AQA 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. Answer ALL questions in the spaces provided.

• 1

  Question SECTION-A1 (1 mark)

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

  A. Group 7, Period 3B. Group 5, Period 2C. Group 7, Period 2D. Group 8, Period 3

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

  Question SECTION-A2 (1 mark)

  Which particle is gained or lost when an atom becomes a negatively charged ion?

  A. It loses a protonB. It gains an electronC. It loses an electronD. It gains a proton

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

  Question SECTION-A3 (1 mark)

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

  A. AlSO4B. Al2(SO4)3C. Al3(SO4)2D. Al2SO4

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

  Question SECTION-A4 (1 mark)

  Which statement about the nucleus of an atom is correct?

  A. It contains protons and electronsB. It has a relative charge of zeroC. It contains protons and neutronsD. It occupies most of the volume of the atom

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

  Question SECTION-A5 (1 mark)

  A substance conducts electricity when molten but not when solid. What type of structure does it most likely have?

  A. Simple molecularB. Giant covalentC. MetallicD. Giant ionic

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

  Question SECTION-A6 (1 mark)

  Which of these is an example of a chemical change?

  A. Melting iceB. Dissolving salt in waterC. Rusting of ironD. Boiling water

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

  Question SECTION-A7 (1 mark)

  The relative formula mass (Mr) of calcium carbonate, CaCO3, is: (Ar: Ca = 40, C = 12, O = 16)

  A. 68B. 84C. 100D. 116

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

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

  Question SECTION-A9 (1 mark)

  Which change would increase the rate of a reaction between marble chips and dilute hydrochloric acid?

  A. Using larger marble chipsB. Lowering the temperatureC. Increasing the acid concentrationD. Adding more water to the acid

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

  Question SECTION-A10 (1 mark)

  Which of the following is an alkane?

  A. C2H4B. C3H8C. C2H5OHD. C3H6

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

  Question SECTION-A11 (1 mark)

  What is the pH range of a strongly acidic solution?

  A. 0 to 2B. 6 to 7C. 7 to 8D. 12 to 14

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

  Question SECTION-A12 (1 mark)

  Which gas turns limewater cloudy (milky)?

  A. HydrogenB. OxygenC. Carbon dioxideD. Chlorine

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

  Question SECTION-A13 (1 mark)

  Two isotopes of the same element always have the same number of:

  A. NeutronsB. ProtonsC. NucleonsD. Occupied energy levels of neutrons

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

  Question SECTION-A14 (1 mark)

  Which process is used to obtain pure water from seawater in the laboratory?

  A. FiltrationB. CrystallisationC. Simple distillationD. Chromatography

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

  Question SECTION-A15 (1 mark)

  In the reaction 2Mg + O2 -> 2MgO, magnesium is:

  A. Reduced, because it loses oxygenB. Oxidised, because it loses electronsC. Reduced, because it gains electronsD. Oxidised, because it gains electrons

  (Total for Question SECTION-A15 is 1 mark)

Section B

Structured short-answer questions. Answer ALL questions in the spaces provided.

• 1

  Question SECTION-B1 (5 marks)

  A student investigates the reaction between zinc metal and dilute sulfuric acid: Zn + H2SO4 -> ZnSO4 + H2. (a) Name the salt produced. (b) Describe the chemical test, and its positive result, that would confirm the gas produced is hydrogen. (c) Explain, in terms of particles, why powdered zinc reacts faster than a single lump of zinc of the same mass.

  (Total for Question SECTION-B1 is 5 marks)
• 2

  Question SECTION-B2 (5 marks)

  Chlorine (2,8,7) and sodium (2,8,1) react to form sodium chloride. (a) Describe, in terms of electron transfer, how a sodium atom and a chlorine atom form ions. (b) Give the charges on the two ions formed. (c) State the type of bonding in sodium chloride and explain why sodium chloride has a high melting point.

  (Total for Question SECTION-B2 is 5 marks)
• 3

  Question SECTION-B3 (4 marks)

  A sample of an oxide of copper is found to contain 8.0 g of copper combined with 2.0 g of oxygen. (Ar: Cu = 64, O = 16.) (a) Calculate the number of moles of copper atoms and the number of moles of oxygen atoms in the sample. (b) Use your answers to determine the empirical formula of the copper oxide. Show your working.

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

  Question SECTION-B4 (5 marks)

  The Haber process is used to manufacture ammonia: N2(g) + 3H2(g) <=> 2NH3(g) (forward reaction is exothermic). (a) State the meaning of the <=> symbol. (b) Typical conditions are 450 degrees C and 200 atmospheres. Explain why a temperature higher than 450 degrees C is NOT used, referring to yield. (c) Explain why a high pressure gives a higher yield of ammonia.

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

  Question SECTION-B5 (5 marks)

  A student carries out a titration to find the concentration of a sodium hydroxide solution. 25.0 cm^3 of the sodium hydroxide solution is neutralised by 20.0 cm^3 of 0.100 mol/dm^3 hydrochloric acid. HCl + NaOH -> NaCl + H2O. (a) Name a suitable indicator and state its colour change from acid to alkali. (b) Calculate the number of moles of HCl used. (c) Calculate the concentration of the sodium hydroxide solution in mol/dm^3. Show your working.

