Soft clean eraser Soft pencil (type B or HB is recommended)

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1 * * ambridge International Examinations ambridge Ordinary Level EMISTRY 5070/11 Paper 1 Multiple hoice May/June 2016 Additional Materials: Multiple hoice Answer Sheet Soft clean eraser Soft pencil (type B or B is recommended) 1 hour READ TESE INSTRUTIONS FIRST Write in soft pencil. Do not use staples, paper clips, glue or correction fluid. Write your name, entre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you. DO NOT WRITE IN ANY BARODES. There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, and D. hoose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet. Read the instructions on the Answer Sheet very carefully. Each correct answer will score one mark. A mark will not be deducted for a wrong answer. Any rough working should be done in this booklet. A copy of the Periodic Table is printed on page 16. Electronic calculators may be used. This document consists of 14 printed pages and 2 blank pages. IB16 06_5070_11/4RP ULES 2016 [Turn over

2 2 1 Which oxide is amphoteric? A Al 2O 3 B O 2 Na 2 O D SO 2 2 Four gas jars each contain one of the gases ammonia, chlorine, hydrogen chloride and oxygen. A strip of damp blue litmus paper and a strip of damp red litmus paper are placed in each jar. In which gas jar will both the damp blue litmus paper and the damp red litmus paper change colour? A B ammonia chlorine red litmus blue litmus red litmus blue litmus D hydrogen chloride oxygen red litmus blue litmus red litmus blue litmus 3 ow can a pure sample of barium sulfate be obtained from barium carbonate? A B D Dissolve it in dilute hydrochloric acid, add dilute sulfuric acid, filter and crystallise. Dissolve it in dilute hydrochloric acid, add dilute sulfuric acid, filter and wash. Dissolve it in water, add dilute sulfuric acid, filter and crystallise. Dissolve it in water, add dilute sulfuric acid, filter and wash. 4 Which statement is not correct? A B D Energy is released when a liquid changes into a solid. Particles move faster in the gaseous state than in the liquid state. The carbon atoms in gaseous methane are further apart than those in solid diamond. There is a large decrease in the volume of a solid metal when pressure is applied to it. ULES /11/M/J/16

3 3 5 The symbols for two ions are shown. 19 F 21 9 Na + 11 Which statement is correct? A B D The fluoride ion contains more electrons than the sodium ion. The sodium ion contains more neutrons than the fluoride ion. The two ions contain the same number of electrons as each other. The two ions contain the same number of protons as each other. 6 Which dot-and-cross diagram, showing all the outer shell electrons of each atom, is not correct? A B D l O O 7 Which statement shows that graphite and diamond are different forms of the element carbon? A B D Both graphite and diamond have giant molecular structures. omplete combustion of equal masses of graphite and diamond produces equal masses of carbon dioxide and no other products. Graphite and diamond have different melting points. Graphite conducts electricity, whereas diamond does not. 8 In order to form a compound with oxygen, an atom of a Group II element must A B D transfer two electrons to an atom of oxygen. receive two electrons from an atom of oxygen. share two electrons with an atom of oxygen. bond with two atoms of oxygen. ULES /11/M/J/16 [Turn over

4 9 opper wire is used to complete an electrical circuit. 4 copper wire lamp What happens in the copper wire? A B Electrons move along the wire to the negative terminal. Positive ions stay in position. Electrons move along the wire to the positive terminal. Positive ions move to the negative terminal. Electrons move along the wire to the positive terminal. Positive ions stay in position. D Negative ions move along the wire to the positive terminal. Positive ions move to the negative terminal. 10 Which uses for sulfuric acid are correct? 1 as a bleach in the manufacture of wood pulp for paper 2 as a food preservative in tinned foods 3 as a raw material in the manufacture of detergents 4 as a fertiliser A 1 and 3 B 2 and 4 2 only D 3 only 11 Group I metals form compounds with Group VII halogens. The compounds formed are 1 in water and contain 2 bonds. Which words correctly complete gaps 1 and 2? 1 2 A insoluble covalent B insoluble ionic soluble covalent D soluble ionic ULES /11/M/J/16

5 12 ompound P is the only substance formed when two volumes of ammonia gas react with one volume of carbon dioxide gas (both volumes being measured at r.t.p.). What is the formula of P? A N 2 O 2 N 4 5 B (N 2 ) 2 O N 4 O 2 N 4 D (N 4 ) 2 O 3 13 Two isotopes of chlorine are 35 l and 37 l. Using these isotopes, how many different relative molecular masses are possible for the compound with molecular formula 2 3 l 3? A 2 B 3 4 D 5 14 Gases can diffuse through porous pots. The diagram shows a beaker full of nitrogen inverted over a porous pot containing carbon monoxide. beaker nitrogen porous pot carbon monoxide water The water level does not move. Which statement explains this? A B D Nitrogen is almost inert. The two gases have equal molecular masses. Both gases have two atoms in a molecule. Neither gas is soluble in water. ULES /11/M/J/16 [Turn over

6 6 15 Aqueous copper(ii) sulfate is electrolysed using carbon electrodes. Which observations will be made? at the positive electrode electrolyte at the negative electrode A colourless gas forms blue colour fades pink solid forms B colourless gas forms no change colourless gas forms electrode decreases in mass blue colour fades colourless gas forms D electrode decreases in mass no change pink solid forms 16 Which ion is not present in dilute sulfuric acid? A + B O SO 3 2 D SO The diagram shows an energy profile diagram for a chemical reaction, both with and without a catalyst. Which energy change is the activation energy for the catalysed reaction? energy A B reactants D products reaction pathway 18 Which equation does not represent a redox reaction? A 2N SO 4 (N 4 ) 2 SO 4 B 2SO 2 + O 2 2SO 3 2KI + l 2 2Kl + I 2 D Zn + 2 SO 4 ZnSO ULES /11/M/J/16

