Electrolysis (Cambridge (CIE) IGCSE Chemistry)

Aluminium is obtained from purified alumina, Al₂O₃, by electrolysis.

Alumina is obtained from the main ore of aluminium.

State the name of this ore.

Separate: Chemistry and Extended Only

Describe the extraction of aluminium from alumina. Include the electrolyte, the electrodes and the reactions at the electrodes.

Extended Only

Aluminium is resistant to corrosion. It is protected by an oxide layer on its surface. The thickness of this oxide layer can be increased by anodising.

i) State a use of aluminium due to its resistance to corrosion.

[1]

ii) Anodising is an electrolytic process. Dilute sulfuric acid is electrolysed with an aluminium object as the anode. The thickness of the oxide layer is increased.

Complete the equations for the reactions at the aluminium anode.

.......OH^– → O₂ + 2H₂O + ......e^–

....Al + ......... → ......... Al₂O₃

[4]

Extended Only

During electrolysis, ions move in the electrolyte and electrons move in the external circuit. Reactions occur at the electrodes.

The diagram shows the electrolysis of molten lithium iodide.

 i) Draw an arrow on the diagram to show the direction of the electron flow in the external circuit.

[1]

 ii) Electrons are supplied to the external circuit. How and where is this done?

[2]

iii) Explain why solid lithium iodide does not conduct electricity but when molten it is a good conductor.

[1]

Extended Only

The results of experiments on electrolysis are shown in the following table.

Complete the table. The first line has been done as an example.

[4]

The diagram below shows the electrolysis of dilute sulfuric acid. Hydrogen is formed at the negative electrode (cathode) and oxygen at the positive electrode (anode) and the concentration of sulfuric acid increases.

The ions present in the dilute acid are H⁺ (aq), OH^– (aq) and SO₄^2– (aq).  

i) Write an equation for the reaction at the negative electrode (cathode).

[2]

ii) Complete the equation for the reaction at the positive electrode (anode).

4OH^– (aq) → O₂ (g) + .....H₂O (l) + ....... 

[1]

iii) Suggest an explanation of why the concentration of the sulfuric acid increases.

[1]

The electrolysis of concentrated aqueous sodium chloride, between inert electrodes, is used to make four important chemicals.

hydrogen chlorine sodium hydroxide sodium chlorate(I)

The ions present in the electrolyte are Na⁺, H^+, Cl^– and OH^–

i) Hydrogen ions are discharged at the negative electrode (cathode). Write an equation for this reaction.

[2]

ii) The hydrogen ions are from the water.

H₂O     H⁺ + OH^–

Suggest an explanation why the concentration of hydroxide ions increases.

[2]

iii) When a dilute solution of sodium chloride is used, chlorine is not formed at the positive electrode (anode), a different gas is produced. Name this gas.

[1]

iv) State an example of an inert electrode.

[1]

i) State a use of hydrogen. 

[1]

ii) Why is chlorine used to treat the water supply?

[1]

Extended Only

The results of experiments on electrolysis using inert electrodes are given in the table.

Complete the table; the first line has been completed as an example.

[8]

Copper has the structure of a typical metal. It has a lattice of positive ions and a “sea” of mobile electrons. The lattice can accommodate ions of a different metal.

Give a different use of copper that depends on each of the following.

i) The ability of the ions in the lattice to move past each other

[1]

ii) The presence of mobile electrons

[1]

 iii) The ability to accommodate ions of a different metal in the lattice

[1]

Aqueous copper(II) sulphate solution can be electrolysed using carbon electrodes. The ions present in the solution are as follows.

Cu²⁺      SO₄^2–      H⁺     OH^–

i) Write an ionic equation for the reaction at the negative electrode (cathode).

[1]

ii) A colourless gas was given off at the positive electrode (anode) and the solution changes from blue to colourless. Explain these observations.

[2]

Aqueous copper(II) sulphate can be electrolysed using copper electrodes. The reaction at the negative electrode is the same but the positive electrode becomes smaller and the solution remains blue.

i) Write a word equation for the reaction at the positive electrode.

[1]

ii) Explain why the colour of the solution does not change.

[1]

iii) What is the large scale use of this electrolysis?

[1]

Separate: Chemistry and Extended Only

Zinc is extracted from zinc blende, ZnS.

Zinc blende is heated in air to give zinc oxide and sulfur dioxide. Most of the sulfur dioxide is used to make sulfur trioxide. This is used to manufacture sulfuric acid. Some of the acid is used in the plant, but most of it is used to make fertilisers.

i) Describe how sulfur dioxide is converted into sulfur trioxide.

[3]

ii) Name a fertiliser made from sulphuric acid.

[1]

Extended Only

The remaining zinc oxide reacts with sulfuric acid to give aqueous zinc sulfate. This is electrolysed with inert electrodes (the electrolysis is the same as that of copper(II) sulfate with inert electrodes). Ions present: Zn²⁺ (aq)    SO₄^2- (aq)     H⁺ (aq)     OH^- (aq)

i) Zinc forms at the negative electrode (cathode). Write the equation for this reaction.

[1]

ii) Write the equation for the reaction at the positive electrode (anode).

[2]

iii) The electrolyte changes from aqueous zinc sulfate to .............................. . 

[1]

Extended Only

Give two uses of zinc.

Molten potassium bromide can be electrolysed. Predict the products of this electrolysis at:

the anode the cathode

Electrolysis of concentrated aqueous sodium chloride using inert electrodes forms chlorine, hydrogen and sodium hydroxide.

What is meant by the term electrolysis?

Name a substance that can be used as the inert electrodes.

