Cambridge A Level Chemistry 9701 — 2005 Oct/Nov Paper 1 · Variant 1

1 The petrol additive tetraethyl-lead(IV), Pb(C2H5)4, is now banned in many countries. When it is completely burned in air, lead(II) oxide, CO2 and H2O are formed. How many moles of oxygen are required to burn one mole of Pb(C2H5)4? A 9.5 B 11 C 13.5 D 27

Mark scheme: C

More questions on Reacting masses and volumes (of solutions and gases)

2 Which ion has more electrons than protons and more protons than neutrons? [H = 1 1H ; D = 2 1 H ; O = 16 8 O] A D– B H3O+ C OD– D OH–

Mark scheme: D

More questions on Particles in the atom and atomic radius

3 What is the electronic configuration of an element with a second ionisation energy higher than that of each of its neighbours in the Periodic Table? A 1s22s22p63s2 B 1s22s22p63s23p1 C 1s22s22p63s23p2 D 1s22s22p63s23p3

Mark scheme: B

More questions on Ionisation energy

4 Which compound has a boiling point that is influenced by hydrogen bonding? A CH3CHO B CH3OCH3 C HCO2H D HCO2CH3

Mark scheme: C

More questions on Intermolecular forces, electronegativity and bond properties

5 Which gas is likely to deviate most from ideal gas behaviour? A HCl B He C CH4 D N2

Mark scheme: A

More questions on The gaseous state: ideal and real gases and pV = nRT

6 Given S(s) + O2(g) → SO2(g), ∆H o = –297 kJ mol –1 f and S(s) + 1 O2(g) → SO3(g) 1 ∆H o = –395 kJ mol –1 2 f what is the enthalpy change of reaction, ∆H o, of 2SO2(g) + O2(g) → 2SO3(g)? A –196 kJ mol –1 B –98 kJ mol –1 C +98 kJ mol –1 D +196 kJ mol –1

Mark scheme: A

More questions on Hess’s law

7 The table shows the enthalpy change of neutralisation per mole of water formed, ∆H, for various acids and bases. acid base ∆H / kJ mol–1 hydrochloric acid sodium hydroxide –57.0 P sodium hydroxide –54.0 hydrochloric acid Q –52.0 nitric acid R –57.0 What are P, Q and R? P Q R A ethanoic acid ammonia potassium hydroxide B ethanoic acid sodium hydroxide ammonia C sulphuric acid ammonia potassium hydroxide D sulphuric acid sodium hydroxide ammonia

Mark scheme: A

More questions on Enthalpy change, ΔH

8 During the electrolysis of brine using a diaphragm cell, which reaction occurs at the cathode? A 2Cl –(aq) → Cl2(g) + 2e– B 4OH –(aq) → O2(g) + 2H2O(l) + 4e– C 2H2O(l) + 2e– → H2(g) + 2OH–(aq) D Na+(aq) + e– → Na(s)

Mark scheme: C

More questions on Electrolysis

9 Chlorine dioxide is produced on a large scale as it is used for bleaching paper pulp. It is made by the following reaction. 2Cl O (aq) + SO2(g) → 2Cl O2(g) + SO − 2 4 (aq) − 3 How do the oxidation numbers of chlorine and sulphur change in this reaction? chlorine sulphur A decreases by 1 increases by 1 B decreases by 1 increases by 2 C decreases by 3 increases by 1 D decreases by 3 increases by 2

Mark scheme: B

More questions on Redox processes: electron transfer and changes in oxidation number (oxidation state)

10 An experiment is set up to measure the rate of hydrolysis of methyl ethanoate. CH3CO2CH3 + H2O CH3CO2H + CH3OH The hydrolysis is found to be slow in neutral aqueous solution but it proceeds at a measurable rate when the solution is acidified with hydrochloric acid. What is the function of the hydrochloric acid? A to dissolve the methyl ethanoate B to ensure that the reaction reaches equilibrium C to increase the reaction rate by catalytic action D to suppress ionisation of the ethanoic acid formed

Mark scheme: C

More questions on Homogeneous and heterogeneous catalysts

11 The distribution of molecular kinetic energies within a gas at temperature T1 and T2 are shown in the diagram. T2 > T1 fraction of Ea = activation energy total molecules T1 T2 Ea 00 kinetic energy Which statement correctly explains why a small increase in temperature leads to a significant increase in the rate of a gaseous reaction? A The frequency of collisions between molecules is greater at a higher temperature. B The activation energy of the reaction is less when the gases are at a higher temperature. C The frequency of collisions between molecules with kinetic energy greater than the activation energy is greater at higher temperature. D The proportion of molecules with more kinetic energy than the activation energy is lower at a higher temperature.

