Edexcel GCSE Chemistry Paper 2 Foundation November 2021 question paper 1CH0/2F

Figure 1 shows a mug made of clay ceramic.

Which property of clay ceramic makes it suitable for use as a mug?

Figure 2 shows the properties of some materials.

Figure 3 shows an electrical cable. The electrical cable is made of metal wire coated with another material. The metal wire inside the electrical cable conducts electricity.

Name a material from Figure 2 that would be suitable for coating the metal wire.

Which type of particle moves through the metal wire to allow it to conduct electricity?

There are some concerns that nanoparticles may cause harm if they enter the human body.

Suggest one way that nanoparticles can enter the human body.

Suggest one possible risk if nanoparticles enter the human body.

The surface area of a nanoparticle of gold is 150 nm². The volume of a nanoparticle of gold is 125 nm³.

Calculate the surface area to volume ratio of this nanoparticle of gold.

surface area to volume ratio =_........

Magnesium reacts with dilute sulfuric acid to form magnesium sulfate and hydrogen gas.

A student wants to find out the effect of temperature on the rate of this reaction.

The student used the following method.

step 1pour 25 cm³ of dilute sulfuric acid into a conical flask step 2 warm the acid until its temperature is 30 °C step 3 add a piece of magnesium to the acid step 4 start a stopwatch step 5 wait until the reaction has finished step 6 stop the stopwatch step 7 repeat steps 1–6 but at 50 °C.

The student kept the volume of sulfuric acid the same when they repeated the method at 50 °C.

State two other variables that should be kept the same.

Which piece of equipment can be used to find the volume of 25 cm³ of sulfuric acid?

State how the student will know that the reaction has finished.

The reaction at 50 °C was faster than the reaction at 30 °C.

Give one reason, in terms of particles, why the reaction at 50 °C was faster than the reaction at 30C.

At 50 °C, 15.0 cm³ of gas was produced during the first 60 seconds of the reaction.

Calculate the average rate of reaction, in cm³ s^–1, for the first 60 seconds of the reaction.

average rate of reaction =_........ cm³

This question is about the noble gases.

State, in terms of outer shell electrons, why the noble gases are unreactive.

Figure 4 shows an airship, filled with helium, floating above the ground.

Helium, hydrogen and krypton are gases. Figure 5 shows the reactivity and density, at room temperature and pressure, of helium, hydrogen and krypton.

The density of air is 0.001225 gcm^–3.

Helium is used in airships.

Explain why hydrogen and why krypton are not used in airships.

Mendeleev produced one of the earliest periodic tables.

State why he could not include any of the noble gases in his periodic table.

Figure 6 shows the boiling points of some of the noble gases.

Complete the bar chart to show the boiling points of neon and argon.

Predict the boiling point of xenon.

boiling point of xenon =_........

A student carried out some tests on copper sulfate.

A flame test was carried out on some copper sulfate crystals.

The student used the following method.

step 1 dip a wire in hydrochloric acid, then hold the wire in a roaring Bunsen burner flame

step 2 dip the wire in hydrochloric acid again, then dip the wire in the copper sulfate crystals

step 3 hold the wire with the copper sulfate in the roaring Bunsen burner flame.

State why in step 1 the wire is dipped in hydrochloric acid and held in a roaring Bunsen burner flame.

State why in step 2 the wire is dipped in hydrochloric acid again before dipping it in the copper sulfate crystals.

What colour should be seen when the flame test is carried out on copper sulfate?

A solution of the copper sulfate was tested in a flame photometer.

Give an advantage of using a flame photometer, rather than a flame test, to test for copper ions.

Figure 7 shows some values obtained when producing a calibration graph for copper ions in a flame photometer.

Draw a line of best fit through the points.

A solution containing copper ions gave a display reading of 0.030.

Use the calibration graph in Figure 7 to find the concentration of copper ions in this solution.

concentration of copper ions =_........

The student tested an unknown solution for sulfate ions by

1. adding a few drops of dilute sulfuric acid to the unknown solution

2. then adding a few drops of barium chloride solution.

A white precipitate was formed.

The student cannot conclude from this result that the unknown solution contains sulfate ions.

Explain what the student should change to obtain a valid result.

Calculate the percentage by mass of copper in copper sulfate, CuSO₄.

(relative atomic masses: Cu = 63.5 relative formula mass of CuSO₄ = 159.5)

Give your answer to the nearest whole number.

percentage by mass of copper =_........

Fluorine, chlorine, bromine and iodine are elements in group 7 of the periodic table.

State the name given to the group 7 elements.

Name one other element that is in group 7. Use the periodic table on the back of this exam paper to help you.

Which element is liquid at room temperature and pressure?

Which element is dark-grey in colour at room temperature and pressure?

