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Calculate the qunatity of electricity(in...

Calculate the qunatity of electricity(in colulombs) necessary to deposti 15.89 g of copper form a `CuSO_(4)` solution (atomic weight of Cu 63.6)

A

48250 colulombs

B

96500 colulombs

C

48220 colulombs

D

12062 coulombs

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0.5 Faraday of electricity was passed jo deposit áll the copper present in 500ml of CuSO_4, solution. What was the molarity of this solution?

The mass of copper that will be deposited at cathode in electrolysis of 0.2M solution of copper sulphate when a quantity of electricity equal to that required to liberate 2.24L of hydrogen from 0.1M aqueous H_(2)SO_(4) is passed ( atomic mass of Cu=63.5) will be (a) 1.59g (b) 3.18g (c) 6.35g (d) 12.70g

The density of copper is 8.95 g mL^(-1) . Find out the number of coulombs needed to plate an area of 100cm^(2) to a thickness of 10^(-2)cm using CuSO_(4) solution as electrolyte. ( Atomic weight of Cu=63.5g)

The density of copper is "8.94 g mL"^(-1) . Find the charge needed to plate an area of 10xx10cm^(2) to a thickness of 10^(-2)cm using a CuSO_(4) solution as electrolyte (atomic weight of Cu = 63.6 g/mol).

When a quantity of electricity is passed through CuSO_(4) solution, 0.16 g of copper gets deposited. If the same quantity of electricity is passed through acidulated water, then the volume of H_(2) liberated at STP will be : (given atomic weight of Cu=64)

Calculate the equivalent weight and electrochemical equivalent of copper deposited from cupric salt (At. Wt of Cu = 63.5) .

If same quantity of electricity is passed through CuCI and CuSO_(4) the ratio of the weights of Cu deposited from CuSO_(4) and CuCI is:-

A metal is know to form fluoride MF_(2) . When 10A of electricity is passed through a molten sat for 330sec, 1.95g of metal is deposited. Find the atomic weight of M. what will be the quantity electricity required to deposit the same mass of Cu form CuSO_(4) ?

In an electrolysis experiment, current was passed for 5h through two cells connected in series. The first cell contains a solution of gold and second contains copper sulphate solution. In the first cell, 9.85g of gold was deposited. If the oxidation number of gold is +3 , find the amount of copper deposited at the cathode of the second cell. Also calculate the magnitude of the current in ampere, ( Atomic weight of Au is 1197 and atomic weight of Cu is 63.5) .

Calculate the time required to deposit 1.27 g of copper at cathode when a current of 2A was passed through the solution of CuSO_(4) . ("Molar mass of "Cu=63.5g mol^(-1), 1F =96500 C mol^(-1)).

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