A current of 19296 C is passed through an aqueous solution of copper sulphate using copper electrodes . What is the mass (in g) of copper deposited at the cathode ?
(molar mass of Cu = `63.5 g mol^(-1)` )

Options

A. 3.17
B. 1.58
C. 6.35
D. 0.79

Answer

C

Explanation

Given ,
In an aqueous solution of copper sulphate `(CuSO_4)` using copper electrodes ,
Current = 19296 C
Molar mass of Cu = `63.5 gmol^(-1)`
In `CuSO_4 , Cu` has `Cu^(2+)` charge
Thus,
2 x 96500 C of charge gives = 63.5 g of Cu
19296 C of charge gives = ?
`=(19296xx63.5)/(2xx96500)`
=6.35 g
`therefore` Mass of copper deposited at the cathode = 6.35 g