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  4. An electrolytic cell contains a solution of Ag2SO4 and have platinum electrodes. A current is passed until 1.6 gm of O2 has been liberated at anode. The amount of silver deposited at cathode would be

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Q. An electrolytic cell contains a solution of $Ag_2SO_4$ and have platinum electrodes. A current is passed until 1.6 gm of $O_2$ has been liberated at anode. The amount of silver deposited at cathode would be

Electrochemistry

Solution:

$\frac{\text{Weight of oxygen}}{\text{Eq.wt.of oxygen}} = \frac{\text{Wt. of} Ag}{\text{Eq. wt of} Ag}$
(Faraday's second law )
$\frac{1.6}{8} = \frac{\text{Wt. of}Ag}{108}$
Weight of $Ag$ deposited $= 21.60 \,gm$
[Eq. wt. of oxygen $= \frac{\text{atomic weight }}{\text{valency}}$ $= \frac{16}{2} = 8$]