Mark scheme: C

More questions on Effect of temperature on reaction rates and the concept of activation energy

12 One mole of magnesium, aluminium and sulphur are each completely burned in an excess of oxygen gas. Which graph shows the moles of oxygen used in each case? A B moles of moles of oxygen oxygen used used 0 0 Mg Al S Mg Al S C D moles of moles of oxygen oxygen used used 0 0 Mg Al S Mg Al S

Mark scheme: D

More questions on Periodicity of chemical properties of the elements in Period 3

13 In 1999, researchers working in the USA believed that they had made a new element and that it had the following electronic structure. [Rn] 5f146d107s27p6 In which Group of the Periodic Table would you expect to find this element? A II B IV C VI D 0

Mark scheme: D

More questions on Electrons, energy levels and atomic orbitals

14 Consecutive elements X, Y, Z are in Period 3 of the Periodic Table. Element Y has the highest first ionisation energy and the lowest melting point. What could be the identities of X, Y and Z ? A sodium, magnesium, aluminium B magnesium, aluminium, silicon C aluminium, silicon, phosphorus D silicon, phosphorus, sulphur

Mark scheme: D

More questions on Periodicity of physical properties of the elements in Period 3

15 Use of the Data Booklet is relevant to this question. What volume of oxygen, measured under room conditions, can be obtained from the thermal decomposition of 8.2 g of calcium nitrate (Mr = 164)? A 150 cm3 B 300 cm3 C 600 cm3 D 1200 cm3

Mark scheme: C

More questions on Reacting masses and volumes (of solutions and gases)

16 When a mineral was heated in a Bunsen flame to constant mass, a colourless gas that turned lime water milky was evolved. The remaining solid was cooled and then added to aqueous hydrochloric acid. Vigorous effervescence was seen. What was the mineral? A aragonite, CaCO3 B artinite, MgCO3.Mg(OH)2.3H2O C barytocalcite, BaCO3.CaCO3 D dolomite, CaCO3.MgCO3

Mark scheme: C

More questions on Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

17 How does ammonia behave when its aqueous solution is used to dissolve silver chloride, AgCl ? A as a base B as a ligand with the Ag+ ion C as a ligand with the Cl – ion D as a reducing agent

Mark scheme: B

More questions on General characteristic chemical properties of the first set of transition elements, titanium to copper

18 Lime, CaO, is used to reduce the acidity of soil, and ammonium sulphate is a nitrogenous fertiliser. Why can they not be used in a mixed form? A The dry mixture is explosive. B CaSO4, formed on mixing, causes hard water. C When dampened, ammonia is given off. D Sulphuric acid will form.

Mark scheme: C

More questions on Nitrogen and sulfur

19 The diagram shows the structure of vitamin C. HO OH C C O C CH CH CH2OH O OH How many chiral centres are there in one molecule?

Mark scheme: B

More questions on Isomerism: structural isomerism and stereoisomerism

20 What is the number of isomers of C2H2Cl2 including cis-trans isomers? A 2 B 3 C 4 D 5

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More questions on Isomerism: structural isomerism and stereoisomerism

21 Which hydrocarbon, on treatment with hot acidified potassium manganate(VII), would give ethanoic acid only? A CH3CH CH2 B CH3CH CHCH3 CH3 C C CHCH3 CH3 CH3 CH3 D C C CH3 CH3

Mark scheme: B

More questions on Alkenes

22 In the upper atmosphere chlorofluoroalkanes (CFCs) are broken down to give chlorine radicals but not fluorine radicals. What is the best explanation for this? A Fluorine is more electronegative than chlorine. B Fluorine radicals are less stable than chlorine radicals. C The C–F bond is stronger than the C–Cl bond. D The chlorine atom is larger than the fluorine atom.

Mark scheme: C

More questions on Intermolecular forces, electronegativity and bond properties

23 An amine is produced in the following reaction. C2H5I + 2NH3 → C2H5NH2 + NH4I What is the mechanism? A electrophilic addition B electrophilic substitution C nucleophilic addition D nucleophilic substitution

Mark scheme: D

More questions on Halogenoalkanes

24 Compound X on reaction with hot concentrated sulphuric acid gave a mixture of three alkenes. What could X be? A butan-2-ol B propan-2-ol C 2-methylbutan-2-ol D 2-methylpropan-2-ol

Mark scheme: A

More questions on Alcohols

25 Compounds X, Y and Z all react with PCl5 to release hydrogen chloride, but only one of them reacts with 2,4-dinitrophenylhydrazine reagent. Which one of the following combinations could be X, Y and Z ? X Y Z CH2OH CHO CO2H A CH2OH CHO CO2H CH2OH CH2OH CHO B CH2OH CHO CO2H CH2OH CH2OH CHO C CHO CO2H CO2H CH2OH CHO CO2H D CO2H CO2H CO2H

Mark scheme: D

More questions on Formulas, functional groups and the naming of organic compounds

26 In 1903 Arthur Lapworth became the first chemist to investigate a reaction mechanism. The reaction he investigated was that of hydrogen cyanide with propanone. What do we now call the mechanism of this reaction? A electrophilic addition B electrophilic substitution C nucleophilic addition D nucleophilic substitution