Extended Only

Write an ionic half-equation for the formation of hydrogen during this electrolysis.

Extended Only

Give the formulae of the four ions present in concentrated aqueous sodium chloride.

Extended Only

Explain how sodium hydroxide is formed during this electrolysis.

When concentrated hydrochloric acid is electrolysed, gases are produced at the electrodes. The incomplete apparatus is shown.

Complete the diagram by:

• labelling the anode and cathode

• showing how the gases are collected.

Extended Only

When concentrated hydrochloric acid is electrolysed, gases are produced at the electrodes. The incomplete apparatus is shown.

Predict the products of this electrolysis at the:

positive electrode:

negative electrode:

When concentrated hydrochloric acid is electrolysed, gases are produced at the electrodes. The incomplete apparatus is shown.

Graphite (carbon) electrodes are used in this electrolysis. Suggest one other element that can be used as an electrode and give a reason, other than that it can conduct electricity.

element:

reason:

Extended Only

When concentrated hydrochloric acid is electrolysed, gases are produced at the electrodes. The incomplete apparatus is shown.

Hydrogen chloride is produced when chlorine reacts with hydrogen. Complete the chemical equation for this reaction.

Cl₂ + .......... → .....HCl

Predict the products of the electrolysis of molten aluminium oxide at:

the positive electrode ........................................

the negative electrode.......................................

Extended Only

The diagram shows a simple cell.

Write an equation for the overall reaction occurring in the cell.

Extended Only

Explain why all cell reactions are exothermic and redox.

Extended Only

Which electrode, zinc or iron, is the negative electrode? Give a reason for your choice.

Extended Only

Zinc alloys have been used for over 2500 years.

i) Explain the phrase zinc alloy.

[1]

ii) Describe the bonding in a typical metal, such as zinc, and then explain why it is malleable. You may use a diagram to illustrate your answer.

[3]

iii) Suggest why the introduction of a different atom into the structure makes the alloy less malleable than the pure metal.

[2]

Extended Only

Describe how zinc metal can be obtained from zinc sulfate solution by electrolysis.

A labelled diagram is acceptable. Include all the products of this electrolysis. The electrolysis is similar to that of copper(II) sulfate solution with inert electrodes.

The ore of aluminium is bauxite which is impure aluminium oxide. Alumina, pure aluminium oxide, is obtained from bauxite.

Aluminium is formed at the cathode when a molten mixture of alumina and cryolite, Na₃AlF is electrolysed.

i) Name two products formed at the anode in this electrolysis.

[2]

ii) All the aluminium formed comes from the alumina not the cryolite. Suggest two reasons why the electrolyte must contain cryolite.

[2]

The purification of bauxite uses large amounts of sodium hydroxide.

i) Describe the chemistry of how sodium hydroxide is made from concentrated aqueous sodium chloride. The description must include at least one ionic equation.

[5]

ii) Making sodium hydroxide from sodium chloride produces two other chemicals. Name these two chemicals and state one use of each chemical.

chemical ..........................................................................................................

use ..........................................................................................................

chemical ..........................................................................................................

use ..........................................................................................................

[2]

Zinc is an important metal. Its uses include making alloys and the construction of dry cells (batteries).

Name an alloy which contains zinc. What is the other metal in this alloy?

The main ore of zinc is zinc blende, ZnS.

i) The ore is heated in the presence of air to form zinc oxide and sulfur dioxide.

Write the equation for this reaction.

[2]

ii) Give a major use of sulfur dioxide.

[1]

Extended Only

Zinc can be obtained from zinc oxide in a two step process. Aqueous zinc sulfate is made from zinc oxide and then this solution is electrolysed with inert electrodes. The electrolysis is similar to that of copper(II) sulfate with inert electrodes.

i) Name the reagent which will react with zinc oxide to form zinc sulfate.

 [1]

ii) Complete the following for the electrolysis of aqueous zinc sulfate.

Write the equation for the reaction at the negative electrode. Name the product at the positive electrode. The electrolyte changes from zinc sulfate to .................................................................... .

[3]

Extended Only

A dry cell (battery) has a central rod, usually made of graphite. This is the positive electrode which is surrounded by the electrolyte, typically a paste of ammonium chloride and manganese(IV) oxide, all of which are in a zinc container which is the negative electrode.

i) Suggest why the electrolyte is a paste.

 [1]

ii) The following changes occur in a dry cell. For each change, decide if it is oxidation or reduction and give a reason for your choice.

Zn to Zn²⁺

..........................................................................................................

manganese(IV) oxide to manganese(III) oxide

..........................................................................................................

[2]

Lithium bromide is an ionic compound. It can be electrolysed when it is molten or in aqueous solution. It cannot be electrolysed as a solid.

Solid lithium bromide is a poor conductor of electricity. The ions cannot move to the electrodes, they are held in an ionic lattice by strong forces.

i) Describe the motion of the ions in the solid state.

[1]

ii) Define the term ionic bonding.

[2]

iii) What is meant by the term ionic lattice?

[2]

Extended Only

The diagram shows the electrolysis of molten lithium bromide.

i) Mark on the diagram the direction of the electron flow. 

[1]

ii) Write an ionic equation for the reaction at the negative electrode (cathode).

[1]

iii) Write an ionic equation for the reaction at the positive electrode (anode).

[2]

iv) Which ion is oxidised? Explain your answer.

[2]

Extended Only

When aqueous lithium bromide is electrolysed, a colourless gas is formed at the negative elctrode and the solution becomes alkaline.

Explain these observations and include an equation in your explanation.