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UK GCSE 2010 : Higher Tier, Chemistry Paper 1

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Centre Number 71 Candidate Number General Certificate of Secondary Education 2010 Paper 1 Higher Tier G1403 Science: Chemistry [G1403] WEDNESDAY 26 MAY, 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(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 Total Marks 5472 Marks 1 (a) The modern Periodic Table has been in use for over 100 years. Its development included the work of several chemists including John Newlands and Dmitri Mendeleev. Examiner Only Marks Remark (i) What name was given to the law developed by John Newlands? ___________________________________________________ [1] (ii) State three features of the Periodic Table developed by Mendeleev which are different from the modern Periodic Table. 1. ___________________________________________________ _____________________________________________________ 2. ___________________________________________________ _____________________________________________________ 3. ___________________________________________________ ___________________________________________________ [3] (b) The modern Periodic Table is made up of Groups and Periods. What name is given to the following Groups? Group I __________________________________________________ Group VII ______________________________________________ [2] 5472 2 [Turn over (c) Often a short form of the Periodic Table like the one shown below is used. Group I II III IV V VI VII H Li Examiner Only Marks Remark 0 He Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ge As Se Br Kr Ca Ga Using ONLY the elements in the table above: (i) Name one noble gas. ___________________________________________________ [1] (ii) Name one element which is a liquid at room temperature and pressure. ___________________________________________________ [1] (iii) Name one diatomic gas. ___________________________________________________ [1] (iv) Name one non-metal which is a solid at room temperature and pressure. ___________________________________________________ [1] (v) Name one element which forms a simple ion with a charge of 2 ___________________________________________________ [1] (vi) Suggest one reason why hydrogen may be placed in Group I. _____________________________________________________ ___________________________________________________ [1] 5472 3 [Turn over (d) Group III of the Periodic Table contains the elements boron, aluminium and gallium. Examiner Only Marks Remark Group III 11 5B 27 13 Al 70 31 Ga All of these elements form compounds with oxygen and chlorine. (i) Write the formula of aluminium oxide. ___________________________________________________ [1] (ii) Write a balanced symbol equation for the reaction of aluminium with chlorine. ___________________________________________________ [3] (iii) In which period of the Periodic Table is gallium found? ___________________________________________________ [1] (iv) Suggest why boron would have different physical properties to the other elements of Group III. ___________________________________________________ [1] (v) The elements of Group III can form a simple ion with a 3+ charge. Name one other element, apart from those in Group III, which forms an ion with a 3+ charge. You may use your Data Leaflet to help answer this question. ___________________________________________________ [1] 5472 4 [Turn over BLANK PAGE (Questions continue overleaf) 5472 5 [Turn over 2 Some substances dissolve very well in water and are said to have high solubility. Examiner Only Marks Remark (a) Explain what is meant by the term solubility. _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [4] (b) To determine the solubility of potassium chloride in water, 20 g of potassium chloride were placed in a beaker. 40 cm3 of water were added to the beaker and warmed until all the potassium chloride had dissolved. The beaker was then allowed to cool. The temperature at which crystals first appeared was recorded. The experiment was repeated five more times adding an extra 5 cm3 of water each time. The results obtained are shown in the table below. Mass of potassium chloride (g) Volume of water (cm3) 20 40 Temperature at which crystals first appear ( C) 80 20 45 59 20 50 41 20 55 27 36.4 20 60 15 33.3 20 65 5 30.8 Solubility (g/100 g water) 50.0 44.4 (i) Calculate the solubility of potassium chloride at 41 C and insert the value in the table. Solubility_________ g/100 g water [1] 5472 6 [Turn over (ii) Use the results table to plot a solubility curve for potassium chloride on the graph provided below. 55 Solubility/g/100 g water 50 45 40 35 30 25 0 0 10 20 30 40 50 60 70 80 90 Temperature/ C Examiner Only Marks Remark [4] (iii) How does the solubility of potassium chloride vary with increasing temperature? ___________________________________________________ [1] (iv) Using your graph, determine the solubility of potassium chloride at 10 C. ___________________________________________________ [1] (v) If a saturated solution of potassium chloride containing 50 g of water is cooled from 80 C to 5 C, what mass of potassium chloride will crystallise out of solution? _____________ g [3] 5472 7 [Turn over (c) The solution of potassium chloride was tested for the presence of chloride ions. Name a suitable reagent that could be used to test for the presence of chloride ions and state the observations for a positive test. Examiner Only Marks Remark Suitable reagent ____________________________________________ Observations ______________________________________________ _______________________________________________________ [3] (d) Many substances, such as sodium hydroxide and anhydrous calcium chloride interact with moist air. (i) Describe the observations made when some pellets of sodium hydroxide are left on a watch glass in the laboratory for several days. _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] (ii) Explain what you understand by the term anhydrous. _____________________________________________________ ___________________________________________________ [2] 5472 8 [Turn over (e) Bottles of sodium hydroxide often have a white crust around their neck. This crust forms when sodium hydroxide reacts with carbon dioxide in the air. Examiner Only Marks Remark CCEA (i) Write the chemical name of the white crust. ___________________________________________________ [1] (ii) Write a balanced symbol equation to show the formation of the white crust. __________________________________________________ [3] 5472 9 [Turn over 3 Sulphur is a non-metallic element which occurs native in the Earth s crust. It is an important raw material in the chemical industry. Examiner Only Marks Remark (a) Sulphur undergoes combustion when heated in air. (i) Write a balanced symbol equation for the combustion of sulphur. ___________________________________________________ [2] (ii) Describe what would be observed when sulphur is heated in air. _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] (b) Air pollution is caused by the presence of substances which are bad for health. One of the main pollutants in air is sulphur dioxide. (i) Name one source of sulphur dioxide