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Three electrolytic celss A,B,C containin...

Three electrolytic celss A,B,C containing solutions of `ZnSO_(4),AgNO_(3)` and `CuSO_(4)`, respectively are connected in series. A steady current of `1.5` amperes was passes through them until `1.45` g of silver deposited at the cathode of cell B. How long did the current flow ? What mass of copper and zinc were deposited.

Text Solution

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`Ag^(+)+e^(-)rarrAg`
`because` 108 g of Ag is deposited by 1 F = 96500C
`therefore` 1.45g of Ag is deposited by 1 F = `(96500)/(108)xx1.45 = 1295.6 C`
`therefore Q = It`
`therefore t = (Q)/(I) = (1295.6)/(1.5) = 863.75 sec`.
Now, `Cu^(2+) + 2e^(-) rarr Cu`
`therefore` Copper, Cu deposited = `(63.5)/(2xx96500)xx1295.6 = 0.426g`
Also, `Zn^(2+)+2e^(-)rarrZn`
`therefore` Zinc, Zn deposited = `(65.4)/(2xx96500)xx1295.6 = (84732.24)/(193000) = 0.439g`
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