How long would it take to deposit 50g of Al from an electrolytic cell containing Al2O3 using a current of 105 ampere?
A
1.54 h
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B
1.42 h
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C
1.32 h
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D
2.15 h
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Solution
The correct option is B1.42 h
Faraday's First Law of Electrolysis states that only, According to this law, the chemical deposition due to flow of current through an electrolyte is directly proportional to the quantity of electricity (coulombs) passed through it.
The reaction of Al is,
Al3++3e−→Al
Now as n=3, Equivalent weight of Al=273=9
As per Faraday's first law,
W=Z×I×t⟹Z=Eq.wt96500
⟹t=W×96500Eq.wt×1=50×965009×105=5102.2 or 1.42hours