pollution. ___________________________________________________ [1] (ii) Sulphur dioxide reacts with water vapour in the air to form acid rain. Write a balanced symbol equation for this reaction. ___________________________________________________ [2] (iii) Acid rain is a weak acid. Suggest the pH value of a sample of acid rain. __________________________________________________ [1] (iv) State two effects of acid rain. 1. ___________________________________________________ _____________________________________________________ 2. ___________________________________________________ ___________________________________________________ [2] 5472 10 [Turn over (v) Suggest two ways of preventing the formation of acid rain. Examiner Only Marks Remark 1. ___________________________________________________ _____________________________________________________ 2. ___________________________________________________ ___________________________________________________ [2] (c) Sulphur is used in the manufacture of sulphuric acid. The first stage in this process is the combustion of sulphur to form sulphur dioxide. The second stage is the conversion of sulphur dioxide to sulphur trioxide using a catalyst. (i) Write a balanced symbol equation for the conversion of sulphur dioxide to sulphur trioxide. ___________________________________________________ [3] (ii) Name the catalyst used in this reaction. ___________________________________________________ [1] (d) Concentrated sulphuric acid is a dehydrating agent. (i) Explain the meaning of the term dehydrating agent. _____________________________________________________ ___________________________________________________ [1] (ii) Describe what you would observe when concentrated sulphuric acid is added to sugar. _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] 5472 11 [Turn over 4 Lithium is a metal which is used in LCD televisions, computer monitors and mobile phones. Examiner Only Marks Remark mart_m / iStockphoto (a) Most lithium is obtained from lithium carbonate. The diagram below shows how solid lithium is produced from lithium carbonate. lithium carbonate reaction with hydrochloric acid lithium chloride solution recrystallisation solid lithium chloride heating molten lithium chloride electrolysis molten lithium cooling solid lithium 5472 12 [Turn over (i) Write a balanced symbol equation for the reaction of lithium carbonate with hydrochloric acid. Examiner Only Marks Remark ___________________________________________________ [3] (ii) Explain what is meant by the term electrolysis. _____________________________________________________ ___________________________________________________ [2] (b) Complete the table below by placing a tick ( ) to indicate if the substance conducts electricity or does not conduct electricity. Place only one tick for each substance. Substance Conducts electricity Does not conduct electricity solid lithium molten lithium solid lithium chloride lithium chloride solution [4] 5472 13 [Turn over (c) The electrolysis of molten lithium chloride may be carried out using the apparatus shown below. Molten lithium chloride is the electrolyte. Examiner Only Marks Remark + electrode A electrode B crucible tripod molten lithium chloride HEAT heatproof mat (i) What is meant by the term electrolyte? _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] (ii) Name electrode A and electrode B. Electrode A ___________________________________________ Electrode B _________________________________________ [2] (iii) What material is used to make the electrodes? ___________________________________________________ [1] 5472 14 [Turn over (iv) State one reason why this material is chosen to make the electrodes. Examiner Only Marks Remark ___________________________________________________ [1] (v) At which electrode, A or B, is lithium produced? ___________________________________________________ [1] (vi) What would you observe at the other electrode? _____________________________________________________ ___________________________________________________ [2] (vii)Write half equations for the reactions which are occurring at each electrode. Electrode A _________________________________________ [3] Electrode B _________________________________________ [2] 5472 15 [Turn over 5 Ethene is a very important and versatile organic compound. Examiner Only Marks Remark (a) (i) Name the homologous series to which ethene belongs. ___________________________________________________ [1] (ii) Complete the table below giving the molecular formula, structural formula and physical state of ethene at room temperature and pressure. Molecular formula of ethene Structural formula of ethene Physical state of ethene at room temperature and pressure [3] (iii) Ethene is described as an unsaturated molecule. Explain what is meant by the term unsaturated. _____________________________________________________ ___________________________________________________ [1] (b) One use of ethene in industry is in the manufacture of ethanol. (i) Write a balanced symbol equation for the reaction between ethene and steam. ___________________________________________________ [2] (ii) Draw the full structural formula of ethanol, showing all bonds. [2] 5472 16 [Turn over (c) The ethanol present in alcoholic drinks is made by fermentation. Describe in detail how ethanol is produced by fermentation. Include: Examiner Only Marks Remark names of the reactants names of the products (other than ethanol) necessary conditions _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [5] Quality of written communication [2] (d) Wine and other alcoholic drinks are often used in cooking during which the ethanol may undergo combustion. (i) Write a balanced symbol equation for the complete combustion of ethanol. ___________________________________________________ [3] (ii) What colour is the flame when ethanol burns? ___________________________________________________ [1] 5472 17 [Turn over (e) If a bottle of wine is left open to the atmosphere for a number of days it is oxidised by oxygen in the air and a solution of ethanoic acid forms. Examiner Only Marks Remark (i) Explain what you understand by the term oxidation. _____________________________________________________ ___________________________________________________ [2] (ii) Draw the full structural formula of ethanoic acid showing all bonds. [2] (iii) A solution of ethanoic acid is widely used as a food flavouring. By what name is this solution more commonly known? ___________________________________________________ [1] (f) Ethanoic acid reacts as a typical dilute acid. (i) State what you would observe when a strip of magnesium metal is dropped into a solution of ethanoic acid. _____________________________________________________ _____________________________________________________ ___________________________________________________ [2] (ii) Write a balanced symbol equation for the reaction between magnesium metal and ethanoic acid. ___________________________________________________ [3] 5472 18 [Turn over THIS IS THE END OF THE QUESTION PAPER 5472 19 [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. 1847-030-1

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