Calculate the number of coulombs required to deposit 40 . 5 g of Al when the electrode reaction is Al 3 + + 3 e - → Al ( s ) .

Electrode reaction : Al 3 + + 3 e - → Al ( s ) Given : Weight of aluminium to be deposited = 40 . 5 g Solution : Number of electrons exchanged in 1 mol n = 3 Amount of charge deposited q = n × F Amount of charge required to deposit 1 mol of Al = 3 × 96500 Amount of charge required to deposit 1 g of Al = 3 × 96500 27 . 0 Amount of charge required to deposit 40 . 5 g of Al = 3 × 96500 × 40 . 5 27 = 434250 C Thus, 434250 coulombs are required to deposit 40 . 5 g of aluminium.

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What will happen during the electrolysis of aqueous solution of ${CuSO}_{4}$ by using platinum electrodes?

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What will happen during the electrolysis of aqueous solution of CuSO4 by using platinum electrodes?

Important Questions on Electrochemistry

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What will happen during the electrolysis of aqueous solution of ${CuSO}_{4}$ by using platinum electrodes?