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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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Below a typical questions that will be covered in this test. You final score will be logged on your account

Why is graphite often used as an electrode material in high-temperature molten salt electrolysis?
Which of these best explains why ionic compounds only conduct electricity when molten or dissolved?
In an industrial cell that electrolyses molten aluminium oxide dissolved in cryolite, what is the primary purpose of adding cryolite?
Which of the following is NOT a correct feature of electrolysis of molten ionic compounds?
Why are molten ionic compounds often electrolysed at high temperatures?
For electroplating a metal object, which of the following is the usual role of the object being plated?
Which adjustment would reduce the energy cost of electrolysing a solid ionic compound industrially?
Which statement correctly compares electrolysis of a molten ionic compound with electrolysis of an aqueous solution of the same salt?
In the electrolysis of molten lead(II) bromide, what are the main products collected?
Which half-equation correctly shows the reduction taking place at the cathode during electrolysis of molten NaCl?
In the electrolysis of molten sodium chloride, which species is produced at the negative electrode (cathode)?