OCR GCSE Combined Science
Topic questions Chemical changes Using electrolysis to extract metals
9 questions · 53 marks · about 1 hour
When is electrolysis used to extract a metal from its ore?
A The metal dissolves in water.
B The metal has a high melting point.
C The metal is in high demand.
D The metal is very reactive.
Which equation shows a reaction where copper is extracted using electrolysis?
Aluminium is extracted from a rock called bauxite which contains aluminium oxide.
The diagram shows information from a life-cycle assessment for the manufacture and use of aluminium products.
Give one reason why a life-cycle assessment is carried out.
Give two reasons why the products should be recycled at the end of their useful life.
18% of the bauxite rock is turned into aluminium.
Calculate the mass of aluminium that is extracted from 7500 kg of bauxite.
Give your answer to 2 significant figures.
Aluminium is extracted from aluminium oxide, Al2O3, by electrolysis.
This is the equation for the electrolysis of aluminium oxide.
A student thinks that this reaction is an example of reduction.
Explain why the student is correct.
Extracting aluminium by electrolysis is expensive.
Which statements about why the electrolysis is expensive are true, and which are false ?
Tick one (✓) box in each row.
It would be cheaper if aluminium could be extracted by heating the aluminium oxide with carbon.
Explain why aluminium oxide does not react with carbon.
Aluminium is extracted from a rock called bauxite which contains aluminium oxide.
The diagram shows information from a life-cycle assessment for the manufacture and use of aluminium products.
Give one reason why a life-cycle assessment is carried out.
Give two reasons why the products should be recycled at the end of their useful life.
18% of the bauxite rock is turned into aluminium.
Calculate the mass of aluminium that is extracted from 7500 kg of bauxite.
Give your answer to 2 significant figures.
Aluminium is extracted from aluminium oxide, Al2O3, by electrolysis.
This is the equation for the electrolysis of aluminium oxide.
A student thinks that this reaction is an example of reduction.
Explain why the student is correct.
Extracting aluminium by electrolysis is expensive.
Which statements about why the electrolysis is expensive are true, and which are false ?
Tick one (✓) box in each row.
It would be cheaper if aluminium could be extracted by heating the aluminium oxide with carbon.
Explain why aluminium oxide does not react with carbon.
The reversible reaction.
The reaction of a very reactive metal.
The reaction of a green gas.
The reaction where a more reactive metal displaces a less reactive metal.
The reaction where a metal is extracted using electrolysis.
The student writes the word equation for the reaction.
Complete the word equation for the reaction.
Why does this reaction happen?
Use the reactivity series in Fig. 12.1.
Use the reactivity series in Fig. 12.1 to answer parts (b), (c) and (d).
Another student repeats the experiment but places a different metal in the solution of copper sulfate.
There is no chemical reaction.
Suggest a metal that this student used.
Name one metal that can be extracted by heating its oxide with carbon.
Name one metal that can be extracted from its oxide by electrolysis but not by heating its oxide with carbon.
Complete the sentence below to explain the difference in the reactivity of sodium and lithium.
Use one of the words.
electrons neutrons protons
Sodium atoms lose........ more easily than lithium atoms.
State the trend in reactivity of the Group 1 metals.
Name a Group 1 metal which is more reactive than sodium.
Aluminium is extracted from aluminium oxide using electrolysis.
Carbon cannot be used to do this.
Why is electrolysis used?
A Aluminium is more reactive than carbon.
B Aluminium oxide dissolves in water.
C Aluminium oxide has a high melting point.
D Electrolysis uses less energy than extraction with carbon.
Aluminium oxide is mixed with cryolite in the electrolysis cell.
Explain why cryolite is used.
Aluminium is made at the negative electrode (cathode) from aluminium ions, Al3+.
Write a half equation for this reaction. Use e− to represent an electron.
Oxygen, O2, is made at the positive electrode (anode).
The anodes in the cell have to be replaced every few weeks.
Suggest why.
Write the overall balanced symbol equation for the electrolytic breakdown of aluminium oxide, Al2O3.
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