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

Calculate the number of Faradays required to electrolyze `6.35g` of `C

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

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

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