AQA GCSE Trilogy Chemistry Paper 1 Higher June 2022 question paper 8464/C/1H

This question is about salts. Green copper carbonate and sulfuric acid can be used to produce blue copper sulfate crystals.

Excess copper carbonate is added to sulfuric acid. Give three observations you would make.

How can the excess copper carbonate be removed?

The pH of the solution changes during the reaction. What is the pH of the solution at the end of the reaction?

Copper carbonate and sulfuric acid react to produce copper sulfate. What type of reaction is this?

Ammonium nitrate is a salt. Figure 1 shows the maximum mass of ammonium nitrate that can dissolve in 100 cm³ of water at different temperatures.

A student adds ammonium nitrate to water at 80 °C until no more dissolves. The student cools 100 cm³ of this solution of ammonium nitrate from 80 °C to 20 °C to produce crystals of ammonium nitrate.

Determine the mass of ammonium nitrate that crystallises on cooling 100 cm³ of this solution from 80 °C to 20 °C

This question is about electrolysis. Figure 2 shows the apparatus used to investigate the electrolysis of potassium sulfate solution.

Potassium sulfate contains K⁺ and SO₄^2– ions. What is the formula of potassium sulfate? Tick (✓) one box.

What are the volumes of gases collected in the electrolysis experiment? Use Figure 2.

A student made the following hypothesis: ‘The volumes of gases collected in this electrolysis experiment are in the same ratio as hydrogen atoms to oxygen atoms in a water molecule.’ Explain how the volumes of gases collected in the experiment in Figure 2 support the student’s hypothesis. Use your answer to Question 02.2

The experiment is repeated 4 times. The volumes of oxygen collected in the 4 experiments are:

The mean volume of oxygen collected in the 4 experiments is 9 cm³ The measure of uncertainty is the range of a set of measurements about the mean.

What is the measure of uncertainty in the 4 experiments? Tick (✓) one box.

Calculate the mass of potassium sulfate needed to make 1.0 dm³ of solution.

Plan an investigation to find the order of reactivity of three metals. You should use the temperature change when each metal reacts with hydrochloric acid.

This question is about Group 7 elements.

What are the Group 7 elements known as?

Why do Group 7 elements react in similar ways?

Figure 3 shows the structure of a molecule of chlorine oxide.

What is the molecular formula of the chlorine oxide molecule in Figure 3 ?

Figure 4 shows the melting points of some Group 7 elements.

The melting point of fluorine is –220 °C Complete Figure 4. You should:

• complete the scale on the y-axis

• draw the bar for the melting point of fluorine.

Explain the trend in the melting points of the Group 7 elements. Use Figure 4.

What is the state symbol for bromine at –50 °C? Use Figure 4. Tick (✓) one box.

Evaporation and boiling occur at the surface of bromine at its boiling point. Name one more process that happens at the surface of bromine at its boiling point.

This question is about structure and bonding.

Figure 5 represents part of a carbon molecule.

Name the type of carbon molecule in Figure 5.

Suggest one property that makes the carbon molecule in Figure 5 useful in nanotechnology.

An alloy of aluminium contains small amounts of other metals. Explain why other metals are added to aluminium.

Figure 6 represents part of the structure of a polymer.

Compare the bonding within the chains with the forces between the chains in this polymer.

This question is about hydrogen chloride and hydrochloric acid.

Complete the dot and cross diagram to represent the bonding in hydrogen chloride on Figure 7. Use dots (o) and crosses (x) to represent electrons. You should show only the electrons in the outer shells.

Hydrogen chloride dissolves in water to produce hydrochloric acid. Hydrochloric acid is a strong acid. What is meant by the term strong acid?

Describe how magnesium can be used to distinguish between a strong acid and a weak acid of the same concentration.

The concentration of hydrochloric acid is increased by a factor of 100 What is the change in pH?

Ethene and hydrogen chloride react to produce chloroethane. The displayed formulae equation for the reaction is:

The reaction is exothermic. In the reaction the energy released forming new bonds is 56 kJ/mol greater than the energy needed to break existing bonds. Table 1 shows some bond energies.

Calculate the bond energy X.

This question is about elements and compounds.

Figure 8 shows a reactivity series.

Figure 8

Give the method and conditions used to extract metal Y from a compound of metal Y

Sodium reacts with titanium chloride (TiCl₄) to produce titanium.

Complete the equation. You should balance the equation.

The reaction between sodium and titanium chloride is a redox reaction. Write a half-equation to show that sodium is oxidised in this reaction.

108 g of aluminum reacts with 1.21 kg of copper chloride to produce copper. The equation for the reaction is:

Calculate the maximum mass of copper produced in grams (g). You should determine the limiting reactant. Relative atomic masses (A_r): Al = 27 Cu = 63.5 Relative formula masses (M_r): CuCl₂ = 134.5 AlCl₃ = 133.5

Limiting reactant is Mass of copper = g

Sodium metal and sodium chloride are both able to conduct electricity.

Describe how sodium metal conducts electricity.

Explain how sodium chloride can conduct electricity.