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16. Three electrolytic cells A, B and C containing electrolytes ZnSO​4, AgNO​​3 and CuSO4 respectively were connected in series. A steady current of 1.50 ampere was passed through them until 1.45 g of Ag were deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?                                                                                                                                                                                                       (At. wts. of Cu=63.5, Zn=65.3, Ag=108)

Dear Student,

Ag+ + e-   AgNow,  1F of e- deposits 1 mol of Agi.e. 96500 C deposits 108 g of AgSo, 1.45 g of Ag is deposited by 96500108×1.45 = 1295.6 Cand, we know that Q = Itor, t=Qi=1295.61.50=863.7 sSince the connection is in series, then the amount of charge is same. So,    Cu2+  +  2e-      CuHere, 2F e- deposits 1 mol of Cui.e. 2×96500Cdeposits 63.5 g CuSo, 1295.6 C will deposit 63.52×96500×1295.6=0.4263 gSimilarly, Zn2+ + 2e-  ZnHere, 2F e- deposits 1 mol of Zni.e. 2×96500Cdeposits 65.4 g CuSo, 1295.6 C will deposit 65.42×96500×1295.6=0.44 g

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