2024 AQA
GCSE CHEMISTRY 8462/2H
Please write clearly in block capitals.
HIGHER TIER PAPER 2
Centre number
MERGED QUESTION PAPER &
MARKING SCHEME COMBINED
Surname JUNE 2024
Forename(s)
Candidate signature
Candidate number
I declare this is my own work.
GCSE
CHEMISTRY H
Higher Tier Paper 2
Tuesday 11 June 2024 Morning Time allowed: 1 hour 45 minutes
Materials
For this paper you must have: For Examiner’s Use
• a ruler
• a scientific calculator Question Mark
• the periodic table (enclosed).
1
Instructions 2
• Use black ink or black ball-point pen. 3
• Pencil should only be used for drawing. 4
• Fill in the boxes at the top of this page.
5
• Answer all questions in the spaces provided. Do not write outside
the box around each page or on blank pages. 6
• If you need extra space for your answer(s), use the lined pages at the end of 7
this book. Write the question number against your answer(s).
8
• Do all rough work in this book. Cross through any work you do not want
9
to be marked.
TOTAL
Information
• The maximum mark for this paper is 100.
• The marks for questions are shown in brackets.
• You are expected to use a calculator where appropriate.
• In all calculations, show clearly how you work out your answer.
• You are reminded of the need for good English and clear
presentation in your answers.
,GCSE Chemistry Higher Tier Paper 2 Summary
The GCSE Chemistry Higher Tier Paper 2, scheduled for Tuesday, 11 June 2024, will assess
students' knowledge and understanding of various core topics in chemistry. This includes:
1. Chemical Reactions: Types of reactions (e.g., combustion, oxidation, reduction), balancing
chemical equations, and understanding reaction rates and equilibrium.
2. Acids and Bases: pH scale, neutralization reactions, and titrations.
3. Organic Chemistry: Properties and uses of hydrocarbons, alkanes, alkenes, and alcohols.
4. Energy Changes: Exothermic and endothermic reactions, energy profiles, and calculations
related to energy.
5. The Periodic Table and Trends: Group properties, periodic trends in reactivity, and
elements' characteristics.
6. Materials and Properties: Properties of metals, alloys, and ceramics, as well as
polymerization and the uses of different materials.
7. Rates of Reaction and Reversible Reactions: Factors affecting the rate of reaction and
dynamic equilibrium principles.
8. Electrolysis and Chemical Cells: Processes involving electricity in chemistry, including
electrolysis and the function of chemical cells and batteries.
9. Quantitative Chemistry: Using molar calculations to determine concentrations, yields, and
the empirical formula.
This paper is designed to test a range of problem-solving skills, conceptual understanding, and
practical application of the chemical principles covered throughout the course. Students are expected
to apply their knowledge in real-world contexts and demonstrate analytical and evaluative skills in
chemistry.
, 2
Do not write
outside the
0 1 A student investigated an aqueous solution of a salt. box
The student identified that the salt solution contained only sodium ions and chloride
ions.
0 1 . 1 Describe a test to identify sodium ions.
Give the result of the test.
[2 marks]
Test for sodium ions
Result
0 1 . 2 Describe a test to identify chloride ions.
Give the result of the test.
[2 marks]
Test for chloride ions
Result
*02*
IB/M/Jun24/8462/2H
, 3
Do not write
outside the
The student determined the concentration of sodium chloride in the salt solution. box
This is the method used.
1. Weigh an empty evaporating dish.
2. Add 25.0 cm3 of the salt solution into the evaporating dish.
3. Heat the evaporating dish and contents.
4. Weigh the evaporating dish and contents.
5. Repeat steps 3 to 4 until there is no further change in mass.
6. Repeat steps 1 to 5 three more times.
0 1 . 3 Why did the student heat the evaporating dish and contents until the mass did not
change?
[1 mark]
0 1 . 4 How did the student calculate the mass of solid sodium chloride remaining after steps 1
to 5?
[1 mark]
Tick () one box.
Mass of 25 cm3 of salt solution + mass of empty evaporating dish
Mass of 25 cm3 of salt solution − mass of empty evaporating dish
Mass of evaporating dish and dry contents + mass of empty
evaporating dish
Mass of evaporating dish and dry contents − mass of empty
evaporating dish
Question 1 continues on the next page
Turn over ►
*03*
IB/M/Jun24/8462/2H
, 4
Do not write
outside the
0 1 . 5 The student calculated the concentration of sodium chloride in the salt solution. box
Table 1 shows the results.
Table 1
Concentration of sodium chloride in g/dm3
Trial 1 Trial 2 Trial 3 Trial 4
35.2 34.6 36.4 33.8
The percentage by mass of sodium ions in sodium chloride is 39.3%.
Calculate the mean concentration of sodium ions in the salt solution.
[4 marks]
10
Mean concentration = g/dm3
*04*
IB/M/Jun24/8462/2H
, 5
Do not write
outside the
0 2 This question is about ammonia and nitric acid. box
In the Haber process ammonia is produced from nitrogen and hydrogen.
Figure 1 represents the Haber process.
