AQA GCSE Trilogy Chemistry Paper 2 Higher June 2019 question paper 8464/C/2H

Water that is safe to drink contains dissolved substances.

What do we call water that is safe to drink? Tick (✓) one box.

Describe a test for pure water. Give the result of the test if the water is pure.

Describe a method to determine the mass of dissolved solids in a 100 cm³ sample of river water.

A sample of river water contains 125 mg per dm³ of dissolved solids. Calculate the mass of dissolved solids in grams in 250 cm³ of this sample of river water. Give your answer to 2 significant figures.

A water company allows a maximum of 500 mg per dm³ of sulfate ions in drinking water. A sample of drinking water contains 44 mg per dm³ of sulfate ions. Calculate the percentage (%) of the maximum allowed mass of sulfate ions in the sample of drinking water.

This question is about atmospheric pollutants from fuels.

Fuel burns in a car engine. Describe how oxides of nitrogen are produced in a car engine.

Table 1 shows the carbon footprint during the manufacture and use of three cars.

Evaluate the carbon footprint of the cars. Use information from Table 1.

This question is about chromatography of food colouring.

Food colouring is a formulation. What is a formulation?

Explain how paper chromatography separates the dyes in a food colouring. Do not give details of how to do the experiment.

Explain how the student could tell from the chromatogram that the food colouring contained more than one dye.

Explain how the student could use chromatography to identify unknown dyes in the food colouring.

This question is about copper and fuels.

Copper is extracted from low-grade ores by phytomining. Describe how copper metal is produced by phytomining.

Another method of extracting copper from low-grade ores is bioleaching. A solution of copper sulfate (CuSO₄) produced by bioleaching has a

Relative atomic masses (A_r): Cu = 63.5 O = 16 S = 32 Calculate the number of moles of copper that can be produced from 1 dm³ of this solution.

Copper is used as a catalyst. Figure 1 shows reaction profiles for a reaction with and without a catalyst.

How do the reaction profiles show that using a catalyst does not affect the overall energy change for the reaction?

Tick (✓) one box.

Copper is a catalyst in a reaction to produce ethanol from carbon dioxide. Ethanol (C₂H₅OH) is used as a fuel. Suggest why producing ethanol from carbon dioxide is sustainable.

Chemistry plays an important role in sustainable development. What is sustainable development?

This question is about magnesium. A student investigated the rate of the reaction between magnesium and hydrochloric acid. Figure 2 shows the apparatus.

Which is the correct ionic equation for the reaction? Tick (✓) one box.

What happens in the reaction between magnesium and hydrochloric acid? Tick (✓) one box.

Table 2 shows the student’s results.

Plot the data from Table 2 on Figure 3. Draw a line of best fit.

Describe the changes in the rate of this reaction.

Explain why the rate of this reaction changes. Give your answer in terms of collision theory.

This question is about oxygen (O₂) and sulfur dioxide (SO₂).

Give the test and result for oxygen gas.

The reaction between oxygen and sulfur dioxide is at equilibrium.

Some of the sulfur trioxide (SO₃) is removed. Explain what happens to the position of the equilibrium.

Sulfur dioxide is an atmospheric pollutant. Sulfur dioxide pollution is reduced by reacting calcium oxide with sulfur dioxide to produce calcium sulfite.

7.00 g of calcium oxide reacts with an excess of sulfur dioxide. Relative atomic masses (A_r): O = 16 S = 32 Ca = 40 Calculate the mass of calcium sulfite produced.

This question is about hydrocarbons and crude oil.

Hydrocarbon fuels are produced from crude oil. Describe how crude oil is separated into fractions.

Butane is a hydrocarbon.

Two equations for the combustion of butane are:

Why are different products formed?

One other product of the combustion of butane is carbon monoxide. Balance the equation.

Carbon dioxide is a greenhouse gas. Describe the greenhouse effect in terms of the interaction of short and long wavelength radiation with matter.