Cambridge International Examinations Cambridge Ordinary Level

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1 ambridge International Examinations ambridge rdinary Level EMISTRY 5070/12 Paper 1 Multiple hoice ctober/november 2015 dditional Materials: RE TESE INSTRUTINS FIRST Multiple hoice nswer Sheet Soft clean eraser Soft pencil (type or recommended) 1 hour Write in soft pencil. o not use staples, paper clips, 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. NT WRITE IN NY RES. 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 15 printed pages and 1 blank page. I15 11_5070_12_3/FP ULES 2015 [Turn over

2 1 The diagram shows the fractional distillation of an aqueous solution of ethanol. 2 water out cold water in ethanol ethanol and water heat Which statement explains why ethanol is collected as the distillate? Ethanol has a higher boiling point than water. Ethanol has a higher melting point than water. Ethanol has a lower boiling point than water. Ethanol has a lower melting point than water. 2 In a titration between an acid (in the burette) and an alkali, you may need to re-use the same titration flask. Which is the best procedure for rinsing the flask? Rinse with distilled water and then with the alkali. Rinse with tap water and then with distilled water. Rinse with tap water and then with the acid. Rinse with the alkali. ULES /12//N/15

3 3 3 Which statements are correct? 1 The volume of a gas at constant pressure increases as the temperature increases. 2 The rate of diffusion of a gas increases as the temperature increases. 3 The pressure of a gas at constant volume decreases as the temperature increases. 1 and 2 only 1 and 3 only 2 and 3 only 1, 2 and 3 4 colourless solution is known to contain a sodium salt. Tests were carried out to determine the identity of the anion in the solution. test observation dilute hydrochloric acid dilute nitric acid followed by aqueous silver nitrate dilute nitric acid followed by aqueous barium nitrate no reaction no precipitate no precipitate Which anion could the solution contain? carbonate chloride nitrate sulfate 5 Which physical changes are both exothermic? condensation and evaporation evaporation and melting freezing and condensation melting and freezing ULES /12//N/15 [Turn over

4 4 6 The following data may refer to the atom or to the ion of the same element. electronic configuration 2,8,8 nucleon number 40 proton number 20 Which element is described by these data? argon calcium chlorine neon 7 molecule of sulfuric acid has the structural formula shown. S ow many electrons are involved in forming all the covalent bonds in one molecule? metal consists of a lattice of positive ions in a sea of electrons. What happens to the electrons and positive ions in a metal wire when an electric current is passed through it? electrons positive ions replaced by new electrons replaced by new ions replaced by new electrons unchanged unchanged replaced by new ions unchanged unchanged ULES /12//N/15

5 9 The apparatus shown is set up to plate a steel key with copper. 5 + copper steel key aqueous copper(ii) sulfate The key does not get coated with copper. Which change needs to be made to plate the key? Increase the concentration of the aqueous copper(ii) sulfate. Increase the voltage. Replace the solution with dilute sulfuric acid. Reverse the electrical connections. 10 What is the number of moles of hydrogen atoms in 3.2 g of methane? The formula of the gas ozone is 3. What is the volume of 48 g of ozone at r.t.p.? 16 dm 3 24 dm 3 36 dm 3 72 dm 3 12 Which substance, when added to pure water, will produce a solution which conducts electricity? calcium chloride graphite iron sugar ULES /12//N/15 [Turn over

6 13 Two gases, X and Y, react together to form a gas Z, as shown. 6 X(g) + 3Y(g) 2Z(g) = 92 kj / mol Which change in condition will both increase the rate of reaction and increase the equilibrium yield of Z? decrease concentration of X increase pressure increase temperature use a catalyst 14 solution of sodium carbonate was added to tap water. white precipitate formed. Which ion present in the tap water caused the precipitate to form? chloride magnesium potassium sulfate 15 In which reaction is nitric acid acting as an oxidising agent? u + 4N 3 u(n 3 ) N 2 u + 2N 3 u(n 3 ) Na N 3 2NaN Na + N 3 NaN Which reaction does not involve neutralisation? 2 S 4 (aq) + 2N 3 (aq) (N 4 ) 2 S 4 (aq) 2 S 4 (aq) + al 2(aq) as 4 (s) + 2l (aq) 2 S 4 (aq) + u(s) us 4 (aq) + 2 (l) 2 S 4 (aq) + 2Na(aq) Na 2 S 4 (aq) (l) ULES /12//N/15

7 17 Which pair of substances reacts to form a salt and water only? 7 aqueous sodium chloride and aqueous silver nitrate aqueous sodium hydroxide and dilute ethanoic acid aqueous sodium carbonate and dilute sulfuric acid zinc and dilute hydrochloric acid 18 Iron is obtained in the blast furnace from the ore haematite. Which reaction takes place in the blast furnace? alcium carbonate is used to remove acidic impurities. oke is reduced to carbon dioxide. aematite is oxidised by carbon monoxide. aematite undergoes thermal decomposition. 19 luminium is manufactured from aluminium oxide by electrolysis. The compound cryolite is used in this process. Which statement about cryolite is correct? It is the common name for aluminium oxide. It is used to dissolve the aluminium oxide. It is used to make the positive electrode. It is used to make the negative electrode. 20 n element is burned in an excess of oxygen. Which statement about the oxide formed is always correct? The mass of oxide formed is greater than the mass of element burned. The oxide formed is a crystalline solid. The oxide formed is soluble in water. The oxide formed is white in colour. 21 Which statement about the Periodic Table is correct? Elements are arranged in order of decreasing proton number. Group number is the number of electron shells in atoms of the elements in the group. Group numbers can be used to predict the charges of ions. Metallic character increases left to right across a period. ULES /12//N/15 [Turn over

