Edexcel GCSE Chemistry Paper 1 Foundation June 2022 question paper 1CH0/1F

Figure 1 shows a bag of NPK fertiliser.

N, P and K are the symbols of three elements that are essential for plant growth.

N is the symbol for nitrogen.

Name the other two elements, P and K, that are essential for plant growth.

You may want to refer to the periodic table.

Many fertilisers are produced using ammonia.

Ammonia is produced on an industrial scale from the reaction of nitrogen with hydrogen.

The equation for the reaction is

nitrogen + hydrogen ammonia

State the name of this industrial process.

State the meaning of the symbol in the equation.

Figure 2 shows the electronic configurations for an atom of nitrogen and an atom of hydrogen.

Which dot and cross diagram for ammonia, NH₃, is correct?

Ammonia reacts with nitric acid to produce ammonium nitrate.

Write the word equation for this reaction.

Figure 3 shows a metal spoon and two test tubes being heated in a water bath.

One test tube contains a piece of chocolate, the other some liquid egg white.

After heating, the spoon, the chocolate and the egg white are allowed to cool to room temperature.

Figure 4 shows the state of the three different substances before heating, when hot and after cooling.

Describe the differences in the arrangement and movement of the particles in a solid and in a liquid.

difference in arrangement of particles

difference in movement of particles

Give a reason why the metal spoon has not changed state during the experiment.

Explain how we know the change to the egg white is a chemical change rather than a physical change.

Potable water is water that is suitable for drinking.

River water can be treated to make it potable. Chlorination, filtration and sedimentation are three of the processes involved in making the river water potable.

Which row of the table shows these three processes in the order in which they are carried out?

State the reason why chlorine is added during the water treatment.

Describe how sedimentation is carried out.

Figure 5 shows the results of an analysis of a sample of potable water.

Using this information, explain why this sample of potable water is not the same as pure water.

A student wanted to distil a sample of potable water. Figure 6 shows apparatus the student used.

Name the piece of equipment labelled X in Figure 6.

The student made an error when setting up the equipment in Figure 6. This error meant no water could be collected in the test tube.

Explain what the student needs to do so water can be collected.

A student wanted to find the volume of dilute hydrochloric acid that would react with 25.0 cm³ of lithium hydroxide solution.

They used the equipment in Figure 7 to carry out a rough titration and then a further two accurate titrations.

Suggest why the student carried out a rough titration before the two accurate titrations.

Figure 8 shows the results of the rough titration.

What was the volume of acid added in the rough titration?

Describe how the rough titration should be carried out once the dilute hydrochloric acid, lithium hydroxide solution and indicator are placed in the apparatus in Figure 7.

Which is the name of an indicator that is suitable to use in this titration?

During the titration the dilute hydrochloric acid, HC l, is reacting with the lithium hydroxide solution, LiOH.

Explain what type of reaction is taking place in the titration.

An atom of aluminium has an atomic mass of 27.

Aluminium has an atomic number of 13.

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

Aluminium reacts with bromine to form aluminium bromide. A sample of aluminium bromide contains 1.35 g of aluminium atoms and 12.00 g of bromine atoms.

Calculate the empirical formula of this sample of aluminium bromide.

(relative atomic masses: A l = 27.0, Br = 80.0)

Gallium is in the same group in the periodic table as aluminium and in the same period in the periodic table as bromine.

State in which group and period of the periodic table gallium can be found.

You may want to refer to the periodic table.

Gallium had not been discovered when Mendeleev created his first periodic table.

Figure 9 shows some properties of gallium that Mendeleev predicted and some of the actual properties of gallium.

Describe how Mendeleev predicted these properties of gallium.

3.14 g of solid copper sulfate was dissolved in water and made up to 250 cm³ of solution.

Calculate the concentration of this copper sulfate solution in g dm⁻³.

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

Sodium hydroxide solution was added to a solution of copper sulfate. A precipitate of copper hydroxide and a solution of sodium sulfate were formed.

