Question 1: Aluminium is the most abundant metal in the Earth's crust, occurring naturally as bauxite....
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Question 1: Aluminium is the most abundant metal in the Earth's crust, occurring naturally as bauxite. Pure aluminium metal is very reactive so it is nearly always found in combination with other minerals. In terms of application, its low density and its ability to resist corrosion has led to it becoming the most widely used non-ferrous metal alloy. 1.1 Interestingly, elemental aluminium cannot simply be produced by the electrolysis of aqueous aluminium salts. Explain the chemistry behind why that is the case. (3 marks) 1.2 How is aluminium currently produced and how did it revolutionise the way aluminium was produced before this? You answer should include a brief description of the steps (and chemistry) involved in both those productions. (6 marks) 1.3 Is the same process used for the recycling of aluminium? Explain briefly. (3 marks) 1.4 In the electrolytic production of aluminium, what mass (in grams) of aluminium can be deposited in 2.00 hours by a current of 1.8 A? (4 marks) 1.5 Calculate the mass of aluminium which can be produced with the same quantity of electricity that is used to produce 1.00 kg of copper metal. (4 marks) Question 2: On learning about the utility of aluminium, a group of school kids want to set up an electrochemical cell using lead (Pb | Pb) and aluminium (All Al) half-cells. 2.1 Help them to determine the correct oxidation and reduction half-reactions. (2 marks) 2.2 They incorrectly determined the cell voltage to be 1.79 V. Explain chemically what they did wrong? Justify your answer thereby calculating the correct cell voltage. (3 marks) 2.3 They eventually set up the cell according to the diagram below. Fully annotate the diagram below to explain what is happening in the cell. (5 marks) electrode 4,3 Question 1: Aluminium is the most abundant metal in the Earth's crust, occurring naturally as bauxite. Pure aluminium metal is very reactive so it is nearly always found in combination with other minerals. In terms of application, its low density and its ability to resist corrosion has led to it becoming the most widely used non-ferrous metal alloy. 1.1 Interestingly, elemental aluminium cannot simply be produced by the electrolysis of aqueous aluminium salts. Explain the chemistry behind why that is the case. (3 marks) 1.2 How is aluminium currently produced and how did it revolutionise the way aluminium was produced before this? You answer should include a brief description of the steps (and chemistry) involved in both those productions. (6 marks) 1.3 Is the same process used for the recycling of aluminium? Explain briefly. (3 marks) 1.4 In the electrolytic production of aluminium, what mass (in grams) of aluminium can be deposited in 2.00 hours by a current of 1.8 A? (4 marks) 1.5 Calculate the mass of aluminium which can be produced with the same quantity of electricity that is used to produce 1.00 kg of copper metal. (4 marks) Question 2: On learning about the utility of aluminium, a group of school kids want to set up an electrochemical cell using lead (Pb | Pb) and aluminium (All Al) half-cells. 2.1 Help them to determine the correct oxidation and reduction half-reactions. (2 marks) 2.2 They incorrectly determined the cell voltage to be 1.79 V. Explain chemically what they did wrong? Justify your answer thereby calculating the correct cell voltage. (3 marks) 2.3 They eventually set up the cell according to the diagram below. Fully annotate the diagram below to explain what is happening in the cell. (5 marks) electrode 4,3
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Answer rating: 100% (QA)
ANS 11 Because of the high discharge potential Al 3 ions cannot be produced by electrolyzing aqueous aluminum salts Hydrogen gas H 2 is evolved at the ... View the full answer
Related Book For
Inorganic Chemistry
ISBN: 9780198768128
7th Edition
Authors: Mark Weller, Tina Overton, Jonathan Rourke
Posted Date:
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