UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Ordinary Level

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1 * * UNIVERSITY OF MRIGE INTERNTIONL EXMINTIONS General ertificate of Education Ordinary Level EMISTRY 5070/11 Paper 1 Multiple hoice May/June 2013 dditional Materials: Multiple hoice nswer Sheet Soft clean eraser Soft pencil (type or is recommended) 1 hour RE TESE INSTRUTIONS FIRST Write in soft pencil. o not use staples, paper clips, highlighters, glue or correction fluid. Write your name, entre number and candidate number on the nswer Sheet in the spaces provided unless this has been done for you. O NOT WRITE IN NY ROES. There are forty questions on this paper. nswer all questions. For each question there are four possible answers,, and. hoose the one you consider correct and record your choice in soft pencil on the separate nswer Sheet. Read the instructions on the nswer Sheet very carefully. Each correct answer will score one mark. mark will not be deducted for a wrong answer. ny rough working should be done in this booklet. copy of the Periodic Table is printed on page 16. Electronic calculators may be used. This document consists of 13 printed pages and 3 blank pages. I13 06_5070_11/4RP ULES 2013 [Turn over

2 1 In which method of separation are R f values used? 2 chromatography crystallisation filtration fractional distillation 2 The diagrams show the arrangement of particles in three solids: krypton, potassium and sodium chloride e e e e e e In which order are the solids shown? krypton; potassium; sodium chloride krypton; sodium chloride; potassium sodium chloride; krypton; potassium sodium chloride; potassium; krypton 3 In which pair do neither of the gases change the colour of damp blue litmus paper? ammonia and hydrogen ammonia and hydrogen chloride carbon dioxide and chlorine carbon dioxide and sulfur dioxide 4 Naturally-occurring bromine has a relative atomic mass of 80 and consists entirely of two isotopes of relative atomic masses 79 and 81. What can be deduced about naturally-occurring bromine from this information only? romine contains the two isotopes in equal proportions. romine has different oxidation states. romine isotopes have different numbers of protons. romine is radioactive. 5 Which compound has molecules each of which contains only two covalent bonds? 4 2 O Mgl 2 Na 2 O ULES /11/M/J/13

3 6 What can be deduced about two gases that have the same relative molecular mass? 3 They have the same boiling point. They have the same number of atoms in one molecule. They have the same rate of diffusion at room temperature and pressure. They have the same solubility in water at room temperature. 7 n ionic bond is formed by electron sharing between metals and non-metals. electron sharing between non-metals. electron transfer between non-metals. electron transfer from metals to non-metals. 8 oth magnesium oxide, MgO, and aluminium oxide, l 2O 3, are solids at room temperature, 25. MgO has a melting point of 2852 and a boiling point of l 2O 3 has a melting point of 2072 and a boiling point of Over which temperature range will both pure compounds conduct electricity? 25 to to to to Which substance conducts an electric current but remains chemically unchanged? aluminium aqueous sodium chloride molten lead(ii) bromide pure ethanoic acid 10 Which statement most clearly indicates that diamond and graphite are forms of carbon? oth are crystalline solids. omplete combustion of equal masses of both solids produces equal masses of carbon dioxide as the only product. Graphite conducts electricity whereas diamond is an insulator. Under suitable conditions graphite can be partially converted into diamond. ULES /11/M/J/13 [Turn over

4 4 11 In an experiment, 1 cm 3 of a gaseous hydrocarbon X required 4 cm 3 of oxygen for complete combustion to give 3 cm 3 of carbon dioxide. ll gas volumes are measured at r.t.p. Which formula represents X? What is the concentration of a solution containing 1.0 g of sodium hydroxide in 250 cm 3 of solution? mol / dm mol / dm mol / dm mol / dm 3 13 The diagrams show an electrolysis experiment using inert electrodes. liquid Y + + before electrolysis after electrolysis Which could be liquid Y? aqueous copper(ii) sulfate concentrated aqueous sodium chloride dilute sulfuric acid ethanol ULES /11/M/J/13

