Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Electrolysis
198 practice questions
Topics covered
- Why things conduct electricity17 practice questions
- Passing electricity through compounds: electrolysis20 practice questions
- The electrolysis of molten compounds19 practice questions
- Electrolysis and redox19 practice questions
- The electrolysis of other molten substances19 practice questions
- The electrolysis of aqueous solutions18 practice questions
- The electrolysis of sodium chloride solution19 practice questions
- The electrolysis of copper(ii) sulfate solution using inert electrodes18 practice questions
- The electrolysis of some other solutions using inert electrodes19 practice questions
- What would happen with non-electrolytes?19 practice questions
Practice questions
91–100 of 198
Question 91
4 marks · Normal
Answer and see the solution →This question is about the electrolysis of molten tin(II) chloride (SnCl2).
(a)[2 marks]Write the balanced ionic half-equation for the reaction at the cathode.
(b)[2 marks]Write the balanced ionic half-equation for the reaction at the anode.
Question 92
2 marks · Hard
Answer and see the solution →Balance the following ionic half-equation for the electrolysis of a molten ionic compound, so that both the number of atoms and the charges are equal on both sides:
where M represents a generic metal.
Question 93
5 marks · Hard
Answer and see the solution →A molten ionic compound XY is electrolysed using inert electrodes.
(a)[2 marks]State which element is produced at the cathode. Explain your answer.
(b)[2 marks]State which element is produced at the anode. Explain your answer.
(c)[1 mark]Give one reason why these predictions are valid only for molten binary ionic compounds, not aqueous ones.
Question 94
2 marks · Hard
Answer and see the solution →Write the ionic half-equation for the reaction that occurs at the cathode during the electrolysis of molten magnesium oxide (MgO).
Question 95
1 mark · Easy
Answer and see the solution →State why the volume of chlorine gas collected at the anode is usually less than expected during the electrolysis of concentrated sodium chloride solution.
Question 96
3 marks · Easy
Answer and see the solution →A student is asked to investigate the electrolysis of an aqueous sodium chloride solution in the laboratory.
(a)[2 marks]Describe how you would set up apparatus to collect the products formed during this electrolysis.
(b)[1 mark]State one safety precaution you should take when performing this experiment.
Question 97
2 marks · Easy
Answer and see the solution →During the electrolysis of concentrated sodium chloride solution, a total of 8 cm³ of gas is collected at the cathode. The experiment is carried out at room temperature and pressure.
(a)[1 mark]Name the product formed at the cathode.
(b)[1 mark]What volume of chlorine gas would you expect to collect at the anode under the same conditions?
Question 98
2 marks · Easy
Answer and see the solution →A student finds that the volume of chlorine gas collected during the electrolysis of concentrated sodium chloride solution is less than expected.
(a)[1 mark]Explain why less chlorine gas is collected than expected.
(b)[1 mark]Suggest one way you could change the experiment to collect more chlorine gas.
Question 99
1 mark · Easy
Answer and see the solution →Name one piece of apparatus you would need to collect the gas produced at the cathode during the electrolysis of concentrated sodium chloride solution.
Question 100
3 marks · Easy
Answer and see the solution →The electrolysis of concentrated sodium chloride solution is carried out using carbon electrodes.
(a)[1 mark]State the product formed at the cathode.
(b)[1 mark]State the product formed at the anode.
(c)[1 mark]Write a word equation for the reaction that occurs at the anode.