In the electrolysis of concentrated sodium chloride (brine) using inert electrodes, chlorine gas is produced at the positive electrode (anode) according to the half-equation:
2Cl−(aq)→Cl2(g)+2e− 2\text{Cl}^-(\text{aq}) \to \text{Cl}_2(\text{g}) + 2\text{e}^- 2Cl−(aq)→Cl2(g)+2e−Suggest a suitable element that can be used as an inert electrode in this process.
The volume of chlorine gas collected at the anode is often slightly less than the expected volume, even though there are no leaks in the apparatus. Suggest an explanation for this observation.
During an electrolysis experiment, a total of 579 000 coulombs579\,000\text{ coulombs}579000 coulombs of electric charge was passed through the solution. Calculate the amount, in moles, of chlorine gas (Cl2\text{Cl}_2Cl2) formed.
[One faraday = 96 500 coulombs96\,500\text{ coulombs}96500 coulombs]
21 exam-style questions on Edexcel IGCSE Chemistry Electrolysis. Each one has a worked solution and a mark scheme showing where the marks go.