AP Chemistry
9.11 Electrolysis and Faraday’s Law
A student models the recovery of copper from a battery-recycling solution by passing a constant current through an electrolytic cell. Copper is deposited at the cathode according to the following half-reaction.
\(\text{Cu}^{2+}\text{(aq)}+2\text{e}^-\rightarrow\text{Cu(s)}\)
The current is \(1.93\text{ A}\) and is applied for \(1.00\times10^3\text{ s}\). Assume that all the current is used to deposit copper. The Faraday constant is \(9.65\times10^4\text{ C/mol }\text{e}^-\), and the molar mass of copper is \(63.5\text{ g/mol}\). What mass of copper is deposited on the cathode?
\(\text{Cu}^{2+}\text{(aq)}+2\text{e}^-\rightarrow\text{Cu(s)}\)
The current is \(1.93\text{ A}\) and is applied for \(1.00\times10^3\text{ s}\). Assume that all the current is used to deposit copper. The Faraday constant is \(9.65\times10^4\text{ C/mol }\text{e}^-\), and the molar mass of copper is \(63.5\text{ g/mol}\). What mass of copper is deposited on the cathode?
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