Edexcel GCSE Chemistry 2027 Predicted Practice Paper — Paper 1 Higher

Answer ALL questions. Write your answers in the spaces provided. You must write down all the stages in your working.

Section A

Multiple choice questions. Answer ALL questions.

• 1

  Question SECTION-A1 (1 mark)

  Which of these particles has a relative charge of 0 and a relative mass of 1?

  A. ProtonB. NeutronC. ElectronD. Positron

  (Total for Question SECTION-A1 is 1 mark)
• 2

  Question SECTION-A2 (1 mark)

  An atom has the electronic configuration 2,8,7. In which group of the periodic table is this element found?

  A. Group 1B. Group 5C. Group 7D. Group 0

  (Total for Question SECTION-A2 is 1 mark)
• 3

  Question SECTION-A3 (1 mark)

  Which of the following is the correct formula of aluminium sulfate?

  A. AlSO4B. Al2SO4C. Al2(SO4)3D. Al3(SO4)2

  (Total for Question SECTION-A3 is 1 mark)
• 4

  Question SECTION-A4 (1 mark)

  Which type of bonding holds the particles together in solid magnesium chloride?

  A. Metallic bondingB. Ionic bondingC. Covalent bondingD. Hydrogen bonding

  (Total for Question SECTION-A4 is 1 mark)
• 5

  Question SECTION-A5 (1 mark)

  Which statement about the noble gases in Group 0 is correct?

  A. They are very reactive metalsB. They have full outer electron shellsC. They readily form ionic compoundsD. Their boiling points decrease down the group

  (Total for Question SECTION-A5 is 1 mark)
• 6

  Question SECTION-A6 (1 mark)

  During electrolysis of molten lead(II) bromide, which product forms at the negative electrode (cathode)?

  A. BromineB. OxygenC. LeadD. Hydrogen

  (Total for Question SECTION-A6 is 1 mark)
• 7

  Question SECTION-A7 (1 mark)

  Which of these changes indicates that a chemical reaction, rather than a physical change, has taken place?

  A. Ice melting to waterB. Salt dissolving in waterC. A new gas being produced with a colour changeD. Water evaporating

  (Total for Question SECTION-A7 is 1 mark)
• 8

  Question SECTION-A8 (1 mark)

  The pH of a solution is 2. Which description best fits this solution?

  A. A weak alkaliB. A neutral solutionC. A strongly acidic solutionD. A strongly alkaline solution

  (Total for Question SECTION-A8 is 1 mark)
• 9

  Question SECTION-A9 (1 mark)

  Which gas is produced when dilute hydrochloric acid reacts with magnesium metal?

  A. OxygenB. Carbon dioxideC. ChlorineD. Hydrogen

  (Total for Question SECTION-A9 is 1 mark)
• 10

  Question SECTION-A10 (1 mark)

  Which statement correctly describes an exothermic reaction?

  A. It takes in energy from the surroundingsB. It causes the temperature of the surroundings to fallC. It releases energy to the surroundingsD. It has no overall energy change

  (Total for Question SECTION-A10 is 1 mark)
• 11

  Question SECTION-A11 (1 mark)

  Which of the following is the general formula of the alkanes?

  A. CnH2nB. CnH2n+2C. CnH2n-2D. CnHn

  (Total for Question SECTION-A11 is 1 mark)
• 12

  Question SECTION-A12 (1 mark)

  Crude oil is separated into fractions using fractional distillation. On what property does this separation depend?

  A. Colour of the hydrocarbonsB. Boiling point of the fractionsC. Solubility in waterD. Density in air

  (Total for Question SECTION-A12 is 1 mark)
• 13

  Question SECTION-A13 (1 mark)

  Which of these gases is a major greenhouse gas produced by the complete combustion of fossil fuels?

  A. NitrogenB. Carbon dioxideC. ArgonD. Hydrogen

  (Total for Question SECTION-A13 is 1 mark)
• 14

  Question SECTION-A14 (1 mark)

  Which piece of apparatus is most suitable for measuring exactly 25.0 cm^3 of an acid in a titration?

