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1 Centre Number Candidate Number Candidate Name UNIVERSITY OF CAMBRIDGE LOCAL EXAMINATIONS SYNDICATE General Certificate of Education Ordinary Level CHEMISTRY 5070/2 PAPER 2 Theory MAY/JUNE SESSION 2000 Additional materials: Answer paper Electronic calculator and/or Mathematical tables 1 hour 30 minutes TIME 1 hour 30 minutes INSTRUCTIONS TO CANDIDATES Write your name, Centre number and candidate number in the spaces at the top of this page and on any separate answer paper used. Section A Answer all questions. Write your answers in the spaces provided on the question paper. Section B Answer any three questions. Write your answers on the separate answer paper. At the end of the examination, fasten any separate answer paper used securely to the question paper. INFORMATION FOR CANDIDATES The number of marks is given in brackets [ ] at the end of each question or part question. Mathematical tables are available. You may use a calculator. A copy of the Periodic Table is printed on page 12. FOR EXAMINER S USE Section A B8 B9 B10 B11 TOTAL This question paper consists of 12 printed pages. SB (DJ) QF06368/4 UCLES 2000 [Turn over

2 2 SECTION A Answer all the questions in this section in the spaces provided. The total mark for this section is 45. A1 Choose from the following substances to answer the questions below. aluminium ammonia iron lithium magnesium oxide potassium hydroxide silicon sulphur dioxide Each substance can be used once, more than once, or not at all. Name a substance which is an acidic gas, is a compound with a very high melting point and can be used in the lining of furnaces, is a metal with a high melting point and a high density, (d) is a solid at room temperature and dissolves in water to form an alkaline solution, (e) is an element which is soft with a low density. 5070/2 S00

3 A2 3 Two isotopes of carbon are carbon-12 and carbon-13. The proportion of these isotopes in ivory elephant tusks can be used to determine where in the world the tusks come from. What is the meaning of the term isotopes? Complete the table about atoms of carbon-12 and carbon-13. isotope symbol number of protons per atom number of electrons per atom number of neutrons per atom carbon C carbon-13 [2] Elephants eat plants that contain carbon-12 and carbon-13 combined in compounds such as carbohydrates. Carbohydrates in plants are formed from glucose that is made by the process of photosynthesis. Briefly describe, including a word equation, the process of photosynthesis....[3] 5070/2 S00 [Turn over

4 A3 Alkenes are an homologous series of hydrocarbons. The table below shows the properties of some alkenes. 4 alkene molecular formula melting point/ C boiling point/ C ethene C 2 H propene C 4 H pentene C 5 H hexene C 6 H Describe how alkenes are manufactured....[3] Name the alkene with the molecular formula C 4 H 8. What is the molecular formula of propene? (d) Name an alkene that is a liquid at room temperature. (e) Draw a dot and cross diagram to show the bonding in ethene. You need only draw the electrons in the outer shells of carbon and hydrogen. [2] (f) (i) Write the equation for the reaction between ethene and steam.... (ii) What name is given to this type of reaction?...[2] 5070/2 S00

5 A4 An excess of hydrochloric acid in the stomach causes indigestion. An indigestion tablet contains a mixture of calcium carbonate and magnesium hydroxide. Give the formulae of two salts formed when the tablets react with hydrochloric acid and...[2] 3.0 dm 3 of 0.10 mol/dm 3 hydrochloric acid is spilled on a laboratory floor. The spilt acid is neutralised by 1.0 mol/dm 3 aqueous sodium hydrogencarbonate. HCl(aq) + NaHCO 3 (aq) NaCl (aq) + CO 2 (g) + H 2 O(l) Calculate the volume of aqueous sodium hydrogencarbonate needed to neutralise the hydrochloric acid. [2] Aqueous ammonia is spilled on a laboratory floor. Name a compound that will neutralise the ammonia. (d) Some plants cannot grow in soils that are too acidic. Name a solid that is used to neutralise acidic soils. A5 Aqueous iron(ii) ions react with acidified potassium manganate(vii) according to the equation below. 5Fe 2+ (aq) + 8H + (aq) + MnO 4 - (aq) 5Fe 3+ (aq) + 4H 2 O(l) + Mn 2+ (aq) What is the reducing agent in this reaction? Explain your answer....[2] Describe briefly how aqueous potassium iodide can be used to test for an oxidising agent. 5070/2 S00 [Turn over

6 A6 6 Many cars are fitted with air-bags which inflate in an accident. Air-bags contain the solid sodium azide, NaN 3, which decomposes rapidly to form sodium and nitrogen. The nitrogen formed fills the air-bag. Construct the equation, including state symbols, for the decomposition of sodium azide....[2] In a crash, an air-bag fills with 72 dm 3 of nitrogen at room temperature and pressure. What mass of sodium azide is needed to provide the nitrogen? [3] Sodium azide, NaN 3, reacts with dilute hydrochloric acid to give sodium chloride and a compound A. Compound A contains 2.33 % hydrogen and 97.7% nitrogen by mass. (i) What is the empirical formula for compound A? (ii) Construct the equation for the reaction between sodium azide and dilute hydrochloric acid....[3] 5070/2 S00

