AQA GCSE Chemistry Paper 1 Higher June 2024 question paper 8462/1H

A student produced a salt by reacting copper carbonate with sulfuric acid.

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.

Complete the word equation for the reaction.

copper + sulfuric → + + carbon

Give one observation the student could make during Step 4 which shows that the copper carbonate is in excess.

Give one reason for filtering the mixture in Step 5.

Name the equipment that can be used to warm the filtrate gently in Step 6.

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:

Some salts can be produced by reacting sulfuric acid with a metal.

Neither copper nor sodium is used to produce a salt with sulfuric acid.

Give one reason why each metal is not used.

This question is about the periodic table.

Sodium and potassium are in Group 1 of the periodic table.

Give one similarity and one difference between the electronic structures of sodium and potassium.

Group 1 elements react with water.

Give two observations made when potassium reacts with water.

Potassium hydroxide solution is produced when potassium reacts with water.

What is the colour of universal indicator when added to potassium hydroxide solution?

Give one reason for your answer.

Colour of universal indicator

Table 1 shows the densities of some of the elements in Group 0 of the periodic table.

Plot the data from Table 1 on Figure 1.

Estimate the density (X) of krypton.

Use Figure 1 and Table 1.

The elements in Group 7 are called the halogens.

A more reactive halogen can displace a less reactive halogen from a solution of its salt.

Which combination of solutions will produce a reaction when mixed?

Tick () one box.

Which of the following describes the trends going down Group 7?

Tick () one box.

This question is about models of the atom.

Figure 2 shows two early models of the atom.

Name the models of the atom shown in Figure 2.

Compare model A with the model of the atom used today.

Use Figure 2.

Chadwick’s experiments showed the existence of neutrons in an atom.

This led to an understanding of isotopes.

Define the term ‘isotopes’.

Refer to subatomic particles in your answer.

A student investigated the energy change of the reaction between zinc and copper sulfate solution.

This is the method used.

1. Measure 25 cm³ of copper sulfate solution into a polystyrene cup.

2. Measure the temperature of the copper sulfate solution.

3. Add 0.20 g of zinc powder to the copper sulfate solution.

4. Stir the reaction mixture.

5. Record the highest temperature reached.

6. Repeat steps 1 to 5 with different masses of zinc powder.

Figure 3 shows the results.

Draw two lines of best fit on Figure 3.

The lines should cross.

Explain the results shown in Figure 3.

Do not refer to anomalous points.

Use data from Figure 3.

Explain why using a polystyrene cup gives more accurate results than using a glass beaker.

Complete the ionic equation for the reaction between zinc and copper sulfate solution.

Include state symbols.

A different student repeated steps 1 to 5 of the method four times using 0.50 g of zinc powder.

Table 2 shows the results.

Calculate the mean highest temperature reached.

Include the uncertainty in your answer.

The results show random errors.

The student did not make any measuring errors.

Suggest one reason for the random errors in this experiment.

This question is about ionic compounds and electrolysis.

Calcium chloride is an ionic compound.

Calcium and chlorine react to produce calcium chloride.

Describe what happens to calcium atoms and chlorine atoms when the ionic compound calcium chloride is formed.

Solid calcium chloride cannot be electrolysed.

Give one reason why.

Name the product formed at the negative electrode when aqueous calcium chloride solution is electrolysed.

What is the half equation for the reaction at the positive electrode when aqueous calcium chloride solution is electrolysed?

Tick () one box.

A student investigated the electrolysis of green copper chromate solution.

Figure 4 shows the apparatus.

Figure 5 shows the results.

Copper chromate solution contains the ions Cu²⁺ and CrO₄^2–

Explain the results shown in Figure 5.

A student investigated the voltage produced by different pairs of metal electrodes in a chemical cell.

Figure 6 shows the apparatus.

This is the method used.

1. Place a nickel electrode and an electrode made from a different metal (electrode A in 1.0 mol/dm³ sodium chloride solution.

2. Measure the voltage produced.

3. Repeat using different metals for electrode A.

Table 3 shows the results.

Write the symbols of the five metals in Table 3 in order of reactivity.

Justify your answer.

Most reactive Least reactive

The voltage produced by a chemical cell depends on the concentration of the electrolyte solution.

Plan an experiment to investigate how the voltage produced by a chemical cell varies with the concentration of the electrolyte solution.

The following substances are available:

• the metal electrodes in Table 3

• 1.0 mol/dm³ sodium chloride solution

• pure water.

Describe how a hydrogen fuel cell produces a potential difference.

This question is about iron.

Iron is a metal.

Describe how iron conducts thermal energy.

Pure iron is too soft for many uses.

Explain why mixing iron with other metals makes alloys which are harder than pure iron.

When iron reacts with chlorine, 0.12 mol of iron reacts with 0.18 mol of chlorine (Cl₂).

Which is the correct equation for the reaction?

Tick () one box.

The most common oxides of iron are Fe₂O₃ and Fe₃O₄

What is the ratio of the numbers of ions in Fe₃O₄?

Tick () one box.

Calculate the percentage (%) by mass of iron in Fe₃O₄

Relative atomic masses (A_r): O = 16 Fe = 56

Fe₂O₃ reacts with carbon to produce carbon dioxide.

The equation for the reaction is:

Calculate the volume of carbon dioxide gas at room temperature and pressure that is produced from 40.0 kg of Fe₂O₃ using excess carbon.

Relative formula mass (M_r): Fe₂O₃ = 160

The volume of 1 mole of any gas at room temperature and pressure is 24 dm³.

This question is about propane (C₃H₈).

Figure 7 shows the displayed structural formula of propane.

Explain why propane has a low boiling point.

Propane reacts with oxygen to produce carbon dioxide and water.

The reaction is exothermic.

Figure 8 shows four reaction profiles.

Which is the correct reaction profile and labels for the reaction between propane and oxygen?

Tick () one box.

Figure 9 shows the displayed formula equation for the reaction between propane and oxygen.

The overall energy change of this exothermic reaction is 2219 kJ/mol.

Table 4 shows the bond energies of the bonds in the reaction.

Calculate the bond energy of the C — H bond (X).

This question is about acids and their reactions.

Acids can be either weak or strong.

What is meant by ‘a weak acid’?

Explain what happens to the pH of an acid as the acid is diluted with water.

A student does a titration to find the volume of acid needed to neutralise an alkali.

The student fills a burette with the acid.

Give three more steps the student must do before adding the acid to the alkali from the burette.

You should name any equipment used.

The student titrated a solution containing 0.0045 moles of sodium hydroxide with 0.15 mol/dm³ hydrochloric acid.

The equation for the reaction is:

Calculate the volume of hydrochloric acid in cm³ needed in the titration.

A calcium atom is larger than a magnesium atom.

Explain why calcium reacts more vigorously than magnesium with hydrochloric acid of the same concentration.