Download 2025 Pearson Edexcel International GCSE Chemistry (4CH1/2C) Question Paper 2C and MS and more Exams Chemistry in PDF only on Docsity!
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Pearson Edexcel International GCSE (9–1)
Friday 13 June 2025
Morning (Time: 1 hour 15 minutes)
Chemistry
Paper
reference
4CH1/2C
Total Marks
Instructions
If pencil is used for diagrams/sketches/graphs it must be dark (HB or B).
centre number and candidate number.
Answer the questions in the spaces provided
- there may be more space than you need.
Show all the steps in any calculations and state the units.
Information
The total mark for this paper is 70.
- use this as a guide as to how much time to spend on each question.
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Read each question carefully before you start to answer it.
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UNIT: 4CH
PAPER: 2C
Pearson Edexcel International GCSE Chemistry (4CH1/2C) Question Paper
2C and Mark Scheme Summer 2025
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calcium fluorine
petrol silicon
helium neon
Answer ALL questions.
Some questions must be answered with a cross in a box. If you change your mind about an
answer, put a line through the box and then mark your new answer with a cross.
1 This question is about elements, compounds and mixtures.
(a) The box gives the names of some substances.
Choose a substance from the box to answer each of these questions.
(i) Give the name of a compound.
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(ii) Give the name of a mixture.
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(iii) Give the name of a diatomic molecule.
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(iv) Give the name of a metal element.
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(b) (i) Name the technique used to separate crude oil into fractions.
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(ii) Give one use of the kerosene fraction.
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(Total for Question 1 = 6 marks)
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(d) Explain why increasing the temperature of the hydrochloric acid affects the rate of
the reaction.
Refer to collision theory in your answer.
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(e) Draw a reaction profile diagram for the reaction, showing Δ H and
activation energy.
Label the reactants and products.
Energy
...........................................
(Total for Question 2 = 13 marks)
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3 This question is about Group 2 elements and their compounds.
(a) A sample of magnesium contains three isotopes.
Mass number of isotope 24 25 26
Percentage abundance (%) 76.5 10.5 13.
(i) State, in terms of subatomic particles, what is meant by the term isotopes.
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(ii) Calculate the relative atomic mass ( A r ) of magnesium.
Give your answer to one decimal place.
(b) Which of these compounds is an insoluble solid?
A calcium nitrate
B calcium sulfate
C magnesium nitrate
D magnesium sulfate
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(d) The table lists some substances and shows which substance conducts electricity.
Substance Conducts electricity?
water no
solid magnesium chloride no
aqueous magnesium chloride yes
Explain these observations.
Refer to structure and bonding in your answer.
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(e) A concentrated aqueous solution of magnesium chloride is electrolysed.
Chlorine forms at the positive electrode.
(i) Give the half-equation for the reaction at the positive electrode.
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(ii) Give a reason why this reaction is classified as oxidation.
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(Total for Question 3 = 16 marks)
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(c) A student prepares the ester, ethyl ethanoate, by reacting ethanol with
ethanoic acid.
This is the student’s method.
- mix equal amounts of ethanol and ethanoic acid in a boiling tube
- add a few drops of concentrated sulfuric acid
- place the boiling tube in a hot water bath for several minutes
(i) State the role of sulfuric acid in this reaction.
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(ii) State why the student heats the mixture in a water bath instead of directly
with a Bunsen burner flame.
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(iii) State how the student would know that ethyl ethanoate has formed.
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(iv) Draw the displayed formula of ethyl ethanoate.
(Total for Question 4 = 12 marks)
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5 A student does a titration to find the concentration of a solution of sulfuric acid.
This is the student’s method.
- fill a burette with sulfuric acid and record the reading
- transfer 25.0 cm
3
of potassium hydroxide solution to a conical flask
- add a few drops of methyl orange to the conical flask
- place the conical flask on a white tile
- swirl the flask continuously while adding sulfuric acid from the burette
- keep adding sulfuric acid until the end-point has been reached
- record the rough reading at the end-point
(a) (i) Name the most suitable piece of apparatus for measuring 25.0 cm
3
of
potassium hydroxide solution.
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(ii) State why the student places the conical flask on a white tile.
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(d) Another student also does the titration.
(i) The student uses 25.0 cm
3
of potassium hydroxide solution with a
concentration of 0.500 mol/dm
3
.
The mean volume of sulfuric acid added is 26.50 cm
3
.
This is the equation for the reaction.
2KOH(aq) + H 2
SO
4 (aq) → K 2
SO
4 (aq) + 2H 2 O(l)
Calculate the concentration of the sulfuric acid.
concentration of sulfuric acid =........................... mol/dm
3
(ii) The student repeats the titration without the methyl orange indicator.
They add exactly 26.50 cm
3
of sulfuric acid to the potassium hydroxide solution.
Describe how the student could obtain pure, dry potassium sulfate crystals
from the reaction mixture.
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(Total for Question 5 = 13 marks)
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(c) An excess of hydrogen reacts with 50.8 g of iodine.
At equilibrium, the yield of hydrogen iodide is 80%.
Calculate the volume, in cm
3
, of hydrogen iodide produced at rtp.
Give your answer in standard form.
[at rtp, molar volume = 24 000 cm
3
]
volume of hydrogen iodide = ........................... cm
3
(Total for Question 6 = 10 marks)
TOTAL FOR PAPER = 70 MARKS
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