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1

The diagram shows four pieces of apparatus that are used to measure the volume of a gas or liquid. Which piece of apparatus should always be filled to the same level?

12. Experimental techniques and chemical analysis  →  12.1. Experimental design

12. Experimental techniques and chemical analysis  →  12.2. Acid-base titrations

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2

Aqueous sodium thiosulfate reacts with acid to make a precipitate of sulfur. Na2S2O3+ 2HCl → 2NaCl + H2O+ SO2+ SA student investigates the effect of temperature on the rate of this reaction. The student: ● places a piece of paper with a cross on it below the reaction mixture as shown...

12. Experimental techniques and chemical analysis  →  12.1. Experimental design

6. Chemical reactions  →  6.2. Rate of reaction

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3

A paper chromatography experiment is carried out to find an Rf value for Fe3+. The result is shown...

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases

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4

The diagram shows two experiments. Al 3+add a few drops of NaOHadd an excess of NaOHCu2+add a few drops of NaOHexperiment 1 experiment 2 no precipitate no precipitate precipitate formed precipitate formed add an excess of NaOH?

7. Acids, bases and salts  →  7.3. Preparation of salts

12. Experimental techniques and chemical analysis  →  12.1. Experimental design

12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases

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5

Which methods of separation require a change of state from liquid to gas?

12. Experimental techniques and chemical analysis  →  12.4. Separation and purification

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6

Hydrogen sulfide, H2S, and hydrogen chloride, HCl, are both gases at temperatures above –50 °C. Which gas will diffuse most rapidly at the temperature given?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

1. States of matter  →  1.2. Diffusion

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7

The diagram shows the relative mass and the relative charge of two particles, and , present in atoms and ions. –1 relative charge relative mass Which of these particles are present in a hydrogen atom and in a hydrogen ion?

3. Stoichiometry  →  3.2. Relative masses of atoms and molecules

2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table

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8

Which ion has the most shells that contain electrons?

2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table

8. The Periodic Table  →  8.1. Arrangement of elements

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9

Which substance conducts electricity both when solid and when molten?

4. Electrochemistry  →  4.1. Electrolysis

2. Atoms, elements and compounds  →  2.4. Ion and ionic bonds

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10

When they react together, which pair of elements form an ionic compound?

2. Atoms, elements and compounds  →  2.4. Ion and ionic bonds

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11

How many shared electrons are in one carbon dioxide molecule?

2. Atoms, elements and compounds  →  2.5. Simple molecules and covalent bonds

11. Organic chemistry  →  11.5. Alkenes

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12

Element X has a lattice of positive ions and a ‘sea of electrons’. e– e– e– e– e– e– e– e– e– e– e– e– e– e– e– Which property will X have?

2. Atoms, elements and compounds  →  2.7. Metallic bonding

2. Atoms, elements and compounds  →  2.4. Ion and ionic bonds

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13

Which row shows the correct state symbols for the reaction between calcium carbonate and dilute hydrochloric acid?

7. Acids, bases and salts  →  7.1. The characteristic properties of acids and bases

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14

The expression shown...

3. Stoichiometry  →  3.2. Relative masses of atoms and molecules

3. Stoichiometry  →  3.3. The mole and the Avogadro constant

2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table

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15

A mixture of 5 cm3 of CH4 and 100 cm3 of air is exploded. Assume air is 80% N2 by volume and 20% O2 by volume. The resulting mixture is cooled. All volumes are measured at room temperature and pressure. CH4+ 2O2→ CO2+ 2H2OWhat is the composition of the resulting gas?

10. Chemistry of the environment  →  10.3. Air quality and climate

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

1. States of matter  →  1.1. Solids, liquids and gases

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16

Which arrangement is used to electroplate copper onto a steel key?

4. Electrochemistry  →  4.1. Electrolysis

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17

The chloride of metal X is dissolved in water. A concentrated solution of this chloride is electrolysed using inert electrodes. inert anode inert cathode concentrated aqueous solution of chloride of metal X X is above sodium in the reactivity series. In addition to chlorine, which gas is liberated and at which electrode?

4. Electrochemistry  →  4.1. Electrolysis

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18

Which change in conditions, for the reaction between zinc and dilute sulfuric acid, increases the rate of reaction by lowering the activation energy?