Figure 1
0 2 . 1 Pipe P links the condenser to the reactor. Why
is the condenser linked to the reactor? Use
Figure 1.
[1 mark]
0 2.2 Which metal is used as a catalyst in this reaction?
[1 mark]
Turn over ►
*05*
IB/M/Jun24/8462/2H
, 6
Do not write
outside the
Nitric acid is produced by reacting ammonia with oxygen. box
The word equation for the production of nitric acid is:
ammonia + oxygen → water + nitric acid
Platinum is a catalyst in this reaction.
0 2 . 3 Describe the test for oxygen gas.
Give the result if oxygen gas is present.
[2 marks]
Test
Result
Figure 2 represents the reaction profile of the catalysed reaction between ammonia
and oxygen.
Figure 2
*06*
IB/M/Jun24/8462/2H
, 7
Do not write
outside the
0 2 . 4 Complete the reaction profile for the catalysed reaction in Figure 2. box
You should:
• label the activation energy
• label the reactants and products, using the names of the reactants and products.
[2 marks]
0 2.5 How would Figure 2 be different if no catalyst was used?
[1 mark]
Tick () one box.
The final energy level would be higher.
The final energy level would be lower.
The line would reach a higher peak.
The line would reach a lower peak.
0 2 . 6 Ammonia and nitric acid react to produce the salt, ammonium nitrate.
Ammonium ions and nitrate ions both contain nitrogen.
Suggest one use of ammonium nitrate.
[1 mark]
8
Turn over for the next question
Turn over ►
*07*
IB/M/Jun24/8462/2H
, 8
Do not write
outside the
There are no questions printed on this page box
DO NOT WRITE ON THIS PAGE
ANSWER IN THE SPACES PROVIDED
*08*
IB/M/Jun24/8462/2H
, 9
Do not write
outside the
0 3 This question is about water. box
0 3 . 1 Hydrogen gas reacts with oxygen gas to produce water.
Water is decomposed into hydrogen gas and oxygen gas using electricity.
Which two words describe the reaction between hydrogen gas and oxygen gas?
[2 marks]
Tick () two boxes.
Alloying
Combustion
Corrosion
Endothermic
Reversible
0 3.2 Water molecules break down into hydrogen ions and hydroxide ions.
The equation for the reaction is:
H2O ⇌ H+ + OH–
Which sentence describes this reaction at equilibrium?
[1 mark]
Tick () one box.
Water molecules break down at a higher rate than they reform.
Water molecules break down and reform at the same rate.
Water molecules break down at a lower rate than they reform.
Question 3 continues on the next page
Turn over ►
*09*
IB/M/Jun24/8462/2H
GCSE CHEMISTRY 8462/2H
Please write clearly in block capitals.
HIGHER TIER PAPER 2
Centre number
MERGED QUESTION PAPER &
MARKING SCHEME COMBINED
Surname JUNE 2024
Forename(s)
Candidate signature
Candidate number
I declare this is my own work.
GCSE
CHEMISTRY H
Higher Tier Paper 2
Tuesday 11 June 2024 Morning Time allowed: 1 hour 45 minutes
Materials
For this paper you must have: For Examiner’s Use
• a ruler
• a scientific calculator Question Mark
• the periodic table (enclosed).
1
Instructions 2
• Use black ink or black ball-point pen. 3
• Pencil should only be used for drawing. 4
• Fill in the boxes at the top of this page.
5
• Answer all questions in the spaces provided. Do not write outside
the box around each page or on blank pages. 6
• If you need extra space for your answer(s), use the lined pages at the end of 7
this book. Write the question number against your answer(s).
8
• Do all rough work in this book. Cross through any work you do not want
9
to be marked.
TOTAL
Information
• The maximum mark for this paper is 100.
• The marks for questions are shown in brackets.
• You are expected to use a calculator where appropriate.
• In all calculations, show clearly how you work out your answer.
• You are reminded of the need for good English and clear
presentation in your answers.
,GCSE Chemistry Higher Tier Paper 2 Summary
The GCSE Chemistry Higher Tier Paper 2, scheduled for Tuesday, 11 June 2024, will assess
students' knowledge and understanding of various core topics in chemistry. This includes:
1. Chemical Reactions: Types of reactions (e.g., combustion, oxidation, reduction), balancing
chemical equations, and understanding reaction rates and equilibrium.
2. Acids and Bases: pH scale, neutralization reactions, and titrations.
3. Organic Chemistry: Properties and uses of hydrocarbons, alkanes, alkenes, and alcohols.
4. Energy Changes: Exothermic and endothermic reactions, energy profiles, and calculations
related to energy.
5. The Periodic Table and Trends: Group properties, periodic trends in reactivity, and
elements' characteristics.
6. Materials and Properties: Properties of metals, alloys, and ceramics, as well as
polymerization and the uses of different materials.
7. Rates of Reaction and Reversible Reactions: Factors affecting the rate of reaction and
dynamic equilibrium principles.
8. Electrolysis and Chemical Cells: Processes involving electricity in chemistry, including
electrolysis and the function of chemical cells and batteries.
9. Quantitative Chemistry: Using molar calculations to determine concentrations, yields, and
the empirical formula.
