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1

A mixture of sand and sodium chloride can be separated in three steps. Step 1 is to add water to the mixture. The diagram shows step 2 and step 3. Where is pure sodium chloride collected?

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

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

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2

The results of two tests on solution X are shown...

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

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

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3

Which diagram shows the arrangement of particles inside a balloon containing a mixture of the gases nitrogen and oxygen?

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

1. States of matter  →  1.2. Diffusion

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

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4

A student follows the rate of the reaction between marble chips, CaCO3, and dilute hydrochloric acid. CaCO3 + 2HCl → CaCl 2 + CO2 + H2O Which diagrams show apparatus that is suitable for this experiment?

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

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

6. Chemical reactions  →  6.2. Rate of reaction

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5

A chemist wishes to separate and identify a mixture of substances using paper chromatography. The diagram shows the apparatus used. The solvent is water. solvent The solvent front is allowed to reach the top of the paper before the chemist removes the paper from the solvent. Which problem does this cause?

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

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

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6

Which particle contains the same number of both neutrons and electrons?

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

2. Atoms, elements and compounds  →  2.3. Isotopes

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7

Which statement is correct for all metals?

9. Metals  →  9.1. Properties of metals

4. Electrochemistry  →  4.1. Electrolysis

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8

X represents the element of atomic number 8 and Y represents the element of atomic number 19. The two elements react together to form a compound. Which row is correct for the compound formed?

3. Stoichiometry  →  3.1. Formulae

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

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9

The empirical formula of a liquid compound is C2H4O. To find the empirical formula, it is necessary to know A the density of the compound. B the percentage composition by mass of the compound. C the relative molecular mass of the compound. D the volume occupied by 1 mole of the compound.

3. Stoichiometry  →  3.1. Formulae

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10

25.0 g of hydrated copper(sulfate crystals are heated to produce anhydrous copper(sulfate and water vapour. CuSO4.5H2O→ CuSO4+ 5H2OWhat is the mass of anhydrous copper(sulfate formed?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

4. Electrochemistry  →  4.1. Electrolysis

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

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11

Which sample contains the most atoms?

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

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

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12

The relative atomic mass of chlorine is 35.5. What is the mass of 2 moles of chlorine gas?

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

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

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13

One mole of an organic compound, Q, is completely burnt in oxygen and produces exactly three moles of water. Which compound is Q?

11. Organic chemistry  →  11.3. Fuels

11. Organic chemistry  →  11.6. Alcohols

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14

In an experiment, 1 mol of powdered copper and 1 mol of powdered zinc are placed in a flask. Dilute acid, containing 1 mol of acid, is added to the flask. The flask is left until all the reactions, if any, are complete. Which diagram shows the result of the experiment?

9. Metals  →  9.4. Reactivity series

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

4. Electrochemistry  →  4.1. Electrolysis

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15

A simple cell can be made using two different metals as the electrodes and an aqueous solution as the electrolyte. Which statements about simple cells are correct?

4. Electrochemistry  →  4.1. Electrolysis

9. Metals  →  9.4. Reactivity series

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16

Magnesium can be produced by electrolysis of molten magnesium chloride, MgCl 2. What are the equations for the reactions that occur at the positive electrode and at the negative electrode?

4. Electrochemistry  →  4.1. Electrolysis

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17

Three different solutions were electrolysed using inert electrodes. solution 1 aqueous sodium chloride solution 2 concentrated hydrochloric acid solution 3 dilute sulfuric acid Which solutions produce hydrogen at the negative electrode?

4. Electrochemistry  →  4.1. Electrolysis

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18

Compound Y reacts with oxygen. This reaction has a positive enthalpy change of reaction, ∆H. What information can be deduced about Y and its reaction with oxygen?

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

6. Chemical reactions  →  6.2. Rate of reaction

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19

The formation of liquid water from hydrogen and oxygen may occur in three stages. 2H2+ O2→ 4H+ 2O2 4H+ 2O→ 2H2O3 2H2O→ 2H2O(Which stages are endothermic?

