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.

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) ).

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))

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 .

A copper refining cell consists of two parallel copper plate electrodes 5 cm apart and 1 metre squre, immersed in a copper sulphate solution of resistivity 12xx10^(-2)Omegam . Then the potential difference which must be established between the plates to provide a constant current to deposit 0.66kg of copper on cathode in one hour is nearly (Z=3.33xx10^(-7)kg//C)

A copper refining cell consists of two parallel copper plate electrodes 5 cm apart and 1 metre squre, immersed in a copper sulphate solution of resistivity 12xx10^(-2)Omegam . Then the potential difference which must be established between the plates to provide a constant current to deposit 0.66kg of copper on cathode in one hour is nearly (Z=3.33xx10^(-7)kg//C)

In a silver plating system, an electrolysis current of 5.0 A is used for a certain time and 0.5 mol of silver is deposited. How many moles of copper and iron will be deposited in their respective plating system if an electrolysis current of 10.0 A is passed for twice the time for silver plating. ( Relative atomic mass of silver=107.3, of copper -63.54, of iron=55.85).

A study potential difference of 1.62 V is maintained across two Pt electrodes placed in a solution of CuCl_(2) . At the end of 600s, the mass of copper deposited on the cathode is measured to be 5.92 g. The back emf of the voltameter is given to be 1.34 V. Estimate the resistance of voltameter. Faraday constant =96500 C mol^(-1) , relative atomic mass of copper =63.5.

The potential difference across the terminals of a battery of emf 12 V and internal resistance 2 Omega drops to 10 V when it is connected to a silver voltameter. Find the silver deposited at the cathode in half an hour. Atomic weight of silver is 107.9 g mol^(-1) .

The potential difference across the terminals of a battery of emf 12 V and internal resistance 2 Omega drops to 10 V when it is connected to a silver voltameter. Find the silver deposited at the cathode in half an hour. Atomic weight of silver is 107.9 g mol^(-1) .

The potential difference across the terminals of a battery of emf 12 V and internal resistance 2 Omega drops to 10 V when it is connected to a silver voltameter. Find the silver deposited at the cathode in half an hour. Atomic weight of silver is 107.9 g mol^(-1) .