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To deposit 0.5 kg of silver per hour on ...

To deposit 0.5 kg of silver per hour on the cathode of a silver voltameter of resis - tance 0.70 milliohm .How much p./d must be maintained between the plates ?
`("Atomic mass of "Ag=108,F =965000 C "mole"^(-1))`

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0.086 V
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To deposit 0.5 kg of silver per hour on the cathode of a silver voltameter of resistance 0.70 milliohm , how much p.d. must be maintained between the plates ? ( Atomic mass of Ag = 108 , F = 96500 C mol^(-1) ).

It is desied 0.54 kg of silver per hour on the cathode of silver voltsmeter whose resistance is 0.72mOmega How much potential difference must be maintained between the plates of the voltameter during eletrolysis .Use the know value of Farday's constant .Relative atomic mass of silver is 108.

Three electrolytic cells A, B and C containing solutions of zinc sulphate, silver nitrate and copper sulphate, respectively are connected in series. A steady current of 1.5 ampere was passed through them until 1.45 g of silver were deposited at the cathode of cell B. How long did the current flow? What mass of copper and what mass of zinc were deposited in the concerned cells? (Atomic masses of Ag = 108, Zn = 65.4, Cu = 63.5)

It is desired to deposit 0.254 kg of copper on the cathode of a copper voltameter . How long will it take to deposit this amount if a steady current of 100 A is maintained . Use the known value of Faraday constant . Relative atomic mass of copper is 63.5 .

How long will it take to deposit electrolytically 10.79 g of silver on the cathode of a silver voltameter by a current of 25 A ? (ECE of silver= 0.001118 g C^(-1) ).

A current of 1.50 A was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The weight of silver deposited was 1.50g . How long did the current flow ? (Molar mass of Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1) ).

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