This paper is designed to test a range of problem-solving skills, conceptual understanding, and
practical application of the chemical principles covered throughout the course. Students are expected
to apply their knowledge in real-world contexts and demonstrate analytical and evaluative skills in
chemistry.
, 2
Do not write
outside the
0 1 A student investigated an aqueous solution of a salt. box
The student identified that the salt solution contained only sodium ions and chloride
ions.
0 1 . 1 Describe a test to identify sodium ions.
Give the result of the test.
[2 marks]
Test for sodium ions
Result
0 1 . 2 Describe a test to identify chloride ions.
Give the result of the test.
[2 marks]
Test for chloride ions
Result
*02*
IB/M/Jun24/8462/2H
, 3
Do not write
outside the
The student determined the concentration of sodium chloride in the salt solution. box
This is the method used.
1. Weigh an empty evaporating dish.
2. Add 25.0 cm3 of the salt solution into the evaporating dish.
3. Heat the evaporating dish and contents.
4. Weigh the evaporating dish and contents.
5. Repeat steps 3 to 4 until there is no further change in mass.
6. Repeat steps 1 to 5 three more times.
0 1 . 3 Why did the student heat the evaporating dish and contents until the mass did not
change?
[1 mark]
0 1 . 4 How did the student calculate the mass of solid sodium chloride remaining after steps 1
to 5?
[1 mark]
Tick () one box.
Mass of 25 cm3 of salt solution + mass of empty evaporating dish
Mass of 25 cm3 of salt solution − mass of empty evaporating dish
Mass of evaporating dish and dry contents + mass of empty
evaporating dish
Mass of evaporating dish and dry contents − mass of empty
evaporating dish
Question 1 continues on the next page
Turn over ►
*03*
IB/M/Jun24/8462/2H
, 4
Do not write
outside the
0 1 . 5 The student calculated the concentration of sodium chloride in the salt solution. box
Table 1 shows the results.
Table 1
Concentration of sodium chloride in g/dm3
Trial 1 Trial 2 Trial 3 Trial 4
35.2 34.6 36.4 33.8
The percentage by mass of sodium ions in sodium chloride is 39.3%.
Calculate the mean concentration of sodium ions in the salt solution.
[4 marks]
10
Mean concentration = g/dm3
*04*
IB/M/Jun24/8462/2H
, 5
Do not write
outside the
0 2 This question is about ammonia and nitric acid. box
In the Haber process ammonia is produced from nitrogen and hydrogen.
Figure 1 represents the Haber process.
Figure 1
0 2 . 1 Pipe P links the condenser to the reactor. Why
is the condenser linked to the reactor? Use
Figure 1.
[1 mark]
0 2.2 Which metal is used as a catalyst in this reaction?
[1 mark]
Turn over ►
*05*
IB/M/Jun24/8462/2H
, 6
Do not write
outside the
Nitric acid is produced by reacting ammonia with oxygen. box
The word equation for the production of nitric acid is:
ammonia + oxygen → water + nitric acid
Platinum is a catalyst in this reaction.
0 2 . 3 Describe the test for oxygen gas.
Give the result if oxygen gas is present.
[2 marks]
Test
Result
Figure 2 represents the reaction profile of the catalysed reaction between ammonia
and oxygen.
Figure 2
*06*
IB/M/Jun24/8462/2H
, 7
Do not write
outside the
0 2 . 4 Complete the reaction profile for the catalysed reaction in Figure 2. box
You should:
• label the activation energy
• label the reactants and products, using the names of the reactants and products.
[2 marks]
0 2.5 How would Figure 2 be different if no catalyst was used?
[1 mark]
Tick () one box.
The final energy level would be higher.
The final energy level would be lower.
The line would reach a higher peak.
The line would reach a lower peak.
0 2 . 6 Ammonia and nitric acid react to produce the salt, ammonium nitrate.
Ammonium ions and nitrate ions both contain nitrogen.
Suggest one use of ammonium nitrate.
[1 mark]
8
Turn over for the next question
Turn over ►
*07*
IB/M/Jun24/8462/2H
, 8
Do not write
outside the
There are no questions printed on this page box
DO NOT WRITE ON THIS PAGE
ANSWER IN THE SPACES PROVIDED
*08*
IB/M/Jun24/8462/2H
, 9
Do not write
outside the
0 3 This question is about water. box
0 3 . 1 Hydrogen gas reacts with oxygen gas to produce water.
Water is decomposed into hydrogen gas and oxygen gas using electricity.
Which two words describe the reaction between hydrogen gas and oxygen gas?
[2 marks]
Tick () two boxes.
Alloying
Combustion
Corrosion
Endothermic
Reversible
0 3.2 Water molecules break down into hydrogen ions and hydroxide ions.
The equation for the reaction is:
H2O ⇌ H+ + OH–
Which sentence describes this reaction at equilibrium?
[1 mark]
Tick () one box.
Water molecules break down at a higher rate than they reform.
Water molecules break down and reform at the same rate.
Water molecules break down at a lower rate than they reform.
Question 3 continues on the next page
Turn over ►
*09*
IB/M/Jun24/8462/2H
