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Electrolysis Of Molten Ionic Compounds (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Electrolysis Of Molten Ionic Compounds' from the broader topic Chemical Changes. The test is geared towards the AQA exam board style syllabus.
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Why is a porous barrier or mesh sometimes used between compartments in an electrolysis cell?
Which half-equation correctly shows the reduction taking place at the cathode during electrolysis of molten NaCl?
Which of these best explains why ionic compounds only conduct electricity when molten or dissolved?
Why are molten ionic compounds often electrolysed at high temperatures?
Which of the following best describes the electricity flow in an electrolytic cell used with molten ionic compounds?
What is the main industrial use of molten-salt electrolysis in aluminium production?
In an industrial cell that electrolyses molten aluminium oxide dissolved in cryolite, what is the primary purpose of adding cryolite?
In a molten ionic electrolyte, which particles move through the liquid toward the electrodes?
In a cell electrolysing molten copper(II) chloride, what would you expect to collect at the anode?
In the electrolysis of molten lead(II) bromide, what are the main products collected?
Which property of molten ionic salts makes them suitable electrolytes for producing reactive metals like sodium?