Edexcel GCSE Chemistry Paper 1 Higher June 2022 question paper 1CH0/1H

Chemical cells produce a voltage.

A chemical cell can be made by placing the metals copper and zinc in a beaker of sodium chloride solution.

Figure 1 shows a diagram of this chemical cell.

Describe what will happen to the brightness of the light bulb over a long period of time.

Copper is a transition metal.

Which of the following is most likely to be a property of copper?

A copper atom has a diameter of 0.256 nm.

What is the size of this copper atom in metres?

Brass is an alloy of copper and zinc. One type of brass contains 70% copper.

Zinc atoms are slightly larger than copper atoms.

Draw a labelled diagram in the box to show the arrangement of copper and zinc atoms in this alloy.

Use the circle in the box as a guide to the size of a copper atom.

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?

A student wanted to investigate how the pH of the mixture changes as barium hydroxide is added to dilute hydrochloric acid.

They followed this method.

step 1 measure out 50.0 cm3³ of dilute hydrochloric acid into a beaker using a measuring cylinder step 2 use a glass rod to place a drop of the acid onto a piece of universal indicator paper and record the pH step 3 add 0.2 g of barium hydroxide to the acid in the beaker and stir step 4 use the glass rod to place a drop of the mixture onto a new piece of universal indicator paper and record the pH again step 5 repeat steps 3–4 until there is no further change in the pH.

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 2 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.

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)

percentage by mass of magnesium =_........

Magnesium carbonate reacts with dilute hydrochloric acid. Water and carbon dioxide are two of the products of the reaction.

Complete the balanced equation for this reaction.

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 3.

The percentage yield is calculated using

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

actual yield

theoretical yield

Use the information in Figure 3 to calculate the percentage yield of ethanol in this experiment.

percentage 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)

atom economy =_........

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

When copper sulfate solution is electrolysed using copper electrodes, the mass of each electrode changes.

Draw a labelled diagram to show the apparatus that can be used to electrolyse copper sulfate solution using copper electrodes.

Before the electrolysis is carried out, the mass of each electrode is determined.

Explain what should be done to the copper electrodes before their masses are determined.

Figure 4 shows the results obtained from an electrolysis experiment when copper sulfate solution was electrolysed for 10 minutes.

Explain, in terms of ions, the changes in mass of the two electrodes shown in the results in Figure 4.

The electrolysis was repeated using another pair of copper electrodes of the same masses.

Explain a change that could be made to the electrolysis experiment to cause the mass of the cathode to increase by 2.34 g in 10 minutes.

The method used to extract a metal from its ore depends on the position of the metal in the reactivity series.

Aluminium is extracted from its ore by electrolysis.

Explain why this method is used to extract aluminium from its ore.

One step in the extraction of titanium metal involves the displacement reaction between titanium chloride, TiCl₄, and magnesium.

This equation can be simplified as

Explain why this displacement reaction can be described as a redox reaction.

The formula of the sulfate ion is SO²⁻₄.

Which of the following is the formula of titanium sulfate containing the Ti⁴⁺ ion?

Phytoextraction is an alternative biological method that can be used to extract metals from very low-grade ores.

Give one disadvantage of phytoextraction as a method of extraction of metals.

Copper is low down in the reactivity series and can be obtained from copper oxide.

Devise a simple method to obtain a sample of copper from copper oxide in the laboratory.

The volume of dilute sulfuric acid required to neutralise 25.0 cm³ of ammonia solution can be found by titration.

In the titration, a few drops of methyl orange indicator were added to the ammonia solution in a conical flask before adding the dilute sulfuric acid.

State the change in colour of the methyl orange at the end point when the ammonia solution has just been neutralised.

When the ammonia solution was neutralised by the dilute sulfuric acid, a solution of ammonium sulfate was formed.

Complete the balanced equation for the reaction between ammonia solution and sulfuric acid.

The titration was repeated to obtain a mean volume of dilute sulfuric acid required to neutralise the 25.0 cm³ of ammonia solution. The volumes of the two solutions were measured accurately.

