Question 1: Define molten electrolysis and explain how it differs from aqueous electrolysis.

Answer: Molten electrolysis is the process of passing an electric current through a molten ionic compound to decompose it into its elements, unlike aqueous electrolysis which involves solutions with water.

Question 2: Describe the mechanism by which ions are transported during molten electrolysis.

Answer: Ions migrate through the liquid electrolyte towards the electrodes under the influence of the electric field, where they gain or lose electrons to form neutral substances or elements.

Question 3: Identify two advantages of using molten electrolysis in the production of medical materials.

Answer: It allows the extraction of elements that decompose in aqueous solutions and produces high purity products essential for medical applications.

Question 1: Calculate the amount of electric charge (in coulombs) required to deposit 10 grams of aluminium during electrolysis. (Atomic mass of aluminium = 27 g/mol; valency = 3).

Answer: Q = n × F; n = m / M × valency = 10 / 27 × 3 ≈ 1.11 mol; Q = 1.11 mol × 96485 C/mol ≈ 107,133.5 C

Question 2: If a current of 5 amperes is used in electrolysis to produce a certain quantity of element, how long (in hours) does the process take to deposit 2 grams? (Atomic mass of the element = 20 g/mol; valency = 2).

Answer: n = m / M = 2 / 20 = 0.1 mol; Q = n × F × valency = 0.1 × 96485 × 2 = 19,297 C; time = Q / current = 19,297 / 5 ≈ 3859.4 seconds ≈ 1.07 hours

Question 1: Design a basic outline of an experiment to extract titanium from its ore using molten electrolysis for medical implant manufacturing. Include key variables and safety precautions.

Answer: The experiment involves heating titanium ore (e.g., titanium dioxide) to a molten state with a suitable electrolyte, then passing an electric current to reduce Ti ions to metallic titanium. Key variables include temperature, electrolyte composition, and current density. Safety precautions entail handling high temperatures with insulated equipment, working in a well-ventilated area, and wearing protective gear to prevent burns and exposure to toxic fumes.

Question 1: During an electrolysis process for producing medical-grade sodium, the current efficiency was observed to be 85%. If 3 moles of sodium were deposited, how much electric charge was actually used? (F = 96485 C/mol).

Answer: Total charge without efficiency consideration: Q = n × F = 3 × 96485 = 289,455 C; actual charge used = Q × efficiency = 289,455 × 0.85 ≈ 246,036 C

Question 1: Explain how molten electrolysis can be used in the production of magnesium for medical devices, and discuss the advantages over other methods.

Answer: Molten electrolysis of magnesium chloride involves heating magnesium salt to a molten state and passing an electric current to reduce Mg ions to metallic magnesium. This method produces high-purity magnesium essential for medical implants due to its strength and biocompatibility. Advantages include lower energy consumption compared to traditional methods, fewer impurities, and the ability to produce magnesium directly from its ore without aqueous complications.

Question 1: Describe how molten electrolysis is used to produce pure aluminium for medical surgical instruments and explain why purity is crucial.

Answer: Molten electrolysis decomposes aluminium oxide into aluminium metal, which is then used to make surgical tools. High purity is essential to prevent reactions within the body, reduce toxicity, and ensure the instruments are durable and corrosion-resistant.