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Question

The number of coulombs required to deposit 5.4g of Aluminium when the given electrode reaction is represented as Al3++3eAl.

A
1.83×105C
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B
57900C
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C
5.86×105C
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D
3F
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Solution

The correct option is D 57900C
According to Faraday's law of electrolysis

W=Z×QF

W= mass deposited =5.4g

Z= Equivalent mass =Molarmasseaccepted

F= Faraday constant =96500C

Q= Charge

5.4g=(27g3)×Q96500C

Q=57900C

Thus, 57900C is required to deposit 5.4g of Al

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