AP Chemistry
9.11 Electrolysis and Faraday’s Law
In an electroplating experiment, a constant current of \(9.65\text{ A}\) is passed through an electrolytic cell containing an aqueous \(\text{CuSO}_4\) solution for \(1000\text{ s}\). Assuming that all the current is used in the reduction of \(\text{Cu}^{2+}\text{(aq)}\) to deposit \(\text{Cu(s)}\) on the cathode, what is the mass of copper deposited?
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