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

Explanation

To calculate the number of Faradays required to electrolyze 6.35 g of Cu\(^+\) ions from an aqueous solution, we can follow these steps:

### Step 1: Calculate the number of moles of Cu\(^+\)
To find the number of moles of Cu\(^+\), we use the formula:
\[ \text{Number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]
Given:
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