State what would be seen in the reaction.

Complete the balanced equation for the reaction by adding a number in front of NaOH.

Describe how to obtain a pure, dry sample of the precipitate of copper hydroxide from the reaction mixture.

Figure 11 shows the ions in the sodium sulfate solution.

Draw a circle around each of the ions in Figure 11 that are attracted to the negative graphite electrode during the electrolysis.

State why it is important that the electrodes are inert.

Explain, in terms of its structure, how graphite conducts electricity.

When iron wool reacts with oxygen from the air, the iron corrodes and iron oxide is formed.

What happens to the iron in this reaction?

A piece of damp iron wool was placed in a measuring cylinder with 50 cm³ of air, as shown in Figure 12.

Figure 13 shows the apparatus one week later.

Complete the table of results.

Use these results to calculate the percentage decrease in the volume of gas in the measuring cylinder after one week.

Not all of the oxygen in the air in the measuring cylinder has reacted with the iron.

Give a reason why.

*(c) Pure metals can be made more useful by converting them into alloys or by electroplating them.

Explain what alloying and electroplating are and how they can make metals more useful.

Barium hydroxide reacts with dilute hydrochloric acid to form barium chloride and water.

The equation for the reaction is

Which row of the table shows the correct state of each of the substances in the equation for the reaction?

Name a piece of equipment which could be used to measure out 50.0 cm³ of dilute hydrochloric acid more accurately than the measuring cylinder.

Describe how the pH of the mixture is determined when a drop of it is placed on the universal indicator paper.

In the method, universal indicator paper is used to determine the pH.

Explain why litmus paper would not be a suitable indicator to use in this experiment.

Figure 14 shows the student’s results.

On the grid opposite:

• Add suitable scales to the vertical and horizontal axes.

• Plot a graph of the pH of the mixture against the mass of barium hydroxide.

Figure 15 shows a hazard symbol placed on a container of barium hydroxide.

What is the meaning of the hazard symbol in Figure 15?

Barium hydroxide is also corrosive.

Give one precaution that the student should take when using barium hydroxide.

Magnesium carbonate has the formula MgCO₃.

Magnesium carbonate contains Mg²⁺ and CO₃²⁻ ions.

The atomic number of magnesium is 12.

What is the electronic configuration of the Mg²⁺ ion?

Explain why solid magnesium carbonate cannot conduct electricity but solid magnesium can.

Calculate the percentage by mass of magnesium in magnesium carbonate, MgCO₃.

(relative atomic masses: C = 12.0, O = 16.0, Mg = 24.0)

*(c) A student has two separate test tubes containing sulfuric acid.

The student adds a spatula measure of magnesium carbonate, MgCO₃, to the first test tube and a piece of magnesium to the second test tube.

Explain what the student would see in each test tube and the tests that they should carry out to identify the gases produced.

Your answer should include word equations for the reactions that would take place.

Sucrose is a carbohydrate.

When a solution of sucrose is fermented using yeast, ethanol is formed.

sucrose + water ethanol + carbon dioxide

In one experiment, 100.00 g of sucrose was dissolved in water.

Yeast was added and the mixture allowed to ferment until no more bubbles of carbon dioxide were seen to be formed.

The ethanol was obtained from the mixture and its mass determined.

The results are shown in Figure 16.

The percentage yield is calculated using

State the meanings of the terms actual yield and theoretical yield.

actual yield

theoretical yield

State two reasons why the actual yield of a reaction is usually less than the theoretical yield.

The balanced equation for the fermentation of sucrose is

Calculate the atom economy of this reaction to produce ethanol.

Give your answer to two significant figures.

(relative formula masses: C₁₂H₂₂O₁₁ = 342, H₂O = 18, C₂H₅OH = 46, CO₂ = 44)

Explain the effect on the atom economy of this reaction if the carbon dioxide produced was used to make fizzy drinks.