7 7 19 The diagram shows the apparatus used to measure the rate of the reaction between calcium carbonate and dilute hydrochloric acid. The mass of the flask and the contents is measured at regular intervals of time. cotton wool dilute hydrochloric acid calcium carbonate balance Which graph correctly shows how the mass of the flask and contents changes with time? A B D mass mass mass mass time 0 time 0 time 0 time 20 Which row correctly compares high carbon steels and low carbon steels? high carbon steels low carbon steels A stronger more brittle B stronger more easily shaped weaker more brittle D weaker more easily shaped 21 Which process does not involve the use of a catalyst? A B D the extraction of iron from haematite in a blast furnace the manufacture of sulfur trioxide the production of ammonia from nitrogen and hydrogen the redox reactions that remove combustion pollutants from car exhausts ULES /11/M/J/16 [Turn over

8 8 22 Gaseous compound X is an oxidising agent. X is bubbled through separate solutions of aqueous potassium iodide and acidified potassium manganate(vii). X X aqueous potassium iodide acidified potassium manganate(vii) Which row shows the colour changes when X is bubbled through these two solutions? aqueous potassium iodide acidified potassium manganate(vii) A brown to colourless no change B brown to colourless purple to colourless colourless to brown no change D colourless to brown purple to colourless 23 Which metal oxide will be reduced by heating with iron? A B D calcium oxide lead oxide magnesium oxide zinc oxide 24 Which pair of substances can be used to prepare a sample of lead(ii) chloride when added to water and mixed? A B D lead and sodium chloride lead(ii) nitrate and sodium chloride lead(ii) carbonate and sodium chloride lead and hydrochloric acid 25 The p of an aqueous solution of hydrochloric acid is 2. What will be the p of the acid after the addition of 10 g of sodium chloride? A 1 B 2 7 D 9 ULES /11/M/J/16

9 26 Which statement about the elements in the Periodic Table is correct? 9 A B All the elements in the same group of the Periodic Table have the same reactivity. All the elements with four electrons in their outer shells are metals. An element in Group II of the Periodic Table would form an ion with a 2 charge. D Elements in the same period of the Periodic Table have the same number of shells of electrons. 27 Iron is extracted from haematite in the blast furnace. waste gases raw materials air molten iron Which other raw material is added in this extraction? A B D bauxite cryolite limestone slag ULES /11/M/J/16 [Turn over

10 28 The diagram shows a flow chart for the manufacture of fertiliser. 10 fractional distillation of air gas W pressure Y and 450 product Z fertiliser cracking of hydrocarbons gas X In the flow chart, what are W, X, Y and Z? W X Y Z A 2 N 2 high N 3 B O 2 SO 2 high SO 3 O 2 SO 2 low SO 3 D N 2 2 high N 3 29 The table gives the melting points, densities and electrical conductivities of four elements. Which element is copper? melting point in density in g / cm 3 electrical conductivity A good B poor good D good 30 Which gases are all present at the positive electrode during the manufacture of aluminium? A O, 2, O 2 B O, SO 2, 2 O O 2, O, O 2 D SO 2, 2, O 2 ULES /11/M/J/16

11 11 31 The diagram shows the structure of brass. zinc atom copper atom Why is brass harder than pure copper? A B D The zinc atoms form strong covalent bonds with copper atoms. The zinc atoms prevent layers of copper atoms from sliding over each other easily. The zinc atoms prevent the sea of electrons from moving freely in the solid. Zinc atoms have more electrons than copper atoms. 32 Which pollutant causes eutrophication in rivers? A B D acid rain carbon monoxide fertiliser metal compounds 33 ow many moles of hydrogen chloride are formed when one mole of methane reacts with a large excess of chlorine in sunlight? A 1 B 2 3 D 4 ULES /11/M/J/16 [Turn over

12 12 34 Which statements about alcohols are correct? 1 All alcohols contain the hydroxide ion, O. 2 Ethanol can be formed from ethene using a reaction catalysed by yeast. 3 Methanol can be oxidised to methanoic acid. 4 The alcohols X and Y shown are isomers. X Y O O A 1 and 2 B 1 and 3 2 and 4 D 3 and 4 35 Amino acids are essential building blocks in the human body. Macromolecules in food are hydrolysed to form amino acids. Which macromolecules provide the body with amino acids? A B D carbohydrates fats proteins sugars 36 Ethanol, 2 6 O, was reacted with propanoic acid, 3 6 O 2, in the presence of concentrated sulfuric acid. Which statement about the organic product of this reaction is correct? A It has the formula 5 10 O 2. B It has the formula 5 12 O 3. D It is formed by an addition reaction. It is propyl ethanoate. 37 ow can alkenes be manufactured? A B D by polymerisation reactions by the addition of hydrogen to unsaturated vegetable oils by the combustion of alkanes by the cracking of hydrocarbons ULES /11/M/J/16

13 13 38 Which statement about alkanes is correct? A B Ethane reacts with chlorine in an addition reaction. Propane has a higher boiling point than butane. The molecule of the alkane that contains 99 carbon atoms has 200 hydrogen atoms. D There are three isomers with the formula Which statement about ethanoic acid is correct? A B Ethanoic acid can be made by the catalysed addition of steam to ethene. Propanoic acid can react with ethanoic acid to produce an ester. Solutions of 1.0 mol / dm 3 ethanoic acid and 1.0 mol / dm 3 hydrochloric acid will react with magnesium at equal rates. D The formula of ethanoic acid is 3 O Polymer Z has the structure shown. O O O O N N N N These four terms can be used to describe polymers. 1 addition polymer 2 condensation polymer 3 polyamide 4 polyester Which two terms can be applied to polymer Z? A 1 and 3 B 1 and 4 2 and 3 D 2 and 4 ULES /11/M/J/16

