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Three electrolytic cell A,B, and C contaning solutions of ZnSO_(4), AgNO_(3), and CuSO_(4), respectively, are connected in series. A steady current of 1.5A was passed 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 ? |
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Answer» Solution :`AG^(+)+e^(-)rarr Ag(s)` 108 g of SILVER is DEPOSITED by 96500 C. `"1.45 g silver is deposited by"=(96500xx1.45)/(108)` `=1295.6C` `Q=Ixxt` `1295.6=1.5xxt` `t=(12956)/(1.5)=863s` In cell A, the electrode reaction is 5.6 `Zn^(2+)+2e^(-)rarr Zn` 2F of electricity deposit Zn = 65.3 g `"1295.6 of electricity deposit Zn"=(65.3xx1295.6)/(2xx96500)` `=0.438g` In cell C, the electrode reaction is `Cu^(2+)+2e^(-)rarrCu(s)` 2F of electricity deposit Cu = 63.5 g `"1295.6 of electricity deposit Cu"=(63.5xx1295.6)/(2xx96500)` `=0.426g` |
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