AQA GCSE Chemistry Paper 1 Foundation June 2018 question paper 8462/1F

This question is about mixtures.

Substances are separated from a mixture using different methods.

Draw one line from each substance and mixture to the best method of separation.

Substance and mixture
Method of separation

A student filters a mixture.

Figure 1 shows the apparatus.

Suggest one improvement to the apparatus.

Complete the sentences.

Choose answers from the box.

Figure 2 shows the arrangement of atoms in a pure metal and in a mixture of metals.

Calculate the percentage of metal B atoms in the mixture of metals shown in Figure 2.

What is a mixture of metals called?

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Why is the mixture of metals in Figure 2 harder than the pure metal?

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A nanoparticle of pure metal A is a cube.

Each side of the cube has a length of 20 nm.

Figure 3 shows the cube.

What is the volume of the nanoparticle?

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The halogens are elements in Group 7.

Bromine is in Group 7.

Give the number of electrons in the outer shell of a bromine atom.

Bromine reacts with hydrogen. The gas hydrogen bromide is produced.

What is the structure of hydrogen bromide?

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What is the formula for fluorine gas?

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A student mixes solutions of halogens with solutions of their salts.

Table 1 shows the student’s observations.

Explain how the reactivity of the halogens changes going down Group 7.

Use the results in Table 1.

A company uses chlorine to produce titanium chloride from titanium dioxide.

What is the relative formula mass (M_r) of titanium dioxide, TiO₂ ?

Relative atomic masses (A_r): O = 16 Ti = 48

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The company calculates that 500 g of titanium dioxide should produce 1.2 kg of titanium chloride.

However, the company finds that 500 g of titanium dioxide only produces 900 g of titanium chloride.

Calculate the percentage yield.

This question is about the structure of the atom.

Complete the sentences.

Choose answers from the box.

Each word may be used once, more than once, or not at all.

The two types of particle in the centre of the atom are the proton

Niels Bohr suggested particles orbit the centre of the atom. This type of particle

The two types of particle with the same mass are the neutron

Suggest the identity of element X.

Use the periodic table.

The radius of an atom of element X is 1.2 10^-10 m

The radius of the centre of the atom is the radius of the atom.

Calculate the radius of the centre of an atom of element X.

Give your answer in standard form.

A student investigated the electrolysis of sodium chloride solution.

Figure 4 shows the apparatus.

The student measured the volume of gas collected in each measuring cylinder every minute for 20 minutes.

Figure 5 shows the volume of hydrogen gas collected in the measuring cylinder after 8 minutes.

What is the volume of hydrogen gas collected?

Figure 6 shows the results of the investigation.

Which of the lines on Figure 6 show that the volume of gas collected is directly proportional to the time?

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Which of the lines on Figure 6 show a positive correlation between the volume of gas collected and time?

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A teacher demonstrates the electrolysis of different substances using graphite electrodes.

Figure 7 shows the apparatus used.

Figure 7

Why can graphite conduct electricity?

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The teacher demonstrates the electrolysis of:

molten zinc chloride

potassium bromide solution.

Complete Table 3 to predict the products.

Choose answers from the box.

A student investigated the mass of copper oxide produced by heating copper carbonate.

This is the method used.

1. Weigh an empty test tube.

2. Weigh 2.00 g of copper carbonate into the test tube.

3. Heat the copper carbonate until there appears to be no further change.

4. Re-weigh the test tube and copper oxide produced.

5. Subtract the mass of the empty tube to find the mass of copper oxide.

6. Repeat steps 1–5 twice.

7. Repeat steps 1–6 with different masses of copper carbonate.

Table 4 shows the student’s results.

The equation for the reaction is:

Complete the sentence.

Why do the contents of the test tube lose mass in the investigation?

Calculate the mean mass X in Table 4.

One of the results in Table 4 is anomalous.

Which result is anomalous?

Determine the mass of magnesium oxide produced by 8.4 g of magnesium carbonate.

Use Figure 8.

Calculate the mass of magnesium oxide produced when 168 g of magnesium carbonate is heated.

Use your answer to Question 05.7

A student investigated the temperature change in displacement reactions between metals and copper sulfate solution.

This is the method used.

1. Measure 50 cm³ of the copper sulfate solution into a polystyrene cup.

2. Record the starting temperature of the copper sulfate solution.

3. Add the metal and stir the solution.

4. Record the highest temperature the mixture reaches.

5. Calculate the temperature increase for the reaction.

6. Repeat steps 1-5 with different metals.

Draw one line from each type of variable to the name of the variable in the investigation.

The student used a polystyrene cup and not a glass beaker.

Why did this make the investigation more accurate?

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Table 5 shows the student’s results.

Complete Figure 9.

Use data from Table 5.

The student concluded that the reactions between the metals and copper sulfate solution are endothermic.

Give one reason why this conclusion is not correct.

The temperature increase depends on the reactivity of the metal.

Write the metals magnesium, nickel and zinc in order of reactivity.

Use Table 5.

Y is an unknown metal.

Describe a method to find the position of Y in the reactivity series in Question 06.5

Figure 10 shows the reaction profile for the reaction between zinc and copper sulfate solution.

Which letter represents the products of the reaction?

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Which letter represents the activation energy?

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This question is about elements in Group 1.

A teacher burns sodium in oxygen.

What is the name of this type of reaction?

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The teacher dissolves the product of the reaction in water and adds universal indicator.

The universal indicator turns purple.

What is the pH value of the solution?

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The solution contains a substance with the formula NaOH

Give the name of the substance.

All alkalis contain the same ion.

What is the formula of this ion?

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A solution of NaOH had a concentration of 40 g/dm³

What mass of NaOH would there be in 250 cm³ of the solution?

The melting points of the elements in Group 1 show a trend.

Table 6 shows the atomic numbers and melting points of the Group 1 elements.

Plot the data from Table 6 on Figure 11.

Predict the melting point, X, of rubidium, atomic number 37

Use Figure 11.

Soluble salts are formed by reacting metal oxides with acids.

Give one other type of substance that can react with an acid to form a soluble salt.

Calcium nitrate contains the ions Ca²⁺ and NO₃^–

Give the formula of calcium nitrate.

Describe a method to make pure, dry crystals of magnesium sulfate from a metal oxide and a dilute acid.

This question is about metals and metal compounds.

Iron pyrites is an ionic compound.

Figure 12 shows a structure for iron pyrites.

Determine the formula of iron pyrites.

Use Figure 12.

An atom of iron is represented as⁵⁶₂₆Fe

Give the number of protons, neutrons and electrons in this atom of iron.

Iron is a transition metal.

Sodium is a Group 1 metal.

Give two differences between the properties of iron and sodium.

Nickel is extracted from nickel oxide by reduction with carbon.

Explain why carbon can be used to extract nickel from nickel oxide.

Chemical reactions can produce electricity.

Figure 13 shows a simple cell.

Which of these combinations would not give a zero reading on the voltmeter in Figure 13 ?

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Electrode A
Electrode B
Electrolyte

Alkaline batteries are non-rechargeable.

Why do alkaline batteries eventually stop working?

Why can alkaline batteries not be recharged?

Hydrogen fuel cells and rechargeable lithium-ion batteries can be used to power electric cars.

Complete the balanced equation for the overall reaction in a hydrogen fuel cell.

Table 7 shows data about different ways to power electric cars.

Evaluate the use of hydrogen fuel cells compared with rechargeable lithium-ion batteries to power electric cars.

Use Table 7 and your own knowledge.