Explain two other practical steps that should be used in the titration to ensure that an accurate titre volume is obtained.

The mean volume of dilute sulfuric acid required to neutralise the ammonia solution was determined from the results of the titration.

This volume of dilute sulfuric acid was added to 25.0 cm³ of ammonia solution in a conical flask.

Devise a plan to produce a sample of dry ammonium sulfate from the contents of the conical flask.

Bromine is a liquid at room temperature and vaporises readily. Bromine has a simple molecular structure.

Which row of the table shows the most likely melting and boiling points of bromine?

Part of the structure of graphene is shown in Figure 5.

Explain why graphene will be a good conductor of an electric current.

Part of the structure of potassium chloride is shown in Figure 6.

Potassium chloride has a melting point of 770 °C.

Explain why potassium chloride has a high melting point.

*(d) A molecule of methane can be represented in several different ways as shown in Figure 7. These representations have been labelled A – E to assist you in your answer.

Describe what information can be obtained from each representation including the limitations of these representations of methane.

A student carried out an investigation to determine the order of reactivity of four metals, W, X, Y and Z. A piece of metal W was added to a test tube containing excess dilute hydrochloric acid. This was repeated with the other three metals, X, Y and Z. In each case, the size of each piece of metal was the same. The student recorded observations on each reaction for three minutes.

The observations obtained are shown in Figure 8.

Use the information in Figure 8 to place the metals in order of reactivity from the least reactive to the most reactive.

The experiment was repeated using an excess of dilute sulfuric acid in place of the dilute hydrochloric acid.

metal + sulfuric acid metal sulfate + hydrogen

When metal Y reacts with dilute sulfuric acid, bubbles form quickly at first and then the reaction stops. Most of the solid metal remains.

Explain why the reaction between metal Y and excess dilute sulfuric acid stopped even though there was solid metal Y left.

The reactions between metals and dilute ethanoic acid are slower than reactions between metals and dilute hydrochloric acid. This is because ethanoic acid is a weak acid.

Explain the meaning of the term weak acid.

The formula of aluminium sulfate is Al₂(SO₄)₃.

Calculate the total number of atoms that combine to form 5.13 g of aluminium sulfate.

(relative atomic masses: O = 16.0, A l = 27.0, S = 32.0 Avogadro number = 6.0210²³)

number of atoms =_........

Iron is more reactive than lead. Iron reacts with lead nitrate solution to form solid lead. Two possible balanced equations for the reaction are

Equation 1 Fe + Pb(NO₃)₂ Fe(NO₃)₂ + Pb

Equation 2 2Fe + 3Pb(NO₃)₂ 2Fe(NO₃)₃ + 3Pb

In one experiment, it was found that 4.48 g of iron reacted with excess lead nitrate solution to form 24.84 g of lead.

Carry out a calculation, using the information above, to show which equation represents the reaction taking place.

(relative atomic masses: Fe = 56.0, Pb = 207)

When hydrogen is removed from an alkane, an alkene is formed.

This is an example of a dehydrogenation reaction.

Under certain conditions the dehydrogenation of propane forms propene and a dynamic equilibrium is reached.

State what is meant by dynamic in this context.

*(ii) The equation for this equilibrium reaction is

propane propene

The forward reaction takes in heat energy and is endothermic. A manufacturer produces large quantities of propene using this equilibrium reaction.

Suggest, with explanations, suitable conditions that the manufacturer could use to maximise the yield and rate of production of propene from propane.

C₃H₈(g) C₃H₆(g) + H₂(g) propane propene

State the maximum volume of propene, in dm³, formed by the dehydrogenation of 300 dm³ of propane.

(assume all volumes of gases are measured under the same conditions of temperature and pressure)

maximum volume of propene =_........

900 dm³ of propane, measured at room temperature and pressure, were dehydrogenated to form propene.

propane propene

Calculate the maximum mass, in kg, of hydrogen formed in this reaction.

(relative atomic mass: H = 1.0; 1 mol of any gas at room temperature and pressure occupies 24 dm³)

mass of hydrogen =_........