AP Chemistry
9.11 Electrolysis and Faraday’s Law
In an industrial process, molten sodium chloride, \(\text{NaCl}(l)\), is electrolyzed in an electrochemical cell according to the following overall reaction:
\[ 2\,\text{NaCl}(l) \rightarrow 2\,\text{Na}(l) + \text{Cl}_2(g) \]
A constant electric current of \(9.65\text{ A}\) is passed through the molten salt for \(100.0\text{ minutes}\). Given that Faraday's constant is \(96{,}500\text{ C/mol } e^-\), what is the total number of moles of electrons transferred through the cell during this process?
\[ 2\,\text{NaCl}(l) \rightarrow 2\,\text{Na}(l) + \text{Cl}_2(g) \]
A constant electric current of \(9.65\text{ A}\) is passed through the molten salt for \(100.0\text{ minutes}\). Given that Faraday's constant is \(96{,}500\text{ C/mol } e^-\), what is the total number of moles of electrons transferred through the cell during this process?
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