7 A7 Calcium carbonate reacts with dilute nitric acid to give carbon dioxide. 7 The rate of reaction can be investigated by measuring the change in mass of a mixture of calcium carbonate and nitric acid over a period of time. As carbon dioxide escapes, the mixture loses mass. The graph below shows the results obtained when a 3.0 g lump of calcium carbonate was added to an excess of 1.0 mol/dm 3 nitric acid. mass of calcium carbonate and acid/g 0 10 time/minutes 20 Name the other products of the reaction between calcium carbonate and dilute nitric acid. Had the reaction between calcium carbonate and nitric acid finished after 20 minutes? Explain your answer. The experiment was repeated using a 3.0 g lump of calcium carbonate but an excess of 2.0 mol/dm 3 nitric acid. Draw on the graph above, the curve you would expect. Label the curve X. [1] 5070/2 S00 [Turn over

8 (d) (e) 8 Suggest why it is difficult to investigate the rate of reaction in this experiment using powdered calcium carbonate instead of a lump. Draw a labelled diagram to show another method of investigating the rate of reaction between nitric acid and a lump of calcium carbonate. [3] 5070/2 S00

9 9 SECTION B Answer three questions from this section. The total mark for this section is 30. B8 Methane is a fuel. It completely burns to form carbon dioxide and water. When one mole of methane is burned, 890 kj of energy are released. H H C H + 2 O = O O = C = O + 2 O H H H Calculate the energy released when 0.32 g of methane is burned. [2] ideas of bond breaking and bond forming to explain why the reaction is exothermic. [3] Name the products of the incomplete combustion of methane. [1] (d) (e) Draw the dot and cross diagram to show all the electrons in a molecule of methane. [2] Give either the names or the structural formulae of two products of the reaction between chlorine and methane. [2] 5070/2 S00 [Turn over

10 B9 Some information about four elements, W, X, Y and Z is shown in the table. 10 element W X Y Z number of electrons in outer shell density in g/cm melting point in C atomic radius in pm ions formed W 4+ X + and X 2+ Y + Z 2+ and Z 4+ formulae and appearance of chlorides WCl 4 - a colourless liquid XCl - a white solid XCl 2 - a green solid YCl - a white solid ZCl 2 - a white solid ZCl 4 - a colourless liquid Y reacts with dilute sulphuric acid to give hydrogen. Construct the equation for this reaction. [1] Which one of the elements is a transition element? Give three pieces of evidence from the table to support your answer. [3] Copper and iron are transition elements. (i) Describe the bonding in metals. [2] (ii) Explain, in terms of metallic bonding, why copper and iron are good electrical conductors and are malleable. [2] (d) Compare the action of steam on copper and on iron. [2] B10 Fats and oils are compounds formed by the reaction between carboxylic acids and an alcohol. The general formula for a saturated carboxylic acid is C n H 2n+1 COOH. What type of compound are fats and oils? [1] A diet containing unsaturated fats is healthier than one containing only saturated fats. (i) (ii) (iii) What is the meaning of the term unsaturated? Suggest a chemical test that could be used to show whether a fat is saturated or unsaturated. Name the reagent used and state the observations that would be made with the unsaturated and the saturated fat. Are fats made from stearic acid, C 17 H 35 COOH, or oleic acid, C 17 H 33 COOH, more healthy in your diet? Explain your answer. [6] Describe how soaps are manufactured from fats. [2] (d) Name a synthetic polymer that contains the same linkage as a fat. [1] 5070/2 S00

11 B11 Diamond and silicon carbide are both macromolecules. Part of the structure of silicon carbide is shown below. 11 C C C Si C (i) State one difference between the structures of silicon carbide and diamond. (ii) State one similarity between the structures of silicon carbide and diamond. [2] Suggest two physical properties of silicon carbide. [2] Silicon carbide is manufactured by the reduction of silicon dioxide with carbon. SiO 2 + 3C 2CO + SiC (i) State one source of silicon dioxide. (ii) What mass of carbon is needed to make 20 tonnes of silicon carbide? [4] (d) Silicones are polymers that contain the elements silicon, oxygen, carbon and hydrogen. Suggest the names of three combustion products of a silicone polymer. [2] 5070/2 S00 [Turn over

12 12 DATA SHEET The Periodic Table of the Elements Group I II III IV V VI VII H Hydrogen 2 4 He Helium 3 7 Li Lithium 4 9 Be Beryllium 5 11 B Boron 6 12 C Carbon 7 14 N Nitrogen 8 16 O Oxygen 9 19 F Fluorine Ne Neon Na Sodium Mg Magnesium Al Aluminium Si Silicon P Phosphorus S Sulphur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium 96 Mo Molybdenum Tc Technetium Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Caesium Fr Francium Ba Barium 226 Ra Radium 139 La Lanthanum 57 * 227 Ac Actinium Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth 84 Po Polonium 85 At Astatine 86 Rn Radon *58-71 Lanthanoid series Actinoid series Key b a X a = relative atomic mass X = atomic symbol b = proton (atomic) number Ce Cerium 232 Th Thorium 141 Pr Praseodymium 59 Pa Protactinium Nd Neodymium 238 U Uranium Pm Promethium Np Neptunium Sm Samarium Pu Plutonium Eu Europium Am Americium Gd Gadolinium Cm Curium Tb Terbium Bk Berkelium Dy Dysprosium Cf Californium Ho Holmium Es Einsteinium Er Erbium Fm Fermium Tm Thulium Md Mendelevium Yb Ytterbium No Nobelium Lu Lutetium Lr Lawrencium 103 The volume of one mole of any gas is 24 dm 3 at room temperature and pressure (r.t.p.) /2 S00

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