CAIE Chemistry (9701)

Equations involving four enthalpy changes are shown.

+ 2e Which equation represents the second ionisation energy of sodium? A X B X + Y - W C X - W D Z - W

This question refers to isolated gaseous atoms in the ground state. In which atom are all electrons paired? A Ba B Br C S D Si

Which sample contains the most iodine?A 1 g of CaI 2 B 1 g of KI C 1 g of NaI D 1 g of NH4I

When a small sample of hydrocarbon Q is completely combusted, it produces 3.52 g of carbon dioxide and 1.44 g of water. What could be the structure of hydrocarbon Q? A DBC HCC C HC

Ethane and ethene are both hydrocarbon molecules. What is a feature of both molecules? A a planar structure

Elements J and L are both in Group 15. J and L each form a gaseous covalent hydride in which their oxidation number is -3. In the liquefied forms of these hydrides, significant hydrogen bonding occurs only in the hydride of L. Which row about J and L could be correct? identity of J identity of L outer shell electron configuration A As N p B As N s C N As p D N As s

Which gas will behave least like an ideal gas at 150 A ammonia B fluorine C krypton D steam

When an evacuated glass bulb of volume 200 is filled with a gas at 300 K and 101 kPa, the mass of the bulb increases by 0.68 g. The gas obeys the ideal gas equation. What is the identity of the gas? A argon B krypton C neon D nitrogen

The standard enthalpy of formation of NO2

is + 33.2 kJ mol The standard enthalpy of formation of N 2O4

is + 9.2 kJ mol What is the standard enthalpy change for the reaction 2NO A -57.2 kJ mol B -24.0 kJ mol C +42.4 kJ mol D +75.6 kJ mol

Separate samples of 25.0 of 0.1 mol dm NaOH(aq) are added to each of three different acid solutions, as described. The temperature of each of the solutions was 298 K before mixing. sample acid type of acid concentration mol dm volume / cm 1 H 2SO4 strong 0.05 25.0 2 HC l strong 0.05 25.0 3 CH 3CO2H weak 0.05 25.0 Which statement describes the temperature rises that occur on mixing each of these three acids separately with NaOH? A The temperature rise in all three mixtures is the same. B The temperature rise using H 2SO4 and HCl is the same. C The temperature rise using CH 3CO2H is greater than using HCl. D The greatest temperature rise occurs using H 2SO4. 11 NCl 3 reacts with H2O. NCl The oxidation state of nitrogen does not change in this reaction. Which statement is correct? A Chlorine is reduced. B Chlorine is oxidised. C Hydrogen is both oxidised and reduced. D This is not a redox reaction.

In which row do the oxidation numbers of vanadium increase? smallest largest A VO 4 3- VO 3 - VO 2 B VO V 2O3 VO 4 C V 2O3 VO VO 3 D VO 4 3- VO 2 + VO

A synthesis for methanol is shown. 2 + 3H2 Which conditions would produce the greatest yield of methanol at equilibrium? pressure temperature A high 80 B high 20 C low 80 D low 20

Hydrogen and iodine can react reversibly to produce hydrogen iodide. The equation is shown. 2

+ I 2

4.00 mol of hydrogen gas and X mol of iodine vapour are mixed in a sealed container of volume 1.00 at a temperature of 460 K. The system is allowed to reach equilibrium. The equilibrium mixture contains 2.00 mol of hydrogen iodide. The equilibrium constant, K c, for the reaction at 460 K is 4.0. What is the value of X? A 0.50 mol B 1.17 mol C 1.33 mol D 2.50 mol

A large amount of N 2O

decomposes into nitrogen gas and oxygen gas in the presence of a tiny amount of a gold foil catalyst. The gold foil provides a solid surface on which the catalysed reaction takes place. The graph shows the concentration of N 2O

against time as it decomposes. The graph is a straight line. concentration of N O

0 10 time / min Which row describes: 2O

decomposes from 0 to 10 minutes amount and concentration of N 2O

? change in rate of reaction as 2O

decomposes effect of adding more gold foil on the rate of decomposition A none increases B none none C decreases increases D decreases none

The Haber process for the manufacture of ammonia is represented by the equation shown. 2

+ 3H2

Which statement is correct about this reaction when the temperature is increased? A Both forward and backward rates increase. B The backward rate only increases. C The forward rate only increases. D There is no effect on the backward or forward rates.

NH 3(aq) is added to separate samples of NaCl (aq), MgCl 2(aq), BaCl 2(aq) and SiCl 4

. Under the conditions of this experiment, only two samples will produce a white precipitate when NH 3(aq) is added. What are these two samples? A MgCl 2(aq) and BaCl 2(aq) B MgCl 2(aq) and SiCl 4

C NaCl

and BaCl 2(aq) D NaCl

and SiCl 4(l)

Why is the ionic radius of a sulfide ion larger than the ionic radius of a potassium ion? A Ionic radius always decreases with increasing atomic number. B Positive ions always have smaller radii than negative ions. C The potassium ion has more protons in its nucleus than the sulfide ion. D The sulfide ion is doubly charged; the potassium ion is singly charged.

