Hall Heroult cell solutions
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1) Cheap electricity is essential for the commercial viability of an aluminium smelter. a) Calculate the electric charge required to produce 0.500 kg of alluminium from alumina in Hall-Heroult cell. Al3+(in cryolite) + 3e => Al(l) Step 2 calculate the amount of electrons in mol Step 3 calculate the charge |
b) How long must a current of 150,000 A flow in order to deposit 1.00 tonne(106g ) of aluminium? Step 1 convert 106g of aluminium to mol. Step 2 calculate the mol of electrons needed Step 3 calculate the charge this represents Step 4 calculate the time in seconds taken to deliver this charge at acurrent of 150,000 A |
c) What is the mass of carbon consumed at the anodes if a cell operates at 150,000 A for 2.00 hours? Al3+(in cryolite) + 3e => Al(l) Step 2 calculate the mole of aluminium produced 2Al2O3(in cryolite) + 3C(s) => 4Al(l) + 3CO2(g) => 3/4 X 380 = 285 Step 4 calculate the mass of carbon |
d) How does an aluminium smelter contribute to global warming? Production of carbon dioxide and use of high amounts of electrical energy which may also cause the generation of carbon dioxide at the power station if it is not a hydroelectric power station or other renewable energy source. |
e) What is the mass of carbon dioxide produced per day by an aluminium smelter producing 1,000 tonnes of aluminium per day? 2Al2O3(in cryolite) + 3C(s) => 4Al(l) + 3CO2(g) Step 1 convert 109 grams of Aluminium into mol Step 2 find the mol of carbon dioxide produced according to the equation above. Step 3 find the mass of carbon dioxide. 2.78 X 107 X 44 =1.2 X109 grams |