1)How can the melting point of the molten salt be lowered
2)Explain why sodium metal cannot be extracted by reduction methods
3)Why is it possible to separate molten sodium from molten sodium chloride
4)Give two uses of sodium metal
5)How would you store sodium metal in the laboratory. Give a reason for your answer
6)State the form in which sodium occurs and give the formula of these compounds
7)Why is the down's cell lined with fire bricks on the outside?Explain
8)Name the two electrode used during the extraction of sodium
9)Why is calcium chloride added to molten sodium chloride during the extraction
1) The melting point of molten salt can be lowered by adding impurities or other materials that disrupt the crystal structure and prevent solidification at higher temperatures.
2) Sodium metal cannot be extracted by reduction methods because it is highly reactive and will react with water or oxygen in the air, making it difficult to isolate in its pure form.
3) It is possible to separate molten sodium from molten sodium chloride because sodium is less dense than sodium chloride and will float to the top, allowing for easy extraction.
4) Two uses of sodium metal include as a reducing agent in organic and inorganic synthesis, and in the production of various chemical compounds and pharmaceuticals.
5) Sodium metal should be stored under a layer of mineral oil in the laboratory to prevent it from reacting with moisture or air, which can lead to fires or explosions.
6) Sodium occurs in nature as various compounds such as sodium chloride (NaCl), sodium carbonate (Na2CO3), and sodium hydroxide (NaOH).
7) The Downs cell is lined with fire bricks on the outside to provide thermal insulation and prevent heat loss, as the high temperatures required for the extraction process can easily dissipate without proper insulation.
8) The two electrodes used during the extraction of sodium are a graphite anode and a molten sodium cathode.
9) Calcium chloride is added to molten sodium chloride during the extraction process to lower the melting point of the mixture and improve the conductivity of the electrolyte.