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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 can molten sodium chloride be electrolysed but solid sodium chloride cannot?
What is the main industrial use of molten-salt electrolysis in aluminium production?
Which particle moves through the external wire of an electrolysis circuit (not through the molten electrolyte)?
Which of the following best describes the electricity flow in an electrolytic cell used with molten ionic compounds?
Which practical reason explains why molten electrolysis cells are often sealed or have gas-handling systems in industry?
For electroplating a metal object, which of the following is the usual role of the object being plated?
Why does electrolysis of molten sodium bromide produce a different gas at the anode than electrolysis of an aqueous sodium bromide solution?
Why is graphite often used as an electrode material in high-temperature molten salt electrolysis?
Which half-equation correctly shows the reduction taking place at the cathode during electrolysis of molten NaCl?
If an inert carbon anode is used in electrolysis of aluminium oxide, what is one consequence at the anode?
Why are molten ionic compounds often electrolysed at high temperatures?