This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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a) Why is the anode made of graphite in this case instead of steel which is a better conductor of electricity? Graphite is used because it is inert and resistant to corrosion by the chlorine gas produced at the anode at high temperatures. Steel, despite being a better electrical conductor, would react with chlorine gas at the high operating temperatures, forming iron chlorides and corroding. b) How are the electrolytic products separated from reacting? The products, molten sodium and chlorine gas, are separated by their physical properties and the design of the cell. Molten sodium is less dense than the molten electrolyte, so it floats to the top and is collected in a separate channel. Chlorine gas, being less dense, bubbles up and is collected by an inverted dome above the anode. A steel gauze diaphragm is typically used to prevent the molten sodium and chlorine gas from mixing and reacting. c) Give reasons why large quantities of electricity is required for this process. Large quantities of electricity are required for several reasons: • The high melting point of sodium chloride (even with additives) requires significant electrical energy to melt the electrolyte and maintain it in a molten state. • A high decomposition voltage is needed to overcome the strong ionic bonds in molten sodium chloride to produce sodium and chlorine. • The process is run continuously to produce large quantities of sodium, demanding a constant and substantial supply of electrical energy. That's 2 down. 3 left today — send the next one.