14 14 BLANK PAGE ULES /11/M/J/16

15 15 BLANK PAGE 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. To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the ambridge International Examinations opyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at after the live examination series. ambridge International Examinations is part of the ambridge Assessment Group. ambridge Assessment 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/16

16 16 ULES /11/M/J/16 Group The Periodic Table of Elements 1 hydrogen 1 2 e helium 4 I II III IV V VI VII VIII 3 Li lithium 7 4 Be beryllium 9 atomic number atomic symbol Key name relative atomic mass 11 Na sodium Mg magnesium K potassium a calcium Rb rubidium Sr strontium s caesium Ba barium Fr francium 88 Ra radium 5 B boron Al aluminium Ga gallium In indium Tl thallium carbon Si silicon Ge germanium Sn tin Pb lead Ti titanium Zr zirconium f hafnium Rf rutherfordium 23 V vanadium Nb niobium Ta tantalum Db dubnium 24 r chromium Mo molybdenum W tungsten Sg seaborgium 25 Mn manganese Tc technetium 75 Re rhenium Bh bohrium 26 Fe iron Ru ruthenium Os osmium s hassium 27 o cobalt Rh rhodium Ir iridium Mt meitnerium 28 Ni nickel Pd palladium Pt platinum Ds darmstadtium 29 u copper Ag silver Au gold Rg roentgenium 30 Zn zinc d cadmium g mercury n copernicium 114 Fl flerovium 116 Lv livermorium 7 N nitrogen P phosphorus As arsenic Sb antimony Bi bismuth O oxygen S sulfur Se selenium Te tellurium Po polonium 9 F fluorine l chlorine Br bromine I iodine At astatine 10 Ne neon Ar argon Kr krypton Xe xenon Rn radon 21 Sc scandium Y yttrium lanthanoids actinoids 57 La lanthanum Ac lanthanoids actinoids The volume of one mole of any gas is 24 dm 3 at room temperature and pressure (r.t.p.) actinium 58 e cerium Th thorium Pr praseodymium Pa protactinium Nd neodymium U uranium Pm promethium 93 Np neptunium 62 Sm samarium Pu plutonium 63 Eu europium Am americium 64 Gd gadolinium m curium 65 Tb terbium Bk berkelium 66 Dy dysprosium f californium 67 o holmium Es einsteinium 68 Er erbium Fm fermium 69 Tm thulium Md mendelevium 70 Yb ytterbium No nobelium 71 Lu lutetium Lr lawrencium

17 * * ambridge International Examinations ambridge Ordinary Level EMISTRY 5070/12 Paper 1 Multiple hoice May/June 2016 Additional Materials: Multiple hoice Answer Sheet Soft clean eraser Soft pencil (type B or B is recommended) 1 hour READ TESE INSTRUTIONS FIRST Write in soft pencil. Do not use staples, paper clips, glue or correction fluid. Write your name, entre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you. DO NOT WRITE IN ANY BARODES. There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, and D. hoose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet. Read the instructions on the Answer Sheet very carefully. Each correct answer will score one mark. A mark will not be deducted for a wrong answer. Any rough working should be done in this booklet. A copy of the Periodic Table is printed on page 16. Electronic calculators may be used. This document consists of 16 printed pages. IB16 06_5070_12/4RP ULES 2016 [Turn over

18 2 1 Which row correctly identifies the gas? gas test observation A l 2 damp litmus paper the litmus paper turns blue B N 3 damp litmus paper the litmus paper turns red O 2 limewater no change is observed D SO 2 acidified aqueous potassium manganate(vii) the colour of the solution changes from purple to colourless 2 A student plans two experiments. experiment 1 experiment 2 find the concentration of a solution of sodium hydroxide by titration with dilute hydrochloric acid find the rate of the reaction between pieces of calcium carbonate and dilute hydrochloric acid by measuring the volume of gas given off every minute A flask is provided. Which other apparatus is needed? A experiment 1 experiment 2 balance, measuring cylinder, thermometer gas syringe, clock B burette, pipette balance, measuring cylinder, thermometer burette, pipette gas syringe, clock D gas syringe, clock burette, pipette 3 Q is a pure sample of a substance that has a single R f value of 0.9. In the chromatogram shown, which letter represents Q? solvent front A B D baseline ULES /12/M/J/16

19 4 Which statement about the isotopes of bromine is correct? They are atoms with the same number of 3 A B D electrons and a different number of protons. neutrons and the same number of electrons. protons and the same chemical properties. protons and the same physical properties. 5 ompound Z is made from element X and element Y. ompound Z is a good conductor of electricity when molten but not when solid. Which statement is correct? A B D ompound Z has strong forces of attraction between electrons and positive ions. ompound Z has strong forces of attraction between negative ions and positive ions. Elements X and Y are both metals. Elements X and Y are both non-metals. 6 opper wire is used to complete an electrical circuit. copper wire lamp What happens in the copper wire? A B Electrons move along the wire to the negative terminal. Positive ions stay in position. Electrons move along the wire to the positive terminal. Positive ions move to the negative terminal. Electrons move along the wire to the positive terminal. Positive ions stay in position. D Negative ions move along the wire to the positive terminal. Positive ions move to the negative terminal. ULES /12/M/J/16 [Turn over