  (Total for Question SECTION-B5 is 5 marks)
• 6

  Question SECTION-B6 (5 marks)

  Crude oil is separated into useful fractions by fractional distillation. (a) State what is meant by a 'fraction'. (b) Explain why hydrocarbons with larger molecules have higher boiling points. (c) Long-chain hydrocarbons can be broken down by cracking. Give one reason why cracking is carried out and name the type of useful, more reactive hydrocarbon produced that is used to make polymers.

  (Total for Question SECTION-B6 is 5 marks)
• 7

  Question SECTION-B7 (4 marks)

  Calcium carbonate decomposes when heated strongly: CaCO3 -> CaO + CO2. A student heats 25.0 g of pure calcium carbonate until it fully decomposes. (Mr: CaCO3 = 100, CaO = 56, CO2 = 44.) (a) Calculate the number of moles of calcium carbonate used. (b) Calculate the mass of calcium oxide produced. (c) Calculate the mass of carbon dioxide lost to the surroundings.

  (Total for Question SECTION-B7 is 4 marks)
• 8

  Question SECTION-B8 (5 marks)

  The alkali metals are in Group 1 of the periodic table. (a) Describe what you would observe when a small piece of lithium is added to a trough of water. (b) Write a balanced symbol equation for the reaction of lithium with water. (c) Explain, in terms of electronic structure, why potassium is more reactive than lithium.

  (Total for Question SECTION-B8 is 5 marks)
• 9

  Question SECTION-B9 (5 marks)

  Diamond and graphite are both forms (allotropes) of carbon. (a) State one physical property of diamond and one different physical property of graphite. (b) Explain, in terms of structure and bonding, why graphite can conduct electricity but diamond cannot. (c) Give one use of graphite that depends on its ability to conduct electricity.

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

  Question SECTION-B10 (5 marks)

  A student uses a gas syringe to measure the volume of carbon dioxide produced over time when calcium carbonate reacts with excess dilute hydrochloric acid. (a) Sketch and describe the shape of the graph of volume of gas (y-axis) against time (x-axis), stating what happens to the gradient during the reaction. (b) Explain, using collision theory, why the rate of reaction decreases as the reaction proceeds. (c) State how you could tell from the graph when the reaction had finished.

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

  Question SECTION-B11 (6 marks)

  Copper sulfate crystals can be made in the laboratory by reacting excess copper(II) oxide (a base) with dilute sulfuric acid. CuO + H2SO4 -> CuSO4 + H2O. (a) Explain why excess copper(II) oxide is added. (b) Describe how the excess (unreacted) copper(II) oxide is removed from the mixture. (c) Describe how pure, dry crystals of copper sulfate are obtained from the copper sulfate solution.

  (Total for Question SECTION-B11 is 6 marks)
• 12

  Question SECTION-B12 (6 marks)

  The Earth's early atmosphere was very different from the atmosphere today. (a) Name the gas thought to have been the main component of the early atmosphere, and state its likely source. (b) The amount of carbon dioxide in the atmosphere decreased over billions of years. Give TWO different processes that removed carbon dioxide from the atmosphere, and for each briefly explain how it lowered the carbon dioxide level. (c) State one human activity that is increasing the concentration of carbon dioxide in the atmosphere today.

  (Total for Question SECTION-B12 is 6 marks)

Section C

Extended response. Answer ALL questions in the spaces provided.

• 1

  Question SECTION-C1 (6 marks)

  Aluminium is extracted from its ore by electrolysis of molten aluminium oxide (Al2O3) mixed with cryolite. This produces aluminium at the cathode and oxygen at the anode. Explain the full process of the electrolysis of aluminium oxide. In your answer you should: identify what the mobile charge carriers are and why the oxide must be molten; write the half equation for the reaction at the cathode; write the half equation for the reaction at the anode; explain why cryolite is added; explain why the carbon (graphite) anodes must be replaced regularly.

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

  Question SECTION-C2 (7 marks)

  A student is given a colourless solution and told it contains a single soluble salt. Design and describe a full laboratory plan to identify both the metal (positive) ion and the negative ion present in the salt. In your answer include: a flame test procedure and two example flame colours with the metal ions they indicate; a test for sulfate ions and its positive result; a test for halide (chloride, bromide, iodide) ions and how the different halides are distinguished; a suitable safety precaution.

  (Total for Question SECTION-C2 is 7 marks)
• 3

  Question SECTION-C3 (6 marks)

  Hydrogen and ethanol are both being considered as fuels. Ethanol (C2H5OH) can be produced by fermentation of sugars, and hydrogen can be produced by the electrolysis of water. Compare hydrogen and ethanol as fuels for cars. In your answer you should discuss: the products formed when each is burned completely; one advantage and one disadvantage of using hydrogen as a car fuel; one advantage and one disadvantage of using ethanol as a car fuel; a comment on whether each can be described as carbon neutral. Write a balanced symbol equation for the complete combustion of ethanol.

  (Total for Question SECTION-C3 is 6 marks)
• 4

  Question SECTION-C4 (6 marks)

  This question is about the structure and properties of metals and alloys. Copper is a pure metal; brass is an alloy of copper and zinc. Explain, in terms of structure and bonding, the properties of metals and why alloys such as brass are often harder than the pure metals they are made from. In your answer you should: describe the structure and bonding in a pure metal; explain why metals conduct electricity; explain why pure metals can be bent and shaped (are malleable); explain why brass is harder than pure copper.

  (Total for Question SECTION-C4 is 6 marks)