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 .

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 .

What mass of copper oxide will will be obtained by heating 12.35 g of copper carbonate ? (Atomic mass of Cu = 63.5).

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.

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 steady current of 1.5 A flows through a copper volammeter for 10 min. If the electorchemical equivalent of copper is 30 xx 10^(-5) gC^(-1) , the mass of copper deposited on the electrode will be