5 5 14 Which substance, when added to water, does not make a solution that is a good conductor of electricity? barium nitrate calcium chloride lead(ii) nitrate zinc carbonate 15 simple cell is shown below. voltmeter V zinc electrode copper electrode electrolyte Which statement about the process occurring when the cell is in operation is correct? u 2+ ions are formed in solution. Electrons travel through the solution. The reaction Zn Zn e occurs. Zinc increases in mass. 16 The usual conditions for the aber process are 250 atm pressure, 450 and an iron catalyst. Which change in conditions would give the reactants more energy? addition of more catalyst a decrease in pressure an increase in concentration of the reactants an increase in temperature ULES /11/M/J/13 [Turn over

6 6 17 hlorine can be manufactured by the following reaction. 4l (g) + O 2 (g) 2 2 O(g) + 2l 2(g) is negative mixture in dynamic equilibrium is formed. Which change to the mixture will increase the amount of chlorine at equilibrium? adding a catalyst adding more l (g) decreasing the pressure increasing the temperature 18 Equations for reactions of iron and iron compounds are shown. Fe + 2l Fel Fel 2 + l 2 2Fel 3 FeSO 4 + Mg Fe + MgSO 4 FeSO 4 + 2NaO Fe(O) 2 + Na 2 SO 4 ow many of these are redox reactions? Which is a use of sulfuric acid? as a bleach in the manufacture of ammonia in the manufacture of fertilisers in the manufacture of sulfur trioxide ULES /11/M/J/13

7 20 The table shows the solubility of some compounds of metal Q in cold water. 7 salt carbonate chloride sulfate solubility in cold water insoluble soluble insoluble What is metal Q? barium lead magnesium sodium 21 metal M forms a chloride which dissolves in cold water and has an oxide which dissolves in both strong acids and strong alkalis. What is M? iron lead sodium zinc 22 Which element has a variable oxidation state, can act as a catalyst and forms coloured compounds? carbon iron lead nitrogen 23 n atom of which element has the same electronic configuration as the strontium ion? calcium krypton rubidium selenium ULES /11/M/J/13 [Turn over

8 24 The boiling points of gaseous elements increase as the size of their atoms increases. Which of these noble gases has the highest boiling point? 8 argon helium krypton neon 25 The sentence describes two metals and their oxides. Metal X could be copper because its oxide is 1 and metal Y could be 2 because its oxide is amphoteric. Which words correctly complete gaps 1 and 2? 1 2 acidic aluminium basic aluminium acidic magnesium basic magnesium 26 Which gas could be used to convert copper(ii) oxide to copper? carbon dioxide hydrogen nitrogen oxygen 27 luminium and copper are often used to make coins but iron is not. Which statement explains this? Iron is above both aluminium and copper in the reactivity series. Iron is more expensive to manufacture than aluminium or copper. Iron is rarer than both aluminium and copper. Iron reacts with water. ULES /11/M/J/13

9 9 28 In the electrolysis of molten aluminium oxide for the extraction of aluminium, the following three reactions take place. 1 l e l 2 2O 2 O 2 + 4e 3 + O 2 O 2 Which reactions take place at the positive electrode? 1 only 2 only 1 and 3 only 2 and 3 only 29 Which two substances are removed from the bottom of the blast furnace? 1 coke 2 iron 3 limestone 4 slag 1 and 3 1 and 4 2 and 3 2 and 4 30 n alloy of copper and zinc is added to an excess of dilute hydrochloric acid. The resulting mixture is then filtered. Which observations are correct? filtrate residue colourless solution none colourless solution red-brown blue solution grey blue solution none 31 Which aqueous reagent liberates ammonia from ammonium nitrate on warming? calcium nitrate potassium hydroxide sodium chloride sulfuric acid ULES /11/M/J/13 [Turn over

