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 steady current of 10.0 A is maintained in a copper voltameter . Calculate the time required to deposit 2.5 g of copper . Relative atomic mass of copper = 63.5 g .

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.

A metal surface of surface area 250 cm^(2) is to coated onboth sides with copper by eletrolysis .How long will it take to deposit copper lauyer 0.01 cm in thick if a currect of 1.5 A is used ECE of copper =0.0003gC^(-1) and density of copper =9 g cm^(-3)

When a current of 0.75 A is passed through a CuSO_4 solution for 25 min , 0.369 g of copper is deposited . Calculate the atomic mass of copper .

0.2864 g of Cu was deposited on passage of a current of 0.5 ampere for 30 minutes through a copper sulphate solution. The electrochemical equivalent of copper is

If a current of 3 A be passedd through a voltameter for 100 minutes, the amount of copper deposited is found to be 5.94 g. Calculate the electrochemical equivalent of nickel, when relativr atomic masses of copper and nickel are 63.57 and 58.68 respectively.