AQA-GCSE CHEMISTRY 8462/1H
HIGHER TIER PAPER 1
Please write clearly in block capitals.
MERGED QUESTION PAPER &
Centre number
MARKING SCHEME COMBINED
JUNE 2024
Surname
Forename(s)
Candidate signature
Candidate number
I declare this is my own work.
GCSE
CHEMISTRY
Higher Tier Paper 1
H
Friday 17 May 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 1 Summary
The GCSE Chemistry Higher Tier Paper 1, scheduled for Friday, 17 May 2024 (Morning Session),
will focus on a range of foundational chemistry topics. The time allowed for this exam is 1 hour 45
minutes. This paper will assess students' knowledge in the following areas:
1. Atomic Structure and the Periodic Table:
o Structure of atoms, isotopes, and ions.
o The arrangement of elements in the periodic table, periodic trends, and properties of
metals and non-metals.
2. Chemical Bonding, Structure, and Properties:
o Ionic, covalent, and metallic bonding.
o Structure and properties of materials based on different types of bonding.
3. Quantitative Chemistry:
o Calculations involving moles, mass, and concentration.
o Understanding of the law of conservation of mass, empirical and molecular formulas,
and yield calculations.
4. Chemical Changes:
o Reactions involving acids (e.g., acid-alkali reactions, titration).
o Redox reactions, including oxidation and reduction.
o The reactivity series of metals and displacement reactions.
5. Energy Changes in Reactions:
o Exothermic and endothermic reactions.
o Energy profiles and enthalpy changes.
6. The Rate and Extent of Chemical Reactions:
o Factors that affect the rate of reaction, including temperature, concentration, surface
area, and catalysts.
7. Bonding, Structure, and Properties of Materials:
o Examination of solids, liquids, and gases, and their different states and transitions.
8. The Industrial Applications of Chemistry:
o Industrial processes such as the Haber process and the extraction of metals.
This paper will focus on assessing theoretical understanding, practical skills, and the ability to apply
chemical concepts to real-life scenarios. Students will also be expected to solve numerical problems
and demonstrate clear reasoning in their answers.
, 2
Do not write
outside the
0 1 A student produced a salt by reacting copper carbonate with sulfuric acid. box
This is the method used.
1. Measure 50 cm3 of sulfuric acid into a beaker.
2. Add copper carbonate powder.
3. Stir the mixture.
4. Repeat steps 2 and 3 until copper carbonate is in excess.
5. Filter the mixture.
6. Warm the filtrate gently until crystals start to appear.
7. Leave the solution to cool and crystallise.
0 1.1 Complete the word equation for the reaction.
[2 marks]
copper + sulfuric → + + carbon
carbonate acid dioxide
0 1 . 2 Give one observation the student could make during Step 4 which shows that the
copper carbonate is in excess.
[1 mark]
0 1.3 Give one reason for filtering the mixture in Step 5.
[1 mark]
*02*
IB/M/Jun24/8462/1H
, 3
Do not write
outside the
0 1.4 Name the equipment that can be used to warm the filtrate gently in Step 6. box
[1 mark]
0 1 . 5 The maximum theoretical mass of the salt that could be produced using 50 cm3 of the
sulfuric acid is 12.5 g.
The percentage yield of the salt is 92.8%.
Calculate the mass of salt actually produced.
Use the equation:
mass of salt actually produced
% yield = ×100
maximum theoretical mass of salt that could be produced
[3 marks]
Mass of salt actually produced = g
Question 1 continues on the next page
Turn over ►
*03*
IB/M/Jun24/8462/1H
HIGHER TIER PAPER 1
Please write clearly in block capitals.
MERGED QUESTION PAPER &
Centre number
MARKING SCHEME COMBINED
JUNE 2024
Surname
Forename(s)
Candidate signature
Candidate number
I declare this is my own work.
GCSE
CHEMISTRY
Higher Tier Paper 1
H
Friday 17 May 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 1 Summary
The GCSE Chemistry Higher Tier Paper 1, scheduled for Friday, 17 May 2024 (Morning Session),
will focus on a range of foundational chemistry topics. The time allowed for this exam is 1 hour 45
minutes. This paper will assess students' knowledge in the following areas:
1. Atomic Structure and the Periodic Table:
o Structure of atoms, isotopes, and ions.
o The arrangement of elements in the periodic table, periodic trends, and properties of
metals and non-metals.
2. Chemical Bonding, Structure, and Properties:
o Ionic, covalent, and metallic bonding.
o Structure and properties of materials based on different types of bonding.
3. Quantitative Chemistry:
o Calculations involving moles, mass, and concentration.
o Understanding of the law of conservation of mass, empirical and molecular formulas,
and yield calculations.
4. Chemical Changes:
o Reactions involving acids (e.g., acid-alkali reactions, titration).
o Redox reactions, including oxidation and reduction.
o The reactivity series of metals and displacement reactions.
5. Energy Changes in Reactions:
o Exothermic and endothermic reactions.
o Energy profiles and enthalpy changes.
6. The Rate and Extent of Chemical Reactions:
o Factors that affect the rate of reaction, including temperature, concentration, surface
area, and catalysts.
7. Bonding, Structure, and Properties of Materials:
o Examination of solids, liquids, and gases, and their different states and transitions.
8. The Industrial Applications of Chemistry:
o Industrial processes such as the Haber process and the extraction of metals.
This paper will focus on assessing theoretical understanding, practical skills, and the ability to apply
chemical concepts to real-life scenarios. Students will also be expected to solve numerical problems
and demonstrate clear reasoning in their answers.
, 2
Do not write
outside the
0 1 A student produced a salt by reacting copper carbonate with sulfuric acid. box
This is the method used.
1. Measure 50 cm3 of sulfuric acid into a beaker.
2. Add copper carbonate powder.
3. Stir the mixture.
4. Repeat steps 2 and 3 until copper carbonate is in excess.
5. Filter the mixture.
6. Warm the filtrate gently until crystals start to appear.
7. Leave the solution to cool and crystallise.
0 1.1 Complete the word equation for the reaction.
[2 marks]
copper + sulfuric → + + carbon
carbonate acid dioxide
0 1 . 2 Give one observation the student could make during Step 4 which shows that the
copper carbonate is in excess.
[1 mark]
0 1.3 Give one reason for filtering the mixture in Step 5.
[1 mark]
*02*
IB/M/Jun24/8462/1H
, 3
Do not write
outside the
0 1.4 Name the equipment that can be used to warm the filtrate gently in Step 6. box
[1 mark]
0 1 . 5 The maximum theoretical mass of the salt that could be produced using 50 cm3 of the
sulfuric acid is 12.5 g.
The percentage yield of the salt is 92.8%.
Calculate the mass of salt actually produced.
Use the equation:
mass of salt actually produced
% yield = ×100
maximum theoretical mass of salt that could be produced
[3 marks]
Mass of salt actually produced = g
Question 1 continues on the next page
Turn over ►
*03*
IB/M/Jun24/8462/1H