20 7 Which statement shows that graphite and diamond are different forms of the element carbon? 4 A B D Both graphite and diamond have giant molecular structures. omplete combustion of equal masses of graphite and diamond produces equal masses of carbon dioxide and no other products. Graphite and diamond have different melting points. Graphite conducts electricity, whereas diamond does not. 8 Ethene, 2 4, is a covalent compound with a simple molecular structure. Which statement about ethene is correct? A B D Ethene is a liquid at room temperature and pressure. Liquid ethene conducts electricity. One ethene molecule contains sixteen protons. The total number of shared pairs of electrons in ethene is five. 9 An organic compound has the molecular formula 8 16 O 4. What is the empirical formula of the compound? A 2 4 O B 4 8 O O 3 D 8 16 O 4 10 ompound P is the only substance formed when two volumes of ammonia gas react with one volume of carbon dioxide gas (both volumes being measured at r.t.p.). What is the formula of P? A N 2 O 2 N 4 B (N 2 ) 2 O N 4 O 2 N 4 D (N 4 ) 2 O 3 ULES /12/M/J/16

21 5 11 Gases can diffuse through porous pots. The diagram shows a beaker full of nitrogen inverted over a porous pot containing carbon monoxide. beaker nitrogen porous pot carbon monoxide water The water level does not move. Which statement explains this? A B D Nitrogen is almost inert. The two gases have equal molecular masses. Both gases have two atoms in a molecule. Neither gas is soluble in water. 12 opper is purified by electrolysis. Which statement is not correct? A B D Both electrodes contain copper. opper is both oxidised and reduced in the process. Pure copper is deposited on the positive electrode. The electrolyte is aqueous copper(ii) sulfate. 13 oncentrated aqueous sodium chloride is electrolysed using inert electrodes until no more chlorine gas is evolved. What could be the p of the resulting solution? A 1 B 4 7 D 11 ULES /12/M/J/16 [Turn over

22 14 Ammonia can be produced industrially from nitrogen and hydrogen. 6 N 2 (g) (g) 2N 3 (g) The forward reaction is exothermic. Which change would not alter the yield of ammonia? A B D adding a catalyst decreasing the pressure decreasing the temperature removing some ammonia during the reaction 15 The diagram shows an energy profile diagram for a chemical reaction, both with and without a catalyst. Which energy change is the activation energy for the catalysed reaction? energy A B reactants D products reaction pathway 16 Oil floats on water. Which statement is not true of oil and water? A B Oil and water are immiscible. Oil is less dense than water. Some molecules in oil have a higher relative molecular mass than water. D The type of bonding within water molecules is different from the type of bonding within molecules in oil. ULES /12/M/J/16

23 17 Which process does not involve the use of a catalyst? 7 A B D the extraction of iron from haematite in a blast furnace the manufacture of sulfur trioxide the production of ammonia from nitrogen and hydrogen the redox reactions that remove combustion pollutants from car exhausts 18 Which statement does not describe a reduction reaction? A B D Electrons are gained during the reaction. ydrogen is gained during the reaction. It takes place at the negative electrode during electrolysis. Oxygen is gained during the reaction. 19 The p of an aqueous solution of hydrochloric acid is 2. What will be the p of the acid after the addition of 10 g of sodium chloride? A 1 B 2 7 D 9 20 One mole samples of each of the solid carbonates of lead, calcium, barium and magnesium are reacted in turn with excess dilute sulfuric acid. excess dilute sulfuric acid solid carbonate Which sample of carbonate will release the greatest volume of carbon dioxide? A B D barium calcium lead magnesium ULES /12/M/J/16 [Turn over

24 21 In which reaction are two of the products salts? 8 A B D aqueous lead(ii) nitrate and aqueous copper(ii) sulfate aqueous sodium hydroxide and solid ammonium sulfate dilute hydrochloric acid and aqueous sodium carbonate dilute hydrochloric acid and magnesium 22 The diagram shows the structure of brass. zinc atom copper atom Why is brass harder than pure copper? A B D The zinc atoms form strong covalent bonds with the copper atoms. The zinc atoms prevent layers of copper atoms from sliding over each other easily. The zinc atoms prevent the sea of electrons from moving freely in the solid. The zinc atoms have more electrons than the copper atoms. 23 From their position in the Periodic Table, which statement is correct? A B D Atoms of elements in Group VII react to form ions by losing one electron. Iodine can displace bromine from its salts. Potassium reacts more rapidly than lithium with water to form the hydroxide and hydrogen. The melting point of caesium is greater than that of potassium. ULES /12/M/J/16

25 9 24 The table gives the melting points, densities and electrical conductivities of four elements. Which element is copper? melting point in density in g / cm 3 electrical conductivity A good B poor good D good 25 An atom of an element has eight electrons only. Which statement about this element is correct? A B D It forms an ion with two negative charges. It has a full outer shell of electrons. It is a metal. It is in Group VIII of the Periodic Table. 26 The diagram shows a flow chart for the manufacture of fertiliser. fractional distillation of air gas W pressure Y and 450 product Z fertiliser cracking of hydrocarbons gas X In the flow chart, what are W, X, Y and Z? W X Y Z A 2 N 2 high N 3 B O 2 SO 2 high SO 3 O 2 SO 2 low SO 3 D N 2 2 high N 3 ULES /12/M/J/16 [Turn over

26 27 Which oxide can be reduced to the metal by roasting with powdered iron? 10 A B D calcium oxide copper(ii) oxide magnesium oxide zinc oxide 28 Which element, if attached to iron immersed in salt water, would prevent the iron from corroding? A B D carbon copper magnesium sulfur 29 The final reaction in the extraction of metal X is represented by the following equation. What is X? X 2 O 3 + 3O 2X + 3O 2 A B D aluminium copper iron sodium 30 ydrated sodium carbonate decomposes when heated in a Bunsen burner flame. Which equation shows this decomposition correctly? A B D 2Na 2 O O(s) 4Na(s) + 2O 2 (g) + O 2 (g) O(g) Na 2 O O(s) Na 2 O 3 (s) O(g) Na 2 O O(s) NaO 3 (s) + NaO(s) O(g) Na 2 O O(s) Na 2 O(s) + O 2 (g) O(g) ULES /12/M/J/16

