Question 1: Molten electrolysis involves passing an electric current through a molten (liquid) ionic compound to decompose it into its elements. This process requires the ionic compound to be in a liquid state so that ions are free to move and carry charge.

Answer: Molten electrolysis is the process of decomposing a molten ionic compound into elements by passing an electric current through it.

Question 1: Define electrolysis in the context of molten ionic compounds.

Answer: Electrolysis is the chemical decomposition of a molten ionic compound by passing an electric current through it.

Question 2: Explain why ionic compounds need to be in a molten state for electrolysis to occur.

Answer: Because ions need to be free to move and carry charge; in a solid, ions are fixed in a lattice and cannot move.

Question 3: What is the role of the electrodes in molten electrolysis?

Answer: Electrodes conduct electricity and provide a site for reduction and oxidation reactions during electrolysis.

Question 1: Calculate the amount of aluminium (Al) produced when passing 96,000 Coulombs of charge through molten aluminium oxide (Al₂O₃). (Atomic masses: Al = 27 g/mol, O = 16 g/mol).

Answer: Mass of Al = (Q / (n × F)) × molar mass of Al; where Q=96000 C, n=3 (electrons per Al atom), F=96485 C/mol.

Question 2: How many moles of sodium (Na) are produced when 1,929,700 Coulombs of charge are passed during the electrolysis of molten sodium chloride? (F = 96485 C/mol).

Answer: Moles of Na = Q / F; so, 1,929,700 / 96485.

Question 1: Describe the key safety precautions that should be taken when performing molten electrolysis in a laboratory.

Answer: Use appropriate protective equipment, ensure proper ventilation, handle high temperatures carefully, and avoid contact with molten substances.

Question 2: Identify the variables that can affect the efficiency of molten electrolysis and explain how they influence the process.

Answer: Variables include temperature, electrode material, current applied, and purity of the ionic compound; these affect ion mobility, reaction rates, and product purity.

Question 1: In an electrolysis experiment, the mass of copper deposited on the cathode was 3.4 grams after passing 0.5 Faradays of charge. Calculate the atomic mass of copper based on this data.

Answer: Use M = (mass × n × F) / Q; with Q = 0.5 × 96485 C, n=2 (electrons per Cu atom).

Question 1: Explain how molten electrolysis is used in the extraction of aluminium from bauxite ore. Include the key steps involved.

Answer: Bauxite is processed to produce aluminium oxide, which is melted to form molten Al₂O₃. An electric current is passed through the melt using carbon electrodes, causing reduction of Al³⁺ ions to aluminium metal at the cathode. This process is energy-intensive but essential for aluminium extraction.

Question 2: Identify a modern technological application that relies on molten electrolysis and briefly describe its significance.

Answer: Electrolytic refining of metals like copper and aluminium is crucial in electronics manufacturing, ensuring high purity for industrial use.