Which graph correctly shows relative electronegativity plotted against relative atomic radius for the elements Na, Mg, Al and Si? electronegativity atomic radius electronegativity atomic radius electronegativity atomic radius electronegativity atomic radius

The table gives information about calcium carbonate and calcium hydroxide. Which row is correct? calcium carbonate is more soluble in water than calcium hydroxide calcium hydroxide can be manufactured using calcium carbonate A no no B no yes C yes no D yes yes

Q is a Group 2 metal. An excess of QCO 3

is added to H2SO4(aq) followed by filtration. A sample of QSO4 is then obtained by evaporation of the filtrate. What could be the identity of Q? A barium, calcium or magnesium B barium or calcium only C calcium only D calcium or magnesium only

X, Y and Z are three elements in Group 17. 2 has weaker covalent bonds than Y2. 2 has stronger instantaneous dipole-induced dipole forces between its molecules than Z 2. 2 is a stronger oxidising agent than Z2. What could be X, Y and Z? X Y Z A Br C l I B Cl Br I C I Br C l D I C l Br

Chlorine reacts with aqueous sodium hydroxide forming two chlorine-containing products. Which row shows the oxidation states of chlorine in the products under the conditions stated? conditions oxidation state of Cl in products A cold NaOH(aq) -1 and +3 B cold NaOH(aq) -1 and +5 C hot NaOH(aq) -1 and +3 D hot NaOH(aq) -1 and +5

A catalytic converter reduces the amount of pollutants in the fumes from a car exhaust. Which row identifies a pollutant and shows how it is removed by the action of the catalyst? pollutant chemical removal A carbon dioxide reduced to carbon B carbon monoxide oxidised to carbon dioxide C oxides of nitrogen oxidised to nitric acid D unburnt hydrocarbons oxidised to carbon dioxide and hydrogen

Solid R is added to a solution of ammonium nitrate and the mixture is heated. A gas is given off which turns red litmus to blue. What could be R? A aluminium chloride B magnesium chloride C sodium oxide D phosphorus oxide

A skeletal formula is shown. What is the total number of stereoisomers including the one shown? A 4 B 6 C 8 D 16

The molecular formula CH 3 can represent an anion, a cation or a free radical. Species with the molecular formula CH 3 can act as an electrophile, a free radical or a nucleophile depending on the number of outer shell electrons on the central carbon atom. How many outer shell electrons on the central carbon atom must be present for CH 3 to act in these different ways? 3 as an electrophile CH 3 as a free radical CH 3 as a nucleophile A 6 7 8 B 6 8 7 C 7 6 8 D 8 7 6 28 Compound Z, C 7H13Br, has two chiral centres. A sample of Z contains all four possible optical isomers. This sample of Z reacts with hot ethanolic NaOH to produce a mixture of only three isomers. Two of these isomers are optical isomers of each other. What could be the formula of Z? A B

The free-radical substitution reaction between methane and chlorine involves initiation, propagation and termination stages. Which row is correct? involved in initiation stage radical produced in a propagation stage

The alkene shown reacts with an excess of HBr via an electrophilic addition reaction. What is the major product formed? A 3,5-dibromo-2-methylhexane B 2,5-dibromo-2-methylhexane C 2,6-dibromo-2-methylhexane D 3,6-dibromo-2-methylhexane

The diagram shows the structures of two halogenoalkanes, P and Q. Both compounds can be hydrolysed. Which row is correct? compound more readily hydrolysed reaction mechanism A P S N1 B P S N2 C Q S N1 D Q S N2

The structure of coniine is shown. coniine Coniine can be synthesised by reacting ammonia with a dibromo compound, X. What is compound X? A 1,1-dibromo-2-propylcyclopentane B 1,2-dibromo-2-propylcyclopentane C Br(CH 2)3CHBr(CH2)3CH3 D Br(CH 2)4CHBr(CH2)2CH3

Primary alcohols can be oxidised to aldehydes using either acidified potassium dichromate( VI) or acidified potassium manganate( VII). The reaction mixtures change colour as the oxidising agent is reduced. What are the colour changes seen? acidified potassium dichromate( VI) acidified potassium manganate(VII) before after before after A green orange purple colourless B orange green colourless purple C orange green purple colourless D purple colourless orange green

Which reaction has a product that gives a yellow precipitate when treated with alkaline I 2(aq)? A 2-chloropropane is warmed with a dilute aqueous solution of sodium hydroxide. B Ethanal is heated under reflux with acidified potassium dichromate( VI). C Methyl ethanoate is heated under reflux with dilute sulfuric acid. D Propanal is reacted with NaBH 4, followed by dilute sulfuric acid.

