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Question

Calculate the number of coulombs required to deposit 5.4 g of Aluminium when the given electrode reaction is
Al3++3eAl

A
1.83×105 C
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B
57900 C
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C
5.86×105 C
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D
60500 C
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Solution

The correct option is B 57900 C
According to Faraday's first law of electrolysis
W=Z×QF
W=Mass deposited =5.4 g
Z=Equivalent mass =Molar massn-factor
F=Faraday constant =96500 C
Q=Charge
For the given reaction,
Al3++3eAl
n-factor is 3

5.4=(273)×Q96500

Q=57900 C

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

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