures are given in the table below. Temperature ( C) 0 10 20 30 40 50 13 21 32 46 63 83 106 Solubility of potassium nitrate (g/100 g water) 28 30 5 33 36 39 42 Remark 60 Solubility of potassium chloride (g/100 g water) Examiner Only Marks 45 The solubility curve for potassium nitrate has been plotted on the graph opposite. (i) Using your graph, find the solubility of potassium nitrate at 45 C. ___________________________________________________ [1] (ii) Using your graph, find the temperature at which 19 g of potassium nitrate saturates 50 g of water. ______________________________________________________ ___________________________________________________ [2] (iii) On the same axes plot the solubility curve for potassium chloride. [3] (iv) At what temperature do the two salts have the same solubility? ___________________________________________________ [1] (v) What mass of potassium chloride will crystallise from a saturated solution containing 1000 g of water, if the solution is cooled from 58 C to 24 C? [4] G142H6 880 6 [Turn over 110 100 90 80 Solubility/g/100 g water 70 60 50 40 30 20 10 0 0 10 20 30 40 50 60 Temperature/ C G142H6 880 7 [Turn over 3 The diagram below shows a blast furnace for the production of iron. Examiner Only Marks Remark Waste gases A A B C (a) (i) Complete the table to give information about the main raw materials which are fed into the top of the blast furnace. Common name Chemical name Formula or symbol Iron(III) oxide Limestone Carbon [6] (ii) Name the raw material which is blasted into the furnace at point A. ___________________________________________________ [1] (iii) Name the substances tapped off at points B and C. B _________________________________________________ [1] C _________________________________________________ [1] G142H6 880 8 [Turn over (b) At the bottom of the blast furnace, coke reacts to form carbon dioxide. Write a balanced symbol equation for this reaction. Examiner Only Marks Remark ______________________________________________________ [2] (c) The carbon dioxide reacts with more coke to form carbon monoxide. (i) Write a balanced symbol equation for this reaction. ___________________________________________________ [3] (ii) What is the importance of carbon monoxide in the extraction process? ___________________________________________________ [1] (iii) Write a balanced symbol equation to show the part played by the carbon monoxide in the extraction process. ___________________________________________________ [3] (d) Sand (SiO2) is an impurity in the raw materials. The sand is removed from the blast furnace by reacting it with calcium oxide. (i) Write a balanced symbol equation to show how calcium oxide is formed in the blast furnace. ___________________________________________________ [2] (ii) Write a balanced symbol equation for the reaction of sand with calcium oxide. ___________________________________________________ [2] (e) Large quantities of limestone for use in the blast furnace are obtained from quarries. Give two environmental problems that could be caused by quarrying limestone. _________________________________________________________ ______________________________________________________ [2] G142H6 880 9 [Turn over 4 (a) Chlorine gas can be prepared in the laboratory using concentrated hydrochloric acid. The reaction can be represented by the equation Examiner Only Marks Remark 2HCl + [O] H2O + Cl2 (i) State the name and type of substance represented by [O]. Name: ________________________________________________ Type: ______________________________________________ [2] (ii) Describe the appearance of the chlorine gas produced. ___________________________________________________ [1] (b) In industry, chlorine can be produced by the electrolysis of concentrated sodium chloride solution using carbon electrodes. (i) State the electrode at which chlorine is produced. ___________________________________________________ [1] (ii) The electrodes cannot be made from iron, since iron reacts with chlorine. Write a balanced symbol equation for the reaction of iron with chlorine. ___________________________________________________ [3] (c) Chlorine is a reactive gas. Write balanced symbol equations and give the observations for the following reactions. (i) chlorine + sodium hydroxide solution Equation: ___________________________________________ [3] Observations:________________________________________ [1] (ii) chlorine + sodium bromide solution Equation: ___________________________________________ [3] Observations:___________________________________________ ___________________________________________________ [2] G142H6 880 10 [Turn over (d) Large amounts of liquid chlorine are transported in tankers by road to water treatment works. Examiner Only Marks Remark (i) How is chlorine gas turned into liquid chlorine? ___________________________________________________ [1] (ii) Why is chlorine transported as a liquid and not as a gas? ______________________________________________________ ___________________________________________________ [1] Every tanker transporting chlorine must have a Hazchem warning label as shown below. 2XE 1017 Box A Chlorine (iii) What word is missing from Box A on the Hazchem label to describe the hazard associated with chlorine? ___________________________________________________ [1] (iv) Why are small amounts of chlorine added to water at the water treatment works? ___________________________________________________ [2] (v) Give another use of chlorine. ___________________________________________________ [1] G142H6 880 11 [Turn over (e) Hydrochloric acid can also be transported by road in tankers. The tanker has the Hazchem warning label shown below. 2R 1789 Examiner Only Marks Remark Box B Hydrochloric Acid (i) What is the word missing from Box B on this Hazchem label to describe the hazard associated with hydrochloric acid? ___________________________________________________ [1] (ii) Hydrochloric acid can be made by using sodium chloride. What other substance reacts with sodium chloride to produce hydrogen chloride gas? ___________________________________________________ [2] (iii) Describe the test for hydrogen chloride gas and give the expected result. ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [4] G142H6 880 12 [Turn over BLANK PAGE (Questions continue overleaf) G142H6 880 13 [Turn over 5 (a) The following reactions A and B can be classified in different ways. A copper(II) carbonate copper(II) oxide + carbon dioxide B sodium hydroxide + hydrochloric acid sodium chloride + water Complete the table by placing a tick ( ) in each column for reactions A and B indicating which terms apply to each reaction. More than one term can be applied to each reaction. Term Examiner Only Marks Remark Reaction A B Exothermic Endothermic Thermal decomposition Thermal cracking Combustion Neutralisation Displacement G142H6 880 [4] 14 [Turn over (b) Solid copper(II) oxide can be reduced by passing a stream of hydrogen gas over the heated solid. Examiner Only Marks Remark Glass tube Excess hydrogen burning Hydrogen gas HEAT Porcelain boat containing copper(II) oxide (i) Write a balanced symbol equation for the reaction between copper(II) oxide and hydrogen gas. ___________________________________________________ [2] (ii) What would you observe during this reaction? ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] (iii) Write a balanced symbol equation for the hydrogen burning. ___________________________________________________ [3] G142H6 880 15 [Turn over (c) The table below gives a series of equations for oxidation and reduction reactions in two industrial processes. Reaction Equation A Type 2O2 O2 + 4e S + O2 SO2 Aluminium manufacture by electrolysis oxidation C Remark Industrial process reduction B Examiner Only Marks oxidation Sulphuric acid manufacture D 2SO2 + O2 2SO3 oxidation (i) Complete the table giving the reduction reaction in the industrial manufacture of aluminium. [3] (ii) Explain why reaction C is described as oxidation. ______________________________________________________ ___________________________________________________ [2] (iii) What is the name of the process for the industrial manufacture of sulphuric acid? ___________________________________________________ [1] (iv) Name the catalyst used in reaction D. ___________________________________________________ [1] G142H6 880 16 [Turn over BLANK PAGE (Questions continue overleaf) G142H6 880 17 [Turn over 6 Ionic compounds like lead(II) bromide conduct electricity when molten. Examiner Only Marks Remark (a) Explain as fully as possible why ionic compounds conduct electricity when molten. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (b) (i) Draw a labelled diagram of the assembled apparatus used to carry out the electrolysis of molten lead(II) bromide. [5] (ii) Name the material used to make the electrodes in this electrolysis. ___________________________________________________ [1] (iii) What would be observed at the positive electrode during the experiment? ______________________________________________________ ___________________________________________________ [2] G142H6 880 18 [Turn over (iv) Name the products of this electrolysis. Examiner Only Marks Remark ______________________________________________________ ___________________________________________________ [2] (v) Why does this electrolysis experiment need to be carried out in a fume cupboard? ______________________________________________________ ___________________________________________________ [2] (c) The diagram below shows the apparatus used in the refining of copper by electrolysis. Anode Cathode Electrolyte (i) What material is used for the anode? ___________________________________________________ [2] (ii) Write a balanced, ionic equation for the reaction which takes place at the anode. ___________________________________________________ [3] (iii) Name one substance which may be used as the electrolyte. ___________________________________________________ [1] G142H6 880 19 [Turn over 7 (a) Oxygen forms ozone gas, O3, in the upper atmosphere according to the equation Examiner Only Marks Remark 3O2(g) 2O3(g) 150 m3 of oxygen reacts completely to form ozone. (i) State Avogadro s Law. ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] (ii) Using Avogadro s Law or otherwise, calculate the volume of ozone gas produced. ______________________ m3 [2] (b) In the laboratory ozone gas can be produced by passing an electrical discharge through dry air. 450 cm3 of ozone gas is produced when the temperature is 300 K and the pressure is 1 atmosphere. The ozone gas is compressed using a pressure of 8 atmospheres and the temperature is decreased to 200 K. Calculate the volume of ozone gas under these new conditions. ______________________ cm3 [4] G142H6 880 20 [Turn over (c) Ozone is used in very small amounts in underground railway stations to remove compounds which cause stations to be stuffy. One of the compounds which is formed is formaldehyde, CH2O. Examiner Only Marks Remark Calculate the percentage by mass of carbon in CH2O. ______________________ % [3] G142H6 880 21 [Turn over (d) 1.92 g of sulphur dioxide, SO2, reacts completely with ozone to form 2.40 g of sulphur trioxide, SO3. Examiner Only Marks Remark (i) Calculate the number of moles of sulphur dioxide used. [2] (ii) Calculate the mass of ozone which reacts. [1] (iii) Calculate the number of moles of ozone which reacts. [2] (iv) Calculate the number of moles of sulphur trioxide formed. [2] (v) Using your answers to (i), (iii) and (iv) or otherwise, balance the symbol equation for the reaction. Equation: G142H6 880 SO2 + O3 22 SO3 [1] [Turn over (e) Oxygen gas is prepared by the decomposition of hydrogen peroxide solution using the catalyst manganese(IV) oxide. Examiner Only Marks Remark 2H2O2 2H2O + O2 A solution of hydrogen peroxide is labelled 0.1 mol/dm3 (moles per litre). 25.0 cm3 of this solution is decomposed completely using manganese(IV) oxide. (i) What is meant by the term catalyst? ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] (ii) Calculate the volume of oxygen gas produced in this decomposition. State the units. (1 mole of any gas occupies a volume of 24 dm3) ______________________ [7] G142H6 880 23 [Turn over S 5/05 5300 302507(35)

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