10 10 32 n aqueous solution of a compound X reacts with aqueous zinc chloride to form a white precipitate which dissolves when X is in excess, aluminium sulfate solution to form a white precipitate which is insoluble when X is in excess. What is the identity of X? ammonia barium chloride silver nitrate sodium hydroxide 33 F compounds were commonly used as aerosol propellants. The structure of one F compound is shown. F l F F Which element in this compound causes a depletion of ozone in the atmosphere? carbon chlorine fluorine hydrogen 34 Which gas is most likely to react with limestone? ammonia carbon monoxide methane sulfur dioxide ULES /11/M/J/13

11 11 35 The diagram shows the structure of an ester. O O What are the starting materials for making this compound? butanol and butanoic acid butanol and propanoic acid propanol and butanoic acid propanol and propanoic acid 36 Which information is correct regarding the formation of ethanol by the process of fermentation? substances fermented gas evolved during fermentation carbohydrates carbon dioxide carbohydrates carbon monoxide hydrocarbons carbon dioxide hydrocarbons carbon monoxide 37 Nylon, poly(ethene) and Terylene are macromolecules. In which of these macromolecules is the =O group present in the linkage? nylon and Terylene only nylon only poly(ethene) and Terylene only Terylene only ULES /11/M/J/13 [Turn over

12 12 38 Which partial structure is correct for the product of polymerisation of butene, 2 = 2 3? n n 3 n 3 n 39 Glucose is a simple sugar. Glycine is an amino acid. In the diagram, which two arrows correctly show the hydrolysis products of a carbohydrate and of a protein? a carbohydrate 1 glucose 2 3 a protein 4 glycine 1 and 3 1 and 4 2 and 3 2 and 4 40 When crude oil is distilled several products are obtained. What is the correct order of their boiling points? highest boiling point lowest boiling point diesel paraffin (kerosene) petrol (gasoline) lubricating oil lubricating oil diesel paraffin (kerosene) petrol (gasoline) paraffin (kerosene) petrol (gasoline) lubricating oil diesel petrol (gasoline) paraffin (kerosene) diesel lubricating oil ULES /11/M/J/13

13 13 LNK PGE ULES /11/M/J/13

14 14 LNK PGE ULES /11/M/J/13

15 15 LNK PGE ULES /11/M/J/13

16 16 T SEET The Periodic Table of the Elements Group I II III IV V VI VII e ydrogen elium Li e N O F Ne Lithium eryllium oron arbon Nitrogen Oxygen Fluorine Neon Na Mg l Si P S l r Sodium Magnesium luminium Silicon Phosphorus Sulfur hlorine rgon K a Sc Ti V r Mn Fe o Ni u Zn Ga Ge s Se r Kr Potassium alcium Scandium Titanium Vanadium hromium Manganese Iron obalt Nickel opper Zinc Gallium Germanium rsenic Selenium romine Krypton Rb Sr Y Zr Nb Mo Tc Ru Rh Pd g d In Sn Sb Te Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver admium Indium Tin ntimony Tellurium Iodine Xenon I Xe s a La f Ta W Re Os Ir Pt u g Tl Pb i Po t Rn aesium arium Lanthanum afnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thallium Lead ismuth Polonium statine Radon * Fr Ra c Francium Radium ctinium *58-71 Lanthanoid series ctinoid series Key b a X a = relative atomic mass X = atomic symbol b = proton (atomic) number e erium 232 Th Thorium 141 Pr Praseodymium 59 Pa Protactinium Nd Neodymium U Uranium Pm Promethium Np Neptunium Sm Samarium Pu Plutonium Eu Europium m mericium Gd Gadolinium m urium Tb Terbium k erkelium y ysprosium f alifornium o olmium 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.). Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (ULES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. University of ambridge International Examinations is part of the ambridge ssessment Group. ambridge ssessment is the brand name of University of ambridge Local Examinations Syndicate (ULES), which is itself a department of the University of ambridge. ULES /11/M/J/13