Mark scheme: C

More questions on Nitriles and hydroxynitriles

27 What is formed when propanone is refluxed with an anhydrous solution of NaBH4? A propanal B propan-1-ol C propan-2-ol D propane

Mark scheme: C

More questions on Aldehydes and ketones

28 What is the structure of the ester formed from propanoic acid and ethanol? A B H H H O O H H H H H H C C H C C C O C C C H O C C H H H H H H H H H C D H H H O O H C H H H H C C H C C O C H O C C H H H H C H H H H

Mark scheme: B

More questions on Esters

29 Lactic acid occurs naturally, for example in sour milk. Its displayed formula is shown. H H O O H C C C O H H H Which reaction occurs with lactic acid? A It decolourises aqueous bromine rapidly. B It is insoluble in water. C It reduces Fehling’s reagent. D Two molecules react with each other in the presence of a strong acid.

Mark scheme: D

More questions on Carboxylic acids

30 PHB (polyhydroxybutyric acid) is a natural polymer produced by a range of micro-organisms. It can also be manufactured from sugar. PHB is readily biodegradable. CH3 O [ O CH CH2 C [ n PHB (polyhydroxybutyric acid) What type of reaction will cause PHB to break down? A addition B hydrolysis C reduction D substitution

Mark scheme: B

More questions on Condensation polymerisation

31 The relative molecular mass of a molecule of chlorine is 72. Which properties of the atoms in this molecule are the same? 1 radius 2 nucleon number 3 relative isotopic mass

Mark scheme: D

More questions on Isotopes

32 Which molecules are planar? 1 BCl3 2 NH3 3 PH3

Mark scheme: D

More questions on Shapes of molecules

33 Boron is a non-metallic element which is placed above aluminium in Group III of the Periodic Table. It forms a compound with nitrogen known as boron nitride which has a graphite structure. Which of the following conclusions can be drawn from this information? 1 The empirical formula of boron nitride is BN. 2 The boron and nitride atoms are likely to be arranged alternately in a hexagonal pattern. 3 Boron nitride has a layer structure with van der Waals’ forces between the layers.

Mark scheme: A

More questions on Bonding and structure

34 Hydroxyapatite, Ca5(PO4)3OH, is the main constituent of tooth enamel. In the presence of saliva, the following equilibria exist. Ca5(PO4)3OH(s) 5Ca2+(aq) + 3PO (aq) + OH–(aq) 3 − 4 HPO (aq) 2 − H+(aq) + PO (aq) 3 − 4 4 Which of the following statements help to explain why tooth enamel is dissolved more readily when saliva is acidic? 1 The hydroxide ions are neutralised by the acid. 2 The phosphate ion PO (aq) accepts H+(aq) 3 − 4 3 Calcium ions react with acids.

Mark scheme: B

More questions on Acids and bases

35 What properties enable magnesium oxide to be used as a refractory lining in a furnace? 1 It has a high melting point. 2 It has a low thermal conductivity. 3 It does not react with basic slags.

Mark scheme: A

More questions on Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

36 Chlorine reacts with hot concentrated aqueous sodium hydroxide according to the equation below. 3Cl2(g) + 6NaOH(aq) → NaCl O3(aq) + 5NaCl (aq) + 3H2O(l) Which conclusions can be drawn from this information? 1 The oxidation state of the chlorine in one of the products is +5. 2 The chlorine undergoes disproportionation. 3 The sodium hydroxide acts as a reducing agent.

Mark scheme: B

More questions on The reactions of chlorine

37 Which equations represent stages in the Contact process for manufacturing sulphuric acid? 1 S + O2 → SO2 2 H2O + SO2 → H2SO3 3 H2SO3 + O2 → H2SO4 1 2

Mark scheme: D

More questions on Nitrogen and sulfur

38 For the reaction (CH3)3SiCl + C2H5O– → (CH3)3SiOC2H5 + Cl – which statements are likely to be true? 1 It involves nucleophilic attack by C2H5O–. 2 Cl – is displaced by C2H5O–. 3 The oxygen-carbon bond is not broken.

Mark scheme: A

More questions on Halogen compounds

39 Modern cars are fitted with catalytic converters. These remove carbon monoxide, unburnt hydrocarbons and oxides of nitrogen from exhaust gases. Which of these pollutant gases are removed by oxidation? 1 carbon monoxide 2 hydrocarbons 3 nitrogen oxides

Mark scheme: B

More questions on Homogeneous and heterogeneous catalysts

40 The sex-attractant of the house-fly is muscalure, with the following formula. CH3(CH2)7CH = CH(CH2)12CH3 Which statements about muscalure are correct? 1 It will decolourise aqueous bromine. 2 It will be oxidised by cold aqueous alkaline KMnO4 to give a diol. 3 It will be optically active.

Mark scheme: B

More questions on Alkenes