6. Chemical reactions  →  6.2. Rate of reaction

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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19

Many reactions can be classified as redox reactions. Which equations show redox reactions?

6. Chemical reactions  →  6.4. Redox

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20

Which row correctly shows whether the hydrogen ion concentration and the pH of ethanoic acid are higher or lower than those of hydrochloric acid of the same concentration?

7. Acids, bases and salts  →  7.1. The characteristic properties of acids and bases

11. Organic chemistry  →  11.3. Fuels

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21

Which aqueous reagent liberates ammonia from ammonium nitrate on warming?

12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases

7. Acids, bases and salts  →  7.3. Preparation of salts

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22

Two fertilisers are made by mixing chemical compounds. Fertiliser X contains 500 g of NH4NO3 and 500 g of (NH4)2SO4 per kilogram. Fertiliser Y contains 700 g of NH4NO3 and 300 g of CaSO4 per kilogram. Which fertiliser contains the higher percentage of nitrogen by mass and which contains the higher percentage of sulfur by mass?

3. Stoichiometry  →  3.3. The mole and the Avogadro constant

10. Chemistry of the environment  →  10.2. Fertilisers

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23

Which processes occur in the manufacture of sulfuric acid?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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24

A lump of element X can be cut by a knife. During its reaction with water, X floats and melts. What is X?

9. Metals  →  9.4. Reactivity series

8. The Periodic Table  →  8.1. Arrangement of elements

9. Metals  →  9.1. Properties of metals

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25

Chlorine is passed into separate samples of aqueous potassium iodide and aqueous potassium bromide. In which solutions is there a colour change?

6. Chemical reactions  →  6.4. Redox

12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

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26

Which diagram shows the structure of an alloy?

9. Metals  →  9.3. Alloys and their properties

11. Organic chemistry  →  11.8. Polymers

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27

Which element can only be extracted from its ore using electrolysis?

4. Electrochemistry  →  4.1. Electrolysis

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28

Which equation shows a thermal decomposition that occurs in the blast furnace?

9. Metals  →  9.6. Extraction of metals

10. Chemistry of the environment  →  10.3. Air quality and climate

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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29

Which diagram correctly shows the conditions necessary for the rusting of iron and also the metal that can be used to prevent rusting by sacrificial protection?

9. Metals  →  9.5. Corrosion of metals

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30

Aluminium is produced by the electrolysis of pure aluminium oxide. One of the electrodes in the process has to be replaced often. Which statement is correct?

4. Electrochemistry  →  4.1. Electrolysis

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31

Which row correctly compares carbon dioxide and methane?

10. Chemistry of the environment  →  10.3. Air quality and climate

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32

Sea water has to be purified in order to obtain drinking water from it. Which processes are used to purify the sea water?

10. Chemistry of the environment  →  10.1. Water

12. Experimental techniques and chemical analysis  →  12.4. Separation and purification

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33

Which structure represents an isomer of butane?

11. Organic chemistry  →  11.1. Formulae, functional groups and terminology

11. Organic chemistry  →  11.2. Naming organic compounds

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34

Which statement about the organic compounds CH4, C2H4, C2H6 and C3H8 is correct?

11. Organic chemistry  →  11.5. Alkenes

11. Organic chemistry  →  11.3. Fuels

11. Organic chemistry  →  11.1. Formulae, functional groups and terminology

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35

The alkenes are a homologous series. Which statement about alkenes is correct?

11. Organic chemistry  →  11.5. Alkenes

11. Organic chemistry  →  11.1. Formulae, functional groups and terminology

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36

Which organic compound is used as a solvent, a renewable fuel and in the production of vinegar?

11. Organic chemistry  →  11.6. Alcohols

11. Organic chemistry  →  11.7. Carboxylic acids

11. Organic chemistry  →  11.2. Naming organic compounds

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37

Which structure shows the carboxylic acid with the lowest relative molecular mass?

3. Stoichiometry  →  3.2. Relative masses of atoms and molecules

2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table

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38

What is the name of the ester shown...

11. Organic chemistry  →  11.2. Naming organic compounds

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39

The diagram shows the structure of a monomer. H C H H C F C Cl H Which diagram shows the partial structure of its polymer?

11. Organic chemistry  →  11.8. Polymers

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40

Which statement about polymers is correct?

11. Organic chemistry  →  11.8. Polymers

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