Tin reacts with chlorine to form tin chloride. A sample of tin chloride contains 1.19 g of tin and 1.42 g of chlorine.

Calculate the empirical formula of this tin chloride.

(relative atomic masses: C l = 35.5, Sn = 119.0)

You must show your working.

empirical formula of this tin chloride =_........

Tin also reacts with fluorine. The reaction between fluorine and tin is much more vigorous than the reaction between chlorine and tin.

Figure 8 shows the electronic configurations of fluorine and chlorine.

Explain, in terms of their electronic configurations, why fluorine reacts with tin more vigorously than chlorine reacts with tin.

Figure 9 shows a sample of hydrogen peroxide solution decomposing to form water and oxygen gas.

Write the word equation for hydrogen peroxide solution decomposing.

In this reaction hydrogen peroxide is a solution, water is a liquid and oxygen is a gas.

Draw one straight line from each substance to its correct state symbol.

Describe the test to show the gas produced is oxygen.

Figure 10 shows the electron arrangement for an atom of hydrogen and an atom of oxygen.

Complete the dot and cross diagram in Figure 11 for a molecule of water, H₂O.

Draw outer shell electrons only.

Liver contains the enzyme catalase.

A piece of liver was added to another sample of hydrogen peroxide solution.

Figure 12 shows the results.

Figure 13 shows a graph of the volume of oxygen produced from the hydrogen peroxide with and without liver.

Figure 13

Complete the missing label on the axis of the graph.

Describe what the graph shows about the difference in decomposition of hydrogen peroxide with and without liver.

Describe how the apparatus in Figure 12 could be modified to find the volume of gas produced when the liver is added to the hydrogen peroxide.

This question is about alcohols.

Figure 14 shows an incomplete diagram of the structure of a molecule of

Complete the structure of the molecule of propanol in Figure 14.

Figure 14

Propanol can be converted into propanoic acid.

What happens to propanol in this reaction?

A student used an alcohol burner to find the mass of different alcohols needed to raise the temperature of 100 cm³ of water by 20 °C.

Figure 15 shows their results.

Calculate the mass of butanol used.

mass of butanol =_........

*(ii) Figure 16 shows equipment that can be used to obtain the results shown in Figure 15.

Describe an experiment, using the equipment in Figure 16, that could be used to obtain results like those shown in Figure 15.

The results show that 0.36 g of pentanol was needed to raise the temperature of the water by 20 °C.

Calculate the mass of pentanol needed to raise the temperature of water by 1 °C.

Give your answer to 2 decimal places.

Show your working.

mass of pentanol =_........

The concentration of a solution can be calculated using the equation

A student dissolved 9.25 g of ammonium chloride in water and made up the

Use the equation to calculate the concentration of this solution in gdm⁻³.

concentration =_........ g dm

Dissolving ammonium chloride in water is an endothermic process. Figure 17 shows part of the reaction profile for this process.

Explain how Figure 17 shows that dissolving ammonium chloride in water is an endothermic process.

Complete the reaction profile in Figure 17 and label the activation energy.

A student used the equipment in Figure 18 to investigate whether electricity can pass through solid ammonium chloride and through ammonium chloride solution.

If an electrical current flows in the circuit, the lamp will light up.

Figure 19 shows the results of the investigation.

Explain the results of the investigation.

Ammonia gas is toxic.

Which symbol should be placed on a container of a toxic gas?

Give one safety precaution that should be taken when working with toxic gases in the laboratory.

Diesel oil is a mixture of hydrocarbons that can be obtained from crude oil.

State the name of the process used to separate diesel oil from crude oil.

Diesel oil contains alkanes. These alkanes are part of an homologous series.

Which statement about compounds in this homologous series is true?

When fuels such as diesel oil are burned, the high temperatures produced can cause nitrogen and oxygen in the air to form the pollutant nitrogen dioxide.

Complete the balanced equation for the reaction.

Explain how the greenhouse effect is caused by the gases produced by the complete combustion of diesel oil.

*(e) Diesel oil can contain impurities of sulfur. Burning diesel oil containing impurities of sulfur can result in acid rain. Acid rain is harmful to the environment.

Explain how acid rain is formed and the harm it can do.

This question is about polymers.

State a problem with recycling polymers.

Describe a problem associated with the disposal of polymers.

Poly(chloroethene) is a polymer made from chloroethene. A molecule of chloroethene is shown in Figure 20.

On Figure 20, draw a circle around the functional group in this molecule.

Draw a section of a poly(chloroethene) molecule containing three repeating units, showing all bonds.

What type of polymer is poly(chloroethene)?

Calculate the relative formula mass of a poly(chloroethene) molecule made from 2850 chloroethene molecules, C₂H₃Cl.

(relative atomic masses: H = 1.00, C = 12.0, C l = 35.5)

Give your answer to three significant figures.

Show your working.

relative formula mass =_........