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A current of 1.50 amp was passed through an electrolytic cell containing AgNO3 solution with inert electrodes. The weight of Ag deposited was 1.50g. How long did the current flow? (2marks)(b) Write the reactions taking place at the anode and cathode in the above cell. |
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Answer» user_photo Type your question... 12th Chemistry Electrochemistry Electrolytic Cells and Electrolysis Three electrolytic cells A,... CHEMISTRY Three electrolytic cells 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 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? November 22, 2019avatar Puneetha Adak SHARE VIDEO EXPLANATION ANSWER Cell B: Ag + +e − ⇌Ag at cathode. 1 mole (108 g) of Ag is deposited by 96500 C. 1.45 g of Ag will be deposited by 108 96500×1.45
=1295.6C. Q=It 1295.6=1.5×t t=864s Cell A: Zn 2+ +2E − →Zn 2 moles of electrons (2×96500 C of current) produces 1 mole (63.5 g) of zinc. 1295.6 C of electricity will deposit 2×96500 65.3
×1295.6=0.438 g of zinc Cell C: CU 2+ +2e − →Cu 2 moles of electrons (2×96500 C) of current will produce 1 mole (63.5 g) of Cu. 1295.6 C of current will deposit 2×96500 63.5×1295.6
=0.426g of copper |
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