The skeletal formula of M is shown. HO O M is reacted with an excess of LiAl H4. Dilute acid is then added. What is the molecular formula of the final organic product?A C 5H6O5 B C 5H10O4 C C 5H10O3 D C 5H12O3

Which compound forms a precipitate when mixed with 2,4-DNPH reagent and also forms a precipitate when mixed with Fehling's reagent? A BC D

Which reaction is a redox reaction? A ethanenitrile heated under reflux with dilute hydrochloric acid B ethanoic acid reacted with aqueous sodium hydroxide C ethanoic acid reacted with sodium D ethyl ethanoate heated under reflux with dilute hydrochloric acid

Ethyl butanoate is a flavouring, with a fruity flavour. Which row is correct? alcohol and acid that react to form ethyl butanoate the mass of water formed when 2.32 g of ester is formedand 0.36and 0.40and 0.36and 0.40

Cyclohexene, as shown in the diagram, can form an addition polymer. cyclohexene Which structure represents a section of the polymer? A BC D

Three organic compounds are listed. 1 ethanal 2 propan-1-ol 3 propan-2-ol Which compounds will have a mass spectrum that contains a fragment peak at m / e = 43? A 1 only B 1 and 2 only C 2 and 3 only D 1, 2 and 3 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 (UCLES) 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 Cambridge Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cambridgeinternational.org after the live examination series. Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge. Important values, constants and standards molar gas constant R = 8.31J Kmol C molmol-19 molar volume of gas V m = 22.4 dmmol at s.t.p. (101 kPa and 273 K) m = 24.0 dmmol at room conditions ionic product of water K-14mol specific heat capacity of water c = 4.18 kJ kg (4.18 J g Group The Periodic Table of Elements hydrogen 1.0 He helium 4.0 1213 14 15 16 17 18 3 4 5 6 7 8 9 10 11 123Li lithium 6.9 beryllium 9.0 atomic number atomic symbolKey name relative atomic mass sodium 23.0 magnesium 24.3 potassium 39.1 calcium 40.1 rubidium 85.5 strontium 87.6 caesium 132.9 barium 137.3 francium Ra radium boron 10.8 13 Al aluminium 27.0 31 Ga gallium 69.7 49 In indium 114.8 thallium 204.4 carbon 12.0 14 Si silicon 28.1 32 Ge germanium 72.6 50 Sntin 118.7 82 Pb lead 207.2 titanium 47.9 40 Zr zirconium 91.2 72 Hf hafnium 178.5 rutherfordium vanadium 50.9 41 Nb niobium 92.9 73 Ta tantalum 180.9 105 Db dubnium chromium 52.0 42 Mo molybdenum 95.9 74 W tungsten 183.8 106 Sg seaborgium manganese 54.9 43 Tc technetium rhenium 186.2 107 Bh bohrium iron 55.8 44 Ru ruthenium 101.1 76 Os osmium 190.2 108 Hs hassium Co cobalt 58.9 45 Rh rhodium 102.9 iridium 192.2 109 Mt meitnerium nickel 58.7 46 Pd palladium 106.4 platinum 195.1 11 0 Ds darmstadtium copper 63.5 47 Ag silver 107.9 79 Au gold 197.0 111 Rg roentgenium zinc 65.4 48 Cd cadmium 112.4 80 Hg mercury 200.6 11 2 Cn copernicium 11 4 flerovium 11 6 livermorium nitrogen 14.0 phosphorus 31.0 33 As arsenic 74.9 51 Sb antimony 121.8 bismuth 209.0 oxygen 16.0 sulfur 32.1 34 Se selenium 79.0 52 Te tellurium 127.6 84 Po polonium fluorine 19.0 17 Cl chlorine 35.5 35 Br bromine 79.9 iodine 126.9 Ne neon 20.2 18 Ar argon 39.9 36 Kr krypton 83.8 54 Xe xenon 131.3 86 Rn radon 11 3 nihonium 11 5 moscovium 11 7 tennessine 11 8 oganesson scandium 45.0 yttrium 88.9 57-71 lanthanoids 89-103 actinoids 57La lanthanum 138.9 89 Ac lanthanoids actinoids actinium Ce cerium 140.1 90 Th thorium 232.0 praseodymium 140.9 91 Pa protactinium 231.0 neodymium 144.4 uranium 238.0 promethium neptunium samarium 150.4 94 Pu plutonium europium 152.0 95 Am americium gadolinium 157.3 96 Cm curium terbium 158.9 97 Bk berkelium dysprosium 162.5 californium holmium 164.9 99 Es einsteinium erbium 167.3 100 Fm fermium Tm thulium 168.9 101 Md mendelevium ytterbium 173.1 102 No nobelium lutetium 175.0 lawrencium