27 11 31 Aluminium is extracted from aluminium oxide by electrolysis. waste gases carbon cathode (-ve) molten aluminium carbon anodes (+ve) purified aluminium oxide dissolved in molten cryolite Which statement about this electrolysis is correct? A B D Aluminium ions gain electrons to form aluminium. ryolite is added to increase the melting point of the electrolyte. ryolite is added to react with impurities to form slag. The carbon cathode has to be replaced regularly as it reacts with oxygen. 32 Which ion is present in both sewage and fertilisers and can cause eutrophication when it enters rivers? A B D carbonate chloride nitrate sulfate ULES /12/M/J/16 [Turn over

28 33 The diagram shows an experiment to determine the percentage of oxygen in air. 12 bell jar lit candle water Which diagram shows the correct level of water after the candle stops burning? A B D 34 ow many of the structures show an unsaturated hydrocarbon molecule? l O O A 1 B 2 3 D 4 35 Which statements are correct for alkenes but not for alkanes? 1 They turn aqueous bromine from brown to colourless. 2 Their general formula is n 2n. 3 They burn in air to form carbon dioxide and water. A 1, 2 and 3 B 1 and 2 only 1 and 3 only D 2 and 3 only ULES /12/M/J/16

29 13 36 Wine is an alcoholic drink that contains ethanol. If wine is left exposed to the air for too long, it can become acidic. This is because the ethanol is to the acid Which word and formula correctly complete gaps 1 and 2? 1 2 A oxidised 3 OO B oxidised 3 2 OO reduced 3 OO D reduced 3 2 OO 37 Polymer Z has the structure shown. O O O O N N N N These four terms can be used to describe polymers. 1 addition polymer 2 condensation polymer 3 polyamide 4 polyester Which two terms can be applied to polymer Z? A 1 and 3 B 1 and 4 2 and 3 D 2 and 4 ULES /12/M/J/16 [Turn over

30 14 38 The diagram shows the structure of poly(dichloroethene). Which statement about this polymer is correct? l l n l A The monomer is. l l B The monomer is. D l The polymer is formed by a condensation reaction. The polymer has a lower melting point than the monomer. 39 ow can the following reaction be described? A B D combustion cracking oxidation reduction ULES /12/M/J/16

31 40 The structures of four hydrocarbons, W, X, Y and Z, are shown. 15 W X Y Z Which row is correct? isomers of each other decolourise bromine branched structures A W and X Y and Z W and Y B W and X Y and Z X and Z Y and Z W and Y X and Z D Y and Z W and Z W and Y 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. To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the ambridge International Examinations opyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at after the live examination series. ambridge International Examinations is part of the ambridge Assessment Group. ambridge Assessment is the brand name of University of ambridge Local Examinations Syndicate (ULES), which is itself a department of the University of ambridge. ULES /12/M/J/16

32 16 ULES /12/M/J/16 Group The Periodic Table of Elements 1 hydrogen 1 2 e helium 4 I II III IV V VI VII VIII 3 Li lithium 7 4 Be beryllium 9 atomic number atomic symbol Key name relative atomic mass 11 Na sodium Mg magnesium K potassium a calcium Rb rubidium Sr strontium s caesium Ba barium Fr francium 88 Ra radium 5 B boron Al aluminium Ga gallium In indium Tl thallium carbon Si silicon Ge germanium Sn tin Pb lead Ti titanium Zr zirconium f hafnium Rf rutherfordium 23 V vanadium Nb niobium Ta tantalum Db dubnium 24 r chromium Mo molybdenum W tungsten Sg seaborgium 25 Mn manganese Tc technetium 75 Re rhenium Bh bohrium 26 Fe iron Ru ruthenium Os osmium s hassium 27 o cobalt Rh rhodium Ir iridium Mt meitnerium 28 Ni nickel Pd palladium Pt platinum Ds darmstadtium 29 u copper Ag silver Au gold Rg roentgenium 30 Zn zinc d cadmium g mercury n copernicium 114 Fl flerovium 116 Lv livermorium 7 N nitrogen P phosphorus As arsenic Sb antimony Bi bismuth O oxygen S sulfur Se selenium Te tellurium Po polonium 9 F fluorine l chlorine Br bromine I iodine At astatine 10 Ne neon Ar argon Kr krypton Xe xenon Rn radon 21 Sc scandium Y yttrium lanthanoids actinoids 57 La lanthanum Ac lanthanoids actinoids The volume of one mole of any gas is 24 dm 3 at room temperature and pressure (r.t.p.) actinium 58 e cerium Th thorium Pr praseodymium Pa protactinium Nd neodymium U uranium Pm promethium 93 Np neptunium 62 Sm samarium Pu plutonium 63 Eu europium Am americium 64 Gd gadolinium m curium 65 Tb terbium Bk berkelium 66 Dy dysprosium f californium 67 o holmium Es einsteinium 68 Er erbium Fm fermium 69 Tm thulium Md mendelevium 70 Yb ytterbium No nobelium 71 Lu lutetium Lr lawrencium

33 ambridge International Examinations ambridge Ordinary Level * * EMISTRY 5070/21 Paper 2 Theory May/June hour 30 minutes andidates answer on the Question Paper. No Additional Materials are required. READ TESE INSTRUTIONS FIRST Write your entre number, candidate number and name on all the work you hand in. Write in dark blue or black pen. You may use an B pencil for any diagrams or graphs. Do not use staples, paper clips, glue or correction fluid. DO NOT WRITE IN ANY BARODES. Section A Answer all questions. Write your answers in the spaces provided in the Question Paper. Section B Answer any three questions. Write your answers in the spaces provided in the Question Paper. Electronic calculators may be used. You may lose marks if you do not show your working or if you do not use appropriate units. A copy of the Periodic Table is printed on page 20. At the end of the examination, fasten all your work securely together. The number of marks is given in brackets [ ] at the end of each question or part question. This document consists of 19 printed pages and 1 blank page. D (NF/SG) /3 ULES 2016 [Turn over