  A. Measuring cylinderB. BeakerC. PipetteD. Conical flask

  (Total for Question SECTION-A14 is 1 mark)
• 15

  Question SECTION-A15 (1 mark)

  A reaction reaches dynamic equilibrium in a closed system. Which statement is correct at equilibrium?

  A. The forward reaction has stoppedB. The concentrations of reactants and products remain constantC. All the reactants have been used upD. Only the backward reaction is occurring

  (Total for Question SECTION-A15 is 1 mark)
• 16

  Question SECTION-A16 (1 mark)

  Which of these metals is most likely to be extracted from its ore by electrolysis rather than by reduction with carbon?

  A. IronB. CopperC. AluminiumD. Lead

  (Total for Question SECTION-A16 is 1 mark)

Section B

Structured, short-answer, and calculation questions. Answer ALL questions.

• 1

  Question SECTION-B1 (4 marks)

  A sample of chlorine gas contains two isotopes: chlorine-35 and chlorine-37. In a sample, 76.0% of the atoms are chlorine-35 and 24.0% are chlorine-37. (a) State what is meant by the term 'isotopes'. (2 marks) (b) Calculate the relative atomic mass of chlorine in this sample. Give your answer to 1 decimal place. (2 marks)

  (Total for Question SECTION-B1 is 4 marks)
• 2

  Question SECTION-B2 (4 marks)

  Sodium hydroxide reacts with sulfuric acid according to the equation: 2NaOH + H2SO4 -> Na2SO4 + 2H2O (a) Name the type of reaction taking place. (1 mark) (b) 25.0 cm^3 of sodium hydroxide solution of concentration 0.100 mol/dm^3 is exactly neutralised. Calculate the number of moles of sodium hydroxide used. (2 marks) (c) Using your answer to (b), calculate the number of moles of sulfuric acid that reacted. (1 mark)

  (Total for Question SECTION-B2 is 4 marks)
• 3

  Question SECTION-B3 (6 marks)

  A student investigates the rate of reaction between marble chips (calcium carbonate) and dilute hydrochloric acid. They measure the total volume of carbon dioxide gas produced over time. (a) Give the balanced symbol equation for the reaction between calcium carbonate and hydrochloric acid, including state symbols. (3 marks) (b) The student repeats the experiment using more concentrated acid, keeping everything else the same. Explain, in terms of particles, why the rate of reaction increases. (3 marks)

  (Total for Question SECTION-B3 is 6 marks)
• 4

  Question SECTION-B4 (5 marks)

  Ethene (C2H4) can be used to make poly(ethene). (a) State the type of polymerisation that produces poly(ethene) from ethene. (1 mark) (b) Draw or describe the repeating unit of poly(ethene). (2 marks) (c) Explain one environmental problem caused by the disposal of poly(ethene) in landfill sites. (2 marks)

  (Total for Question SECTION-B4 is 5 marks)
• 5

  Question SECTION-B5 (7 marks)

  Iron is extracted from iron(III) oxide in a blast furnace by reduction with carbon monoxide: Fe2O3 + 3CO -> 2Fe + 3CO2 (a) Define oxidation and reduction in terms of oxygen. (2 marks) (b) Identify the substance that is reduced in this reaction and explain your answer. (2 marks) (c) Calculate the maximum mass of iron that can be produced from 320 g of iron(III) oxide. (Relative atomic masses: Fe = 56, O = 16.) (3 marks)

  (Total for Question SECTION-B5 is 7 marks)
• 6

  Question SECTION-B6 (4 marks)

  A simple chemical cell can be made using two different metals in an electrolyte. (a) State what determines the size of the voltage produced by a simple chemical cell using two different metals. (1 mark) (b) A hydrogen fuel cell produces electricity from hydrogen and oxygen. Write the overall balanced equation for the reaction that occurs in a hydrogen fuel cell. (1 mark) (c) Give two advantages of using hydrogen fuel cells compared with rechargeable batteries in vehicles. (2 marks)

