Calculate the number of Faradays required to electrolyze `6.35g` of `Cu^(o+)(aq)` ions from an aqueous solution.

Explanation

Reduction of `Cu^(o+)` at cathode
`Cu^(o+)+1e^(-) rarr Cu`
`1e^(-)=1F=1 mol `of `Cu=63.5g `of `Cu`
`:. 6.35 g ` of `Cu` will be deposited `(1F xx 6.35g)/(63.5g)=0.1F`
`=0.1 F`