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1

Hydrogen chloride gas, HCl, reacts with ammonia gas, NH3, to form solid ammonium chloride. The apparatus is set up as shown...

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

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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2

Substance L melts at –7 °C and is a brown liquid at room temperature. Which temperature is the boiling point of pure L?

10. Chemistry of the environment  →  10.1. Water

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

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3

Chromatography is done on a mixture containing a drug. The drug has an Rf value of 0.66. The diagram is not drawn to scale. Which spot on the chromatogram represents the drug?

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

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4

Caesium, Cs, is an element in Group I of the Periodic Table. When caesium reacts it forms a positive ion, Cs+. How is a caesium ion formed?

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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5

The structure of copper is described as a lattice of positive ions in a ‘sea of electrons’. Which statements are correct?

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

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

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6

Three statements about diamond, graphite and silicon(oxide are listed. Diamond and graphite both have giant covalent structures. In silicon(oxide, silicon and oxygen atoms are joined together by covalent bonds throughout the whole structure. Diamond and silicon(oxide have similar structures. Which statements are correct?

2. Atoms, elements and compounds  →  2.6. Giant covalent structures

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7

The concentration of a hydrochloric acid solution is 0.5 mol / dm3. How many moles of hydrochloric acid are present in 25 cm3 of this solution?

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

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8

A sample of an iron oxide contains 50.4 g of iron and 21.6 g of oxygen. What is the empirical formula of the iron oxide?

3. Stoichiometry  →  3.1. Formulae

9. Metals  →  9.6. Extraction of metals

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9

A solution of copper(sulfate can be electrolysed using copper electrodes or carbon electrodes. Which statements are correct?

4. Electrochemistry  →  4.1. Electrolysis

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10

Pairs of metals are connected together to make a simple cell, as shown...

9. Metals  →  9.4. Reactivity series

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11

The energy level diagram for the reaction between X2 and Y2 to form XY gas is shown...

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

6. Chemical reactions  →  6.2. Rate of reaction

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12

Methane burns in oxygen to form carbon dioxide and water. CH4 + 2O2 → CO2 + 2H2O The bond energies are shown...

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

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13

Methanol is made by reacting carbon monoxide with hydrogen. The reaction is reversible. CO+ 2H2CH3OHThe forward reaction is exothermic. Which combination of temperature and pressure gives the highest equilibrium yield of methanol?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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14

The ionic equation for the reaction between zinc and aqueous copper ions is shown...

9. Metals  →  9.4. Reactivity series

6. Chemical reactions  →  6.4. Redox

4. Electrochemistry  →  4.1. Electrolysis

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15

In which reaction is the rate of reaction not affected by light?

6. Chemical reactions  →  6.2. Rate of reaction

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16

Calcium carbonate reacts with dilute hydrochloric acid to form bubbles of carbon dioxide. At a higher temperature, the same reaction is faster. Which row explains this observation?

6. Chemical reactions  →  6.2. Rate of reaction

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17

Ethanoic acid reacts with water to produce an acidic solution. Which row describes the roles of ethanoic acid and water in this reaction?

11. Organic chemistry  →  11.7. Carboxylic acids

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

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18

A solution of compound Z gives a light blue precipitate with aqueous ammonia. The precipitate dissolves in an excess of ammonia. A flame test is done on compound Z. What is the colour of the flame?

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

9. Metals  →  9.4. Reactivity series

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19

Carbon, copper, magnesium, sodium and sulfur can all form oxides. How many of these elements form acidic oxides?

9. Metals  →  9.4. Reactivity series

7. Acids, bases and salts  →  7.2. Oxides

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20

Which method is used to make the salt copper(sulfate?

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

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

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21

The Periodic Table lists all the known elements. Elements are arranged in order of 1 number. The melting points of Group I elements 2 down the group. The melting points of Group VII elements 3 down the group. Which words correctly complete gaps 1, 2 and 3?

8. The Periodic Table  →  8.1. Arrangement of elements

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22

Metal X reacts with non-metal Y to form an ionic compound with the formula X2Y. Which statements are correct?

8. The Periodic Table  →  8.1. Arrangement of elements

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

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23

Which statements about Group I and Group VII elements are correct?

8. The Periodic Table  →  8.3. Group VII properties

8. The Periodic Table  →  8.1. Arrangement of elements

8. The Periodic Table  →  8.2. Group I properties

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24

Which two properties are physical properties of all pure metals?

9. Metals  →  9.1. Properties of metals

9. Metals  →  9.3. Alloys and their properties

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25

Aluminium is extracted from aluminium oxide using electrolysis. Carbon dioxide is formed in this process. Which equation shows the formation of carbon dioxide during the extraction of aluminium from aluminium oxide by electrolysis?

9. Metals  →  9.6. Extraction of metals

9. Metals  →  9.4. Reactivity series

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26

A sample of solid X was added to three different solutions to predict the position of X in the reactivity series. X+ FeSO4→ no reaction X+ 2HCl→ XCl 2+ H2X+ Zn(NO3)2→ no reaction Which other solution would react with solid X?

9. Metals  →  9.4. Reactivity series

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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27

Which statement about the uses of aluminium, copper and iron is correct?

9. Metals  →  9.2. Uses of metals

9. Metals  →  9.3. Alloys and their properties

9. Metals  →  9.6. Extraction of metals

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28

Air is a mixture of gases. The melting and boiling points of some gases present in clean, dry air are shown...

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

10. Chemistry of the environment  →  10.1. Water

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

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29

Water must be purified before it is suitable for use in the home. Which processes are used to remove solid impurities and to kill bacteria?

10. Chemistry of the environment  →  10.1. Water

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

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30

Which processes do not produce carbon dioxide?

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

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31

Which pair of compounds would make an NPK fertiliser?

10. Chemistry of the environment  →  10.2. Fertilisers

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

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32

Which pollutant gas is produced by the decomposition of vegetation?

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

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33

The equation for the formation of sulfur trioxide from sulfur dioxide is shown...

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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34

The diagram shows the pH values of the soil in two parts of a garden, X and Y. X pH 7.0 Y pH 5.5 Lime is used to neutralise the soil in one part of the garden. To which part of the garden should the lime be added and why?

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

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35

Statement 1 Hydrogen is used as a fuel. Statement 2 When hydrogen burns in the air to form water, heat energy is produced. Which is correct?

4. Electrochemistry  →  4.2. Hydrogen–oxygen fuel cells

11. Organic chemistry  →  11.3. Fuels

11. Organic chemistry  →  11.6. Alcohols

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36

Which row identifies compounds in the same homologous series?

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

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37

Three chemical reactions are shown...

6. Chemical reactions  →  6.2. Rate of reaction

1. States of matter  →  1.2. Diffusion

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

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38

How is ethanol produced by fermentation?

11. Organic chemistry  →  11.6. Alcohols

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39

Which substances react together to form ethyl propanoate?

11. Organic chemistry  →  11.6. Alcohols

11. Organic chemistry  →  11.2. Naming organic compounds

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40

The structure of a chlorofluorocarbon polymer is shown...

11. Organic chemistry  →  11.8. Polymers

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