Calculate the number of faradays required to electrolyze $6.35 g$ of $C u^{+} (a q)$ ions from an aqueous solution.

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Solution

${C u}^{+} + e^{-} \to C u$
1 mol $F \to 63.5 g$ of copper
1g of copper $\to \frac{1}{63.5} m o l$
6.35g of copper $\to \frac{6.35}{63.5} = 0.1 F$ of electricity

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

Cu++e−→Cu1 mol F→63.5g of copper1g of copper →163.5mol6.35g of copper →6.3563.5=0.1F of electricity

Calculate the number of faradays required to electrolyze $6.35 g$ of $C u^{+} (a q)$ ions from an aqueous solution.

${C u}^{+} + e^{-} \to C u$
1 mol $F \to 63.5 g$ of copper
1g of copper $\to \frac{1}{63.5} m o l$
6.35g of copper $\to \frac{6.35}{63.5} = 0.1 F$ of electricity