34 2 Section A Answer all the questions in this section in the spaces provided. The total mark for this section is 45. A1 hoose from the following polymers to answer the questions. Terylene O O O O O O O O PTFE F F F F F F F F F F F F F F F F nylon N N N N O O O O starch O O O O O poly(propene) PV l l l l ULES /21/M/J/16

35 3 protein N N N N O O O O polyester O O O O O O O O poly(ethene) Each polymer can be used once, more than once or not at all. Which is a polymer that (a) is made from propene,... [1] (b) will form hydrogen chloride when combusted,... [1] (c) can be hydrolysed to form amino acids,... [1] (d) can be hydrolysed to make simple sugars,... [1] (e) contains the same linkage as that present in a fat?... [1] [Total: 5] ULES /21/M/J/16 [Turn over

36 4 A2 ydrogen sulfide, 2 S, has a simple molecular structure. It is soluble in water. (a) Suggest one other physical property of hydrogen sulfide.... [1] (b) Aqueous hydrogen sulfide is a weak acid. (i) Write an equation to show the dissociation of hydrogen sulfide.... [1] (ii) Why is aqueous hydrogen sulfide described as a weak acid? [1] (c) Aqueous hydrogen sulfide reacts with aqueous potassium hydroxide. 2 S(aq) + 2KO(aq) K 2 S(aq) O(l) What is the minimum volume, in cm 3, of mol / dm 3 KO required to completely react with a solution containing g of 2 S? volume of KO(aq) =... cm 3 [3] ULES /21/M/J/16

37 (d) Magnesium reacts with sulfur to make the ionic compound magnesium sulfide. 5 (i) Predict two physical properties of magnesium sulfide [2] (ii) Explain, in terms of electrons, how a magnesium atom reacts with a sulfur atom to make a magnesium ion and a sulfide ion [2] [Total: 10] ULES /21/M/J/16 [Turn over

38 6 A3 Esters, such as propyl ethanoate, are often used as solvents. (a) Give one other use for esters such as propyl ethanoate.... [1] (b) Draw the structure of propyl ethanoate, showing all of the atoms and all of the bonds. (c) A bottle of propyl ethanoate is opened in a room. Some of the propyl ethanoate evaporates and then diffuses into the room. [1] (i) What is meant by the term diffusion? [1] (ii) What happens to the rate of diffusion of propyl ethanoate as the temperature of the room increases? Explain your answer in terms of the kinetic particle theory [2] ULES /21/M/J/16

39 7 (iii) The table shows some information about different esters. name structure relative molecular mass (M r ) methyl methanoate O ethyl methanoate O propyl methanoate O butyl methanoate O pentyl methanoate O Which ester has the greatest rate of diffusion at room temperature and pressure?... Explain your answer [2] [Total: 7] ULES /21/M/J/16 [Turn over

40 8 A4 Ammonia is manufactured by the reaction between hydrogen and nitrogen in the aber process. (a) State the conditions used in the aber process. temperature... pressure... catalyst... [2] (b) Describe and explain the effect of increasing the pressure on the rate of this reaction.... [2] (c) Explain how a catalyst speeds up the rate of a chemical reaction.... [1] (d) Ammonia is used to make fertilisers. The table gives some information about two fertilisers made from ammonia. fertiliser formula relative formula mass (M r ) ammonium nitrate N 4 NO 3 80 urea (N 2 ) 2 O 60 Use the data in the table to show that urea contains a greater percentage by mass of nitrogen than ammonium nitrate. [2] [Total: 7] ULES /21/M/J/16

41 A5 The statements give some of the chemical properties of metal X and its compounds. X does not react with cold water. X fizzes slowly with dilute hydrochloric acid. X does not react with aqueous sodium chloride. X reacts with aqueous lead(ii) nitrate. X reacts with aqueous silver nitrate. XO reacts with magnesium to form X. (a) Use the information to help arrange the following metals in order of reactivity. 9 lead, magnesium, silver, sodium and X most reactive least reactive... [2] (b) Suggest a possible identity for X.... [1] (c) onstruct the equation for the reaction between the oxide, XO, and magnesium.... [1] (d) onstruct the ionic equation for the reaction between X and aqueous lead(ii) nitrate, Pb(NO 3 ) 2 (aq).... [1] (e) Metal X is a good electrical conductor and has a high melting point. Explain why X conducts electricity, has a high melting point [3] [Total: 8] ULES /21/M/J/16 [Turn over

42 10 A6 The atmosphere contains a large number of gases including oxygen, nitrogen, carbon dioxide, sulfur dioxide, oxides of nitrogen, methane and chlorofluorocarbons (Fs). (a) arbon dioxide, methane and Fs are greenhouse gases. (i) State one effect of an increase in the atmospheric concentration of carbon dioxide and methane [1] (ii) State one source of methane gas.... [1] (iii) State one other environmental effect of the presence of Fs in the atmosphere.... [1] (b) The formula of one chlorofluorocarbon is Fl 3. Draw the dot-and-cross diagram to show the bonding in a molecule of Fl 3. Only draw the outer-shell electrons. [1] ULES /21/M/J/16

43 11 (c) Oxides of nitrogen are produced during the combustion of petrol (gasoline) in a car engine. (i) Describe the chemical reaction that takes place within a car engine to form nitric oxide, NO [1] (ii) Most of the nitric oxide and other pollutants present in the exhaust gases of a car are removed in a catalytic converter. Describe the redox reactions that happen within a catalytic converter [2] (d) Nitrogen dioxide is one of the causes of acid rain. Two moles of nitrogen dioxide react with one mole of water to make an aqueous solution of two acids only. One of these acids is nitric acid. Deduce the formula of the other acid.... [1] [Total: 8] ULES /21/M/J/16 [Turn over