  (Total for Question SECTION-B6 is 4 marks)
• 7

  Question SECTION-B7 (5 marks)

  Ammonia is manufactured in the Haber process: N2(g) + 3H2(g) <=> 2NH3(g) (forward reaction is exothermic) (a) State the source of the nitrogen and the source of the hydrogen used in this process. (2 marks) (b) The reaction is carried out at a pressure of about 200 atmospheres. Explain, using Le Chatelier's principle, why a high pressure increases the yield of ammonia. (3 marks)

  (Total for Question SECTION-B7 is 5 marks)
• 8

  Question SECTION-B8 (6 marks)

  A student carries out a titration to find the concentration of a hydrochloric acid solution using 0.150 mol/dm^3 sodium hydroxide. HCl + NaOH -> NaCl + H2O The student finds that 20.0 cm^3 of the sodium hydroxide solution exactly neutralises 25.0 cm^3 of the hydrochloric acid. (a) Name a suitable indicator for this titration and state the colour change seen at the end point (from acid to alkali). (2 marks) (b) Calculate the concentration of the hydrochloric acid in mol/dm^3. (4 marks)

  (Total for Question SECTION-B8 is 6 marks)
• 9

  Question SECTION-B9 (5 marks)

  Sodium chloride solution (brine) is electrolysed industrially. (a) Name the three products formed from the electrolysis of concentrated sodium chloride solution. (3 marks) (b) Write the half equation for the reaction occurring at the negative electrode (cathode). (2 marks)

  (Total for Question SECTION-B9 is 5 marks)
• 10

  Question SECTION-B10 (5 marks)

  A student measures the temperature change when a metal is added to copper(II) sulfate solution as part of a reactivity investigation. (a) State whether a displacement reaction between a more reactive metal and copper(II) sulfate is exothermic or endothermic, and describe what would be observed for the temperature. (2 marks) (b) Zinc is more reactive than copper. Write the balanced ionic equation for the displacement reaction between zinc and copper(II) ions, including state symbols. (3 marks)

  (Total for Question SECTION-B10 is 5 marks)
• 11

  Question SECTION-B11 (5 marks)

  Hydrocarbons can undergo cracking to produce more useful, smaller molecules. (a) Explain why long-chain hydrocarbons are cracked in industry. (2 marks) (b) Decane (C10H22) can be cracked to produce octane (C8H18) and one other product. Write a balanced equation for this cracking reaction and identify the other product. (3 marks)

  (Total for Question SECTION-B11 is 5 marks)

Section C

Extended response questions. Answer ALL questions.

• 1

  Question SECTION-C1 (6 marks)

  Chlorine, bromine and iodine are all elements in Group 7 of the periodic table (the halogens). Describe and explain the trend in reactivity of the halogens as you go down Group 7. In your answer you should refer to atomic structure, electron gain, and give an example of a displacement reaction to support your explanation.

  (Total for Question SECTION-C1 is 6 marks)
• 2

  Question SECTION-C2 (6 marks)

  Diamond, graphite and graphene are all forms (allotropes) of carbon, but they have very different properties. Compare the structure and bonding of diamond and graphite, and explain how their structures give rise to their different properties in terms of hardness and electrical conductivity.

  (Total for Question SECTION-C2 is 6 marks)
• 3

  Question SECTION-C3 (8 marks)

  A student is asked to prepare a pure, dry sample of copper(II) sulfate crystals starting from copper(II) oxide (an insoluble base) and dilute sulfuric acid. Describe a method the student could follow to prepare the crystals, explaining the purpose of the key steps. Include how they would ensure the reaction is complete and how they obtain dry crystals.

  (Total for Question SECTION-C3 is 8 marks)
• 4

  Question SECTION-C4 (8 marks)

  The Earth's early atmosphere was very different from the atmosphere today. Describe how the composition of the atmosphere is thought to have changed over the first few billion years of Earth's history, and explain the roles that volcanic activity, the oceans and early photosynthesising organisms played in these changes.

  (Total for Question SECTION-C4 is 8 marks)