In the Hall process, aluminium is produced by the electrolysis of molten `Al_2O_3`. How many second would it take to produce enough aluminium by the Hall process to make a case of 24 cans of auminium soft-drink, if each can uses 5.0g of Al, a current of 9650amp is employed and the current efficiency of the cell is 90%:
A
203.2
B
148.14
C
333
D
6.17
Text Solution
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The correct Answer is:
B
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How many moles of electrons are required to Produce 10.0 g of Al from molten Al_2O_3 ?
Al_2O_3 is reduced by elecrrolysis at low potentals and high current. If 4.0xx10^4 amperes of current is passed through molten Al_2O_3 for 6 hours, what mass of aluminium is produced?
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In a hydrogen oxyge fuel cell, electricity is produced. In this process H_2 (g) is oxided at anode and O_2 (g) reduced at cathode Given: Cathode O_2(g)+2H_2O(l)+4e^(-)to4OH^(-)(aq) Anode H_2(g)+2OH^(-)(aq)to2H_2O(l)+2e^(-) 4.48 litre H_2 at 1atm and 273 k oxidised in 9650 sec. The current produced is (in amp):
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