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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Aluminium is produced commercially by the electrolysis of Al_(2)O_(3) . How many hours would be required to produce 250 g of Al usinga 5.00 ampere current?
How many coulombs are required to produce 50.0 g of aluminium from molten Al_(2)O_(3) ?
A factory produces 40 kg of calcium in two hours by electrolysis. How much aluminium can be produced by same current in 2 hours if current efficiency is 50%?
A chemist wants to produce Cl_(2)(g) from molten NaCl. How many grams could be produced if the uses a steady current of 1 amp for 5.0 minutes ?
How many grams of Cl_(2)(g) can be produced by the electrolysis molten NaCl with a current of 5.5A for 25 m i n ? [ Atomic weight of Cl=35.5 am u]
How many Coulombs are required to produce 54 grams of aluminium from molten Al_(2)O_(3) ? (Eq. wt of Al=9)
