AP Chemistry
9.11 Electrolysis and Faraday’s Law
An electrolytic cell is used to electroplate gold onto an electrode from an aqueous solution of gold(III) nitrate, \(\text{Au(NO}_3)_3\text{(aq)}\). The cathodic half-reaction is represented below.
\[ \text{Au}^{3+}\text{(aq)} + 3\,e^- \rightarrow \text{Au(s)} \]
A constant current of \(9.65\text{ A}\) is passed through the cell for \(50.0\text{ min}\). Assuming that the reduction of \(\text{Au}^{3+}\text{(aq)}\) is the only process occurring at the cathode and proceeds with \(100\%\) current efficiency, which of the following is closest to the mass of \(\text{Au(s)}\) deposited on the electrode? (Faraday's constant \(F = 96{,}500\text{ C/mol } e^-\); molar mass of \(\text{Au} = 197.0\text{ g/mol}\))
\[ \text{Au}^{3+}\text{(aq)} + 3\,e^- \rightarrow \text{Au(s)} \]
A constant current of \(9.65\text{ A}\) is passed through the cell for \(50.0\text{ min}\). Assuming that the reduction of \(\text{Au}^{3+}\text{(aq)}\) is the only process occurring at the cathode and proceeds with \(100\%\) current efficiency, which of the following is closest to the mass of \(\text{Au(s)}\) deposited on the electrode? (Faraday's constant \(F = 96{,}500\text{ C/mol } e^-\); molar mass of \(\text{Au} = 197.0\text{ g/mol}\))
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