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

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)).

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)).

Calculate the time to deposit 1.5 g of silver at cathode when a current of 1.5 A is passed through the solution of AgNO_(3) .

(a) Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO_(3) for 15 minutes (Given : Molar mass of Ag = 108 g mol^(-1) 1F = 96500 C mol^(-1) ) (b) Define fuel cell

(a) Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO_(3) for 15 minutes (Given : Molar mass of Ag = 108 g mol^(-1) 1F = 96500 C mol^(-1) ) (b) Define fuel cell

Find the mass of copper deiposited on cathode when a current of 1.5A is passed through copper sulphate solution for 5 minutes (At. Mass of Cu=63.5).

How much time would it take in minutes to deposit 1.18 g of metallic copper on a metal object when a current of 2.0 A is passed through the electrolytic cell containing Cu ^2 +ions? [ Molar mass of Cu =63.5 g /mol;IF=96,500 Cmol^-1]