8 22 Which negative ions are present in aqueous copper(ii) sulfate? 8 copper(ii) ions and hydrogen ions copper(ii) ions only sulfate ions and hydroxide ions sulfate ions only 23 The reaction shown for the aber process can reach equilibrium. N 2 (g) (g) 2N 3 (g) Which row shows the gases present at equilibrium? nitrogen hydrogen ammonia no no yes no yes yes yes no yes yes yes yes 24 Which statement about graphite is not correct? It burns to form carbon dioxide. It is a carbon compound. It is a giant molecular substance. It is used as a lubricant. ULES /12//N/15

9 25 The energy profile diagram for a reaction is shown. 9 3 energy 2 products 1 reactants progress of reaction Which statement is correct? The activation energy of the reaction is ( 3 1 ). The activation energy of the reaction is ( 3 2 ). is ( 1 2 ). is ( 1 3 ). 26 The Periodic Table shows the positions of elements,, and. These are not the usual symbols of these elements. Which element has a high melting point and can be used as a catalyst? I II III IV V VI VII 0 27 Which of the statements about iron and steel is not correct? oth iron and steel conduct electricity. Mild steel is used in car bodies. Pure iron is formed in the blast furnace. The addition of carbon to mild steel makes it stronger. ULES /12//N/15 [Turn over

10 10 28 Some reactions are shown. 1 2S S Which of these reactions use a catalyst when carried out industrially? 1 only 1 and 2 only 2 and 3 only 1, 2 and 3 29 Which change is endothermic? 4 (g) (g) 2 (g) (l) (g) + l (g) l (g) 2 (g) 2(g) + (g) 2 (l) 2 (s) 30 Which two elements are the major constituents of brass? r and s u and Sn u and Zn Sn and Zn 31 Two statements about copper are given. 1 opper is below hydrogen in the reactivity series. 2 opper can be obtained by heating its oxide with carbon. Which statements are correct? both 1 and 2 1 only 2 only neither 1 nor 2 32 What is the order of reactivity of the halogens? most reactive least reactive bromine chlorine iodine chlorine bromine iodine iodine bromine chlorine iodine chlorine bromine ULES /12//N/15

11 33 The flow chart shows how impure water can be treated to produce drinkable water. 11 impure water pass through large-sized gravel pass through small-sized gravel pass through carbon pass chlorine through it drinkable water What is not removed from the water by this process? clay particles microbes nitrates odours 34 Which diagram shows the isomer of butane? ULES /12//N/15 [Turn over

12 35 The diagram shows the structure of a monomer used to make a polymer What is the structure of the polymer? Which property of a liquid ester can be used to check its purity before use as a food flavouring? boiling point colour smell solubility in water ULES /12//N/15

13 37 The structures of three hydrocarbons from the same homologous series are shown. 13 W X Y Which statement is correct? ll three molecules are unsaturated hydrocarbons. ll three molecules have the same empirical formula. W has the lowest boiling point. X is an isomer of Y. 38 ow many of the following statements about ethanol are correct? 1 molecular formula is manufactured from ethane and steam 3 oxidises to ethanoic acid 4 produced by the fermentation of glucose 5 used as a fuel 6 used as a solvent Proteins and nylon both possess the same amide linkages. Which arrangement of atoms represents an amide linkage? N N N ULES /12//N/15 [Turn over

14 14 40 carbohydrate such as starch can be represented as shown. X X X X What is X? carbon hydrogen nitrogen oxygen ULES /12//N/15

15 15 LNK PGE ULES /12//N/15

16 16 T SEET The Periodic Table of the Elements Group I II III IV V VI VII ydrogen 2 4 e elium 3 7 Li Lithium 4 9 e eryllium 5 11 oron 6 12 arbon 7 14 N Nitrogen 8 16 xygen 9 19 F Fluorine Ne Neon Na Sodium 24 Mg Magnesium l luminium Si Silicon 31 P Phosphorus S Sulfur l hlorine r rgon K Potassium a alcium Sc Scandium Ti Titanium V Vanadium r hromium 55 Mn Manganese Fe Iron o obalt Ni Nickel u opper Zn Zinc Ga Gallium 73 Ge Germanium s rsenic Se Selenium r romine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium 96 Mo Molybdenum 42 Tc Technetium Ru Ruthenium Rh Rhodium Pd Palladium g Silver d admium In Indium Sn Tin Sb ntimony Te Tellurium I Iodine Xe Xenon s aesium Fr Francium a arium 226 Ra Radium 139 La Lanthanum 57 * c ctinium f afnium Ta Tantalum W Tungsten Re Rhenium s smium Ir Iridium Pt Platinum u Gold g Mercury Tl Thallium Pb Lead i ismuth 84 Po Polonium 85 t statine 86 Rn Radon *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 162 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.). To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the ambridge International Examinations opyright cknowledgements ooklet. This is produced for each series of examinations and is freely available to download at after the live examination series. ULES /12//N/15