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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 cu

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Three electrolytic cell A,B , and C contaning solutions of ZnSO4,AgNO3 , and CuSO4 , respectively, are connected in series. A steady current of 1.5A was passed through them until 1.45g of silver deposited at the cathode of cell B . How long did the current flow ? What mass of copper and zinc were deposited ? Select the correct answer from above options

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Correct Answer - 863.7s,0.426gofCu,0.438gZn Ag⊕+e-→Ag,i.e.,108g of Ag are deposited by 1F=96500C ∴1.45gofAg will be deposited by 96500 108 ×1.45C =1295.C Q=I×tort=Q/I=1295.6/1.50=863.7s=14min24s Cu2++2e-→Cu i.e.,2×96500C deposits Cu=63.5g = 63.5 2×96500 ×1295.6=0.426g ∴Zn deposited = 63.5 2×96500 ×1295.6=0.438g

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