44 12 BLANK PAGE ULES /21/M/J/16

45 13 Section B Answer three questions from this section in the spaces provided. The total mark for this section is 30. B7 Silver nitrate has the formula AgNO 3. (a) Describe how a pure sample of silver nitrate crystals can be prepared from solid silver oxide, which is insoluble in water.... [4] (b) Aqueous zinc chloride is added to a sample of acidified aqueous silver nitrate. (i) Describe what you would observe.... [1] (ii) onstruct the ionic equation, with state symbols, for the reaction that occurs.... [2] (c) Aqueous silver nitrate is electrolysed using graphite electrodes. (i) Identify the product formed at the cathode (negative electrode).... [1] (ii) Oxygen and water are formed at the anode (positive electrode). onstruct the equation for the reaction at the anode.... [1] (d) Silver nitrate decomposes on heating to form Ag 2 O, NO 2 and O 2. onstruct the equation for this reaction.... [1] [Total: 10] ULES /21/M/J/16 [Turn over

46 14 B8 yclohexane, 6 12, is a cycloalkane. ycloalkanes react in a similar way to alkanes. cyclohexane (a) yclohexane is a saturated hydrocarbon. (i) What is the meaning of the term saturated? [1] (ii) What is the meaning of the term hydrocarbon? [1] (b) onstruct the equation for the complete combustion of cyclohexane.... [1] (c) yclohexane reacts with chlorine in the presence of ultraviolet light. This is a substitution reaction. Write the molecular formulae of two products of this reaction.... [2] ULES /21/M/J/16

47 (d) yclohexane can be manufactured from hexane as shown in the equation alculate the mass of cyclohexane that can be made from 258 g of hexane. [M r of cyclohexane = 84] mass of cyclohexane =... g [2] (e) Another cycloalkane has the following percentage composition by mass., 85.7%;, 14.3% (i) Use the percentage composition by mass to show that the empirical formula of the cycloalkane is 2. [2] (ii) Draw the structure of the cycloalkane with an M r of 56, showing all of the atoms and all of the bonds. [1] [Total:10] ULES /21/M/J/16 [Turn over

48 16 B9 arbon reacts with steam in a reversible reaction. (s) + 2 O(g) 2 (g) + O(g) Δ = +131 kj / mol The reaction reaches an equilibrium if carried out in a closed container. (a) Explain, in terms of bond breaking and bond forming, why this reaction is endothermic.... [2] (b) When one mole of hydrogen, 2, is formed, 131 kj of energy is absorbed. alculate the amount of energy absorbed when 240 dm 3 of hydrogen, measured at room temperature and pressure, is formed. energy absorbed =... kj [2] (c) Predict, with a reason, how the position of equilibrium of this reaction changes as the (i) pressure is increased at constant temperature, [2] (ii) temperature is increased at constant pressure [2] ULES /21/M/J/16

49 (d) The reaction between carbon and steam is a possible source of hydrogen. 17 (i) Suggest one disadvantage of using this reaction as a source of hydrogen [1] (ii) Another source of hydrogen is the cracking of hydrocarbons from crude oil. Give one advantage of manufacturing hydrogen from the reaction of carbon with steam rather than from crude oil [1] [Total: 10] ULES /21/M/J/16 [Turn over

50 18 B10 Both zinc and iron react with dilute sulfuric acid. Zn(s) + 2 SO 4 (aq) Fe(s) + 2 SO 4 (aq) ZnSO 4 (aq) + 2 (g) FeSO 4 (aq) + 2 (g) (a) A 0.65 g sample of zinc is reacted with excess sulfuric acid. (i) alculate the volume of hydrogen, measured at room temperature and pressure, formed in this reaction. volume of hydrogen =... dm 3 [2] (ii) Explain why a different volume of hydrogen, measured at room temperature and pressure, is formed when 0.65 g of iron is reacted with excess sulfuric acid [1] (b) A mixture of iron powder and zinc powder is added to excess sulfuric acid. When the reaction stops, aqueous sodium hydroxide is added drop by drop to the reaction mixture until it is in excess. Describe what you would observe during the addition of aqueous sodium hydroxide and explain the reactions taking place. observations explanations [4] ULES /21/M/J/16

51 19 (c) The products of heating iron(ii) sulfate are iron(iii) oxide, sulfur dioxide and sulfur trioxide. (i) Explain how you can tell that the reaction involves an oxidation [1] (ii) Describe the chemical test for sulfur dioxide. test observation [2] [Total: 10] 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. To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the ambridge International Examinations opyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at after the live examination series. ambridge International Examinations is part of the ambridge Assessment Group. ambridge Assessment is the brand name of University of ambridge Local Examinations Syndicate (ULES), which is itself a department of the University of ambridge. ULES /21/M/J/16

