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1

A sample of ethanol is left in an open beaker at room temperature. After 24 hours, no ethanol remains in the beaker. What has happened to the ethanol?

11. Organic chemistry  →  11.6. Alcohols

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2

A gas is in a sealed container with a fixed volume. Which statements describe what happens to the molecules in the gas when the temperature is increased?

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

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3

What happens when sodium atoms combine with chlorine atoms to form sodium chloride?

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

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

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4

The table shows some properties of four substances. substance melting point electrical conductivity when solid electrical conductivity when molten high poor poor high poor good low poor poor high good good Which substances are ionic?

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

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

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5

Which statement about methane is correct?

11. Organic chemistry  →  11.3. Fuels

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

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6

A sample of iridium has a relative atomic mass of 192.29. The sample contains two isotopes only. 64.50% of the sample is 193Ir. What is the other isotope in the sample?

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

2. Atoms, elements and compounds  →  2.3. Isotopes

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7

Ammonium iron(citrate contains in its formula: ● more than one ammonium ion ● one iron ion ● two C6H4O7 4– ions. What is the formula of ammonium iron(citrate?

9. Metals  →  9.6. Extraction of metals

3. Stoichiometry  →  3.1. Formulae

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

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8

Silicon(oxide reacts with chlorine and carbon to form liquid silicon(chloride, SiCl 4, and carbon dioxide gas. If the reaction is carried out at r.t.p., which symbol equation represents this reaction?

3. Stoichiometry  →  3.1. Formulae

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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9

The structure of ethene is shown...

3. Stoichiometry  →  3.1. Formulae

11. Organic chemistry  →  11.2. Naming organic compounds

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

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10

A known volume and concentration of aqueous sodium hydroxide is titrated against dilute hydrochloric acid. The volume of dilute hydrochloric acid needed to exactly neutralise the sodium hydroxide is measured. Five calculation steps are shown...

9. Metals  →  9.4. Reactivity series

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

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11

Two different substances are electrolysed using inert electrodes in two separate experiments. Hydrogen is produced in both experiments. Which row identifies the two substances and the electrode at which hydrogen is produced?

4. Electrochemistry  →  4.1. Electrolysis

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12

Aqueous copper(sulfate can be electrolysed using either carbon electrodes or copper electrodes. Which statement describes what happens at the positive electrode?

4. Electrochemistry  →  4.1. Electrolysis

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13

Which statement about a hydrogen–oxygen fuel cell is not correct?

4. Electrochemistry  →  4.2. Hydrogen–oxygen fuel cells

11. Organic chemistry  →  11.3. Fuels

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14

Which reaction pathway diagram is correctly labelled?

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

6. Chemical reactions  →  6.2. Rate of reaction

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15

Which row describes a reaction where the overall energy change is exothermic?

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

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16

Which process involves a physical change only?

6. Chemical reactions  →  6.1. Physical and chemical changes

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

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

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17

In the Haber process, an equilibrium is established. N2+ 3H22NH3The forward reaction is exothermic. Which change to the reaction conditions will move the position of equilibrium to the left?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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18

The flow chart shows some properties of a metal oxide. water + salt reduction metal oxide component of brass water + salt reaction with HCl reaction with NaOHWhat is the metal oxide?

9. Metals  →  9.4. Reactivity series

9. Metals  →  9.5. Corrosion of metals

7. Acids, bases and salts  →  7.2. Oxides

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19

Which statement about reactants in redox reactions is correct?

6. Chemical reactions  →  6.4. Redox

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20

Aluminium is extracted from aluminium oxide by electrolysis. The ionic half-equation for the reaction at one of the electrodes is shown...

6. Chemical reactions  →  6.4. Redox

4. Electrochemistry  →  4.1. Electrolysis

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21

Which statement about dilute hydrochloric acid is correct?

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

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22

Which row describes and gives the formula of hydrated copper(sulfate?

4. Electrochemistry  →  4.1. Electrolysis

10. Chemistry of the environment  →  10.1. Water

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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23

The equations for three reactions are shown...

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

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24

Acidified potassium dichromate(, K2Cr2O7, is used to oxidise ethanol, C2H5OH. The ionic equation for the reaction is shown...

8. The Periodic Table  →  8.4. Transition elements

6. Chemical reactions  →  6.4. Redox

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25

Which statements describe the Periodic Table?

8. The Periodic Table  →  8.1. Arrangement of elements

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

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26

Which row shows the correct order of reactivity of the four named metals?

9. Metals  →  9.4. Reactivity series

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27

Four iron nails are added to four different metal sulfate solutions. In which solution does a displacement reaction occur?

9. Metals  →  9.4. Reactivity series

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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28

A fertiliser contains ammonium nitrate and potassium phosphate. Why is the fertiliser described as 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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29

What are the approximate percentages of oxygen and nitrogen in clean, dry air?

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

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

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30

Which compounds have similar chemical properties?

11. Organic chemistry  →  11.2. Naming organic compounds

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

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

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31

Four statements about organic compounds P, Q, R and S are listed. P is a saturated hydrocarbon. The formula of Q is CH3CH3. A molecule of R contains only one oxygen atom. Compound S is a carboxylic acid. Which statement about these compounds is correct?

11. Organic chemistry  →  11.2. Naming organic compounds

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

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32

The structure of an organic compound is shown...

11. Organic chemistry  →  11.2. Naming organic compounds

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33

Which statement about the manufacture of ethene from larger alkane molecules is correct?

11. Organic chemistry  →  11.5. Alkenes

11. Organic chemistry  →  11.6. Alcohols

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34

Which processes are used to make ethanoic acid?

11. Organic chemistry  →  11.7. Carboxylic acids

11. Organic chemistry  →  11.6. Alcohols

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35

Which statement about propene, C3H6, is correct?

11. Organic chemistry  →  11.5. Alkenes

11. Organic chemistry  →  11.7. Carboxylic acids

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36

How many of each type of bond are present in ethanoic acid, CH3COOH?

11. Organic chemistry  →  11.2. Naming organic compounds

11. Organic chemistry  →  11.7. Carboxylic acids

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37

Which diagram represents the structure of a protein?

11. Organic chemistry  →  11.8. Polymers

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38

The chromatogram of substance S is shown...

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

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

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

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39

Some information about solid silver chloride and solid sodium chloride is shown...

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

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

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40

Which statement describes how a flame test is done?

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

11. Organic chemistry  →  11.5. Alkenes

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