4. Electrochemistry  →  4.2. Hydrogen–oxygen fuel cells

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

10. Chemistry of the environment  →  10.1. Water

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20

Sulfur trioxide is produced by the following reaction. 2SO2+ O22SO3∆H = –195 kJ Which change in conditions would produce a greater amount of SO3 at equilibrium?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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21

Magnesium reacts with dilute sulfuric acid. Mg+ H2SO4→ MgSO4+ H2Two experiments were carried out. experiment 1 24.0 g of magnesium was reacted with 100 cm3 of 1.0 mol / dm3 sulfuric acid. experiment 2 24.0 g of magnesium was reacted with 50 cm3 of 2.0 mol / dm3 sulfuric acid. In each experiment the volume of hydrogen was measured at various times. The results were plotted on a graph. Which graph is correct?

6. Chemical reactions  →  6.2. Rate of reaction

9. Metals  →  9.4. Reactivity series

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22

Which statement is correct for both aluminium and iron?

9. Metals  →  9.2. Uses of metals

9. Metals  →  9.5. Corrosion of metals

9. Metals  →  9.4. Reactivity series

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23

A household cleaning compound is used to remove calcium carbonate from bathroom surfaces. The compound reacts with the calcium carbonate to form a soluble salt, carbon dioxide and water. What is the pH of this cleaning compound?

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

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

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24

Dilute hydrochloric acid is added separately to samples of copper, copper(oxide and copper(carbonate. Which row correctly shows whether copper(chloride is produced?

4. Electrochemistry  →  4.1. Electrolysis

10. Chemistry of the environment  →  10.1. Water

9. Metals  →  9.4. Reactivity series

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25

Which ions are present when hydrochloric acid has exactly neutralised aqueous sodium hydroxide?

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

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

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26

Which experiment will result in the formation of a white precipitate?

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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27

Which statement about both the Group I and Group VII elements is correct?

8. The Periodic Table  →  8.3. Group VII properties

8. The Periodic Table  →  8.1. Arrangement of elements

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28

The elements helium, argon and neon are noble gases. Which statement is correct?

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

8. The Periodic Table  →  8.5. Noble gases

8. The Periodic Table  →  8.4. Transition elements

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29

Which row shows the correct catalyst for each industrial process?

11. Organic chemistry  →  11.5. Alkenes

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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30

In the solid state, germanium has the same structure as diamond. What is the likely melting point of germanium?

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

10. Chemistry of the environment  →  10.1. Water

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31

Aluminium is a metal that is often used to make caps for bottles. When thrown away and buried in the soil, the caps do not corrode. Why is this?

9. Metals  →  9.4. Reactivity series

9. Metals  →  9.2. Uses of metals

9. Metals  →  9.6. Extraction of metals

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32

Which statement about Group I metals is correct?

8. The Periodic Table  →  8.2. Group I properties

8. The Periodic Table  →  8.4. Transition elements

9. Metals  →  9.1. Properties of metals

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33

CFC compounds were used as aerosol propellants. The structure of one CFC compound is shown...

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

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34

Dry air is a mixture of gases of which 99% is nitrogen and oxygen. What is the main constituent of the remaining 1%?

11. Organic chemistry  →  11.3. Fuels

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

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35

Why is chlorine added to the water supply?

10. Chemistry of the environment  →  10.1. Water

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36

When the alcohol of molecular formula C4H10O is oxidised, what is the molecular formula of the acid formed?

11. Organic chemistry  →  11.7. Carboxylic acids

3. Stoichiometry  →  3.1. Formulae

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37

The diagrams show the structures of five hydrocarbons. H C C C H H H H H H H H H H C C H H C C C H H H H H H C H H H H C C C H H H H H C H H H C H H H H C C C H H H H H H C H H H H H C C C C H H H H H H H H H H C Which three hydrocarbons are isomers of each other?

11. Organic chemistry  →  11.2. Naming organic compounds

11. Organic chemistry  →  11.3. Fuels

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38

Which alcohol and acid will react together to make the ester CH3COOC2H5?

11. Organic chemistry  →  11.7. Carboxylic acids

11. Organic chemistry  →  11.6. Alcohols

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39

Which compound has a pH of less than 7 in aqueous solution?

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

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40

Which statement about polymers is correct?

11. Organic chemistry  →  11.8. Polymers

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