52 /21/M/J/16 ULES 2016 Group The Periodic Table of Elements 1 hydrogen 1 2 e helium 4 I II III IV V VI VII VIII 3 Li lithium 7 4 Be beryllium 9 atomic number atomic symbol Key name relative atomic mass 11 Na sodium Mg magnesium K potassium a calcium Rb rubidium Sr strontium s caesium Ba barium Fr francium 88 Ra radium 5 B boron Al aluminium Ga gallium In indium Tl thallium carbon Si silicon Ge germanium Sn tin Pb lead Ti titanium Zr zirconium f hafnium Rf rutherfordium 23 V vanadium Nb niobium Ta tantalum Db dubnium 24 r chromium Mo molybdenum W tungsten Sg seaborgium 25 Mn manganese Tc technetium 75 Re rhenium Bh bohrium 26 Fe iron Ru ruthenium Os osmium s hassium 27 o cobalt Rh rhodium Ir iridium Mt meitnerium 28 Ni nickel Pd palladium Pt platinum Ds darmstadtium 29 u copper Ag silver Au gold Rg roentgenium 30 Zn zinc d cadmium g mercury n copernicium 114 Fl flerovium 116 Lv livermorium 7 N nitrogen P phosphorus As arsenic Sb antimony Bi bismuth O oxygen S sulfur Se selenium Te tellurium Po polonium 9 F fluorine l chlorine Br bromine I iodine At astatine 10 Ne neon Ar argon Kr krypton Xe xenon Rn radon 21 Sc scandium Y yttrium lanthanoids actinoids 57 La lanthanum Ac lanthanoids actinoids The volume of one mole of any gas is 24 dm 3 at room temperature and pressure (r.t.p.) actinium 58 e cerium Th thorium Pr praseodymium Pa protactinium Nd neodymium U uranium Pm promethium 93 Np neptunium 62 Sm samarium Pu plutonium 63 Eu europium Am americium 64 Gd gadolinium m curium 65 Tb terbium Bk berkelium 66 Dy dysprosium f californium 67 o holmium Es einsteinium 68 Er erbium Fm fermium 69 Tm thulium Md mendelevium 70 Yb ytterbium No nobelium 71 Lu lutetium Lr lawrencium

53 ambridge International Examinations ambridge Ordinary Level * * EMISTRY 5070/22 Paper 2 Theory May/June hour 30 minutes andidates answer on the Question Paper. No Additional Materials are required. READ TESE INSTRUTIONS FIRST Write your entre number, candidate number and name on all the work you hand in. Write in dark blue or black pen. You may use an B pencil for any diagrams or graphs. Do not use staples, paper clips, glue or correction fluid. DO NOT WRITE IN ANY BARODES. Section A Answer all questions. Write your answers in the spaces provided in the Question Paper. Section B Answer any three questions. Write your answers in the spaces provided in the Question Paper. Electronic calculators may be used. You may lose marks if you do not show your working or if you do not use appropriate units. A copy of the Periodic Table is printed on page 20. At the end of the examination, fasten all your work securely together. The number of marks is given in brackets [ ] at the end of each question or part question. This document consists of 19 printed pages and 1 blank page. D (NF/SG) /3 ULES 2016 [Turn over

54 2 Section A Answer all the questions in this section in the spaces provided. The total mark for this section is 45. A1 hoose from the following polymers to answer the questions. polymer A N N N N O O O O polymer B polymer O O O O O O O O polymer D O O O O O polymer E polymer F l l l l ULES /22/M/J/16

55 3 polymer G N N N N O O O O polymer O O O O O O O O polymer I F F F F F F F F F F F F F F F F Each polymer can be used once, more than once or not at all. (a) Which two polymers are polyesters?... and... [1] (b) Which polymer is used to make both clingfilm and plastic bags?... [1] (c) Give the letter of an addition polymer.... Give the letter of a condensation polymer.... [1] (d) Give the letter of a polymer that is a saturated hydrocarbon.... [1] (e) Which polymer could be part of a protein?... [1] [Total: 5] ULES /22/M/J/16 [Turn over

56 4 A2 ydrogen fluoride, F, has a simple molecular structure. It is soluble in water. (a) Suggest one other physical property of hydrogen fluoride.... [1] (b) ydrogen fluoride dissociates in water to form dilute hydrofluoric acid. (i) Write an equation to show the dissociation of hydrogen fluoride.... [1] (ii) Explain why an acidic solution is formed when hydrogen fluoride dissociates in water [1] (c) Dilute hydrofluoric acid reacts with aqueous calcium hydroxide. 2F(aq) + a(o) 2 (aq) af 2 (aq) O(l) What is the minimum volume, in cm 3, of mol / dm 3 a(o) 2 required to react completely with a solution containing g of F? volume of a(o) 2 (aq) =... cm 3 [3] ULES /22/M/J/16

57 (d) Magnesium reacts with fluorine to make the ionic compound magnesium fluoride. 5 (i) Predict two physical properties of magnesium fluoride [2] (ii) Explain, in terms of electrons, how a magnesium atom reacts with a fluorine molecule, F 2, to make a magnesium ion and two fluoride ions [2] [Total: 10] ULES /22/M/J/16 [Turn over

58 A3 Esters are used as food flavourings and solvents. (a) Draw the structure of ethyl methanoate, showing all of the atoms and all of the bonds. 6 [1] (b) Ethyl ethanoate evaporates at room temperature. (i) What is meant by the term evaporation? [1] (ii) A sample of ethyl ethanoate in a beaker is moved into a colder room. Explain, in terms of the kinetic particle theory, why this results in a decrease in the rate of evaporation [2] ULES /22/M/J/16

59 7 (iii) The table shows some information about different esters. name structure relative molecular mass (M r ) methyl ethanoate 3 O ethyl ethanoate 3 O propyl ethanoate 3 O butyl ethanoate 3 O pentyl ethanoate 3 O Which ester has the lowest rate of evaporation at room temperature and pressure?... Explain your answer [2] [Total: 6] ULES /22/M/J/16 [Turn over

60 A4 Sulfuric acid is manufactured by the contact process. (a) State the conditions used in the contact process. 8 temperature... pressure... catalyst... [2] (b) In the contact process, sulfur dioxide reacts with oxygen. 2SO 2 (g) + O 2 (g) 2SO 3 (g) Describe and explain the effect of increasing the concentration of oxygen on the rate of this reaction.... [2] (c) The catalyst used in the contact process increases the rate of the reaction. Describe one other advantage of using a catalyst in an industrial process.... [1] (d) Sulfuric acid is used to make the fertiliser potassium sulfate, K 2 SO 4. alculate the percentage by mass of potassium in this fertiliser. [2] [Total: 7] ULES /22/M/J/16