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, Charge used `=19296 C`
Molar mass of `Cu=635`
`:'` Cu in `CuSO_(4)` has `Cu^(2+)` charge means :
`2xx96500` C of charge give `=63.5 g` of Cu
Thus, 19296 C of charge give `=(63.5xx19296)/(2xx96500)`
`=6.35g` of copper (Cu).
Hence, option (c) is the correct answer.